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Chemistry Semester 2

Total questions: 106

Worksheet time: 8hrs 27mins

Name
Class
Date
1.

Match the expressions to their resulting units.

a)
1.

yards

b)
2.

centimeters

c)
3.

kilometers

d)
4.

meters

e)
5.

inches

2.

How many inches are in 1 mile? (5280ft = 1mi; 12in = 1ft)

a)

66330in

b)

63360in

c)

63660in

d)

63066in

3.

How many hours are in 2 weeks?

1 week = 7 days; 1 day = 24 hours [Note: do not round answer]

a)

672 hours

b)

168 hours

c)

336 hours

d)

504 hours

4.

Jonathan raised 60 goats, then he traded all the goats for sheep at an exchange rate of 5 goats for 7 sheep. Next, he exchanged all the sheep for hogs at a rate of 4 sheep for 2 hogs. How many hogs did he get?

a)

62 hogs

b)

42 hogs

c)

84 hogs

d)

86 hogs

5.

You roof has a leak. If it leaks at a rate of 14 drops per minute, how many hours will it take to fill a 5 gallon bucket? (20 drops = 1 mL; 30 mL = 1oz; 64 oz = 1 gal) [Round answer to 2 sig figs]

a)

230 hours

b)

950 hours

c)

190 hours

d)

1900 hours

6.
The smallest particle of an element that still retains all the properties of that element. 
a)
atom
b)
cathode ray
c)
electron
d)
compound
7.
Atoms of different elements are exactly alike
a)
Always true
b)
Always false
c)
Sometimes true
8.
Electrons can be found in
a)
The protons
b)
The nucleus
c)
Electron Clouds
d)
exact locations
9.
This particle is found in the nucleus and has no charge.
a)
Neutron
b)
Proton
c)
Electron
d)
quark
10.
This contains most of the mass of an atom
a)
Electron Cloud
b)
Nucleus
c)
Electron
11.
An atom's overall charge is ________.
a)
positive 
b)
depends
c)
neutral 
d)
negative 
12.

What is Neils Bohr's contribution to the atomic theory?

a)

Created the atomic theory

b)

Created a model of the atom with electrons moving around the nucleus in a fixed orbits

c)

Discovered that the proton had a positive charge

d)

Believed that atoms of a given element are identical

e)

Discovered the electron

13.
What is the mass number of this atom?
a)
1
b)
3
c)
4
d)
7
14.
What is the atomic number of this atom?
a)
2
b)
4
c)
6
d)
none of the above
15.
How many valence electrons?
a)
2
b)
3
c)
5
d)
10
16.
Isotopes are elements with a different amount of
a)
protons
b)
neutrons
c)
electrons
d)
atoms
17.
What does the nucleus of an atom contain?
a)
Electrons and neutrons
b)
Protons and neutrons
c)
Neutrinos and positrons
d)
Electrons and megatrons
18.
How many neutrons does the an element with an atomic number of 3 and a mass of 6.9 contain?
a)
6.9
b)
4
c)
3
d)
7
19.
Ions are: 
a)
atoms with a positive or negative charge
b)
atoms with no charge
c)
atoms with ONLY a positive charge
d)
atoms with ONLY a negative charge
20.
How are electrons arranged in an atom?
a)
In groups of five
b)
In energy levels
c)
By color
d)
By shape
21.

What group is carbon (C) in?

a)

1

b)

2

c)

13

d)

14

e)

15

22.

What causes the increase in reactivity in an alkli metal?

a)

The increase in protons

b)

The decrease in protons

c)

The increase in atom size

d)

The decrease in atom size

23.

Are the alkline earth metals more or less reactive than the alkali metals

a)

More

b)

Less

24.

Where are the transition metals located

a)

Left side of table

b)

Top of table

c)

middle of table

d)

right side of table

25.

Why are halogens so reactive

a)

Need 7 valence electrons

b)

Need to lose 1 electron to be stable

c)

Need to add 1 electron to be stable

d)

They are super large atoms

26.

