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Chemistry Semester 1 Review

Total questions: 205

Worksheet time: 3hrs 15mins

Name
Class
Date
1.
The splitting of a nucleus into smaller nuclei is
a)
fusion
b)
fission
c)
half-life
d)
gamma radiation
2.
The product of nuclear fission includes
a)
neutrons and electrons
b)
several nuclei and neutrons
c)
several nuclei and electrons
d)
several nuclei and protons
3.
What is a chain reaction?
a)
When electrons travel are emitted causing electricity
b)
When a nuclear fission reaction occurs, the protons emitted can strike other nuclei in the sample, and cause them to split
c)
When a nuclear fission reaction occurs, the neutrons emitted can strike other nuclei in the sample, and cause them to split
d)
When a nuclear fission reaction occurs, the electrons emitted can strike other nuclei in the sample, and cause them to split
4.
Two nuclei with low masses are combined to form one nucleus of larger mass is called what?
a)
Nuclear fission
b)
Nuclear fussion
c)
Nuclear half-life
d)
Half-life
5.
This is an example of...
a)
Fission  reaction
b)
Fusion reaction
c)
Decomposition reaction
d)
Decay
6.
Which type of nuclear radiation is being emitted here?
a)
Alpha
b)
beta
c)
gamma 
d)
none
7.
Which type of nuclear radiation is being emitted here?
a)
Alpha
b)
beta
c)
gamma 
d)
none
8.
What makes something radioactive?
a)
elements with an atomic number above 81
b)
an unstable nucleus
c)
contaminated sewage
d)
It decays over time
9.
The three types of nuclear radiation in increasing order of penetrating power are ____.  
a)
  alpha, beta, gamma 
b)
X ray, beta, gamma
c)
alpha, gamma, beta 
d)
X ray, gamma, beta 
10.
When a nucleus undergoes nuclear decay by gamma rays, the atomic number of the element....
a)
remains the same
b)
  decreases by one.
c)
increases by one.
d)
increases by two.
11.

finish the equation


22688Ra --> ____ + 22688Ra

a)

42He

b)

0-1e

c)

y

12.
What do these isotopes of carbon all have in common?
a)
neutrons & mass number
b)
atomic number and neutrons
c)
atomic number and electrons
d)
protons, atomic number, and mass number
13.
How many neutrons does the isotope of lithium have?
a)
8
b)
3
c)
4
d)
5
14.
Isotopes are atoms of the same element with different #’s of __________ & therefore different __________.
a)
n0 ;  atomic #’s
b)
p+ ; atomic #’s
c)
e- ; atomic masses
d)
n0 ; atomic masses
15.
If 10 mg of iodine 131 is given to a patient, how much is left after 24 days? The half-life of iodine-131 is 8 days.
a)
1.25mg
b)
1.25g
c)
10g
d)
10mg
16.
The half-life of strontium-90 is 25 years. How much strontium-90 will remain after 100 years if the initial amount is 4.0 g?
a)
3.0g
b)
0.25mg
c)
0.3g
d)
0.25g
17.

Convert 675 mL to L

a)

6500 L

b)

0.675 L

c)

67.5 L

d)

675,000 L

18.
Convert from meters to cm:  9 meters
a)
900 cm
b)
90 cm
c)
0.9 cm
d)
0.09 cm
19.
Convert 17 m to cm:
a)
0.17 cm
b)
0.017 cm
c)
1,700 cm
d)
170 cm
20.
2804 mg = ___________ g
a)
0.2804
b)
2.804
c)
28.04
d)
280.4
21.
What is the correct SI unit for mass?
a)
Kilograms
b)
newtons
c)
pounds
d)
grams
22.
The SI unit for temperature is __?__.
a)
degree fahrenheit  (° F)
b)
degree celsius  (° C)
c)
kelvin  (K)
d)
degree centigrade  (°C)
23.

The SI unit for time is the __?__.

a)

hours (h)

b)

liter (L)

c)

gram (g)

d)

second (s)

24.

