Consider the molecule below. Determine the molecular geometry at each of the 3 labeled atoms.

Consider the molecule below. Determine the molecular geometry at each of the 3 labeled atoms.

A) 1=trigonal planar, 2=tetrahedral, 3=trigonal pyramidal
B) 1=tetrahedral, 2=tetrahedral, 3=tetrahedral
C) 1=trigonal planar, 2=tetrahedral, 3=tetrahedral
D) 1=tetrahedral, 2=tetrahedral, 3=trigonal planar
E) 1=trigonal planar, 2=trigonal pyramidal, 3=trigonal pyramidal


Answer: A

Consider the molecule below. Determine the molecular geometry at each of the 2 labeled carbons.

Consider the molecule below. Determine the molecular geometry at each of the 2 labeled carbons.

A) C1 = tetrahedral, C2 = linear
B) C1 = trigonal planar, C2= bent
C) C1 = bent, C2 = trigonal planar
D) C1 = trigonal planar, C2 = tetrahedral
E) C1 = trigonal pyramidal, C2 = see-saw



Answer: D

Determine the electron geometry (eg) and molecular geometry (mg) of XeF4.

Determine the electron geometry (eg) and molecular geometry (mg) of XeF4.

A) eg=tetrahedral, mg=tetrahedral
B) eg=linear, eg=linear
C) eg=tetrahedral, mg=bent
D) eg=trigonal bipyramidal, mg=tetrahedral
E) eg=octahedral, mg=square planar


Answer: E

Determine the electron geometry (eg) and molecular geometry (mg) of XeF2.

Determine the electron geometry (eg) and molecular geometry (mg) of XeF2.

A) eg=trigonal bipyramidal, mg=bent
B) eg=linear, mg=linear
C) eg=tetrahedral, mg=linear
D) eg=trigonal bipyramidal, mg=linear
E) eg=tetrahedral, mg=bent


Answer: D

Determine the electron geometry (eg) and molecular geometry (mg) of ICl2?.

Determine the electron geometry (eg) and molecular geometry (mg) of ICl2?.

A) eg=tetrahedral, mg=bent
B) eg=tetrahedral, mg=trigonal pyramidal
C) eg=trigonal bipyramidal, mg=linear
D) eg=trigonal bipyramidal, mg=trigonal planar
E) eg=octahedral, mg=linear


Answer: C

Determine the electron geometry (eg) and molecular geometry (mg) of BrF3.

Determine the electron geometry (eg) and molecular geometry (mg) of BrF3.

A) eg=trigonal planar, mg=trigonal planar
B) eg=trigonal bipyramidal, mg= T-shape
C) eg=trigonal planar, mg=bent
D) eg=trigonal bipyramidal, mg=see-saw
E) eg=tetrahedral, mg=trigonal pyramidal


Answer: B

Determine the electron geometry (eg) and molecular geometry (mg) of the underlined carbon in CH3CN.

Determine the electron geometry (eg) and molecular geometry (mg) of the underlined carbon in CH3CN.

A) eg=tetrahedral, mg=tetrahedral
B) eg=linear, mg=trigonal planar
C) eg=trigonal planar, mg=bent
D) eg=linear, mg=linear
E) eg=trigonal planar, mg=trigonal planar


Answer: D

Determine the electron geometry (eg) and molecular geometry (mg) of PF5.

Determine the electron geometry (eg) and molecular geometry (mg) of PF5.

A) eg=trigonal bipyramidal, mg=trigonal bipyramidal
B) eg=octahedral, mg=octahedral
C) eg=trigonal bipyramidal, mg=tetrahedral
D) eg=tetrahedral, mg=trigonal pyramidal
E) eg=trigonal planar, mg=octahedral


Answer: A

Determine the electron geometry (eg) and molecular geometry (mg) of SiF4.

Determine the electron geometry (eg) and molecular geometry (mg) of SiF4.

A) eg=tetrahedral, mg=trigonal pyramidal
B) eg=octahedral, mg=square planar
C) eg=trigonal bipyramidal, mg=trigonal pyramidal
D) eg=tetrahedral, mg=bent
E) eg=tetrahedral, mg=tetrahedral


Answer: E

Determine the electron geometry (eg) and molecular geometry (mg) of CH3+1.

Determine the electron geometry (eg) and molecular geometry (mg) of CH3+1.

A) eg=tetrahedral, mg=tetrahedral
B) eg=tetrahedral, mg=trigonal pyramidal
C) eg=trigonal planar, mg=bent
D) eg=trigonal planar, mg=trigonal planar
E) eg=tetrahedral, mg=trigonal planar


Answer: D

Determine the electron geometry (eg) and molecular geometry (mg) of CO32?

Determine the electron geometry (eg) and molecular geometry (mg) of CO32?

