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CHEM I Spring 2022 Final Exam Practice Quiz

Total questions: 165

Worksheet time: 3hrs 45mins

Name
Class
Date
1.
all matter is made of what 
a)
energy 
b)
atoms 
c)
electrons 
d)
compounds 
2.
The positive particles of an atom are 
a)
electrons 
b)
positrons 
c)
neutrons 
d)
protons 
3.
the central region of an atom where its neutrons and protons are is its 
a)
nucleus 
b)
electron cloud
c)
core 
d)
center 
4.
an atom with atomic number 6 would have how many protons 
a)
6
b)
12
c)
3
d)
cannot be determined 
5.
How many protons does this atom have?
a)
2.5
b)
6
c)
5
d)
10.811
6.
What part of the atom is the arrow pointing to?
a)
nucleus
b)
proton
c)
electron shell
d)
electron
7.
Which of the following represents an element?
a)
H2O
b)
H2
c)
NaCl
d)
CaCO3
8.
A combination of substances that are not chemically combined is called a(n)____________. 
a)
mixture
b)
compound
c)
physical
9.
The theory that states that all matter is made of atoms & molecules and those particles are always in motion. 
a)
Conservation Theory 
b)
Kinetic Theory of Matter
c)
Phases of Matter Theory 
d)
The Theory of Energy & Matter 
10.
Higher temperatures make particles move ___________.
a)
Slower
b)
In different directions 
c)
Faster
d)
In one direction 
11.
In the liquid phase, particles are tightly packed together, vibrating in a fixed position. 
a)
True
b)
False, particles in a liquid are closely packed together but can slide past each other
c)
False, particles in a liquid are moving very rapidly and are very far apart
d)
False, liquids have a definite shape and volume
12.
Melting, evaporation, and sublimation are all examples of ___________ phase changes. 
a)
Endothermic
b)
Exothermic 
13.
The temperature at which a liquid becomes a gas is called its ___________________.
a)
Melting point
b)
Freezing point 
c)
Condensation point 
d)
Boiling point 
14.
Which phase of matter has an indefinite shape and volume?
a)
Gas
b)
Solid
c)
Plasma
d)
Liquid 
15.

What is a physical property?

a)

A property that describes how something changes over time

b)

An observable property that describes the state of a system

c)

A property that describes how reactive something is

16.

Is crumpling a piece of paper a physical or chemical change?

a)

Physical

b)

Chemical

17.

Physical Properties can be ________

a)

observed without changing the matter being studied

b)

observed and measured but the matter has to be changed

c)

observed and measured without changing the matter being studied

18.

What are properties that do depend on the amount of matter present called?

a)

Mass

b)

Hardness

c)

Extensive

d)

Intensive

19.

Name an extensive property

a)

Color

b)

Mass

c)

Odor

d)

Luster

20.

Name an extensive property

a)

Harness

b)

Boiling point

c)

Density

d)

Weight

21.

Freezing point is an example of

a)

extensive property

b)

intensive property

22.

Surface area is an

a)

Extensive property

b)

Intensive Property

23.
a)
Student A
b)
Student B
c)
Student C
d)
Cannot be determined
24.
The students measured length during a science experiement, they got 12 cm. But the actual measurement was 14.25 cm. What was the percent error?
a)
15.79%
b)
18.75%
c)
2.25%
d)
18%
25.

Which is the more precise measurement?

a)

4 mL

b)

4.3 mL

c)

4.30 mL

d)

4.300 mL

26.
Describe the accuracy and precision of the image
a)
Accurate and Precise
b)
Accurate and not precise
c)
Not Accurate and Precise
d)
not accurate and not precise
27.
Volume?
a)
63.5 mL
b)
63 mL
c)
63.55 mL
d)
6 mL
28.
Which of the following numbers has three significant figures?
a)
1014 miles
b)
101 feet
c)
1000 yards
d)
all of the choices
29.
How would you write 4.3756 x 104 in standard form?
a)
437,560,000
b)
0.00043756
c)
43,756
d)
4,3756
30.
Calculate the answer to the following problem and round the final answer to the correct number of sig figs:
24.567 + 0.04478 =
a)
24.61178
b)
24.612
c)
24.611
d)
24.61
31.
Express the following number in scientific notation: 
0.00075
a)
7.5 x 10-4
b)
7.5 x 104
c)
7.5 x 103
d)
7.5 x 10-3
32.