What SI unit is used to measure length?

a)

meters

b)

liters

c)

centimeters

d)

kilograms

25.
How many significant figures: 216 m
a)
1
b)
2
c)
3
d)
0
26.
How many significant figures: 2016 m
a)
1
b)
2
c)
3
d)
4
27.
How many significant figures: 153.0 mL
a)
1
b)
2
c)
3
d)
4
28.
How many significant figures: 0.012 km
a)
1
b)
2
c)
3
d)
4
29.
How many significant figures: 1000 mL
a)
1
b)
2
c)
3
d)
4
30.
How many significant figures: 100.000 cL
a)
1
b)
3
c)
5
d)
6
31.

The atomic number is the same as......

a)

the number of protons

b)

the number of electrons

c)

the number of neutrons

d)

the number of protons plus neutrons

32.

The mass number is the same as......

a)

the number of protons

b)

the number of electrons

c)

the number of neutrons

d)

the number of protons plus neutrons

33.

If we are talking about the isotope carbon-14, the mass number of this isotope is.....

a)

12

b)

13

c)

14

d)

6

34.

Isotopes of an element have different numbers of ......

a)

protons

b)

neutrons

c)

electrons

35.

The number of these particles determines what element an atom represents.

a)

protons

b)

neutrons

c)

electrons

d)

photons

36.

Whether an atom's nucleus is stable is determined by:

a)

the ratio of protons to neutrons

b)

the ratio of protons to electrons

c)

the ratio of neutrons to electrons

d)

the number of electrons in each energy level

37.

To determine the charge of an atom you should:

a)

compare protons and electrons

b)

combine protons and neutrons

c)

compare protons and neutrons

d)

combine neutrons and electrons

38.

Which particle(s) has/have a positive (+) charge

a)

protons

b)

neutrons

c)

electrons

d)

photons

39.

Which particle(s) has/have a neutral (0) charge?

a)

protons

b)

neutrons

c)

electrons

d)

photons

40.

If you change the number of electrons in an atom, what are possible effects? (check all that apply)

a)

nucleus may become more or less stable

b)

the atomic mass will change

c)

the charge of the atom will change

d)

it will become a different element

41.
Why are ions formed?
a)
To make our lives difficult
b)
Because atoms want 8 valence electrons
c)
Because atoms have the same number of protons and electrons
d)
Because atoms gained neutrons
42.
An atom becomes _________ when it gains electrons.
a)
Positive
b)
Negative
c)
Neutral
d)
Invinsible
43.
Elements on the LEFT side of the periodic table will most likely form:
a)
Positive ions
b)
Negative ions
c)
Neutral Ions
d)
None of these
44.
An atom becomes _______ when it loses electrons.
a)
Positive
b)
Negative
c)
Neutral
d)
Invinsible
45.
When an atom loses a valence electron, it becomes a(n) _____________ ion.
a)
positive
b)
negative
c)
neutral
d)
polyatomic
46.
If an element has 3 valence electrons, what charge will likely form on its ion ?  Hint:  It will lose those electrons.  What happens to the charge when it loses 3 electrons?
a)
+3
b)
+5
c)
-3
d)
-5
47.
What is the charge of an atom that has gained one electron?
a)
-1
b)
-2
c)
+1
d)
+2
48.
What is the charge of an atom that has lost one electron?
a)
-1
b)
-2
c)
+1
d)
+2
49.

JJ Thomson was credited for the discovery of the

a)

center of the universe

b)

proton

c)

electron

d)

neutron

50.

The atomic model associated with Thomson is the

a)

plum pudding model

b)

nuclear mode.

c)

planetary model

d)

the electron cloud model

51.

Which device did JJ Thomson use to discover the electron?

a)

X-ray machine

b)

scanning tunneling electron microscope

c)

spectrometer

d)

cathode ray tube

52.