A) eg=tetrahedral, mg=tetrahedral
B) eg=tetrahedral, mg=trigonal pyramidal
C) eg=trigonal planar, mg=bent
D) eg=trigonal planar, mg=trigonal planar
E) eg=tetrahedral, mg=trigonal planar


Answer: D

Determine the electron geometry (eg) and molecular geometry(mg) of BCl3.

Determine the electron geometry (eg) and molecular geometry(mg) of BCl3.

A) eg=trigonal planar, mg=trigonal planar
B) eg=tetrahedral, mg=trigonal planar
C) eg=tetrahedral, mg=trigonal pyramidal
D) eg=trigonal planar, mg=bent
E) eg=trigonal bipyramidal, mg= trigonal bipyramidal


Answer: A

Give the approximate bond angle for a molecule with a tetrahedral shape.

Give the approximate bond angle for a molecule with a tetrahedral shape.

A) 109.5°
B) 180°
C) 120°
D) 105°


Answer: A

Give the approximate bond angle for a molecule with a trigonal planar shape.

Give the approximate bond angle for a molecule with a trigonal planar shape.

A) 109.5°
B) 180°
C) 120°
D) 105°


Answer: C

Give the number of valence electrons for SF4.

Give the number of valence electrons for SF4.

A) 28
B) 30
C) 32
D) 34


Answer: D

Which molecule or compound below contains an ionic bond?

Which molecule or compound below contains an ionic bond?

A) CO2
B) C2Cl4
C) SiF4
D) OCl2
E) NH4NO3


Answer: E

Which molecule or compound below contains a polar covalent bond?

Which molecule or compound below contains a polar covalent bond?

A) C2H4
B) ZnS
C) LiI
D) NCl3
E) AgCl


Answer: D

Which molecule or compound below contains a pure covalent bond?

Which molecule or compound below contains a pure covalent bond?

A) Li2CO3
B) SCl6
C) Cl2
D) PF3
E) NaCl


Answer: C

Using periodic trends, place the following bonds in order of increasing ionic character. Si-P Si-Cl Si-S

Using periodic trends, place the following bonds in order of increasing ionic character.
Si-P Si-Cl Si-S

A) Si-P < Si-Cl < Si-S
B) Si-P < Si-S < Si-Cl
C) Si-S < Si-Cl < Si-P
D) Si-Cl < Si-P < Si-S
E) Si-Cl < Si-S < Si-P


Answer: B

Using periodic trends, place the following bonds in order of decreasing ionic character. Sb-Cl P-Cl As-Cl

Using periodic trends, place the following bonds in order of decreasing ionic character.
Sb-Cl P-Cl As-Cl

A) Sb-Cl > As-Cl > P-Cl
B) As-Cl > Sb-Cl > P-Cl
C) Sb-Cl > P-Cl > As-Cl
D) P-Cl > As-Cl > Sb-Cl
E) Sb-Cl > P-Cl > As-Cl


Answer: A

Using periodic trends, place the following bonds in order of increasing ionic character. S-F Se-F O-F

Using periodic trends, place the following bonds in order of increasing ionic character.
S-F Se-F O-F

A) Se-F < S-F < O-F
B) S-F < Se-F < O-F
C) O-F < Se-F < S-F
D) Se-F < O-F < S-F
E) O-F < S-F < Se-F


Answer: E

Choose the bond below that is least polar.

Choose the bond below that is least polar.

A) P-F
B) C-Br
C) C-F
D) C-I
E) C-Cl


Answer: D

Choose the bond below that is most polar.

Choose the bond below that is most polar.

A) H-I
B) H-Br
C) H-F
D) H-Cl
E) C-H


Answer: C

Choose the bond below that is most polar.

Choose the bond below that is most polar.

A) C-N
B) C-F
C) C-O
D) C-C
E) F-F

Answer: B

List the following compounds in decreasing electronegativity difference. Cl2 HCl NaCl

List the following compounds in decreasing electronegativity difference.
Cl2 HCl NaCl

A) NaCl > Cl2 > HCl
B) Cl2 > HCl > NaCl
C) HCl > NaCl > Cl2
D) NaCl > HCl > Cl2


Answer: D

Place the following elements in order of increasing electronegativity. Sr N Na

Place the following elements in order of increasing electronegativity.
Sr N Na

A) Sr < Na < N
B) Na < N < Sr
C) Sr < N < Na
D) N < Sr < Na
E) N < Na < Sr


Answer: A

Place the following elements in order of decreasing electronegativity. S Cl Se

Place the following elements in order of decreasing electronegativity.
S Cl Se

A) Se > S > Cl
B) Cl > Se > S
C) Se > Cl > S
D) S > Cl > Se
E) Cl > S > Se


Answer: E

Place the following elements in order of increasing electronegativity. K Cs P

Place the following elements in order of increasing electronegativity.
K Cs P

A) P < K < Cs
B) K < P < Cs
C) Cs < P < K
D) Cs < K < P
E) P < Cs < K


Answer: D

Which of the following statements is TRUE?

