Which classification of elements on the periodic table does not combine chemically with other elements?

Which classification of elements on the periodic table does not combine chemically with other elements?

A) Non-metals
B) Metals
C) Noble gases
D) Transitions


Answer: C) Noble gases

Any atom, except hydrogen and helium, is considered chemically stable when there are how many electrons in the outermost shell?

Any atom, except hydrogen and helium, is considered chemically stable when there are how many electrons in the outermost shell?

A) 5
B) 3
C) 2
D) 8


Answer: D) 8

What type of chemical bond is usually formed between atoms that readily give up electrons and atoms that readily accept electrons?

What type of chemical bond is usually formed between atoms that readily give up electrons and atoms that readily accept electrons?

A) Ionic
B) Transitional
C) Covalent
D) Noble


Answer: A) Ionic

Atoms that have become charged from losing or gaining electrons are called ______.

Atoms that have become charged from losing or gaining electrons are called ______.

A) Anodes
B) Molecules
C) Ions
D) Pairs


Answer: C) Ions

All of the elements in a vertical column of the periodic table have ______.

All of the elements in a vertical column of the periodic table have ______.

A) Eight electrons in the outermost shell
B) Identical numbers of protons
C) The same number of outer shell electrons
D) The same total number of electrons


Answer: C) The same number of outer shell electrons

Two or more elements combine chemically to form a _______.

Two or more elements combine chemically to form a _______.

A) Substance
B) Mixture
C) Composite
D) Compound


Answer: D) Compound

What happens in a single displacement reaction?

What happens in a single displacement reaction?

A) A single element decomposes into new elements
B) Two or more different reactants combine to form a single product.
C) A compound breaks down into the singular compounds or elements that formed it
D) An element replaces one of the elements in the molecules of the compound.


Answer: D) An element replaces one of the elements in the molecules of the compound

The quantity of an element that has a weight in grams numerically equal to the element's atomic weight is called _______.

The quantity of an element that has a weight in grams numerically equal to the element's atomic weight is called _______.

A) A carbon ratio
B) The molecular weight
C) A mole
D) The reactant weight


Answer: C) A mole

When the maximum amount of solute that the solvent can dissolve is added, it is called a ______ solution.

When the maximum amount of solute that the solvent can dissolve is added, it is called a ______ solution.

A) Polar
B) Saturated
C) Combination
D) Concentrated


Answer: B) Saturated

The nucleus of an atom is comprised of ______.

The nucleus of an atom is comprised of ______.

A) Electrons
B) Ions and electrons
C) Anions
D) Protons and neutrons


Answer: D) Protons and neutrons

The notation that expresses the number of electrons involved when an atom reacts chemically is the ______ number.

The notation that expresses the number of electrons involved when an atom reacts chemically is the ______ number.

A) Combination
B) Period
C) Reaction
D) Valence


Answer: D) Valence

What type of chemical bond is formed when electrons are shared between atoms?

What type of chemical bond is formed when electrons are shared between atoms?

A) Noble
B) Transitional
C) Covalent
D) Ionic


Answer: C) Covalent

Which of these is the best way to express the formula HOH?

Which of these is the best way to express the formula HOH?

A) HHO
B) 2HO
C) 2H1O
D) H20


Answer: D) H2O

Which classification of elements on the periodic table tends to give up electrons when combining chemically with other elements?

Which classification of elements on the periodic table tends to give up electrons when combining chemically with other elements?

A) Noble gases
B) Transitions
C) Non-metals
D) Metals


Answer: D) Metals

When a compound is formed, the total of all the valences must equal _____.

When a compound is formed, the total of all the valences must equal _____.

A) 1
B) 0
C) 2
D) 100


Answer: B) 0

What happens in a decomposition reaction?

What happens in a decomposition reaction?

A) A compound breaks down into the compounds or elements that formed it
B) Two or more different reactants combine to form multiple products
C) Two or more different reactants combine to form a single product
D) An element replaces one of the elements in the molecules of the compound


Answer: A) A compound breaks down into the compounds or elements that formed it

Most water solutions can conduct electricity to varying degrees and are called ______ solutions.

Most water solutions can conduct electricity to varying degrees and are called ______ solutions.

A) Saturated
B) Electrolyte
C) Galvanic
D) Cathodic


Answer: B) Electrolyte

Which of the following is a correct way to write chemical equations?

Which of the following is a correct way to write chemical equations?

A) Products are shown only if they are gases
B) Reactants are shown to the right of the arrow
C) Products are shown to the right of the arrow
D) Reactants are shown only if they are solids


Answer: C) Products are shown to the right of the arrow

What is the smallest particle of an element that still retains the chemical properties of that element?

What is the smallest particle of an element that still retains the chemical properties of that element?

