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2nd Six Weeks - Test

Total questions: 108

Worksheet time: 9hrs 33mins

Name
Class
Date
1.

3 subatomic particles that makeup an atom.

a)

Positive, negative, neutral

b)

Positron, Neutral, Electron

c)

Proton. Neutron, Electron

2.

This subatomic particle has a positive charge.

a)

Proton

b)

Neutron

c)

Electron

3.

The subatomic particle holds the atom together.

a)

Proton

b)

Neutron

c)

Electron

d)

Nucleus

4.

The subatomic particle that identifies the element.

a)

Proton

b)

Positron

c)

Neutron

d)

Electron

5.

The subatomic particle that determines reactivity.

a)

Electron

b)

Proton

c)

Shell

d)

Neutron

6.

A neutron has a _____ charge.

a)

Positive

b)

Negative

c)

Neutral

d)

1/2 charge

7.

A electron has a ______ charge.

a)

No charge

b)

Positive

c)

Neutral

d)

Negative

8.

The atomic number tells you the number of

a)

Neutrons

b)

Protons

c)

Neutrons plus Protons

9.

An isotope has different number of ______.

a)

Neutrons

b)

Protons

c)

Electrons

d)

Nucleus

10.

Bohr stated that _______ are found in shells orbiting the nucleus.

a)

Electrons

b)

Protons

c)

Neutrons

d)

Clouds

11.

A piece of paper contains_______ of atoms.

a)

Hundreds

b)

Tens

c)

Millions

12.
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
13.
A negative ion is a 
a)
cation
b)
anion
14.
When an atom LOSES an electron it is a
a)
cation
b)
anion
15.

What two particles determine the mass number?

a)

Protons and electrons

b)

Electrons and neutrons

c)

Protons and neutrons

16.
a)
beaker
b)
cup-with-lines
c)
wash bottle
d)
graduated cylinder
17.
a)
Erlenmeyer flask
b)
beaker
c)
wash bottle
d)
watch glass
18.
a)
graduated cylinder
b)
beaker
c)
Erlenmyer flask
d)
bunsen burner
19.

The following piece of glassware is used to ...

a)

measure a precise volume of a liquid

b)

prepare solutions to an accurate volume

c)

hold and mix chemicals without spilling

20.

A measurement of how strongly gravity pulls on an object is called

a)

weight

b)

mass

21.

Is this a physical or chemical change?

a)

Physical

b)

Chemical

22.

This is an example of _____ change.

a)

Physical

b)

Chemical

23.
a)
heterogeneous mixture
b)
homogeneous mixture
24.
Define Atom
a)
It is the smallest piece of an element that still represents that element
b)
Is an element has the electrons in their electron cloud
c)
A positively charged isotope
25.

Nonmetals tend to

a)

gain electrons

b)

lose electrons

26.

Metals tend to

a)

gain electrons

b)

lose electrons

27.
When metals bond with non-metals they form what type of bonds
a)
covalent
b)
ionic
c)
cooperative
d)
lewis
28.
How do the following two elements bond together?
Cr3+  O2-         
a)
CrO
b)
Cr3O2
c)
Cr2O3
d)
CrO3
29.
How do the following two elements bond together?
Na1+  F1-         
a)
NaF
b)
NaF3
c)
Na3F
d)
Na1F2
30.
How do the following two elements bond together?
K1+  S2- 
a)
KS
b)
K8S
c)
K6S3
d)
K2S
31.
How do the following two elements bond together?
Al3+  O2-         
a)
AlO
b)
Al2O3
c)
Al3O6
d)
Al3O2
32.
The first step in naming an ionic compound is always...
a)
Naming the anion
b)
Changing the ending to -ide
c)
Naming the cation
d)
Writing the cation charge
33.
Valence electrons are: 
a)
Electrons farthest away from the nucleus
b)
Electrons closest to the nucleus
c)
Electrons that just come and go - they don't stay with the atom
d)
Electrons in the second shell
34.

Anions are formed from

a)

Metals giving away electrons

b)

Non-metals receiving additional electrons

c)

Non-metals giving away electrons

d)

Cations losing their charge

35.
Name the compound using appropriate rules:
FeCl3
a)
Chloride Iron
b)
Iron III Chloride
c)
Chloride III Iron
d)
I have no clue
36.

