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Chemistry CP Fall Final Exam Review

Total questions: 88

Worksheet time: 1hrs 25mins

Name
Class
Date
1.
2.   Which of these recorded observations is qualitative, rather than quantitative?
a)
a.  A chemical reaction is complete in 2.3 s.
b)
a.  The solid has a mass of 23.4 g.
c)
The compound melts at 87.5°C.
d)
Iron is denser than aluminum.
2.
3.  A sample of bismuth has a mass of 343g and a volume of 35.0cm3. What is the density of bismuth?
a)
a.  0.102 g/cm3 
b)
b. 9.80 g/cm3 
c)
c. 378 g/cm3 
d)
d. 1.20 x 104 g/cm3
3.
4.  How many meters are there in 1,865 cm?
a)
0.1865 m
b)
1.865 m
c)
18.65 m
d)
186.5 m
4.
7.  Convert the following measurement:  5.4 L to mL
a)
54. mL
b)
5400. mL
c)
540. mL
d)
54000. mL
5.
12.  Which element does the following configuration represent?  1s2,2s2,2p6,3s2,3p5
a)
   Phosphorus
b)
     Chlorine
c)
   Silicon
d)
    Argon
6.
13.  What is the correct electron configuration for Calcium?
a)
a.  1s2,2s2,2p6,3s2,3p6,4s1
b)
a.  1s2,2s2,2p6,3s2,3p6,4s2
c)
a.  1s2,2s2,2p6,3s2,3p5,4s2
d)
1s2,2s2,2p6,3s3,3p5,4s1
7.
15.  What is the correct formula for the compound made of magnesium and nitrogen?
a)
   Mg2N3
b)
      Mg3N2
c)
    MgN2
d)
      MgN
8.

Which of the following statements is NOT true about what happens in all chemical reactions?

a)

The ways in which atoms are joined together change

b)

New atoms are formed as products

c)

The starting substances are called reactants

d)

The bonds of reactants are broken and new bonds of products are formed

9.
The charge of a chlorine ion.
a)
-1
b)
+1
c)
-2
d)
+2
10.
Carbon is in the...
a)
s-block
b)
p-block
c)
d-block
d)
f-block
11.
The name of group 17.
a)
Alkali metals
b)
Noble Gases
c)
Alkaline Earth metals
d)
Halogens
12.
Noble gases don't react with anything else because...
a)
they are too large
b)
they are gases
c)
they have 8 valence electrons
d)
they need to gain 1 valence electron
13.
The most reactive metals are the...
a)
Alkaline earth metals
b)
Transition metals
c)
Alkali metals
d)
Halogens
14.
Burning & decomposition are _____ changes.
a)
Chemical
b)
Physical
15.
Which of the following is an intensive property?
a)
Color
b)
Length
c)
Width
d)
Mass
16.
The state of matter with the highest energy is...
a)
Solid
b)
Liquid
c)
Gas
17.
How many dots should be on a Lewis Dot Structure for nitrogen (N)?
a)
7
b)
8
c)
1
d)
5
18.
What is the name for this compound?
MgCl2
a)
Magnesium dichloride
b)
Monomagnesium dichloride
c)
Magnesium chloride
d)
Chloride dimagnesium
19.
What is the formula for density?
a)
density = mass x volume
b)
density = mass / volume
c)
density = mass + volume
d)
density = mass - volume
20.
Frank has an eraser. It has a mass of 4g, and a volume of 2cm3. What is its density?
a)
8 g/cm3
b)
2 g/cm3
c)
1/2 g/cm3
d)
24 g/cm3
21.

The study of the composition, structure, and properties of matter and the changes it undergoes.

a)

Chemistry

b)

Physics

c)

Biology

d)

Social Science

22.
The leaf is 5mm wide.
a)
Qualitative
b)
Quantitative
23.
The temperature of the room is decreasing by 4 degrees Celsius.
a)
Qualitative
b)
Quantitative
24.
What is matter?
a)
a pure substance
b)
anything that occupies space and possesses mass
c)
an element
d)
a compound
25.
What is the measure of how much space an object takes up?
a)
matter
b)
volume
c)
substance
d)
properties
26.
Which one of these is a chemical property?
a)
melting point
b)
boiling point
c)
color
d)
flammability
27.
Which is an example of a physical property?
a)
ability to react with acid
b)
 state of matter
c)
flammability
d)
ability to react with oxygen
28.
Which of the following is a chemical change?
a)
human digestion
b)
cutting a tree down
c)
melting a chocolate bar
d)
Has a density of 1 gm/mL
29.

