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Unit 1 and 2 Matter, radioactivity, Lewis Dot, Naming cmpds

Total questions: 153

Worksheet time: 2hrs 55mins

Name
Class
Date
1.

What is the main type of bonding in ionic compounds?

a)

Covalent bonding

b)

Metallic bonding

c)

Ionic bonding

d)

Hydrogen bonding

2.

What is the main type of bonding in covalent compounds?

a)

Ionic bonding

b)

Metallic bonding

c)

Covalent bonding

d)

Hydrogen bonding

3.

What are Lewis dot diagrams used for?

a)

Determining molecular shape

b)

Calculating molar mass

c)

Predicting boiling points

d)

Representing valence electrons

4.

Which of the following is an example of an ionic compound?

a)

H2O

b)

CO2

c)

NaCl

d)

CH4

5.

Which of the following is an example of a covalent compound?

a)

NaCl

b)

H2O

c)

CaO

d)

KBr

6.

How many valence electrons does oxygen have?

a)

2

b)

4

c)

6

d)

8

7.

What is the charge of a chloride ion?

a)

+1

b)

-1

c)

+2

d)

-2

8.

Which of the following elements is most likely to form a positive ion?

a)

Fluorine

b)

Oxygen

c)

Sodium

d)

Chlorine

9.

Which of the following elements is most likely to form a negative ion?

a)

Potassium

b)

Calcium

c)

Bromine

d)

Helium

10.

What is the formula for sodium chloride?

a)

NaCl2

b)

Na2Cl

c)

NaCl

d)

Na2Cl2

11.

What type of bond occurs when two or more nonmetals share valence electrons?

a)

Covalent

b)

Ionic

c)

Metallic

d)

None of the above

12.

What type of bond occurs when two or more nonmetals share valence electrons?

a)

Covalent

b)

Ionic

c)

Metallic

d)

None of the above

13.

What type of bond occurs when a metal transfer its valence electrons to a nonmetal?

a)

Covalent

b)

Ionic

c)

Metallic

d)

None of the above

14.

Which of the following is NOT a property of a metallic bond..

a)

Malleable

b)

Ductile

c)

Conducts heat & electricity

d)

Brittle and breaks easily

15.

Which of the following compounds would form a ionic bond with chlorine, Cl?

a)

Phosphorus

b)

Carbon

c)

Oxygen

d)

Zinc

16.

Which of the following would be considered a covalent molecule?

a)

NaOH

b)

H2O

c)

ZnCl2

d)

KI

17.

What is the name for the following compound: N2O5

a)

nitrogen oxide

b)

dinitrogen hexoxide

c)

dinitrogen pentoxide

d)

trinitrogen dioxide

18.

What is the name for the following compound: NaOH

a)

sodium oxygen hydride

b)

sodium hydroxide

c)

nitrogen hydroxide

d)

nitrogen monoxide

19.

What is the formula for the following compound: magnesium bromide

a)

MgBr

b)

MgB

c)

MgBr2

d)

Mg2Br

20.

What is the formula for the following compound: iodine heptafluoride

a)

IF7

b)

IF5

c)

I2F7

d)

I7F

21.

What type of bonds are present in the molecule above?

a)

Ionic bonds

b)

Metallic bonds

c)

Covalent bonds

d)

Polar bonds

22.

What type of bond would form between a sodium atom and a chlorine atom?

a)

Ionic bonds

b)

Covalent bonds

c)

Metallic bonds

d)

None of the above

23.

What is the formula for the following compound: Mercury (II) Chloride

a)

MCl

b)

MCl2

c)

Hg2Cl

d)

HgCl2

24.

An unknown substance was found in a test tube. The substance did not dissolve in water, melted very quickly, and did not conduct electricity. What type of bonds are most likely present?

a)

Covalent

b)

Ionic

c)

Metallic

d)

Cannot be determined

25.

Which element would form a covalent bond with hydrogen?

a)

Lithium

b)

Magnesium

c)

Calcium

d)

Fluorine

26.

What type of bond forms a "sea of electrons"?

a)

covalent

b)

ionic

c)

metallic

d)

none of the above

27.

Which of the following compounds would form a ionic bond with chlorine, Cl?

a)

Phosphorus

b)

Carbon

c)

Oxygen

d)

Zinc

28.

What is the name for the following compound: N2O5

a)

nitrogen oxide

b)

dinitrogen hexoxide

c)

dinitrogen pentoxide

d)

trinitrogen dioxide

29.