The name of FeCl₂ is

a)

iron chloride

b)

iron (II) chloride

c)

iron (I) chloride

d)

iron dichloride

37.
Because the overall charge in a compound must be ____________, the charge of iron in Fe2O3 can be calculated as 3+.
a)
2+
b)
1+
c)
0
d)
1-
38.

Each row on the periodic table represents:

a)

an energy level

b)

a sublevel

c)

an electron

39.

There are 4 different types of subshells(orbitals) s,p,d,f

a)

true

b)

false

40.

What is the maximum number of electrons that an S orbital can have?

a)

1 electron

b)

2 electrons

c)

3 electrons

d)

4 electrons

41.
How many electrons can the d sublevel hold?
a)
8
b)
10
c)
2
d)
4
42.

Which area on the periodic table represents the electrons in the "d" sublevel?

a)

representative elements

b)

columns 3-8

c)

rare earth elements

d)

transition elements

43.
How many electron can be found in a p orbital?
a)
2
b)
3
c)
4
d)
6
44.
How many electrons does Si contain? (click to see image)
a)
14
b)
28
c)
2
d)
4
45.
How many valence electrons does Chlorine have?
a)
5
b)
2
c)
7
d)
5
46.

How many electrons can the f sublevel hold?

a)

14

b)

10

c)

8

d)

2

47.

Which atom has the largest atomic radius?

a)

potassium

b)

rubidium

c)

francium

d)

cesium

48.
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.
49.
Atomic radius generally increases as we move __________.  
a)
down a group and from right to left across a period 
b)
up a group and from left to right across a period 
c)
down a group and from left to right across a period 
d)
up a group and from right to left across a period 
50.
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. 
51.

Ionization energy is the energy needed to...

a)

remove an electron

b)

remove a proton

c)

gain an electron

d)

gain a proton

52.
The element with the largest electronegativity in the halogens is - 
a)
At
b)
F
c)
Cl
d)
Br
53.
a)
Periods
b)
Groups
54.
a)
Periods
b)
Groups
55.
a)
energy levels
b)
valence electrons
c)
protons
d)
neutrons
56.
a)
energy levels
b)
valence electrons
c)
protons
d)
neutrons
57.
a)
Group 1
b)
Group 17
c)
Group 2
d)
Group 18
58.
a)
Group 1
b)
Group 17
c)
Group 18
d)
Group 2
59.
a)
Group 1
b)
Group 17
c)
Group 18
d)
Group 2
60.
a)
Metals
b)
Nonmetals
c)
Metalloids
61.
a)
Metals
b)
Nonmetals
c)
Metalloids
62.
a)
Metals
b)
Nonmetals
c)
Metalloids
63.
a)
Metals
b)
Nonmetals
c)
Metalloids
64.
a)
Metals
b)
Nonmetals
c)
Metalloids
65.
a)
Metals
b)
Nonmetals
c)
Metalloids
66.

Who invented the Periodic Table?

a)

Mendeleev

b)

Bohr

c)

Lewis

d)

Democritus

67.

What happens to the number of shells as you move down a group?

a)

They decrease by 1

b)

They increase by 1

c)

Nothing

68.
The majority of elements on the periodic table are
a)
man made.
b)
nonmetals.
c)
metals.
d)
gases.
69.
What does the 6 represent?
a)
atomic mass
b)
atomic number
c)
element name
d)
chemical symbol 
70.
What does 12.011 represent?
a)
atomic mass
b)
atomic number
c)
element name
d)
chemical symbol 
71.

Which change creates a NEW substance?

a)

Physical change

b)

Chemical Change

72.

The wick of a candle burning is a

a)

chemical change

b)

physical change

73.

Wax in a candle melting, the wax can be reformed to its original shape.

a)

physical change

b)

chemical change

c)

proton

74.
a)

Homogeneous

b)

Heterogeneous

75.
Elements in the same column of the periodic table always have the same # of _______ as one another.
a)
Protons
b)
Neutrons
c)
Electrons
d)
Valence Electrons
76.
How many valence electrons are found in atoms of group 14?
a)
4
b)
3
c)
14
d)
16
77.
Which group has the greatest number of valence electrons?
a)
1
b)
14
c)
18
d)
16
78.

True or False: Atoms that have a valence electrons of less than eight are not stable.

a)

true

b)

false

79.

