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2nd Semester Review

Total questions: 147

Worksheet time: 3hrs 20mins

Name
Class
Date
1.

On the periodic table, Groups are

a)

Horizontal rows

b)

Vertical columns

2.

On the periodic table, Periods are

a)

Horizontal rows

b)

Vertical columns

3.

What is a valence electron?

a)

Electrons in the first energy shell

b)

Electrons in the second energy shell

c)

Electrons in the outer shell

d)

Total number of electrons

4.

What does the Bohr Model represent?

a)

The structure of molecules

b)

The structure of the Solar System

c)

The structure of an atom

d)

The structure of East Hills

5.

Which element is this?

a)

Nickel

b)

Neon

c)

Sodium

d)

Nitrogen

6.

Name this element.

a)

Argon

b)

Chlorine

c)

Aluminum

d)

Boron

7.

Name this element.

a)

Neon

b)

Magnesium

c)

Sodium

d)

Manganese

8.

What is the atomic number of this atom?

a)

2

b)

4

c)

6

d)

8

9.

What is the mass number of this atom?

a)

1

b)

3

c)

4

d)

7

10.

The nucleus of an atom contains which subatomic particles?

a)

protons and electrons

b)

protons and neutrons

c)

electrons and neutrons

d)

protons, electrons, and neutrons

11.

Typically in an atom, which two subatomic particles are equal in number?

a)

protons and neutrons

b)

all subatomic particles are equal in number

c)

neutrons and electrons

d)

protons and electrons

12.
Particles in an atom that are neutral and have no charge are 
a)
negatrons 
b)
electrons 
c)
neutrons 
d)
protons 
13.

How many neutron are in the atom "K"?

a)

29

b)

19

c)

58

d)

20

14.
The atomic number is equal to _.
a)
the number of protons and electrons
b)
the number of neutrons only
c)
the total number of protons and neutrons
d)
the number of protons neutrons and electrons
15.
The atomic mass is equal to _.
a)
the number of protons only
b)
the number of neutrons only
c)
the total number of protons and neutrons
d)
the number of protons, neutrons, and electrons.
16.
An atom becomes _________ when it gains electrons.
a)
Positive
b)
Negative
c)
Neutral
d)
Invinsible
17.
An atom that has gained or lost electrons is called ...
a)
a winner
b)
an isotope
c)
an ion
d)
a loser
18.

When an atom loses an electron, it becomes a

a)

positive ion

b)

negative ion

c)

neutral ion

d)

neutral atom

19.

What is the center of an atom called?

a)

The headquarters

b)

The centrometer

c)

The hypothesis

d)

The nucleus

20.
How many electrons does a Copper atom have?
a)
63
b)
29
c)
92
d)
34
21.
How many electrons does an atom of Krypton have?
a)
36
b)
83.80
c)
47.80
d)
119.80
22.
How many neutrons does a Hydrogen atom have?
a)
1
b)
2
c)
3
d)
0
23.
How many protons are present in phosphorus-31
a)
15
b)
16
c)
31
d)
46
24.
What is the atomic number for an element with 41 neutrons and a mass number of 80?
a)
39
b)
41
c)
80
d)
121
25.
Atomic mass - Atomic Number =
a)
protons
b)
neutrons
c)
electrons
d)
Average Mass
26.
Most of an atom's mass is found in the
a)
electrons.
b)
nucleus.
27.

What did Dmitri invent?

a)

book

b)

Periodic Table

c)

Russian currency

d)

Calculator

28.

The subatomic particles are called:

a)

protons, nucleus and electrons

b)

protons, electrons and neutrons

c)

protons, positives and negatives

d)

cloud, shell and quarks

29.

Who invented the simplified version of the atom?

a)

Dmitri Mendeleev

b)

Niels Bohr

c)

Sir Isaac Newton

d)

Albert Einstein

30.

Dmitri had an element named after him

True of False?

a)

True

b)

False

31.

