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Chem A Final Prep

Total questions: 88

Worksheet time: 2hrs 34mins

Name
Class
Date
1.
How many electrons can the first energy level hold?
a)
1
b)
2
c)
8
d)
0
2.
Which particles are found in the nucleus
a)
electrons and protons
b)
neutrons and protons
c)
neutrons and electrons
d)
footballs and soccer balls
3.
Which particles are found in the nucleus
a)
electrons and protons
b)
neutrons and protons
c)
neutrons and electrons
d)
footballs and soccer balls
4.
Atomic mass - Atomic Number =
a)
protons
b)
neutrons
c)
electrons
d)
Average Mass
5.
Found in the nucleus of the atom
a)
electrons only
b)
protons only
c)
neutrons and protons
d)
neutrons and electrons
6.
How many neutrons does this isotope of lithium have?
a)
8
b)
3
c)
4
d)
5
7.
What does the 6 represent above the C
a)
Symbol 
b)
Name 
c)
Mass Number 
d)
Atomic Number 
8.
An element is defined by its number of 
a)
protons
b)
electrons
c)
neutrons
d)
protons + electrons
9.
Which of the subatomic particles is the lightest
a)
all have the same mass
b)
protons 
c)
neutrons 
d)
electrons
10.
Which of the subatomic particles is the heaviest?
a)
electrons 
b)
protons 
c)
neutrons 
d)
protons and neutrons have equal mass
11.
Particles in an atom's nucleus that are neutral and have no charge are 
a)
megatrons. 
b)
electrons.
c)
neutrons.
d)
protons. 
12.
A neutral atom of the element sodium has 11 protons and ____ electrons.
a)
22
b)
23
c)
8
d)
11
13.
What atom matches this electron configuration?
1s22s22p63s23p64s23d10
a)
Zinc
b)
Copper
c)
Nickel
d)
Germanium
14.
What atom matches this electron configuration?
1s22s22p63s2
a)
Neon
b)
Magnesium
c)
Aluminum
d)
Potassium
15.
How many electrons can the first energy level hold?
a)
1
b)
2
c)
8
d)
0
16.
What do you start electron configuration with?
a)
1s2
b)
1d10
c)
1f14
d)
1p6
17.
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
18.

Valence electrons are defined a the ...........

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

19.

When atoms _____________ energy, their electrons move to higher energy levels. These electrons _____________ energy by emitting light when they return to lower energy levels.

a)

lose, absorb

b)

absorb, lose

c)

lose, lose

d)

absorb, absorb

20.

How many electrons can f orbital hold?

a)

2

b)

6

c)

10

d)

14

21.

How many orbitals are in the p block.

a)

1

b)

3

c)

6

d)

10

22.
Which section of the spectrum is the ONLY one we can see?
a)
X-rays
b)
Visible Light
c)
Gamma Rays
d)
Ultraviolet Rays
23.
Which of the following electromagnetic waves is given off as heat? 
a)
Radio Waves
b)
Infrared Rays
c)
Visible Light
d)
Gamma Rays
24.
The _______________ determines the color of visible light. 
a)
wavelength
b)
speed
c)
amplitude
d)
light
25.
As the frequency of an electromagnetic wave increases, the amount of energy in that wave...
a)
increases.
b)
decreases.
c)
stays the same.
26.
High frequency waves have _________ wavelengths.
a)
varying
b)
long
c)
the same
d)
short
27.
The distance between two crests or two troughs of a wave is called:
a)
frequency
b)
amplitud
c)
wavelength
d)
hertz
28.
All electromagnetic waves have the same...
a)
frequency
b)
speed
c)
wavelength
d)
energy
29.
A wave with a large wavelength will have a ______ frequency and _____ energy
a)
high, low
b)
high, high
c)
low, high
d)
low, low
30.

How many electrons can the first energy level hold?

a)

2

b)

8

c)

18

d)

10

31.

How many electrons can the 2nd energy level hold?

a)

2

b)

8

c)

18

d)

10

32.