Which of the following statements is TRUE?

A) An ionic bond is much stronger than most covalent bonds.
B) An ionic bond is formed through the sharing of electrons.
C) Ionic compounds at room temperature typically conduct electricity.
D) Once dissolved in water, ionic compounds rarely conduct electricity.
E) None of the above are true.


Answer: A

Choose the compound below that should have the lowest melting point according to the ionic bonding model.

Choose the compound below that should have the lowest melting point according to the ionic bonding model.

A) LiF
B) NaCl
C) CsI
D) KBr
E) RbI


Answer: C

Choose the compound below that should have the highest melting point according to the ionic bonding model.

Choose the compound below that should have the highest melting point according to the ionic bonding model.

A) SrI2
B) MgF2
C) CaCl2
D) SrF2
E) SrBr2


Answer: B

Choose the compound below that should have the highest melting point according to the ionic bonding model.

Choose the compound below that should have the highest melting point according to the ionic bonding model.

A) AlN
B) MgO
C) NaF
D) CaS
E) RbI


Answer: A

Place the following in order of decreasing magnitude of lattice energy. KF MgS RbI

Place the following in order of decreasing magnitude of lattice energy.
KF MgS RbI

A) RbI > KF > MgS
B) RbI > MgS > KF
C) MgS > RbI > KF
D) KF > RbI > MgS
E) MgS > KF > RbI


Answer: E

Place the following in order of increasing magnitude of lattice energy. MgO LiI CaS

Place the following in order of increasing magnitude of lattice energy.
MgO LiI CaS

A) CaS < MgO < LiI
B) LiI < CaS < MgO
C) MgO < CaS < LiI
D) LiI < MgO < CaS
E) MgO < LiI < CaS


Answer: B

Place the following in order of increasing magnitude of lattice energy. CaO MgO SrS

Place the following in order of increasing magnitude of lattice energy.
CaO MgO SrS

A) MgO < CaO < SrS
B) SrS < MgO < CaO
C) SrS < CaO < MgO
D) CaO < MgO < SrS
E) CaO < SrS < MgO


Answer: C

Place the following in order of decreasing magnitude of lattice energy. NaF RbBr KCl

Place the following in order of decreasing magnitude of lattice energy.
NaF RbBr KCl

A) RbBr > NaF > KCl
B) NaF > KCl > RbBr
C) KCl > NaF > RbBr
D) NaF > RbBr > KCl
E) RbBr > KCl > NaF


Answer: B

Place the following in order of decreasing magnitude of lattice energy. K2O Rb2S Li2O

Place the following in order of decreasing magnitude of lattice energy.
K2O Rb2S Li2O

A) Li2O > K2O > Rb2S
B) Li2O > Rb2S > K2O
C) Rb2S > K2O > Li2O
D) Rb2S > Li2O > K2O
E) K2O > Li2O > Rb2S


Answer: A

Which of the following reactions is associated with the lattice energy of RbI (?H°latt)?

Which of the following reactions is associated with the lattice energy of RbI (?H°latt)?

A) Rb(s) +1/2I2(g) ? RbI(s)
B) RbI(s) ? Rb? (g) + I? (g)
C) RbI(s) ? Rb(s) + I2(g)
D) RbI(s) ? Rb? (aq) + I? (aq)
E) Rb? (g) + I? (g) ? RbI(s)


Answer: E

Which of the following reactions is associated with the lattice energy of CaS (?H°latt)?

Which of the following reactions is associated with the lattice energy of CaS (?H°latt)?

A) Ca(s) + S(s) ? CaS(s)
B) CaS(s) ? Ca(s) + S(s)
C) Ca2? (aq) + S2? (aq) ? CaS(s)
D) Ca2? (g) + S2? (g) ? CaS(s)
E) CaS(s) ? Ca2? (aq) + S2? (aq)


Answer: D

Which of the following reactions is associated with the lattice energy of Li2O (?H°latt)?

Which of the following reactions is associated with the lattice energy of Li2O (?H°latt)?

A) Li2O(s) ? 2 Li? (g) + O2? (g)
B) 2 Li? (aq) + O2? (aq) ? Li2O(s)
C) 2 Li? (g) + O2? (g) ? Li2O(s)
D) Li2O(s) ? 2 Li? (aq) + O2? (aq)
E) 2 Li(s) + 1/2O2(g) ? Li2O(s)


Answer: C

Use Lewis theory to determine the chemical formula for the compound formed between K and I.

Use Lewis theory to determine the chemical formula for the compound formed between K and I.

A) KI2
B) K2I
C) KI
D) K2I2


Answer: C

Use Lewis theory to determine the chemical formula for the compound formed between Ca and N.