Which part of the atomic theory did Niels Bohr prove?

a)

there are electrons

b)

there is a nucleus

c)

electrons are in energy levels

d)

gold foil experiment

33.

Which part of the atomic theory did JJ Thomson prove?

a)

there are electrons

b)

electrons are in energy levels

c)

there is a nucleus

d)

cathode ray tube

34.

What experiment did JJ Thomson use?

a)

gold foil experiment

b)

cathode ray tube experiment

35.

John Dalton wrote postulates to make the idea of the atom useful. Which postulate below was proven wrong?

a)

All elements are made up of tiny indivisible particles called atoms.

b)

The atoms of one element are different from the atoms of another element.

c)

Atoms of different elements chemically combine to form chemical compounds.

d)

During chemical reactions, atoms are rearranged.

36.

JJ Thomson came up with which model for the atom?

a)

planetary model

b)

electron cloud model

c)

plum pudding model

d)

nuclear model

37.

After Rutherford discovered the nucleus, which model is believed to be true?

a)

protons, neutrons, and electrons are evenly distributed

b)

the nucleus is made of protons, neutrons, and electrons

c)

the nucleus is made of protons and electrons

d)

the model is mostly empty space with a central nucleus

38.

Where is most of the mass of an atom located?

a)

the nucleus

b)

the electron cloud

c)

the space in between particles

d)

in shells

39.

Mass number is ______.

a)

number of protons + electrons

b)

number of neutrons + protons

c)

number of electrons only

d)

number of neutrons only

40.

Isotopes are _______.

a)

elements with the same atomic number and same mass

b)

elements with different atomic number but same mass

c)

elements with same atomic number but different masses

d)

different elements with same number of electrons

41.

Select the true statements about Isotopes.

a)

Isotopes are elements with the same atomic number but different masses

b)

isotopes are elements with different number of protons but same number of neutrons

c)

isotopes are elements with Same number of protons and electrons but different number of neutrons

d)

elements exist as mixtures of isotopes

42.
He developed the planetary model of the atom.
a)
Rutherford
b)
Bohr
c)
Chadwick
d)
Dalton
43.
The scientist responsible for "discovering" the nucleus is:
a)
Bohr
b)
Rutherford
c)
Schroedinger
d)
Einstein
44.
How many nitrogen atoms in 
Mg(NO3)2
a)
1
b)
2
c)
3
d)
6
45.

How many different elements are present in the following chemical formula: CO2

a)

1

b)

2

c)

3

d)

4

46.

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

47.

What is the empirical formula for N2S3?

a)

NS

b)

N3S2

c)

N2S3

d)

N1S1.5

48.

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

49.
The atomic number tells you what?
a)
number of electrons
b)
number of protons
c)
number of neutrons
d)
both electrons and protons in an atom.
50.
Elements which are shiny, conduct electricity and heat are called
a)
metal
b)
nonmetal
c)
metalloid
d)
nonexistent
51.
Which is a halogen?
a)
Helium
b)
Chlorine
c)
Oxygen
d)
Neptune
52.
Which is an alkali metal?
a)
Magnesium
b)
Iron
c)
Sodium
d)
Europium
53.
If an atom had the same properties as fluorine (F), it would probably be located in
a)
period 1.
b)
period 2.
c)
group 2.
d)
group 17.
54.
Atoms with similar properties are most likely located...
a)
in the same period.
b)
in the same group.
c)
in different periods.
d)
to the right and left of each other.
55.
Looking at atoms in the same group/family, what factor affects Coulombic attraction?
a)
number of protons
b)
distance from the nucleus
56.
Ionization energy is the...
a)
energy needed to remove the outermost electron.
b)
ability of an atom to attract electrons from another atom.
57.
Electronegativity is the...
a)
energy needed to remove the outermost electron.
b)
ability of an atom to attract electrons from another atom.
58.
As the Coulombic attraction increases the atomic radius: increases or decreases?
a)
increases
b)
decreases
59.
Which element has the smaller atomic radius: potassium (K) or bromine (Br)?
a)
potassium (K)
b)
bromine (Br)
60.
Which element has the greatest ionization energy: Aluminum (Al)    or    Chlorine (Cl)?
a)
Aluminum (Al)
b)
Chlorine (Cl)
61.

