Considering the following precipitation reaction: Pb(NO3)2(aq) + 2KI(aq) ? PbI2(s) + 2KNO3(aq) What is the correct net ionic equation?

Considering the following precipitation reaction:
Pb(NO3)2(aq) + 2KI(aq) ? PbI2(s) + 2KNO3(aq)
What is the correct net ionic equation?

A) Pb2+ + I2- ? PbI2(s)
B) 2NO3- + 2K+ ? 2KNO3
C) Pb2+ + 2NO3- + 2K+ + 2I- ? PbI2(s) + 2K+ + 2NO3-
D) Pb2+ + 2I- ? PbI2(s)
E) none of the above

Answer: D

Considering the following precipitation reaction: Pb(NO3)2(aq) + 2KI(aq) ? PbI2(s) + 2KNO3(aq) What is the correct complete ionic equation?

Considering the following precipitation reaction:
Pb(NO3)2(aq) + 2KI(aq) ? PbI2(s) + 2KNO3(aq)
What is the correct complete ionic equation?

A) Pb2+ + (NO3)2- + 2K+ + 2I- ? PbI2(s) + 2K+ + 2NO3-
B) Pb2+ + 2NO3- +2K+ + I- ? PbI2(s) + 2K+ + NO3-
C) Pb2+ + 2NO3- + 2K+ + 2I- ? PbI2(s) + 2K+ + 2NO3-
D) Pb2+ + 2NO3- + 2K+ + 2I- ? Pb2+ + 2I- + 2K+ + 2NO3-
E) none of the above

Answer: C

Considering the following precipitation reaction: Pb(NO3)2(aq) + 2KI(aq) ? PbI2(s) + 2KNO3(aq) Which ion(s) would NOT be spectator ions?

Considering the following precipitation reaction:
Pb(NO3)2(aq) + 2KI(aq) ? PbI2(s) + 2KNO3(aq)
Which ion(s) would NOT be spectator ions?

A) Pb2+, NO3-
B) K+, I-
C) NO3-, Pb2+
D) Pb2+, I -
E) All the above ions are in the net ionic equation.

Answer: D

Considering the following precipitation reaction: Pb(NO3)2(aq) + 2KI(aq) ? PbI2(s) + 2KNO3(aq) Which ion(s) would NOT be present in the net ionic equation?

Considering the following precipitation reaction:
Pb(NO3)2(aq) + 2KI(aq) ? PbI2(s) + 2KNO3(aq)
Which ion(s) would NOT be present in the net ionic equation?

A) Pb2+, NO3-
B) K+, NO3-
C) K+, Pb2+
D) K+, I-
E) All the above ions are in the net ionic equation.

Answer: B

Considering the following precipitation reaction: Pb(NO3)2(aq) + 2KI(aq) ? PbI2(s) + 2KNO3(aq) Which ion would NOT be present in the complete ionic equation?

Considering the following precipitation reaction:
Pb(NO3)2(aq) + 2KI(aq) ? PbI2(s) + 2KNO3(aq)
Which ion would NOT be present in the complete ionic equation?

A) Pb2+
B) K+
C) NO3-
D) I-
E) All the above ions are in the complete ionic equation.

Answer: E

Considering the following precipitation reaction: Pb(NO3)2(aq) + 2KI(aq) ? PbI2(s) + 2KNO3(aq) Which compound would not form ions in the complete ionic equation?

Considering the following precipitation reaction:
Pb(NO3)2(aq) + 2KI(aq) ? PbI2(s) + 2KNO3(aq)
Which compound would not form ions in the complete ionic equation?

A) PbI2
B) KNO3
C) Pb(NO3)2
D) KI
E) All compounds form ions in the complete ionic equation.

Answer: A

What would be the formula of the precipitate that forms when Pb(NO3)2 (aq) and K2SO4 (aq) are mixed?

What would be the formula of the precipitate that forms when Pb(NO3)2 (aq) and K2SO4 (aq) are mixed?

A) K(NO3)2
B) PbSO4
C) PbK2
D) H2O
E) none of the above

Answer: B

A precipitate is expected to be formed when an aqueous solution of sodium sulfate is added to an aqueous solution of:

A precipitate is expected to be formed when an aqueous solution of sodium sulfate is added to an aqueous solution of:

A) iron(III) chloride.
B) potassium chloride.
C) magnesium chloride.
D) barium chloride.
E) none of the above

Answer: D

What type of a reaction occurs when a potassium nitrate solution is mixed with a barium acetate solution?

What type of a reaction occurs when a potassium nitrate solution is mixed with a barium acetate solution?

A) precipitation
B) acid-base neutralization
C) oxidation-reduction
D) gas evolution
E) no reaction

Answer: E

In writing the chemical equation for a precipitation reaction, what abbreviation of the physical state must appear with one of the products?

In writing the chemical equation for a precipitation reaction, what abbreviation of the physical state must appear with one of the products?

A) (s)
B) (g)
C) (l)
D) (w)
E) none of the above

Answer: A

If you had an aqueous mixture that contained Ag+, K+, and Pb2+ cations, how many different solids could precipitate if a chloride solution was added?

If you had an aqueous mixture that contained Ag+, K+, and Pb2+ cations, how many different solids could precipitate if a chloride solution was added?

A) 1
B) 2
C) 3
D) 4
E) no solids will precipitate

Answer: B

Several grams of sodium chloride are stirred into a glass of water and are no longer visible to the eye. Which of the following statements is FALSE?

Several grams of sodium chloride are stirred into a glass of water and are no longer visible to the eye. Which of the following statements is FALSE?

A) The sodium chloride solid has dissociated into its component ions.
B) An aqueous solution has been prepared.
C) No precipitate has formed.
D) Sodium chloride is insoluble in water.
E) All of the statements are true.

Answer: D

When solid NaCl is stirred into water, which of the following is NOT true?

When solid NaCl is stirred into water, which of the following is NOT true?

A) Individual sodium and chloride ions are present.
B) The solution will conduct electricity.
C) The solution will taste salty.
D) The NaCl will fail to dissociate.
E) none of the above

Answer: D

The compound sodium sulfate is soluble in water. When this compound dissolves in water, which ion listed below would be present in solution?

The compound sodium sulfate is soluble in water. When this compound dissolves in water, which ion listed below would be present in solution?

A) SO42-
B) S2-
C) O2-
D) Na22+
E) none of the above

Answer: A

All of the following compounds are soluble in water EXCEPT:

All of the following compounds are soluble in water EXCEPT:

A) NaCl.
B) CaCl2.
C) FeCl3.
D) NH4Cl.
E) PbCl2.

Answer: E

Which of the following compounds is SOLUBLE?

Which of the following compounds is SOLUBLE?

A) aluminum hydroxide
B) aluminum sulfide
C) aluminum carbonate
D) aluminum sulfate
E) none of the above

Answer: D

Which of the following compounds is SOLUBLE?

Which of the following compounds is SOLUBLE?

A) copper carbonate
B) calcium carbonate
C) potassium carbonate
D) strontium carbonate
E) none of the above

Answer: C

Which of the following compounds is INSOLUBLE?

Which of the following compounds is INSOLUBLE?

A) magnesium phosphate
B) magnesium sulfate
C) magnesium iodide
D) magnesium nitrate
E) none of the above

Answer: A

Which of the following compounds is INSOLUBLE?

Which of the following compounds is INSOLUBLE?

A) potassium acetate
B) lithium carbonate
C) magnesium bromide
D) aluminum sulfide
E) none of the above

Answer: D

An aqueous solution is:

An aqueous solution is:

A) any liquid with another compound dissolved in it.
B) an ionic compound with water dissolved in it.
C) water with a molecular compound dissolved in it.
D) water with another compound dissolved in it.
E) none of the above

Answer: D

Sodium metal reacts with water to form aqueous sodium hydroxide and hydrogen gas. Which equation below best describes the balanced equation for this reaction?

Sodium metal reacts with water to form aqueous sodium hydroxide and hydrogen gas. Which equation below best describes the balanced equation for this reaction?

A) Na + H2O ? NaOH (aq) + H (g)
B) S + H2O ? SOH (aq) + H (g)
C) Na + H2O ? NaOH (aq) + H2 (g)
D) 2Na + 2H2O ? 2NaOH (aq) + H2 (g)
E) 2Na + H2O ? Na2OH (aq) + H (g)

Answer: D

Which of the following equations is NOT balanced properly?

Which of the following equations is NOT balanced properly?