Which is a finding attributed to Rutherford's Gold Foil Experiment?

a)

atoms are indivisible and have a dense positive nucleus.

b)

atoms are divisible and have multiple layers of electrons scattered uniformly about the atom.

c)

atoms are like plum pudding with positive and negative charges uniformly scattered throughout the atom.

d)

atoms are mostly empty space with a dense positive nucleus.

53.

Rutherford used what type of radiation to bombard the gold foil?

a)

alpha particles.

b)

beta particles.

c)

gamma radiation.

d)

neutrinos.

54.

What did Rutherford expect to happen to the alpha particles bombarding the gold foil?

a)

they would be absorbed by the gold.

b)

they would be deflected by the gold.

c)

they would go completely through the gold foil.

d)

the would be changed into beta radiation by the gold foil.

55.

Which scientist first theorized atoms cannot be created destroyed or divided?

a)

Niels Bohr

b)

Richard Feynman

c)

Democritus

d)

Ernest Rutherford

56.

Check all of Daltons Postulates

a)

All matter is composed of extremely small particles called atoms

b)

All atoms of a given element are identical, having the same size, mass, and chemical properties. Atoms of a specific element are different from those of any other element.

c)

Atoms cannot be created, divided into smaller particles, or destroyed.

d)

Different atoms combine in simple whole number ratios to form compounds.

e)

In a chemical reaction, atoms are separated, combined, or rearranged.

57.

How is the modern periodic table arranged?

a)

By increasing atomic mass

b)

By increasing atomic number

c)

Alphabetically

d)

By increasing number of protons

58.

Aluminum

a)

Metal

b)

Non-metal

c)

Metalloid

59.

Atoms in the same family have

a)

Similar masses

b)

The same number of valence electrons

c)

Different properties

d)

The same number of protons

60.

Most metals are NOT

a)

Ductile

b)

Good conductors

c)

Gases at room temperature

d)

Shiny

61.

What is the name of group number 1?

a)

halogens

b)

noble gases

c)

alkali metals

d)

alkaline earth metals

62.

where are the metaloids found

a)

far left, vertical

b)

stair step/diagonal

c)

far right horizontal

d)

at the bottom

63.

What group number are the halogens found?

a)

18 (8A)

b)

1

c)

2

d)

17 (7A)

64.

Periodic law states that the elements are arranged according to their atomic ________ so that elements with similar chemical properties are in the same ________ and properties repeat periodically.

a)

numbers, rows

b)

masses, rows

c)

masses, column

d)

numbers, column

65.

A grouping of elements based on similar chemical properties, arranged by columns in the periodic table; also known as a group

a)

family

b)

period

c)

row

d)

isotope

66.

A row on the Periodic Table of Elements

a)

family

b)

period

c)

row

d)

isotope

67.

Metals (select all that apply)

a)

are found on the right side of the periodic table.

b)

are found on the left side of the periodic table.

c)

are good conductors of heat and electricity.

d)

are brittle.

e)

are malleable and ductile.

68.

Nonmetals (select all that apply)

a)

are found on the right side of the periodic table.

b)

are found on the left side of the periodic table.

c)

are good conductors of heat and electricity.

d)

are brittle.

e)

can be solid, liquids, or gases at room temperature.

69.
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. 
70.
Which atom has the largest atomic radius?
a)
potassium
b)
rubidium 
c)
francium
d)
cesium
71.
As you move down a group, atomic radius increases because - 
a)
you add more and more neutrons
b)
you add more and more protons
c)
you add more and more shells (energy levels)
d)
you add more atomic mass
72.
As you move across the periodic table from left to right, the atomic radius decreases.  This is because - 
a)
the number of protons increases, so attraction to electrons increases
b)
the number of energy levels increases
c)
the number of electrons increases
d)
the atomic mass increases
73.

The lines in the emission spectrum for hydrogen are formed from ___.

a)

energy given off when the electron moves from higher energy levels to lower energy levels

b)

electrons given off as hydrogen burns

c)

protons given off when protons move from higher energy levels to lower energy levels

d)

electrons given off as hydrogen cools

74.