Use Lewis theory to determine the chemical formula for the compound formed between Ca and N.

A) Ca3N2
B) Ca2N3
C) CaN2
D) CaN


Answer: A

Use Lewis theory to determine the chemical formula for the compound formed between Al and O.

Use Lewis theory to determine the chemical formula for the compound formed between Al and O.

A) Al3O2
B) Al2O3
C) AlO2
D) Al2O
E) AlO


Answer: B

Use Lewis theory to determine the chemical formula for the compound formed between Mg and Br.

Use Lewis theory to determine the chemical formula for the compound formed between Mg and Br.

A) MgBr
B) Mg2Br3
C) Mg3Br2
D) MgBr2
E) Mg2Br


Answer: D

Use Lewis theory to determine the chemical formula for the compound formed between Rb and S.

Use Lewis theory to determine the chemical formula for the compound formed between Rb and S.

A) RbS
B) RbS2
C) Rb2S
D) Rb2S3
E) Rb3S2


Answer: C

Use Lewis theory to determine the chemical formula for the compound formed between Ca and N.

Use Lewis theory to determine the chemical formula for the compound formed between Ca and N.

A) CaN
B) Ca3N2
C) CaN2
D) Ca2N
E) Ca2N3


Answer: B

Which of the following statements is TRUE?

Which of the following statements is TRUE?

A) A covalent bond is formed through the transfer of electrons from one atom to another.
B) A pair of electrons involved in a covalent bond are sometimes referred to as "lone pairs."
C) It is not possible for two atoms to share more than two electrons.
D) Single bonds are shorter than double bonds.
E) A covalent bond has a lower potential energy than the two separate atoms.


Answer: E

Give the ground state electron configuration for Mg2+.

Give the ground state electron configuration for Mg2+.

A) 1s22s22p63s2
B) 1s22s22p6
C) 1s22s22p63s23p2
D) 1s22s22p63s23p6
E) 1s22s22p63s1



Answer: B

Give the ground state electron configuration for Br-.

Give the ground state electron configuration for Br-.

A) [Ar]4s23d104p6
B) [Ar]4s23d104p5
C) [Ar]4s24p6
D) [Ar]4s24d104p6
E) [Ar]4s23d104p4



Answer: A

How many of the following species are diamagnetic? Cs Zr2+ Al3+ Hg2+

How many of the following species are diamagnetic?
Cs Zr2+ Al3+ Hg2+

A) 1
B) 3
C) 0
D) 2
E) 4


Answer: D

How many of the following species are paramagnetic? Sc3+ Br- Mg2+ Se

How many of the following species are paramagnetic?
Sc3+ Br- Mg2+ Se

A) 0
B) 2
C) 1
D) 4
E) 3


Answer: C

Choose the paramagnetic species from below.

Choose the paramagnetic species from below.

A) Ti4+
B) O
C) Ar
D) All of the above are paramagnetic.
E) None of the above are paramagnetic.


Answer: B

Choose the diamagnetic species from below.

Choose the diamagnetic species from below.

A) Sn2+
B) Br
C) P
D) Cr
E) None of the above are diamagnetic.


Answer: A

Place the following in order of decreasing metallic character. P As K

Place the following in order of decreasing metallic character.
P As K

A) P > As > K
B) As > P > K
C) K > P > As
D) As > K > P
E) K > As > P


Answer: E

Place the following in order of increasing IE1. K Ca Rb

Place the following in order of increasing IE1.
K Ca Rb

A) Ca < K < Rb
B) Rb < Ca < K
C) Ca < Rb < K
D) Rb < K < Ca
E) K < Ca < Rb


Answer: D

Place the following in order of decreasing IE1. Cs Mg Ar

Place the following in order of decreasing IE1.
Cs Mg Ar

A) Cs > Mg > Ar
B) Mg > Ar > Cs
C) Ar > Mg > Cs
D) Cs > Ar > Mg
E) Mg > Cs > Ar


Answer: C

Place the following in order of increasing IE1. N F As

Place the following in order of increasing IE1.
N F As

A) N < As < F
B) As < N < F
C) F < N < As
D) As < F < N
E) F < N < As


Answer: B

What period 3 element having the following ionization energies (all in kJ/mol)? IE1 = 1012 IE2 = 1900 IE3= 2910 IE4= 4960 IE5= 6270 IE6 = 22,200

What period 3 element having the following ionization energies (all in kJ/mol)?
IE1 = 1012 IE2 = 1900 IE3= 2910 IE4= 4960 IE5= 6270 IE6 = 22,200

A) Si
B) S
C) P
D) Cl
E) Mg


Answer: C

Which reaction below represents the second ionization of Sr?

Which reaction below represents the second ionization of Sr?

