wayground logo

Free Printable Worksheets

Font size

S
M
L
XL
Worksheets

Chemistry Review

Total questions: 181

Worksheet time: 2hrs 14mins

Name
Class
Date
1.

Synthesis

a)

AB → A + B

b)

A + B → AB

c)

CxHy + O2 → CO2 + H2O

d)

AB + CD →AD + BC

2.

Decomposition

a)

A + BC → B + AC

b)

A + B → AB

c)

AB + CD →AD + BC

d)

AB → A + B

3.

Combustion

a)

A + B →AB

b)

AB → A + B

c)

CxHy + O2 → CO2 + H2O

d)

A + BC →B + AC

4.

Single Replacement

a)

A + BC →B + AC

b)

AB →A + B

c)

AB + CD → AD + BC

d)

CxHy + O2 → CO2 + H2O

5.

Double Displacement

a)

CxHy + O2 → CO2 + H2O

b)

AB + CD → AD + BC

c)

A + B →AB

d)

A + BC → B + AC

6.

( Single Displacement)

Sodium + Silver Phosphate →

a)

3Na + AuPO4 → 3Au + Na3PO4

b)

2Na + AgPO4 → 4Ag + NaPO4

c)

3Na + AgPO4 →3Ag + Na3PO4

d)

3Na + AgPO3 →3Ag + Na3PO3

7.

(Double Displacement)

Sodium Chloride + Calcium Sulfate →

a)

NaCI2 + SO4Ca2 →SO4Na + Ca2Cl

b)

2NaCl + CaSO4 → Na2SO4 + CaCl2

c)

3NaCl + CaSO3 → Na3SO3 + 3ClCa2

d)

2NaCl + Ca3SO4 →NaCl3 + 3CaCl2

8.

(Combustion)

limited CH4 + excess O2 → CO2 + H2O

Select two

a)

Incomplete

b)

Complete

c)

CH4 +2O4 → CO2 + 2H2O

d)

The reaction does not occur

9.

(Combustion)

Excess CH4 + limited O2 →CO + H2O

Select two

a)

Incomplete

b)

Complete

c)

2CH4 + 3O2 → 2CO + 4H2O

d)

The reaction does not occur

10.

Balance The Equation

P4O10 + H2O → H3PO4

(Feel free to use an equal sign instead of an arrow if needed, and subscripts can be beside an element)

(a)  

11.

This diagram represents a...

a)

pure substance that is a compound

b)

mixture of elements

c)

mixture of compounds

d)

pure substance that is an element

12.

Alex goes into the garden and digs up a shovel full of dirt. This is a _____________ mixture.

a)

Heterogenous

b)

Homogeneous

13.

Milk is a . . .

a)

Heterogeneous mixture

b)

homogeneous solution

c)

Element

d)

Compound

14.

What is a homogeneous mixture?

a)

a mixture that is the same throughout.

b)

a mixture that is made up of one type of atom.

c)

a mixture that is made up of one type of compound

d)

a mixture that cannot be separated through physical changes

15.

Physical properties are

a)

properties that can be observed without changing the identity of the substance

b)

properties that describe how a substance changes into a completely different substance

16.

Which of the following is not a chemical property?

a)

rusting

b)

rotting

c)

burning

d)

boiling

17.

This diagram represents a _____.

a)

pure substance that is a compound

b)

mixture of elements

c)

mixture of compounds

d)

pure substance that is an element

18.

Which is an example of a physical property?

a)

rusting

b)

boiling point

c)

combustion

d)

reactivity with water

19.

Sugar dissolves in water. This is an example of....

a)

Physical Change

b)

Chemical Change

20.

Which is the best set of techniques to use for separating a mixture of water, sugar, and pebbles?

a)

magnetism and crystallization

b)

filtration and crystallization

c)

filtration

d)

filtration and magnetism

21.

Which one of these is a chemical property?

a)

melting point

b)

color

c)

flammability

d)

boiling point

22.

