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Unit 4 Review Quizziz

Total questions: 134

Worksheet time: 2hrs 54mins

Name
Class
Date
1.

According to the VSEPR theory, ... want to ... each other.

a)

protons, repel

b)

protons, attract

c)

electrons, repel

d)

electrons, attract

2.
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
3.
What is the VSEPR theory used to predict?
a)
Bond Strength
b)
Polarity
c)
Molecular Shape
d)
Electronegativity
4.

What is the AXE # of this molecule?

a)

AX2

b)

AX2E2

c)

AX2E

d)

AX2E4

5.

What is the AXE # of this molecule?

a)

AX2

b)

AX2E2

c)

AX2E

d)

AX2E4

6.

What is the AXE # of this molecule?

a)

AX

b)

AXE

c)

AX3E

d)

AX3

7.

VSEPR theory is used to predict

a)

the number of unshared pairs of electrons in a Lewis structure.

b)

the number of multiple bonds in a Lewis structure.

c)

the three-dimensional geometry of a molecule.

d)

the three-dimensional crystal lattice structure of ionic compounds.

8.
 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
9.
Which of the following shapes has an unshared pairs of electrons on the central atom? 
a)
Bipyramidal
b)
Bent
c)
Trigonal Planar
d)
Tetrahedral
10.
Which molecule would have this molecular geometry?
a)
BF3
b)
CH4
c)
PCl5
d)
CO2
11.
What molecule could this be? 
a)
BF3
b)
CH4
c)
H2O
d)
CO2
12.
Who could this molecule be?
a)
CH4
b)
CO2
c)
PCl5
d)
BF3
13.
Who could this be? 
a)
CO2
b)
NH3
c)
H2S
d)
CH4
14.
Who could this be?
a)
H2O
b)
NH3
c)
CO2
d)
CH4
15.

What molecular geometry would PH3 have?

a)

Trigonal Pyramidal

b)

Trigonal Bipyramidal

c)

Bent

d)

Linear

16.

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

a)
1
b)
2
c)
3
d)
0
17.
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
18.

How many bonds are in this molecule's structure? (Hint: the green atoms are fluorine.)

a)

6

b)

2

c)

0

d)

4

19.

How many electron domains are in this molecule's structure? (Hint: the green atoms are fluorine.)

a)

6

b)

2

c)

0

d)

4

20.

How many lone pairs are in this molecule's structure? (Hint: the green atoms are fluorine.)

a)

6

b)

2

c)

0

d)

4

21.
What elements generally make a covalent bond?
a)
metal and nonmetal
b)
2 nonmetals
c)
metal
d)
none of the above
22.
In chemical compounds, covalent bonds form when
a)
the electronegativity difference between two atoms is very large.
b)
electrons are completely transferred between two metals.
c)
pairs of electrons are shared between two nonmetal atoms.
d)
two nonmetal atoms are attracted to each other by opposite charges.
23.
Predict the bond that will form between Be and F.
a)
Ionic
b)
Covalent
24.
Predict the bond that will form between Se and Cl
a)
Ionic
b)
Covalent
25.

Which of these is the shape of CCl4?

a)
b)
c)
d)
e)
26.

Which of these is the shape of BF3?

a)
b)
c)
d)
e)
27.

Which of these is the shape of NH3?

a)
b)
c)
d)
e)
28.

Which of these is the shape of CO2?