A) 2Cr + 6HCl ? 2CrCl3 + 3H2
B) 2NaHCO3 ? Na2CO3 + CO2 + H2O
C) Cr2(SO4)3 + 6KOH ? 2Cr(OH)3 + 3 K2SO4
D) 4NH3 + 14O2 ? 4NO2 + 6H2O
E) none of the above

Answer: D

When the equation __NO2 + __H2O + __O2 ? __HNO3 is balanced, the coefficient of HNO3 is:

When the equation __NO2 + __H2O + __O2 ? __HNO3 is balanced, the coefficient of HNO3 is:

A) 2
B) 3
C) 4
D) 5
E) none of the above

Answer: C

When the equation __Ca3N2 + __H2O ? __Ca(OH)2 + __NH3 is balanced, the coefficient of H2O is:

When the equation __Ca3N2 + __H2O ? __Ca(OH)2 + __NH3 is balanced, the coefficient of H2O is:

A) 2
B) 3
C) 6
D) 12
E) none of the above

Answer: C

What are the coefficients for the following reaction when it is properly balanced? ___nitrogen monoxide + ___carbon monoxide ? ___nitrogen +___carbon dioxide

What are the coefficients for the following reaction when it is properly balanced?
___nitrogen monoxide + ___carbon monoxide ? ___nitrogen +___carbon dioxide

A) 2, 1, 1, 2
B) 2, 2, 1, 2
C) 2, 2, 2, 1
D) 1, 1, 2, 2
E) none of the above

Answer: B

What are the coefficients for the following reaction when it is properly balanced? ___potassium iodide + ___lead (II) acetate ? ___lead (II) iodide +___potassium acetate

What are the coefficients for the following reaction when it is properly balanced?
___potassium iodide + ___lead (II) acetate ? ___lead (II) iodide +___potassium acetate

A) 2, 1, 1, 1
B) 2, 1, 1, 2
C) 3, 2, 2, 1
D) 1, 1, 2, 2
E) none of the above

Answer: B

What are the coefficients for the following reaction when it is properly balanced? ___nitric acid + ___sodium hydroxide ? ___sodium nitrate + ___water

What are the coefficients for the following reaction when it is properly balanced?
___nitric acid + ___sodium hydroxide ? ___sodium nitrate + ___water

A) 2, 1, 1, 1
B) 2, 3, 2, 2
C) 5, 2, 2, 1
D) 1, 1, 1, 1
E) none of the above

Answer: D

What are the coefficients for the following reaction when it is properly balanced? ___Na3PO4 + ___Ba(NO3)2 ? ___NaNO3 + ___Ba3(PO4)2

What are the coefficients for the following reaction when it is properly balanced?
___Na3PO4 + ___Ba(NO3)2 ? ___NaNO3 + ___Ba3(PO4)2

A) 2, 1, 1, 3
B) 2, 3, 1, 6
C) 2, 3, 6, 1
D) 6, 1, 3, 2
E) none of the above

Answer: C

What are the coefficients for the following reaction when it is properly balanced? ___O2 + ___CH4 ? ___CO2 + ___H2O

What are the coefficients for the following reaction when it is properly balanced?
___O2 + ___CH4 ? ___CO2 + ___H2O

A) 2, 1, 3, 1
B) 2, 3, 2, 2
C) 1, 3, 2, 1
D) 2, 1, 1, 2
E) none of the above

Answer: D

What are the coefficients for the following reaction when it is properly balanced? ___HCl + ___Mg ? ___MgCl2 + ___H2

What are the coefficients for the following reaction when it is properly balanced?
___HCl + ___Mg ? ___MgCl2 + ___H2

A) 2, 1, 1, 1
B) 2, 1, 2, 2
C) 1, 2, 1/2, 1
D) 1, 1, 1, 2
E) none of the above

Answer: A

When the equation, ___O2 + ___C5H12 ? ___CO2 + ___H2O is balanced, the coefficient: of O2 is:

When the equation, ___O2 + ___C5H12 ? ___CO2 + ___H2O is balanced, the coefficient: of O2 is:

A) 3
B) 4
C) 5
D) 8
E) none of the above

Answer: D

When the equation, ___N2 + ___H2 ? ___NH3 is balanced, the coefficient of hydrogen is:

When the equation, ___N2 + ___H2 ? ___NH3 is balanced, the coefficient of hydrogen is:

A) 1
B) 2
C) 3
D) 4
E) none of the above

Answer: C

Before a chemical equation can be written, one must know:

Before a chemical equation can be written, one must know:

A) the atomic mass of all the elements involved.
B) the molar mass of all the compounds.
C) the symbols and formulas of all reactants and products.
D) the number of moles of all reactants and products.
E) none of the above.

Answer: C

Which of the following statements about balancing reactions is FALSE?

Which of the following statements about balancing reactions is FALSE? 

A) If there is no coefficient or subscript, a one is implied.
B) When coefficients are added the type of compounds is changed in the chemical reaction.
C) Subscripts are multiplied by the coefficients to determine the number of atoms in a compound.
D) Coefficients are added to compounds to ensure both sides of the reaction have equal numbers of each atom.
E) All of the above statements are true.

Answer: B

When water is heated, bubbles form in the water. Is this evidence of a chemical reaction? Why?

When water is heated, bubbles form in the water. Is this evidence of a chemical reaction? Why?

A) No, boiling water is a physical change.
B) Yes, the formation of a gas is evidence of a chemical reaction.
C) No, the formation of gas bubbles is a secondary chemical reaction which is ignored.
D) Yes, the formation of a gas is proof a new compound has been made.
E) none of the above

Answer: A

Which of the following is NOT typically a sign of a chemical reaction?

Which of the following is NOT typically a sign of a chemical reaction?

A) absorbing heat when chemicals are contacted with each other
B) emission of heat when chemicals are contacted with each other
C) emission of light when chemicals are contacted with each other
D) absorbing light when chemicals are contacted with each other
E) All of the above are signs of a chemical reaction.

Answer: D

Which of the following is NOT evidence that a chemical reaction has occurred?

Which of the following is NOT evidence that a chemical reaction has occurred?

A) color change when chemicals are contacted with each other
B) solid formation when chemicals are contacted with each other
C) gas formation when chemicals are contacted with each other
D) emission of light when chemicals are contact with each other
E) All of the above are evidence of a chemical reaction.

Answer: E

A reaction in which a substance reacts with oxygen, emitting heat and forming oxygen-containing compounds is an example of a(n):

A reaction in which a substance reacts with oxygen, emitting heat and forming oxygen-containing compounds is an example of a(n):

A) acid-base reaction.
B) combustion reaction.
C) precipitation reaction.
D) gas evolution reaction.
E) none of the above

Answer: B

A reaction which forms a solid product is an example of a(n):

A reaction which forms a solid product is an example of a(n):

A) oxidation-reduction reaction.
B) combustion reaction.
C) precipitation reaction.
D) gas evolution reaction.
E) none of the above

Answer: C

A reaction which forms a gaseous product is an example of a(n)________.

A reaction which forms a gaseous product is an example of a(n)________.

A) oxidation-reduction reaction
B) combustion reaction
C) precipitation reaction
D) gas evolution reaction
E) none of the above

Answer: D

It has been shown that the ozone molecule (O3) can be formed when a single oxygen atom (O) adds to a molecule of oxygen (O2), so this type of reaction is known as a double displacement reaction.

It has been shown that the ozone molecule (O3) can be formed when a single oxygen atom (O) adds to a molecule of oxygen (O2), so this type of reaction is known as a double displacement reaction.

Answer: false

The reaction 2 KClO3 ? 2 KCl + 3 O2 would be correctly classified as a decomposition reaction.

The reaction 2 KClO3 ? 2 KCl + 3 O2 would be correctly classified as a decomposition reaction.

Answer: true

Decomposition reactions usually require energy to initiate the reaction.

Decomposition reactions usually require energy to initiate the reaction.

Answer: true

Combustion reactions emit heat and so can be classified as endothermic.

Combustion reactions emit heat and so can be classified as endothermic.

Answer: false

In an oxidation-reduction reaction, if one substance loses electrons, then another substance must gain electrons.

In an oxidation-reduction reaction, if one substance loses electrons, then another substance must gain electrons.

Answer: true

Evidence of a redox reaction is when one substance transfers protons to another substance.

Evidence of a redox reaction is when one substance transfers protons to another substance.

Answer: false

Evidence of a redox reaction is when a substance reacts with elemental oxygen.

Evidence of a redox reaction is when a substance reacts with elemental oxygen.

Answer: true

An oxidation-reduction reaction must involve reaction with oxygen.

An oxidation-reduction reaction must involve reaction with oxygen.

Answer: false

The net ionic equation for the reaction of sodium hydroxide plus hydrochloric acid is Na+ + Cl- > NaCl-

The net ionic equation for the reaction of sodium hydroxide plus hydrochloric acid is Na+ + Cl- > NaCl-

Answer: false

Carbon dioxide gas is a product when an acid reacts with a carbonate or a bicarbonate.

Carbon dioxide gas is a product when an acid reacts with a carbonate or a bicarbonate.

Answer: true

An acid-base reaction always produces a salt plus carbon dioxide.

An acid-base reaction always produces a salt plus carbon dioxide.

Answer: false

One of the characteristics of an acid-base reaction is that this type of reaction forms water.

One of the characteristics of an acid-base reaction is that this type of reaction forms water.

Answer: true

Mixing HNO3 (aq) and NaHCO3 (aq) will produce carbon dioxide gas as a product.

Mixing HNO3 (aq) and NaHCO3 (aq) will produce carbon dioxide gas as a product.

Answer: true

A spectator ion is one that does not actively participate in a chemical reaction.

A spectator ion is one that does not actively participate in a chemical reaction.

Answer: true

A net ionic equation shows all ionic species that are present in solution.

A net ionic equation shows all ionic species that are present in solution.

Answer: false

We remove the spectator ions from the complete ionic equation to form the net ionic equation.

We remove the spectator ions from the complete ionic equation to form the net ionic equation.

Answer: true

A precipitate will form when you mix solutions of potassium chloride and lead nitrate.

A precipitate will form when you mix solutions of potassium chloride and lead nitrate.

Answer: true

A precipitation reaction will occur when sodium chloride is mixed with potassium nitrate.

A precipitation reaction will occur when sodium chloride is mixed with potassium nitrate.

