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Final Semester 1 Review

Total questions: 130

Worksheet time: 3hrs 33mins

Name
Class
Date
1.

Contains only one kind of atom.

a)

Element

b)

Compound

c)

Mixture

2.

Contains more than one type of atom held together by a chemical bond.

a)

Element

b)

Compound

c)

Mixture

3.
Classify the picture with the correct label.
a)
Element
b)
Compound
c)
Mixture of Elements
d)
Mixture of Compounds
4.
Classify the picture with the correct label.
a)
Element
b)
Compound
c)
Mixture of Elements and Compounds
d)
Mixture of Elements
5.
Classify the picture with the correct label.
a)
Compounds
b)
Mixture of Elements
c)
Mixture of Compounds
d)
Mixture of Elements & Compounds
6.
Classify the picture with the correct label.
a)
Element
b)
Compound
c)
Mixture of Compounds
d)
Mixture of Elements
7.
Classify the picture with the correct label.
a)
Element
b)
Compound
c)
Mixture of Elements & Compounds
d)
Mixture of Elements
8.
Classify the picture with the correct label.
a)
Mixture of Elements
b)
Mixture of Elements & Compounds
c)
Mixture of Compounds
d)
Compounds
9.

A ______ is the smallest building block of matter.

a)

compound

b)

element

c)

atom

10.

The center of an atom is called a ______.

a)

electron

b)

proton

c)

nucleus

11.

A group of the same atoms that are bonded together is called...

a)

element

b)

compound

c)

mixture

12.

The students measured length during a science experiment, they got 12 cm. But the actual measurement was 14.25 cm. What was the percent error?

a)

15.79%

b)

18.75%

c)

2.25%

d)

18%

13.
?
a)
High Accuracy & High Precision
b)
High Accuracy & Low Precision
c)
Low Accuracy & High Precision
d)
Low Accuracy & Low Precision
14.
A set of data are all close to each other, and they are close to the actual value.  This set of data can be described as...
a)
accurate
b)
precise
c)
both precise and accurate
15.
It is a measure of how close measurements come to each other when they are made in the same way
a)
Accuracy
b)
Precision
c)
Error
d)
Extrapolation
16.
Describe the accuracy and precision of the image
a)
Accurate and Precise
b)
Accurate and not precise
c)
Not Accurate and Precise
d)
not accurate and not precise
17.
True or False: a physical change may produce a new substance.
a)
True
b)
False
18.

Choose the best description below for the image

a)

physical change

b)

chemical change

19.

What kind of change occurs if matter changes in amount, size, or shape?

a)

substance change

b)

chemical change

c)

physical change

d)

elemental change

20.

1) True or False: Intensive Properties change as the amount of substance changes.

a)

True

b)

False

21.
What is the definition of a chemical change?
a)
Characteristics that describe how a substance behaves under different conditions
b)
Alteration in the physical state of matter without changing its chemical composition
c)
Transformation that results in the creation of new substances
d)
Inherent characteristics that help us identify and describe matter
22.
What is the definition of physical changes?
a)
changes that describe how a substance behaves under different conditions
b)
characteristics that describe how a substance interacts with other substances
c)
changes that alter the form or appearance of a substance, but not its chemical composition
d)
changes that lead to the formation of new substances with different chemical properties
23.

In a chemical reaction, 4 grams of sodium must combine with how many grams of chlorine to produce 10 grams of table salt?

a)

4 grams

b)

6 grams

c)

8 grams

d)

10 grams

24.
In a reaction A + B ----> C,  reactant A has 5g and product  C has 9g. How many grams does reactant B should have? 
a)
4g
b)
5g
c)
9g
d)
14g
25.

Determine the number of oxygen atoms in Al(OH)3

a)

1

b)

2

c)

3

d)

4

26.

Calculate the molar mass of CuBr2

a)

143.45 g/mol

b)

223.35 g/mol

c)

287.30 g/mol

d)

307.90 g/mol

27.

What is the percent by mass of Cu in CuBr2?

a)

50%

b)

71.6%

c)

28.4%

d)

44.3%

28.