A) Atom
B) Neutron
C) Electron
D) Proton


Answer: A) Atom

Water will dissolve ionic compounds because____________.

Water will dissolve ionic compounds because____________.

A) Water takes electrons away from the ions
B) The ions are much smaller than the water molecules
C) Water provides electrons to neutralize the bond between the ions
D) The polar water molecule is attracted to the ions


Answer: D) The polar water molecule is attracted to the ions

In a titration experiment, if the initial solution pH is 4.0 and the equivalence point occurs at pH 9.0, then the reaction corresponds to

In a titration experiment, if the initial solution pH is 4.0 and the equivalence point occurs at pH 9.0, then the reaction corresponds to

a. the titration of a weak acid by a strong base.
b. the titration of a weak acid by a weak base.
c. the titration of a weak base by a strong acid.
d. the titration of a strong acid by a strong base.


Answer: a

Which indicator is most appropriate for the titration of acetic acid ? (Ka = 1.8 105) with NaOH

Which indicator is most appropriate for the titration of acetic acid ? (Ka = 1.8 105) with NaOH

a. methyl red (pH 5)
b. bromthymol blue (pH 7)
c. phenolphthalein (pH 9)
d. Both methyl red and bromthymol blue are suitable.


Answer: c

In a titration of HCl(aq) with NaOH(aq), the equivalence point is the point at which equal volumes of HCl and NaOH have been combined.

In a titration of HCl(aq) with NaOH(aq), the equivalence point is the point at which equal volumes of HCl and NaOH have been combined.

the concentration of H+ equal 1.0 10-14 M.
equal moles of HCl and NaOH have reacted.
half of the HCl has been neutralized by hydroxide ion.


Answer: C

What is the effect on pH when a buffer is diluted by a factor of 10? The buffer pH deceases by 10.

What is the effect on pH when a buffer is diluted by a factor of 10? The buffer pH deceases by 10.

The buffer pH decreases by 1.
The buffer pH decreases by 1.
The buffer pH does not change appreciably.


Answer: d

When mixed together, all of the following pairs can form buffers EXCEPT

When mixed together, all of the following pairs can form buffers EXCEPT

a.H3PO4 and NaH2PO4.
b.NaH2PO4 and Na2HPO4.
c.NaI and NaOH.
d.HCl and NaCH3CO2.


Answer: c

Which of the following chemical equations corresponds to Kb1 for SO32-?

Which of the following chemical equations corresponds to Kb1 for SO32-?

a. HSO3-(aq) + H2O(l)
b. SO32-(aq) + H3O+(aq)
c. H2SO3(aq) + OH-(aq)
d. SO32-(aq) + H2O(l)

H2SO3(aq) + OH-(aq) HSO3-(aq) + H2O(l) HSO3-(aq) + H2O(l)
HSO3-(aq) + OH-(aq)


Answer: d

Which of the following reactions are acid-base reactions according to the Brønsted-Lowry model?

Which of the following reactions are acid-base reactions according to the Brønsted-Lowry model?

1. NH4+(aq) + H2O(l) NH3(aq) + H3O+(aq)
2. 2HF(aq) + Ca2+(aq)
3. H2PO4(aq) + OH(aq)

a. 1 only
b. 2 only
c. 3 only
d. 1 and 3


Answer: d

All of the following species are amphiprotic EXCEPT

All of the following species are amphiprotic EXCEPT

a. H2O.
b. HSO4-
c. HPO42-
d. SO42-


Answer: d

What is the conjugate acid of ammonia?

What is the conjugate acid of ammonia?

a.H+
b. H-
c.NH4+
d.NH3


Answer: c

According to the Brønsted-Lowry definition, a base

According to the Brønsted-Lowry definition, a base

a. is a proton acceptor.
b. increases the OH- concentration in an aqueous solution.
c. is an electron-pair donor.
d. increases the pH of a solution.


Answer: a

The Haber process for the production of ammonia relies on a heterogeneous catalyst. How does the use of this catalyst affect the yield of the reaction at equilibrium?

The Haber process for the production of ammonia relies on a heterogeneous catalyst. How does the use of this catalyst affect the yield of the reaction at equilibrium?

N2(g) + 3H2(g) 2NH3(g) H = 92.2 kJ


a. yield is increased
b. yield is decreased
c. depends on the catalyst used
d. doesn't affect yield


Answer: d

The formation of ammonia from elemental nitrogen and hydrogen is an exothermic process. N2(g) + 3H2(g) 2NH3(g) H = 92.2 kJ/mol. Assuming the reaction is at equilibrium, which one of the following changes will drive the reaction to the right?

