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Midterm Review 2.0

Total questions: 100

Worksheet time: 2hrs 10mins

Name
Class
Date
1.

What is the atomic number?

a)

the number of protons in the nucleus

b)

the number of protons and neutrons in the nucleus

c)

the number of neutrons in the nucleus

d)

the number of protons in the energy levels

2.

What is the mass number?

a)

the number of protons in the nucleus

b)

the number of protons and neutrons in the nucleus

c)

the number of neutrons in the nucleus

d)

the number of protons and electrons in the atom

3.

What is the atomic number of this atom?

a)

1

b)

3

c)

4

d)

7

4.

What is the mass number of this atom?

a)

1

b)

3

c)

4

d)

7

5.
Most of the mass in an atom is made up of _____________________?
a)
protons and electrons
b)
protons and neutrons
c)
neutrons and electrons
d)
electrons and quarks
6.
In order for an atom to be neutral what has to be true?
a)
The atom has more protons than neutrons
b)
The atom has more neutrons than protons
c)
The atom has the same number of protons and neutrons
d)
The atom has the same number of protons and electrons
7.
What does the C represent?
a)
atomic mass
b)
atomic number
c)
element name
d)
chemical symbol 
8.

What does the 6 represent?

a)

Atomic mass

b)

atomic number

c)

chemical symbol

d)

element name

9.
How is the number of neutrons in the nucleus of an atom calculated?
a)
Add the number of e- and p+ together
b)
Subtract the number of e- from p+
c)
Subtract the number of p+ from the mass number
d)
Add the mass number to the number of e-
10.
What subatomic particles would you find in the nucleus of an atom?
a)
Protons only
b)
Protons and Neutrons
c)
Neutrons and Electrons
d)
Protons and Electrons 
11.
Which subatomic particles contribute the most to the mass of an atom?
a)
Protons, Neutrons, Electrons
b)
Protons only
c)
Protons and Electrons
d)
Protons and Neutrons
12.
If an atom has 12 positively charged subatomic particles, which of the following must it also have to be considered a neutral atom?
a)
12 neutrons
b)
12 electrons
c)
12 protons
d)
24 protons and neutrons
13.

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

a)

20

b)

10

c)

35

d)

25

14.

How many electrons does this atom have?

a)

2

b)

4

c)

6

d)

10

15.
The atomic number of an element that has 9 protons, 9 electrons, and 10 neutrons is _____.
a)
9
b)
10
c)
19
d)
28
16.
An element with a mass number of 11 and an atomic number of 5 has how many neutrons?
a)
11
b)
5
c)
6
d)
16
17.
Where is most of the mass in an atom located?
a)
in the nucleus
b)
in the protons
c)
in the neutrons
d)
in the electrons
18.
An atom has an atomic number of 15 and a mass number of 31. How many protons are there in the atom?
a)
15
b)
31
c)
16
d)
47
19.
What is the atomic number of the atom pictured? 
a)
9
b)
10
c)
18
d)
19
20.

Which of the following determines the identity of an element?

a)

number of protons

b)

atomic mass

c)

number of neutrons

d)

number of shells

21.

Carbon is considered an element, while carbon dioxide is considered a compound. This is because carbon dioxide is ---

a)

a gas at room temperature.

b)

made of two different elements.

c)

given off by green plants.

d)

useful to human beings

22.

What is the pH range of an acid?

a)

4-6

b)

1-7

c)

1-6

d)

8-14

23.

Which of the following pH values would be the strongest acid?

a)

1

b)

3

c)

4

d)

6

24.

A substance is found to have the following characteristics:


Very bitter taste

Feels slippery to the touch

Produces OH- ions when dissolved in water


In what category would the substance be classified?

a)

acid

b)

base

c)

enzyme

d)

fatty acid

25.
Pure water has a pH of 7. Pure water _______.
a)
is a base
b)
is a neutral substance
c)
could be either an acid or a base
d)
is an acid
26.

Which of the following is an example of COHESION?

a)

water sticking to water

b)

water sticking to glass

c)

oil sticking to plastic

d)

hydrogen sticking to oxygen

27.

What is the correct chemical formula for water?

a)

H2O

b)

HO2

c)

H2O2

d)

2H1O

28.

Water is polar. What does that mean?

a)

it is a molecule with opposite charges on opposite ends

b)

it is a molecule with no charge

c)

it is a molecule with identical charges on opposite ends

d)

it is a molecule with too many protons

29.

Water sticks well to many materials. What term relates to this property of water?

a)

cohesion

b)

adhesion

c)

density

d)

surface tension

30.

What is the term for water's ability to defy gravity and climb up a tube?

a)

Capillary Action

b)

Specific Heat

c)

Universal Solvent

d)

Magic

31.