___________ are the smallest unit of an element that maintains the properties of that element.

a)

Atoms

b)

Elements

c)

Compounds

d)

Mixtures

30.

An _______________ is made up of one or more of the same kind of atom chemically combined.

a)

atom

b)

element

c)

molecule

d)

compound

31.

A _____________ contains a variety of elements and compounds that are not chemically combined with each other.

a)

compound

b)

element

c)

molecule

d)

mixture

32.

A __________________ is a substance that has definite physical and chemical properties such as appearance, melting point, and reactivity.

a)

mixture

b)

pure substance

c)

compound

d)

element

33.

A ______________ mixture is one that does not have a uniform composition.

a)

heterogeneous

b)

homogenous

c)

pure substance

34.

A _________________ mixture is one where the substances are evenly spread throughout.

a)

heterogeneous

b)

homogeneous

c)

pure substance

35.

Which of these is an element?

a)

Salt (NaCl)

b)

Water (H20)

c)

Oxygen (O)

d)

Carbon Dioxide (CO2)

36.

Which of these is a compound?

a)

Aluminium (Al)

b)

Carbon Dioxide (CO2)

c)

Nitrogen (N)

d)

Sand

37.

What is at the center of every atom?

a)

An electron

b)

A compound

c)

A molecule

d)

A nucleus

38.
Which two particles make up the nucleus of an atom?
a)
Protons and Electrons
b)
Protons and Neutrons
c)
Molecules and Compounds
d)
Neutrons and Electrons
39.
What is the role of an electron in an atom?
a)
Electrons live inside the nucleus and carry a neutral charge.
b)
Electrons circle the nucleus and have a positive charge.
c)
Electrons circle the nucleus and have a negative charge.
d)
Electrons live inside the nucleus and have a negative charge.
40.
Which of the following determines the type of element that an atom makes?
a)
The size of the nucleus.
b)
The number of protons.
c)
How much the atom weighs.
d)
The number of neutrons.
41.
What forms when two atoms combine?
a)
A molecule.
b)
A nucleus.
c)
A proton.
d)
An electron.
42.
An electron is a _____ charged particle.
a)
Positively
b)
Negatively
43.
A proton is a _____ charged particle.
a)
Negatively
b)
Positively
44.
The atoms of any given element ____ have the same number of protons.
a)
sometimes
b)
always
c)
never
45.
What charge does a neutron have?
a)
positive
b)
negative
c)
no charge
d)
neutral
46.
Which element has 31 protons ?
a)
Gallium 
b)
Germanium
c)
Gadolinium
d)
Polonium
47.
Which element has 56 electrons ?
a)
Barium
b)
Boron
c)
Beryllium
d)
Bromine
48.
How many neutrons are in Mercury (Hg) ?
a)
200
b)
80
c)
121
d)
72
49.

Person that discovered electrons using the cathode ray experiment. He created the plum pudding model

a)

Neils Bohr

b)

Ernest Rutherford

c)

JJ Thomson

d)

Dmitri Mendeleev

50.

Rutherford's experiment that he used to discover protons and the nucleus.

a)

gold foil experiment

b)

cathode ray experiment

c)

neither of these is correct

51.
What is an isotope? 
a)
A charged atom
b)
An atom with different amounts of neutrons
c)
An atom with different amounts of protons
d)
A neutral atom
52.

What is the speed of light?

a)

3.0x108 ms

b)

3.0x108 m/s

c)

6.626x10-34 Js

d)

6.626x10-34 J/s

53.
The distance from one point to the next corresponding point on a wave is called the ________________.
a)
waveform
b)
peak
c)
amplitude
d)
wavelength
54.
High frequency waves have _________ wavelength.
a)
varying
b)
high
c)
the same
d)
low
55.

What happens when an electron gains energy?

a)

The electron goes to an excited state, and electrons move to an outer shell

b)

The electron goes to an excited state, and electrons move to an inner shell

c)

The electron goes to the ground state, and electrons move to an outer shell

d)

The electron goes to the ground state, and electrons move to an inner shell

56.