What is the name of group number 1?

a)

halogens

b)

noble gases

c)

alkali metals

d)

alkaline earth metals

32.

What is the name of group number 2?

a)

transition metals

b)

halogens

c)

metaloids

d)

alkaline earth metals

33.

where are the metaloids found

a)

far left, vertical

b)

stair step/diagonal

c)

far right horizontal

d)

at the bottom

34.

What group number are the halogens found?

a)

18 (8A)

b)

1

c)

2

d)

17 (7A)

35.

Periodic law states that the elements are arranged according to their atomic ________ so that elements with similar chemical properties are in the same ________ and properties repeat periodically.

a)

numbers, rows

b)

masses, rows

c)

masses, column

d)

numbers, column

36.

Which element is found in group 2, period 6?

a)

Oxygen (O)

b)

Barium (Ba)

c)

Selenium (Se)

d)

Carbon (C)

37.

Which halogen is found in period 4?

a)

Krypton (Kr)

b)

Xenon (Xe)

c)

Bromine (Br)

d)

Iodine (I)

38.

Find this family: This family contains nitrogen and phosphorus.

a)
b)
c)
d)
39.
Which of the following atomic symbols for bromine is written correctly?
a)
bR
b)
BR
c)
Br
d)
br
40.

Zinc fluoride

a)

ZnF2

b)

Zn2F

c)

ZnF

d)

Zn2F4

41.

How many Aluminum atoms are in Al2O3?

a)

3

b)

5

c)

2

d)

1

42.

Write the correct formula for Sodium Chloride.

a)

SC

b)

SCl

c)

NaCl

d)

NaCl2

43.

Mg3N2

a)

Magnesium nitride

b)

Magnesium (II) nitride

c)

Trimagnesium dinitrogen

44.

What two types of atoms make a covalent bond?

a)

2 Nonmetals

b)

1 Metal and 1 Nonmetal

c)

2 Metals

d)

2 Noble Gases

45.

Ionic Bonds

a)

metal with nonmetal

b)

nonmetal with nonmetal

46.

Covalent Bonds

a)

metal with nonmetal

b)

nonmetal with nonmetal

47.

CaCl

a)

Ionic Bond

b)

Covalent Bond

48.

NH3

a)

Ionic Bond

b)

Covalent Bond

49.

NaO

a)

Ionic Bond

b)

Covalent Bond

50.
Atoms are most stable when their outer shell is complete.
a)
true
b)
false
51.
Covalent bonds actually "share" electrons?
a)
true
b)
false
52.
How are ionic bonds formed?
a)
Transfer of electrons
b)
Sharing of electrons
53.

Where are metals located on the periodic table?

a)

Blue (left)

b)

Green (middle)

c)

Red (right)

54.

Where are the nonmetals located on the periodic table?

a)

Blue left

b)

Red right

c)

Green middle

55.

Where are the metalloids located on the periodic table?

a)

Blue left

b)

Red right

c)

Green middle

56.
What is the name of NF3?
a)
mononitrogen trifluoride
b)
nitrogen trifluoride
c)
nitrogen flouride
d)
nitrogen fluorine 
57.
What is the name for CO?
a)
Copper Oxide
b)
Carbon monoxide
c)
monocarbon oxide
d)
Copper monoxide
58.
What is the formula for sulfur pentoxide?
a)
SO2
b)
SO3
c)
SO4
d)
SO5
59.

Which of the following is an ionic compound?

a)

CO2

b)

SiO2

c)

ZnF

d)

N2O4

60.

This could be the dot diagram of

a)

Mg

b)

Cl

c)

C

d)

O

61.
This could be the dot diagram of
a)
Mg
b)
Cl
c)
C
d)
O
62.

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

63.

Which of these is correct?

a)
b)
c)
64.

Which of these is incorrect?

a)
b)
65.
According to the octet rule most elements need _______ valence electrons.
a)
2
b)
8
c)
6
d)
18
66.