Answer: false

The key to predicting a precipitation reaction is the formation of an insoluble compound from soluble compounds.

The key to predicting a precipitation reaction is the formation of an insoluble compound from soluble compounds.

Answer: true

A precipitation reaction occurs when water is formed as a product.

A precipitation reaction occurs when water is formed as a product.

Answer: false

Mixing two aqueous solutions will always result in formation of a precipitate.

Mixing two aqueous solutions will always result in formation of a precipitate.

Answer: false

Precipitation reactions always occur when two aqueous solutions are mixed.

Precipitation reactions always occur when two aqueous solutions are mixed.

Answer: false

Cl-, Br-, and I- are mostly insoluble.

Cl-, Br-, and I- are mostly insoluble.

Answer: false

Li+, Na+, K+ and NH4+ compounds are soluble.

Li+, Na+, K+ and NH4+ compounds are soluble.

Answer: true

When compounds containing polyatomic ions dissolve, the polyatomic ions usually dissolve as intact units.

When compounds containing polyatomic ions dissolve, the polyatomic ions usually dissolve as intact units.

Answer: true

An insoluble compound will completely dissolve in water.

An insoluble compound will completely dissolve in water.

Answer: false

A strong electrolyte solution contains ionic compounds that completely dissociate in water.

A strong electrolyte solution contains ionic compounds that completely dissociate in water.

Answer: true

An aqueous solution is a homogeneous mixture of a substance with water and should be designated with the (l) abbreviation.

An aqueous solution is a homogeneous mixture of a substance with water and should be designated with the (l) abbreviation.

Answer: false

All ionic compounds dissolve in water.

All ionic compounds dissolve in water.

Answer: false

The following equation IS balanced: HNO3 + NaHSO3 ? NaNO3 + H2O + SO2

The following equation IS balanced: HNO3 + NaHSO3 ? NaNO3 + H2O + SO2

Answer: true

The following equation IS balanced: 2 C4H10O + 13 O2 ? 8 CO2 + 10 H2O

The following equation IS balanced: 2 C4H10O + 13 O2 ? 8 CO2 + 10 H2O

Answer: false

The following reaction IS balanced: BaCl2 + H2SO4 ? 2HCl + BaSO4

The following reaction IS balanced: BaCl2 + H2SO4 ? 2HCl + BaSO4

Answer: true

The following equation IS balanced: CH4 + 2O2 ? CO2 + H2O

The following equation IS balanced: CH4 + 2O2 ? CO2 + H2O

Answer: false

When balancing a chemical equation you may alter the coefficients but not the subscripts in the equation.

When balancing a chemical equation you may alter the coefficients but not the subscripts in the equation.

Answer: true

Bubbles in water that appear during boiling show that a chemical reaction is occurring.

Bubbles in water that appear during boiling show that a chemical reaction is occurring.

Answer: false

The formation of a new solid or gas is evidence of a chemical reaction.

The formation of a new solid or gas is evidence of a chemical reaction.

Answer: true

The formation of a gas is evidence of a chemical reaction while the emission of light is not.

The formation of a gas is evidence of a chemical reaction while the emission of light is not.

Answer: false

Color change is evidence that a chemical reaction has occurred.

Color change is evidence that a chemical reaction has occurred.

Answer: true

Combustion reactions are a subcategory of oxidation-reduction reactions.

Combustion reactions are a subcategory of oxidation-reduction reactions.

Answer: true

The reaction of baking soda and vinegar to produce carbon dioxide gas is an example of a precipitation reaction.

The reaction of baking soda and vinegar to produce carbon dioxide gas is an example of a precipitation reaction.

Answer: false

When a molecule has four electron groups with none of them lone pairs, the molecular geometry will be:

When a molecule has four electron groups with none of them lone pairs, the molecular geometry will be:

A) linear
B) bent
C) trigonal pyramidal
D) tetrahedral
E) none of the above

Answer: D

How many lone electron pairs does the ClO (-1 charged) polyatomic anion have?

How many lone electron pairs does the ClO (-1 charged) polyatomic anion have?

A) one
B) three
C) six
D) two
E) none of the above

Answer: C

How does soap work?

How does soap work?

A) Soap works by breaking grease molecules into smaller molecules that dissolve in water.
B) Soap works by making water into a nonpolar liquid which grease can dissolve in.
C) Soap works by having a polar end and a nonpolar end which allows the water and oil to interact indirectly.
D) Soap works by having a polar end which attaches to the grease molecule and polarizes it and turns the grease molecule into another soap molecule. This is a chain reaction.
E) none of the above

Answer: C

Which compound below is a polar molecule AND has a linear molecular geometry?

Which compound below is a polar molecule AND has a linear molecular geometry?

A) CO
B) CO2
C) CH4
D) H2O
E) none of the above

Answer: A

Consider the following electronegativity values: H=2.1, Cl= 3.0, F=4.0 Which molecule below would you expect to have the more polar bond?

Consider the following electronegativity values: H=2.1, Cl= 3.0, F=4.0
Which molecule below would you expect to have the more polar bond?

A) H2
B) Cl2
C) F2
D) HCl
E) HF

Answer: E

The electronegativity value for Mg is 1.2 and the value for O is 3.5. Based on these values, what type of bond is expected for a compound formed between Mg and O?

The electronegativity value for Mg is 1.2 and the value for O is 3.5. Based on these values, what type of bond is expected for a compound formed between Mg and O?

A) ionic
B) pure covalent
C) polar covalent
D) not enough information
E) none of the above

Answer: A

The electronegativity value for N is 3.0 and that for O is 3.5. Based on these values, which of the following statements is True about the compound NO?

The electronegativity value for N is 3.0 and that for O is 3.5. Based on these values, which of the following statements is True about the compound NO?

A) NO is an ionic compound.
B) NO is a pure covalent compound.
C) NO is a polar covalent compound.
D) There is not enough enough information to determine the nature of NO.
E) None of the above statements is True.

Answer: C

Which of the following statements are True about the BF3 molecule?

Which of the following statements are True about the BF3 molecule?

A) BF3 has a trigonal planar molecular geometry.
B) BF3 violates the octet rule for the central atom.
C) BF3 is nonpolar.
D) All of the above statements are True.
E) None of the above are True.

Answer: D

Which of the following statements about the water molecule is True?

Which of the following statements about the water molecule is True?

A) A water molecule has two dipole moments and they cancel each other.
B) A water molecule is symmetrical and therefore is nonpolar.
C) A water molecule is asymmetric and therefore is polar.
D) The electronegativities of hydrogen and oxygen are equal and therefore a water molecule is nonpolar.
E) none of the above

Answer: C

Which of the following statements is True for the covalent molecule HCl?

Which of the following statements is True for the covalent molecule HCl?

A) Chlorine is more electronegative and the shared electron pair is likely to be found on the hydrogen atom.
B) Chlorine is more electronegative and the shared electron pair is likely to be found on the chlorine atom.
C) Hydrogen is more electronegative and the shared electron pair is likely to be found on the hydrogen atom.
D) Hydrogen is more electronegative and the shared electron pair is likely to be found on the chlorine atom.
E) none of the above

Answer: B

Which compound listed below will dissolve in carbon tetrachloride, CCl4?

Which compound listed below will dissolve in carbon tetrachloride, CCl4?

A) NaCl
B) CS2
C) NH3
D) all of the compounds
E) none of the compounds

Answer: B

Which compound listed below will dissolve in NH3?

Which compound listed below will dissolve in NH3?

A) H2S
B) CO2
C) O2
D) all of the compounds
E) none of the compounds

Answer: A

Which compound listed below will dissolve in water?

Which compound listed below will dissolve in water?

A) CCl4
B) SiO2
C) NH3
D) all of the compounds
E) none of the compounds

Answer: C

Which molecule listed below is a nonpolar molecule?

Which molecule listed below is a nonpolar molecule?

A) CCl4
B) CO2
C) BH3
D) all of the compounds
E) none of the compounds

Answer: D

Which substance listed below is a polar molecule?

Which substance listed below is a polar molecule?

A) NH4+
B) Cl2O
C) SiCl4
D) all of the compounds
E) none of the compounds

Answer: B

Which molecule listed below is a polar molecule?

Which molecule listed below is a polar molecule?

A) NH3
B) H2O
C) HCN
D) all of the compounds
E) none of the compounds

Answer: D

Which molecule listed below has a polar covalent bond?

Which molecule listed below has a polar covalent bond?

A) NaCl
B) H2O
C) H2
D) all of the compounds
E) none of the compounds

Answer: B

Which molecule listed below has a nonpolar covalent bond?

Which molecule listed below has a nonpolar covalent bond?

A) NaCl
B) H2O
C) H2
D) all of the compounds
E) none of the compounds

Answer: C

Which term matches the definition: The ability of an element to attract electrons within a covalent bond?

Which term matches the definition: The ability of an element to attract electrons within a covalent bond?

A) coulombic attraction
B) dipole moment
C) polar covalent
D) nonpolar covalent
E) electronegativity

Answer: E

The elements with the highest electronegativity values tend to be found in the:

The elements with the highest electronegativity values tend to be found in the:

A) upper right-side of the periodic table.
B) lower right-side of the periodic table.
C) upper left-side of the periodic table.
D) lower left-side of the periodic table.
E) center of the periodic table.

Answer: A

Which term matches the definition: A separation of charge within a bond?

Which term matches the definition: A separation of charge within a bond?

