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Chemistry Molecular Geometry Unit 2

Total questions: 81

Worksheet time: 1hrs 21mins

Name
Class
Date
1.
Choose the correct shape for this molecule:
a)
Trigonal planar
b)
Trigonal pyramidal
c)
Tetrahedral
d)
Linear
2.
Choose the correct shape for this molecule:
a)
Trigonal planar
b)
Trigonal pyramidal
c)
Bent
d)
Linear
3.
Choose the correct shape for this molecule:
a)
Bent
b)
Trigonal pyramidal
c)
Trigonal planar
d)
Linear
4.
Choose the correct shape for this molecule:
a)
Trigonal planar
b)
Trigonal pyramidal
c)
Bent
d)
Tetrahedral
5.
Choose the correct shape for this molecule:
a)
linear
b)
Trigonal pyramidal
c)
Bent
d)
Tetrahedral
6.
Choose the correct shape for this molecule:
a)
linear
b)
Trigonal pyramidal
c)
Bent
d)
Tetrahedral
7.
Choose the correct shape for this molecule:
a)
linear
b)
Trigonal pyramidal
c)
Bent
d)
Trigonal planar
8.
Choose the correct shape for this molecule:
a)
Tetrahedral
b)
Trigonal pyramidal
c)
Bent
d)
Trigonal planar
9.
Choose the correct shape for this molecule:
a)
Bent
b)
Trigonal pyramidal
c)
Tetrahedral
d)
Trigonal planar
10.
Choose the correct shape for this molecule:
a)
Bent
b)
Linear
c)
Tetrahedral
d)
Trigonal pyramidal
11.
What geometry will this molecular structure have?: H2S
a)
bent
b)
tetrahedral
c)
linear
d)
trigonal pyramidal
12.
What two types of atoms make a covalent bond?
a)
2 Nonmetals
b)
1 Nonmetal and 1 Metal
c)
2 Metals
d)
2 Noble Gases
13.
Phosphorous trichloride
a)
PCl3
b)
P3Cl
c)
P3Cl3
d)
PCL
14.
Bromine monoflouride
a)
Br1F1
b)
BrF
c)
Br2F
d)
BrF2
15.
Disulfur trioxide
a)
S3O2
b)
SO
c)
S2O3
d)
S2O
16.
P2O5
a)
Phosphorus Oxide
b)
Pentaphosphorus Dioxide
c)
Diphosphorous pentoxide
d)
Phosphoric Oxygen
17.
How many electrons should Oxygen have around its Lewis dot model?
a)
5
b)
6
c)
7
d)
8
18.
What is the correct formula for this molecule?
a)
NH
b)
N3H
c)
NH3
d)
NH4
19.
According to the octet rule most elements need _______ valence electrons.
a)
2
b)
8
c)
6
d)
18
20.
This is a correct dot diagram for fluorine (F)
a)
true
b)
false
21.
This is a correct dot diagram for oxygen (O)
a)
true
b)
false
22.

The geometry of a molecule with 2 bonded pairs of electrons and 2 lone pairs of electrons, AB2E2

a)

Tetrahedral

b)

Trigonal Planar

c)

Bent

d)

Trigonal Pyramidal

e)

Linear

23.

The geometry of a molecule with 3 bonded pairs of electrons and 0 lone pairs of electrons, AB3

a)

Tetrahedral

b)

Trigonal Planar

c)

Bent

d)

Trigonal Pyramidal

e)

Linear

24.
*
a)
linear
b)
trigonal planar
c)
trigonal pyramid
d)
bent of angular
25.
*
a)
trigonal pyramid
b)
linear
c)
bent
d)
angular
26.

The Lewis structure of N2H2 shows __________.

a)

a nitrogen-nitrogen triple bond

b)

a nitrogen-nitrogen single bond

c)

each nitrogen has one lone pair

d)

each nitrogen has two lone pairs

e)

each hydrogen has one lone pair

27.

In the nitrite ion (NO2-), __________.

a)

both bonds are single bonds

b)

both bonds are double bonds

c)

both bonds are the same because of resonance

d)

there are 20 valence electrons

e)

there is one single and one double bond

28.