a)
b)
c)
d)
e)
29.
What is the ELECTRONIC geometry of the following?
a)
Linear
b)
Trigonal planar
c)
Tetrahedral
d)
Trigonal Bipyramidal
30.
What is the MOLECULAR geometry of the molecule?
a)
Linear
b)
Bent
c)
Trigonal Planar
d)
Seesaw
31.
What is the MOLECULAR geometry of the central oxygen?
a)
Linear
b)
Trigonal Planar
c)
Bent
d)
Tetrahedral
32.
What is the name of the CaF2?
a)
Calcium Fluoride
b)
Calcium Difluoride
c)
Monocalcium Difluoride
d)
Calcium (II) Fluoride
33.
What is the name of SO3?
a)
Sulfur Oxide
b)
Sulfur trioxide
c)
Monosulfur trioxide
d)
Sulfur (VI) Oxide
34.
What is the name of TiF3?
a)
Titanium Fluoride
b)
Titanium Trifluoride
c)
Titanium (III) Fluoride
d)
Monotitanium Trifluoride
35.
What is the chemical formula for Phosphorus Pentachloride?
a)
PCl
b)
PCl3
c)
PCl5
d)
P5Cl
36.
What is the chemical formula for Sodium Sulfide?
a)
NaS
b)
Na2S2
c)
Na2S
d)
NaS2
37.
What is the best explanation of VSEPR theory?
a)
It explains the shapes that electrons make around atoms when they repel
b)
It explains how many electrons fit into an element's valent shell
c)
It explains why electrons pair up
d)
It explains why electrons repel each other
38.
Which is true of VSEPR theory?
a)
It explains the origins of the universe
b)
It describes different molecular shapes
c)
It is loosely based on the Norse myth of Woden
d)
It describes which orbital electrons will fill
39.

How many CORE ELECTRONS does Chlorine have?

a)

2

b)

4

c)

8

d)

10

e)

17

40.

How many VALENCE ELECTRONS does Chlorine have?

a)

2

b)

7

c)

8

d)

10

e)

17

41.

Ionic bonds are formed when electrons get

a)

Shared between two atoms

b)

Removed from both atoms

c)

Transferred from one atom to another

d)

Added to both atoms

42.

How many valence electrons does Mg have? (use the PTable)

a)

1

b)

2

c)

3

d)

4

e)

5

43.

How many valence electrons does Po (Polonium) have? (Use your PTable)

a)

2

b)

4

c)

6

d)

8

44.

Ionic bonds typically form between

a)

A metal and a nonmetal

b)

Two nonmetals

c)

Two metals

d)

A metalloid and a metal

45.

Atoms are most stable when their outer shell is complete.

a)

True

b)

False

46.

Why do elements form chemical bonds?

a)

Because they're friendly

b)

To create a new element

c)

To become stable

d)

Because they all need to gain more electrons

47.

What is the correct formula for Sodium Chloride?

a)

SCl

b)

NaCl

c)

SC

d)

NaCl2

48.

Name this ionic compound: Al2O3

a)

Dialuminum oxide

b)

Aluminum oxygen

c)

Oxygen Aluminide

d)

Aluminum oxide

49.

If you were to draw the lewis dot structure for Germanium (Ge), how many dots would you put around it?

a)

2

b)

4

c)

6

d)

8

50.

Cations _______ electrons, becoming _______ charged.

a)

Gain; positively (+)

b)

Gain; negatively (-)

c)

Lose; positively (+)

d)

Lose; negatively (-)

51.

Anions ____ electrons, becoming _____ charged.

a)

Gain; positively (+)

b)

Gain; negatively (-)

c)

Lose; positively (+)

d)

Lose; negatively (-)

52.

Write the chemical formula for K and Br (potassium bromide).

a)

KBr

b)

K2Br

c)

KBr3

d)

KBr2

53.

Write the chemical formula for Na and S (sodium sulfide).

a)

NaS

b)

S2S2

c)

Na2S

d)

NaS2

54.

Metals (like Na) typically _____ electrons in the formation of ionic bonds.

a)

Gain

b)

Lose

c)

Keep the same

55.

Nonmetals (like Cl) typically ____ electrons when they form ionic bonds.

a)

Gain

b)

Lose

c)

Keep the same

56.

Why are there two sodiums (Na), in the formation of this ionic compound?

a)

There always has to be 2 metals

b)

The overall charge needs to add up to 4

c)

The overall charge has to be 0

d)

It needs to have more metal atoms than nonmetal

57.