The formation of ammonia from elemental nitrogen and hydrogen is an exothermic process. N2(g) + 3H2(g) 2NH3(g) H = 92.2 kJ/mol.
Assuming the reaction is at equilibrium, which one of the following changes will drive the reaction to the right?

a. adding ammonia
b. increasing the temperature
c. increasing the pressure
d. adding a catalyst


Answer: c

If the value of Q is less than K, then

If the value of Q is less than K, then

a. the system is in equilibrium.
b. the reaction will go left or right depending upon the reaction stoichiometry.
c. the reaction will proceed to the right until equilibrium is established.
d. the reaction will proceed to the left until equilibrium is established.


Answer: c

In which of the following equilibrium systems will an increase in the pressure have no effect on the concentrations of products and reactants?

In which of the following equilibrium systems will an increase in the pressure have no effect on the concentrations of products and reactants?

a. H2(g) + F2(g) 2 HF(g)
b. N2(g) + 3 H2(g) 2 NH3(g)
c. CaCO3(s) CaO(s) + CO2(g)
d. 2 NOBr(g) 2 NO(g) + Br2(g)


Answer: a

Assume that the following chemical reaction is at equilibrium.

Assume that the following chemical reaction is at equilibrium.

2ICl(g) I2(g) + Cl2(g) H = +26.9 kJ


At 25C, K = 2.0 105. If the temperature is increase to 45C, which statement applies?
a. K will decrease and the reaction will proceed in the backward direction.
b. K will decrease and the reaction will proceed in the forward direction.
c. K will increase and the reaction will proceed in the backward direction.
d. K will increase and the reaction will proceed in the forward direction.


Answer: d

In a titration experiment, if the initial solution pH is 10.0 and equivalence point at pH 4.0, then reaction corresponds to

In a titration experiment, if the initial solution pH is 10.0 and equivalence point at pH 4.0, then reaction corresponds to

a. WA and SB
b.WA and WB
c.WB and SA
d. SA and WB


Answer: c

Which indicator is most appropriate for the titration of ammonia with HCl?

Which indicator is most appropriate for the titration of ammonia with HCl?

a. Methyl red
b. Bromthymol blue
c.Phenolphthalein
d. Both red and Blue


Answer: a

Which of the following statements concerning acid-base indicators are true?

Which of the following statements concerning acid-base indicators are true?

1. Acid Base indicators are derived from weak acids
2. The acid and base forms of the indicators are different colors
3.Phenolphthalein shows pink color in acidic solutions


Answer: c

In a titration of HCl with NaOH, the equivalence point is the point at which

In a titration of HCl with NaOH, the equivalence point is the point at which

a. equal volumes of HCL and NaOH have been combined
b. the concentration of H+ equal 1.0x10^-7
c. equal masses of HCl and NaOH have reacted
d. half of HCL has been neutralized by hydroxide ion


Answer: b

What is the effect on pH when a Hclo4 is diluted by a factor of 10?

What is the effect on pH when a Hclo4 is diluted by a factor of 10?

a. pH increases by 10
b. pH decreases by 1
c. pH increases by 1
d. pH does not change


Answer: c

A buffer may be prepared by mixing a weak acid with a certain amount of strong base. Which of the acids best for preparation of a buffer with pH of 7.00

A buffer may be prepared by mixing a weak acid with a certain amount of strong base. Which of the acids best for preparation of a buffer with pH of 7.00

a. ammonium ;Ka=5.6x10^-10
b. formic acid;Ka=1.9X10^-4
c. benzoic acid;Ka=6.6x10^-5
d. dihydrogen phosphate ion;Ka=6.2x10^-8


Answer: d

When mixed together, all of the following pairs can form buffers EXCEPT

When mixed together, all of the following pairs can form buffers EXCEPT

a. H3PO4 and NaH2PO4-
b. NaH2PO4 and Na2HPO2-
c.H3PO4 and NaOH
d. HCL and HcH3CO2


Answer: d

According to the Lewis definition, a base

According to the Lewis definition, a base

a. Is a proton acceptor
b. Increases the OH- concentration in an aqueous solution
c. Is an electron-pair donor
d. increases the pH of a solution


Answer: c

Which of the following is a Lewis acid NOT a Bronstead-Lowry acid

Which of the following is a Lewis acid NOT a Bronstead-Lowry acid

a. HF
b.NH4+
c.ZN2+
d.HPO42-


Answer: c

A salt solution can be acidic, basic or neutral. When dissolved in water, which of the following will make the solution acidic: NaBr, Fe(NO3)3, BaCO3, and CrCl3

A salt solution can be acidic, basic or neutral. When dissolved in water, which of the following will make the solution acidic: NaBr, Fe(NO3)3, BaCO3, and CrCl3

a. BCO3 and NaBr
b. Fe(NO3)3 and CrCl3
c.BaCO3 and CrCl3
d. NaBr and Fe(NO3)3


Answer: b

A salt solution can be acidic, basic or neutral. When dissolved in water, which of the following will make the solution basic: NaBr, KF, BaCO3, and CrCl3