Based on the image on the last slide. As you go across a period, does the atomic radius get smaller or larger?

a)

Smaller

b)

Larger

c)

Stays the same

62.

Put these elements in order of INCREASING atomic radius.

Li, O, C, F

a)

O, C, F, Li

b)

F, O, C, Li

c)

Li, C, O, F

d)

C, F, Li, O

63.

Put these elements in order of DECREASING atomic radius.

Ca, Be, Ba, Sr

a)

Sr, Ba, Be, Ca

b)

Be, Ca, Sr, Ba

c)

Ba, Sr, Ca, Be

d)

Ca, Be, Ba, Sr

64.

Which elements do you think will have a low ionization energy and lose electrons more readily?

a)

elements that form anions (negative charge)

b)

Elements that form cations (positive charge)

c)

Transition metals

65.

Element A has a ionization energy of 419 kJ/mol. What block is it likely in?

a)

P block

b)

S block

c)

D block

d)

F block

66.

Element B has an ionization energy of 1000 kJ/mol. What block is it likely to be in?

a)

P block

b)

S block

c)

F block

d)

D block

67.

What is the name of PBr3

a)

phosphorus tribromide

b)

phosphorus bromide

c)

phosphorus (III) bromide

d)

phosphorus bromine

68.

What is the name of FeO?

a)

iron(III) oxide

b)

iron(II) oxide

c)

iron(III) oxygen

d)

iron oxide

69.

What is the name of NaHCO3?

a)

sodium carbonate

b)

sodium bicarbonate

c)

sodium hydride

d)

sodium hydroxide

70.

What is the name of Cu(NO3)3?

a)

copper(III) nitrate

b)

copper trinitrate

c)

copper nitride

d)

copper(III) nitrite

71.

What is the correct formula for nickel(II) carbonate?

a)

NiCO3

b)

Ni(CO3)2

c)

NiHCO3

d)

Ni(NO3)2

72.

What is the correct formula for tin(II) nitrate?

a)

SnNO3

b)

Sn2NO3

c)

TiNO3

d)

Sn(NO3)2

73.

What is the correct name of MgCl2?

a)

magnesium chlorine

b)

magnesium dichloride

c)

magnesium chloride

d)

magnesium (II) chloride

74.

Covalent Compounds HAVE a positive (+) or negative (-) charge

a)

True

b)

False

c)

huh?

d)

What was that now?

75.
CO2
a)
Ionic
b)
Covalent
c)
Polyatomic Ion 
d)
Metallic 
76.
NaCl
a)
Ionic
b)
Covalent
c)
Metallic
d)
Polyatomic Ion 
77.
MgCl2
a)
Ionic
b)
Covalent
c)
Polyatomic Ion
d)
Metallic 
78.
Ionic compounds are bonds between
a)
Metals and Metals
b)
Metals and Nonmetals
c)
Nonmetals and Nonmetals
d)
None of the above
79.
Which is most likely to form a negative ion?
a)
an element from group 17
b)
a metal
c)
an element from group 1
d)
an element with atoms that have eight valence electrons
80.
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
81.

Classify ionic or molecular

C2H2

a)

Ionic

b)

Molecular

82.
Which following is a nonmetal?
a)
Se
b)
Mn
c)
Na
d)
Be
83.
Which following is a molecular compound?
a)
SO2
b)
K2O
c)
CaO
d)
BeO
84.

How will you prepare a 10% v/v HCl?

a)

10 ml HCl in 10 ml water

b)

1ml HCl in 9 ml water

c)

10 ml water in 1ml HCl

d)

10 ml HCl in 20 ml water

85.

It is a measurement of the moles in the total volume of the solution.

a)

MOLALIY

b)

MOLARITY

c)

NORMALITY

86.

Which sweet tea would you expect to taste the sweetest?

a)

0.5 M

b)

1 M

c)

2 M

d)

3 M

87.