What percentage of the total atomic mass of magnesium bromide (MgBr2) is composed of magnesium?

a)

13%

b)

43%

c)

63%

d)

87%

67.
What is the mass of one mole of aluminum chloride (remember to determine the correct formula first)?
a)
62.435g
b)
116.399g
c)
133.341g
d)
97.888g
68.

What id the molar mass of UF6?

a)

101 g/mol

b)

238 g/mol

c)

257 g/mol

d)

352 g/mol

69.

Find the percent composition of cuprous sulfide?

a)
%Cu= 67.987 %S= 32.013
b)
%Cu= 79.854   %S= 20.145
c)
%Cu= 35.946   %S= 64.054
70.

An element sample is 44% Zinc. If the sample has a mass of 5.0 g, what the mass of the Zinc in the sample?

a)

5.0 g

b)

220 g

c)

2.2 g

d)

There is no Zinc

71.

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


(a)  
Choose from the below words
Cation
Metal
Nonmetal
Anion
72.

Which two elements would NOT form an ionic bond?

a)

calcium and lithium

b)

calcium and oxygen

c)

lithium and oxygen

d)

calcium and carbon

73.

LiBr is called


(a)  
Choose from the below words
lithium bromide
lithium bromine
lithium(I) bromine
lithuim(I) bromide
74.

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

a)

Sodium sulfate

b)

Sodium sulfide

c)

Sodium sulfite

d)

Sodium sulfuroxide

75.

What is the name of the following compound: NaCl

a)

sodium chloride

b)

sodium(I) chloride

c)

sodium chlorine

d)

sodium(I) chlorine

76.
How do the following two elements bond together?
Al3+  O2-         
a)
AlO
b)
Al2O3
c)
Al3O6
d)
Al3O2
77.

Compounds made from only nonmetals are (a)   compounds.

78.

Match the following prefixes with the correct number

a)

Hexa

1.

6

b)

Hepta

2.

7

c)

Nona

3.

9

d)

Tetra

4.

4

e)

Deca

5.

10

79.

What is the prefix for the number 5 ?

a)

tetra-

b)

penta-

c)

hexa-

d)

hepta-

80.
In the compound TiO2, titanium has a charge of
a)
4+
b)
2+
c)
2-
d)
4-
81.
Name the following compound: FeCl3
a)
iron chloride
b)
iron III chloride
c)
iron chlorate
d)
iron III chlorate
82.
Write the formula for copper (I) phosphide
a)
Cu3P
b)
CuP
c)
Cu1P
d)
CuP3
83.

Which of the following is the correct name for NiF2?

a)

Nickel (I) fluoride

b)

Nickel (II) fluoride

c)

Nickel (III) fluoride

d)

Nickel (IV) fluoride

84.

What is the formula for phosphorous acid?

(a)  

85.

What is the formula for nitric acid?

(a)  

86.
What is the formula for perchloric acid?
a)
H3ClO3
b)
H3ClO4
c)
HClO3
d)
HClO4
87.
HBr
a)
hydrogen bromine acid
b)
hydrobromide acid
c)
hydrobromic acid
88.

When naming oxyacids, change "-ite" to:

a)

-ate

b)

-ic

c)

-ous

d)

-ite

89.

Name this acid: H2SO4

a)

hydrogen sulfate

b)

hydrosulfuric acid

c)

sulfuric acid

d)

sulfurous acid

90.

What is the correct classic name for Sn2+

a)

plumbous

b)

stannous

c)

Stannic

d)

Plumbic

91.

C6H12O9

a)

molecular

b)

empirical

92.

What is the empirical formula for:

Mg8Si4O16

a)

MgSiO

b)

Mg2SiO4

c)

Mg4Si2O8

d)

Mg2O

93.

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

94.

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

95.
What is the molecular formula if the empirical formula is CH2O and the molecular molar mass is 180.18?
a)
CH2O
b)
C2H4O2
c)
C4H8O4
d)
C6H12O6
96.

Determine the oxidation number of phosphorus in the molecule H3PO4.

a)

+5

b)

-5

c)

+3

d)

-3

97.