A salt solution can be acidic, basic or neutral. When dissolved in water, which of the following will make the solution basic: NaBr, KF, BaCO3, and CrCl3

a. BaCO3 and KF
b. BaCO3 and CrCl3
c.NaBr and CrCl3
d. NaBr and KF


Answer: a

Which of the following chemical equations corresponds to Ka2 for H2SO3

Which of the following chemical equations corresponds to Ka2 for H2SO3

a. H2SO3-->HSO3-+H+
b. SO32-+H3O+--->HSO3-+H2O
c.HSO3---->SO32-+H+
d. SO32-+H2O--->HSO3-+OH-


Answer: c

Which of the following reactions are acid-base reactions according to Bronstead Lowry model?

Which of the following reactions are acid-base reactions according to Bronstead Lowry model?

1. NH4+ + H2O --->NH3+H3O+
2.HF+NH3--->F-+NH4+
3.PO43-+H3O+--->HPO42-+H20


Answer: d

What is conjugate acid of [Al(H20)5OH]^2+

What is conjugate acid of [Al(H20)5OH]^2+

a. [Al(H20)5]^3+
b.[Al(H20)5H3O]^4+
c.[Al(H20)6]^3+
d. H3O+


Answer: c

All of the following species are amphiprotic EXCEPT

All of the following species are amphiprotic EXCEPT

a. H20
b.Po43-
c.H2PO4-
d.HPO42-


Answer: b

Assuming the reaction below is at equilibrium which of the following changes will drive the reaction to the left?

Assuming the reaction below is at equilibrium which of the following changes will drive the reaction to the left?

Co2(g)--->C(s)+O2(g) = +395.5 kJ


1. Decreasing the temperature
2. Adding Co2
3. Adding C


Answer: 1

Which of the following statements is CORRECT for the following system at equilibrium?

Which of the following statements is CORRECT for the following system at equilibrium?

H2(g)+F2(g)---->2HF(g)


a) Addition of catalyst will cause the reaction to proceed in forward direction
b)Increasing pressure of system will cause the reaction to the forward direction
c) The partial pressure of HF(g) will decrease when HF(g) added
d) The partial pressure of H2(g) will increase if HF(g) added


Answer: d

The formation of ammonia from elemental nitrogen and hydrogen is an exothermic process.

The formation of ammonia from elemental nitrogen and hydrogen is an exothermic process.

N2(g)+3H2(g)--->2NH3(g) = -92.2KJ

Assuming the reaction is at equilibrium, which one of the following changes will drive the reaction to the left?

a) Adding hydrogen gas
b)Adding a catalyst
c) compress the volume to half
d) increasing the temperature


Answer: d

If the value of Q is greater than K, then

If the value of Q is greater than K, then

a) The reaction will go left till equilibrium
b) The reaction will go right till equilibrium
c)The reaction will go left or right until equilibrium
d) The system is in equilibrium


Answer: a

Assume that the following chemical reaction is at equilibrium.

Assume that the following chemical reaction is at equilibrium.

2ICl(g)--->I2(g)+Cl2(g) =+26.9 kj

a)K will increase and the reaction will go backwards
b)K will increase and the reaction will go forward
c) K will decrease and the reaction will go backward
d) K will decrease and the reaction will go forward


Answer: c

Which response includes all the acids listed below that are strong acids, and no weak acids?

Which response includes all the acids listed below that are strong acids, and no weak acids?

H2SO4, HI, HF, H3PO4, HNO3

A. HI, HF, HNO3
B. H2SO4, HNO3
C. H2SO4, HI, HNO3
D. H2SO4, H3PO4, HNO3
E. another one or another combination


Answer: H2SO4, HI, HNO3

Which response gives all of the members of the following list that are basic salts and none that are not basic salts?

Which response gives all of the members of the following list that are basic salts and none that are not basic salts?

Al(OH)Cl2, Al(OH)2Cl, AlCl3, Ca(OH)Cl, CaCl2•2H2O


A. Al(OH)Cl2, Al(OH)2Cl, AlCl3
B. Al(OH)Cl2, Al(OH)2Cl, Ca(OH)Cl
C. Al(OH)2Cl, CaCl2•2H2O
D. Al(OH)Cl2, Ca(OH)Cl
E. Al(OH)Cl2, Al(OH)2Cl, Ca(OH)Cl, CaCl2•2H2O


Answer: Al(OH)Cl2, Al(OH)2Cl, Ca(OH)Cl

According to the Brønsted-Lowry theory, which of these acids would have the weakest conjugate base?

According to the Brønsted-Lowry theory, which of these acids would have the weakest conjugate base?