What is the percent by mass of Br in CuBr2?

a)

50%

b)

71.6%

c)

28.4%

d)

44.3%

29.

How many H atoms are in (NH4)3PO4?

a)

4

b)

7

c)

12

d)

15

30.

What did Rutherford discover about atoms?

a)

An atom is always negatively charged.

b)

An atom is mostly empty space, but has a dense positively charged center(nucleus).

c)

An atom is always positively charged.

d)

All particles will pass straight through gold foil with no change in path.

31.

Rutherford's "gold-foil" experiment using alpha particle scattering concluded that

a)

the center of the atom is empty

b)

atomic mass is spread over the whole atom

c)

the center of the atom has a negative charge

d)

most of the atom is empty space

32.
What makes something radioactive?
a)
elements with an atomic number above 81
b)
an unstable nucleus
c)
contaminated sewage
d)
It decays over time
33.
Has a mass of 4 and a charge of +2
a)
Alpha
b)
Beta
c)
Gamma
34.
Takes two small nuclei and combines them into a larger nucleus
a)
fission
b)
fusion
35.
The splitting of a nucleus into smaller nuclei is
a)
fusion
b)
fission
c)
half-life
d)
gamma radiation
36.
Which type of nuclear radiation is being emitted here?
a)
Alpha
b)
beta
c)
gamma 
d)
none
37.
Which type of nuclear radiation is being emitted here?
a)
alpha
b)
beta
c)
gamma
d)
none
38.
What particle completes this reaction?
a)
alpha particle
b)
beta particle
c)
gamma particle
d)
neutron
39.

Why does alpha decay occur?

a)

The nucleus is too large to be stable

b)

The proton to neutron ratio is unstable

c)

The nucleus is in an excited state. This usually follows other types of decay.

40.

Why does beta decay occur?

a)

The nucleus is too large to be stable

b)

The proton to neutron ratio is unstable

c)

The nucleus is in an excited state. This usually follows other types of decay.

41.

Why does gamma decay occur?

a)

The nucleus is too large to be stable

b)

The proton to neutron ratio is unstable

c)

The nucleus is in an excited state. This usually follows other types of decay.

42.

gamma waves

a)

has a high penetrating power

b)

has a lower penetrating power

c)

has a medium penetrating power

43.

if Phosphorus-32 decay into beta reaction the result will be:

a)

Sulfur- 28

b)

Sulfur-32

c)

Al-32

44.

How many protons are in Sodium?

a)

11

b)

22

c)

12

d)

33

45.

How many electrons are in Aluminium?

a)

40

b)

27

c)

13

d)

14

46.

How many neutrons are in Phosphorus?

a)

16

b)

15

c)

31

d)

46

47.

Different isotopes of an element contain different numbers of ___.

a)

protons

b)

neutrons

c)

electrons

d)

elements

48.

If a proton is added or removed from an atom, what happens?

a)

It becomes a different element.

b)

It becomes a different isotope.

c)

Nothing happens.

49.

What is the difference between Neon-20 and Neon-22?

a)

They have different numbers of electrons.

b)

They have different numbers of neutrons.

c)

Only 1 is radioactive.

d)

No difference.

50.
Iron-60 (atomic number 26) is an isotope that is often used to study meteorites.  How many neutrons does iron-60 have?
a)
26
b)
60
c)
34
d)
86
51.
An element has two naturally occurring isotopes. One is 10.013 amu and is 19.9% abundant. The other is 11.01 amu and is 80.1% abundant. What is the average atomic mass? What element is it?
a)
9.012, Beryllium
b)
12.011, Carbon
c)
6.941, Lithium
d)
10.812, Boron
52.

Which EM waves have the longest wavelength?

a)

radio

b)

x-rays

c)

ultraviolet

d)

gamma rays

53.

Which EM waves have the shortest wavelength?

a)

radio

b)

x-rays

c)

ultraviolet

d)

gamma rays

54.

