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QUARTER 3 TEST REVIEW

Total questions: 100

Worksheet time: 17hrs 15mins

Name
Class
Date
1.
Which has the greater Electronegativity: 
N or C?
a)
C
b)
N
2.
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
3.
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. 
4.
Which of the following will have a higher electronegativity than arsenic (As)?
a)
Carbon (C)
b)
Neon (Ne)
c)
Antimony (Sb)
d)
Germanium (Ge)
5.
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
6.
What term is used to describe "an atom's tendency to attract electrons to itself when is is chemically combined with another element"
a)
electronation
b)
electron affinity
c)
electronegativity
d)
electrolysis
7.

What is a group

a)

Up and down row on the table

b)

Up and down column on the table

c)

Side to side row on table

d)

Side to side column on the table

8.

What is a period

a)

Up and down row on the table

b)

Up and down column on the table

c)

Side to side row on table

d)

Side to side column on the table

9.

What atom matches this electron configuration? 1s22s22p63s2

a)

Neon

b)

Magnesium

c)

Aluminum

d)

Potassium

10.

What is the correct formula for when K and F bond?

a)

KF

b)

K2F

c)

KF2

d)

K2F3

11.

Covalent bonds are usually formed between...

a)

A metal and a non-metal

b)

Two non-metals

c)

Two metals

12.

Of these 3 molecules, which represents a covalent bond?

a)

O2

b)

NaI2

c)

NaCl

d)

MgO

13.
How many valence electrons are elements trying to reach in their outer shells?
a)
1
b)
2
c)
5
d)
8
14.

What are valence electrons?

a)

The total number of electrons in an atom

b)

The number of electrons in the outermost shell

c)

The number of electrons in the second shell

d)

The number of protons in the outermost shell

15.

Students were asked to identify the location of elements in the periodic table based on clues printed on game cards.

Based on the data, which periodic table shows the correct location of the four elements?

a)
b)
c)
d)
16.

What type of bond is depicted in the image?

a)

Non-polar Covalent

b)

Polar Covalent

c)

Ionic

17.

What type of bond is depicted in the image?

a)

Non-polar Covalent

b)

Polar Covalent

c)

Ionic

18.

What type of bond is depicted in the image?

a)

Non-polar Covalent

b)

Polar Covalent

c)

Ionic

19.

Which bond shares electrons evenly?

a)

non polar Covalent

b)

Polar Covalent

c)

Ionic

20.

The difference in electronegativity affects the type of bond will be formed. What type of bond would be formed with a difference of 2.0?

a)

Non-polar Covalent

b)

Polar Covalent

c)

Ionic

21.

What is the bond polarity if the electronegativity difference ranges from 0 to 0.3?

a)

Nonpolar Covalent

b)

Polar Covalent

c)

Ionic

22.

What is the difference in electronegativity for 

SO2SO_2  ?

a)

0.5

b)

1.0

c)

2.0

d)

3.5

23.

Which bond shares electrons unevenly?

a)

Covalent

b)

Polar Covalent

c)

Ionic

24.

Which bond involves "stealing" electrons?

a)

Covalent

b)

Polar Covalent

c)

Ionic

25.

The difference in electronegativity affects the type of bond will be formed. What type of bond would be formed with a difference of 2.0?

a)

Covalent

b)

Polar Covalent

c)

Ionic

26.

The difference in electronegativity affects the type of bond will be formed. What type of bond would be formed with a difference of 0.6?

a)

Covalent

b)

Polar Covalent

c)

Ionic

27.

Identify the following compound as ionic or covalent: Na2SO4

a)

ionic

b)

covalent

28.

Identify the following compound as ionic or covalent: CF4

a)

ionic

b)

covalent

29.

A bond between a nonmetal and a nonmetal is called a(n)

a)

covalent bond

b)

ionic bond

c)

metallic bond

d)

transfer bond

30.

A bond between a metal and a nonmetal is called a(n)

a)

covalent bond

b)

ionic bond

c)

metallic bond

d)

transfer bond

31.

Identify the following compound as ionic or covalent: SO2

a)

ionic

b)

covalent

32.

What type of bonding does this picture show?

a)

Ionic

b)

Covalent

33.

What type of bonding does this picture show?

a)

Ionic

b)

Covalent

34.

Generally high melting & boiling points

a)

Ionic compounds

b)

Covalent compounds

35.

Can be a solid, liquid, or gas at room temperature

a)

Ionic compounds

b)

Covalent compounds

36.

Always a solid at room temperature

a)

Ionic compounds

b)

Covalent compounds

37.

Poor electrical conductivity

a)

Ionic compounds

b)

Covalent compounds

38.

Conducts electricity well when melted or dissolved

a)

Ionic compounds

b)

Covalent compounds

39.

Valence electrons are shared

a)

Ionic bonds

b)

Covalent bonds

40.

Valence electrons are transferred

a)

Ionic bonds

b)

Covalent bonds

41.

Carbon and Oxygen will make a ___________ bond.

a)

ionic

b)

covalent

c)

metallic

42.

