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Total questions: 127

Worksheet time: 3hrs 5mins

Name
Class
Date
1.

Which element in Period 2 has the greatest atomic radius?

a)

Be

b)

C

c)

Na

d)

Li

2.

Which of the group 13 elements is the largest?

a)

B

b)

Ti

c)

Fr

d)

Ga

3.

Of the halogens, which has the smallest radius?

a)

F

b)

Br

c)

He

d)

At

4.

Of the halogens, which has the smallest electronegativity?

a)

F

b)

Cl

c)

At

d)

Ne

5.

Which of the alkaline-earth metals has the smallest electronegativity

a)

Be

b)

Sc

c)

Ra

d)

Sr

6.

Which of the period 3 elements has the largest electronegativity?

a)

Ar

b)

Cl

c)

Na

d)

F

7.

Which of the transition metals in the 5th period is the largest?

a)

Y

b)

Mo

c)

Rb

d)

Xe

8.
Which has the greater EN: 
Cl or Al?
a)
Cl
b)
Al
9.
Which has the greater EN: 
N or C?
a)
C
b)
N
10.
As atoms of elements in group 16 are considered in order from top to bottom, the electronegativity of each successive element....
a)
decreases
b)
increases
c)
remains the same
d)
none of the above
11.
Electronegativity is...
a)
how good an atom is at attracting electrons
b)
the ability of an atom to lose electrons
c)
the energy required to remove an electron from a specific atom
d)
how easy it is to make friends. 
12.
Atoms that have a high electronegativity, _______________.
a)
give up their electrons more easily.
b)
hold on to their electrons more tightly.
c)
have more electron shells.
13.
As you move across the periodic table atoms tend to get smaller because, ______________.
a)
the atoms have more mass.
b)
the atoms have less mass
c)
the atoms have more protons.
d)
the atoms have less electrons.
14.
As you move down a group, atomic radius increases because - 
a)
you add more and more neutrons
b)
you add more and more protons
c)
you add more and more shells (energy levels)
d)
you add more atomic mass
15.
The atom with the largest atomic radius in Period 4 (row 4) is - 
a)
K
b)
Kr
c)
Fe
d)
Fe
16.
Francium (Fr) has the lowest ionization energy in Group 1 because - 
a)
it has the smallest number of valence electrons
b)
it has the greatest atomic mass
c)
it has the greatest number of protons, so it attracts its electrons the strongest
d)
its 1 valence electron is very far from the nucleus, so little energy is needed to remove it
17.

What is the correct Lewis Dot Structure for ammonia NH3

a)
b)
c)
d)
18.

Which is the correct molecular structure for carbon dioxide?

a)
b)
c)
d)
19.

CO2 has how many lone pairs?

a)

0

b)

1

c)

2

d)

3

e)

4

20.

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

21.

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

22.
How many electrons are in the outer (valence) shell of Chlorine (Cl)?
a)
1
b)
3
c)
6
d)
7
23.
What is this element? 
1s22s22p63s23p6
4s23d104p6
a)
Argon
b)
Krypton
c)
Selenium
d)
Bromide
24.
How many electrons should Lithium have around its Lewis dot model?
a)
1
b)
2
c)
3
d)
4
25.
How many electrons should Silicon have around its Lewis dot model?
a)
1
b)
2
c)
3
d)
4
26.
What is the measure of a tetrahedral bond angle?
a)
90 Degrees
b)
109.5 Degrees
c)
120 Degrees
d)
180 Degrees
27.
Which of the following molecular shapes would have a bond angle of 180 Degrees?
a)
Bent
b)
Trigonal Planar
c)
Tetrahedral
d)
Linear
28.
Which molecule would have this shape?
a)
BF3
b)
CH4
c)
PCl5
d)
CO2
29.
What molecular shape is this? 
a)
Trigonal Planar
b)
Trigonal Bipyramidal
c)
Tetrahedral
d)
Pyramidal
30.
According to the VESPR theory  three electron pairs give a
a)
linear shape
b)
bent shape
c)
trigonal planar shape
d)
tetrahedral shape
31.
What molecular shape is this? 
a)
Trigonal Planar
b)
Trigonal Bipyramidal
c)
Tetrahedral
d)
Pyramidal
32.
Which statement is TRUE, based on the diagram provided?
a)
atomic orbital overlap to produce sigma bond
b)
s orbital overlap to produce π bond
c)
s orbital overlap with s orbital to produce sigma bond
d)
p orbital overlap to produce π bond
33.
Which statement is TRUE, based on the diagram provided?
a)
atomic orbital overlap to produce sigma bond
b)
s orbital overlap to produce π bond
c)
s orbital overlap with s orbital to produce sigma bond
d)
p orbital overlap to produce π bond
34.