Which color has the highest frequency?

a)

green

b)

blue

c)

red

d)

yellow

75.

Which color has the highest energy per photon quanta?

a)

green

b)

blue

c)

red

d)

yellow

76.

Energy of a photon is ___ proportional to frequency.

a)

directly

b)

inversely

77.

Frequency of light is ___ proportional to wavelength.

a)

directly

b)

inversely

78.

When electron falls from an excited state to a ground state, (a)   is emitted by the electron.

79.

If a photon hits an atom, the electron will ___________ the energy. It is promoted from a _____ energy level to a ______ energy level.

a)

absorb; lower; higher

b)

emit; lower; higher

c)

absorb; higher; lower

d)

emit; higher; lower

80.

_____________________ is the lowest energy level an electron will occupy in an atom.

a)

ground state

b)

excited state

81.

Which of the following statements is false?

a)

The energy of a photon is directly related to its wavelength

b)

A line spectrum is produced when light is emitted from an excited atom

c)

The energy of a photon is directly related to its frequency

d)

Light is composed of photons with specific amounts of energy

82.

According to Bohr, the energy absorbed by an electron upon excitation comes in a fixed amount called

a)

exact energy

b)

fixed energy

c)

quantized energy

d)

None of the above

83.
How are electrons arranged in an atom?
a)
In groups of five
b)
In energy levels
c)
By color
d)
By shape
84.

What is a photon?

a)

A ray from the sun

b)

An electron

c)

A particle with no mass that can be thought of as a bundle of energy

d)

A particle that has the ability to blow up an atom

85.

How many valence electrons does Nitrogen Have?

a)

1 Valence electron

b)

2 Valence electron

c)

3 Valence electron

d)

4 Valence electron

e)

5 Valence electron

86.

How many valence electrons does Helium Have?

a)

1 Valence electron

b)

2 Valence electron

c)

3 Valence electron

d)

4 Valence electron

e)

5 Valence electron

87.

How many valence electrons does Hydrogen Have?

a)

1 Valence electron

b)

2 Valence electron

c)

3 Valence electron

d)

4 Valence electron

e)

5 Valence electron

88.

How many valence electrons does Magnesium Have?

a)

1 Valence electron

b)

2 Valence electron

c)

3 Valence electron

d)

4 Valence electron

e)

5 Valence electron

89.

How many valence electrons does Aluminum Have?

a)

1 Valence electron

b)

2 Valence electron

c)

3 Valence electron

d)

4 Valence electron

e)

5 Valence electron

90.
an element will always have the same number of 
a)
neutrons
b)
protons
c)
isotopes
d)
atoms
91.
What's a valence electron?
a)
electrons in the second energy level
b)
electrons in the outermost energy level
c)
the atomic number
d)
electrons in the first level
92.

According to the Octet Rule, atoms of elements react with each other in order to attain ____ electrons in their outermost energy level or shell.

a)

2

b)

4

c)

6

d)

8

e)

10

93.

Which of the following elements LOSES 1 electron in order to attain an octet?

a)

potassium

b)

calcium

c)

helium

d)

boron

e)

fluorine

94.

Do you think Carbon at the central already achieved an octet?

a)

Yes

b)

No

95.

Do you think Nitrogen at the central already achieved an octet?

a)

Yes

b)

No

96.

Which of the following states that electrons occupy orbitals of lowest energy first?

a)

Hund’s Rule

b)

Aufbau Principle

c)

Pauli Exclusion Principle

97.

This orbital diagram represents:

a)

Carbon

b)

Boron

c)

Nitrogen

d)

Oxygen

98.

This orbital diagram represents

a)

Nitrogen

b)

Oxygen

c)

Carbon

d)

Neon

99.