Evaporation is what kind of change?

a)

chemical

b)

physical

23.

A pure substance that cannot be broken down into other substances by chemical or physical means.

a)

compound

b)

mixture

c)

element

d)

atom

24.

Is melting point of a substance a physical or chemical property?

a)

chemical

b)

physical

25.

The building block of matter is

a)

mixture

b)

atom

c)

substance

d)

element

26.

When you freeze water, it turns to ice. What kind of change is this?

a)

physical

b)

chemical

27.

The _________ of an element equals the number of protons in an atom of that element.

a)

atomic number

b)

neutrons

c)

isotopes

d)

mass number

28.

If an element has 3 valence electrons, what charge will likely form on its ion ?

a)

+3

b)

+5

c)

-3

d)

-5

29.

If an atom of oxygen has a charge of -2, how many electrons does the atom have?

a)

6

b)

8

c)

18

d)

10

30.

What is the atomic number of the atom pictured?

a)

9

b)

10

c)

18

d)

19

31.

How many protons does this isotope of titanium have?

a)

48

b)

22

c)

26

d)

70

32.

An aluminum isotope consists of 13 protons, 13 electrons, and 14 neutrons. Its mass number is

a)

13

b)

14

c)

27

d)

40

33.

number of neutrons =

a)

atomic number - mass number

b)

isotope number - atomic weight

c)

mass number - atomic weight

d)

mass number - atomic number

34.

Isotopes have different numbers of

a)

neutrons

b)

protons

c)

electrons

d)

properties

35.

Atomic mass is equal to the number of...

a)

Protons + Electrons

b)

Electrons

c)

Protons + Neutrons

d)

Electrons + Neutrons

36.

When an atom loses a valence electron, it becomes a(n) _____________ ion.

a)

negative

b)

positive

c)

polyatomic

d)

neutral

37.

Where can you find the protons and neutrons?

a)

outside the atom

b)

electron cloud

c)

nucleus

d)

cytoplasm

38.

Rounding the atomic weight to the nearest whole number gives us the _____

a)

mass number

b)

atomic number

c)

electrons

d)

neutrons

39.

Atomic mass is equal to the number of...

a)

Protons + Electrons

b)

Electrons

c)

Protons + Neutrons

d)

Electrons + Neutrons

40.

What is the atomic mass of the atom pictured?

a)

9

b)

10

c)

18

d)

19

41.

How many neutrons does an atom of the isotope Neon-22 have?

a)

10

b)

12

c)

22

d)

20

42.

An atom has 10 protons, 15 neutrons and 10 electrons what is its mass number.

a)

20

b)

10

c)

5

d)

25

43.

Magnesium's ion

a)

Mg+

b)

Mg2-

c)

Mg-

d)

Mg2+

44.

What is the mass number of an atom of gold with 117 neutrons?

a)

197

b)

117

c)

196

d)

196.97

45.

How many neutrons does an atom of Nitrogen-13 have?

a)

6

b)

7

c)

5

d)

13

46.

Ions are:

a)

atoms with a positive or negative charge

b)

atoms with no charge

c)

atoms with ONLY a negative charge

d)

atoms with ONLY a positive charge

47.

If an atom of nickel has a charge of +3, how many electrons does the atom have?

a)

28

b)

25

c)

31

d)

26

48.

What charge does the nucleus have?

a)

negative

b)

positive

c)

neutral

49.

How many protons does this isotope of titanium have?

a)

48

b)

22

c)

70

d)

26

50.

How do you find atomic mass?

a)

Multiply the protons by the neutrons

b)

Subtract the number of protons and neutrons and divide by the atomic mass

c)

Add the number of neutrons and protons

d)

Multiply the number of protons by the atomic mass

51.

average atomic mass is _______ the most abundant isotope(s) (the isotope(s) that is most common in nature)

a)

average of

b)

closest to

c)

a combination of

52.