Calculate the molarity of a solution containing 1.5 moles of NaCl in 0.5 L of solution.

a)

1.5 M

b)

3 M

c)

0.33 M

d)

0.75 M

88.

When making sweet tea, sugar is the (1) and the tea is the (2).

a)

1-solute, 2-solvent

b)

1-solvent, 2-solute

c)

1-solution, 2- solute

d)

1-solvent, 2- solution

89.

According the solubility graph, what is the solubility of KNO3 at 60 °C? (answers in g/100g of water)

a)

40

b)

90

c)

130

d)

20

90.

A pharmacist creates a cream for a skin rash that has 2. 75g of the actual medication in a 20 g tube. What is the %m/m?

a)

13.75 %

b)

27.5 %

c)

6.9 %

d)

55 %

91.

How many mL of stock solution of 2M NaCl do you need to prepare 100 mL of 0.150M NaCl?

a)

7.5 mL

b)

15 mL

c)

1333 mL

d)

200 mL

92.
Molality is measured in
a)
mols per L
b)
mols per kg
c)
mols per kJ
d)
mols per mL
93.

Which solution is more concentrated?

Solution 1:

500 mL of water

100 g of salt


Solution 2:

500 mL of water

90 g of salt

a)

Solution 1

b)

Solution 2

c)

They have the same concentration

d)

I have no idea

94.

What is the left part of a chemical equation called?

2H2 + O2 ---> 2H2O

a)

Reactants

b)

Yields

c)

Products

d)

Chemical equation

95.

What is the right part of a chemical equation called?

2H2 + O2 ---> 2H2O

a)

Reactants

b)

Yields

c)

Products

d)

Chemical Equation

96.

Which of the following equations are correctly balanced?

a)

12CO2 + H2O ---> C6H12O6 + O2

b)

CO2 + H2O ---> 3C6H12O6 + O2

c)

CO2 + 9H2O ---> C6H12O6 + O2

d)

6CO2 + 6H2O ---> C6H12O6 + 6O2

97.
How many HCl molecules do you need to balance this equation? 
Mg +  __HCl --->  MgCl2 + H2
a)
1
b)
2
c)
3
d)
4
98.

Balance the following equation:

___ H2+ ___ O2→___ H2O

a)

1, 1, 3

b)

2, 2, 2

c)

1, 2, 1

d)

2,1, 2

99.

Which type of reaction has the general formula

AB + CD → AD + CB

a)

Double Replacement

b)

Single Replacement

c)

Synthesis

d)

Decomposition

e)

Combustion

100.

What type of reaction is this?

Cl2 + 2KI → I2 + 2KCl

a)

Synthesis

b)

Single replacement

c)

Double replacement

d)

Decomposition

e)

Combustion

101.

What type of reaction is this?

2C5H10 + 15O2 → 10CO2 + 10H2O

a)

Synthesis

b)

Decomposition

c)

Single replacement

d)

Double replacement

e)

Combustion

102.

Which of the following is an example of synthesis?

a)

Na + Br2 → NaBr

b)

KClO3 → KCl + O2

c)

HgO + Cl2 →HgCl + O2

d)

Cl2 + NaBr → NaCl + Br2

103.
Which of the following is the general formula for a decomposition reaction?
a)
A + B  → AB
b)
AB → A + B
c)
AB + C → AC + B
d)
AB + CD → AC + BD
104.

Which of the following is an example of a single replacement reaction?

a)

2NaF ⟶ 2 Na + F2

b)

P2O5 + 3 H2O ⟶ 2H3PO4

c)

2FeCl3 + 3Zn ⟶ 2Fe + 3ZnCl2

d)

C6H12O6 + 6O2 ⟶ 6CO2 + 6 H2O

105.
What is the mole ratio of H2O to H3PO4 in the following chemical equation?   P4O10 + 6 H2O --> 4 H3PO4 
a)
6:4
b)
4:6
c)
1:3
d)
3:1
106.
2Al + 3H2SO4 -> Al2(SO4)3 + 3H2
How many grams of aluminum sulfate would be formed if 250g H2SO4 completely reacted with aluminum?
a)
0.85 g
b)
290 g
c)
450 g
d)
870 g
107.
For the reaction represented by the equation Cl2 + 2KBr → Br2 + 2KCl, how many grams of potassium chloride can be produced from 356 grams potassium bromide?
a)
749 g
b)
225 g
c)
479 g
d)
814 g
108.
Identify the limiting reagent when 6.00 g HCl combines with 5.00 g Mg to form MgCl2.
 