Which EM waves are have a SHORTER wavelength than visible?

a)

radio

b)

none

c)

infrared

d)

x-rays

55.

Which EM waves are have the highest energy & are the most dangerous?

a)

radio

b)

gamma rays

c)

infrared

d)

x-rays

56.
A certain photon of light has a wavelength of 4.22x10-7nm. What is the frequency? (v=c/λ)
a)
7.11x1014 Hz
b)
7.11Hz
c)
1.41x10-15
d)
-1.41x1015
57.
Select the correct order of waves on the EMS 
a)
Radio, Micro, Infra, Visible, Ultra, X-ray, Gamma
b)
Gamma, X-ray, Ultra, Vis, Infra, Micro, Radio
c)
Vis, Micro, Infra, Ultra, X-ray, Gamma, Radio
d)
Micro, Radio, Vis, Infra, Ultra, X-ray, Gamma
58.
What is the energy of a quantum of light with a frequency of 7.39x1014Hz.(E=Hv)
a)
4.88x1019
b)
4.88x10-19
c)
2.22x1023
d)
2.22x10-23
59.

The relationship between wavelength and frequency

a)

direct relationship

b)

straight relationship

c)

inverse relationship

d)

no relationship

60.

The full range of frequencies of electromagnetic radiation is called

a)

visible light.

b)

radio waves.

c)

the electromagnetic spectrum.

d)

invisible radiation.

61.

Calculate the energy of the photons in a type of electromagnetic radiation if the frequency is 4,5 x 1018 Hz.

a)

2,98 X 1015 joules

b)

1,47 x 10-52 joules

c)

6,79 x 1051 joules

d)

2,98 X 10-15 joules

62.

Which two terms describe the dual nature of light?

a)

particle and solid

b)

wave and flat line

c)

transverse and longitudinal

d)

wave and particle

63.

Which example shows a violation of Hund's Rule?

a)

A

b)

B

c)

C

d)

D

64.
All orbitals of equal energy are occupied by one electron before any single orbital is occupied by a second electron.
a)
Aufbau principle
b)
Pauli exclusion principle
c)
Hund’s rule
d)
Core Notation
65.

An aluminium ion would have which electron configuration?

a)

1s2 2s2 2p6 3s2

b)

1s2 2s2 2p6 3s2 3p1

c)

1s2 2s2 2p6 3s2 3p6

d)

1s2 2s2 2p6

66.

Which ion is this an electron configuration of: 1s22s22p63s23p6

a)

Na+

b)

O2-

c)

P3-

d)

Rb+

67.

This orbital diagram represents

a)

Nitrogen

b)

Oxygen

c)

Carbon

d)

Neon

68.
Which electron configuration belongs to Chlorine (Cl)?
a)
1s2 2s2 2p6 3s2 3p5
b)
1s2 2s2 2p6 3s2 3p6
c)
1s2 2s2 2p6 3s2 3p7
69.
What atom matches this electron configuration?
1s22s22p63s23p64s23d10
a)

Zinc (Zn)

b)

Copper (Cu)

c)

Nickel (Ni)

d)

Germanium (Ge)

70.

What element has the following electron configuration:

1s22s22p63s23p64s23d104p5

a)

Bromine (Br)

b)

Chlorine (Cl)

c)

Calcium (Ca)

d)

Manganese (Mn)