When you have Br-Br, what is the polarity?

a)

Polar

b)

nonpolar

c)

Ionic

35.
S
a)
2-
b)
2+
c)
3-
d)
4+
36.
C
a)
4+/4-
b)
0
c)
1+
d)
2-
37.
P
a)
3-
b)
3+
c)
3-
d)
2-
38.
Li
a)
1+
b)
1-
c)
3+
d)
2-
39.
Na
a)
1+
b)
1-
c)
3+
d)
2-
40.

Oxidation number of O in its stable elemental form, O2:

a)

0

b)

-1

c)

-2

d)

+2

41.

Oxidation number of O in the compound H2O2:

a)

0

b)

-1

c)

-2

d)

+2

42.

Oxidation number of H in H2:

a)

0

b)

+1

c)

-1

d)

+2

43.

How many valence electrons do elements in Group 15 have?

a)

15

b)

5

c)

4

44.

How many electrons are required to fill the outer shell for elements in Group 15

a)

15

b)

3

c)

5

45.

How many valence electrons do elements in Group 13 have?

a)

13

b)

5

c)

3

46.
In this image, the information in red is called the_______.
a)
Products
b)
Reactants
c)
Chemical Subscript
d)
Ingredients
47.
Is the following equation balanced or unbalanced ? 
Al + O2 --> Al2O3
a)
Balanced
b)
Unbalanced
48.
Is the following equation balanced or unbalanced ? 
N2 +3 H2 --> 2NH3
a)
Balanced
b)
Unbalanced
49.
What coefficient should be used to make the following equation balanced?
N2+O2--> _NO 
a)
1
b)
2
c)
3
d)
4
50.
At the end of chemical reactions, what is the total mass of the reactants compared to the total mass of the products?
a)
the product is doubled
b)
the product is half the mass of the reactants
c)
the mass is the same
d)
the mass changes depending on the reaction
51.

Balance this equation

(a)  

52.

Fill in the blanks with coefficient:

PCl5+_ H2O→_ HCl+H3PO4

a)

4, 5

b)

1, 6

c)

3, 8

d)

2,2

53.
Balance this equation.
_Mg + _Cl2 --> _MgCl2
a)
1, 2,1
b)
already balanced
c)
2,1,1
d)
1,1,2
54.

Balance this equation, CaCO3(s) → CaO(s) + CO2(g)?

a)

3,1,2

b)

1,1,1

c)

1,3,1

d)

2,6,3

55.

Which one is balanced?

a)

PbO2 + 2H2--> H2SO4

b)

SO2 + H20 --> H2SO4

c)

2Na + 2H2O --> 2NaOH + H2

d)

2Na + 2H2O --> 2NaOH + H

56.

Balance the following equation: Cr(s) + Fe(NO3)2 (ag) → Fe(s) + Cr(NO3)3 (ag)

a)

2,3,3,2

b)

2,3,2,3

c)

4,6,6,2

d)

1,3,3,1

57.
How many atoms of aluminum are on each side of the following equation: 4Al + 3O2 --> 2Al2 O3
a)
2
b)
6
c)
1
d)
4
58.
Which number should go in the blank?
2 Na+ _ Cl2 -> 2 NaCl
a)
1
b)
2
c)
3
d)
0
59.

Which of the following statements regarding the mole is INCORRECT?

a)

A mole is a unit of quantity equal to 6.02 x 1023 particles.

b)

The number of particles in a mole is known as Avogadro’s number.

c)

A mole of particles of an element is numerically equal to the atomic mass of the element.

d)

none of the above

60.

The mass of one mole of an element is equal to

a)

its atomic number from the periodic table, but in amus.

b)

its atomic mass from the periodic table, but in amus.

c)

its atomic mass from the periodic table, but in grams.

d)

its atomic number from the periodic table, but in grams.

61.
How many molecules are there in 31.8 moles of water?
a)
5.28 x 10-23 molecules
b)
1.91 x 1025 molecules
c)
5.28x 10-25
d)
1.91 x 1022
62.

Shivani measures out 6.0 moles of epsom salt (MgSO4) to put in her bath. How many grams of MgSO4 went in the bath?

a)

3.6 x 1024 g

b)

720 g

c)

0.050 g

d)

340 g

63.

Determine the mass of 4.20 moles of C6H12

a)

353 g

b)

0.0499 g

c)

337 g

d)

2.53 x 1024 g

64.