Mg +  2HCl --> MgCl2  +  H2   
 
a)
Mg
b)
H2
c)
MgCl2
d)
HCl
109.

If a chemist calculates the maximum amount of product that could be obtained in a chemical reaction, he or she is calculating the

a)

theoretical yield

b)

mole ratio

c)

actual yield

d)

percentage yield

110.
If we start with 42 grams of C, what is the theoretical yield of Fe (in grams)?
a)
3.5 grams
b)
4.66 grams
c)
260.6 grams
d)
521.2 grams
111.
If we produce 258 grams of a certain product in a reaction, but we could have produced up to 510 grams, what is the percent yield?
a)
50.6%
b)
198%
c)
98%
d)
150.6%
112.
Which of the following is the correct Lewis dot structure for the molecule fluorine (F2)?
a)
A
b)
B
c)
C
d)
D
113.

NH3 has how many lone pairs?

a)

0

b)

1

c)

2

d)

3

114.
How many electrons should Lithium have around its Lewis dot model?
a)
1
b)
2
c)
3
d)
4
115.
According to the octet rule most elements need _______ valence electrons.
a)
2
b)
8
c)
6
d)
18
116.

What is the correct Lewis Dot Structure for ammonia NH3

a)
b)
c)
d)
117.

Which is the correct molecular structure for carbon dioxide?

a)
b)
c)
d)
118.
This is the correct dot diagram for nitrogen (N)
a)
true
b)
false
119.
Define the term resonance structure
a)
Delocalization of electrons in an atom
b)
Delocalization of π electrons within a molecule
c)
Spread of π electrons in an atom
d)
Spread of π electrons within a molecule
120.
How many resonance structures for CH3COO- ion?
a)
1
b)
2
c)
3
d)
4
121.
How many resonance structure can you draw for benzene?
a)
1
b)
2
c)
3
d)
4
122.

Is this molecule polar or non-polar?

a)

Polar

b)

Non-polar

123.

Is this molecule polar or non-polar?

a)

Polar

b)

Non-polar

124.

Is this molecule polar or non-polar?

a)

Non-polar

b)

Polar

125.
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
126.
What geometry will this molecular structure have?: PH3
a)
bent
b)
tetrahedral
c)
linear
d)
trigonal pyramidal
127.
What geometry will this molecular structure have?: H2S
a)
bent
b)
tetrahedral
c)
linear
d)
trigonal pyramidal
128.
What geometry will this molecular structure have?: CCl4
a)
bent
b)
tetrahedral
c)
linear
d)
trigonal pyramidal
129.

What is the molecular geometry for this molecule?

a)

Bent

b)

Trigonal pyramidal

c)

Trigonal planar

d)

Linear

130.
Choose the correct shape for this molecule:
a)
Bent
b)
Linear
c)
Tetrahedral
d)
Trigonal pyramidal
131.
According to Boyle's law of PV, at constant temperature, as the pressure of a given sample of gas is increased, the volume will –
a)
Increase
b)
Decrease
c)
Remains the same
132.
Boyle's PV law : When _______ is held constant, the pressure and volume of a gas are ________  proportional
a)
temperature,  equally
b)
mass, inversely
c)
temperature, inversely
d)
mass, equally
133.
Definite shape and a definite volume.
a)
Gas
b)
Liquid
c)
Solid
134.
In which state are the particles least able to move?  (Which is the solid?)
a)
State A
b)
State B
c)
State C
d)
None
135.
With pressure constant, the temperature of a gas is increased from 30oC to 90oC.  The volume will _____. (Be sure to convert to Kelvin first.)  
a)
 increase by about 20%
b)
 triple
c)
decrease by 1/2 
d)
remain the same
136.
If you collect 22.4 L of oxygen (O2) at standard conditions, you will have ____.  
a)
1 mole of gas
b)
6.02 x 1023 molecules of gas
c)
32 g of gas
d)
All of these answers
137.
The volume occupied by 3 moles of N2 at 0oC and 101.3 kPa is ____.  
a)
67.2 L
b)
22.4 L
c)
7.47 L
d)
134.4 L
138.
A sealed bottle of wet air has a total of 100 kPa of pressure in it. How many kPa of pressure is exerted by just the dry air if the water vapor chart says that the water exerts 4 kPa?
a)
100 kPa
b)
96 kPa
c)
104 kPa
d)
4 kPa
139.
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.
140.

