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Ionic Covalent Dot Diagram Quiz Review #JayChem

Total questions: 101

Worksheet time: 17hrs 50mins

Name
Class
Date
1.

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.

2.

How many valence electrons should Lithium have in its Lewis dot model?

a)

1

b)

2

c)

3

d)

4

3.

How many valence electrons should Oxygen have in its Lewis dot model?

a)

5

b)

6

c)

7

d)

8

4.

How many valence electrons should Magnesium have in its Lewis dot model?

a)

1

b)

2

c)

3

d)

4

5.

How many electrons should Boron have around its Lewis dot model?

a)

1

b)

2

c)

3

d)

4

6.
Which of these elements has 8 valence electrons?
a)
P
b)
Be
c)
O
d)
Ar
7.
Which of the following is the correct Lewis dot structure for the molecule fluorine (F2)?
a)
A
b)
B
c)
C
d)
D
8.
Which is the correct structure for ammonia?
(Top picture is A, bottom picture is D.)
a)
Option A
b)
Option B
c)
Option C
d)
Option D
9.
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
10.
What is the correct formula for this molecule?
a)
NH
b)
N3H
c)
NH3
d)
NH4
11.
According to the octet rule most elements need _______ valence electrons.
a)
2
b)
8
c)
6
d)
18
12.

What type of bonding does this picture show?

a)

Ionic

b)

Covalent

13.

What type of bonding does this picture show?

a)

Ionic

b)

Covalent

14.

Generally low melting and boiling points

a)

Ionic compounds

b)

Covalent compounds

15.

Generally high melting & boiling points

a)

Ionic compounds

b)

Covalent compounds

16.

Valence electrons are shared

a)

Ionic bonds

b)

Covalent bonds

17.

Valence electrons are transferred

a)

Ionic bonds

b)

Covalent bonds

18.
Where are the nonmetals located on the periodic table? 
a)
Blue
b)
Red
c)
Green
19.

The chemical bond between a non-metal and another non-metal will be a ________ bond.

a)

metal

b)

ionic

c)

covalent

d)

polar

20.

The chemical bond between a metal and a non-metal will be a _____ bond.

a)

metal

b)

ionic

c)

covalent

d)

polar

21.

Sodium and Bromine will make a _____ bond.

a)

ionic

b)

covalent

c)

metallic

22.

Carbon and Oxygen will make a ___________ bond.

a)

ionic

b)

covalent

c)

metallic

23.

MgO

a)

ionic

b)

covalent

c)

metallic

24.

NaCl

a)

ionic

b)

covalent

c)

metallic

25.

If two fluorine atoms bond they will make a _____ bond.

a)

ionic

b)

covalent

c)

metallic

26.

Which of the following elements LOSES 1 electron in order to have a full outer shell of electrons?

a)

potassium

b)

calcium

c)

helium

d)

boron

e)

fluorine

27.

Which of the following elements LOSES 1 electron in order to have a full outer shell of electrons?

a)

potassium

b)

calcium

c)

helium

d)

boron

e)

fluorine

28.

Which of the following elements GAINS 1 electron in order to have a full outer shell of electrons?

a)

sodium

b)

calcium

c)

helium

d)

boron

e)

chlorine

29.

Which of the following elements LOSES 2 electrons in order to have a full outer shell of electrons?

a)

lithium

b)

magnesium

c)

helium

d)

sulfur

e)

bromine

30.

Generally, atoms form bonds so that _______________.

a)

Each atom loses its electrons

b)

Each atom has an electron configuration similar to a noble gas.

c)

Each atom has an unstable electron configuration

d)

Each atom gains electrons

31.

Mg and Cl create...

a)
Mg2Cl
b)
MgCl2
c)
Mg2Cl2
d)
MgCl
32.

Ca and N create...

a)
Ca2N3
b)
Ca3N2
c)
CaN3
d)
Ca2N
33.

Li and P create...

a)
Li3P
b)
LiP3
c)
LiP
d)
Li2P
34.

Na and Cl create...

a)

Na2Cl

b)

NaCl2

c)

Na2Cl2

d)

NaCl

35.

Mg and O will bond to make...

a)

Mg2O3

b)

MgO2

c)

MgO

d)

Mg2O

36.

If Ca and F bond together to form a stable, binary ionic compound, the formula will be...

a)

Ca2F2

b)

Ca3F

c)

CaF2

d)

Ca2F

37.

