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bonds

Total questions: 175

Worksheet time: 4hrs 58mins

Name
Class
Date
1.

Element Astros (symbol Ao) is found in group 6 and element Braves (symbol Bv) is found in group 16. What is the name of the compound Ao2Bv3?

a)

Astros bravide

b)

Astros (I) bravide

c)

Astros (II) bravide

d)

Astros (III) bravide

e)

Can not be determined from the information provided.

2.
barium phosphide
a)
Ba3(PO4)2
b)
BaP
c)
Ba3P2
d)
Ba2P3
3.
Lithium fluoride
a)
LiF
b)
LiF2
c)
Li2F
d)
Li2F3
4.

What is the correct name for this formula: BeI2?

a)

beryllium (II) iodide

b)

beryllium diiodide

c)

beryllium iodine

d)

beryllium iodide

5.

Element Astros (symbol Ao) is found in group 1 and element Braves (symbol Bv) is found in group 16. What is the name of the compound Ao2Bv3?

a)

Astros bravide

b)

Astros (I) bravide

c)

Astros (II) bravide

d)

Astros (III) bravide

e)

Can not be determined from the information provided.

6.

Using IUPAC rules, state the name of the following compound:
FeCl3

a)
Chloride Iron
b)

Iron (III) Chloride

c)

Chloride (III) Iron

d)

Iron (I) Chloride

7.

What is the chemical name for the compound FeCl₂?

a)

iron chloride

b)

iron (II) chloride

c)

iron (I) chloride

d)

iron dichloride

8.

Name the following compound: FeO

a)

iron oxide

b)

iron (II) oxide

c)

iron (III) oxide

d)

ugly

9.

What is the correct name for this formula: BeI2?

a)

beryllium (II) iodide

b)

beryllium diiodide

c)

beryllium iodine

d)

beryllium iodide

10.
Name the following ionic compound: Cr(NO2)3
a)
chromium nitrite
b)
chromium nitride
c)
chromium III nitride
d)
chromium III nitrite
11.
Name the following ionic compound: BeCl2
a)
beryllium chlorine
b)
beryllium II chloride
c)
beryllium chloride
d)
beryllium dichloride
12.
Name the following compound: FeCl3
a)
iron chloride
b)
iron III chloride
c)
iron chlorate
d)
iron III chlorate
13.
Name the following ionic compound: MgSO4
a)
magnesium sulfoxide
b)
magnesium sulfide
c)
magnesium sulfate
d)
magnesium oxide
14.

Name the following ionic compound: BeCl2

a)

beryllium chlorine

b)

beryllium II chloride

c)

beryllium chloride

d)

beryllium dichloride

15.
The name for CrN:
a)
Chromium nitride
b)
Chromium (I) nitride
c)
Chromium (III) nitride
d)
Chromium nitride (III)
16.

Name the ionic compound SnSe2

a)

Tin diselenide

b)

Tin (IV) Selenide

c)

Tin selenide

d)

Tin (II) triselenide

17.
What is the NAME of....
Na2S
a)
sodium (II) sulfide
b)
sodium sulfide
c)
disodium sulfide
d)
sodium sulfur
18.

When naming a compound, which of these is written first?

a)

Metal

b)

Nonmetal

c)

Anion

d)

Cation

19.

What is the name of the compound Sc(OH)3?

a)

Scandium (III) hydroxide

b)

Scandium (I) hydroxide

c)

Scandium (II) hydroxide

d)

Scandium hydroxide

20.

Name the following ionic compound: Cs2S

a)

cesium sulfide

b)

cesium sulfate

c)

cesium II sulfate

d)

cesium II sulfide

21.

The name of FeCl₂ is

a)

iron chloride

b)

iron (II) chloride

c)

iron (I) chloride

d)

iron dichloride

22.

What is the name for MgF2 ?

a)

magnesium fluoride

b)

manganese Phosphide

c)

magnesium(III) fluoride

d)

magnesium fluoride(II)

23.
Lithium fluoride
a)
LiF
b)
LiF2
c)
Li2F
d)
Li2F3
24.

A tightly-bound group of atoms that is covalently bonded, yet carries a net charge:

a)

monatomic ion

b)

polyatomic ion

25.

A tightly-bound group of atoms that is covalently bonded, yet carries a net charge:

a)

monatomic ion

b)

polyatomic ion

26.

