wayground logo

Free Printable Worksheets

Font size

S
M
L
XL
Worksheets

Chem 10. Inv 3

Total questions: 120

Worksheet time: 2hrs 50mins

Name
Class
Date
1.

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

2.

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

a)

potassium

b)

calcium

c)

helium

d)

boron

e)

fluorine

3.

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

a)

sodium

b)

calcium

c)

helium

d)

boron

e)

chlorine

4.

Which of the following elements GAINS 2 electrons in order to attain an octet?

a)

cesium

b)

magnesium

c)

phosphorus

d)

sulfur

e)

iodine

5.

Which of the following elements LOSES 3 electrons in order to attain an octet?

a)

nitrogen

b)

lithium

c)

aluminum

d)

oxygen

e)

iodine

6.

Which of the following elements GAINS 3 electrons in order to attain an octet?

a)

nitrogen

b)

lithium

c)

boron

d)

oxygen

e)

fluorine

7.

Each of the following elements will LOSE ELECTRONS in order to attain an octet EXCEPT _______

a)

iodine

b)

magnesium

c)

potassium

d)

copper

e)

strontium

8.

Each of the following elements attains a stable valence shell WITHOUT having an octet in its outermost shell EXCEPT _______.

a)

lithium

b)

hydrogen

c)

beryllium

d)

helium

e)

nitrogen

9.

According to the Octet Rule, atoms want ____ electrons in their outermost energy level or shell.

a)

2

b)

4

c)

6

d)

8

10.

When atoms LOSE electrons, they get a...

a)

Positive (+) charge

b)

Negative (-) charge

c)

No charge (zero)

11.

Boron (B) needs to lose 3 electrons to satisfy the Octet Rule. What is the resulting charge of the B ion?

a)

+ 3

b)

- 3

c)

+ 6

d)

Zero

12.

What does Neon need to do fulfill the Octet Rule?

a)

Gain 2

b)

Lose 2

c)

Nothing - it already fulfills the Octet Rule.

13.

When atoms GAIN electrons, they get a...

a)

Positive (+) charge

b)

Negative (-) charge

c)

No charge (zero)

14.

When fluorine gains 1 electron to satisfy the Octet Rule, what is the resulting charge of the ion?

a)

+ 1

b)

- 1

c)

Zero

15.

Fluorine gains 1 electron to satisfy the Octet Rule. What kind of ion is formed?

a)

Anion (-)

b)

Cation (+)

16.

What does Oxygen have to do to satisfy the Octet Rule? What would its charge be after? (TAKE YOUR TIME!)

a)

Lose 6 electrons, + 6

b)

Gain 8 electrons, - 8

c)

Lose 2 electrons, + 2

d)

Gain 2 electrons, - 2

17.

Which group already satisfies the Octet Rule and therefore does not bond with other atoms?

a)

Group 1 (H at top)

b)

Group 2 (Be at top)

c)

Group 13 (B at top)

d)

Group 18 (He at top)

18.

Which 2 atoms are EXCEPTIONS to the Octet Rule and only need 2 valence electrons?

a)

H, Na

b)

H, He

c)

He, Ne

d)

There are no exceptions to the Octet Rule

19.

This atom will

a)

lose 2 electrons

b)

gain 2 electrons

c)

lose 6 electrons

d)

gain 6 electrons

e)

do nothing

20.
Same repel, opposites
a)
avoid
b)
attract
c)
push
d)
pull
21.
Is this ionic bond drawn correctly?
a)
Yes
b)
No
22.
Ionic bonds are between...
a)
Metal and Non-metal
b)
Non-metal and Non-metal
c)
Metal and Metal
23.
Atoms are most stable when their outer shell is complete.
a)
true
b)
false
24.
How are ionic bonds formed?
a)
Transfer of electrons
b)
Sharing of electrons
25.
Why do elements bond?
a)
To be friends
b)
To create a new element
c)
To become stable
26.
Which of these is not a real bond in chemistry?
a)
James
b)
Ionic
c)
Covalent
27.

How many Aluminum atoms are in Al2O3?

a)

3

b)

5

c)

2

d)

1

28.

Write the correct formula for Sodium Chloride.

a)

SC

b)

SCl

c)

NaCl

d)

NaCl2

29.

Which of the following is the correct ionic formula for calcium sulfide?

a)

Ca2S2

b)

CaS

c)

S2Ca2

d)

SCa

30.

Aluminum will react spontaneously with oxygen in the air to form aluminum oxide. Write the formula for the compound that is produced in this reaction.

a)

AlO

b)

Al2O3

c)

O3Al2

d)

Al6O3

31.