Using the model for the formation of Scandium Fluoride (an ionic compound), write the chemical formula.

a)

Sc3F

b)

Sc3F3

c)

Sc+3F-1

d)

ScF3

58.

Using the model, write the chemical formula for an ionic compound that has Mg and Cl.

a)

MgCl2

b)

Mg2Cl2

c)

Mg+2Cl-1

d)

Mg2Cl2

59.
What is the basis of a metallic bond?
a)
the attraction of neutral metal atoms.
b)
the attraction between protons and neutrons.
c)
the attraction between positive metal ions and interlocking electrons.
d)
the attraction between positive metal ions and free floating electrons.
60.
There are more metals than non metals in the periodic table.
a)
True
b)
False
61.
At room temperature, most metals are
a)
liquid
b)
solid
c)
gas
d)
an alloy
62.
What does malleable mean?
a)
able to be shaped
b)
will break easily
c)
can be used for wire
d)
is shiny
63.
Which of these is NOT an alloy?
a)
bronze
b)
copper
c)
brass
d)
stainless steel
64.
Electrons that are free to move in metals
a)
delocalized electrons
b)
oxidation number
c)
chemical bond
d)
salts
65.
What is the ability of a substance to be pulled into a thin strand?
a)
Malleability
b)
Ductility 
c)
Conductivity
d)
Solubility
66.
Why do metals have high melting points?
a)
They don't
b)
The negatively charged electrons act as a glue to hold the positively charged ions together.
c)
All the electrons become delocalised
67.
Why do metals conduct
a)
They are shiny
b)
The electrons are held tightly within the lattice
c)
The electrons are delocalised and able to move
d)
The electrons are shared between two metal ions
68.

Why does the melting point of metals increase across period 3, from Sodium (Na) to Aluminium (AI)?

a)

Size of atoms gets smaller

b)

Attraction force between nuclei and free electron increases

c)

Increased space between the valence electrons in the "sea"

d)

Increased number of valence electrons contributed to the "sea"

69.
This is the correct dot diagram for sodium (Na)
a)
true
b)
false
70.
This is a correct dot diagram for oxygen (O)
a)
true
b)
false
71.
This is a correct dot diagram for fluorine (F)
a)
true
b)
false
72.

What are valence electrons?

a)

The innermost electrons

b)

The outermost electrons

73.

What is the octet rule?

a)

Elements can only have 8 electrons in its outermost shell

b)

The elements must form an octopus like structure

74.

How many valence electrons does Carbon have

a)

1

b)

4

75.

How many valence electrons does Argon have

a)

8

b)

11

76.

Electron dot notation is . . . .

a)

A representation of an element in which only valence electrons of an atom are shown

b)

A representation of how compounds are formed.

77.
How many electrons should Helium have around its Lewis dot model?
a)
1
b)
2
c)
7
d)
8
78.

Which of the elements in the picture has correct electron dot notation?

a)

1

b)

2

c)

3

d)

4

79.

How many valence electrons does Hydrogen Have?

a)

1 Valence electron

b)

2 Valence electron

c)

3 Valence electron

d)

4 Valence electron

e)

5 Valence electron

80.

How many valence electrons does Helium Have?

a)

1 Valence electron

b)

2 Valence electron

c)

3 Valence electron

d)

4 Valence electron

e)

5 Valence electron

81.

How many valence electrons does Nitrogen Have?

a)

1 Valence electron

b)

2 Valence electron

c)

3 Valence electron

d)

4 Valence electron

e)

5 Valence electron

82.

How many valence electrons does Magnesium Have?

a)

1 Valence electron

b)

2 Valence electron

c)

3 Valence electron

d)

4 Valence electron

e)

5 Valence electron

83.

How many valence electrons does Aluminum Have?

a)

1 Valence electron

b)

2 Valence electron

c)

3 Valence electron

d)

4 Valence electron

e)

5 Valence electron

84.