A water strider can skate along the top of a pond because:

a)

covalent bonds result in water cohesion (surface tension)

b)

hydrogen bonds result in water cohesion (surface tension)

c)

water striders have adapted to take advantage of water cohesion

d)

water striders are afraid of water and avoid it

32.

Why does ice float?

a)

water expands when it freezes, making ice less dense than water

b)

water compacts when it freezes, making ice more dense than water

c)

hydrogen bonds in water push the ice to the surface

d)

ice is afraid of water, and avoids it

33.
Large bodies of water do not quickly fluctuate in temperature. Why?
a)
Water is a solvent.
b)
Water has a high heat capacity.
c)
Water acts as a buffer.
d)
Water is non-polar.
34.
Water is a universal solvent because it...
a)
It can be found anywhere
b)
It freezes when it gets cold
c)
floats when frozen
d)
Dissolves most substances
35.
The tightness across the surface of water that enables paper clips to float is ____________.
a)
adhesion
b)
capillary action
c)
surface tension
d)
polarity
36.

What two elements make up water?

a)

Helium and Oxygen

b)

Hydrogen and Oxygen

c)

Helium and Carbon

d)

Oxygen and Carbon

37.

How many hydrogen atoms are in a water molecule?

(HINT: H20)

a)

5

b)

1

c)

2

d)

0

38.
A(n) _____________ is an atom or group of atoms that has an electric charge. 
a)
ion
b)
electron
39.
When an atom loses a valence electron, it becomes a(n) _________ion.
a)
positive 
b)
negative
40.

How do you write the formula for sodium chloride?

a)

NACL

b)

NaCl

c)

nacl

d)

KI

41.

How is an ionic bond formed?

a)

Sharing of electrons

b)

Delocalised electrons

c)

Transfer of electrons

42.
The chemical bond formed when two atoms share electrons  is called a(an) IONIC bond. 
a)
True
b)
False
43.
Covalent bonds usually form when a nonmetal combines with a(an) METAL.
a)
True
b)
False
44.
Covalent bonds usually form when a nonmetal combines with a(an) METAL.
a)
True
b)
False
45.
What two types of atoms make a covalent bond?
a)
2 Nonmetals
b)
1 Nonmetal and 1 Metal
c)
2 Metals
d)
2 Noble Gases
46.
Element or compound?
O2
a)
Element
b)
Compound
47.
Element or compound?
H2O
a)
Element
b)
Compound
48.
What is the left part of a chemical equation called?
2H2 + O2 --> 2H2O
a)
Reactants
b)
Products 
c)
Yields 
d)
Chemical Equation 
49.
What is the right part of a chemical equation called...
2H2 + O2 --> 2H2O
a)
Reactants
b)
Products 
c)
Yields 
d)
Chemical Equation 
50.
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. 
51.
How many Hydrogen are in 4H2O?
a)
6
b)
8
c)
2
d)
4
52.
Is the following equation balanced?...
Al + O2 --> 2Al2O3
a)
Yes!
b)
No!
53.
Is the following equation balanced?
4Fe + 3O2 --> 2Fe2O3
a)
yes
b)
no
54.
How many HCl molecules do you need to balance this equation? 
Mg +  __HCl --->  MgCl2 + H2
a)
1
b)
2
c)
3
d)
4
55.
Balance this equation:
 2Li + Cl2 -> LiCl
a)
2Li + Cl2 -> 4LiCl2
b)
2Li + Cl2 -> LiCl2
c)
2Li + Cl2 -> 2LiCl
56.
Why do elements bond?
a)
To be friends
b)
To create a new element
c)
To become stable
57.
How are covalent bonds formed?
a)
Sharing of electrons
b)
Transfer of electrons
58.
How are ionic bonds formed?
a)
Transfer of electrons
b)
Sharing of electrons
59.
Atoms are most stable when their outer shell is complete.
a)
true
b)
false
60.
Noble gases will form chemical bonds with other elements
a)
True
b)
False
c)
Sometimes
61.

Why do elements bond?

a)

To be friends

b)

To create a new element

c)

To become stable

d)

To get bigger

62.
What is a valence electron?
a)
The sum of neutrons and protons.
b)
The # of electrons in the last shell.
c)
A type of bond.
d)
A popular compound.
63.

The octet rules states that most elements want to have _____ valence electrons.

a)

2

b)

4

c)

6

d)

8

64.

How many valence electrons does Oxygen (O) have?

a)

6

b)

8

c)

15

d)

16

65.

Force of attraction between atoms or ions.

a)

Mixture

b)

Compound

c)

Chemical Bond

d)

Formula

66.

What two types of atoms make a covalent bond?

a)

2 nonmetals

b)

2 metals

c)

1 metal and 1 nonmetal`

67.