Name the compound from it's formula: BaI2

a)

Iodine barium

b)

Iodine bariumide

c)

Barium iodine

d)

Barium iodide

32.

When magnesium burns in oxygen it produces MgO. Use the ionic formula to name the compound produced.

a)

Magnesium oxygen

b)

Oxygen magnesium

c)

Magnesium oxide

d)

Oxygen magnesiumide

33.
An atom that has gained or lost electrons is called ...
a)
a winner
b)
an isotope
c)
an ion
d)
a loser
34.

If an aluminum atom has 13 protons (+) and 10 electrons (-), what is it's charge?

a)

Al+3

b)

Al+13

c)

Al+10

d)

Al-10

35.
Which of the following is a property of an ionic compound?
a)
high melting point
b)
soft
c)
malleable
d)
liquid at room temperature
36.

The following properties are all characteristics of ionic compounds EXCEPT

a)

high melting and boiling points

b)

soft

c)

crystal lattice structure

d)

conduct electricity when dissolved in water

37.

What type of forces hold on an ionic lattice together?

a)

Electrostatic attraction forces

b)

Covalent bond

c)

Metallic bond

d)

Van der Waals forces

38.

Ionic compounds form giant ionic lattices. What forces hold the giant ionic lattices together?

a)

strong frictional forces between the surfaces of the atoms

b)

strong magnetic forces of attraction between the poles of ions

c)

strong electrostatic forces of attraction between oppositely charged ions

39.

True or false? Ionic compounds have low boiling points.

a)

true

b)

false

40.

Which two substances are ionic compounds?

a)

sodium chloride (NaCl)

b)

carbon dioxide (CO₂)

c)

water (H₂O)

d)

magnesium oxide (MgO)

41.

What property is describing an ionic compound?

a)

shares electrons

b)

high melting point

c)

weak bonds

d)

made up of nonmetals.

42.

A metallic bond is a bond between ________.

a)

nonmetals

b)

metals

c)

transition metals

d)

metalloids

43.

Which of the following is NOT a property of metals?

a)

Hard

b)

Can conduct electricity

c)

Very brittle (breaks easily)

d)

Malleable (can bend without breaking)

44.

What do electrons do in a metallic bond?

a)

They stay on the metal atom.

b)

They are transferred from atom to atom.

c)

They form a covalent bond with another atom.

d)

They float around freely.

45.

What is meant by the term "sea of electrons"?

a)

It's what we call all the free floating electrons in a metal.

b)

It's what we call electrons that are floating in a liquid.

c)

It's the total number of electrons in a metal atom.

d)

It's the total number of electrons in the ocean.

46.

What do we call electrons that move freely in a metallic bond?

a)

sea of electrons

b)

lone electrons

c)

unpaired electrons

d)

covalent electrons

47.

What property of metals is the image describing?

a)

malleable (bend without breaking)

b)

ductile (stretched into a wire)

c)

conductive (can conduct electricity)

d)

shiny

48.

Why are metals good conductors?

a)

they have mobile electrons

b)

they have mobile atoms

c)

they have crystal structures that can rearrange

d)

they have mobile protons

49.

Have a high melting point

a)

Metals

b)

Non-Metals

50.

Steel is an example of an

a)

Metal

b)

Non-Metal

c)

Alloy

51.

The following that shows the correct meaning for ductility of metals is

a)

they can be drawn into wires.

b)

they can be drawn into sheets.

c)

they are shiny

52.

What is the correct Electron Dot Structure for ammonia NH3

a)
b)
c)
d)
53.

Which is the correct molecular structure for carbon dioxide?

a)
b)
c)
d)
54.
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
55.
What type of bond is shown in this image?
a)
Ionic
b)
Polar Covalent
c)
Nonpolar Covalent
d)
Van der Waals Force
56.
In an electron dot diagram, two pairs of shared electrons represents a ...
a)
single bond
b)
double bond
c)
triple bond
d)
quadruple bond
57.
A Nitrogen molecule (N2) has one triple bond. How many electrons do the nitrogen atoms share?
a)
1
1
b)
3
c)
4
d)
6
58.
Compared to ionic compounds, molecular compounds generally have...
a)
good conductivity
b)
greater densities
c)
more chemical bonds
d)
a low boiling point
59.
Compared to ionic compounds, molecular compounds generally have...
a)
stronger chemical bonds
b)
poor conductivity
c)
a high melting point
d)
lower densities
60.
what type of bond is the strongest
a)
single
b)
Double
c)
coordination
d)
triple
61.
 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
62.
In an electron dot diagram, two pairs of shared electrons represents a ...
a)
single bond
b)
double bond
c)
triple bond
d)
quadruple bond
63.