What is the name for the following compound: NaOH

a)

sodium oxygen hydride

b)

sodium hydroxide

c)

nitrogen hydroxide

d)

nitrogen monoxide

30.

What is the formula for the following compound: magnesium bromide

a)

MgBr

b)

MgB

c)

MgBr2

d)

Mg2Br

31.

What is the formula for the following compound: iodine heptafluoride

a)

IF7

b)

IF5

c)

I2F7

d)

I7F

32.

What type of bonds are present in the molecule above?

a)

Ionic bonds

b)

Metallic bonds

c)

Covalent bonds

d)

Polar bonds

33.

What type of bond would form between a sodium atom and a chlorine atom?

a)

Ionic bonds

b)

Covalent bonds

c)

Metallic bonds

d)

None of the above

34.

What is the formula for the following compound: Mercury (II) Chloride

a)

MCl

b)

MCl2

c)

Hg2Cl

d)

HgCl2

35.

An unknown substance was found in a test tube. The substance did not dissolve in water, melted very quickly, and did not conduct electricity. What type of bonds are most likely present?

a)

Covalent

b)

Ionic

c)

Metallic

d)

Cannot be determined

36.

Which element would form a covalent bond with hydrogen?

a)

Lithium

b)

Magnesium

c)

Calcium

d)

Fluorine

37.

Why do atoms form chemical bonds?

a)

To have a stable noble gas configuration

b)

To have a complete outermost shell

c)

To satisfy the octet rule

d)

All of the above

38.

What type of bond would most likely form between a sodium and a bromine?

a)

ionic

b)

polar covalent

c)

non-polar covalent

d)

metallic

39.

Nitrogen can be classified as a....

a)

metal

b)

non-metal

c)

metalloid

d)

solid at room temperature

40.

The elements located in groups 3-12 are known as the...

a)

alkali metals

b)

halogens

c)

transition metals

d)

rare earth metals

41.

Which of the following compounds is a result of the transfer of valence electrons from a cation to an anion?

a)

H2O

b)

MgCl2

c)

PCl3

d)

N2O4

42.

What type of bond is considered a covalent bond?

a)

KI

b)

MgCl2

c)

SF8

d)

NaOH

43.

What type of bond is considered a covalent bond?

a)

KI

b)

MgCl2

c)

SF8

d)

NaOH

44.

What is the correct name for Cs2S?

a)

cesium disulfide

b)

cesium (I) sulfide

c)

cesium sulfide

d)

carbon disulfide

45.

What is the correct name for FeCl2?

a)

iron dichloride

b)

iron chloride

c)

iron chlorate

d)

iron (II) chloride

46.

What is the formula for carbon monoxide?

a)

CO

b)

Co

c)

CO2

d)

C2O

47.

What is the name for N2O4?

a)

nitrogen oxide

b)

nitrogen (IV) oxide

c)

dinitrogen tetraoxide

d)

dinitrogen tetroxide

48.

What kind of bond will form between two nitrogen atoms, N2?

a)

single bond

b)

double bond

c)

triple bond

49.

Which of the following is the correct Lewis Dot for water, H2O?

a)

A

b)

B

c)

C

d)

D

50.

Which of the following is the correct Lewis Dot for water, H2O?

a)

A

b)

B

c)

C

d)

D

51.

What kind of bond is a result of four electrons being shared?

a)

single bond

b)

double bond

c)

triple bond

52.

What is the correct formula for calcium permanganate?

a)

Ca(MnO)

b)

Ca(MnO4)

c)

Ca2(MnO4)

d)

Ca(MnO4)2

53.

What is the correct formula for CH4?

a)

monocarbon tetrahydride

b)

carbon hydroxide

c)

carbon tetrahydride

d)

carbon tetrahydroxide

54.

How many valence electrons will a lithium atom lose when it forms a bond with chlorine to form lithium chloride?

a)

1

b)

2

c)

3

d)

7

55.

Which of the following is considered an ionic compound?

a)

silicon trichloride

b)

sulfur dioxide

c)

calcium chloride

d)

diphosphorous tetroxide

56.

Covalent compounds are formed when ________________ bond by _______________ their electrons.

a)

a metal and a non-metal, transferring

b)

non-metals, transferring

c)

non-metals, sharing

d)

a metal and a non-metal, sharing

57.

How many valence electrons are in an atom of aluminum?

a)

13

b)

3

c)

4

d)

5

58.