A. HBrO3
B. HNO2
C. HClO4
D. HClO2
E. HF


Answer: HClO4

Based on the reactions we have studied, ammonia can be considered as ____.

Based on the reactions we have studied, ammonia can be considered as ____.

A. an Arrhenius base (only)
B. a Lewis base (only)
C. a Brønsted-Lowry base (only)
D. both an Arrhenius base and a Lewis base
E. both a Brønsted-Lowry base and a Lewis base


Answer: both a Bronsted-Lowty base and a Lewis

For which one of the pairs of acid and bases does the following represent the correct net ionic equation?

For which one of the pairs of acid and bases does the following represent the correct net ionic equation?

CH3COOH + OH− → CH3COO− + H2O


A. NaOH, HBr
B. CH3COOH, Ca(OH)2
C. HNO3, Mg(OH)2
D. CH3COOH, Cu(OH)2
E. CH3COOH, Cr(OH)3


Answer: CH3COOH, Ca(OH)2

Which one of the following statements is true?

Which one of the following statements is true?

CH 3NH 2 + H 2O --> CH 3NH 3+ + OH −
methylamine, water
methylammonium ion, hydroxide ion


A. CH3NH2 is the conjugate base of H2O.
B. CH3NH3+ is the conjugate base of CH3NH2.
C. H2O is the conjugate acid of OH−.
D. OH− is the conjugate acid of H2O.
E. There are no conjugate acid-base pairs.


Answer: H2O is the conjugate acid of OH-

Write the net ionic equation for the complete neutralization of HBr by Ca(OH) 2. Use H + rather than H 3O +. What is the sum of the coefficients?

Write the net ionic equation for the complete neutralization of HBr by Ca(OH) 2. Use H + rather than H 3O +. What is the sum of the coefficients?

A. 6
B. 8
C. 3
D. 4
E. 5


Answer: 3

Write the balanced formula unit equation for the complete neutralization of dilute sulfuric acid with sodium hydroxide in aqueous solution. What is the sum of the coefficients?

Write the balanced formula unit equation for the complete neutralization of dilute sulfuric acid with sodium hydroxide in aqueous solution. What is the sum of the coefficients?

A. 6
B. 8
C. 9
D. 4
E. 5


Answer: 6

Write the balanced formula unit equation for the reaction of iron(II) hydroxide with hydrobromic acid. What is the sum of the coefficients?

Write the balanced formula unit equation for the reaction of iron(II) hydroxide with hydrobromic acid. What is the sum of the coefficients?

A. 6
B. 7
C. 8
D. 4
E. 5


Answer: 6

In the following reaction, the Cl − functions as a(n) ____.

In the following reaction, the Cl − functions as a(n) ____.

AlCl3 + Cl− → AlCl4−


A. Brønsted-Lowry acid
B. Brønsted-Lowry base
C. Arrhenius base
D. Lewis acid
E. Lewis base


Answer: Lewis base

According to the Brønsted-Lowry theory, which of these anions is the strongest base?

According to the Brønsted-Lowry theory, which of these anions is the strongest base?

A. NO3−
B. Cl−
C. CN−
D. ClO4−
E. HSO4−


Answer: CN-

Which one of the following is not a soluble, strong base?

Which one of the following is not a soluble, strong base?

A. KOH
B. CsOH
C. NH3
D. Ca(OH)2
E. Sr(OH)2


Answer: NH3

Which response gives all of the members of the following list that are acidic salts and none that are not acidic salts?

Which response gives all of the members of the following list that are acidic salts and none that are not acidic salts?

KH2PO4, K2HPO4, K3PO4, NaHCO3, LiOH, LiH


A. KH2PO4, K2HPO4, LiH
B. KH2PO4, NaHCO3, LiOH
C. K3PO4, LiH
D. KH2PO4, K2HPO4, NaHCO3
E. KH2PO4, K2HPO4, NaHCO3, LiH


Answer: KH2PO4, K2HPO4, NaHCO3

Why is HI a stronger acid than HCl?

Why is HI a stronger acid than HCl?

A.
Because I is more electronegative than Cl.
B.
Because Cl is more electronegative than I.
C.
The bond strength of HCl is greater than the bond strength of HI.
D.
The bond strength of HI is greater than the bond strength of HCl.
E.
HI is not a stronger acid than HCl.


Answer: The bond strength of HCl is greater than the bond strength of HI.

Which one of the following pairs of acids and conjugate bases is incorrectly labeled or incorrectly matched?

Which one of the following pairs of acids and conjugate bases is incorrectly labeled or incorrectly matched?

Acid / Conjugate Base


A. water / hydroxide
B. sulfuric acid / sulfate
C. perchloric acid / perchlorate
D. nitric acid / nitrate
E. hydrobromic acid / bromide


Answer: sulfuric acid / sulfate

Which of the following statements is false?