What happens when an electron releases energy?

a)

The electron goes to an excited state, and electrons move to an outer shell

b)

The electron goes to an excited state, and electrons move to an inner shell

c)

The electron goes to the ground state, and electrons move to an outer shell

d)

The electron goes to the ground state, and electrons move to an inner shell

57.
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
58.

How are the elements arranged on the periodic table today?

a)

By atomic mass

b)

By number of electrons

c)

By atomic number

d)

By alphabetic order

59.

Who arranged the known elements into horizontal rows of increasing atomic mass leaving gaps for as yet undiscovered elements?

a)

Mendeleev

b)

Meyer

c)

Newlands

d)

Moseley

60.
Which of the following is the atomic number of an alkali metal?
a)
31
b)
20
c)
18
d)
19
61.

Sulfur is a...

a)

metal

b)

nonmetal

c)

metalloid

62.

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

63.

The is family has properties of both metals and nonmetals.

a)

Alkali

b)

Halogens

c)

Nonmetals

d)

Metalloids

64.
Which of the following in not a diatomic element?
a)
hydrogen
b)
carbon
c)
nitrogen
d)
oxygen
65.
How many valence electrons does a halogen have? 
a)
1
b)
2
c)
7
d)
8
66.
Argon (Ar)
a)
alkali metal
b)
alkaline earth metal
c)
halogen
d)
noble gas
67.
Which element is not in the Alkali metal family?
a)
Li
b)
H
c)
Fr
d)
Cs 
68.
Gold (Au)
a)
Transition Metal
b)
Alkali Metal
c)
Alkaline Earth Metal
d)
Heavy Metal
69.

Which atom has the largest atomic radius?

a)

potassium

b)

rubidium

c)

francium

d)

cesium

70.
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
71.
Which periodic group has the smallest atomic radius?
a)
Alkali metals
b)
Halogens
c)
Noble Gases
d)
Transition metals
72.

Ionization energy __________ as you do across a period

a)

has no pattern

b)

stays the same

c)

decreases

d)

increases

73.

What is Ionization energy?

a)

The energy used in a chemical reaction

b)

Potential energy

c)

The energy it takes to remove one electron from an atom or ion in its gaseous state

74.
What is the VSEPR theory used to predict?
a)
Bond Strength
b)
Polarity
c)
Molecular Shape
d)
Electronegativity
75.
Which molecule would have this molecular geometry?
a)
BF3
b)
CH4
c)
PCl5
d)
CO2
76.
Who could this molecule be?
a)
CH4
b)
CO2
c)
PCl5
d)
BF3
77.
What molecular shape is the structure shown here? (H2O)
a)
tetrahedral
b)
trigonal planar
c)
bent
d)
trigonal pyramidal
78.

When one atom transfers one or more valence electrons to another atom, a(n) __________ is formed.

a)

covalent bond

b)

ionic bond

c)

metallic bond

d)

hair bond

79.

When electron(s) are shared between two or more atoms, they form?

a)

Covalent bond

b)

Ionic bond

c)

Metallic bond

d)

Carbon bond

80.
According to the octet rule most elements need _______ valence electrons.
a)
2
b)
8
c)
6
d)
18
81.
Hydrogen needs _____ electrons in its valence shell to be stable.
a)
4
b)
6
c)
8
d)
2
82.
If electrons are shared unequally then the bond is....
a)
Non-polar covalent
b)
Ionic
c)
Non-polar ionic
d)
Polar covalent
83.
If electrons are shared equally then the bond is....
a)
Non-polar covalent
b)
Ionic
c)
Non-polar ionic
d)
Polar covalent
84.
How strongly an atom attracts electrons is called....................
a)
Ionization energy
b)
Electronegativity
c)
Electricity
d)
Nuclear force
85.

How would you draw a Lewis dot diagram for Magnesium?

a)
b)
c)
d)
86.
All chemical bonds involve two atoms sharing electrons.
a)
True
b)
False
87.
If an atom loses two electrons what charge will it have?
a)
+ 2
b)
 - 2
c)
+1
d)
-1
88.
If an atom gains one electron what charge will it have?
a)
-2
b)
-1
c)
+1

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