How many valence electrons does Potassium Have?

a)

1 Valence electron

b)

2 Valence electron

c)

3 Valence electron

d)

4 Valence electron

e)

5 Valence electron

80.

How many valence electrons does Lithium Have?

a)

1 Valence electron

b)

2 Valence electron

c)

3 Valence electron

d)

4 Valence electron

e)

5 Valence electron

81.

This picture represents which of the following?

a)

Element

b)

Compound

c)

Molecule

82.
This picture represents which of the following?
a)
element
b)
compound
c)
mixture
83.

What is the correct chemical formula for magnesium chloride? Magnesium is in group 2 and chlorine is in group 17.

a)

MgCl

b)

Mg2Cl

c)

MgCl2

d)

MgCl3

e)

Mg3Cl

84.

Name the following compound: CaCl2

a)

calcium dichloride

b)

calcium chloride

c)

calcium (II) chloride

d)

carbon chloride

e)

None of these.

85.

Name the following compound: Na2S

a)

sodium sulfide

b)

disodium sulfide

c)

sodium sulfur

d)

sodium monosulfide

e)

None of these.

86.

What is the formula for: magnesium sulfide. Magnesium is in group 2 and sulfur is in group 16.

a)

MgS

b)

Mg2S2

c)

MnS

d)

MgS2

e)

None of these.

87.

What is the formula for: aluminum phosphide. Aluminum is in group 13 and phosphorous is in group 15.

a)

AlP

b)

AlP3

c)

Al3P3

d)

Al3P2

e)

None of these.

88.

What is the name of the compound CuO? Cu is a transition metal and O is in group 16.

a)

Copper(II) oxide

b)

Copper(I) oxide

c)

Copper oxide

d)

Copper(II) oxate

89.

What is the name of the compound PbCl4? Pb is a transition metal and Cl is in group 17.

a)

Lead chloride

b)

Lead chlorate

c)

Lead(IV) chloride

d)

Lead(IV) chlorate

90.
What electron configuration matches an oxygen atom?
a)
1s22s22p63s2, 3p64s23d104p5
b)
1s22s22p4
c)
1s22s22p6
d)
1s22s22p63s23p64s23d1
91.
The electron configuration of an atom is 1s22s22p6.  The number of electrons in the atom is 
a)
3
b)
6
c)
8
d)
10
92.

How many electrons are in this element?

1s2 2s2 2p6 3s2

a)

2

b)

12

c)

8

d)

6

93.

What energy level are the valence electrons located?

1s2 2s2 2p6 3s2

a)

1

b)

unknown

c)

2

d)

3

94.

The s and p represent?

1s2 2s2 2p6 3s2

a)

energy levels

b)

sub shells

c)

valence electrons

d)

protons

95.

The d subshell begins in this energy level.

a)

3

b)

4

c)

1

96.

The f subshell begins in this energy level.

a)

1

b)

2

c)

3

d)

4

97.

An ionic compound is between

a)

2 metals

b)

2 nonmetals

c)

a metal and a nonmetal

d)

metalloids

98.

In an ionic compound electrons are

a)

shared

b)

transferred

c)

equalized

d)

exploded

99.

When the number of this subatomic particle changes a new element is formed

a)

electrons

b)

neutrons

c)

protons

d)

valence electrons

100.

Why are noble gases unreactive?

a)

They are gases

b)

They have a full outer shell of electrons

c)

The inner shell of electrons is always 2

d)

They are in the d subshell

101.

Which group is referred to as Alkali Metals?

a)

3

b)

1

c)

7

d)

17

102.

What is the name of the family that is highlighted?

a)

Alkali Metal Family

b)

Halogen Family

c)

Noble Gas Family

d)

Transition Metal Family

103.
Name group 2A on the periodic table.
a)
alkali metals
b)
alkaline earth metals
c)
noble gases
d)
transition metals
104.
Name group 8A on the periodic table.
a)
alkali metals
b)
alkaline earth metals
c)
transition metals
d)
noble gases
105.

Which elements have 1 valence electron?

a)

period 1

b)

group 1

c)

group 4

106.

Which element has 3 valence electrons?

a)

A

b)

B

c)

E

d)

C

107.
Which elements are in the same period?
a)
A & F
b)
F, B & D
c)
E & D
d)
F & B
108.

How many valence electrons do the atoms of elements in group 13 have (the Boron Group)?

a)

3

b)

5

c)

8

d)

13

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