The ability of an atom in a molecule to attract electrons is best quantified by the ______.

a)

electronegativity

b)

paramagnetism

c)

diamagnetism

d)

electron change-to-mass ratio

e)

first ionization energy

29.

Which atom can accommodate an octet of electrons, but doesn't necessarily have to accommodate an octet?

a)

N

b)

C

c)

H

d)

O

e)

B

30.

As the number of covalent bonds between two atoms increases, the distance between the atoms ______ and the strength of the bond between them ______.

a)

increases, increases

b)

decreases, decreases

c)

increases, decreases

d)

decreases, increases

e)

is unpredictable

31.

The Lewis structure of the CO32- ion is

a)
b)
c)
d)
e)
32.

Which of these bonds takes the most energy to break?

a)

single

b)

double

c)

triple

d)

quadruple

33.

The ion NO- has _____ valence electrons.

a)

10

b)

12

c)

14

d)

15

e)

16

34.

Potassium iodide, KI,has the following bonding:

a)

ionic

b)

metallic

c)

nonpolar covalent

d)

polar covalent

35.
The electronegativity of C is 2.5, F is 4.0.  predict the character of a C-F bond.
a)
polar covalent
b)
nonpolar covalent
c)
ionic
d)
metallic
36.
The following molecules all contain polar bonds however only one is a polar molecule.  Which one?
a)
CCl4
b)
CO2
c)
NH3
d)
CH4
37.
 A lone pair is defined as
a)
A pair of bonding electrons
b)
One non-bonding electron
c)
A pair of non-bonding electrons
d)
A pair of electrons on the central atom
38.
How are compounds with metallic bonds similar to ionic compounds? 
a)
Both tend to have double and triple bonds
b)
Both tend to have low boiling points 
c)
Both tend to have poor conductivity
d)
Both tend to have high melting points 
39.
What is the VSPER shape of PCl5
a)
See-saw
b)
trigonal planar
c)
octahedral
d)
trigonal bipyramidal
40.
Of the following molecules, which has the largest dipole moment?
a)
CO
b)
CO2
c)
O2
d)
HF
41.
What is the VSEPR theory used to predict?
a)
Bond Strength
b)
Polarity
c)
Molecular Shape
d)
Electronegativity
42.

Is this molecule polar or non-polar?

a)

Polar

b)

Non-polar

43.

Is this molecule polar or non-polar?

a)

Polar

b)

Non-polar

44.

Is this molecule polar or non-polar?

a)

Non-polar

b)

Polar

45.

Is this molecule polar or non-polar?

a)

Non-polar

b)

Polar

46.
In covalent bonds, electrons are ___________.
a)
transferred
b)
gained
c)
lost
d)
shared
47.
In a polar covalent bond, electrons are shared ___________.
a)
equally
b)
unequally
c)
between non-metals with similar electronegativities
d)
between a metal and a non-metal
48.
In this Lewis structure, the symbol above F means...
a)
electrons are being transferred to Fluorine
b)
electrons are less attracted to F than H
c)
electrons are more attracted to F than H
d)
Fluorine has formed a cation
49.
This is an example of a __________ bond.
a)
non-polar covalent
b)
polar covalent
c)
ionic
d)
metallic
50.
What atom matches this electron configuration?
1s22s22p63s23p64s23d10
a)
Zinc
b)
Copper
c)
Nickel
d)
Germanium
51.
What atom matches this electron configuration?
1s22s22p63s2
a)
Neon
b)
Magnesium
c)
Aluminum
d)
Potassium
52.
What electron configuration matches an oxygen atom?
a)
1s22s22p63s2, 3p64s23d104p5
b)
1s22s22p4
c)
1s22s22p6
d)
1s22s22p63s23p64s23d1
53.
How many electrons does Si contain? (click to see image)
a)
14
b)
28
c)
2
d)
4
54.
How many electrons can the first energy level hold?
a)
1
b)
2
c)
8
d)
0
55.
There are 4 different types of subshells s,p,d,f
a)
true
b)
false
56.
How many valence electrons are represented here?
a)
7
b)
5
c)
2
d)
8
57.
How many d orbitals are there in a given sublevel?
a)
1
b)
3
c)
5
d)
7
58.
How many p orbitals are there in a sublevel?
a)
2
b)
1
c)
4
d)
3
59.
How many electrons can the d sublevel hold?
a)
8
b)
10
c)
2
d)
4
60.
What atom matches this electron configuration?
[Xe] 6s2 4f14 5d9
a)
Mercury
b)
Gold
c)
Platinum
d)
Thallium
61.
What is the shorthand electron configuration for Sulfur atom?
a)
[Ar] 3p4
b)
[He] 3s23p4
c)
[Ne] 3s23p4
d)
[Na] 3s23p3
62.
Which element is pictured?
a)
neon
b)
fluorine
c)
magnesium
d)
argon
63.