What is incorrect about this orbital diagram?

a)

Both arrows in the 2p box should be pointing up

b)

There are too many electrons in the 1s orbital

c)

In the 2p boxes, there should only be 1 electron in the first 2p box and one in the 2nd 2p box

d)

All the arrows should be pointing up

100.

What does the Pauli Exclusion Principle state?

a)

An orbital can only hold a maximum of 2 electrons, each with opposite spins

b)

An orbital can hold a minimum of 6 electrons, each with opposite spins

c)

An orbital can hold a maximum of 6 electrons, each with the same spin

d)

An orbital can hold a maximum of 2 electrons, each with the same spin

101.

Which orbital diagram violates of Hund's Rule?

a)

A

b)

B

c)

C

d)

D

102.

This orbital diagram represents

a)

Nitrogen

b)

Oxygen

c)

Carbon

d)

Neon

103.
What is incorrect about this orbital diagram?
a)
Both arrows in the 2p box should be pointing up
b)
There is nothing incorrect with this diagram
c)
In the 2p box there should only be 1 electron in the first 2p box and one in the 2nd 2p box
d)
All the arrows should be pointing up.
104.
What atom matches this electron configuration?
1s22s22p63s23p64s23d10
a)
Zinc
b)
Copper
c)
Nickel
d)
Germanium
105.
What electron configuration matches an oxygen atom?
a)
1s22s22p63s2, 3p64s23d104p5
b)
1s22s22p4
c)
1s22s22p6
d)
1s22s22p63s23p64s23d1
106.
The electron configuration of an atom is 1s22s22p6.  The number of electrons in the atom is 
a)
3
b)
6
c)
8
d)
10
107.
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
108.

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

109.

How many electrons can the d sublevel(orbital) hold?

a)

8

b)

10

c)

2

d)

4

110.

Why do all bonds form?

a)

to fill the outermost energy level

b)

so an atom can be unstable

c)

so the number of protons and electrons can equal.

d)

so they can gain neutrons.

111.

What two types of atoms make a covalent bond?

a)

2 nonmetals

b)

2 metals

c)

1 metal and 1 nonmetal`

112.

Ionic bonds are between

a)

metals and nonmetals

b)

2 metals

c)

2 nonmetals

113.

Water is an example of what?

a)

molecular compound (covalent compound)

b)

ionic compound

114.

Salt is an example of what?

a)

ionic compound

b)

covalent compound

115.
Covalent bonds are between...
a)
Metal and Non-metal
b)
Non-metal and Non-metal
c)
Metal and Metal
116.
How are covalent bonds formed?
a)
Sharing of electrons
b)
Transfer of electrons
117.
How are ionic bonds formed?
a)
Transfer of electrons
b)
Sharing of electrons
118.
Why do elements bond?
a)
To be friends
b)
To create a new element
c)
To become stable
119.
Where are the nonmetals located on the periodic table? 
a)
Blue
b)
Red
c)
Green
120.
In a covalent bond, one or more electrons are? 
a)
shared 
b)
lost 
c)
gained 
d)
transferred 
121.

What are the seven diatomic elements?

a)

H2, Cl2, Br2, O2, N2, I2, F2

b)

H2, Cl2, I2, F2, Hg2, Br2, Fe2

c)

H2, Cu2, Ni2, B2, O2, I2, Fe2

122.

What are diatomic elements?

a)

Elements that form two-atom molecules when not combined in a compound.

b)

Two elements that combine with one atom from each element.

c)

Elements that are always in pairs no matter what.

123.

Is O2 a diatomic element?

a)

Yes

b)

No

124.

Classify the following molecule.

a)

polar

b)

nonpolar

125.

Why is the molecule nonpolar?

a)

There are nonbonding pairs on the central atom.

b)

There are different types of elements bonded to the central atom.

c)

There are no nonbonding pairs on the central atom and all of the atoms bonded to the central atom are the same.

126.

Classify the following molecule.

a)

polar

b)

nonpolar

127.