Which of the following statements is false?

A. Arrhenius acids are also Brønsted-Lowry acids.
B. Brønsted-Lowry acids are also Lewis acids.
C. Brønsted-Lowry bases are also Arrhenius bases.
D. Arrhenius bases are also Brønsted-Lowry bases.
E. Brønsted-Lowry bases are also Lewis bases.


Answer: Bronsted-Lowry bases are also Lewis bases

According to the Brønsted-Lowry theory, which of these anions is the weakest base?

According to the Brønsted-Lowry theory, which of these anions is the weakest base?

A. Br−
B. ClO−
C. NO2−
D. F−
E. CH3COO−


Answer: Br-

What is the basis for referring to "H +" as a proton?

What is the basis for referring to "H +" as a proton?

A. The Arrhenius definition of an acid
B. The Brønsted-Lowry definition of an acid
C. The Lewis definition of an acid
D. H+ exists as a bare proton
E. None of these


Answer: H+ exists as a bare proton

Which pair of acids would each react with barium hydroxide and have the net ionic equation:

Which pair of acids would each react with barium hydroxide and have the net ionic equation:

H+ + OH− → H2O

A. HCl and HNO2
B. HBr and HF
C. HCl and HNO3
D. HNO3 and H2CO3
E. HClO4 and H2SO4


Answer: HCl and HNO3

Which one of the following is a weak acid?

Which one of the following is a weak acid?

A. HNO3
B. H3PO4
C. HClO3
D. HClO4
E. HI


Answer: H3PO4

Which of the following reactions is the net ionic equation for the acid-base reaction between H 2CO 3 and Sr(OH) 2?

Which of the following reactions is the net ionic equation for the acid-base reaction between H 2CO 3 and Sr(OH) 2?

A. H2CO3 + Sr2+ + 2OH− → SrCO3 + 2H2O
B. H3O+ + OH− → 2H2O
C. 2H3O+ + Sr2+ + 2OH− → Sr2+ + 4H2O
D. H2CO3 + 2OH− → 2H2O + CO32−
E. H2CO3 + Sr(OH)2 → 2H2O + Sr2+ + CO32−


Answer: H2CO3 + Sr2+ + 2OH− → SrCO3 + 2H2O

According to the Lewis theory, which one of the following compounds would be expected to react as a Lewis acid, but not as a Lewis base?

According to the Lewis theory, which one of the following compounds would be expected to react as a Lewis acid, but not as a Lewis base?

A. BCl3
B. NH3
C. PH3
D. H2O
E. all of these


Answer: BCl3

In the equation HF + H2O H3O+ + F−

In the equation
HF + H2O H3O+ + F−

A. H2O is a base, and HF is its conjugate acid.
B. H2O is an acid, and HF is the conjugate base.
C. HF is an acid, and F− is its conjugate base.
D. HF is a base, and H3O+ is its conjugate acid.
E. HF is a base, and F− is its conjugate acid.


Answer: HF is an acid, and F- is its conjugate base

Write the balanced net ionic equation for the complete neutralization of chromium(III) hydroxide with sulfuric acid. Use H + rather than H 3O +. What is the sum of the coefficients?

Write the balanced net ionic equation for the complete neutralization of chromium(III) hydroxide with sulfuric acid. Use H + rather than H 3O +. What is the sum of the coefficients?

A. 8
B. 11
C. 16
D. 18
E. 22


Answer: 8

Arrange the following in order of increasing acid strength:

Arrange the following in order of increasing acid strength:

H2O, H2Se, H2Te, H2S

A. H2O < H2Te < H2Se < H2S
B. H2Se < H2Te < H2O < H2S
C. H2S < H2Se < H2Te < H2O
D. H2O < H2S < H2Se < H2Te
E. H2Se < H2Te < H2S < H2O


Answer: H2O < H2S < H2Se < H2Te

Which one of the following is a soluble, strong base?

Which one of the following is a soluble, strong base?

A. Cu(OH)2
B. Fe(OH)3
C. Al(OH)3
D. Sr(OH)2
E. Mg(OH)2


Answer: Sr(OH)2

Which one of the following species could not react as a Brønsted-Lowry base?

Which one of the following species could not react as a Brønsted-Lowry base?

A. NH4+
B. NH2−
C. CN−
D. F−
E. CH3COO−


Answer: NH4+

For which one of the pairs of acids and bases does the following represent the net ionic equation?

For which one of the pairs of acids and bases does the following represent the net ionic equation?

H3O+ + OH− → 2H2O


A. NaOH, HBr
B. CH3COOH, Ca(OH)2
C. HNO3, Mg(OH)2
D. CH3COOH, Cu(OH)2
E. CH3COOH, Cr(OH)3


Answer: NaOH, HBr

According to the Lewis theory, a base ____.