71.
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
72.
What is the shape of an s orbital?
a)
sphere
b)
dumbbell
c)
double dumbbell
d)
TOO COMPLEX TO KNOW IT.
73.
An electron occupies the lowest energy orbital that can receive it.
a)
Hund’s rule
b)
Pauli exclusion principle
c)
Bohr model of the atom
d)
Aufbau principle
74.
All orbitals of equal energy are occupied by one electron before any single orbital is occupied by a second electron.
a)
Aufbau principle
b)
Pauli exclusion principle
c)
Hund’s rule
d)
Core Notation
75.
No two electrons in the same atom can have the same four quantum numbers.
a)
Aufbau principle
b)
Pauli exclusion principle
c)
Hund’s rule
d)
Noble gas notation
76.
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
77.
Which guideline, Hund’s rule or the Pauli exclusion principle, is violated in the following orbital diagrams?
a)
Aufbau's
b)
Hund's
c)
Pauli exclusive
78.
The blue atoms are called 
a)
metals
b)
nonmetals
c)
metalloids
d)
noble gases
79.
Each column in the periodic table is called a 
a)
period
b)
group
c)
cluster
d)
unit
80.
The atomic number tells you what?
a)
number of electrons
b)
number of protons
c)
number of neutrons
d)
both electrons and protons in an atom.
81.
Elements which are shiny, conduct electricity and heat are called
a)
metal
b)
nonmetal
c)
metalloid
d)
nonexistent
82.
Which is a halogen?
a)
Helium
b)
Chlorine
c)
Oxygen
d)
Neptune
83.
Which is an alkali metal?
a)
Magnesium
b)
Iron
c)
Sodium
d)
Europium
84.
In the modern periodic table elements are arranged by:
a)
atomic mass
b)
atomic number
c)
valence electrons
d)
number of isotopes
85.

Which one is NOT TRUE about isotopes of an element?

a)

The amount of protons stays the same.

b)

The amount of neutrons may be different

c)

The mass changes based on the total of protons and neutrons

d)

A new element is made with every neutron added.

86.

The _______________electrons are the electrons on the outer most energy level of the atom.

a)

valence

b)

core

c)

excited

d)

ground state

87.

Elements of the same ______________ have the same number of valence electrons, which determines the elements chemical properties.

a)

Period

b)

Row

c)

Group

88.

Group 1: These metals are extremely reactive. They all have one valence electron. They are shiny and silver in color. They are soft and can be cut with a knife.

a)

Transition Metals

b)

Alkali Metals

c)

Alkaline Metals

d)

Lanthanides

89.

Group 2: Slightly less reactive because they have 2 valence electrons. They are silver colored and more dense that Group 1 metals.

a)

Transition Metals

b)

Alkali Metals

c)

Alkaline-earth Metals

d)

Actinides

90.

Group 17: All nonmetals. Very reactive. Poor conductors of heat and electricity. Tend to form salts with metals. Example NaCl: sodium chloride which is known as table salt. These elemtns have 7 valence electrons (Group # minus 10).

a)

Boron Group

b)

Oxygen Group

c)

Nitrogen Group

d)

Halogens

91.

Group 18: Unreactive nonmetals. All are colorless, odorless gases at room temperature. These elements have a full outer energy level, usually 8 valence electrons, except for Helium which only has 2 valence electrons.

a)

Nitrogen Group

b)

Oxygen Group

c)

Noble Gases

d)

Halogens

92.
How many PERIODS does the Periodic Table have?
a)
1
b)
7
c)
8
d)
18
93.
How many GROUPS does the Periodic Table have? 
a)
1
b)
5
c)
7
d)
18
94.

Which pair of elements would most likely have similar properties?

a)

Calcium (Ca) and cobalt (Co)

b)

sodium (Na) and chlorine (Cl)

c)

boron (B) and phosphorus (P)

d)

oxygen (O) and sulfur (S)

95.

Valence electrons are those that are

a)

closest to the nucleus.

b)

freely floating between atoms.

c)

in the outermost energy level of the atom.

d)

unable to become involved in chemical bonding.

96.

Oxygen has six valence electrons. When forming an ion, oxygen will

a)

lose six electrons and have a charge of +6.

b)

lose six electrons and have a charge of -6.

c)

gain two electrons and have a charge is +2.

d)

gain two electrons and have a charge of -2.

97.

Look at the periodic table. What should be the charge on the ion formed by calcium?

a)

+1

b)

+2

c)

-1

d)

-2

98.

Atoms that have gained electrons form

a)

cations.

b)

anions.

c)

negions.

d)

positrons.

99.

Most elements are most stable when their outermost energy levels contain ________ electrons.

a)

2

b)

6

c)

8

d)

18

100.