A single atom with a positive or negative charge.

a)

monatomic ion

b)

polyatomic ion

c)

diatomic ion

27.

Produces a hydrogen ion when dissolved in water:

a)

acid

b)

base

28.

Produces a hydroxide ion when dissolved in water:

a)

acid

b)

base

29.

When naming a transition metal ion that can have more than one common ionic charge, the numerical value of the charge is indicated by a __________.

a)

prefix

b)

suffix

c)

superscript after the name

d)

Roman numeral following the name

30.

The nonmetals in Groups 6A and 7A ______.

a)

lose electrons when they form ions

b)

have a numerical charge that is found by subtracting 8 form the group number

c)

all have ions with a -1 charge

d)

end in -ate

31.

Which of the following is NOT a cation?

a)

iron (III) ion

b)

sulfate

c)

Ca2+

d)

sodium ion

32.

Which of the following is true about the composition of ionic compounds?

a)

They are composed of anions and cations.

b)

They are composed of anions only.

c)

They are composed of cations only.

d)

They are formed from two or more nonmetallic elements.

33.

An -ate or -ite at the end of a compound name usually indicates that the compound contains _____________.

a)

fewer electrons than protons

b)

neutral molecules

c)

only two elements

d)

a polyatomic anion

34.

Which element, when combined with fluorine, would most likely form an ionic compound?

a)

lithium

b)

carbon

c)

phosphorus

d)

chlorine

35.

What is the correct formula for potassium sulfite?

a)

KHSO3

b)

KHSO4

c)

K2SO3

d)

K2SO4

36.

Which of the following compounds contains the lead(II) ion?

a)

PbO

b)

PbCl4

c)

Pb2O

d)

Pb2S

37.

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

38.

When naming acids, the prefix hydro- is used when the name of the acid anion ends in _______.

a)

-ide

b)

-ate

c)

-ite

d)

-ic

39.

What is the name of H2SO3?

a)

hyposulfuric acid

b)

hydrosulfuric acid

c)

sulfuric acid

d)

sulfurous acid

40.

What is the correct name for the compound CoCl2?

a)

cobalt(I) chlorate

b)

cobalt(I) chloride

c)

cobalt(II) chlorate

d)

cobalt(II) chloride

41.

What is the correct formula for barium chlorate?

a)

Ba(ClO)2

b)

Ba(ClO2)2

c)

Ba(ClO3)2

d)

BaCl2

42.

Consider a mystery compound having the formula MxTy. If the compound is not an acid, if it contains only two elements, and if M is not a metal, which of the following is true about the compound?

a)

It contains a polyatomic ion.

b)

Its name ends in -ite or -ate.

c)

Its name ends in -ic.

d)

It is a binary molecular compound.

43.
If an atom becomes an ion with a 2+ charge, what does that mean?
a)
It has lost 2 electrons
b)
It has gained 2 electrons
c)
The atom is in period 2
d)
The atom has an atomic # of 2
44.
How do the following two elements bond together?
Cr3+  O2-         
a)
CrO
b)
Cr3O2
c)
Cr2O3
d)
CrO3
45.
How do the following two elements bond together?
K1+  S2- 
a)
KS
b)
K8S
c)
K6S3
d)
K2S
46.
What is the formula for magnesium chloride?
a)
MgCl
b)
Mg2Cl
c)
MgCl2
d)
Mg(ClO3)2
47.
What is the formula for copper(I) sulfate?
a)
Cu(SO3)
b)
Cu(SO4)
c)
Cu2(SO3)
d)
Cu2(SO4)
48.
Which of these combinations is an ionic compound made of?
a)
Metal and Metal
b)
Nonmetal and Nonmetal
c)
Metal and Nonmetal
d)
Cation and Cation
49.