Why are noble gases not reactive

a)

Too few electrons

b)

Too many electrons

c)

They have a full set of electrons

d)

They need more electrons

27.

Which elements have properties in common (also why they are also called families)?

a)

elements in a group

b)

elements in a period

28.

Which elements have a full set of valence electrons?

a)

period 1

b)

group 1

c)

period 18

d)

group 18

29.

How many electrons does Na1+ have?

a)

9

b)

10

c)

11

d)

12

30.

How many electrons does O2- have

a)

6

b)

8

c)

10

d)

12

31.

How many electrons does C need to complete the octet rule?

a)

1

b)

2

c)

3

d)

4

e)

5

32.

What is the electron configuration for Krypton?

a)

1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6

b)

[Ar] 4s2 3d10 4p6

c)

1s2 2s2 3s2 2p6 4s2 3p6 4p6 3d10

d)

[Ne] 4s2 3d10 4p6

33.

Each row on the periodic table represents:

a)

an energy level

b)

a sublevel

c)

an electron

d)

an orbital

34.
There are 4 different types of subshells (orbitals) s,p,d,f.
a)
true
b)
false
35.
Identify the element in Period 5 that has 1 valence electron?
a)
Rb
b)
Nb
c)
Ag
d)
Sb
36.
What atom matches this electron configuration?
1s2 2s2 2p6 3s2
a)
Neon
b)
Magnesium
c)
Aluminum
d)
Potassium
37.
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
38.
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
39.
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
40.

An element's electron configuration and number of valence electrons can be determined by its ______.

a)

atomic mass

b)

position on the periodic table

c)

melting and boiling points

d)

chemical symbol

41.

What is ionization energy?

a)

The energy required to remove an electron from a neutral atom of an element.

b)

The energy change that occurs when an electron is acquired by a neutral atom.

c)

The measure of the ability of an atom in a chemical compound to attract electrons from another atom in the compound.

d)

How close an atom is to its neighboring atom.

42.

When an atom loses an electron, it becomes a __________, and when an atom gains an electron, it becomes a __________.

a)

positive ion, negative ion

b)

negative ion, positive ion

c)

neutral ion, positive ion

d)

neutral atom, negative ion

43.

The is family has properties of both metals and nonmetals.

a)

Alkali

b)

Halogens

c)

Nonmetals

d)

Metalloids

44.

This type of element is dull, brittle solids and gases, insulators, poor conductors of heat and electricity, as well as having low melting points.

a)

metals

b)

metalloids

c)

nonmetals

45.
Which group contains elements that are inert?
a)
1
b)
2
c)
17
d)
18
46.
This class of elements are sometimes called "semiconductors."
a)
Metals
b)
Nonmetals
c)
Metalloids
d)
Groups
47.

This could be the dot diagram of

a)

Mg

b)

Cl

c)

C

d)

O

48.

What is the goal of the Lewis Dot Structure?

a)

To determine the electron position.

b)

To show the element's valence electrons & bonding capabilities.

c)

To find the atomic mass of an element.

d)

To search for the number of electrons in an individual atom.

49.

How many valence electrons should Magnesium have in its Lewis dot model?

a)

1

b)

2

c)

3

d)

4

50.

This is a correct dot diagram for neon (Ne)

a)

true

b)

false

51.
How many valence electrons does chlorine (Cl) have?
a)
2
b)
5
c)
6
d)
7
52.
Which of the following is the correct Lewis structure for the compound PBr3?
a)
structure A
b)
structure B
c)
structure C
d)
structure D
53.
What is the correct formula for this molecule?
a)
NH
b)
N3H
c)
NH3
d)
NH4
54.
According to the octet rule most elements need _______ valence electrons.
a)
2
b)
8
c)
6
d)
18
55.
What type of bond occurs between a metal and a non-metal element?
a)
Ionic
b)
Covalent
c)
Metallic
d)
Sliding-Pair
56.
What type of bond occurs when two or more elements share electrons?
a)
Ionic
b)
Covalent
c)
Metallic
d)
Caring
57.
What type of bond is illustrated above?
a)
Metallic
b)
Ionic
c)
Covalent
d)
Wiggly
58.
Which formula represents an ionic compound?
a)
CaCl2
b)
CH3OH
c)
CH4
d)
H2
59.
Which formula represents an covalent compound?
a)
CO2
b)
Ag
c)
FeCl3
d)
Cs3P
60.