Which of the following tend to gain electrons when forming ions?

a)

metalloids

b)

metals

c)

nonmetals

d)

cations

101.

Which of the following groups on the Periodic Table will only form ions with positive charges?

a)

Group 2

b)

Group 15

c)

Group 17

d)

Group 18

102.
What charge will a Beryllium ion have?
a)
+
b)
2+
c)
2-
d)
-
103.
A bond between a metal and nonmetal is
a)
Ionic Bond
b)
Covalent Bond
c)
Metallic Bond
104.
A bond between a metal and metal is called
a)
Ionic Bond
b)
Covalent Bond
c)
Metallic Bond
105.
Which type of bond creates a "pool" of electrons between atoms?
a)
Ionic Bonds
b)
Covalent Bonds
c)
Metallic Bonds
d)
Saving Bonds
106.
Nitrogen will ____ valence electrons when forming an ionic bond.
a)
gain 1
b)
lose 1
c)
gain 3
d)
lose 3
107.
Which of the following will have a larger radius than Zinc?
a)
Gallium
b)
Aluminum
c)
Magnesium
d)
Strontium
108.
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
109.
Which atom has the largest atomic radius?
a)
potassium
b)
rubidium 
c)
francium
d)
cesium
110.
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
111.
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.
112.
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. 
113.
Which statement correctly and completely identifies a trend?
a)
Atomic radius decreases across a period and increases down a group.
b)
Electronegativity decreases across a period and decreases down a group.
c)
Ionization energy increases across a period and increases down a group.
d)
Ionic radius increases across a period and increases down a group.
114.

Ionic bonds involve a transfer of electrons from a __________ to a ___________.

(a)  

115.

Which is the formula for aluminum oxide?

a)

AlO

b)

Al2O2

c)

Al2O3

d)

Al3O2

116.

What is the formula for calcium oxide?

a)

CaO

b)

Ca2O2

c)

CaO2

d)

Ca2O

117.

Why do transition metals get different rules for their names and formulas?

a)

atoms are larger

b)

cations have many different charges

c)

they have more protons

d)

they are rare elements

118.

What is the correct name for this compound?

a)

fluorine chlorine

b)

iron chloride

c)

iron(II) chloride

d)

iron(I) chloride

119.

What is the correct name for this formula?

a)

lead(IV) iodide

b)

lead iodide

c)

lead iodine

d)

lead(I) iodide

120.

What is the formula for iron(III) oxide?

a)

FeO

b)

Fe(III) O

c)

Fe2O3

d)

Fe3O2

121.

What is the name of this ion?

a)

fluorine 3

b)

iron(III) ion

c)

iron(III)

122.

What is the name of this ion?

a)

copper(I) ion

b)

copper

c)

copper(+1) ion

123.

What is the formula for copper(I) oxide?

a)

Cu2O

b)

CuO

c)

CO

d)

C2O

124.

What is the name of this compound? Na2S

a)

nitrogen(II) sulfide

b)

sodium(II) sulfide

c)

sodium sulfide

d)

sodium(I) sulfide

125.
When naming ionic compounds with transition metals you need to include roman numerals to show the _____ of the metal..
a)
atomic number
b)
mass number
c)
charge
d)
ionization energy
126.

In the compound TiO2, Titanium has a charge of

a)

+4

b)

+3

c)

+2

d)

+1

127.
What is the NAME of...
CrN
a)
chromium (II) nitride
b)
chromium (III) nitride
c)
chromium nitride
d)
chromium (I) nitride
128.
The name of the compound NH4F is
a)
Nitrogen hydrogen fluorine
b)
Ammonium Fluoride
c)
Ammonia Fluoride
d)
Nitrogen tetrahydride fluoride
129.
The name of Al₂(SO₄)₃ is
a)
aluminum sulfur oxide
b)
aluminum sulfate
c)
aluminum trisulfate
d)
aluminum (III) sulfate
130.
The name of Fe(OH)₂ is
a)
iron oxide
b)
iron hydroxide
c)
iron (II) hydroxide
d)
iron dihydroxide

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