Hydrogen nitrite (nitrous acid)

a)
H2NO3
b)
HNO3
c)
HNO2
d)
H2NO2
50.
What is the element/ion symbol for Iron(III)?
a)
Fe
b)
Fe3+
c)
Fe3-
d)
Fe(III)
51.
What is the name of the compound Li(OH)?
a)
lithium hydrogen oxide
b)
lithium hydroxide
c)
lithium hydride
d)
lithium oxide hydride
52.
The chemical formula for an ionic compound of potassium and oxygen is
a)
KO.
b)
K2O.
c)
K2O2.
d)
KO2.
53.
Name this compound: 
Ca(CO3)
a)
Calcium carbon oxide
b)
Calcium (II) carbonate
c)
Calcium carbonate
d)
Carbonate (I) calcide
54.
What is the formula for sodium nitrate?
a)
Na3(NO)
b)
Na(NO)
c)
Na3(NO3)
d)
Na(NO3)
55.
What is the compound made between Chlorate and Magnesium
a)
Cl2Mg
b)
(ClO3)2Mg
c)
MgCl2
d)
Mg(ClO3)2
56.
How do the following two elements bond together?
Pb4+  O2-       
a)
PbO
b)
Pb4O2
c)
PbO2
d)
Pb2O4
57.
The name of FeCl₂ is
a)
iron chloride
b)
iron (II) chloride
c)
iron (I) chloride
d)
iron dichloride
58.
The name of Cu₃N₂ is
a)
copper (III) nitride
b)
copper (II) nitride
c)
copper nitride
d)
tricopper dinitride
59.
Whats the formula
Sr+2  +  (CO3)-2
a)
Sr(CO3)
b)
Sr2 (CO3)2
c)
Sr1(CO)5
d)
Sr(CO5)
60.
What is the formula for Copper II Sulfide?
a)
CuS
b)
Cu₂S
c)
CuS₂
d)
CuSO₃
61.
Which of the following compounds is an example of hydrocarbon?
a)
CO2
b)
C2H6
c)
C2H5OH
d)
CH3COOH
62.
Which formula represents a saturated hydrocarbon?
a)
A
b)
B
c)
C
d)
D
63.
Name this compound
a)
2,2-dimethyl-4-ethylhexane
b)
4-ethyl-2,2-dimethylhexane
c)
3-ethyl-5,5-dimethylhexane
d)
4-ethyl-2-methylhexane
64.

Name the compound.

a)

nonene

b)

2,2-dimethylhept-3-ene

c)

1,1,5-trimethylhex-2-ene

d)

2,6-dimethylhept-3-ene

65.

Name this organic molecule.

4 lines
66.

Name this organic molecule.

4 lines
67.

Which compound belongs to the alkene family?

a)

C2H2

b)

C2H4

c)

C6H6

d)

C6H14

68.

Name this organic molecule.

4 lines
69.

Name this organic molecule.

4 lines
70.

Name this organic molecule.

4 lines
71.

A molecule of 2,3 dimethyl hexane would have how many TOTAL carbons?

a)

6

b)

7

c)

8

d)

9

72.
Name the organic family for this structure:
a)
alkanes
b)
alkenes
c)
alkynes
d)
aromatics
73.
What is the organic family for propane?  
a)
alkanes
b)
alkenes
c)
alkynes
d)
aromatics
74.
Name the organic family for this structure:
a)
alkanes
b)
alkenes
c)
alkynes
d)
aromatics
75.
What is the organic family for propene (propylene)?  
a)
alkanes
b)
alkenes
c)
alkynes
d)
aromatics
76.
Explain, in terms of carbon-carbon bonds, why this hydrocarbon is saturated.
a)
The molecule has the maximum amount of hydrogen it can have.
b)
It is an alkane so it is saturated.
c)
There are only single bonds between the hydrogen and carbon.
d)
There are only single bonds between the carbon.
77.
Which formula represents an unsaturated hydrocarbon?
a)
A
b)
B
c)
C
d)
D
78.
Which formula represents a saturated hydrocarbon?
a)
A
b)
B
c)
C
d)
D
79.
Hydrocarbons are compounds that contain
a)
Carbon, only
b)
Carbon and Hydrogen, only
c)
Carbon, Oxygen, and Hydrogen, only
d)
Carbon, Oxygen, Hydrogen, and Nitrogen, only
80.
If an alkane has 32 hydrogen atoms, how many carbon atoms does it have?
a)
64
b)
66
c)
15
d)
16
81.
If an alkane has 20 carbon atoms, how many hydrogen atoms will it have?
a)
20
b)
22
c)
40
d)
42
82.
How many hydrogen atoms are in propane
a)
4
b)
6
c)
8
d)
10
83.
How many hydrogen atoms are in ethane
a)
4
b)
6
c)
8
d)
10
84.
what kind of molecule is this?
a)
alkane
b)
alkene
c)
alkyne
d)
cycloalkane
85.
Organic compounds are compounds contain ______________.
a)
O
b)
C
c)
N
d)
S
86.
Which is an unsaturated hydrocarbon?
a)
C2H6
b)
C3H8
c)
C4H8
87.
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.
88.
Hydrogen bonding occurs when hydrogen is bonded to N, O, or F.  Which of the following has hydrogen bonding?
a)
CBr4
b)
NO2
c)
H2S
d)
NH3
89.
Does H2O have hydrogen bonding?
a)
yes
b)
no
90.
Does CH4 have hydrogen bonding?
a)
yes
b)
no
91.
Which is the second strongest intermolecular force, after hydrogen bonding?
a)
dipole-dipole attraction
b)
London forces
92.