What happens to electrons in a covalent bond?

a)

they are shared

b)

they are transferred

c)

they are negative

68.

Ionic bonds are between

a)

metals and nonmetals

b)

2 metals

c)

2 nonmetals

69.

What type of bonding does this picture show?

a)

Ionic

b)

Covalent

70.

Carbon and Oxygen will make a ___________ bond.

a)

ionic

b)

covalent

c)

metallic

71.

Sodium and Bromine will make a _____ bond.

a)

ionic

b)

covalent

c)

metallic

72.

When electrons are lost by one atom and gained by another, so that they both get full outer shells.

a)

Covalent bond

b)

Ionic bond

c)

Pairing

d)

Compound

73.
Where are the nonmetals located on the periodic table? 
a)
Blue
b)
Red
c)
Green
74.

Why don't noble gases form bonds?

a)

They all have a full octet

b)

Noble gases do form bonds

c)

They only bond when with eachother

d)

none of these answers are correct

75.

During a chemical reaction, atoms can

a)

be destroyed to form a new substance

b)

be created to form a new substance

c)

be rearranged to form a new substance

76.

What is a coefficient?

a)

Number behind molecule (does not apply)

b)

Number in front of molecule (applies to whole thing)

c)

Applies to the element it follows

77.

We balance equations to show...

a)

Change

b)

Reactants

c)

Products

d)

Conservation of mass

78.

Subscripts apply to

a)

The whole reaction

b)

The individual element

c)

The product side

d)

The reactant side

79.
the starting materials in a chemical reaction
a)
Products
b)
Reactants
c)
Starters
d)
Enders
80.
The substances listed on the right side of a chemical equation are the
a)
Yields
b)
Reactants
c)
Products
d)
Precipitates
81.

The process by which one or more substances change to produce one or more different substances

a)

Chemical Process

b)

Reactant

c)

Chemical Reaction

82.
In the equation,          2Mg + O2 ---> 2MgO, which are the reactants?
a)
Mg and O
b)
MgO
c)
Mg and MgO
d)
O and MgO
83.
What are Chemical Reactions?
a)
It's when you mix substances.
b)
a process in which atoms rearrange to form new substances
c)
When something bubbles.
d)
letter and numbers showing the types and number of atoms
84.

6CO2+ 6H2O → C6H12O6 + 6O26CO_2+\ 6H_2O\ \rightarrow\ C_6H_{12}O_{6\ }+\ 6O_2  

The carbon atoms are balanced with ____ on each side of the reaction.

a)

1

b)

6

c)

2

85.

Determined whether the following equation is balanced or unbalanced. Ag + O2 ---> 2Ag2O

a)

Balanced

b)

Unbalanced

86.

Determine whether the following equations is balanced or unbalanced. H4 + O2 ---> 2H2O

a)

Balanced

b)

Unbalanced

87.

Determine whether the following equation is balanced or unbalanced. H2 + Br2 ---> 2HBr

a)

Balanced

b)

Unbalanced

88.

Determine whether the following equation is balanced or unbalanced. 2Fe + 3Cl2 ---> FeCl3

a)

Balanced

b)

Unbalanced

89.

In order for an equation to be balanced, there must be ...

a)

an equal amount of atoms on both sides

b)

a greater mass on the product side

c)

a greater mass on the reactant side

d)

elements with the same atomic # on both sides

90.
In this image, what are the information in red is called the_______.
a)
Product
b)
Reactant
c)
Chemical Subscript
d)
Coefficient
91.
In this image, what are the information to the right of the arrow (in black) is called the_______.
a)
Product
b)
Reactant
c)
Chemical Subscript
92.
The law of conservation of mass states that....
a)
Matter can be made
b)
Matter can be destroyed
c)
Matter can neither be made or destroyed
d)
Matter can evaporate
93.
Is the following equation balanced or unbalanced?
Fe + S --> FeS
a)
balanced
b)
unbalanced
94.
Is this balanced?...
Al + O2 --> 2Al2O3
a)
Yes!
b)
NO!
95.

Determine whether the following equation is balanced or unbalanced. 4P +5O2 ---> 2P2O5

a)

Balanced

b)

Unbalanced

96.
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
97.
Grinding a seltzer tablet into powder increases the rate of reaction due to increased
a)
concentration
b)
surface area
c)
temperature
d)
reactants
98.
Which factors increase the rate of a reaction.
a)
increasing temperature
b)
increasing concentration
c)
increasing surface area
d)
all of these
99.

The electrons in the outermost shell (main energy level) of an atom; these are the electrons involved in forming bonds

a)

alkali metals (group 1)

b)

Halogens (Group 17)

c)

atomic number

d)

valence electrons

100.

A subatomic particle that has a negative charge

a)

nobles gases

b)

protons

c)

electrons

d)

neutrons

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