The image is a model of a/an_____

a)

atom

b)

molecule

c)

compound

d)

element

64.

An atom is described by which of the following?

a)

The smallest unit of an element that has the chemical identity of that element.

b)

It is the incorrect spelling of Adam.

c)

Can only be described by its volume.

d)

Something that Mr. Crear did not discuss with me.

65.

What is an element?

a)

Two or more substances combined.

b)

The shorthand spelling of "elementary."

c)

A substance that cannot be separated or broken down into simpler substances by chemical means.

66.

What were John Dalton three contributions to atomic history?

a)

Created the atomic theory

b)

Discovered that the atom is mostly empty space

c)

Believed that atoms of a given element are identical

d)

Hypothesized that the atom is a tiny, hard sphere

e)

Believed that the universe was made of tiny "uncuttable" particles

67.

What were J. J. Thomson's three contributions to the atomic theory?

a)

Discovered the electron

b)

Discovered the nucleus -did the gold foil experiment

c)

Used the cathode ray tube in his discovery

d)

Created a model of the atom with electrons moving around the nucleus in fixed orbits

e)

Created the "plum pudding" model of the atom

68.
Which scientist saw the atom as a solid sphere?
a)
Dalton
b)
Thomson
c)
Rutherford
d)
Bohr
69.
In the Thomson Model, he discovered the existence of what particle?
a)
Electrons
b)
Protons
c)
Neutrons
d)
Quarks
70.
Rutherford’s experiment determined that the nucleus of an atom is tiny, dense and  ______ charged. 
a)
neutrally
b)
negatively
c)
positively
71.
He discovered the Theory of Relativity
a)
Harold Weinstein
b)
John Nash
c)
Albert Einstein
d)
Christiaan Huygens
72.
Created the periodic table of elements.
a)
Marie Curie
b)
Niels Bohr
c)
Enrico Fermi
d)
Dmitri Mendeleev
73.
Which scientist became known as "the father of the nuclear age"?
a)
J. J. Thomson
b)
John Dalton
c)
Ernest Rutherford
d)
Niels Bohr
74.
Who stipulated that electrons orbit the nucleus at fixed energies and distances?
a)
Albert Einstein
b)
Max Planck
c)
Ernest Rutherford
d)
Niels Bohr
75.
Who showed it was impossible to determine both the exact position and speed of electrons as they moved around an atom?
a)
Werner Heisenberg
b)
Niels Bohr
c)
Max Planck
d)
Albert Einstein
76.
Which is the second strongest intermolecular force, after hydrogen bonding?
a)
dipole-dipole attraction
b)
London forces
77.
All molecules have London forces between them, but dipole-dipole and hydrogen bonding are so much stronger that when they are present we can ignore London forces.  Which of these has ONLY London forces?
a)
I2
b)
NH3
c)
OCl2
d)
SH2
78.

Which substance would have the weakest intermolecular forces of attraction?

a)

CH4

b)

NaCl

c)

H2O

d)

MgF2

79.
What explains the very high melting and boiling point of water
a)
Strong dipole-dipole bonds between water molecules
b)
Strong hydrogen bonds between water molecules
c)
Dispersion forces which are present in all molecules
d)
Asymmetrical shape of the polar bonds.
80.

Intermolecular forces for: CO2

a)

Dispersion Force

b)

Dipole dipole

c)

Hydrogen bonding

81.
Which is the strongest intermolecular force below"
a)
Ionic
b)
Dispersion
c)
Hydrogen
d)
Metallic

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