How many valence electrons does Potassium Have?

a)

1 Valence electron

b)

2 Valence electron

c)

3 Valence electron

d)

4 Valence electron

e)

5 Valence electron

85.

How many valence electrons does Phosphorus Have?

a)

1 Valence electron

b)

2 Valence electron

c)

3 Valence electron

d)

4 Valence electron

e)

5 Valence electron

86.

How many valence electrons does Silicon Have?

a)

1 Valence electron

b)

2 Valence electron

c)

3 Valence electron

d)

4 Valence electron

e)

5 Valence electron

87.

How many valence electrons does Lithium Have?

a)

1 Valence electron

b)

2 Valence electron

c)

3 Valence electron

d)

4 Valence electron

e)

5 Valence electron

88.

How many valence electrons does Boron Have?

a)

1 Valence electron

b)

2 Valence electron

c)

3 Valence electron

d)

4 Valence electron

e)

5 Valence electron

89.

How many valence electrons does Sodium Have?

a)

1 Valence electron

b)

2 Valence electron

c)

3 Valence electron

d)

4 Valence electron

e)

5 Valence electron

90.

How many valence electrons does Calcium Have?

a)

1 Valence electron

b)

2 Valence electron

c)

3 Valence electron

d)

4 Valence electron

e)

5 Valence electron

91.

How many valence electrons does Carbon Have?

a)

1 Valence electron

b)

2 Valence electron

c)

3 Valence electron

d)

4 Valence electron

e)

5 Valence electron

92.

How many valence electrons does Beryllium Have?

a)

1 Valence electron

b)

2 Valence electron

c)

3 Valence electron

d)

4 Valence electron

e)

5 Valence electron

93.

How many valence electrons does Oxygen Have?

a)

4 Valence electron

b)

5 Valence electron

c)

6 Valence electron

d)

7 Valence electron

e)

8 Valence electron

94.

How many valence electrons does Neon Have?

a)

4 Valence electron

b)

5 Valence electron

c)

6 Valence electron

d)

7 Valence electron

e)

8 Valence electron

95.

How many valence electrons does Chlorine Have?

a)

4 Valence electron

b)

5 Valence electron

c)

6 Valence electron

d)

7 Valence electron

e)

8 Valence electron

96.

How many valence electrons does Fluorine Have?

a)

4 Valence electron

b)

5 Valence electron

c)

6 Valence electron

d)

7 Valence electron

e)

8 Valence electron

97.

How many valence electrons does Sulfur Have?

a)

4 Valence electron

b)

5 Valence electron

c)

6 Valence electron

d)

7 Valence electron

e)

8 Valence electron

98.

How many valence electrons does Argon Have?

a)

4 Valence electron

b)

5 Valence electron

c)

6 Valence electron

d)

7 Valence electron

e)

8 Valence electron

99.

What is the correct Lewis Dot Structure for ammonia NH3

a)
b)
c)
d)
100.

Which is the correct molecular structure for carbon dioxide?

a)
b)
c)
d)
101.
According to the octet rule most elements need _______ valence electrons.
a)
2
b)
8
c)
6
d)
18
102.
Hydrogen needs _____ electrons in its valence shell to be stable.
a)
4
b)
6
c)
8
d)
2
103.
Which of the following is the correct Lewis dot structure for the molecule fluorine (F2)?
a)
A
b)
B
c)
C
d)
D
104.
Which of the following is the correct LD Diagram for Hydrogen Cyanide? HCN?
a)
A
b)
B
c)
C
d)
D
105.

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

a)

8

b)

4

c)

2

d)

3

106.

CO2 has how many lone pairs?

a)

0

b)

1

c)

2

d)

3

e)

4

107.

NH3 has how many lone pairs?

a)

0

b)

1

c)

2

d)

3

108.

How many valence electrons does Hydrogen Have?

a)

1 Valence electron

b)

2 Valence electron

c)

3 Valence electron

d)

4 Valence electron

e)

5 Valence electron

109.