Why is the molecule polar?

a)

There are nonbonding pairs on the central atom.

b)

There are different types of elements bonded to the central atom.

c)

There are no nonbonding pairs on the central atom and all of the atoms bonded to the central atom are the same.

128.

Classify the following molecule.

a)

polar

b)

nonpolar

129.

Why is the molecule polar?

a)

There are nonbonding pairs on the central atom.

b)

There are different types of elements bonded to the central atom.

c)

There are no nonbonding pairs on the central atom and all of the atoms bonded to the central atom are the same.

130.

Classify the following molecule.

a)

polar

b)

nonpolar

131.
F2
a)
Polar 
b)
Nonpolar 
132.
What is the VSEPR theory used to predict?
a)
Bond Strength
b)
Polarity
c)
Molecular Shape
d)
Electronegativity
133.
 A lone pair is defined as
a)
A pair of bonding electrons
b)
One non-bonding electron
c)
A pair of non-bonding electrons
d)
A pair of electrons on the central atom
134.
Which of the following shapes has an unshared pairs of electrons on the central atom? 
a)
Bipyramidal
b)
Bent
c)
Trigonal Planar
d)
Tetrahedral
135.

What shape would this have?

a)

Trigonal planar

b)

Pyramidal

c)

Tetrahedral

d)

Bent

136.
What molecular shape is the structure shown here? (H2O)
a)
tetrahedral
b)
trigonal planar
c)
bent
d)
trigonal pyramidal
137.
What is the measure of a tetrahedral bond angle?
a)
90 Degrees
b)
109.5 Degrees
c)
120 Degrees
d)
180 Degrees
138.

Any molecule with only two atoms must be linear. Three-atom molecules such as BeCl2 can also be linear. For linear molecules, the bond angle is

a)

360°360\degree

b)

180°180\degree

c)

120°120\degree

d)

90°90\degree

139.
*
a)
linear
b)
trigonal planar
c)
trigonal pyramid
d)
bent of angular
140.
What molecular shape is the structure shown here? (BeCl2)
a)
linear
b)
bent
c)
trigonal planar
d)
tetrahedral
141.

Identify the molecule structure

a)

Bent

b)

Linear

c)

Trigonal Planar

d)

Pyramidal

142.

What is the Molecular Geometry?

a)

Quadralateral

b)

Bent 104

c)

Trigonal Pyramidal

d)

Quad Pyramidal

143.

What is the Molecular Geometry?

a)

Quadrahedral

b)

Tetrahedral

c)

Tetralateral

d)

Quadinterval

144.

What is the Molecular Geometry

a)

Triginal Pyramidal

b)

Linear

c)

Trigonal Planar

d)

SeeSaw

145.

What Molecular Structure is this?

a)

Strait

b)

Planar

c)

Di linear

d)

Linear

146.

What is the Molecular Geometry?

a)

Linear

b)

T Shape

c)

See Saw

d)

Bent

147.
What explains the very high melting and boiling point of water
a)
Strong dipole-dipole bonds between water molecules
b)
Strong hydrogen bonds between water molecules
c)
Dispersion forces which are present in all molecules
d)
Asymmetrical shape of the polar bonds.
148.
Hydrogen bonding occurs when hydrogen is bonded to N, O, or F.  Which of the following has hydrogen bonding?
a)
CBr4
b)
NO2
c)
H2S
d)
NH3
149.
Does HF have hydrogen bonding?
a)
yes
b)
no
150.
Does HCl have hydrogen bonding?
a)
yes
b)
no
151.
Does CH4 have hydrogen bonding?
a)
yes
b)
no
152.
Does NH3 have hydrogen bonding?
a)
yes
b)
no
153.
Which is the second strongest intermolecular force, after hydrogen bonding?
a)
dipole-dipole attraction
b)
London forces
154.
All molecules have London forces between them, but dipole-dipole and hydrogen bonding are so much stronger that when they are present we can ignore London forces.  Which of these has ONLY London forces?
a)
I2
b)
NH3
c)
OCl2
d)
SH2
155.