According to the Lewis theory, a base ____.

A. is a proton acceptor
B. is a proton donor
C. makes available a share in a pair of electrons
D. is any compound that contains electron pairs
E. accepts a share in a pair of electrons


Answer: makes available a share in a pair of electrons

According to the Lewis theory, which one of the following species would be expected to react as a Lewis base, but not as a Lewis acid?

According to the Lewis theory, which one of the following species would be expected to react as a Lewis base, but not as a Lewis acid?

A. BF3
B. F−
C. AlBr3
D. SnCl4
E. H+


Answer: F-

Gaseous methylamine, CH 3NH 2, can be classified as ____.

Gaseous methylamine, CH 3NH 2, can be classified as ____.

A. a Lewis base only
B. Arrhenius and Brønsted-Lowry bases
C. a Brønsted-Lowry base only
D. Arrhenius and Lewis bases
E. Brønsted-Lowry and Lewis bases


Answer: Bronsted-Lowry and Lewis bases

Which statement concerning the autoionization (self-ionization) of water is false?

Which statement concerning the autoionization (self-ionization) of water is false?

2H2O --> H3O+(aq) + OH−(aq)


A. This reaction is an acid-base reaction according to the Brønsted-Lowry theory.
B. Water is amphiprotic.
C. A H2O molecule may react as an acid by donating a proton.
D. In this reaction H3O+ and OH− are a conjugate acid-base pair.
E. A H2O molecule may react as a base by accepting a proton.


Answer: In this reaction, H3O+ and OH- are a conjugate acid-base pair

Which one of the following is a weak acid?

Which one of the following is a weak acid?

A. H2SO4
B. HClO
C. HCl
D. HBr
E. HI


Answer: HClO

If a compound is able to react as either an acid or a base, it is said to be which of these?

If a compound is able to react as either an acid or a base, it is said to be which of these?

A. autoionized
B. amphoteric
C. hydrated
D. balanced
E. neutralized


Answer: amphoteric

Which of the following is a normal salt?

Which of the following is a normal salt?

A. Na3PO4
B. NaOH
C. NaHCO3
D. NaHSO4
E. all of these are normal salts


Answer: Na3PO4

According to the Brønsted-Lowry theory, a base is defined as ____.

According to the Brønsted-Lowry theory, a base is defined as ____.

A. an electron pair acceptor
B. a proton acceptor
C. an electron pair donor
D. a proton donor
E. any species that can produce hydroxide ions in aqueous solution


Answer: a proton acceptor

Write the balanced formula unit equation for the reaction of hydrobromic acid with magnesium hydroxide. What is the sum of the coefficients?

Write the balanced formula unit equation for the reaction of hydrobromic acid with magnesium hydroxide. What is the sum of the coefficients?

A. 6
B. 7
C. 3
D. 4
E. 5


Answer: 6

Examine the reaction below and classify it.

Examine the reaction below and classify it.

FeBr3 + Br− → FeBr4−


A. single displacement
B. combustion
C. decomposition
D. acid-base
E. oxidation-reduction


Answer: acid-base

Which one of the following compounds is not a salt?

Which one of the following compounds is not a salt?

A. K2SO4
B. HClO4
C. CaCrO4
D. CoCl2
E. NaMnO4


Answer: HCl4

Which of the following reactions represents and acid-base reaction according to Lewis theory but not according to Bronsted-Lowry theory?

Which of the following reactions represents and acid-base reaction according to Lewis theory but not according to Bronsted-Lowry theory?

a) NH3 + HCl --> NH4Cl
b) 2H2O <--> H3O+ + OH-
c) Cu2+ + 4NH3 <--> [Cu(NH3)4]2+
d) BaO + H2O <--> Ba2+ + 2OH-


Answer: c) Cu2+ + 4NH3 <--> [Cu(NH3)4]2+

as there is no exchange of H+

Which of the following could not act as a ligand in a complex ion with a transition metal?

Which of the following could not act as a ligand in a complex ion with a transition metal?

a) Cl-
b) NCl3
c) PCl3
d) CH4


Answer: d) CH4 because it does not possess a lone pair

For each of the following, identify the lewis acid and the Lewis base:

For each of the following, identify the lewis acid and the Lewis base:

a) 4NH3 + Zn2+ --> [Zn[NH3)4]2+
b) 2Cl- + BeCl2 --> [BeCl4]2-
c) Mg2+ + 6H2O --> [Mg(H2O)6]2+


a) acid = Zn2+ base = NH3
b) acid = BeCl2 base = Cl-
c) acid = Mg2+ base = H2O

How can all Bronsted-Lowry acid-base reactions be classified under Lewis, but Lewis cannot be classified under Bronsted Lowry?