How many valence electrons does Helium Have?

a)

1 Valence electron

b)

2 Valence electron

c)

3 Valence electron

d)

4 Valence electron

e)

5 Valence electron

110.

How many valence electrons does Nitrogen Have?

a)

1 Valence electron

b)

2 Valence electron

c)

3 Valence electron

d)

4 Valence electron

e)

5 Valence electron

111.

How many valence electrons does Magnesium Have?

a)

1 Valence electron

b)

2 Valence electron

c)

3 Valence electron

d)

4 Valence electron

e)

5 Valence electron

112.

How many valence electrons does Aluminum Have?

a)

1 Valence electron

b)

2 Valence electron

c)

3 Valence electron

d)

4 Valence electron

e)

5 Valence electron

113.

How many valence electrons does Potassium Have?

a)

1 Valence electron

b)

2 Valence electron

c)

3 Valence electron

d)

4 Valence electron

e)

5 Valence electron

114.

How many valence electrons does Phosphorus Have?

a)

1 Valence electron

b)

2 Valence electron

c)

3 Valence electron

d)

4 Valence electron

e)

5 Valence electron

115.
How many electrons should Helium have around its Lewis dot model?
a)
1
b)
2
c)
7
d)
8
116.
How many electrons should Calcium have around its Lewis dot model?
a)
1
b)
2
c)
7
d)
8
117.
an element will always have the same number of 
a)
neutrons
b)
protons
c)
isotopes
d)
atoms
118.
An element with five valence electrons is
a)
phosphorus
b)
oxygen
c)
beryllium
d)
rubidium
119.
Rows on the period table are called _____ while columns are called _____.
a)
groups, families
b)
groups, periods
c)
periods, groups
d)
families, groups
120.
What's a valence electron?
a)
electrons in the second energy level
b)
electrons in the outermost energy level
c)
the atomic number
d)
electrons in the first level
121.

CCl4 has how many double bonds?

a)

0

b)

1

c)

2

d)

3

122.

Carbonate (CO32-) has how many double bonds?

a)

0

b)

1

c)

2

d)

3

123.

In HCN (Carbon is usually the central atom) what kind of bond is between the C and N

a)

Single

b)

Double

c)

Triple

124.
What is the correct structure for BF3?
a)
Option A.
b)
Option B. 
c)
Option C.
d)
Option D.
125.

What are resonance structures?

a)

Structural the same structures that have different bond arrangements

b)

Structures that are similar, but not the same VSEPR shape

c)

Structures that have been drawn three times

126.

How many bonds can hydrogen make?

a)

Only 1

b)

1 or 2 Bonds

c)

1 bond with 6 electrons on it

d)

It never makes bonds

127.
In the correct Lewis structure for water, how many unshared pairs of electrons will oxygen have?
a)
1
b)
4
c)
3
d)
2
128.
After drawing in your bonds, what do you do if you don't have enough electrons to get each atom to its octet?
a)
Place dots until everything has eight
b)
Place dots only around the terminal atoms
c)
Add a multiple bond
d)
Have eight only around the central atom
129.
In a Lewis structure, what do you do  with the total number of valence if your ion is 2- charged?
a)
Add 2 to the valence number
b)
Subtract 2 from the valence number
c)
Multiply the valence number by 2
d)
Divide the valence number by 2
130.
How many electrons does each line indicate are shared?
a)
1
b)
2
c)
3
d)
4
131.

Which Lewis Dot Model drawing correctly shows an O2 molecule?

a)
b)
c)
d)
132.

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.

133.

Which type of bond is being formed in this diagram?

a)

covalent bond

b)

energy bond

c)

ionic bond

134.

Match the following

a)

Can form 4 Bonds

1.

Carbon

b)

Can form 3 bonds

2.

Nitrogen

c)

can form 2 bonds

3.

Oxygen

d)

Can form 1 bond

4.

hydrogen

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