How many electrons can the 3rd energy level hold?

a)

2

b)

8

c)

18

d)

10

33.

Which energy shell do we look to determine the valence electrons?

a)

The closest to nucleus that has electrons

b)

The farthest from the nucleus that has electrons

c)

Always the 3rd shell

d)

All 3 shells

34.

Boron has 5 electrons, how many valence electrons

a)

3

b)

5

c)

2

d)

8

35.

Fluorine has 9 electrons, how many does it have in its valence shell?

a)

7

b)

2

c)

8

d)

9

36.

Fluorine has 9 electrons, how many more valence electrons does it want to reach its octet?

a)

7

b)

2

c)

8

d)

1

37.
How do you determine the number of valence electrons an element has?
a)
Look at its period
b)
Look at its group
c)
Look at its atomic number
d)
Look at its atomic mass
38.

How many electrons does Calcium (Ca) need to lose to satisfy the octet rule?

a)

1

b)

2

c)

3

d)

4

39.

This atom will

a)

lose 2 electrons

b)

gain 2 electrons

c)

lose 6 electrons

d)

gain 6 electrons

e)

do nothing

40.

This atom will

a)

lose 1 electron

b)

gain 1 electron

c)

lose 7 electrons

d)

gain 7 electrons

e)

do nothing

41.

This atom will

a)

gain 1 electron

b)

lose 1 electron

c)

gain 7 electrons

d)

lost 7 electrons

e)

do nothing

42.

What charge will this atom have when it satisfies the octet rule?

a)

+2

b)

-2

c)

+6

d)

-6

e)

8

43.
What is the charge on a chloride ion?
a)
-1
b)
1
c)
+2
d)
+1
44.
Magnesium bromide is an ionic compound with the chemical formula MgBr₂.  What does the "2" tell you?
a)
There are 2 bromide ions for every magnesium ion
b)
Bromide has a 2- charge
c)
Bromide has a 2+ charge
d)
There are 2 magnesium ions to every bromide ion
45.
In what form can an ionic compound conduct electricity?
a)
when dissolved in water
b)
as a solid
c)
as a crystal
d)
when warmed slightly
46.
Elements in Group 1 lose one electron to form ions with a _________________ charge.
a)
1+
b)
2+
c)
0
d)
1-
47.
Why do ionic bonds form?
a)
so the number of protons equals the number of electrons
b)
to fill the outermost energy level
c)
so an atom can become unstable
48.
Atoms that gain electrons become...
a)
negatively charged
b)
positively charged
c)
remain neutrally charged
d)
21
49.
The attraction between oppositely charged ions is called a(n) _______________.
a)
ionic bond
b)
polyatomic ion
50.
In order to have a stable arrangement of 8 valence electrons, metal atoms are likely to _________electrons.
a)
gain
b)
lose
51.
If an oxygen atom has 8 protons (+) and 10 electrons (-), what is it's charge?
a)
O10-
b)
O8+
c)
O2-
d)
O10+
52.
What would be the proper chemical formula for combining Al3+ and Cl- :
a)
AlCl3
b)
Al3Cl
c)
AlCl
d)
Al3Cl3
53.
Name the following ionic compound: BeCl2
a)
beryllium chlorine
b)
beryllium II chloride
c)
beryllium chloride
d)
beryllium dichloride
54.
name the following ionic compound: NaF
a)
nitrogen fluorine
b)
sodium fluoride
c)
nitrogen fluoride
d)
sodium fluorine
55.
Name the following ionic compound: Cs2S
a)
cesium sulfide
b)
cesium sulfate
c)
cesium II sulfate
d)
cesium II sulfide
56.
Name the following ionic compound: MgSO4
a)
magnesium sulfoxide
b)
magnesium sulfide
c)
magnesium sulfate
d)
magnesium oxide
57.
Name the following ionic compound: LiNO3
a)
lithium nitrate
b)
lithium III nitrate
c)
lithium nitride
d)
lithium oxide
58.
Name the following ionic compound: Cr(NO2)3
a)
chromium nitrite
b)
chromium nitride
c)
chromium III nitride
d)
chromium III nitrite
59.
Name the following compound: FeCl3
a)
iron chloride
b)
iron III chloride
c)
iron chlorate
d)
iron III chlorate
60.
This could be the dot diagram of
a)
Ne
b)
H
c)
C
d)
F
61.
How are covalent bonds explained?
a)
When one atom takes the other atom's electron
b)
When the atom shares an electron with an another atom
c)
When the two nucleus merge
d)
When the neutrons leave the nucleus
62.
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
63.
A covalent bond in which electrons are shared unequally is:
a)
polar
b)
a double bond
c)
ionic
d)
polyatomic
64.
What is the correct formula for this molecule?
a)
NH
b)
N3H
c)
NH3
d)
NH4
65.
Atoms that share three pairs of electrons form a ______ covalent bond.
a)
single
b)
double
c)
triple
66.
In covalent bonds, electrons are ___________.
a)
transferred
b)
gained
c)
lost
d)
shared
67.
How many valence electrons are in Phosphorus?
a)
15
b)
4
c)
5
d)
31
68.
According to the octet rule most elements need _______ valence electrons.
a)
2
b)
8
c)
6
d)
18
69.
Hydrogen needs _____ electrons in its valence shell to be stable.
a)
4
b)
6
c)
8
d)
2
70.