A) Sr(g) ? Sr+ (g) + e-
B) Sr2+ (g) + e- ? Sr+ (g)
C) Sr+ (g) + e-? ? Sr(g)
D) Sr- (g) + e- ? Sr2- (g)
E) Sr+ (g) ? Sr2+ (g) + e-


Answer: E

Which reaction below represents the first ionization of O?

Which reaction below represents the first ionization of O?

A) O+ (g) + e- ? O(g)
B) O(g) + e- ? O- (g)
C) O- (g) ? O(g) + e-
D) O(g) ? O+ (g) + e-
E) O- (g) + e- ? O2- (g)


Answer: D

Choose the statement that is TRUE.

Choose the statement that is TRUE.

A) Outer electrons efficiently shield one another from nuclear charge.
B) Core electrons effectively shield outer electrons from nuclear charge.
C) Valence electrons are most difficult of all electrons to remove.
D) Core electrons are the easiest of all electrons to remove.
E) All of the above are true.


Answer: B

Place the following in order of decreasing radius. Te2- F- O2-

Place the following in order of decreasing radius.
Te2- F- O2-

A) F- > O2- > Te2-
B) F- > Te2- > O2-
C) Te2- > O2- > F-
D) Te2- > F- > O2-
E) O2- > F- > Te2-


Answer: C

Place the following in order of increasing radius. Br- Na+ Rb+

Place the following in order of increasing radius.
Br- Na+ Rb+

A) Br- < Rb+ < Na+
B) Na+ < Rb+ < Br-
C) Rb+ < Br- < Na+
D) Br- < Na+ < Rb+
E) Rb+ < Na+ < Br-


Answer: B

Place the following in order of increasing radius. Ca2+ S2- Cl-

Place the following in order of increasing radius.
Ca2+ S2- Cl-

A) Ca2+ < Cl- < S2-
B) Cl- < Ca2+ < S2-
C) S2- < Cl- < Ca2+
D) Ca2+ < S2-< Cl-
E) Cl- < S2- < Ca2+


Answer: A

Place the following in order of increasing atomic radius. As O Br

Place the following in order of increasing atomic radius.
As O Br

A) As < Br < O
B) O < As < Br
C) Br < As < O
D) As < O < Br
E) O < Br < As


Answer: E

Place the following elements in order of decreasing atomic radius. Xe Rb Ar

Place the following elements in order of decreasing atomic radius.
Xe Rb Ar

A) Ar > Xe > Rb
B) Xe > Rb > Ar
C) Ar > Rb > Xe
D) Rb > Xe > Ar
E) Rb > Ar > Xe


Answer: D

Place the following elements in order of increasing atomic radius. P Ba Cl

Place the following elements in order of increasing atomic radius.
P Ba Cl

A) Ba < P < Cl
B) P < Cl < Ba
C) Cl < P < Ba
D) Cl < Ba < P
E) Ba < Cl < P


Answer: C

Give the complete electronic configuration for Mn.

Give the complete electronic configuration for Mn.

A) 1s22s22p63s23p64s24d5
B) 1s22s22p63s23p64s13d6
C) 1s22s22p63s23p64s23d5
D) 1s22s22p63s23p64s24p5


Answer: C

How many valence electrons do the halogens possess?

How many valence electrons do the halogens possess?

A) 5
B) 6
C) 2
D) 1
E) 7


Answer: E

How many valence electrons does an atom of Al possess?

How many valence electrons does an atom of Al possess?

A) 1
B) 2
C) 5
D) 3
E) 8


Answer: D

How many valence electrons does an atom of Cu possess?

How many valence electrons does an atom of Cu possess?

A) 2
B) 9
C) 11
D) 3
E) 1


Answer: E

How many valence electrons does an atom of Ti possess?

How many valence electrons does an atom of Ti possess?

A) 2
B) 4
C) 6
D) 8
E) 0


Answer: A

How many valence electrons does an atom of Ba possess?

How many valence electrons does an atom of Ba possess?

A) 2
B) 1
C) 8
D) 6
E) 3


Answer: A

How many valence electrons does an atom of S have?

How many valence electrons does an atom of S have?

A) 3
B) 1
C) 2
D) 4
E) 6


Answer: E

Identify the number of valence electrons for Mn.

Identify the number of valence electrons for Mn.

A) 8
B) 7
C) 5
D) 2


Answer: D

How many of the following elements have 1 unpaired electron in the ground state? B Al S Cl

How many of the following elements have 1 unpaired electron in the ground state?
B Al S Cl

A) 1
B) 2
C) 3
D) 4


Answer: C

How many of the following elements have 2 unpaired electrons in the ground state? C O Ti Si

How many of the following elements have 2 unpaired electrons in the ground state?
C O Ti Si

A) 1
B) 2
C) 3
D) 4


Answer: D

Write out the orbital diagram that represents the ground state of As. How many unpaired electrons are there?

