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Molecular compounds practice

Total questions: 98

Worksheet time: 3hrs 32mins

Name
Class
Date
1.
phosphorus trichloride
a)
KCl3
b)
PCl3
c)
K3Cl
d)
P3Cl
2.
silicon dioxide
a)
SO2
b)
NaO2
c)
SiO2
d)
SiO
3.
diphosphorus pentoxide
a)
P2O5
b)
PO5
c)
P5O2
d)
P2O6
4.
SiCl4
a)
silicon tetrachloride
b)
silicon quadchloride
c)
monosilicon tetrachloride
d)
silicon chloride
5.
The chemical formula of sulfur hexabromide is
a)
SBr₆
b)
S₆Br
c)
S(VI)Br
d)
S6Br
6.
The chemical formula of carbon tetrachloride is
a)
CCl
b)
C₄Cl
c)
CCl₄
d)
C(IV)Cl
7.
The name of P₄S₁₀ is
a)
phosphorous sulfide
b)
phosphorus sulfide
c)
tetraphosphorus decasulfide
d)
phosphorus (X) sulfide
8.
The chemical formula of tetraphosphorus heptaoxide is
a)
F₄O₁₀
b)
P₄O7
c)
PO
d)
P₁₀O₄
9.
What is the correct name for NO?
a)
Mononitrogen Monoxide
b)
Nitrogen Monoxide
c)
Mononitrogen Dioxide
d)
Nitrogen Oxide
10.
What is the correct chemical formula for Nitrogen Triiodide?
a)
NI3
b)
N3I3
c)
NOI
d)
NeI3
11.
A binary covalent bond exists between
a)
2 metals
b)
1 metal and 1 nonmetal
c)
2 nonmetals
d)
Any 2 elements
12.

What is the formula for tetraphosphorous decasulfide?

a)

PS10

b)

P10S4

c)

P4S10

d)

P6S5

13.
The name of SO₃ compound is
a)
sulfate
b)
sulfur oxide
c)
sulfur trioxide
d)
monosulfur trioxide
14.

Molecular compounds are usually _________.

a)

composed of two or more transition elements

b)

composed of positive and negative ions

c)

composed of two or more nonmetallic elements

d)

exceptions to the law of definite proportions

15.

NaCl is a/an

a)

Ionic compound

b)

molecular compound

c)

Metallic compound

d)
Polyatomic Ion 
16.

Ionic compounds are formed between

a)
Metals and Metals
b)
Metals and Nonmetals
c)
Nonmetals and Nonmetals
d)
None of the above
17.
Which following is a nonmetal?
a)
Se
b)
Mn
c)
Na
d)
Be
18.
Which following is a molecular compound?
a)
SO2
b)
K2O
c)
CaO
d)
BeO
19.

What formula is created when Calcium and Chlorine form an ionic bond?

a)

CaCl

b)

CaCl2

c)

Ca2Cl

d)

Ca2Cl

20.

What is the correct name of MgCl2?

a)

magnesium chlorine

b)

magnesium dichloride

c)

magnesium chloride

d)

magnesium (II) chloride

21.

If the atoms that share electrons have an unequal attraction for the electrons, the bond is called

a)

nonpolar

b)

polar

c)

ionic

d)

dipole

22.

A neutral group of atoms held together by covalent bonds is a

a)

molecular formula

b)

chemical formula

c)

molecule

d)

monoatomic ion

23.

Why do most atoms form bonds?

a)

to be more stable by completing the octet

b)

to be less stable

c)

to add more electrons

d)

to carry out physical changes

24.

If two covalently bonded atoms are identical, the bond is

a)

coordinate covalent

b)

polar covalent

c)

dipole covalent

d)

nonpolar covalent

25.

What are shared in a covalent bond?

a)

ions

b)

Lewis structures

c)

dipoles

d)

electrons

26.

The C-H bond in CH3 (electronegativity for C is 2.55 and for H is 2.2) is

a)

polar covalent

b)

ionic

c)

nonpolar covalent

d)

metallic

27.

Which of the following occurs in an ionic bond?

a)

valence electrons are shared

b)

Two atoms share two electrons.

c)

Oppositely charged ions attract.

d)

Like-charged ions attract.

28.
In the correct Lewis structure for water, how many unshared pairs of electrons will oxygen have?
a)
1
b)
4
c)
3
d)
2
29.
Which of the following is the correct Lewis structure for the compound PBr3?
a)
structure A
b)
structure B
c)
structure C
d)
structure D
30.

Which is the correct molecular structure for carbon dioxide?

a)
b)
c)
d)
31.

How many double bonds are in CHCl3 ?

a)

0

b)

1

c)

2

d)

3

32.
Hydrogen needs _____ electrons in its valence shell to be stable.
a)
4
b)
6
c)
8
d)
2
33.
Three pairs of electrons are shared in a
a)
Single bond
b)
Double bond
c)
Triple bond
34.
Which of the following is the correct Lewis dot structure for the molecule fluorine (F2)?
a)
A
b)
B
c)
C
d)
D
35.
What is the correct structure for BF3?
a)
Option A.
b)
Option B. 
c)
Option C.
d)
Option D.
36.