Which substance would have the weakest intermolecular forces of attraction?

a)

CH4

b)

NaCl

c)

H2O

d)

MgF2

156.

Intermolecular forces for: CO2

a)

Dispersion Force

b)

Dipole dipole

c)

Hydrogen bonding

157.
How will the following molecule bond with itself?
a)
Dispersion
b)
Dipole
c)
Hydrogen bond
158.

The weaker the intermolecular forces of a substance the _____________ the boiling point

a)

higher

b)

lower

159.

Which of the following will have the lowest melting point?

a)
b)
c)
d)
160.

Which substance has the weakest intermolecular forces?

a)

Substance A, boiling point of 75 °C

b)

Substance B, boiling point of 105 °C

c)

Substance C, boiling point of 25 °C

d)

Substance d, boiling point of 45 °C

161.

Melting and boiling points depend on thermal energy and the strength of ________

a)

intramolecular forces

b)

intermolecular forces

c)

polar covalent bonds

d)

metallic bonds

162.
In general, substances with stronger intermolecular forces have ___________  boiling points than those with weaker intermolecular forces
a)
higher
b)
lower
163.
Which of the following factors plays an important role in the identification of specific intermolecular forces in a molecule?
a)
bond type
b)
density
c)
solubility
d)
molecular polarity
164.

From fluorine to iodine, the boiling points of the halogens

a)

decrease down the group BECAUSE fluorine is the most reactive halogen

b)

decrease down the group BECAUSE fluorine is the most electronegative halogen

c)

increase down the group BECAUSE iodine has the most electrons

d)

increases down the group BECAUSE iodine has the largest atomic radius

165.

What intermolecular forces are present for halogen molecules?

a)

permanent dipole-dipole

b)

hydrogen bonding

c)

induced dipole-dipole

d)

ionic

166.

Fill in the blanks:

In the halogens, going down the group, atomic radius _________. More inner shells causes shielding to __________. ____ nuclear attraction to capture an electron from another species. Reactivity ___________.

a)

decreases, decrease, more, increases

b)

increases, decrease, less, increases

c)

increases, increase, less, decreases

d)

decreases, increase, more, decreases

167.

What is the best explanation for the trend in boiling points down the halogens group?

a)

The covalent bonds become stronger

b)

The hydrogen bonds become stronger

c)

The permanent dipole-dipole interactions become stronger

d)

The induced dipole-dipole interactions (London forces) increase

168.
What is a transition metal?
a)
They are elements that charges vary and are represented by roman numerals during nomenclature.
b)
A type of squirrel.
c)
Elements that are not defined as metals or nonmetals.
d)
A metal with no charge.
169.
Where are the transition metals found on the periodic table?
a)
The first 5 elements
b)
The bottom two rows
c)
Group 3-12
d)
Row 3-12
170.
Name the compound using appropriate rules:
FeCl3
a)
Chloride Iron
b)
Iron III Chloride
c)
Chloride III Iron
d)
I have no clue
171.

Which letters are pointing to the subscripts of this compound?

a)

A

b)

B

c)

C

172.
How do the following two elements bond together?
Na1+  F1-         
a)
NaF
b)
NaF3
c)
Na3F
d)
Na1F2
173.
How do the following two elements bond together?
K1+  S2- 
a)
KS
b)
K8S
c)
K6S3
d)
K2S
174.
Name the following ionic compound: BeCl2
a)
beryllium chlorine
b)
beryllium II chloride
c)
beryllium chloride
d)
beryllium dichloride
175.
Manganese II
a)
Mg +2
b)
Mg -2
c)
Mn +2
d)
Mn -2
176.

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

177.

When naming a compound, which of these is written first?

a)

Metal

b)

Nonmetal

c)

Anion

d)

Cation

178.

When naming a compound, what must the last part be?

a)

the element with "ide" at the end

b)

the element with the ending "ite"

c)

the name of the element

d)

the element with "ide" at the end, unless its a polyatomic ion

179.