We round the atomic mass to the nearest ________ if we don't know which isotope to use.

a)

Halogen

b)

Noble Gas

c)

Whole number

d)

Isotope

53.

Carbons average mass is 12.011(carbon -12 is 99% in nature and carbon -13 is 1% in nature) ...so

a)

The average is 11.213 (closest to one found more often in nature, Carbon - 12)

b)

The average is 12.011 (closest to one found more often in nature, Carbon - 12)

c)

The average is 13.076 (closest to one found more often in nature, Carbon - 12)

d)

The average is 14.480 (closest to one found more often in nature, Carbon - 12)

54.

Atomic radius

a)

Components of an atom

b)

Amount of atoms

c)

Weight of an atom

d)

Size of an atom

55.

What is the ionic radius? (cations get smaller = + = lose electrons) and (anions get larger = - = gain electrons)

a)

components of + or - ions

b)

amount of + or - ions

c)

size of + or - ion

d)

weight of + or - ion

56.

What is ionization energy?

a)

energy to add an electron = easier the larger the atom is

b)

energy to remove an electron = easier the larger the atom is

c)

energy to remove an electron = easier to smaller the atom is

d)

energy to add an electron = easier the smaller the atom is

57.

What is electronegativity?

a)

tendency to form negative ion in a chemical reaction ( leave out noble gases)

b)

tendency to form positive ion in a chemical reaction (leave out noble gases)

c)

tendency to form neutral ion in a chemical reaction (leave out noble gases)

58.

What is shielding?

a)

The process by which each element's valence electrons will at times "overshadow" another element's valence electrons

b)

Orbitals

c)

Energy levels

d)

Valence electrons

59.

What is nuclear charge?

a)

Charge of a nucleus (protons)

b)

Charge of an atom (protons)

c)

Charge of nucleus (valence electrons)

d)

Charge of an atom (valence electrons)

60.

Radius increases...

a)

up and right

b)

down and left

c)

up and left

d)

down and right

61.

Ionization energy increases

a)

up and left

b)

up and right

c)

down and right

d)

down and left

62.

Electronegativety increases

a)

up and right

b)

up and left

c)

down and left

d)

down and right

63.

Shielding increases

a)

up

b)

down

c)

right

d)

left

64.

Non-metallic character increases

a)

↙

b)

↗

65.

Metallic character increases

a)

↙

b)

↗

66.

Select all that are true

a)

Cations are +

b)

Anions are +

c)

Cations are -

d)

Anions are -

67.

What family is this?

a)

Noble Gases

b)

Alkaline Earth Metals

c)

Alkali Metals

d)

Halogens

68.

What family is this?

a)

Alkali Metals

b)

Alkaline Earth Metals

c)

Transition Metals

d)

Halogens

69.

What family is this?

a)

Halogens

b)

Noble Gases

c)

Alkali Metals

d)

Alkaline Earth Metals

70.

What is the name of the purple group?

a)

Halogens

b)

Noble Gases

c)

Transitions Metals

d)

Alkali Metals

71.

What is the name of the brown group?

a)

Alkaline Earth Metals

b)

Halogens

c)

Alkali Metals

d)

Transition Metals

72.

What are the names of the families in white?

a)

Lanthanide on top

Actinide on the bottom

b)

Actinide on top

Lanthanide on the bottom

c)

Post-Alakides on top

Alakolds on the bottom

d)

Post-Alakides on top

Harlenthides on the bottom

73.

What is true about ionic size?

a)

The ionic size is when the atom loses or gains electrons to become ONLY positively charged

b)

The ionic size is when the atom loses or gains neutrons to become negatively or positively charged isotopes

c)

The ionic size is when the atom loses or gains electrons to become ONLY negatively charged

d)

The ionic size is when the atom loses or gains electrons to become negatively or positively charged ions

74.