Which of the following is the correct Electron dot structure for the molecule fluorine (F2)?

a)
A
b)
B
c)
C
d)
D
64.
Which of the following is the correct Lewis structure for the compound PBr3?
a)
structure A
b)
structure B
c)
structure C
d)
structure D
65.

Which is the correct molecular structure for carbon dioxide?

a)
b)
c)
d)
66.

CCl4 has how many double bonds?

a)

0

b)

1

c)

2

d)

3

67.

In HCN (Carbon is usually the central atom) what kind of bond is between the C and N

a)

Single

b)

Double

c)

Triple

68.

CHCl3 has how many double bonds?

a)

0

b)

1

c)

2

d)

3

69.
This is a correct dot diagram for oxygen (O)
a)
true
b)
false
70.
This is the correct dot diagram for nitrogen (N)
a)
true
b)
false
71.

The ability of an atom in a molecule to attract electrons is best quantified by the ______.

a)

electronegativity

b)

paramagnetism

c)

diamagnetism

d)

electron change-to-mass ratio

e)

first ionization energy

72.
Choose the set that goes from lowest to highest electronegativity?
a)
Cu, Mg, Sr, Ca
b)
F, Cl, Br, Si
c)
Cs, Rb, Ca, Mg
d)
Zn, Cd, Ag, Cu
73.
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. 
74.
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. 
75.
The element with the largest electronegativity in the halogens is - 
a)
At
b)
F
c)
Cl
d)
Br
76.
Choose the set that goes from lowest to highest electronegativity?
a)
Cu, Mg, Sr, Ca
b)
F, Cl, Br, Si
c)
Cs, Rb, Ca, Mg
d)
Zn, Cd, Ag, Cu
77.
Put these in order of increasing electronegativity:
Se, S, and O
a)
Se < S < O
b)
Se < O < S
c)
O < S < Se
d)
S < Se < O
78.

What type of bond would form between O and H?

a)

Polar Covalent

b)

Non-Polar Covalent

c)

Ionic

79.

What type of bond would form between O and O?

a)

Polar Covalent

b)

Non-Polar Covalent

c)

Ionic

80.

What type of bond would form between Li and O?

a)

Polar Covalent

b)

Non-Polar Covalent

c)

Ionic

81.

The bond between C and Cl is polar covalent. That means

a)

there is a pair of electrons shared equally between them

b)

there is a pair of electrons shared unequally between them

c)

an electron will be stolen from one and given to the other

82.

Water, H2O, is classified as what type of molecule?

a)

a polar molecule

b)

a nonpolar molecule

c)

a coordinate covalent compound

d)

an ionic compound

83.

The dipole moment is represented by an arrow with a plus sign at the tail pointing toward ___

a)

a fluorine atom

b)

the negative side of the molecule

c)

magnetic north

d)

the least electronegative element

84.

A little lowercase delta plus (δ+) or delta minus (δ–) by the individual atoms signify ___

a)

partial charges

b)

the magnetic poles

c)

a difference in electronegativities

d)

nonpolar molecules

85.

Liquids made up of polar molecules are really good at dissolving ___

a)

metallic solids

b)

lipids and fats

c)

molecular solids

d)

solids composed of polar or ionic compounds

86.

H2 is a ____ molecule.

a)

polar

b)

non-polar

87.

CO is a _____ molecule.

a)

polar

b)

non-polar

88.

CO2 is a _____ molecule.

a)

polar

b)

non-polar

89.

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

a)

higher

b)

lower

90.

________________________ have the strongest intermolecular forces of attraction.

a)

Dipole- Dipole

b)

Dispersion

c)

Hydrogen Bonds

91.
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
92.
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.
93.
Does H2S have hydrogen bonding?
a)
yes
b)
no
94.

Which intermolecular force is most notable in noble gases, and non-polar molecules?

a)

London dispersion forces

b)

dipole-dipole forces

c)

hydrogen bonding

d)

gravitational forces

95.

Dipole-dipole attractions occur between polar molecules. Which of these molecules is polar?

a)

H2

b)

HCl

c)

Cl2

d)

Br2

96.

A liquid evaporates fast.

The liquid is said to have ________ volatility.

a)

high

b)

medium

c)

low

d)

none of these

97.

A liquid has low volatility.