Sodium and Bromine will make a _____ bond.

a)

ionic

b)

covalent

c)

metallic

43.
According to the octet rule most elements need _______ valence electrons.
a)
2
b)
8
c)
6
d)
18
44.

This image shows the bonding between Lithium and Fluorine. What does the red arrow show?

a)

electrons being shared

b)

electrons being transferred to Fluorine

c)

electrons being transferred to Lithium

d)

electrons being destroyed

45.

Which of the following is NOT a step in forming an ionic bond?

a)

One atom shares its electrons with another one

b)

Opposite charged ions form due to the transfer of electrons

c)

One atom gives electrons to another one

d)

Oppositely charged ions attract

46.

An ionic bond is the attraction between: (Select ALL that apply)

a)

oppositely charged ions

b)

similarly charged ions

c)

metals and nonmetals

d)

neutral atoms

e)

cations and anions

47.

Which of the following is the correct formula for these two ions: Al+3 & S-2

a)

AlS3

b)

Al2S3

c)

Al3S2

d)

Al3S

48.

If I had a cation with a charge of 2+ how would you describe the formation of that ion?

a)

gained 2 electrons

b)

lost 2 electrons

c)

gained 4 electrons

d)

lost 4 electrons

49.

What is responsible for bringing cations and anions together?

a)

the size of the ions

b)

the opposite charges are attracted to one another

c)

the similar charges are attracted to one another

d)

depends on what period they're in

50.

Which is the correct name for CaBr2?

a)

Calcium Bromine

b)

Bromine Calcium

c)

Calcium Bromide

d)

Bromine Chloride

e)

Calcium Bromate

51.

Which of the below is an ionic compounds?

a)

Ni

b)

MgCl2

c)

H2O

d)

CH4

52.

An example of an ionic compound is Sodium Chloride, which is made from Na+ and Cl- ions. Why do these ions form an ionic bond?

a)

They have like charges

b)

They are from the same group

c)

They are from the same period

d)

They have opposite charges

53.

Which of the following is true for ionic bonding & ionic compounds? (3 correct statements)

a)

They must be made of ions with like charges.

b)

The negative ion must be written first.

c)

Compounds must have an overall charge of zero.

d)

They are made of metals and nonmetals.

e)

The positive ion must be written first.

54.

Which properties are all characteristics of ionic compounds?

a)

solids with high melting and boiling points

b)

soft solids which are highly malleable

c)

when solid, the ions are held in place so the compounds cannot conduct electricity

d)

conduct electricity when dissolved or molten

55.

What properties does an ionic compound have?

a)

A low boiling point and it conducts electricity when dissolved in water

b)

A high melting point and it conducts electricity when molten or dissolved

c)

A high boiling point and it conducts electricity when solid

56.

Which of the following is NOT a property of ionic compounds?

a)

They conduct electricity when molten

b)

They conduct electricity when in solution

c)

They have high boiling points

d)

They are insoluble in water

57.

Which of the following pairs of elements would NOT react to form an IONIC compound?

a)

sulfur and phosphorus

b)

sodium and iodine

c)

iron and oxygen

d)

aluminum and bromine

58.

The diagram represents the general structure of a solid Z.


What is Z?

a)

aluminium

b)

iodine

c)

silicon dioxide

d)

sulfur

59.

Metallic bonding is...

a)

a type of covalent bond.

b)

a type of ionic bond.

c)

an attraction between positive ions and freely moving electrons.

60.
Which type of bonding allows for the conduction of electricity in the solid state?
a)
Metallic
b)
Ionic
c)
Network Covalent
d)
Molecular Covalent
61.

Anions have ionic radii that are larger than their atomic radii.

a)

True

b)

False

62.

Which is larger... P or P3- ? … and why?

a)

P3- because it gains an energy level

b)

P3- due to extra electron repulsion

c)

P because it loses an energy level

d)

P because of extra electron repulsion

63.

Which is the smaller atom: Mg or Mg+2?

a)

Mg because it gains an energy level since it gains 2 electrons.

b)

Mg due to extra electron repulsion created by gaining 2 electrons.

c)

Mg+2 because of extra electron repulsion created by gaining 2 electrons.

d)

Mg+2 because it loses an energy level since it loses 2 electrons.

64.

​ (a)   bonds occur when the two bonding atoms have ​ (b)   electronegativities. ​ (c)   bonds occur when the two bonding atoms have ​different electronegativities.