How can all Bronsted-Lowry acid-base reactions be classified under Lewis, but Lewis cannot be classified under Bronsted Lowry?

Answer: All Bronsted-Lowry involves a transfer of lone pairs of electrons.

However, reactions according to Lewis where no transfer of H+ occurs does not fall under Bronsted-Lowry

A _____ acid can donate more than one proton per molecule.

A ______________ acid can donate more than one proton per molecule.

Answer: polyprotic

All Arrhenius acids are also Bronsted-Lowry acids, because H+ ions are ___________.

All Arrhenius acids are also Bronsted-Lowry acids, because H+ ions are ___________.

Answer: protons

________ definitions rely on water being the solvent.

________ definitions rely on water being the solvent.

Answer: Arrhenius

A _____________ acid can only donate one proton (hydrogen ion) per molecule.

A _____________ acid can only donate one proton (hydrogen ion) per molecule.

Answer: monoprotic

A _____________ solution is a solution that has a relatively small amount of solute, or a low concentration.

A _____________ solution is a solution that has a relatively small amount of solute, or a low concentration.

Answer: dilute

The amount of solute in a given amount of solvent or solution is the _______________ of a solution.

The amount of solute in a given amount of solvent or solution is the _______________ of a solution.

Answer: concentration

_________ is the concentration of a solution expressed as number of moles of solute dissolved in each liter of solution.

_________ is the concentration of a solution expressed as number of moles of solute dissolved in each liter of solution.

Answer: Molarity

In some instances, the concentration of a solution of expressed as molality instead of molarity because ________.

In some instances, the concentration of a solution of expressed as molality instead of molarity because ________.

Answer: molality does not change with changes in temperature

The ____________ of a solution is the number of moles of solute dissolved in each kilogram of solvent.

The ____________ of a solution is the number of moles of solute dissolved in each kilogram of solvent.

Answer: molality

Explain why a molecule formed by two identical atoms is non polar.

Explain why a molecule formed by two identical atoms is non polar.

Answer: the electrons are shared equally in bonds

Which type of bond occurs when atoms share electrons?

Which type of bond occurs when atoms share electrons?

Answer: covalent

Explain how the formula for a binary compound is written.

Explain how the formula for a binary compound is written.

Answer:

1. write name of atom and see if it's positive or negative
2. write the root name of the negative ion
3. add -ide to the root

How do we show the elements that make up a compound and the exact number of atoms in the compound?

How do we show the elements that make up a compound and the exact number of atoms in the compound?

Answer: use a chemical formula

The sum of all oxidation number in a neutral compound is always what?

The sum of all oxidation number in a neutral compound is always what?

Answer: 0

What physical property is used to tell whether a compound is ionic or covalent, and why is this a good indicator?

What physical property is used to tell whether a compound is ionic or covalent, and why is this a good indicator?

Answer:

covalent= gas
ionic= liquid

In a chemical formula, the number of each type of atom in the compound is shown by what types of numbers?

In a chemical formula, the number of each type of atom in the compound is shown by what types of numbers?

Answer: subscripts

Explain what happens to the electrons in a covalent bond.

Explain what happens to the electrons in a covalent bond.

Answer: they share electrons with each other

What do we call a group of covalently bonded atoms that act together as one charged atom?

What do we call a group of covalently bonded atoms that act together as one charged atom?

Answer: polyatomic ion

How many valence electrons are need for most atoms to be chemically stable?

How many valence electrons are need for most atoms to be chemically stable?

Answer: 8

What kind of chemical bond involves an equal exchange of electrons?

What kind of chemical bond involves an equal exchange of electrons?

Answer: ionic

Why do the noble gases not form compounds readily?

Why do the noble gases not form compounds readily?

Answer: they are already stable

How is the oxidation number of an atom shown?

How is the oxidation number of an atom shown?

Answer: a number and its charge

List and compare the properties of the elements that form water with those of water.

List and compare the properties of the elements that form water with those of water.

Answer: Water in its formula and chemically attached to its ion.

What type of bond is formed between two chlorine atoms?

What type of bond is formed between two chlorine atoms?

Answer: covalent

What type of bond is formed between sodium and chlorine? What is the formula?

What type of bond is formed between sodium and chlorine? What is the formula?

Answer: ionic; NaCl

How does the mass spectrum identify compounds?

How does the mass spectrum identify compounds?

Answer: Peaks with Mr of molecules can help identify unknown compounds if the mixture will peak for the molecular ion of each one.

How do you calculate relative atomic mass from a mass spectrum?

How do you calculate relative atomic mass from a mass spectrum?

Answer: 1st for each peak multiply y and x-axes together for total relative mass each isotope, 2nd add these totals and 3rd divide by the largest abundance value on y-axis.