Al and P create...

a)

Al3P

b)

AlP3

c)

AlP

d)

Al2P

38.

Ba and Cl will combine to form which compound

a)

Ba2Cl

b)

BaCl2

c)

Ba2Cl2

d)

BaCl

39.

A Li atom and a P atom will create and ionic bond. To be stable they must combine in which of the following combinations?

a)
Li3P
b)
LiP3
c)
LiP
d)
Li2P
40.

Which of the following elements LOSES 2 electrons in order to have a full outer shell of electrons?

a)

lithium

b)

magnesium

c)

helium

d)

sulfur

e)

bromine

41.

Mg and Cl create...

a)
Mg2Cl
b)
MgCl2
c)
Mg2Cl2
d)
MgCl
42.

Ca and N create...

a)
Ca2N3
b)
Ca3N2
c)
CaN3
d)
Ca2N
43.

Li and P create...

a)
Li3P
b)
LiP3
c)
LiP
d)
Li2P
44.

Na and Cl create...

a)

Na2Cl

b)

NaCl2

c)

Na2Cl2

d)

NaCl

45.

Mg and O will bond to make...

a)

Mg2O3

b)

MgO2

c)

MgO

d)

Mg2O

46.

If Ca and F bond together to form a stable, binary ionic compound, the formula will be...

a)

Ca2F2

b)

Ca3F

c)

CaF2

d)

Ca2F

47.

Al and P create...

a)

Al3P

b)

AlP3

c)

AlP

d)

Al2P

48.

Ba and Cl will combine to form which compound

a)

Ba2Cl

b)

BaCl2

c)

Ba2Cl2

d)

BaCl

49.

The name of FeCl₂ is

a)

iron chloride

b)

iron (II) chloride

c)

iron (I) chloride

d)

iron dichloride

50.

LiBr is called

a)

lithium bromine

b)

lithium (I) bromine

c)

lithium bromide

d)

lithuim (I) bromide

51.

Name the ionic compound SnSe2

a)

Tin diselenide

b)

Tin (IV) Selenide

c)

Tin selenide

d)

Tin (II) triselenide

52.

Name the following ionic compound: BeCl2

a)

beryllium chlorine

b)

beryllium II chloride

c)

beryllium chloride

d)

beryllium dichloride

53.

Name the following ionic compound: Cs2S

a)

cesium sulfide

b)

cesium sulfate

c)

cesium II sulfate

d)

cesium II sulfide

54.

When naming ionic compounds with transition metals you need to include roman numerals to show the _____ of the metal..

a)

atomic number

b)

mass number

c)

charge

d)

ionization energy

55.

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

a)

Metal

b)

Nonmetal

c)

Anion

d)

Cation

56.

When naming a compound, what must the last part be?

a)

the element with "ide" at the end

b)

the element with the ending "ite"

c)

the name of the element

d)

the element with "ide" at the end, unless its a polyatomic ion

57.

What is the name of the compound Na2(SO4)?

a)

Sodium sulfate

b)

Sodium sulfide

c)

Sodium sulfite

d)

Sodium sulfuroxide

58.
phosphorus trichloride
a)
KCl3
b)
PCl3
c)
K3Cl
d)
P3Cl
59.
silicon dioxide
a)
SO2
b)
NaO2
c)
SiO2
d)
SiO
60.

dinitrogen pentoxide

a)

N2O5

b)

NO5

c)

N5O2

d)

N2O6

61.
SiCl4
a)
silicon tetrachloride
b)
silicon quadchloride
c)
monosilicon tetrachloride
d)
silicon chloride
62.

P₄S₁₀

a)

tetrapotassium decasulfide

b)

phosphorus decasulfide

c)

tetraphosphorus decasulfide

d)

phosphorus (X) sulfide

63.

SO₃

a)

sulfate

b)

sulfur oxide

c)

sulfur trioxide

d)

monosulfur trioxide

64.

tetraphosphorus heptoxide

a)

K₄O₁₀

b)

P₄O7

c)

KO

d)

P₁₀O₄

65.

chlorine dioxide

a)

ClO2

b)

ClO

c)

ClO3

d)