A) coulombic attraction
B) dipole moment
C) pure covalent
D) nonpolar covalent
E) electronegativity

Answer: B

Which of the following has a tetrahedral electron geometry and a trigonal pyramidal molecular geometry?

Which of the following has a tetrahedral electron geometry and a trigonal pyramidal molecular geometry?

A) Br2O
B) GeH4
C) SO2
D) PF3
E) none of the above

Answer: D

The electron geometry and the molecular geometry of water are, respectively:

The electron geometry and the molecular geometry of water are, respectively:

A) trigonal planar, bent.
B) tetrahedral, tetrahedral.
C) tetrahedral, trigonal pyramidal.
D) tetrahedral, bent.
E) none of the above

Answer: D

The electron geometry and the molecular geometry of ammonia (NH3) are, respectively:

The electron geometry and the molecular geometry of ammonia (NH3) are, respectively:

A) trigonal planar, bent.
B) tetrahedral, tetrahedral.
C) tetrahedral, trigonal pyramidal.
D) tetrahedral, bent.
E) none of the above

Answer: C

What is the molecular geometry of NH4+?

What is the molecular geometry of NH4+?

A) bent
B) linear
C) tetrahedral
D) trigonal pyramidal
E) not enough information

Answer: C

What is the molecular geometry of SCl2?

What is the molecular geometry of SCl2?

A) bent
B) linear
C) tetrahedral
D) trigonal pyramidal
E) not enough information

Answer: A

What is the molecular geometry of CCl4?

What is the molecular geometry of CCl4?

A) bent
B) linear
C) tetrahedral
D) trigonal pyramidal
E) not enough information

Answer: C

What is the molecular geometry of SiH4?

What is the molecular geometry of SiH4?

A) bent
B) linear
C) tetrahedral
D) trigonal pyramidal
E) not enough information

Answer: C

What is the molecular geometry of carbon dioxide, CO2?

What is the molecular geometry of carbon dioxide, CO2?

A) bent
B) linear
C) tetrahedral
D) trigonal pyramidal
E) not enough information

Answer: B

Which of the following compounds would have a linear molecular geometry?

Which of the following compounds would have a linear molecular geometry?

1. N2
2. H2S
3. CO2



A) 1 and 2 only
B) 1 and 3 only
C) 2 and 3 only
D) 1,2 and 3
E) neither 1, 2,or 3

Answer: B

What is the molecular geometry of ozone, O3?

What is the molecular geometry of ozone, O3?

A) bent
B) linear
C) tetrahedral
D) trigonal pyramidal
E) not enough information

Answer: A

What is the molecular geometry if you have a double bond, a single bond and 1 lone pair around the central atom?

What is the molecular geometry if you have a double bond, a single bond and 1 lone pair around the central atom?

A) bent
B) linear
C) tetrahedral
D) trigonal pyramidal
E) not enough information

Answer: A

What is the molecular geometry if you have 4 single bonds around the central atom?

What is the molecular geometry if you have 4 single bonds around the central atom?

A) bent
B) linear
C) tetrahedral
D) trigonal pyramidal
E) not enough information

Answer: C

What is the molecular geometry if you have 3 single bonds and 1 lone pair around the central atom?

What is the molecular geometry if you have 3 single bonds and 1 lone pair around the central atom?

A) bent
B) linear
C) tetrahedral
D) trigonal pyramidal
E) not enough information

Answer: D

What is the electron geometry if you have 3 electron groups around the center atom?

What is the electron geometry if you have 3 electron groups around the center atom?

A) linear
B) trigonal planar
C) tetrahedral
D) trigonal bipyramidal
E) not enough information

Answer: B

What is the electron geometry if you have 2 electron groups around the center atom?

What is the electron geometry if you have 2 electron groups around the center atom?

A) linear
B) trigonal planar
C) tetrahedral
D) trigonal bipyramidal
E) not enough information

Answer: A

What is the electron geometry if you have 4 electron groups around the center atom?

What is the electron geometry if you have 4 electron groups around the center atom?

A) linear
B) trigonal planar
C) tetrahedral
D) trigonal bipyramidal
E) not enough information

Answer: C

Which of the following is considered a single electron group?

Which of the following is considered a single electron group?

A) a lone pair of electrons
B) a single bond
C) a double bond
D) a triple bond
E) all of the above

Answer: E

What is the angle between electron groups in the tetrahedral geometry?

What is the angle between electron groups in the tetrahedral geometry?

A) 90°
B) 109.5°
C) 120°
D) 180°
E) not enough information

Answer: B

What is the angle between electron groups in the trigonal planar electron geometry?

What is the angle between electron groups in the trigonal planar electron geometry?

A) 90°
B) 109.5°
C) 120°
D) 180°
E) not enough information

Answer: C

What is the angle between electron groups in the linear electron geometry?

What is the angle between electron groups in the linear electron geometry?

A) 90°
B) 109.5°
C) 120°
D) 180°
E) not enough information

Answer: D

Which one of the following molecules is NOT capable of having resonance structures?

Which one of the following molecules is NOT capable of having resonance structures?

A) SeO2
B) H2O
C) SO2
D) O3
E) none of the above

Answer: B

Consider the Lewis structures for the compound SO3 and the polyatomic ions SO32- and SO42-. Which of these must exist as a set of resonance structures?

Consider the Lewis structures for the compound SO3 and the polyatomic ions SO32- and SO42-. Which of these must exist as a set of resonance structures?

A) SO3 only
B) SO32- only
C) SO42- only
D) all of these show resonance
E) none of these show resonance

Answer: A

Which of the following compounds have resonance structures?

Which of the following compounds have resonance structures?

A) CH4
B) H2O
C) NH3
D) O3
E) None of the compounds have resonance structures.

Answer: D

Which set shows the correct resonance structures for SeO2?

Which set shows the correct resonance structures for SeO2?

A) :--: ? ==
B) :=-: ? : -=:
C) := Se =? : O = Se-:? :-Se = O :
D) =-: ? :-=
E) SeO2 does not have a resonance structure.

Answer: D

Which symbol should be used between two structures that represent resonance structures?

Which symbol should be used between two structures that represent resonance structures?

A) ?
B) ?
C) ?
D) =
E) none of the above

Answer: C

Which molecule below would have a Lewis structure that is an exception to the octet rule?

Which molecule below would have a Lewis structure that is an exception to the octet rule?

A) BH3
B) NO
C) SI6
D) PF5
E) all of these

Answer: E

The correct Lewis structure for BF3 would have exactly:

The correct Lewis structure for BF3 would have exactly:

A) 1 double bond.
B) 2 double bonds.
C) 1 triple bond.
D) no double bonds.
E) none of the above

Answer: D

What is the correct Lewis structure for CN?

What is the correct Lewis structure for CN?

A) [C-N]?
B) [:-:]?
C) [=:]?
D) [: C = N :]?
E) none of the above

Answer: D

The Lewis structure, [:-=] best represents:

The Lewis structure, [:-=] best represents:

A) NO2+
B) NO2-
C) NO2
D) both NO2+ and NO2-
E) answers A, B, and C

Answer: B

What is the correct Lewis structure for CO2?

What is the correct Lewis structure for CO2?

A) : --:
B) : ==:
C) : = C =:
D) : = C = :
E) none of the above

Answer: D

The central atom in the chlorite anion, ClO2- is surrounded by:

The central atom in the chlorite anion, ClO2- is surrounded by:

A) one bonding and three unshared pairs of electrons.
B) two bonding and two unshared pairs of electrons.
C) two bonding and one unshared pair of electrons.
D) two double bonds and no unshared pairs of electrons.
E) none of the above

Answer: B

The central atom in the chlorate anion, ClO3- is surrounded by:

The central atom in the chlorate anion, ClO3- is surrounded by:

A) two bonding and two unshared pairs of electrons.
B) one bonding and three unshared pairs of electrons.
C) three bonding and one unshared pair of electrons.
D) two double bonds and no unshared pairs of electrons.
E) none of the above.

Answer: C

The total number of electrons to be counted for the Lewis structure of the PO43- polyatomic ion is:

The total number of electrons to be counted for the Lewis structure of the PO43- polyatomic ion is:

A) 8.
B) 26.
C) 29.
D) 32.
E) none of the above

Answer: D

How many valence electrons are in the nitrate ion?

How many valence electrons are in the nitrate ion?

A) 18
B) 22
C) 23
D) 24
E) 26

Answer: D

Which sequence below represents the proper order of increasing bond strength?

Which sequence below represents the proper order of increasing bond strength?

A) single < double < triple
B) double < single < triple
C) single < triple < double
D) triple < double < single
E) none of the above

Answer: A

The Lewis structure for carbon monoxide is C=O This structures shows:

The Lewis structure for carbon monoxide is C=O This structures shows:

A) 4 lone pairs and 1 bonding pair.
B) 4 lone pairs and 3 bonding pairs.
C) 2 lone pairs and 3 bonding pairs.
D) 2 lone pairs and 1 bonding pair.
E) none of the above

Answer: C

How many bonding electrons are in the Lewis structure of carbon monoxide, CO?

How many bonding electrons are in the Lewis structure of carbon monoxide, CO?

A) 2
B) 3
C) 4
D) 6
E) none of the above

Answer: D

How many bonding electrons are in the Lewis structure of N2?

How many bonding electrons are in the Lewis structure of N2?