If I gain electrons I become

a)

Positive because I've added to my atom

b)

negative because I've added electrons

c)

same because i'm balanced

d)

equal because now I have electrons

180.

By looking at the formula of an ionic compound, we can determine the charge (oxidation state) of a transition metal.

a)

True

b)

False

181.

What is the what charge of manganese in the compound: Mn2O3

a)

+1

b)

+2

c)

+3

d)

-3

182.

What is the charge of copper in the compound: CuBr2

a)

+1

b)

+2

c)

-1

d)

-2

183.

What is the what charge of lead in the compound: lead (IV) iodide

a)

+1

b)

+4

c)

+6

d)

-1

184.

What is the name of the following compound: NaCl

a)

sodium chloride

b)

sodium (I) chloride

c)

sodium chlorine

d)

sodium (I) chlorine

185.

What is the name of the following compound: CuBr2

a)

copper bromine

b)

copper bromide

c)

copper (I) bromide

d)

copper (II) bromide

186.

What is the charge of copper in the compound: CuBr2

a)

+1

b)

+2

c)

-1

d)

-2

187.

Which is the correct formula for the compound: lead (II) fluoride

a)

Pb2F

b)

PbF2

c)

PbF

d)

PbF7

188.
Which of these compounds is ionic? 
a)
Carbon dioxide
b)
Dinitrogen Trioxide
c)
Silicon tetrachloride
d)
Lithium bromide
189.

Unlike Ionic compounds, Covalent compounds require what when naming them?

a)

A roman numeral

b)

A charge

c)

A prefix

190.

When naming covalent compounds: Mono is the prefix for....

a)

1

b)

2

c)

3

d)

4

e)

5

191.

When naming covalent compounds: Di is the prefix for....

a)

1

b)

2

c)

3

d)

4

e)

5

192.

When naming covalent compounds: Tri is the prefix for....

a)

1

b)

2

c)

3

d)

4

e)

5

193.

When naming covalent compounds: Tetra is the prefix for....

a)

1

b)

2

c)

3

d)

4

e)

5

194.

When naming covalent compounds: Penta is the prefix for....

a)

1

b)

2

c)

3

d)

4

e)

5

195.

When is the prefix mono not used?

a)

It is never used when naming covalent compounds

b)

It is never used on the second element

c)

It is never used when on the first element

196.

What is the name for NI3?

a)

Mononitrogen TretraIodide

b)

Nitrogen Triiodide

c)

Nitrogen (III) Triiodide

d)

Nitrogen Iodide

197.

What is the name for CCl4?

a)

Carbon (IIII) Chloride

b)

Carbon Trichloride

c)

Monocarbon Tetrachloride

d)

Carbon Tetrachloride

198.

What is the chemical name for H2O?

a)

Water

b)

Dihydrogen Monoxide

c)

Hydrogen (II) Oxide

d)

Dihydrogen Oxygen

199.

What is the name for P2O5?

a)

Diphosphorous Pentaoxide

b)

Phosphorous Oxide

c)

Phosphorous (III) Oxide

d)

Diphosphide Oxide

200.

What are covalent compounds made up of?

a)

metal(s)

b)

nonmetal(s)

c)

transition metals

d)

noble gasses

201.

What would be the formula for Phosphorous Petaflouride?

a)

P1F6

b)

P1F5

c)

PF6

d)

PF5

202.

What is the formula for Phosphorous Trichloride?

a)

P1Cl3

b)

PCl4

c)

PCl3

d)

PCl5

203.

What is the formula for carbon monoxide?

a)

C1O1

b)

C2O2

c)

CO

d)

CO2

204.

In covalent bonds are cations and anions present?

a)

Yes, they are present.

b)

No, they are not present.

205.

Where are nonmetals typically located on the periodic table?

a)

In the middle of the periodic table

b)

To the left of the transition metals

c)

Staircase of the periodic table

d)

To the right of the staircase

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