Choose from the below words
Nonpolar
similar
Polar
ionic
metallic
65.
Question Image

Match the following bond types to their descriptions:

a)

ionic

1.

electrons are completely transferred from one atom to another (metals and nonmetals)

b)

nonpolar covalent

2.

electrons are shared equally between nonmetal atoms

c)

polar covalent

3.

electrons are shared unevenly between nonmetal atoms

d)

metallic

4.

collective sharing of a sea of electrons between metal atoms

66.
Name the following ionic compound: BeCl2
a)
beryllium chlorine
b)
beryllium (II) chloride
c)
beryllium chloride
d)
beryllium dichloride
67.
Name the following ionic compound: Cs2S
a)
cesium sulfide
b)
cesium sulfate
c)
cesium (II) sulfate
d)
cesium (II) sulfide
68.
Name the compound using appropriate rules:
FeCl3
a)
Chloride Iron
b)
Iron III Chloride
c)
Chloride III Iron
d)
I have no clue
69.
Write formulas for the following compound:
tin (II) fluoride
a)
SnF2
b)
Sn2F
c)
FeF2
d)
Fe2F
70.
What is the formula for magnesium chloride?
a)
MgCl
b)
Mg2Cl
c)
MgCl2
d)
Mg(ClO3)2
71.

Name the following covalent compound:

CCl4

a)

monocarbon quadchloride

b)

carbon tetrachloride

c)

carbon chloride

d)

monocarbon quadchloide

72.

Name the following covalent compound:

NF3

a)

nitrogen triflouride

b)

mononitrogen triflouride

c)

nitrogen flouride

d)

tetranitroflouide

73.

Write the formula for the covalent compound

dinitrogen pentoxide

a)

NO

b)

N2O5

c)

2NO5

d)

O5N

74.

What is the correct name for the covalent compound C4H6?

a)

Carbon Hexahydride

b)

Pentacarbon Pentahydride

c)

Hexacarbon Tetrahydride

d)

Tetracarbon Hexahydride

75.

Which is the correct molecular structure for carbon dioxide?

a)
b)
c)
d)
76.

What is the correct Lewis Dot Structure for ammonia NH3

a)
b)
c)
d)
77.
What is the first thing you need to do when drawing Lewis Structures?
a)
Draw your bonds
b)
Count the number of valence electrons
c)
Subtract to make the valence number even
d)
Add to make the valence number even
78.
Which of the following is the correct Lewis dot structure for the molecule fluorine (F2)?
a)
A
b)
B
c)
C
d)
D
79.
What geometry will this molecular structure have?: H2S
a)
bent
b)
tetrahedral
c)
linear
d)
trigonal pyramidal
80.
Choose the correct shape for this molecule:
a)
Bent
b)
Trigonal pyramidal
c)
Trigonal planar
d)
Linear
81.
Choose the correct shape for this molecule:
a)
linear
b)
Trigonal pyramidal
c)
Bent
d)
Tetrahedral
82.
Choose the correct shape for this molecule:
a)
Bent
b)
Linear
c)
Tetrahedral
d)
Trigonal pyramidal
83.
According to VSEPR, molecules adjust their shapes to keep which of the following as far away as possible?
a)
Pairs of valence electrons
b)
Inner shell electrons
c)
Mobile Electrons
d)
Electrons closest to the nucleus
84.

Determine the molecular geometry of the given structure.

a)

Trigonal Pyramidal

b)

Trigonal Bipyramidal

c)

Trigonal Planar

d)

Tetrahedral

85.

The geometry of a molecule with 4 bonded pairs of electrons and 0 lone pairs of electrons, AB4

a)

Tetrahedral

b)

Trigonal Planar

c)

Bent

d)

Trigonal Pyramidal

e)

Linear

86.
Who could this be? 
a)
CO2
b)
NH3
c)
H2S
d)
CH4
87.
Choose the correct shape for this molecule:
a)
Tetrahedral
b)
Trigonal pyramidal
c)
Bent
d)
Trigonal planar
88.
What does the symbol -10e represent
a)
alpha
b)
beta
c)
gamma
d)
the zero element
89.
Balance the following equation:
146C --> 0-1e + ________
a)
145B
b)
146C
c)
147N
d)
42He
90.
Complete the nuclear equation and determine the type of decay that is occurring in this reaction. 
a)
alpha
b)
beta
c)
gamma
d)
none
91.
What is the missing isotope that will balance the following nuclear equation?
94Be  +  11H →  _____  +  42He
a)
105B
b)
105Ne
c)
63Li
d)
63C
92.
a)
23692U
b)
23693U
c)
23492Np
d)
23493Np
93.

The % of the parent isotope remaining after 3 Half Lives.

a)

50%

b)

25%

c)

12.5%

d)

6.25%

94.

The diagram shows 32 atoms

8 of the Red are parent isotopes

24 of the Green are daughter isotopes

How many half-lives have occurred?

a)

0

b)

1

c)

2

d)

3

95.

What is the Half life of this isotope?

a)

5 seconds

b)

10 seconds

c)

15 seconds

d)

20 seconds

96.
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
97.

Type in the measurement on the graduated cylinder to the correct number of significant digits. No unit.

a)

6.300

b)

6.3

c)

6.32

d)

7.70

98.

Read the graduated cylinder

a)

76.0

b)

76.15

c)

71.9

99.

Type in the measurement on the ruler to the correct number of significant digits. No unit.

a)

41.6

b)

41

c)

42

d)

41.50

100.

Which of the following choices best represents the length reading from the metric ruler pictured?

a)

0.8 cm

b)

0.80 cm

c)

0.800 cm

d)

8 cm

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