What is the name given to the electrons of an atom, which are available for chemical bonding?

a)

orbital electrons

b)

valence electrons

c)

anions

d)

cations

59.

How do metals obey the octet rule when reacting to form compounds?

a)

they gain electrons

b)

they lose all of their valence electrons

c)

they lose some of their valence electrons

d)

they share electrons

60.

What is the net overall charge on an ionic compound?

a)

0

b)

1+

c)

2+

d)

3+

61.

Which of the following occurs in an ionic bond?

a)

valence electrons are shared

b)

Two atoms share two electrons.

c)

Oppositely charged ions attract.

d)

Like-charged ions attract.

62.

Which of the following occurs in a covalent bond?

a)

electrons are transfer

b)

electrostatic forces take over

c)

electrons are shared to always achieve an octet

d)

electrons are shared in order to achieve Nobel gas configuration

63.

Which of the following pairs of elements is most likely to form an ionic compound?

a)

potassium and sodium

b)

nitrogen and sulfur

c)

oxygen and chlorine

d)

magnesium and fluorine

64.

The bonding of a metal and non-metal is known as a _____________________.

a)

Covalent bond

b)

Hydrogen bond

c)

Metallic bond

d)

Ionic bond.

65.

How many dots would you put around carbon, a group 14 element?

a)

4

b)

6

c)

8

d)

18

66.

This could be the dot diagram of

a)

Mg

b)

Cl

c)

C

d)

O

67.

This is a correct dot diagram for neon (Ne)

a)

true

b)

false

68.

How many electrons should sodium, atomic number 11, have around its Lewis dot model?

a)

1

b)

2

c)

3

d)

4

69.

How would you draw a Lewis dot diagram for Magnesium?

a)
b)
c)
d)
70.

Which of these is correct?

a)
b)
c)
71.

What is the correct Lewis Dot Structure for ammonia NH3

a)
b)
c)
d)
72.

Which is the correct molecular structure for carbon dioxide?

a)
b)
c)
d)
73.
Which of the following is an acceptable Lewis structure for CH3Cl?
a)
Option A
b)
Option B
c)
Option C
d)
Option D
74.
Which of the following is the correct Lewis structure for water?
a)
A
b)
B
c)
C
75.
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
76.
What is the correct formula for this molecule?
a)
Si4F
b)
SiF4
c)
SiF
d)
Si4F4
77.

3. Which is a correct Lewis structure for hydrogen cyanide, HCN?

a)
b)
c)
d)
78.

CCl4 has how many double bonds?

a)

0

b)

1

c)

2

d)

3

79.

Why is this Lewis Structure incorrect? Choose all that apply.

a)

There are too many bonds around Si.

b)

There should only be single bonds in this Lewis Structure.

c)

The Structure is missing a triple bond.

d)

Chlorine only has 6 electrons surrounding it.

80.
According to the octet rule most elements need _______ valence electrons.
a)
2
b)
8
c)
6
d)
18
81.
 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
82.
How many electrons does Si contain? (click to see image)
a)
14
b)
28
c)
2
d)
None of these
83.
How many electrons does potassium K contain? (click to see image)
a)
19
b)
39
c)
20
d)
40
84.
What element is represented in this Bohr Model? 
a)
Carbon
b)
Hydrogen
c)
Aluminum
d)
Lithium
85.
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
86.
How many dots would a Lewis Dot structure of Helium have?
a)
1
b)
2
c)
8
d)
0
87.
The majority of an atom's mass exists where?
a)
In the nucleus
b)
In the electron cloud
c)
In the space between the nucleus and the electrons
d)
In the neutrons
88.
How many electrons are in the outer shell of Sodium (Na)?
a)
3
b)
1
c)
2
d)
4
89.
?
a)
Lithium
b)
Boron
c)
Carbon
d)
Neon
90.
?
a)
Helium
b)
Oxygen
c)
Sodium
d)
Phosphorous
91.
?
a)
Helium
b)
Hydrogen
c)
Argon
d)
Silver
92.
?
a)
Beryllium
b)
Boron
c)
Barium
d)
Bromine
93.

Why do carbon, silicon, and tin all react similarly?

a)

They are located in the same period

b)

They have an even atomic number

c)

They have the same number of energy levels

d)

They are located in the same group

94.

What do Rb, Re, and I have in common?

a)

family

b)

number of energy levels

c)

location of discovery

d)

valence electrons

95.

What is the valence electron count of the alkaline earth metal family?

a)

-2

b)

-1

c)

2

d)

1

96.