Write out the orbital diagram that represents the ground state of As. How many unpaired electrons are there?

A) 0
B) 4
C) 3
D) 2
E) 1


Answer: C

How many unpaired electrons are present in the ground state Ge atom?

How many unpaired electrons are present in the ground state Ge atom?

A) 0
B) 3
C) 1
D) 2
E) 4


Answer: D

How many unpaired electrons are present in the ground state Kr atom?

How many unpaired electrons are present in the ground state Kr atom?

A) 1
B) 2
C) 0
D) 3
E) 5


Answer: C

How many unpaired electrons are present in the ground state P atom?

How many unpaired electrons are present in the ground state P atom?

A) 0
B) 3
C) 1
D) 2
E) 4


Answer: B

Identify the element that has a ground state electronic configuration of [Ar]4s23d104p1.

Identify the element that has a ground state electronic configuration of [Ar]4s23d104p1.

A) Al
B) In
C) Ga
D) B


Answer: C

Identify the element that has a ground state electronic configuration of [Kr]5s24d5.

Identify the element that has a ground state electronic configuration of [Kr]5s24d5.

A) Tc
B) Mn
C) Nb
D) Ru


Answer: A

Give the ground state electron configuration for Cd.

Give the ground state electron configuration for Cd.

A) [Kr]5s25d10
B) [Kr]5s24d105p2
C) [Kr]4d10
D) [Kr]5s24d8
E) [Kr]5s24d10


Answer: E

Give the ground state electron configuration for Pb.

Give the ground state electron configuration for Pb.

A) [Xe]6s26p2
B) [Xe]6s25d106p2
C) [Xe]6s25f146d106p2
D) [Xe]6s24f145d106p2
E) [Xe]6s25f145d106p2


Answer: D

Give the ground state electron configuration for Sr.

Give the ground state electron configuration for Sr.

A) [Kr]5s24d2
B) [Kr]5s24d105p2
C) [Kr]5s2
D) [Kr]5s25d105p2
E) [Kr]5s24d10


Answer: C

Give the ground state electron configuration for I.

Give the ground state electron configuration for I.

A) [Kr]5s24d105p6
B) [Kr]5s24d105p5
C) [Kr]4d105p6
D) [Kr]5s25p6
E) [Kr]5s25d105p6


Answer: B

Give the ground state electron configuration for Se.

Give the ground state electron configuration for Se.

A) [Ar]4s23d104p4
B) [Ar]4s24d104p4
C) [Ar]4s23d104p6
D) [Ar]4s23d10
E) [Ar]3d104p4


Answer: A

Which of the following statements is TRUE?

Which of the following statements is TRUE?

A) An orbital that penetrates into the region occupied by core electrons is less shielded from nuclear charge than an orbital that does not penetrate and therefore has a lower energy.
B) An orbital that penetrates into the region occupied by core electrons is more shielded from nuclear charge than an orbital that does not penetrate and therefore has a lower energy.
C) It is possible for two electrons in the same atom to have identical values for all four quantum numbers.
D) Two electrons in the same orbital can have the same spin.
E) None of the above are true.


Answer: A

Give the set of four quantum numbers that represent the last electron added (using the Aufbau principle) to the Zn atom.

Give the set of four quantum numbers that represent the last electron added (using the Aufbau principle) to the Zn atom.

A) n = 4, l = 3, ml = 3, ms = -
B) n = 3, l = 2, ml = 2, ms = -
C) n = 3, l = 1, ml = 1, ms = +
D) n = 3, l = 3, ml = 2, ms = -
E) n = 4, l = 2, ml = 0, ms = +


Answer: B

Give the set of four quantum numbers that could represent the last electron added (using the Aufbau principle) to the Sr atom.

Give the set of four quantum numbers that could represent the last electron added (using the Aufbau principle) to the Sr atom.

A) n = 5, l = 0, ml = 0, ms = -
B) n = 4, l = 1, ml = 1, ms = -
C) n = 5, l = 1, ml = 0, ms = +
D) n = 4, l = 1, ml = -1, ms = +
E) n = 5, l = 1, ml =1 , ms = -


Answer: A

Give the set of four quantum numbers that could represent the last electron added (using the Aufbau principle) to the Cl atom.

Give the set of four quantum numbers that could represent the last electron added (using the Aufbau principle) to the Cl atom.

A) n = 3, l = 1, ml = 1, ms = +
B) n = 3, l = 0, ml = 1, ms = -
C) n = 3, l = 2, ml =1 , ms = +
D) n = 2, l = 1, ml = 1, ms = -
E) n = 3, l =2 , ml = 1, ms = -


Answer: A

Choose the orbital diagram that represents the ground state of N.

Choose the orbital diagram that represents the ground state of N.