A) 2

B) 3
C) 4
D) 6
E) none of the above

Answer: D

What is the correct Lewis structure for N2?

What is the correct Lewis structure for N2?

A) N-N
B) :-:
C) =
D) : N = N :
E) none of the above

Answer: D

What is the correct Lewis structure for O2?

What is the correct Lewis structure for O2?

A) O-O
B) :-:
C) =
D) : O = O :
E) none of the above

Answer: C

What is the correct Lewis structure for Br2?

What is the correct Lewis structure for Br2?

A) Br-Br
B) : - :
C) =
D) : Br = Br :
E) none of the above

Answer: B

What is the correct Lewis structure for water?

What is the correct Lewis structure for water?

A) H-::-H
B) :--:
C) H==H
D) H--H
E) none of the above

Answer: D

When a nonmetal bonds with a nonmetal:

When a nonmetal bonds with a nonmetal:

A) a molecular compound forms.
B) a covalent bond is involved.
C) electrons are shared.
D) all of the above are Answer: True
E) none of the above

Answer: D

The Lewis model predicts that the formula for a compound between potassium and sulfur is:

The Lewis model predicts that the formula for a compound between potassium and sulfur is:

A) KS
B) K2S
C) KS2
D) K3S
E) none of the above

Answer: B

The Lewis model predicts that the formula for a compound between barium and sulfur is:

The Lewis model predicts that the formula for a compound between barium and sulfur is:

A) BaS
B) Ba2S
C) BaS2
D) BaS3
E) none of the above

Answer: A

The Lewis model predicts that the formula for a compound between fluorine and calcium is:

The Lewis model predicts that the formula for a compound between fluorine and calcium is:

A) CaF
B) Ca2F
C) CaF2
D) CaF3
E) none of the above

Answer: C

The Lewis model predicts that the formula of a compound formed between bromine and aluminum is:

The Lewis model predicts that the formula of a compound formed between bromine and aluminum is:

A) AlBr
B) Al2Br
C) AlBr3
D) AlBr2
E) none of the above

Answer: C

Which Lewis structure below correctly represents the compound formed between magnesium and sulfur?

Which Lewis structure below correctly represents the compound formed between magnesium and sulfur?

A) Mg? [::]?
B) Mg? [::]?2 Mg?
C) [::]? Mg?2 [::]?
D) Mg?2 [::]?2
E) none of the above

Answer: D

Which Lewis structure below correctly represents KCl?

Which Lewis structure below correctly represents KCl?

A) K? []?
B) K? [::]?
C) K ::
D) :: ::
E) none of the above

Answer: B

Which of the following statements about Lewis structures is False?

Which of the following statements about Lewis structures is False?

A) An octet is when an atom has 8 valence electrons.
B) A duet is a stable electron configuration for helium.
C) An ionic bond occurs when electrons are transferred.
D) A covalent bond occurs when electrons are shared.
E) All of the above statements are Answer: True.

Answer: E

Water and oil do not mix because water molecules are nonpolar and molecules that compose oil are generally polar.

Water and oil do not mix because water molecules are nonpolar and molecules that compose oil are generally polar.

Answer: False

The compound H2S contains polar bonds but the molecule is nonpolar.

The compound H2S contains polar bonds but the molecule is nonpolar.

Answer: False

When you have 4 electron groups, the electron geometry is tetrahedral.

When you have 4 electron groups, the electron geometry is tetrahedral.

Answer: True

When you have 4 electron groups and none of them are lone pairs, the molecular geometry is trigonal pyramidal.

When you have 4 electron groups and none of them are lone pairs, the molecular geometry is trigonal pyramidal.

Answer: False

When you have 4 electron groups and 1 of them is a lone pair, the molecular geometry is bent.

When you have 4 electron groups and 1 of them is a lone pair, the molecular geometry is bent.

Answer: False

When you have 2 electron groups and none are lone pairs, the molecular geometry is linear.

When you have 2 electron groups and none are lone pairs, the molecular geometry is linear.

Answer: True

The electron geometry of a molecule is never the same as its molecular geometry.

The electron geometry of a molecule is never the same as its molecular geometry.

Answer: False

It is important to identify lone pairs around a central atom because they do not repel other electron groups.

It is important to identify lone pairs around a central atom because they do not repel other electron groups.

Answer: False

The VSEPR theory predicts that the H-C-H angle in CH4 measures 120°.

The VSEPR theory predicts that the H-C-H angle in CH4 measures 120°.

Answer: False

The VSEPR theory predicts that the angle between the central carbon atom and the two oxygen atoms in CO2 measures 180°.

The VSEPR theory predicts that the angle between the central carbon atom and the two oxygen atoms in CO2 measures 180°.

Answer: True

Carbon monoxide contains resonance Lewis structures.

Carbon monoxide contains resonance Lewis structures.

Answer: False

Resonance structures are the best representation we can draw but do not accurately reflect the Answer: True structure.

Resonance structures are the best representation we can draw but do not accurately reflect the Answer: True structure.

Answer: True

Boron forms compounds that violate the octet rule.

Boron forms compounds that violate the octet rule.

Answer: True

The ammonium ion contains 10 valence electrons.

The ammonium ion contains 10 valence electrons.

Answer: False

The sulfate ion contains 28 valence electrons.

The sulfate ion contains 28 valence electrons.

Answer: False

When calculating the number of electrons for the Lewis structure of a polyatomic ion, you must add one electron for each negative charge and subtract one electron for each positive charge.

When calculating the number of electrons for the Lewis structure of a polyatomic ion, you must add one electron for each negative charge and subtract one electron for each positive charge.

Answer: True

The correct Lewis structure for CO2 shows that the carbon atom has two sets of lone pair electrons.

The correct Lewis structure for CO2 shows that the carbon atom has two sets of lone pair electrons.

Answer: False

The correct Lewis structure for CO2 shows that the molecule contains two double bonds.

The correct Lewis structure for CO2 shows that the molecule contains two double bonds.

Answer: True

When calculating the number of electrons for the Lewis structure of a polyatomic ion, subtract one electron for each negative charge.

When calculating the number of electrons for the Lewis structure of a polyatomic ion, subtract one electron for each negative charge.

Answer: False

The triple bond present in diatomic nitrogen, N2, is what makes this molecule so reactive.

The triple bond present in diatomic nitrogen, N2, is what makes this molecule so reactive.

Answer: False

The double bond is shorter and stronger than a single bond.

The double bond is shorter and stronger than a single bond.

Answer: True

The Lewis structure for O2 contains a triple bond.

The Lewis structure for O2 contains a triple bond.

Answer: False

The structure H=H is a proper representation of the bonding in the H2 molecule.

The structure H=H is a proper representation of the bonding in the H2 molecule.

Answer: False

The Lewis structure of water has two sets of lone pair electrons.

The Lewis structure of water has two sets of lone pair electrons.

Answer: True

Lewis theory predicts that the formula for a compound made of aluminum and phosphorus is AlP.

Lewis theory predicts that the formula for a compound made of aluminum and phosphorus is AlP.

Answer: True

The Lewis theory predicts that the formula for a compound made of sodium and fluorine is NaF.

The Lewis theory predicts that the formula for a compound made of sodium and fluorine is NaF.

Answer: True

The Lewis theory predicts that the formula for a compound of magnesium and sulfur is MgS2.

The Lewis theory predicts that the formula for a compound of magnesium and sulfur is MgS2.

Answer: False

Chlorine has 8 valence electrons in the Lewis structure for KCl.

Chlorine has 8 valence electrons in the Lewis structure for KCl.

Answer: True

The correct Lewis structure for potassium in KCl is K+.

The correct Lewis structure for potassium in KCl is K+.

Answer: True

A correct Lewis structure for an atom of carbon would have eight dots surrounding the symbol of the element.

A correct Lewis structure for an atom of carbon would have eight dots surrounding the symbol of the element.

Answer: False

Having eight valence electrons is very stable and is called an octet.

Having eight valence electrons is very stable and is called an octet.

Answer: True

Lewis structures only use the valence electrons in determining the bonding.

Lewis structures only use the valence electrons in determining the bonding.

Answer: True

The Lewis structure of oxygen should have 8 valence electrons.

The Lewis structure of oxygen should have 8 valence electrons.

Answer: False

A chemical bond is classified as a covalent bond if it involves the transfer of electrons.

A chemical bond is classified as a covalent bond if it involves the transfer of electrons.

Answer: False

Li : is the proper Lewis structure (dot structure) for lithium.

Li : is the proper Lewis structure (dot structure) for lithium.

Answer: False

Drugs to fight HIV have been developed using bonding theory models.

Drugs to fight HIV have been developed using bonding theory models.

Answer: True

Bonding theories are used to predict how atoms bond together to form molecules.

Bonding theories are used to predict how atoms bond together to form molecules.

Answer: True

The Heisenberg Uncertainty Principle states that

The Heisenberg Uncertainty Principle states that

a. It is impossible to determine accurately both the position and momentum of an electron simultaneously.
b. No two electrons in the same atom can have the same set of four quantum numbers.
c. electrons of atoms in their ground states enter energetically equivalent sets of orbitals singly before they pair up in any orbital of the set.
d. Two atoms of the same element must have the same number of protons.
e. Charged atoms (ions) must generate a magnetic field when they are in motion.

Answer: A

Which of the following statements is not consistent with the Bohr theory?