The diagram below is the bohr model of an atom. Which best describes this atom?

a)

it has a full outermost shell

b)

it has 6 valence electrons

c)

it has a positive charge

d)

it has 6 electrons

97.

How many valence electrons are in a neutral atom of nitrogen?

a)

5

b)

3

c)

2

d)

15

98.

The elements F, Cl, and I are all in the same column on the periodic table. Which is the best explanation for this arrangement.

a)

They have the same number of energy levels

b)

They were all discovered at ancient times

c)

They were all gases at room temperature

d)

they have the same number of valence electrons

99.

Which element is most similar to potassium (K)

a)

argon

b)

chlorine

c)

phosphorus

d)

sodium

100.

Both calcium and magnesium have the same number of valence electrons. How else can these two elements be the same?

a)

Both elements have the same atomic number

b)

Both elements have the same atomic mass

c)

Both elements are in the same group in the periodic table

d)

Both elements are in the same period on the periodic table

101.

Bob and Tanya study two electron configurations of a neutral atom. What do the two atoms have in common?

a)

Family

b)

Period

c)

Mass number

d)

Atomic number

102.
Which of the following is the correct Lewis dot structure for the molecule fluorine (F2)?
a)
A
b)
B
c)
C
d)
D
103.
What is the name of N2O3
a)
Nitrogen trioxide
b)
Dinitrogen oxide
c)
Dinitrogen trioxide
d)
Nitrogen oxide
104.
What is the name of N2O3
a)
Nitrogen trioxide
b)
Dinitrogen oxide
c)
Dinitrogen trioxide
d)
Nitrogen oxide
105.
What is the chemical formula for Tetrasulfur pentoxide?
a)
SO
b)
S4O
c)
S4O5
d)
S5O4
106.
What is the name of C3Cl8 ?
a)
Carbon octachloride
b)
Tricarbon octachloride
c)
Carbon trichloride
d)
Octacarbon trichloride
107.
What is the chemical formula for Nitrogen triiodide?
a)
NI
b)
N3I
c)
NI3
d)
None of these
108.
What is the name of Br6F10 ?
a)
Bromium fluoride
b)
Hexabromine fluoride
c)
Bromium decafluoride
d)
none of the above
109.
What is the name of CO
a)
Carbon oxide
b)
Carbon dioxide
c)
Carbon monoxide
d)
Carbon II oxide
110.
What is the chemical formula for CP ?
a)
Carbon phosphide
b)
Monocarbon phosphide
c)
Carbon monophosphide
d)
none of the above
111.
phosphorus trichloride
a)
KCl3
b)
PCl3
c)
K3Cl
d)
P3Cl
112.
The chemical formula of sulfur hexabromide is
a)
SBr₆
b)
S₆Br
c)
S(VI)Br
d)
S6Br
113.
The chemical formula of dinitrogen textroxide is
a)
Ni₂O₄
b)
NiO
c)
N₂O₄
d)
NiO₂
114.
The chemical formula of tetraphosphorus heptaoxide is
a)
F₄O₁₀
b)
P₄O7
c)
PO
d)
P₁₀O₄
115.
What's the formula for chlorine dioxide
a)
ClO2
b)
CLO
c)
ClO3
d)
HClO2
116.
What is the formula for Hexaboron Monosilicide
a)
B6Si
b)
BSi
c)
BSi6
d)
B6Si6
117.
What is the OFFICIAL name for H2O
a)
Hydrogen Oxide
b)
Oxygen Dinitride
c)
Agua
d)
Dihydrogen Monoxide
118.
BrO3
a)
bromine oxide
b)
monobromine trioxide
c)
bromine trioxide
d)
bromine (III) oxide
119.
What is the formula for Tricarbon Octahydride?
a)
Ca3O
b)
C2H8
c)
C3H8
d)
Ca3H8
120.
A binary covalent bond exists between
a)
2 metals
b)
1 metal and 1 nonmetal
c)
2 nonmetals
d)
Any 2 elements
121.
Which of the following is NOT an ionic compound:
a)
CaO
b)
NaOH
c)
BaCl2
d)
Br2
122.