A)
B)
C)
D)
E)


Answer: A

No two electrons can have the same four quantum number is known as

No two electrons can have the same four quantum number is known as

A) Pauli exclusion principle
B) Hund's rule
C) Aufbau principle
D) Heisenberg uncertainty principle


Answer: A

If two electrons in the same atom have the same value of "l", they are

If two electrons in the same atom have the same value of "l", they are

A) in the same sublevel, but not necessarily in the same level.
B) in the same level, but different sublevel.
C) in the same orbital.
D) in different levels and in different shaped orbitals.
E) None of the above


Answer: A

How many different values of ml are possible in the 3d sublevel?

How many different values of ml are possible in the 3d sublevel?

A) 2
B) 1
C) 3
D) 5
E) 7


Answer: D

How many different values of l are possible in the third principal level?

How many different values of l are possible in the third principal level?

A) 1
B) 2
C) 3
D) 0
E) 4


Answer: C

How many different values of ml are possible in the 4f sublevel?

How many different values of ml are possible in the 4f sublevel?

A) 1
B) 7
C) 3
D) 5
E) 2


Answer: B

Which of the following quantum numbers describes the orientation of an orbital?

Which of the following quantum numbers describes the orientation of an orbital?

A) magnetic quantum number
B) principal quantum number
C) angular momentum quantum number
D) spin quantum number
E) Schrödinger quantum number


Answer: A

Which of the following quantum numbers describes the shape of an orbital?

Which of the following quantum numbers describes the shape of an orbital?

A) principal quantum number
B) magnetic quantum number
C) spin quantum number
D) Schrödinger quantum number
E) angular momentum quantum number


Answer: E

Which of the following statements are TRUE?

Which of the following statements are TRUE?

A) We can sometimes know the exact location and speed of an electron at the same time.
B) All orbitals in a given atom are roughly the same size.
C) Since electrons have mass, we must always consider them to have particle properties and never wavelike properties.
D) Atoms are roughly spherical because when all of the different shaped orbitals are overlapped, they take on a spherical shape.
E) All of the above are true.


Answer: D

How many sublevels are contained in the second shell (n=2) of a given atom?

How many sublevels are contained in the second shell (n=2) of a given atom?

A) 1
B) 2
C) 9
D) 4
E) 3


Answer: B

How many orbitals are contained in the third principal level (n=3) of a given atom?

How many orbitals are contained in the third principal level (n=3) of a given atom?

A) 9
B) 3
C) 18
D) 7
E) 5


Answer: A

Each of the following sets of quantum numbers is supposed to specify an orbital. Choose the one set of quantum numbers that does not contain an error.

Each of the following sets of quantum numbers is supposed to specify an orbital. Choose the one set of quantum numbers that does not contain an error.

A) n = 4, l = 4, ml =0
B) n = 3, l = 2, ml =+3
C) n = 4, l = 0, ml =-1
D) n = 3, l = 1, ml = -2
E) n = 5, l = 3, ml =-3


Answer: E

Each of the following sets of quantum numbers is supposed to specify an orbital. Choose the one set of quantum numbers that does not contain an error.

Each of the following sets of quantum numbers is supposed to specify an orbital. Choose the one set of quantum numbers that does not contain an error.

A) n = 2, l = 2, ml =-1
B) n = 2, l = 2, ml =0
C) n = 3, l = 2, ml =-3
D) n = 4, l = 3, ml =-2
E) n = 4, l = 2, ml =+4


Answer: D

Each of the following sets of quantum numbers is supposed to specify an orbital. Which of the following sets of quantum numbers contains an error?

Each of the following sets of quantum numbers is supposed to specify an orbital. Which of the following sets of quantum numbers contains an error?

A) n = 2, l = 1 , ml = -1
B) n = 4, l = 2, ml =0
C) n = 3, l =3 , ml = -2
D) n = 1, l = 0, ml =0
E) n = 3, l = 0, ml =0


Answer: C

What value of l is represented by a d orbital?

What value of l is represented by a d orbital?

A) 1
B) 2
C) 0
D) 3


Answer: B

What are the possible orbitals for n = 3?

What are the possible orbitals for n = 3?

A) s, p, d
B) s, p, d, f
C) s
D) s, p


Answer: A

For n = 3 what are the possible sublevels?

For n = 3 what are the possible sublevels?

A) 0
B) 0, 1
C) 0, 1, 2
D) 0, 1,2, 3


Answer: C

Which of the following transitions represent the emission of a photon with the largest energy?

Which of the following transitions represent the emission of a photon with the largest energy?

A) n = 2 to n = 1
B) n = 3 to n = 1
C) n = 6 to n = 3
D) n = 1 to n = 4
E) n = 2 to n = 5


Answer: B

Choose the transition (in a hydrogen atom) below that represents the absorption of the shortest wavelength photon.