Valence electrons are shared

a)

Ionic bonds

b)

Covalent bonds

61.

Valence electrons are transferred

a)

Ionic bonds

b)

Covalent bonds

62.

If an atom loses two electrons what charge will it have?

a)

-1

b)

-2

c)

+1

d)

+2

63.

Anions

a)

Gain electrons, has an overall positive charge

b)

Lose electrons, has an overall positive charge

c)

Lose electrons, has an overall negative charge

d)

Gain electrons, has an overall negative charge

64.

Cations

a)

Gain electrons, has an overall positive charge

b)

Lose electrons, has an overall positive charge

c)

Lose electrons, has an overall negative charge

d)

Gain electrons, has an overall negative charge

65.

How does calcium become an calcium ion?

a)

it loses 2 electrons

b)

it gains 2 electrons

66.

Looking at the molecule of Br2, which of the following correctly represents the number of shared

and unshared electrons in the diagram?

a)

14 shared electrons, 0 unshared electrons

b)

2 shared electrons, 12 unshared electrons

c)

1 shared electrons, 12 unshared electrons

d)

2 shared, 24 unshared

67.

CH4

a)

Covalent bond

b)

Ionic Bond

68.
What is the VSEPR theory used to predict?
a)
Bond Strength
b)
Polarity
c)
Molecular Shape
d)
Electronegativity
69.
What is the measure of a tetrahedral bond angle?
a)
90 Degrees
b)
109.5 Degrees
c)
120 Degrees
d)
180 Degrees
70.

Which of these is the shape of CCl4?

a)
b)
c)
d)
e)
71.

Which of these is the shape of NH3?

a)
b)
c)
d)
e)
72.

The electronegativity difference in the bonds of CH4 is:

a)

0.4

b)

5.9

c)

-0.4

d)

1.7

73.

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

a)

less than 0.4

b)

greater than 1.7

c)

between 0.4 and 1.7

d)

exactly 0

74.

What are the seven diatomic elements?

a)

H2, Cl2, Br2, O2, N2, I2, F2

b)

H2, Cl2, I2, F2, Hg2, Br2, Fe2

c)

H2, Cu2, Ni2, B2, O2, I2, Fe2

75.

How many atoms are in a diatomic molecule?

a)

2

b)

3

c)

4

d)

5

76.

Name the compound: N2O5.

a)

dinitrogen pentaoxide

b)

binitrogen pentaoxide

c)

nitrogen oxide

d)

pentanitrogen dioxide

77.

Name the compound: (NH4)2S

a)

ammonium sulfide

b)

nitrogen tetrahydrogen sulfide

c)

diammounium sulfate

d)

ammonium sulfate

78.

Name the compound: MgCl2

a)

magnesium chloride

b)

magnesium dichloride

c)

monomagnesium chloride

d)

manganese chloride

79.

Name the compound: Cu(NO3)2

a)

copper nitrate

b)

copper(II) nitrate

c)

copper(II) dinitrate

d)

copper dinitrogen hepaoxide

80.

Write the formula: potassium hydroxide

a)

KOH

b)

POH

c)

KH

d)

KO

81.

Write the formula: nitrogen trichloride

a)

NCl3

b)

N1Cl3

c)

N1Cl5

d)

Cl3N

82.

Write the formula: lead(IV) sulfite

a)

Pb2(SO3)4

b)

Pb(SO3)2

c)

Pb2(SO4)4

d)

Pb(SO4)2

83.