Select all that are true

a)

negative means subtract/lose so ion is smaller than neutral atom

b)

positive means add/gain so ion is larger than neutral atom

c)

negative means add/gain so ion is larger than neutral atom

d)

positive means subtract / lose so ion is smaller than neutral atom

75.

To excite an atom, there needs be...

a)

Absorption of energy

b)

Emission of energy

c)

Movement of electrons

d)

A proton

76.

The principle quantum number, n, represents the:

a)

spin value

b)

suborbital value

c)

energy level

d)

magnetic value

77.
There are 4 different types of sublevels: s,p,d,f
a)
true
b)
false
78.

Which shape represents the shape of an "s" orbital?

a)
b)
c)
d)
79.

How many orbitals does an 's' sublevel have?

a)

1

b)

3

c)

5

d)

7

80.

What is the shape of 'p' orbitals?

a)

Dumbbell shaped

b)

Peanut shaped

c)

Spherical shaped

d)

Hybrid structure

81.

The number of orbitals in 'p' sub level

a)

2

b)

3

c)

4

82.

How many electrons can a d sublevel hold?

a)

14

b)

10

c)

2

d)

6

83.

What are the orbitals for n=4

a)

s

b)

s, p

c)

s, p, d

d)

s, p, d, f

84.

Number of electrons present in each orbital

a)

2

b)

3

c)

4

85.

A three-dimensional region around a nucleus where an electron may be found is called ---?

a)

orbit

b)

circle

c)

orbital

d)

circuit

86.

What is the lowest energy state of an atom called?

a)

the ground state

b)

the excited state

c)

the solid state

d)

the chaotic state

87.
What orbital shapes are found at the 2nd energy level
a)
s only
b)
s and p
c)
s, p, d and f
d)
p only
88.
An orbital that can never exist according to the quantum description of the atom is
a)
6d.
b)
3f.
c)
3d.
d)
8s.
89.
1.  What is the shape of an s orbital?
a)
sphere
b)
dumbbell
c)
double dumbbell
d)
TOO COMPLEX TO KNOW IT.
90.
What is the shape of a p orbital?
a)
sphere
b)
it's just too complex to thing about it
c)
dumbbell
d)
I don't know this stuff.
91.
How many d orbitals are there in a given sublevel?
a)
1
b)
3
c)
5
d)
7
92.
How many p orbitals are there in a sublevel?
a)
2
b)
1
c)
4
d)
3
93.
How many electrons can the d sublevel hold?
a)
8
b)
10
c)
2
d)
4
94.
Which is associated with more energy? 
a)
2p
b)
2s
c)
3p
d)
1s
95.
How many total electrons can the f orbitals in a sublevel hold?
a)
2
b)
14
c)
6
d)
10
96.
Which orbital has the least amount of energy? 
a)
p orbital
b)
d orbital
c)
s orbital 
d)
What is an orbital?
97.

How many orbitals does an s sublevel have?

a)

1

b)

3

c)

5

d)

7

98.

How many orbitals does an f sublevel have?

a)

1

b)

3

c)

5

d)

7

99.

What are the orbitals that make up the n=1 energy level?

a)

s

b)

s, p

c)

s, p, d

d)

s, p, d, f

100.

Electrons fill energy levels and sublevels _____ in energy first.

a)

lower

b)

higher

101.
What does Pauli exclusion principle state ?
a)
states that each electron occupies the lowest energy orbital available
b)
states that a maximum of two electrons can occupy a single atomic orbital, but if only if the electros have opposite spins
c)
states that single electrons electrons with the same spin must occupy each-energy orbital before additional electrons with opposite spins can occupy the same orbitals
102.
What does Hund's rule states ?
a)
states that single electrons electrons with the same spin must occupy each-energy orbital before additional electrons with opposite spins can occupy the same orbitals
b)
states that each electron occupies the lowest energy orbital available
c)
states that a maximum of two electrons can occupy a single atomic orbital, but if only if the electros have opposite spins
103.
Electrons occupy orbitals of lowest energy first is part of what electron configuration rule?
a)
Hund’s Rule
b)
Aufbau Principle
c)
Pauli Exclusion Principle
104.
What do you start electron configuration with?
a)
1s2
b)
1d10
c)
1f14
d)
1p6
105.