A wave with a large wavelength will have...

a)

Low Frequency & Low Energy

b)

High Frequency & High Energy

c)

High Frequency & Low Energy

d)

Low Frequency & High Energy

98.

Which has the LONGEST wavelength and therefore the lowest frequency/energy? These waves are used in broadcasting, wifi, and texting.

a)

Gamma rays

b)

Visible light

c)

Radio waves

d)

Infrared rays

99.

How much of the electromagnetic spectrum is made up of visible light?

a)

A small portion of it

b)

Most of it

c)

All of it

d)

None of it

100.

A wave has a frequency of 5 hz and a wave length of 5 m. What is the wave speed (velocity)?

a)

25 m/s

b)

1 m/s

c)

10 m/s

d)

0 m/s

101.
Which letter is a crest?
a)
F
b)
G
c)
H
d)
J
102.
Frequency is measured in
a)
Newtons
b)
Joules
c)
Hertz
d)
Decibels
103.

What is the wavelength of a 2.99 Hz wave?

a)

1.00 x 10^8 m

b)

5.99 x 10^9 m

c)

9.97 x 10^8 m

d)

1.00 m

104.

What is the frequency of a 6.9 x 10^-13 m wave?

a)

2.07 x 10^19 Hz

b)

0.434 x 10^-5 Hz

c)

2.30 x 10^-21 Hz

d)

4.35 x 10^20 Hz

105.
What does the nucleus of an atom contain?
a)
Electrons and neutrons
b)
Protons and neutrons
c)
Neutrinos and positrons
d)
Electrons and megatrons
106.

Match the elements with their electron configuration! (3 minutes)

a)

1s2 2s2p3

1.

Nitrogen, N

b)

1s2 2s2p6 3s2p3

2.

Phosphorus, P

c)

1s2

3.

Helium, He

d)

1s2 2s2p6 3s2p6

4.

Argon, Ar

e)

1s2 2s2p6 3s2p6 d54s2

5.

Manganese, Mn

107.

Each orbital can hold how many electrons?

a)

5

b)

4

c)

8

d)

2

108.
There are 4 different types of subshells (orbitals) s,p,d,f.
a)
true
b)
false
109.

How many electrons can a p orbital hold?

a)

6

b)

10

c)

8

d)

14

110.
[Ne]3s23p5 is the noble gas configuration for which element?
a)
chlorine
b)
fluorine
c)
sulfur
d)
aluminum
111.
Which orbital shows a violation of Hund's Rule?
a)
A
b)
B
c)
C
d)
D
112.
Which orbital shows a violation of the Pauli Exclusion Principle?
a)
A
b)
B
c)
C
d)
D
113.

What is the noble gas notation for V?

a)

[Ar] 4s2p2

b)

[Kr] 3d34s2

c)

[Ar] 4s2 4d3

d)

[Ar] 3d34s2

114.

What is the missing piece?

1s2 2s2 ___ 3s1

a)

2p6

b)

2p4

c)

3p6

d)

3s2

115.

What are the missing pieces?

1s2 2s2 2p6 ___ 3p6 4s2 ___ 4p2

a)

3s2 , 4d10

b)

2p4 , 3d10

c)

3p6 , 3d10

d)

3s2 , 3d10

116.
Which guideline, Hund’s rule or the Pauli exclusion principle, is violated in the following orbital diagrams?
a)
Hund's
b)
Aufbau's
c)
Pauli's Exclusive
117.

2 rows beneath the main periodic table

a)

Lanthanide

b)

Lanthanide and Actinide

c)

Lanthanide and Hydrogen

d)

Actinide and Hydrogen

118.

True or False:

Mendeleev was the only person working on organizing elements into a table.

a)

True

b)

False

119.
Which element is a metalloid?
a)
Titanium
b)
Selenium
c)
Potassium
d)
Polonium
120.

Where are the valence electrons located?