Which of the following dimensional analysis setups will correctly convert 27.76 g of Li to atoms of Li?

a)

A

b)

B

c)

C

d)

D

65.
How many moles are in 4.5x1024 particles?
a)
0.747 particles
b)
0.747 mol
c)
2.71x1047 mol
d)
2.71x1047 particles
66.
What is the molar mass of Mg3N2?
a)
191.6 g/mol
b)
76.64 g/mol
c)
38.32 g/mol
d)
100.95 g/mol
67.
What is the mass of one mole of Al2(SO4)3?
a)
75.04 g
b)
342.14 g 
c)
75.04 mol
d)
342.14 mol
68.
How many molecules are there in 5.9 moles of NaCl?
a)
3.5x1024molecules
b)
9.79x10-24molecules
c)
1.02x1023molecules
69.
How many moles of carbon atoms are there in 5g of carbon?
a)
60 mol
b)
17 mol
c)
0.42 mol
d)
7 mol
70.
How many molecules are present in 69.0 moles of SrO?
a)
4.16x1025molecules
b)
8.72x1021molecules
c)
7,149.78 molecules
d)
6,893.32 molecules
71.
Mass of one mole of CO2
a)
44
b)
44g
c)
28
d)
28g
72.
What is the mass of 54.3x1045molecules of BeO?
a)
3.27x1070 g
b)
9.01 x1022g
c)
2.25 x1024 g
d)
1.31 x1069g
73.
How many molecules are present in 25 g of NaBr?
a)
102.96 molecules
b)
0.24 molecules
c)
1.45x1023 molecules
d)
2.34 x 1020molecules
74.
In chemistry, a "mole" is:
a)
The mass of an atom
b)
a large number used to count particles
c)
based on the volume of a substance
75.
How many atoms of iodine are in a mole of iodine?
a)
53
b)
63.55g
c)
126.9
d)
6.02 x 1023
76.
The number 6.02 x 1023 is called...
a)
Obama's number
b)
Bohr's number
c)
Trump's number
d)
Avogadro's number
77.
How many particles would be in 8.4 moles of Octane (C8H18)?
a)
5.77 x 1023
b)
5.04 x 1024
c)
5.77 x 1026
d)
5.04 x 1023
78.

How many molecules are there in 5.5 moles potassium chloride?

a)

4.08 x 10-24

b)

3.31 x 1024

c)

33.11

d)

0.98

79.
How many students are there in 31.8 moles of students?
a)
5.28 x 10-23 students
b)
1.91 x 1025 students
c)
5.28x 10-25  students
d)
1.91 x 1022 students
80.
How many moles of copper are 4.57 x 1015 atoms of copper?
a)
7.59 x 10-9 moles
b)
2.75 x 10-33 moles
c)
7.59 x 109 moles
d)
2.75 x 1033 moles
81.
Convert 1.5 moles of beryllium oxide to molecules
a)
25.01 molecules
b)
9.0 x 1023 molecules
c)
0.12 molecules
d)
1.80 x 1024 molecules
82.
Which list of number of atoms in Mg(NO2)2 is right?
a)
Mg : 1--NO :  2
b)
Mg : 1-- N :  6--O:  2
c)
Mg :  1-- N:   1--  O: 2
d)
Mg :  1-- N: 2--  O: 4
83.
2H2   +   O2  →  2H2O
How many moles of water can be produced if 8 moles H2 are used?
a)
4 moles
b)
8 moles
c)
16 moles
d)
2 moles
84.
What is the first thing you must do to solve a stoichiometry problem?
a)
Write a Balanced Equation
b)
Panic
c)
Write an Unbalanced Equation
d)
Ask for help
85.
2H2  +   O2  →  2H2O
How many moles of oxygen are consumed if 8 moles H2 are used?
a)
2
b)
4
c)
6
d)
8
86.
B2H6 + 3O2 -->2 HBO2 + 2 H2O
 What mass of O2 will be needed to burn 36.1 g of B2H6?
a)
13.8 g O2
b)
3.86 mol of O2
c)
124 g O2
87.
2Na + 2H2O → 2NaOH+ H2
How many grams of hydrogen are produced if 120 g of Na are available?
a)
5.2 g
b)
2.6 g
c)
690 g
d)
45 g
88.
4 Al + 3 O2 –> 2 Al2O3  How much aluminum would be needed to completely react with 45 grams of O2?
a)
1.05 moles
b)
3.75 moles
c)
1.875 grams
d)
1.875 moles
89.
Electrons move around _______________ the nucleus and have a negative charge.
a)
inside
b)
outside
c)
on top of
d)
without
90.
The center of an atom is called the______________.
a)
middle
b)
top
c)
nucleus
d)
electron
91.
The atomic number determines_____________________.
a)
its symbol
b)
the number of protons and neutrons
c)
what the element is
d)
the number of protons in the atom
92.
If an atom has 5 protons and 3 neutrons, what is its atomic number?
a)
5
b)
2
c)
8
d)
0
93.
What are the 2 parts of the nucleus?
a)
protons and electrons
b)
protons and neutrons
c)
particles and molecules
d)
protons and mass
94.