Which is the correct molecular structure for carbon dioxide?

a)
b)
c)
d)
71.

How many total valence electrons are participating in bonding in the molecule above?

a)

8

b)

4

c)

2

d)

3

72.

Choose the electron dot diagram that correctly shows the bonding in methane CH4.

a)

A

b)

B

c)

C

d)

D

73.

Which electron dot structure is correct for the element chlorine (Cl2)?

a)

A

b)

B

c)

D

d)

D

74.

Which electron dot structure is correct for carbon dioxide CO2?

a)

A

b)

B

c)

C

d)

D

75.

Which two elements are most likely to form a covalent bond?

a)

C and Ca

b)

P and F

c)

Sr an S

d)

Li and Cl

e)

Al and I

76.
Which has the greater EN: 
Cl or Al?
a)
Cl
b)
Al
77.
Which of the following will have a lower ionization energy than Scandium (Sc)?
a)
Helium (He)
b)
Titanium (Ti)
c)
Calcium (Ca)
d)
Magnesium (Mg)
78.
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
79.
Atoms that have a high electronegativity, _______________.
a)
give up their electrons more easily.
b)
hold on to their electrons more tightly.
c)
have more electron shells.
80.
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. 
81.
Ionization energy is...
a)
the energy required to add an electron to a specific atom
b)
how much energy it takes to remove an electron from an atom
c)
the energy required to shield the outer electrons from the nucleus
d)
a measure of the ability of an atom to attract electrons
82.
The element with the largest electronegativity in the halogens is - 
a)
At
b)
F
c)
Cl
d)
Br
83.

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

84.
Electronegativity __________ from left to right within a period and __________ from top to bottom within a group.
a)
decreases, increases 
b)
increases, increases
c)
increases, decreases 
d)
stays the same, increases
85.

What all of the following are true of an ion EXCEPT.

a)

It shares electrons with other ions

b)

an atom that has an electric charge

c)

It could have lost electrons

d)

It could have gained electrons

86.

All of the following are true of an electron EXCEPT.

a)

negatively charged subatomic particle

b)

found in electron cloud around the atom

c)

Much smaller than a neutron

d)

About the same size as proton

87.

All of the following are true of a neutron EXCEPT.

a)

subatomic particle with no charge

b)

found in the electron cloud of an atom

c)

About the same size as a proton

d)

Much larger than an electron

88.

All of the following are true of a proton EXCEPT.

a)

A positive subatomic particle

b)

About the same size as an electron

c)

bout the same size as a neutron

d)

found in the nucleus of an atom

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