Which of the following statements is not consistent with the Bohr theory?

a. An electron may move to a lower energy orbit by emitting radiation of frequency proportional to the energy difference between the two orbits.
b. The energy of an electron is quantized
c. An atom has a number of discrete energy levels (orbits) in which an electron can exist as long as it continually emits radiation of a definite energy
d. An electron moves in a circular orbit around the nucleus
e. An electron may move to a higher energy orbit by absorbing radiation of frequency proportional to the energy difference between the two orbits.

Answer: C

Isotopes are atoms of the same element that

Isotopes are atoms of the same element that

a. have different numbers of protons
b. have different number of electrons
c. have different nuclear charges
d. have different atomic numbers
e. have different number of neutrons





Answer: E

The atomic number of an element gives the number of _____ and _____ in the atom while the mass number gives the total number of _____ and ______.

The atomic number of an element gives the number of _____ and _____ in the atom while the mass number gives the total number of _____ and ______.

a. protons; electrons; neutrons; electrons
b. neutrons; electrons; neutrons; protons
c. protons; electrons; neutrons; protons
d. neutrons; protons; neutrons; electrons
e. neutrons; electrons; protons; electrons



Answer: C

The number of electrons in a neutral atom of an element is always equal to the _____ of the element.

The number of electrons in a neutral atom of an element is always equal to the _____ of the element.

a. Avogadro's number
b. atomic number
c. atomic mass unit
d. mass number
e. isotope number



Answer: B

In the Rutherford gold foil experiment, the fact that most of the alpha particles were not deflected as they passed through the gold foil indicates that

In the Rutherford gold foil experiment, the fact that most of the alpha particles were not deflected as they passed through the gold foil indicates that

a. the nucleus is positively charged.
b. the atom is mostly empty space
c. gold is very dense
d.atoms are solid spheres touching each other in the solid state
e. none of these are correct



Answer: B

Which of these physical changes would require the addition of energy (endothermic process)?

Which of these physical changes would require the addition of energy (endothermic process)?

a. boiling a liquid
b. freezing a liquid
c. condensing a gas
d. deposition, gas to solid
e. none of these




Answer: A

The same amount of heat is added to a 25-g sample of each of the following metal. If each of the metals was initially at 20.0 degrees C, which metal will reach the highest temperature?

The same amount of heat is added to a 25-g sample of each of the following metal. If each of the metals was initially at 20.0 degrees C, which metal will reach the highest temperature?

a. copper 0.385 J/g*degreesC
b. beryllium 1.82 J/g*degreesC
c. gold 0.129 J/g*degreesC
d. calcium 0.653J/g*degreesC
e. nickel 0.444 J/g*degrees C



Answer: C

Water is always 11.1% hydrogen and 88.9% oxygen by mass. This is a statement of the

Water is always 11.1% hydrogen and 88.9% oxygen by mass. This is a statement of the 

a. Law of Conservation of Matter
b. Law of Conservation of Matter and Energy
c. Law of Multiple Proportions
d. Law of Definite Proportions
e. none of these

Answer: D

Which of these physical changes would require the liberation of energy, exothermic?

Which of these physical changes would require the liberation of energy, exothermic?

a. melting point
b. boiling point
c. condensation of steam to form liquid
d. sublimation from a solid to a gas

Answer: C

Identify which of the following properties of methane would be observed only with a change in composition

Identify which of the following properties of methane would be observed only with a change in composition

a. The boiling point is -161.5degreesC
b. The melting point is -182.5degreesC
c. The density is 6.67 x 10^-4 g/cm^3
d. It dissolves slightly in water
e. Carbon dioxide forms when it burns

Answer: E

Dalton's Atomic Theory included all of the ideas listed below except:

Dalton's Atomic Theory included all of the ideas listed below except:

a. Compounds are formed when atoms of different elements combine with one another in small whole-number ratios
b. An element is composed of very small particles called protons, neutrons, and electrons
c. Atoms cannot be created or destroyed
d. All atoms of a given element have identical properties.
e. All atoms of a given element have properties that differ from those of other elements.

Answer: B

Iodine is most likely to form an ionic compound with ______ (circle all that apply).

Iodine is most likely to form an ionic compound with ______ (circle all that apply).

a. Mg
b. Cl
c. Pb
d. Si
e. N


Answer: A & C.

Chlorine is most likely to form a covalent compound with ______ (circle all that apply).

Chlorine is most likely to form a covalent compound with ______ (circle all that apply).

a. O
b. N
c. C
d. Li
e. F

Answer: A, B, C & E.

Which pair of elements below would be least likely to form an ionic bond between them?

Which pair of elements below would be least likely to form an ionic bond between them?

a. Cs / O
b. C / N
c. Na / S
d. Al / F
e. Mg / Br

Answer: B

Which of the following ions is not isoelectronic with the others?

Which of the following ions is not isoelectronic with the others?

a. Te2-
b. Ba2+
c. I-
d. Cs+
e. Sb3+




Answer: E

In which orbital below would an electron (on average) be closest to the nucleus?

In which orbital below would an electron (on average) be closest to the nucleus?

a. 4s
b. 2s
c. 3p
d. 5d
e. 2p





Answer: B

The number of electrons present in the p orbitals in the outermost electron shell (major energy level, n) of the halogen atom is ______.

The number of electrons present in the p orbitals in the outermost electron shell (major energy level, n) of the halogen atom is ______.

a. one
b. seven
c. six
d. two
e. five

Answer: E

An element that has four electrons in its outer shell in its ground state is _____.

An element that has four electrons in its outer shell in its ground state is _____.

a. Nb
b. S
c. Zr
d. Sn
e. Mo



Answer: D

An element has the outermost electron configuration ns2np4. The element could be______.

An element has the outermost electron configuration ns2np4. The element could be______.

a. Si
b. Ar
c. Br
d. O
e. Mn

Answer: D

The number of electrons present in the outermost electron shell of the Group VA element is:

The number of electrons present in the outermost electron shell of the Group VA element is:

a. four
b. five
c. three
d. two
e. one

Answer: B

The number of electrons in p orbitals in the highest energy levels of the Group IV A elements is ______.

The number of electrons in p orbitals in the highest energy levels of the Group IV A elements is ______.

a. three
b. one
c. two
d. four
e. six




Answer: C

The number of electrons present in the s orbitals in the outermost electron shell of the alkaline earth (Group IIA) metals is _____.

The number of electrons present in the s orbitals in the outermost electron shell of the alkaline earth (Group IIA) metals is _____.

a. three
b. four
c. one
d. five
e. two




Answer: E

All orbitals of a given degenerate set must be singly occupied before pairing begins in that set is a statement of _______.

All orbitals of a given degenerate set must be singly occupied before pairing begins in that set is a statement of _______.

Answer: the Hund's Rule

No two electrons in the same atom can have the same set of four quantum numbers is a statement of ______.

No two electrons in the same atom can have the same set of four quantum numbers is a statement of ______.

Answer: the Pauli Exclusion Principle

The principal quantum number of an orbital is n = 1. This must be a(n) _____ orbital.

The principal quantum number of an orbital is n = 1. This must be a(n) _____ orbital.

Answer:  s

Which statement about the four quantum numbers is false?

Which statement about the four quantum numbers is false?

a. ms= spin quantum number, ms= +/- 1/2
b. n= principal quantum number, n= 1,2,3,...
c. ml= magnetic quantum number, ml= (-1),...,0,...,(+1)
d. l = angular momentum quantum number, l = 0,1,2,3,...,(n+1)
e. The values of n, l, and ml describe a particular atomic orbital.



Answer: D

A(n) _____ is a region of space in which there is a high probability of finding an electron in an atom.

A(n) _____ is a region of space in which there is a high probability of finding an electron in an atom.

a. major energy level
b. core
c. shell
d. atomic orbital
e. nucleus

Answer: D

The internuclear distance at which the attractive and repulsive forces balance in a covalent bond is called the ________.

The internuclear distance at which the attractive and repulsive forces balance in a covalent bond is called the ________.

a. single bond
b. bond energy
c. bond length
d. stabilization length
e. none of these



Answer: C

What is the formula for the binary compound of gallium and chlorine?

What is the formula for the binary compound of gallium and chlorine?

a. GaCl2
b. Ga3Cl2
c. Ga2Cl3
d. GaCl3
e. GaCl



Answer: D

Consider the formation of one formula unit of AlF3 from neutral atoms. In the process, each aluminum atom ______ electron(s) and each fluorine atom ______ electron(s).

Consider the formation of one formula unit of AlF3 from neutral atoms. In the process, each aluminum atom ______ electron(s) and each fluorine atom ______ electron(s).

a. gains one; loses three
b. loses three; gains one
c. loses three; gains three
d. gains three; loses one
e. loses one; gains three



Answer: B

Magnesium and nitrogen react to form Mg3N2 an ionic compound. The magnesium ion, Mg2+, has _____ electrons in its highest occupied energy level.

Magnesium and nitrogen react to form Mg3N2 an ionic compound. The magnesium ion, Mg2+, has _____ electrons in its highest occupied energy level.

Answer: 8

Calcium and chlorine react to form CaCl2, an ionic compound. The chloride ion, Cl-, has _____electrons in its outermost occupied shell.

Calcium and chlorine react to form CaCl2, an ionic compound. The chloride ion, Cl-, has _____electrons in its outermost occupied shell.

a. 6
b. 2
c. 7
d. 18
e. 8




Answer: E

What is the hybridization of a carbon atom involved in a triple bond?