1s22s22p63s1

(Sodium)

a)

ionic configuration

b)

regular configuration

c)

shortcut configuration

d)

rearranged configuration

106.

[Kr] 4d105s25p5

(Iodine)

a)

ionic configuration

b)

regular configuration

c)

shortcut configuration

d)

rearranged configuration

107.

1s22s22p63s23p6

(Calcium+2)

a)

ionic configuration

b)

regular configuration

c)

shortcut configuration

d)

rearranged configuration

108.

1s22s22p63s23p63d104s24p6

(Gallium)

a)

ionic configuration

b)

regular configuration

c)

shortcut configuration

d)

rearranged configuration

109.
What atom matches this electron configuration?
1s22s22p63s23p64s23d10
a)
Zinc
b)
Copper
c)
Nickel
d)
Germanium
110.
 The diagram above represents two electrons with 
a)
a. opposite spins.
b)
 b. the same spin.
c)
c. different energies.
d)
d. different energy levels.
111.
What is the correct electron configuration for a ground-state atom with 7 electrons? 
a)
 a. 1s2 2s2 2p3
b)
 b. 1s2 2s2 2p2 3s1
c)
c. 1s2 2s3 2p2
d)
 d. 1s2 2s5
112.
What is the correct noble-gas notation for the electron configuration of an atom of chlorine? 
a)
a. [Ar]3s2 3p5
b)
 b. [Ne]3s2 3p4
c)
 c. [Ar]3s2 3p4
d)
 d. [Ne]3s2 3p5
113.
Which element is pictured?
a)
neon
b)
fluorine
c)
magnesium
d)
argon
114.
This orbital diagram represents:  
a)
C
b)
B
c)
N
d)
O
115.

Which color has the highest frequency?

a)

red

b)

orange

c)

green

d)

blue

116.
Which electron configuration belongs to Chlorine (Cl)?
a)
1s2 2s2 2p6 3s2 3p5
b)
1s2 2s2 2p6 3s2 3p6
c)
1s2 2s2 2p6 3s2 3p7
117.
What electron configuration matches an oxygen atom?
a)
1s22s22p63s2, 3p64s23d104p5
b)
1s22s22p4
c)
1s22s22p6
d)
1s22s22p63s23p64s23d1
118.

What element matches this electron configuration?

1s22s22p63s2

a)

Neon

b)

Magnesium

c)

Aluminum

d)

Potassium

119.
How many electrons can the d sublevel hold?
a)
8
b)
10
c)
2
d)
4
120.
Rows on the period table are called _____ while columns are called _____.
a)
groups, families
b)
groups, periods
c)
periods, groups
d)
families, groups
121.
Electrons occupy orbitals of lowest energy first is part of what electron configuration rule?
a)
Hund’s Rule
b)
Aufbau Principle
c)
Pauli Exclusion Principle
122.
Electrons are paired based on their spin directions, clockwise and counterclockwise, is what electron configuration rule?
a)
Hund’s Rule
b)
Aufbau Principle
c)
Pauli Exclusion Principle
123.

Which is the correct shape of each of the following

a)

s= spherical

p= double donut

d= double dumbbell

f= dumbbell donut

b)

s=spherical

p=dumbell

d= double dumbbell and 1 dumbbell donut

f= complex

c)

s= spherical

p= double bell

d= dumbbell donut

f= complex sphere

124.

Which is the correct amount of orbitals for each of the following

a)

s= 1

p=3

d= 5

f=7

b)

s=2

p=4

d=6

f=8

c)

s=1

p=3

d=6

f=10

125.