What is the symbol for helium?

a)

Hy

b)

H

c)

He

d)

Ho

95.

What is the symbol for lithium?

a)

L

b)

Lt

c)

Li

d)

Lr

96.
mercury
a)
He
b)
Me
c)
Hg
d)
My
97.

Which one is correct about mendeleev's periodic law

a)

Properties of elements are periodic function of their atomic mass

b)

the physical and chemical properties of elements are periodic function of their atomic number.

c)

physical properties of elements are periodic function of their atomic weight.

d)

chemical properties of elements are periodic function of their atomic number.

98.

who discovered the first scientific and systematic periodic table

a)

Henry Mosley

b)

Dmitri Mendeleev

c)

John Dalton

d)

sir Isaac Newton

99.

Number of valence electrons in halogens is ..........

a)

1

b)

4

c)

3

d)

7

100.

D block elements are known as .............

a)

Actinides

b)

Transition elements

c)

Lanthanides

d)

Noble gases

101.

alkali metals are kept in ........

a)

IIA

b)

IIIA

c)

IA

d)

0

102.

The vertical (up and down) columns in the Periodic Table are called

a)

groups

b)

towers

c)

periods

d)

atomic numbers

103.
Sodium (Na) is found in period 
a)
3
b)
2
c)
4
d)
1
104.

The positive ions tend to _____________ electrons.

a)

lose

b)

gain

105.
Why do elements bond?
a)
To be friends
b)
To create a new element
c)
To become stable
106.
Name the following compound: 
N2O4
a)
dinitrogren tetraoxide
b)
tetranitrogen dioxide
c)
nitrogen oxide
d)
dinitrogen tetraoxygen
107.
Name the following compound: 
CO2
a)
monocarbon dioxide
b)
carbon oxide
c)
carbon dioxide
d)
oxygen carbonide
108.
Name the following compound: 
CCl4
a)
monocarbon quadchloride
b)
carbon tetrachloride
c)
carbon chloride
d)
monocarbon quadchloide
109.
Name the following compound: 
N2O4
a)
dinitrogren tetraoxide
b)
tetranitrogen dioxide
c)
nitrogen oxide
d)
dinitrogen tetraoxygen
110.
Name the following compound:
H2O
a)
hydrogen oxide
b)
dihydrogen oxide
c)
trihydroxide
d)
dihydrogen monoxide
111.
Write the formula for:
dinitrogen tetroxide
a)
N2O4
b)
NO2
c)
NO
d)
N4O8
112.
Write the formula for:
dinitrogen pentoxide
a)
NO
b)
N2O5
c)
2NO5
d)
O5N
113.
a)

10

b)

2

c)

1

114.
a)

4

b)

5

c)

7

115.
What is the negative subatomic particle that orbits the nucleus
a)
Proton
b)
Neutron
c)
Electron
d)
Voltron
116.
What is the subatomic particle that gives the nucleus its positive charge?
a)
Proton
b)
Neutron
c)
Electron
d)
Galvatron
117.

Which type of chemical reaction has two or more reactants to make one product?

a)

combustion

b)

single displacement

c)

double displacement

d)

synthesis

e)

decomposition

118.

Identify the following chemical reaction.

2 NaBr + 1 Ca(OH)2 ----> 1 CaBr2 + 2 NaOH

a)

Synthesis (or combination)

b)

Decomposition

c)

Single displacement

d)

Double displacement

119.

What reaction has the following general formula:

A + CD --> C + AD

a)

Combination

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

e)

Combustion

120.

What reaction has the following general formula:

AB + CD --> CB + AD

a)

Combination

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

e)

Combustion

121.

Which of the following is a compound?

a)

zinc (Zn)

b)

magnesium (Mg)

c)

sodium chloride (NaCl)

d)

potassium (K)

122.

Which of the following is an element?

a)

potassium chloride (KCl)

b)

water (H2O)

c)

carbon (C)

d)

calcium carbonate (CaCO3)

123.
Combining substances to form a new substance
a)
Displacement
b)
Synthesis
c)
Decomposition
d)
Oxidation
124.
Breaking down a substance into simpler substances
a)
Displacement
b)
Synthesis
c)
Decomposition
d)
Oxidation
125.
Switching one substance for another
a)
Displacement
b)
Synthesis
c)
Decomposition
d)
Oxidation
126.

1) What type of chemical reaction is represented?

________Some represent 2 types_________


___ KClO3 --> ___ KCl + ___ O2

a)

single replacement

b)

double replacement

c)

combustion

d)

decomposition

e)

synthesis

127.

2) What type of chemical reaction is represented?

________Some represent 2 types_________


_____ Ca + _____ N2 --> _____ Ca3N2

a)

single replacement

b)

double replacement

c)

combustion

d)

decomposition

e)

synthesis

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