Which following is a covalent compound?

a)
SO2
b)
K2O
c)
CaO
d)
BeO
123.
Which of the following is NOT an ionic compound:
a)
CaO
b)
NaOH
c)
BaCl2
d)
CH4
124.
Name this formula: 
Ca3(PO4)2
a)
Calcium Phosphorous
b)
Calcium Phosphide
c)
Calcium Phosphate
d)
Calcium (III) Phosphate
125.
Name this formula: 
NH4OH
a)
Nitrogen Oxigenide
b)
Ammonium Oxide
c)
Ammonium Hydroxide
d)
Nitrogen Peroxide
126.
Name this formula: 
KNO3
a)
Potassium Nitrogen Oxide
b)
Potassium Nitride
c)
Potassium Nitrate
d)
Potassium (I) Nitrite
127.
Name this formula: 
KNO3
a)
Potassium Nitrogen Oxide
b)
Potassium Nitride
c)
Potassium Nitrate
d)
Potassium (I) Nitrite
128.
The proper formula for magnesium hydroxide:
a)
MgOH
b)
Mg2OH
c)
Mg(OH)2
d)
Mg2OH2
129.
What is the formula for sodium nitrate?
a)
Na3NO
b)
NaNO
c)
Na3NO3
d)
NaNO3
130.
What is the formula for iron(II) carbonate?
a)
Fe2CO3
b)
FeCO3
c)
Fe2CO2
d)
FeCO4
131.

Name this compound:

CaCO3

a)

Calcium carbon oxide

b)

Calcium (II) carbonate

c)

Calcium carbonate

d)

Carbonate (I) calcide

132.
Name this formula: 
Ca3(PO4)2
a)
Calcium Phosphorous
b)
Calcium Phosphide
c)
Calcium Phosphate
d)
Calcium (III) Phosphate
133.
What is the formula for potassium carbonate?
a)
P2CO3
b)
PCO3
c)
KCO3
d)
K2CO3
134.
Solve this equation for alpha decay.
85209At = ___ + 24He
a)
83205Bi
b)
86209Rn
c)
81207Tl
d)
85208At
135.
Balance the following equation:
146C --> 0-1e + ________
a)
145B
b)
146C
c)
147N
d)
42He
136.

Solve this equation for beta decay.

614C = ___ + -10e

a)

410Be

b)

714N

c)

210He

d)

613C

137.
Complete the nuclear equation and determine the type of decay that is occurring in this reaction. 
a)
alpha
b)
beta
c)
gamma
d)
none
138.

Uranium 238 emits an alpha particle to become what nucleus?

a)

Thorium-234

b)

Thorium-239

c)

Thorium-236

139.
Solve this equation for beta decay.
614C = ___ + -10e
a)
410Be
b)
714N
c)
210He
d)
613C
140.
What particle completes this reaction?
a)
alpha particle
b)
beta particle
c)
gamma particle
d)
neutron
141.
A helium nucleus with two protons and two neutrons is called a(n) ____.  
a)
alpha particle
b)
electroscope
c)
beta particle
d)
gamma ray
142.
Solve this equation for alpha decay.
85209At = ___ + 24He
a)
83205Bi
b)
86209Rn
c)
81207Tl
d)
85208At
143.
Which type(s) of substances are considered pure substances?
a)
Elements only
b)
Compounds only
c)
Mixtures only
d)
Elements and compounds
144.

What type of substance is the air?

a)

Element

b)

Compound

c)

Mixture

145.
This type of mixture looks the same throughout. 
a)
Homogenous
b)
Heterogeneous
146.
Which of these is a property of metals?
a)
It's malleable
b)
It can't conduct electricity
c)
They are used in food
d)
It's very brittle
147.

Indefinite volume and shape.

a)

gas

b)

solid

c)

liquid

148.
A _________________ is a substance made of 2 or more elements that are chemically combined in a set ratio. 
a)
compound
b)
element
c)
atom
d)
chemical bond
149.
A _____________________ is made of 2 or more substances that are together in the same place, but their atoms are not chemically bonded. 
a)
chemical bond
b)
mixture
c)
molecule
d)
atom
150.
A ______________ mixture is when you can usually see the different parts and the can easily be separated. 
a)
heterogeneous 
b)
homogeneous
151.
An ice cube is put into a heated pan. What will most likely happen to the molecules in the ice as the ice is heated
a)
The molecules will begin to move slower.
b)
The molecules will begin to move faster
c)
The molecules will begin to increase in density
d)
The molecules will begin to condense in the air.
152.
Which among the following is an element?
a)
brass
b)
bronze
c)
silver
d)
stainless steel
153.
Physical or chemical change?
A solid is crushed into a powder?
a)
physical change 
b)
chemical change 

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