In the compound TiO2, titanium has a charge of ______. Hint: The charge on "O" is -2. Use the charge on oxygen to determine the charge on Ti.

a)

4+

b)

2+

c)

2-

d)

4-

84.

H20 - name?

a)

hydroxic acid

b)

dihydrogen oxide

c)

dihydrogen monoxide

d)

hydrogen oxide

85.

What is the formula for Calcium Chlorate?

a)

CaClO3

b)

Ca(ClO3)2

c)

Ca(ClO3)3

d)

Ca(ClO3)4

86.

Consider a mystery compound having the formula MxTy. If the compound is not an acid, if it contains only two elements, and if M is not a metal, which of the following is true about the compound?

a)

It contains a polyatomic ion.

b)

Its name ends in -ite or -ate.

c)

Its name ends in -ic.

d)

It is a binary molecular compound.

87.

Which element, when combined with fluorine, would most likely form an ionic compound?

a)

lithium

b)

carbon

c)

phosphorus

d)

chlorine

88.

Which of the following is true about the composition of ionic compounds?

a)

They are composed of anions and cations.

b)

They are composed of anions only.

c)

They are composed of cations only.

d)

They are formed from two or more nonmetallic elements.

89.

Which of the following is NOT a cation?

a)

iron (III) ion

b)

sulfate

c)

Ca2+

d)

sodium ion

90.

What is the name of the polyatomic ion PO43-

a)
phosphate
b)
phosphite
c)
carbonate
d)
hydroxide
91.
What is the right part of a chemical equation called...
2H2 + O2 --> 2H2O
a)
Reactants
b)
Products 
c)
Yields 
d)
Chemical Equation 
92.
What is the left part of a chemical equation called?
2H2 + O2 --> 2H2O
a)
Reactants
b)
Products 
c)
Yields 
d)
Chemical Equation 
93.
What does the Law of Conservation of Mass state?
a)
Matter cannot be gained or lost in a chemical reaction.
b)
Matter can only be lost in a chemical reaction.
c)
Matter can only be gained in a chemical reaction.
d)
Matter can be gained and lost in a chemical reaction. 
94.
What is the little number after an element in a chemical equation called.
Example: H2
a)
Coefficient 
b)
Subscript
c)
Atom
d)
Equation
95.

Balance this equation:

HgO ---> 2Hg + O2

a)

It is balanced.

b)

2HgO ---> 2Hg + O2

c)

2HgO ---> Hg + O2

d)

HgO ---> Hg + 2O2

96.

Balance the following equation:

___ H2+ ___ O2→___ H2O

a)

1, 1, 3

b)

2, 2, 2

c)

1, 2, 1

d)

2,1, 2

97.

Balance the following equation:

___ Mg+ ___ O2→___ MgO

a)

1, 1, 3

b)

2, 1, 2

c)

1, 2, 1

d)

2, 2, 2

98.
What are the larger numbers that you CAN CHANGE in a chemical equation? 
a)
Coefficient 
b)
Products
c)
Reactants
d)
Subscripts
99.
How many Hydrogen are in 4H2O?
a)
6
b)
8
c)
2
d)
4
100.

How many Oxygen atoms are in Al₂(SO₄)₃?

a)

4

b)

12

c)

7

d)

24

101.
The number 6.02 x 1023 is called...
a)
Obama's number
b)
Bohr's number
c)
Trump's number
d)
Avogadro's number
102.
What is the molar mass of C2H4O2?
a)
40g
b)
50g
c)
60g
d)
68g
103.
What would be the mass of 1.5mol H2O
a)
20
b)
27
c)
32
d)
40
104.
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
105.

The process of comparing units is called ____________________.

a)

stoichiometry

b)

dimensional analysis

c)

algebra

d)

social studies

106.
an atom with atomic number 6 would have how many protons 
a)
6
b)
12
c)
3
d)
cannot be determined 

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