Intermolecular forces for: NH3

a)

Dispersion Force

b)

Dipole dipole

c)

Hydrogen bonding

141.

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

142.

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

a)

higher

b)

lower

143.

Intermolecular forces for: CO2

a)

Dispersion Force

b)

Dipole dipole

c)

Hydrogen bonding

144.
Rank these in order of strength:
covalent bond
London forces
hydrogen bond
dipole-dipole attraction
a)
dipole-dipole>covalent bond>hydrogen bond>London
b)
London>dipole-diple>hydrogen bond>covalent bond
c)
covalent bond>hydrogen bond>dipole-dipole>London
d)
hydrogen bond>dipole-dipole>London>covalent bond
145.
What will be the state of the following molecule?
a)
gas
b)
liquid
c)
solid
146.
What type of forces will the following molecule have?
a)
dispersion forces
b)
dipoles
c)
hydrogen bonding
147.
What forces will the following molecule have?
a)
dispersion
b)
dipole
c)
hydrogen bonding
148.

What letter on the diagram represents a gas?

a)

A

b)

B

c)

C

d)

D

149.

What letter on the diagram represents a liquid?

a)

A

b)

B

c)

C

d)

D

150.

What letter on the diagram represents a solid?

a)

A

b)

B

c)

C

d)

D

151.

What is the melting point of this substance at 1 ATM of pressure?

a)

40

b)

60

c)

100

d)

110

152.

What is the boiling point of this substance at 1 ATM of pressure?

a)

40

b)

60

c)

100

d)

110

153.

What would the state of this substance be at 0.5 ATM of pressure at a 100 degrees Celsius?

a)

Solid

b)

Liquid

c)

Gas

d)

Michigan

154.

The average atmospheric pressure in Michigan is close to 1 ATM. What state would this substance be in if it was a nice summer day with a temperature of 80 o F (27 o C)?

a)

Solid

b)

Liquid

c)

Gas

d)

Michigan

155.

What line segment represents only the solid state? (Diagram F)

a)

A-B

b)

B-C

c)

C-D

d)

D-E

156.

Between which points is the temperature of the substance remaining constant? (Diagram F)

a)

A-B only.

b)

A-B, C-D, E-F

c)

B-C only.

d)

B-C, D-E

157.

A substance's heating curve is shown in the graph. What is its boiling point? (Diagram B)

a)

100 C

b)

60 C

c)

80 C

d)

20 C

158.

Is the substance gaining or losing energy? (Diagram D)

a)

Gaining

b)

Losing

159.

Which line segment demonstrates vaporization occurring? (Diagram E)

a)

B-C

b)

C-D

c)

D-E

d)

E-F

160.

What type of material is this one?

a)

Crystal

b)

Amorphous

c)

Covalent Crystal

d)

Ionic Crystal

161.

Which of the following is an amorphous solid?

a)

Copper(Cu)

b)

Quartz glass (SiO2)

c)

Silicon carbide (SiC)

d)

Sodium Chloride (NaCl)

162.

Which of the following is a network solid or covalent crystalline solid?

a)

Diamond (C)

b)

H2O (Ice)

c)

Calcium Fluoride (CaF2)

d)

Iron Metal (Fe)

163.

Smallest repeating unit of crystal lattice

a)

Lattice site

b)

Unit cell

c)

Crystal lattice

d)

Lattice point

164.

Crystalline solids are

a)

Isotropic

b)

Allotropic

c)

Anisotropic

d)

Isomorphic

165.

An amorphous solid

a)

CaCl2

b)

NaCl

c)

Glass

d)

CsCl