Which substance would have the weakest intermolecular forces of attraction?

a)

CH4

b)

H2O

93.

________________________ have the strongest intermolecular forces of attraction.

a)

Dipole- Dipole

b)

Dispersion

c)

Hydrogen Bonds

94.

Intermolecular forces for: CO2

a)

Dispersion Force

b)

Dipole dipole

c)

Hydrogen bonding

95.
Intermolecular force present in HCl?
a)
dipole dipole
b)
dispersion
c)
H-bond
d)
ionic
96.
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
97.

Intermolecular forces for: NH3

a)

Dispersion Force

b)

Dipole dipole

c)

Hydrogen bonding

98.

Rank these in order of strength:
London dispersion forces
hydrogen bond
dipole-dipole attraction

a)

dipole-dipole>hydrogen bond>London

b)

London>dipole-diple>hydrogen bond

c)

hydrogen bond>dipole-dipole>London

99.
What type of forces will the following molecule have?
a)
dispersion forces
b)
dipoles
c)
hydrogen bonding
100.
What forces will the following molecule have?
a)
dispersion
b)
dipole
c)
hydrogen bonding
101.

Forces that holds atoms together within the molecule

a)

intermolecular forces

b)

intramolecular forces

102.
Which noble gas has the highest boiling point?
a)
Xe
b)
Kr
c)
Ar
d)
He
103.
Type of intermolecular force present in I2, Br2, and Cl2.
a)
dipole dipole
b)
H-bond
c)
dispersion
d)
metallic
104.
Which of the following has the highest boiling point?
a)
H2
b)
NH3
c)
N2
d)
O2
105.
Which of the following has the lowest boiling point?
a)
CaCl2
b)
PH3
c)
Cl2
d)
N2
106.
Intermolecular force present in HCl?
a)
dipole dipole
b)
dispersion
c)
H-bond
d)
ionic
107.
Intermolecular force present in Cl2?
a)
dipole dipole
b)
H-bond
c)
dispersion
d)
metallic
108.

Which substance has the weakest intermolecular forces?

a)

Substance A, boiling point of 75 °C

b)

Substance B, boiling point of 105 °C

c)

Substance C, boiling point of 25 °C

d)

Substance d, boiling point of 45 °C

109.

The weaker the intermolecular forces of a substance the _____________ the boiling point

a)

higher

b)

lower

110.

Which substance will have the highest vapor pressure

a)

CH3CH2CH2CH2CH2CH3

b)

H2O

c)

CH4

d)

CH3F

111.

What is vapor pressure

a)

the amount of energy required to evaporate

b)

the amount of energy required to boil

c)

the force per unit area exerted by the gaseous layer above a liquid

d)

the force per unit area exerted by a liquid on the gaseous layer above it

112.

What is the main intermolecular force in methanol?

a)

hydrogen bonding

b)

dipole-dipole forces

c)

london dispersion forces

d)

none

113.

What are hydrogen bonds?

a)

Any time hydrogen is bonded to another atom

b)

Any time hydrogen is bonded to N, O, or F

c)

An interaction between molecules with H-N, H-O, or H-F bonds in them

d)

Any attraction to hydrogen atoms

114.

What is the relationship between vapor pressure and intermolecular forces?

a)

Vapor pressure does not depend upon intermolecular forces, only the strength of chemical bonds.

b)

Stronger intermolecular forces cause particles to repel each other, raising the vapor pressure.

c)

Stronger IMFs cause particles to stick together, lowering the vapor pressure.

d)

Intermolecular forces cause all liquids to have the same vapor pressure.

115.