What is the hybridization of a carbon atom involved in a triple bond?

a. sp3d
b. sp3
c. sp
d. sp2
e. sp3d2




Answer: C

What is the electronic geometry for 5 regions of high electron density on a central atom?

What is the electronic geometry for 5 regions of high electron density on a central atom?

a. trigonal planar
b. octahedral
c. trigonal bipyramidal
d. tetrahedral
e. square planar




Answer: C

The electrons in the outer shell of an atom are involved in bonding. Another name for the outer shell is _____.

The electrons in the outer shell of an atom are involved in bonding. Another name for the outer shell is _____.

a. valence shell
b. VSEPR shell
c. bonding shell
d. hybridized shell
e. Lewis shell




Answer: A

When you draw a Lewis structure for CH3OCH2CH3, what is the total number of C-C single bonds?

When you draw a Lewis structure for CH3OCH2CH3, what is the total number of C-C single bonds?

a. 2
b. 1
c. 3
d. 4
e. 0



Answer: A

Draw a Lewis structure for CH3OCH2CH3. What is the total number of lone pair electrons (unshared pair electrons)?

Draw a Lewis structure for CH3OCH2CH3. What is the total number of lone pair electrons (unshared pair electrons)?

a. 3
b. 1
c. 4
d. 2
e. 0


Answer: D

Which one of the following compounds contains both ionic and covalent bonding?

Which one of the following compounds contains both ionic and covalent bonding?

a. MgO
b. KNO3
c. HCl
d. Rb3N
e. CaCl2




Answer: B

Oxyacids contains at least one H+ and an oxyanion. The " nitrous " oxyacid contains the oxyanion ________.

Oxyacids contains at least one H+ and an oxyanion. The " nitrous " oxyacid contains the oxyanion ________.

A) nitrite
B) nitrate
C) nitride
D) nitric
E) none of the above

Answer: A

What is the formula mass of magnesium nitride?

What is the formula mass of magnesium nitride?

A) 38.32
B) 90.65
C) 100.95
D) 116.33
E) none of the above

Answer: C

How many O atoms are present in sodium chlorite?

How many O atoms are present in sodium chlorite?

A) 2
B) 6
C) 4
D) 1
E) none of the above

Answer: A

How many C atoms are in ammonium acetate?

How many C atoms are in ammonium acetate?

A) 5
B) 2
C) 1
D) 3
E) none of the above

Answer: B

Suppose that in an ionic compound, "M" represents a metal that could form more than one type of ion. In the formula MF2 , the charge of the M ion would be:

Suppose that in an ionic compound, "M" represents a metal that could form more than one type of ion. In the formula MF2 , the charge of the M ion would be:

A) +2
B) -1
C) +4
D) -2
E) +1

Answer: A

Suppose that in an ionic compound, "M" represents a metal that could form more than one type of ion. In the formula MP , the charge of the M ion would be:

Suppose that in an ionic compound, "M" represents a metal that could form more than one type of ion. In the formula MP , the charge of the M ion would be:

A) +1
B) -1
C) +2
D) -3
E) +3

Answer: E

If the mass ratio of K to F in a compound is 2.06:1, how many grams of F are needed to react with 2.30 g of K?

If the mass ratio of K to F in a compound is 2.06:1, how many grams of F are needed to react with 2.30 g of K?

A) 0.877
B) 1.12
C) 0.112
D) 8.77
E) none of the above

Answer: B

What is the mass ratio of Na to S in sodium sulfide?

What is the mass ratio of Na to S in sodium sulfide?

A) 7.17
B) 55.06
C) 0.717
D) 1.43
E) none of the above

Answer: D

A compound has a formula mass of 61.98 amu and is comprised of atoms of sodium and oxygen in a definite ratio. The name of the compound described here is:

A compound has a formula mass of 61.98 amu and is comprised of atoms of sodium and oxygen in a definite ratio. The name of the compound described here is:

A) sodium monoxide.
B) disodium oxide.
C) sodium oxide.
D) sodium dioxide.
E) none of the above

Answer: C

Which of the following compounds have the smallest formula mass?

Which of the following compounds have the smallest formula mass?

A) CO2
B) SO2
C) NO2
D) SiO2
E) H2O

Answer: E

Which of the following has the largest formula mass?

Which of the following has the largest formula mass?

A) CO2
B) SO2
C) NO2
D) SiO2
E) H2O

Answer: B

What is the formula mass of copper(II) fluoride?

What is the formula mass of copper(II) fluoride?

A) 101.55
B) 146.10
C) 90.00
D) 165.10
E) none of the above

Answer: A

What is the formula mass for diboron tetrachloride?

What is the formula mass for diboron tetrachloride?

A) 127.98 amu
B) 198.89 amu
C) 234.34 amu
D) 163.43 amu
E) none of the above

Answer: D

What is the formula mass for potassium nitrate?

What is the formula mass for potassium nitrate?

A) 92.99 amu
B) 117.11 amu
C) 85.11 amu
D) 101.10 amu
E) none of the above

Answer: D

What is the formula mass of sulfurous acid?

What is the formula mass of sulfurous acid?

A) 82.08 amu
B) 98.08 amu
C) 83.09 amu
D) 66.08 amu
E) none of the above

Answer: A

A certain oxyacid is derived from the oxyanion SO32-. The formula for the oxyacid is:

A certain oxyacid is derived from the oxyanion SO32-. The formula for the oxyacid is:

A) H2SO4.
B) HSO3.
C) H2SO3.
D) H3SO3.
E) none of the above

Answer: C

What is the name of HNO2?

What is the name of HNO2?

A) nitric acid
B) nitrous acid
C) hydronitrous acid
D) hydronitric acid
E) none of the above

Answer: B

What is the name of HIO3?

What is the name of HIO3?

A) iodic acid
B) hydroioidic acid
C) hydroiodous acid
D) iodous acid
E) none of the above

Answer: A

What is the name of HI (aq)?

What is the name of HI (aq)?

A) hydroiodous acid
B) hydroiodic acid
C) iodic acid
D) iodous acid
E) none of the above

Answer: B

What is the proper name for HBr (aq)?

What is the proper name for HBr (aq)?

A) hydrobromous acid
B) hydrousbromic acid
C) hydrobromic acid
D) bromous acid
E) none of the above

Answer: C

What is the correct formula for the molecular compound hepta phosphorus octafluoride?

What is the correct formula for the molecular compound hepta phosphorus octafluoride?

A) P5F8
B) P 7F6
C) P6F7
D) P7F8
E) none of the above

Answer: D

What would the formula of diiodine pentasulfide be?

What would the formula of diiodine pentasulfide be?

A) I5S2
B) I2S5
C) I4S9
D) I2S7
E) none of the above

Answer: B

What is correct name of the compound whose formula is BF3?

What is correct name of the compound whose formula is BF3?

A) boron trifluoride
B) boron fluoride
C) monoboron trifluorine
D) boron(III) fluoride
E) none of the above

Answer: A

What is correct name of the compound whose formula is N2O4?

What is correct name of the compound whose formula is N2O4?

A) nitrogen dioxide
B) nitrogen tetroxide
C) dinitrogen oxide
D) dinitrogen tetroxide
E) none of the above

Answer: D

What is the name of the molecular compound SO3?

What is the name of the molecular compound SO3?

A) sulfur oxide
B) sulfur(IV) oxide
C) sulfur trioxide
D) sulfur tetraoxide
E) none of the above

Answer: C

What is the name of the molecular compound SF5?

What is the name of the molecular compound SF5?

A) sulfur hexafluoride
B) sulfur heptafluoride
C) monosulfur tetrafluoride
D) sulfur pentafluoride
E) none of the above

Answer: D

The name trisodium phosphate is incorrect for the compound Na3PO4 because:

The name trisodium phosphate is incorrect for the compound Na3PO4 because:

A) this compound should be called trisodium monophosphate.
B) the sodium has a negative 3 charge.
C) you cannot use a prefix for the first element in a molecular compound.
D) you cannot use a prefix for the first element of an ionic compound.
E) none of the above

Answer: D

Choose the pair of names and formulas that do NOT match.

Choose the pair of names and formulas that do NOT match.

A) copper(I) nitrate: CuNO3
B) copper(II) nitride: Cu3N2
C) copper(II) nitrate: Cu(NO3)2
D) copper(II) nitrite: Cu(NO2)2
E) all of these are correct

Answer: E

What is the correct name for the BrO4 1- ion?

What is the correct name for the BrO4 1- ion?

A) hypobromite
B) perbromate
C) bromite
D) bromate
E) none of the above

Answer: B

What is the correct formula for the hypochlorite polyatomic ion?

What is the correct formula for the hypochlorite polyatomic ion?

A) ClO
B)ClO2-
C) ClO3-
D) ClO4-
E) none of the above

Answer: A

The charge of a vanadium ion in the compound V2O5 is:

The charge of a vanadium ion in the compound V2O5 is:

A) 5+
B) 2+
C) 10+
D) 10-
E) none of the above

Answer: A

The formula for potassium chlorate is KClO3. The formula for magnesium chloride is MgCl2. What is the formula for magnesium chlorate?

The formula for potassium chlorate is KClO3. The formula for magnesium chloride is MgCl2. What is the formula for magnesium chlorate?

A) MgClO3
B) Mg2ClO3
C) Mg(ClO3)2
D) Mg2(ClO3)3
E) none of the above

Answer: C

What is the correct formula for ammonium hydrogen sulfate?