How many valence electrons are available in the sulfate ion (SO4-2)?

a)
30 electrons
b)
32 electrons
c)
28 electrons
d)
impossible to tell
37.
How many valence electrons are available for bonding in the sulfate ion (SO4-2)?
a)
30 electrons
b)
32 electrons
c)
28 electrons
d)
impossible to tell
38.

What is the goal of the Lewis Dot Structure?

a)

To determine the electron position.

b)

To show the element's valence electrons & bonding capabilities.

c)

To find the atomic mass of an element.

d)

To search for the number of electrons in an individual atom.

39.

What is the correct Lewis structure for NH3?

a)
b)
c)
d)
40.
What is the correct formula for this molecule?
a)
Si4F
b)
SiF4
c)
SiF
d)
Si4F4
41.

Why is this Lewis Structure incorrect? Select all that appy.

a)

There should be a single bond between H and C.

b)

There should be a triple bond between C and N.

c)

Carbon has too many bonds around it.

d)

Hydrogen needs more electrons.

42.

How many total valence electrons are participating in bonding in the molecule below?

a)

8

b)

4

c)

2

d)

3

43.
Which of the following is the correct Lewis structure for CH2O?
a)
Option A
b)
Option B
c)
Option C
d)
Option D
44.

Which of these is the correct Lewis structure for SiBr4?

a)

A

b)

B

c)

C

d)

D

45.
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
46.
This is an example of a __________ bond.
a)
non-polar covalent
b)
polar covalent
c)
ionic
d)
metallic
47.

A diatomic molecule like O2 is always_______ because electrons are shared ________.

a)
nonpolar; equally
b)
polar; equally
c)
nonpolar; unequally
d)
nonpolar; unequally
48.

The geometry of CH4 molecule is:

a)

tetrahedral

b)

Trigonal planar

c)

bent

d)

trigonal pyramidal

49.

In a polar covalent bond, electrons are shared _________________.

a)

between two metals

b)

equally

c)

unequally

d)

between a metal and a non metal

50.

Using your electronegativity handout and the types of atoms involved predict. What type of bond would form between F and Cl?

a)

Non polar Covalent

b)

Polar Covalent

c)

Ionic

d)

Metallic

51.

The bond between O and F is polar covalent. Which direction will the arrow be pointing to show the direction that electrons are moving in this bond?

a)

The arrow will point towards O, which will be partially positive

b)

The arrow will point towards O, which will be partially negative

c)

The arrow will point towards F, which will be partially positive

d)

The arrow will point towards F, which will be partially negative

52.

What type of bond contains cations and anions?

a)

Polar Covalent

b)

Non-Polar Covalent

c)

Ionic

53.

The bond between O and F is polar covalent. Which direction will the arrow be pointing to show the direction that electrons are moving in this bond?

a)

The arrow will point towards O, which will be partially positive

b)

The arrow will point towards O, which will be partially negative

c)

The arrow will point towards F, which will be partially positive

d)

The arrow will point towards F, which will be partially negative

54.

The bond between C and H is non-polar covalent. That means

a)

there is a pair of electrons shared equally between them

b)

there is a pair of electrons shared unequally between them

c)

an electron will be stolen from one and given to the other

55.

The bond between K and N is ionic. Which atom will steal the electrons from the other?

a)

K will steal electrons from N and become (+)

b)

K will steal electrons from N and become (-)

c)

N will steal electrons from K and become (+)

d)

N will steal electrons from K and become (-)

56.
Which molecule would have this molecular geometry?
a)
BF3
b)
CH4
c)
PCl5
d)
CO2
57.
What molecule could this be? 
a)
BF3
b)
CH4
c)
H2O
d)
CO2
58.

Which molecule could have the following structure?

a)
CH4
b)
CO2
c)
PCl5
d)
BF3
59.

Which molecule could have the following geometry?

a)
H2O
b)
NH3
c)
CO2
d)
CH4
60.

How many lone pairs of electrons are on the P atom in PF3?

a)
1
b)
2
c)
3
d)
0
61.
According to VSEPR, molecules adjust their shapes to keep which of the following as far away as possible?
a)
Pairs of valence electrons
b)
Inner shell electrons
c)
Mobile Electrons
d)
Electrons closest to the nucleus
62.
Which of the following molecular shapes would have a bond angle of 180 Degrees?
a)
Bent
b)
Trigonal Planar
c)
Tetrahedral
d)
Linear
63.

How many unshared pairs of electrons will a bent molecule have?

a)

0

b)

2

c)

3

d)

4

64.
In a polar bond, the more electronegative element will assume a partial ________ charge.
a)
positive
b)
negative
65.
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
66.
This is an example of a __________ bond.
a)
non-polar covalent
b)
polar covalent
c)
ionic
d)
metallic
67.