Select the correct order of molecules from lowest to highest boiling point, based on intermolecular forces.

a)

CH4 < C2H6 < H2O < SO2

b)

H2O < SO2 < C2H6 < CH4

c)

C2H6 < CH4 < H2O < SO2

d)

CH4 < C2H6 < SO2 < H2O

116.

Which model represents a LOWER Vapor Pressure?

a)

A

b)

B

117.

Which statement explains why Br2 is a liquid at STP and I2 is a solid at STP?

a)

Molecules of Br2 are polar, and molecules of I2 are nonpolar.

b)

Molecules of I2 are polar, and molecules of Br2 are nonpolar.

c)

Molecules of Br2 have stronger intermolecular forces than molecules of I2.

d)

Molecules of I2 have stronger intermolecular forces than molecules of Br2.

118.

Which type of intermolecular force is the weakest?

a)

hydrogen bonding

b)

Van der Waal's / London Dispersion

c)

dipole-dipole

d)

covalent bonding

119.

If a substance has a high vapor pressure, this indicates that the substance has ____________ IMFs.

a)

Weak

b)

Moderate

c)

Strong

120.

If a substance has a high boiling point, this indicates that the substance has ____________ IMFs.

a)

Weak

b)

Moderate

c)

Strong

121.

A substance has a low melting and boiling point, a high vapor pressure, and is a nonpolar molecule that contains polar covalent bonds. What is the identity of the substance?

a)

H2

b)

H2O

c)

CCl4

d)

HCl

122.

Which of the following does NOT experience hydrogen bonding?

a)

HF

b)

HI

c)

NH3

d)

H2O

123.

Is this molecule polar or non-polar?

a)

Polar

b)

Non-polar

124.

Is this molecule polar or non-polar?

a)

Polar

b)

Non-polar

125.

Is this molecule polar or non-polar?

a)

Non-polar

b)

Polar

126.

Is this molecule polar or non-polar?

a)

Non-polar

b)

Polar

127.
In covalent bonds, electrons are ___________.
a)
transferred
b)
gained
c)
lost
d)
shared
128.
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
129.
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
130.
This is an example of a __________ bond.
a)
non-polar covalent
b)
polar covalent
c)
ionic
d)
metallic
131.
What geometry will this molecular structure have?: PH3
a)
bent
b)
tetrahedral
c)
linear
d)
trigonal pyramidal
132.
What geometry will this molecular structure have?: H2S
a)
bent
b)
tetrahedral
c)
linear
d)
trigonal pyramidal
133.
What geometry will this molecular structure have?: CCl4
a)
bent
b)
tetrahedral
c)
linear
d)
trigonal pyramidal
134.
Will this molecule be polar or nonpolar? H2S
a)
polar
b)
nonpolar
135.
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
136.

What is the molecular geometry for this molecule?

a)

Bent

b)

Trigonal pyramidal

c)

Trigonal planar

d)

Linear

137.
Choose the correct shape for this molecule:
a)
Bent
b)
Linear
c)
Tetrahedral
d)
Trigonal pyramidal
138.

What is the molecular geometry of this molecule?

a)

trigonal bipyramidal

b)

square planar

c)

trigonal pyramidal

d)

square pyramidal

139.

If a molecule has an electronegativity difference of 0.6, and has no lone pairs around the central atom, is the molecule polar, nonpolar, or ionic?

a)

Polar

b)

Nonpolar

c)

Ionic

d)

None of the above

140.

Which of the following is an example of square pyramidal molecular geometry?

a)
b)
c)
d)
141.

What are the bond angles between each H in CH4?

a)

109.5

b)

120

c)

180

d)

360

142.

What are the bond angles between each H in BeH2?

a)

90

b)

120

c)

109.5

d)

180

143.

Why isn't H2O's molecular geometry linear?

a)

It has two atoms around the central atom, which distorts the shape.

b)

It has three atoms around the central atom, which distorts the shape

c)

It has two lone pairs around the central atom, which distort the shape.

d)

It is linear.

144.

Why do lone pairs affect molecular geometry?

a)

They don't affect molecular geometry.

b)

Lone pairs pull the atoms bonded to the central atom towards them

c)

Lone pairs repel other electron domains, such as bonds, away from themselves

d)

Lone pairs are made of protons, which repel the protons in the atoms around the central atom

145.

What is electronegativity?

a)

An electron's charge

b)

The same as atomic bonding

c)

Whether they can easily repel electrons

d)

How easily elements can attract electrons to themselves

146.