1s22s22p63s2p3

a)

2s22p6

b)

1s22s2

c)

2p63s2

d)

3s2p3

121.

How many valence electrons are present?

1s22s22p63s23p63d104s2

a)

2

b)

8

c)

12

d)

8

122.
Define electron affinity.
a)
The energy it takes to add an electron to an atom.
b)
The energy it takes to remove an electron from an atom.
123.
Elements closer to the noble gases have stronger attraction for electrons.
a)
True
b)
False
124.
Which one has the largest radius?
a)
Lithium (Li, atomic #3)
b)
Boron (B, atomic #5)
c)
Neon (Ne, atomic #10)
d)
Nitrogen (N, atomic #7)
125.

When the atomic radius increases, electron affinity

a)

Decreases

b)

Increases

c)

Neutral

d)

No effect

126.

Which of the following has the most electron affinity?

a)

nitrogen

b)

phosphorus

c)

arsenic

d)

lithium

127.
As you move down the periodic table atoms get bigger.  This is because ____________.
a)
The atoms have more mass.
b)
The atoms have more protons.
c)
The atoms have more energy levels
d)
The atoms have more nuetrons
128.
Which of the following will have a lower ionization energy than Scandium (Sc)?
a)
Helium (He)
b)
Titanium (Ti)
c)
Calcium (Ca)
d)
Magnesium (Mg)
129.

Which element is found in group 2, period 6?

a)

Oxygen (O)

b)

Barium (Ba)

c)

Selenium (Se)

d)

Carbon (C)

130.

Name this group: These metals contain familiar metals such as gold, iron, and copper.

a)
b)
c)
d)
131.

How many electrons can be found on the 3rd ring?

a)

Up to 1

b)

Up to 2

c)

Up to 8

d)

Up to 16

132.

Is Silicon (Si) a metal, nonmetal, or metalloid?

a)

metal

b)

nonmetal

c)

metalloid

133.

Which element has the greatest electronegativity?

a)

I

b)

Br

c)

Cl

d)

F

134.

What is the electronegativity difference of HFHF  ?

(a)  

135.

What must the difference in electronegativity between two atoms be in order for the bond between them to be polar covalent?

a)

less than 0.3

b)

greater than 1.7

c)

between 0.3 and 1.7

d)

exactly 0

136.

What is the electronegativity difference of LiFLiF  ?

(a)  

137.

What type of bond does H2H_2   form?

a)

Non-polar covalent

b)

polar covalent

c)

ionic

138.

What is the electron difference of Hydrochloric acid (HCl)?

a)

0.5

b)

0.8

c)

1.7

139.

As atoms bond with each other, they

a)

increase their potential energy, thus creating less-stable arrangements of matter.

b)

decrease their potential energy, thus creating less-stable arrangements of matter.

c)

increase their potential energy, thus creating more-stable arrangements of matter.

d)

decrease their potential energy, thus creating more-stable arrangements of matter.

140.

If two covalently bonded atoms are identical, the bond is

a)

nonpolar covalent

b)

polar covalent

c)

dipole covalent

d)

coordinate covalent

141.

A bond that is less than 25% ionic is considered

a)

polar covalent

b)

ionic

c)

nonpolar covalent

d)

metallic

142.

The electron configuration of nitrogen is 1s22s2p3. How many more electrons does nitrogen need to have to satisfy the octet rule?

a)

1

b)

3

c)

5

d)

8

143.

The substance whose Lewis structure shows three covalent bonds is

a)

H2O

b)

CH2Cl2

c)

NH3

d)

CCl4

144.

The lattice energy is a measure of the

a)

strength of an ionic bond

b)

strength of a metalllic bond

c)

strength of a covalent bond

d)

net charge on a crystal

145.

What is the correct structural formula?

a)

b)

c)

d)

146.

Which of the following is NOT an example of a molecular formula?

a)

NH3

b)

O2

c)

MgO

d)

H2O

147.

NH3 has how many lone pairs?

a)

0

b)

1

c)

2

d)

3

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