Will this molecule be polar or nonpolar? PH3

a)
polar
b)
nonpolar
68.
What molecular shape is the structure shown here? (NH4+)
a)
linear
b)
trigonal planar
c)
tetrahedral
d)
trigonal pyramidal
69.
What is the shape of H2O?
a)
linear
b)
tetrahedral
c)
bent
d)
trigonal pyramidal
70.
VSEPR stands for ________ theory.
a)
Valence Structure of Electron Pyramids and Regression
b)
Varied Structures of Electrons Paired and Replaced
c)
Varied Shell Energy of Protons and Radiation
d)
Valence Shell Electron Pair Repulsion
71.

What is the AXE formula of a molecule with 3 shared pairs and 1 lone pair?

a)

AX3

b)

AX4

c)

AX2E2

d)

AX3E

72.
What molecular shape is the structure shown here? (BCl3)
a)
linear
b)
trigonal planar
c)
tetrahedral
d)
trigonal pyramidal
73.
HCl
a)

Polar molecule

b)

Nonpolar molecule

74.
N2
a)
Polar 
b)
Nonpolar 
75.
NF3
a)
Polar 
b)
Nonpolar 
76.
Which of the following is a polar molecule?
a)
CH4
b)
Xe
c)
H2O
d)
CO2
77.
Which formula represents a nonpolar molecule?
a)
HBr
b)
H2S
c)

BF3

d)
PCl3
78.

CO2 has polar bonds but is a NON POLAR molecule. Why?

a)

it has an asymmetrical shape

b)

bond polarity or dipole moment between C and O atoms cancel

c)

there is net dipole moment between C and O atoms in molecule

d)

bond polarity does not exist between C+ and O- atoms

79.

For polarity to occur in a bond, you need two elements with a difference in their electronegativities of ___

a)

less than 0.5

b)

between 0.5 and 1.7

c)

less than 1.7

d)

greater than 1.7

80.

A little lowercase delta plus (δ+) or delta minus (δ–) by the individual atoms signify ___

a)

partial charges

b)

the magnetic poles

c)

a difference in electronegativities

d)

nonpolar molecules

81.

What kind of molecule is water

a)

polar, bent, asymmetrical

b)

symmetrical, bent, non-polar

c)

linear, symmetrical, polar

d)

symmetrical, polar and pyramidal

82.

CF4 is

a)

a polar molecule because it has polar bond

b)

non-polar molecule because it has symmetrical shape

c)

non-polar molecule because it has asymmetrical shape

d)

polar molecule because it has non-polar bond

83.

In metallic bonds electrons are:

a)

shared

b)

move around the nuclei randomly

c)

transferred

84.

Malleability and ductility are characteristics of compounds with

a)

covalent bonds

b)

metallic bonds

c)

ionic bonds

d)

alloy bonds

85.

Alloys are important because

a)

their properties are often superior to the component elements

b)

their properties are a blend of the component elements

c)

they never corrode

d)

they are less expensive than their component elements.

86.

Malleability means

a)

the ability to be drawn into a wire

b)

the electrons of metals are mobile

c)

the ability to be hammered into a shape

d)

the ability to be a conductor of electricity

87.

Metals are hard because metals have a

a)

sea of electrons that tightly hold the nuclei together

b)

they form triple bonds

c)

low melting point

d)

high luster

88.

Metals conduct electricity because

a)

the metal ions are free to move

b)

their electrons are free to move

c)

the bonds between metal atoms can easily be broken

d)

they have a positive charge

89.

Which of the following would be held together by the metallic bond?

a)

Atoms of iron (Fe)

b)

Molecules of CH4

c)

Atoms of sulfur (S)

d)

Units of NaCl

90.
Identify Cessium Nitrate
a)
CsNO3
b)
Cs2(NO3)3
c)
Cs2NO3
d)
Cs3NO3
91.
Identify Gallium Sulfate
a)
GaSO4
b)
Ga2(SO4)3
c)
Ga3(SO4)2
d)
Ga2SO4
92.
What is the name of K3PO4?
a)
Tripotassium Phosphate
b)
Tripotassium Phosphite
c)
Potassium phosphide
d)
Potassium phosphate
93.
What is the name of Al(NO3)3?
a)
Aluminum trinitrate
b)
Monoaluminum nitrate
c)
Aluminum (III) nitrate
d)
Aluminum Nitrate
94.
What is the name of AgNO3? (hard mode)
a)
Silver Nitrate
b)
Silver Mononitrate
c)
Silver (I) Nitrate
d)
Monosilver Nitrate
95.
What is the name of Mg(OH)2?
a)
Magnesium Hydride
b)
Magnesium Dihydride
c)
Magnesium Dihydroxide
d)
Magnesium Hydroxide
96.
Ammonium and oxygen would combine to form:
a)
(NH4)2O
b)
NH4O2
c)
(NH4)O2
d)
NH6O3
97.
What is iron's charge in the chemical formula FeCl3?
a)
1+
b)
2+
c)
3+
d)
1-
98.

What is the formula for chromium (II) hydroxide?

a)

CrOH

b)

Cr(OH)1

c)

Cr(OH)3

d)

Cr(OH)2

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