Choose the transition (in a hydrogen atom) below that represents the absorption of the shortest wavelength photon.

A) n = 1 to n = 2
B) n = 2 to n = 3
C) n = 4 to n = 5
D) n = 6 to n = 3
E) n = 3 to n = 1


Answer: A

Which of the following transitions (in a hydrogen atom) represent absorption of the smallest frequency photon?

Which of the following transitions (in a hydrogen atom) represent absorption of the smallest frequency photon?

A) n = 5 to n = 6
B) n = 5 to n = 4
C) n = 4 to n = 1
D) n = 1 to n = 3
E) n = 1 to n = 2


Answer: A

Which of the following transitions (in a hydrogen atom) represent emission of the longest wavelength photon?

Which of the following transitions (in a hydrogen atom) represent emission of the longest wavelength photon?

A) n = 1 to n = 2
B) n = 3 to n = 1
C) n = 3 to n = 4
D) n = 4 to n = 2
E) n = 5 to n = 4


Answer: E

It is possible to determine the ionization energy for hydrogen using the Bohr equation. Calculate the ionization energy for an atom of hydrogen making the assumption that ionization is the transition from n=1 to n=8.

It is possible to determine the ionization energy for hydrogen using the Bohr equation. Calculate the ionization energy for an atom of hydrogen making the assumption that ionization is the transition from n=1 to n=8.

A) -2.18 × 10-18 J
B) +2 .18 × 10-18 J
C) +4.59 × 10-18 J
D) -4.59 × 10-18 J
E) +4.36 x 10-18 J


Answer: B

Determine the velocity of a medicine ball (m = 10.0 kg) with a wavelength of 1.33 × 10-35 m.

Determine the velocity of a medicine ball (m = 10.0 kg) with a wavelength of 1.33 × 10-35 m.

A) 8.81 m/s
B) 12.3 m/s
C) 2.21 m/s
D) 4.98 m/s
E) 6.44 m/s


Answer: D

Determine the velocity of a marble (m = 8.66 g) with a wavelength of 3.46 × 10-33 m.

Determine the velocity of a marble (m = 8.66 g) with a wavelength of 3.46 × 10-33 m.

A) 45.2 m/s
B) 11.3 m/s
C) 22.1 m/s
D) 38.8 m/s
E) 52.9 m/s


Answer: C

Calculate the wavelength of a baseball (m = 155 g) moving at 32.5 m/s.

Calculate the wavelength of a baseball (m = 155 g) moving at 32.5 m/s.

A) 7.60 × 10-36 m
B) 1.32 × 10-34 m
C) 2.15 × 10-32 m
D) 2.68 × 10-34 m
E) 3.57 × 10-32 m


Answer: B

Calculate the wavelength of an electron (m = 9.11 × 10-28 g) moving at 3.66 × 106 m/s.

Calculate the wavelength of an electron (m = 9.11 × 10-28 g) moving at 3.66 × 106 m/s.

A) 1.99 × 10-10 m
B) 5.03 × 10-10 m
C) 1.81 × 10-10 m
D) 5.52 × 10-9 m
E) 2.76 × 10-9 m


Answer: A

Which of the following statements is TRUE?

Which of the following statements is TRUE?

A) The emission spectrum of a particular element is always the same and can be used to identify the element.
B) Part of the Bohr model proposed that electrons in the hydrogen atom are located in "stationary states" or particular orbits around the nucleus.
C) The uncertainty principle states that we can never know both the exact location and speed of an electron.
D) An orbital is the volume in which we are most likely to find an electron.
E) All of the above are true.


Answer: E

Determine the longest wavelength of light required to remove an electron from a sample of potassium metal if the binding energy for an electron in K is 1.76 × 103 kJ/mol.

Determine the longest wavelength of light required to remove an electron from a sample of potassium metal if the binding energy for an electron in K is 1.76 × 103 kJ/mol.

A) 147 nm
B) 68.0 nm
C) 113 nm
D) 885 nm
E) 387 nm


Answer: B

Determine the shortest frequency of light required to remove an electron from a sample of Ti metal if the binding energy of titanium is 3.14 × 103 kJ/mol.

Determine the shortest frequency of light required to remove an electron from a sample of Ti metal if the binding energy of titanium is 3.14 × 103 kJ/mol.

A) 7.87 x 1015 Hz
B) 4.74 x 1015 Hz
C) 2.11 x 1015 Hz
D) 1.27 x 1015 Hz
E) 6.19 x 1015 Hz


Answer: A

What total energy (in kJ) is contained in 1.0 mol of photons all with a frequency of 2.75 × 1014 Hz?

What total energy (in kJ) is contained in 1.0 mol of photons all with a frequency of 2.75 × 1014 Hz?

A) 182 kJ
B) 219 kJ
C) 457 kJ
D) 326 kJ
E) 110 kJ


Answer: E