What does VSEPR mean?

a)

Valence electron pairs attract one another

b)

Protons repulse one another

c)

Valence electron pairs repulse each other

d)

Atoms are repulsed from the central atom

147.
What is the percent by mass of oxygen in MgO?
a)
20%
b)
40%
c)
50%
d)
60%
148.
What is the percent by mass of sodium in NaCl?
a)
39%
b)
61%
c)
35%
d)
65%
149.
What is the percent by mass of fluorine in CaF2 (gram-formula mass = 78 g/mol)?
a)
24%
b)
49%
c)
51%
d)
65%
150.
What is the percent composition by mass of oxygen in the compound MgSO4 (gram formula mass = 120 g/mol)?
a)
20%
b)
27%
c)
46%
d)
53%
151.
Which pair has the same empirical formula?
a)
NaCrO4 and Na2Cr2O7
b)
C2H4O2 and C6H12O6
c)
C3H6O3 and C2H6O2
d)
CH4 and C2H6
152.
A compound consists of 72.2% magnesium(Mg) and 27.8% nitrogen(N) by mass. What is the empirical formula?
a)
Mg4N3
b)
MgN2
c)
Mg3N2 
d)
MgN
153.
You are given the following percentages: 40.05% S and 59.95% O. Find the empirical formula for these elements.
a)
SO
b)
SO2
c)
SO3
d)
SO4
154.
A formula with the lowest whole # ratio of elements in a compound is called
a)
Molecular Formula
b)
Chemical Formula
c)
Empirical Formula 
d)
Distance Formula
155.
What is the molecular formula if the empirical formula is CH2O and the molecular molar mass is 180.18?
a)
CH2O
b)
C2H4O2
c)
C4H8O4
d)
C6H12O6
156.
Given the following: 42.07% Na, 18.89% P, and 39.04% O, determine the empirical formula.
a)
 NaPO2
b)
Na2PO3
c)
Na3PO4
d)
NaPO4
157.
What is the molecular formula for a compound with the empirical formula: K2SO4 and a molecular mass of 696g.
a)
K2SO4 
b)
K8SO16
c)
K8S4O8 
d)
K8S4O16 
158.
A chemical formula that shows the actual # and kinds of atoms present in one molecule of a compound is called_________
a)
ionic formula
b)
covalent formula
c)
empirical formula
d)
molecular formula
159.
Which pair has the same empirical formula?
a)
NaCrO4 and Na2Cr2O7
b)
C2H4O2 and C6H12O6
c)
C3H6O3 and C2H6O2
d)
CH4 and C2H6
160.
An empirical formula:
a)
is a formula that calculates the coefficients of a compound in a balanced equation.
b)
is the simplest whole-number ratio of moles of elements in the compound.
161.

What is the correct Lewis Dot Structure for ammonia NH3

a)
b)
c)
d)
162.

Which is the correct molecular structure for carbon dioxide?

a)
b)
c)
d)
163.
Which of the following is an acceptable Lewis structure for CH3Cl?
a)
Option A
b)
Option B
c)
Option C
d)
Option D
164.
Which of the following is the correct Lewis structure for water?
a)
A
b)
B
c)
C
165.
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
166.
What is the correct formula for this molecule?
a)
Si4F
b)
SiF4
c)
SiF
d)
Si4F4
167.

NH3 has how many lone pairs?

a)

0

b)

1

c)

2

d)

3

168.

CCl4 has how many double bonds?

a)

0

b)

1

c)

2

d)

3

169.

3. Which is a correct Lewis structure for hydrogen cyanide, HCN?

a)
b)
c)
d)
170.

Why is this Lewis Structure incorrect? Choose all that apply.

a)

There are too many bonds around Si.

b)

There should only be single bonds in this Lewis Structure.

c)

The Structure is missing a triple bond.

d)

Chlorine only has 6 electrons surrounding it.

171.

CO2 has how many lone pairs?

a)

0

b)

1

c)

2

d)

3

e)

4

172.

Carbonate (CO32-) has how many double bonds?

a)

0

b)

1

c)

2

d)

3

173.
This is a correct dot diagram for fluorine (F)
a)
true
b)
false
174.
According to the octet rule most elements need _______ valence electrons.
a)
2
b)
8
c)
6
d)
18
175.
 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