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SDSMT - Exam 2 Review

Total questions: 34

Worksheet time: 26mins

Name
Class
Date
1.

What is the molecular shape and polarity for xenon tetrafluoride?

a)

Square Planar and non-polar

b)

Tetrahedral and non-polar

c)

Trigonal planar and non-polar

d)

Bent and polar

e)

Square planar and polar

2.

How many polar bonds does CCl4 have in its structure?

a)

0

b)

1

c)

2

d)

3

e)

4

3.

According to the octet rule, which of the elements will have a tendency to lose 2 electrons?

a)

Potassium

b)

Sulfur

c)

Oxygen

d)

Strontium

e)

Cesium

4.

What is the ground-state electron configuration of calcium?

a)

1s²2s²2p6

b)

1s²2s²2p 3s²4s8

c)

1s²2s²2p63s²3p64s²

d)

1s²2s²2p63s²

e)

1s²2s²2p63s²3p64s1

5.

According to VSEPR theory, the shape of an ammonium ion, NH4+, is most similar to:

a)

Trigonal pyramidal, 109.5°

b)

Trigonal planar, 120°

c)

Bent, 120°

d)

Trigonal pyramidal, 120°

e)

Trigonal planar, 90°

6.

Which of the following is true about Fe²+?

a)

Fe²+ is paramagnetic with 0 unpaired electrons

b)

Fe²+ is paramagnetic with 2 unpaired electrons

c)

Fe²+ is paramagnetic with 4 unpaired electrons

d)

Fe²+ is paramagnetic with 5 unpaired electrons

e)

Fe²+ is diamagnetic

7.

According to periodic trends, arrange the following ions, potassium K+, magnesium Mg2+, and aluminum Al³+ in order of increasing ionic size.

a)

K+ < Al³+ < Mg2+

b)

K+ < Mg2+ < Al³+

c)

Al³+ < K+ < Mg2+

d)

Al³+ < Mg2+ < K+

e)

Cannot predict the size trend

8.

Which element has the electron configuration 1s²2s²2p63s²3p64s²3d5?

a)

Tc

b)

Mo

c)

Mn

d)

Fe

e)

Cr

9.

Which of the following would be polar?

a)

CH4

b)

BF3

c)

C₂H₂

d)

CO₂

e)

CH3OH

10.

Which element has four valence electrons in it's Lewis symbol?

a)

sulfur

b)

iron

c)

germanium

d)

indium

e)

zinc

11.

Due to periodicity, which element would you expect to behave most like sodium?

a)

aluminum

b)

barium

c)

calcium

d)

oxygen

e)

potassium

12.

In what block, group, and period on the periodic table can the atom with a

1s22s22p63s23p64s23d104p5 ground-state electron configuration be found?

a)

p-block, group 17, and period 4

b)

d-block, group 7, and period 5

c)

p-block, group 17, and period 3

d)

p-block, group 17, and period 5

e)

d-block, group 7, and period 4

13.

A single electron occupies a subshell and has the quantum numbers n = 3, l = 0, ml = 0, ms = +½.

Which of the following is an acceptable set of quantum numbers for the next electron added to

this subshell? (Hint: draw an orbital diagram)

a)

3, 1, -1, -1/2

b)

3, 0, 0, +1/2

c)

3, 0, 0, -1/2

d)

3, 1, 0, +1/2

e)

3, 2, 0, +1/2

14.

A bright violet line occurs at 435.8 nm in the emission spectrum of mercury vapor. What is

energy of one photon of this light?

a)

4.56×10-28 J

b)

4.56×10-10 J

c)

6.88×1023 J

d)

4.56×10-19 J

e)

6.88×1014 J

15.

Draw the Lewis structure of BrF3, and then determine the bond angle(s) of F–Br–F.

a)

60°

b)

90° and 120°

c)

45°

d)

120°

e)

90° and 180°

16.