The intermolecular forces between molecules in this liquid must be________

a)

strong

b)

medium

c)

weak

d)

none of these

98.
Which of the following statements correctly compares the behavior of a mixture of ethanol and water at STP?
a)
Water will evaporate first, because it has weaker intermolecular forces
b)
Ethanol will evaporate first, because it has weaker intermolecular forces
c)
Ethanol and water will evaporate simultaneously
d)
The aqueous solution will evaporate partially at a temperature between the boiling points of water and of ethanol
99.
Hydrogen bonds are a form of bonding.
a)
True 
b)

False, it's an intermolecular force

100.
What would be the proper chemical formula for combining Al3+ and Cl- :
a)
AlCl3
b)
Al3Cl
c)
AlCl
d)
Al3Cl3
101.

Name the following ionic compound: BeCl2

a)

beryllium chlorine

b)

beryllium( II ) chloride

c)

beryllium chloride

d)

beryllium dichloride

102.

Name the following compound: FeCl3

a)

iron chloride

b)

iron( III ) chloride

c)

iron chlorate

d)

iron( III ) chlorate

103.
Which of the following combinations would need roman numerals in the name?
a)
potassium + fluorine
b)
beryllium + oxygen
c)
boron + iodine
d)
silver + oxygen
104.
What is the ionic compound formed between Calcium and Oxygen?
a)
CaO
b)
Ca2O
c)
Ca2O2
d)
CaO2
105.

Cobalt (II) Oxide

a)

Co2O

b)

CoO2

c)

CoO

d)

Co2O2

106.
What formula results when Ca+2 and Br- ions bond?
a)
Ca2Br2
b)
CaBr
c)
Ca(br)2
d)
CaBr2
107.
A covalent compound made of one sulfur and two oxygen atoms would be named
a)
sulfur dioxide.
b)
sulfur oxide.
c)
disulfur oxide.
d)
sulfide oxygen.
108.
The covalent compound N2O5 would be named
a)
nitrogen oxide.
b)
dinitrogen oxide.
c)
nitrogen pentoxide.
d)
dinitrogen pentoxide.
109.
The name of P₄S₁₀ is
a)
phosphorous sulfide
b)
phosphorus sulfide
c)
tetraphosphorus decasulfide
d)
phosphorus (X) sulfide
110.
The chemical formula of carbon tetrachloride is
a)
CCl
b)
C₄Cl
c)
CCl₄
d)
C(IV)Cl
111.
CF4
a)
carbon fluoride
b)
monocarbon tetrafluoride
c)
carbon tetrafluoride
d)
carbon tetrafluorine
112.
Which of the following is nitrate?
a)
NO-
b)
NO2-
c)
NO3-
d)
NO4-
113.
Which of the following is chromate?
a)
CrO42-
b)
CrO32-
c)
CrO22-
d)
CrO2-
114.
What is the name of K3PO4?
a)
Tripotassium Phosphate
b)
Tripotassium Phosphite
c)
Potassium phosphide
d)
Potassium phosphate
115.
What is the name of Al(NO3)3?
a)
Aluminum trinitrate
b)
Monoaluminum nitrate
c)
Aluminum (III) nitrate
d)
Aluminum Nitrate
116.
What is the name of Mg(OH)2?
a)
Magnesium Hydride
b)
Magnesium Dihydride
c)
Magnesium Dihydroxide
d)
Magnesium Hydroxide
117.

What is the correct name for this polyatomic ion: CN–

a)

carbonate

b)

cyanide

c)

chromate

d)

chromite

118.

What is the correct name for this polyatomic ion: OH–

a)

hydrogen carbonate

b)

oxonium

c)

hydroxide

d)

acetate

119.

What is the correct name for this polyatomic ion: PO43–

a)

phosphorus tetroxide

b)

phosphate

c)

sulphate

d)

hydroxide

120.
What is the name of NH4Cl?
a)
nitrogen tetrahydrogen chloride
b)
ammonium chlorine
c)
ammonium chloride
d)
ammonium chlorate

Similar Resources on Wayground

Honors Chemistry Review

115 questions

Honors Chemistry Review

quiz

Worksheet

•

9th - 12th Grade

Grade 10 Chapter 7.1 and 7.2 Chemistry

115 questions

Grade 10 Chapter 7.1 and 7.2 Chemistry

quiz

Worksheet

•

10th Grade

Science 10 Chemistry Test

123 questions

Science 10 Chemistry Test

quiz

Worksheet

•

10th Grade

Year Review

120 questions

Year Review

quiz

Worksheet

•

9th - 10th Grade

Ionic Compound Nomenclature

117 questions

Ionic Compound Nomenclature

quiz

Worksheet

•

10th - 12th Grade

Review: Atomic Particles and Theories

118 questions

Review: Atomic Particles and Theories

quiz

Worksheet

•

10th Grade

Billings Unit 1 Test Review

121 questions

Billings Unit 1 Test Review

quiz

Worksheet

•

9th - 12th Grade

Final Exam

120 questions

Final Exam

quiz

Worksheet

•

10th Grade