Which is the correct amount of electrons for each of the following

a)

s= 1

p=3

d= 5

f=7

b)

s=2

p=4

d=6

f=8

c)

s=2

p=6

d=10

f=14

126.
This is a correct dot diagram for oxygen (O)
a)
true
b)
false
127.
This is the correct dot diagram for sodium (Na)
a)
true
b)
false
128.
This is a correct dot diagram for fluorine (F)
a)
true
b)
false
129.
This is a correct dot diagram for nitrogen (N)
a)
true
b)
false
130.

Electrons for each sublevel are:

s = 2

p = 6

d = 10

f = 14

a)

True

b)

False

131.

Orbitals for each subelevel are:

s = 1

p = 3

d = 5

f = 7

a)

True

b)

False

132.

What is true about 1s1?

a)

The 1 is the # of electrons

b)

The s is the sublevel

c)

The 1 is the value of the energy level

d)

It is the electron configuration for Hydrogen

e)

All of these

133.

What is true about Cd+2?

a)

The +2 means that two electrons are lost

b)

The +2 means that two electrons are gained

134.

H2O

a)

Ionic Bond

b)

Both Bonds

c)

Neither Bonds

d)

Covalent Bonds

135.
Which of the following has a full valence shell?
a)
Oxygen
b)
Neon
c)
Barium
d)
Carbon
136.
Elements on the LEFT side of the periodic table will most likely form:
a)
Positive ions
b)
Negative ions
c)
Neutral Ions
d)
None of these
137.
An ionic bond forms when atoms ___________ electrons.
a)
gain
b)
share
c)
increase
d)
transfer
138.
Which type of bond has an equal sharing of electrons?
a)
Polar Covalent 
b)
Non Polar Covalent
c)
Ionic
d)
Metallic
139.
Which type of bond has an unequal sharing of electrons?
a)
Polar Covalent 
b)
Non Polar Covalent
c)
Ionic
d)
Metallic
140.
Which type of bond has a transfer of an electron from on atom to another?
a)
Polar Covalent 
b)
Non Polar Covalent
c)
Ionic
d)
Metallic
141.
Bonds that form between two metals are called ______________ bonds.
a)
ionic 
b)
covalent
c)
metallic
d)
pervasive
142.
Covalent compounds
a)
Share electrons
b)
transfer electrons
c)
contain a sea of electrons
d)
conduct electricity
143.
How many valence electrons in this structure?
a)
6
b)
5
c)
4
d)
7
144.
What type of bond forms between two or more atoms that are charged (+/-)?
a)
Covalent bond
b)
Incomplete bond
c)
Ionic bond
d)
Metallic bond
145.
Which of the following is an example of an IONIC COMPOUND?
a)
NaCl
b)
H2O
c)
CO2
d)
NO
146.
Which of the following is an example of a COVALENT COMPOUND?
a)
H2S
b)
KI
c)
CaCl2
d)
MgO
147.
Which category of elements have the property of being malleable and ductile?
a)
gases
b)
metals
c)
metalloids
d)
nonmetals
148.
Alloys include a "sea" of free moving _______. 
a)
electrons
b)
atoms 
c)
molecules 
d)
protons 
149.
Ionic bonds are between _______ and ________. 
a)
nonmetals and nonmetals 
b)
metals and metals 
c)
metals and nonmetals
d)
none
150.
Covalent bonds tend to happen between two
a)
metals
b)
nonmetals
c)
metal and nonmetal
151.
The compound formed between lithium and chlorine is _________.
a)
ionic
b)
covalent
152.
Which type of bond has an equal sharing of electrons?
a)
Polar Covalent 
b)
Non Polar Covalent
c)
Ionic
d)
Metallic
153.
When electrons are shared unequally a/an ___________ bond is formed 
a)
ionic 
b)
hydrogen
c)
polar covalent 
d)
nonpolar covalent
154.
In what form can an ionic compound conduct electricity?
a)
when dissolved in water
b)
as a solid
c)
as a crystal
d)
when warmed slightly
155.
The bonds in Na2O are best described as 
a)
a.  covalent, because valence electrons are shared.
b)
covalent, because valence electrons are transferred
c)
ionic, because valance electrons are shared.
d)
ionic, because valance electrons are transferred. 
156.
Which is the correct lewis dot structure for calcium chloride?
a)
A
b)
B
c)
C
157.