Based on the valence bond theory, HCl is formed by

a)

overlapping the 1s orbital of H and 2pz orbital of Cl to form a single σ bond

b)

overlapping the 2s orbital of H and 3pz orbital of Cl to form a single σ bond.

c)

overlapping the 1s orbital of H and 3pz orbital of Cl to form a single π bond.

d)

overlapping the 1s orbital of H and 2pz orbital of Cl to form a single π bond.

e)

overlapping the 1s orbital of H and 3pz orbital of Cl to form a single σ bond.

17.

Draw the Lewis structure for the hydronium ion (H3O+) and determine the molecular geometry.

Predict the bonding angle of H-O-H according to the VSEPR model.

a)

120o

b)

109.5o

c)

180o

d)

Slightly smaller than 109.5o

e)

Slightly greater than 109.5o

18.

An FM radio station found at 103.1 on the FM dial broadcasts at a frequency of

1.031 x 108 s-1 (103.1 MHz). What is the wavelength of these radio waves in meters?

a)

2.908 × 106 m

b)

2.908 m

c)

2.908 × 104 m

d)

34.27 m

e)

3.427 × 10-1 m

19.

Which of the following is not permitted as a plausible orbital designation according to quantum

theory.

a)

2d

b)

6p

c)

4f

d)

5f

e)

1s

20.

What is the electron configuration of Cu+ and Cu2+ ?

a)

[Ar]3d94s1 and [Ar]3d9

b)

[Ar]3d84s2 and [Ar]3d84s1

c)

[Ar]3d94s1 and [Ar]3d84s1

d)

[Ar]3d10 and [Ar]3d9

e)

[Ar]3d94s1 and [Ar]3d74s2

21.

Using VSEPR theory, predict the molecular shape and bond angles in BCl3.

a)

bent, 120°

b)

trigonal pyramidal, 120°

c)

trigonal planar, 90°

d)

trigonal pyramidal, 109.5°

e)

trigonal planar, 120°

22.

According to periodic trends, which metal has the lowest ionization energy?

a)

Cs

b)

K

c)

Na

d)

Li

e)

Rb

23.

Draw a Lewis structure for the SF5– molecule. What is the set of hybrid orbitals used by the

sulfur atom for bonding?

a)

sp5

b)

sp3

c)

sp3d

d)

sp2

e)

sp3d2

24.

How many σ-bonds and π-bonds, respectively, are in a COCl2 molecule?

a)

2 σ-bonds and 2 π-bonds

b)

4 σ-bonds and 0 π-bonds

c)

3 σ-bonds and 2 π-bonds

d)

3 σ-bonds and 1 π-bond

e)

2 σ-bond and 1 π-bond

25.

Which of the following is an ionic compound?

a)

CuZn

b)

Na2O

c)

CO2

d)

HCl

e)

CO

26.

Based on the geometry of the molecule IF5, what are the bond angles of F–I–F?

a)

180°

b)

120°

c)

90°

d)

109.5°

e)

Can not be determined

27.

Identify the transition metal ion and the number of electrons with the following electron

configuration, [Ar]3d7.

a)

cobalt and 27 electrons

b)

cobalt (I) ion and 26 electrons

c)

cobalt (III) ion and 24 electrons

d)

manganese and 25 electrons

e)

cobalt (II) ion and 25 electrons

28.

The Lewis structure of SeCl3+: is:

a)

b)

c)

d)

e)

29.

In the Lewis structure below, M and X represent various elements in the third period of the

periodic table. The formula of the compound is:

a)

CaO

b)

MgP

c)

CaS

d)

MgS

e)

MgO

30.

What is the hybridization type of nitrogen?

a)

sp3d

b)

sp2

c)

sp3

d)

sp

e)

sp3d2

31.

Which of the following elements have a tendency to gain electrons?

a)

N, O, Al

b)

Cl, O, F

c)

Cl, F, Ga

d)

Na, K, Ca

e)

Cl, B, Al

32.

According to periodic trends, which element is the most electronegative?

a)

Cl

b)

O

c)

F

d)

S

e)

Ne

33.

The compound CF2Cl2 is:

a)

Nonpolar covalent

b)

Ionic

c)

Not enough information

d)

Metalic

e)

Polar Covalent

34.

Identify which of the following molecules has a double bond.

a)

HF

b)

O2

c)

N2

d)

H2

e)

Br2

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