HClO2

66.
What is the correct name for NO?
a)
Mononitrogen Monoxide
b)
Nitrogen Monoxide
c)
Mononitrogen Dioxide
d)
Nitrogen Oxide
67.
What is the formula for Tricarbon Octahydride?
a)
Ca3O
b)
C2H8
c)
C3H8
d)
Ca3H8
68.
What is Sulfur Trichloride?
a)
SCl3
b)
SiCl3
c)
SCl4
d)
Si3Cl
69.
Phosphorous trichloride
a)
PCl3
b)
P3Cl
c)
P3Cl3
d)
PCL
70.
P2O5
a)
Phosphorus Oxide
b)
Pentaphosphorus Dioxide
c)
Diphosphorous pentoxide
d)
Phosphoric Oxygen
71.
PBr5
a)
Phosphorus Bromide
b)
Phosphorus Pentabromide
c)
Pentaphosphorus bromide
d)
Phosphorus Bromine
72.
As4O10
a)
arsenic oxide
b)
quadarsenic decoxide
c)
tetraarsenic decoxide
d)
arsenic decoxide
73.
The covalent compound N2O5 would be named
a)
nitrogen oxide.
b)
dinitrogen oxide.
c)
nitrogen pentoxide.
d)
dinitrogen pentoxide.
74.
Disulfur trioxide
a)
S3O2
b)
SO
c)
S2O3
d)
S2O
75.
In Cl2, the 2 is known as
a)
the subscript.
b)
the coefficient.
c)
the molecular mass.
d)
the number of protons.
76.
Bonds between two nonmetal atoms are 
a)
covalent.
b)
ionic.
c)
incomplete.
d)
complete.
77.
N2, Cl2, and O2 are all 
a)
diatomic molecules.
b)
ionic bonds.
c)
of equal mass.
d)
solids.
78.
Diatomic molecules are __________ found in nature as their single element: I, O, N, H, Br, Cl, or H.
a)
often
b)
never
c)
sometimes
d)
always
79.
Which of the following is NOT formed by a covalent bond?
a)
K2S
b)
H2O
c)
I2
d)
CO2
80.
 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
81.
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
82.
What is the VSEPR theory used to predict?
a)
Bond Strength
b)
Polarity
c)
Molecular Shape
d)
Electronegativity
83.
Who could this molecule be?
a)
CH4
b)
CO2
c)
PCl5
d)
BF3
84.
Which molecule below would have this shape?
a)
BF3
b)
CH4
c)
PCl5
d)
CO2
85.
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
86.

What would be the bond angle between atoms in this molecule?

a)

180

b)

120

c)

90

d)

109.5

87.

What would be the bond angle between atoms in this molecule?

a)

109.5

b)

120

c)

180

d)

90

88.

What is the name of this molecule's shape?

a)

Bent

b)

Linear

c)

Tetrahedral

d)

Trigonal pyramidal

89.

What is the name of this molecular shape?

a)

trigonal pyramid

b)

tetrahedral

c)

bent

d)

trigonal planar

90.

What would be the bond angle between atoms in this molecule?

a)

90

b)

120

c)

180

d)

109.5

91.

Which Lewis Dot Model drawing correctly shows an O2 molecule?

a)
b)
c)
d)
92.
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
93.
A diatomic molecule like O2 is always_______ because electrons are shared ________.
a)
nonpolar; equally
b)
polar; equally
c)
nonpolar; unequally
d)
nonpolar; unequally
94.

The electrons in a POLAR covalent bond are shared...

a)

Evenly

b)

Unevenly

c)

Electrons are not shared

d)

None of the Above

95.

The electrons in a NONPOLAR covalent bond are shared...

a)

Evenly

b)

Unevenly

c)

Electrons are not shared

d)

None of the Above

96.

What type of bond is depicted in the image?

a)

Nonpolar Covalent

b)

Polar Covalent

c)

Ionic

97.

Electronegativity is...

a)

The ability for an atom to ATTRACT electrons

b)

the ability of an atom to LOSE electrons

c)

the energy required to remove an electron from an atom

d)

how easy it is to make friends.

98.

What is the difference in electronegativity for HBr?

a)

0.7

b)

1.9

c)

2.0

d)

2.8

99.

HBr has a difference in electronegativity of 0.7. Based on the table, what kind of bond is HF?

a)

Nonpolar covalent

b)

Polar covalent

c)

Ionic

100.

H2OH_2O  has a difference in electronegativity of 1.4. Based on the table, what kind of bond is 

H2OH_2O ? 

a)

Nonpolar covalent

b)

Polar covalent

c)

Ionic

101.

NH3NH_3   is a polar covalent compound. Which atom, N or H, will electrons spend MORE time with?

a)

N

b)

H

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