Metals have....

Select all that apply

a)

Negatively charged electrons that act as glue to hold positively charged ions together

b)

High melting points

c)

Electrons that are delocalised and able to move (this is why they conduct)

d)

A dull luster

158.

If three electrons are available to fill three empty 2p atomic orbitals, how will the electrons be distributed in the three orbitals?

____in each orbital

a)

One

b)

Two

c)

Three

d)

Four

159.

The total number of electrons in the highest level of the argon atom (atomic number 18) is___

a)

7

b)

8

c)

9

d)

10

160.

If n = 2 how many orbitals are possible?

a)

2

b)

3

c)

4

d)

5

161.

How many unpaired electrons are in a sulfur atom, which has the atomic number 16?

a)

4

b)

3

c)

2

d)

1

162.
What is the measure of a tetrahedral bond angle?
a)
90 Degrees
b)
109.5 Degrees
c)
120 Degrees
d)
180 Degrees
163.
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
164.
Which of the following molecular shapes would have a bond angle of 180 Degrees?
a)
Bent
b)
Trigonal Planar
c)
Tetrahedral
d)
Linear
165.
The bond angle for a trigonal planar molecule is 
a)
90 Degrees
b)
109.5 Degrees
c)
120 Degrees
d)
180 Degrees
166.

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

a)

1

b)

2

c)

3

d)

4

167.
 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
168.
What is the VSEPR theory used to predict?
a)
Bond Strength
b)
Polarity
c)
Molecular Shape
d)
Electronegativity
169.
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
170.

Which of the following will have this geometry?

a)

H2S

b)

CCl4

c)

NH3

d)

HCl

171.

Which of these molecules will have this molecular geometry?

a)

PCl5

b)

SF6

c)

CF5

d)

SnF4

172.

Which of these molecules will have this molecular geometry?

a)

SO4

b)

CCl4

c)

NH2

d)

PCl4

173.

Which of the following molecules has this molecular geometry?

a)

PCl5

b)

SiO4

c)

SCl6

d)

CH4

174.

Which of the following molecules will have this molecular geometry?

a)

SF4

b)

CCl4

c)

SiO4

d)

CF2

175.

Which of these molecules will have this molecular geometry?

a)

BCl3

b)

NH3

c)

CO2

d)

CCl4

176.

Which of these molecules will have this molecular geometry?

a)

H2S

b)

CCl2

c)

NH2

d)

CO2

177.

Which of these structures has one un-shared pairs of electrons?

a)
b)
c)
d)
178.

Which of the following structures would you draw for CCl4 ?

a)
b)
c)
d)
179.

Which of these would be the correct molecular geometry for water?

a)
b)
c)
d)
180.

Which of the following has bond angles of 120 degrees?

a)

tetrahedral

b)

bent

c)

trigonal planar

d)

trigonal pyramidal

181.

Which of these molecular shapes is definitely polar?

a)
b)
c)
d)

Similar Resources on Wayground

Chemistry Final Exam Review

185 questions

Chemistry Final Exam Review

quiz

Worksheet

•

9th - 12th Grade

HC U1 Retake assignment

181 questions

HC U1 Retake assignment

quiz

Worksheet

•

12th Grade

Semester 2 Exam Review

179 questions

Semester 2 Exam Review

quiz

Worksheet

•

9th - 12th Grade

First Weeks Review

184 questions

First Weeks Review

quiz

Worksheet

•

9th - 12th Grade