What is the correct formula for ammonium hydrogen sulfate?

A) NH4HSO4
B) (NH4)2HSO4
C) (NH4)2SO4
D) Am2HSO4
E) none of the above

Answer: A

What is the correct formula for potassium dichromate?

What is the correct formula for potassium dichromate?

A) K(CrO4)2
B) KCr2O7
C) K2CrO4
D) K2Cr2O7
E) none of the above

Answer: D

What is the formula for the acetate polyatomic ion?

What is the formula for the acetate polyatomic ion?

A) C3H2O3-
B) C2H3O22-
C) C2H3O2-
D) C2H3O
E)none of the above

Answer: C

What is the name of the compound whose formula is Na2O?

What is the name of the compound whose formula is Na2O?

A) sodium monoxide
B) disodium oxide
C) disodium monoxide
D) sodium oxide
E) none of the above

Answer: D

Which formula shown is incorrect for the name given?

Which formula shown is incorrect for the name given?

A) strontium carbonate: SrCO3
B) ammonium cyanide: NH4CN
C) potassium acetate: KC2H3O2
D) calcium nitrate: Ca(NO3)2
E) lithium sulfate: LiSO4

Answer: E

Which formula shown is incorrect for the name given?

Which formula shown is incorrect for the name given?

A) magnesium nitrite: Mg(NO2)3
B) calcium carbonate: CaCO3
C) aluminum sulfate: Al2(SO4)3
D) sodium hydrogen carbonate: NaHCO3
E) potassium hydroxide: KOH

Answer: A

What is the name of Ca(NO3)2?

What is the name of Ca(NO3)2?

A) calcium dinitrite
B) calcium nitrate
C) calcium nitride
D) calcium nitrite
E) none of the above

Answer: B

What is the name of CoS?

What is the name of CoS?

A) cobalt(II) sulfide
B) cobalt sulfide
C) cobalt monosulfide
D) cobaltous sulfur
E) none of the above

Answer: A

Which metal atom below cannot form a cation of several different charges?

Which metal atom below cannot form a cation of several different charges?

A) Cr
B) Mn
C) Fe
D) Ba
E) none of the above

Answer: D

What is the name of the compound made from lithium and oxygen?

What is the name of the compound made from lithium and oxygen?

A) lithium dioxide
B) lithium(I) oxide
C) oxygen lithide
D) lithium oxide
E) none of the above

Answer: D

What is the name of the ionic compound made of beryllium and chlorine?

What is the name of the ionic compound made of beryllium and chlorine?

A) beryllium(II) chloride
B) beryllium dichloride
C) beryllium chloride
D) monoberyllium dichloride
E) none of the above

Answer: C

A student wrote the formula for the compound aluminum phosphate as AlPO4 . What is wrong with this formula?

A student wrote the formula for the compound aluminum phosphate as AlPO4 . What is wrong with this formula?

A) The compound is not charge-neutral.
B) Aluminum is a nonmetal so it cannot form an ionic compound.
C) The formula should be Al(PO4) .
D) There cannot be three different atom types in a chemical formula.
E) Nothing is wrong with the formula.

Answer: E

What is the formula for an ionic compound made of aluminum and oxygen?

What is the formula for an ionic compound made of aluminum and oxygen?

A) AlO2
B) Al2O3
C) Al3O2
D) AlO
E) none of the above

Answer: B

The ionic compound that forms between potassium and oxygen is:

The ionic compound that forms between potassium and oxygen is:

A) K2O.
B) KO.
C) KO2.
D) K2O2.
E) none of the above

Answer: A

What is the formula for an ionic compound made of carbon and oxygen?

What is the formula for an ionic compound made of carbon and oxygen?

A) CO2
B) C2O
C) CO
D) CO3
E) Carbon and oxygen do not form an ionic compound.

Answer: E

What is the formula for an ionic compound made of magnesium and sulfur?

What is the formula for an ionic compound made of magnesium and sulfur?

A) MgS
B) MgS2
C) Mg2S
D) Mg2S3
E) none of the above

Answer: A

What is the formula for an ionic compound made of barium and nitrogen?

What is the formula for an ionic compound made of barium and nitrogen?

A) Ba3N2
B) Ba2N3
C) BaN
D) Ba2N4
E) none of the above

Answer: A

Which of the following is a molecular compound?

Which of the following is a molecular compound?

A) barium sulfide
B) calcium acetate
C) potassium hydroxide
D) nitrogen monoxide
E) none of the above

Answer: D

Which of the following species is a molecular element?

Which of the following species is a molecular element?

A) neon
B) sodium
C) chlorine
D) carbon dioxide
E) none of the above

Answer: C

Ammonium fluoride is considered which of the following?

Ammonium fluoride is considered which of the following?

A) atomic element
B) molecular element
C) molecular compound
D) ionic compound
E) none of the above

Answer: D

Fluorine is considered which of the following?

Fluorine is considered which of the following?

A) atomic element
B) molecular element
C) molecular compound
D) ionic compound
E) none of the above

Answer: B

Carbon monoxide is considered which of the following?

Carbon monoxide is considered which of the following?

A) atomic element
B) molecular element
C) molecular compound
D) ionic compound
E) none of the above

Answer: C

Which among the following elements does NOT exist as a diatomic molecule in nature?

Which among the following elements does NOT exist as a diatomic molecule in nature?

A) hydrogen
B) nitrogen
C) fluorine
D) neon
E) none of the above

Answer: D

Carbon is considered which of the following?

Carbon is considered which of the following?

A) atomic element
B) molecular element
C) molecular compound
D) ionic compound
E) none of the above

Answer: A

What is the correct formula of a compound that has ten oxygen atoms and four phosphorus atoms?

What is the correct formula of a compound that has ten oxygen atoms and four phosphorus atoms?

A) O10P4
B) 10OP4
C) 4PO10
D) P4O10
E) none of the above

Answer: D

What is the correct formula for a compound that has three oxygen atoms and one sulfur atom?

What is the correct formula for a compound that has three oxygen atoms and one sulfur atom?

A) O3S
B) SO3
C) 3OS
D) SO3
E) none of the above

Answer: B

How many of each type of atom are there in the formula (NH4)2HPO4?

How many of each type of atom are there in the formula (NH4)2HPO4?

A) N = 2, H = 9, P = 1, O = 4
B) N = 1, H = 5, P = 1, O = 4
C) N = 2, H = 5, P = 1, O = 4
D) N = 2, H = 8, P = 1, O = 4
E) none of the above

Answer: A

How many of each type of atom are there in the formula Ca3(PO4)2?

How many of each type of atom are there in the formula Ca3(PO4)2?

A) Ca = 3, P = 1, O = 4
B) Ca = 3, P = 2, O = 4
C) Ca = 3, P = 2, O = 8
D) Ca = 3, P = 1, O = 8
E) none of the above

Answer: C

How many of each type of atoms are there in the formula NH4C2H3O2?

How many of each type of atoms are there in the formula NH4C2H3O2?

A) N = 4, H = 7, C = 2, O = 2
B) N = 1, H = 4, C = 2, O = 2
C) N = 1, H = 3, C = 2, O = 2
D) N = 1, H = 7, C = 2, O = 2
E) none of the above

Answer: D

Which formula shows the proper use of parentheses?

Which formula shows the proper use of parentheses?

A) Ca(F)2
B) Ca(SO4)
C) (NH4)3(PO4)
D) Ca(NO3)2
E) none of the above

Answer: D

How many oxygen atoms are in the formula Al2(CO3)3?

How many oxygen atoms are in the formula Al2(CO3)3?

A) 3
B) 9
C) 1
D) 6
E) none of the above

Answer: B

How many carbon atoms are in the formula Al2(CO3)3?

How many carbon atoms are in the formula Al2(CO3)3?

A) 3
B) 9
C) 1
D) 6
E) none of the above

Answer: A

How many total atoms are in the formula Al2(CO3)3?

How many total atoms are in the formula Al2(CO3)3?

A) 8
B) 9
C) 12
D) 14
E) none of the above

Answer: D

Which of the following statements about chemical formulas is false?

Which of the following statements about chemical formulas is false?

A) The subscripts represent the relative number of each type of atom in the compound.
B) The subscripts represent the relative mass of each type of atom in the compound.
C) The subscripts do not change for a given compound.
D) Different compounds made of the same elements have different subscripts.
E) All of the statements are Answer: true.

Answer: B

Suppose an unknown compound XY has an X-to-Y mass ratio of 4.0. If decomposition of compound XY gives 12.0 grams of X, then how many grams of Y must form?

Suppose an unknown compound XY has an X-to-Y mass ratio of 4.0. If decomposition of compound XY gives 12.0 grams of X, then how many grams of Y must form?

A) 48.0 grams
B) 12.0 grams
C) 4.0 grams
D) 3.0 grams
E) none of the above

Answer: D

What is the oxygen-to-sulfur mass ratio of sulfur dioxide?

What is the oxygen-to-sulfur mass ratio of sulfur dioxide?

A) 0.5
B) 1.0
C) 2.0
D) 16
E) none of the above

Answer: B

The phosphorous-to-hydrogen mass ratio is 10.2 for a compound. This ratio could correspond to the compound:

The phosphorous-to-hydrogen mass ratio is 10.2 for a compound. This ratio could correspond to the compound:

A) PH.
B) PH2.
C) PH3.
D) PH6.
E) none of the above

Answer: C