wayground logo

Free Printable Worksheets

Font size

S
M
L
XL
Worksheets

Honors Review - Matter, Bonding, & LOCOMatter (SPS1, SPS2, SPS3)

Total questions: 192

Worksheet time: 4hrs 32mins

Name
Class
Date
1.

What do these isotopes of carbon all have in common?

a)

neutrons and mass number

b)

atomic number and neutrons

c)

atomic number and electrons

d)

protons, atomic number, and mass number

2.
How many neutrons does the isotope of lithium have?
a)
8
b)
3
c)
4
d)
5
3.
An atom is electrically neutral when
a)
protons and neutrons are the same
b)
protons and electrons are the same
c)
neutrons and electrons are the same
d)
neutrons balance the protons and electrons
4.

What are the names of the electrons in the outer shell called?

a)

Outer electrons

b)

Valence electrons

c)

Orbital electrons

d)

Outer valence orbital electrons

5.

What is the charge on a lithium atom that loses one electron?

a)

+1

b)

0

c)

-1

d)

-2

6.

Silicon is a semiconductor and has properties of both metals and nonmetals. What type of element is silicon?

a)

Metal

b)

Nonmetal

c)

Metalloid

d)

Pretty

7.

What type of atom is Element C?

a)

Normal atom

b)

Cation

c)

Isotope

d)

Anion

8.

Metals are found on this side of the Periodic Table:

a)

Left side

b)

Right side

c)

On the stair-step line

d)

Below

9.
A student is given a sample of an unknown substance. He is asked to determine if it is classified as a metal, a metalloid, or a nonmetal. He discovered that the unknown element conducted some heat and electricity, had a shiny luster, and broke easily. This element is most likely a 
a)
metal
b)
nonmetal
c)
metalloid
d)
cannot be determined
10.

What is the formula to solve for the neutron?

a)

Mass Number + Atomic Number = Neutrons

b)

Mass Number x Atomic Number = Neutrons

c)

Mass Number - Atomic Number = Neutrons

d)

Mass Number + Number of Protons = Neutron

11.
An atom with 19 protons, and 19 electrons and a mass of 39 has how many neutrons?
a)
19
b)
39
c)
20
d)
58
12.

What is the mass number of this neon atom?

a)

10

b)

11

c)

21

d)

20

13.

How many electrons does this magnesium ion have?

a)

24

b)

12

c)

10

d)

14

14.
Which of the following tables correctly lists the physical properties of metals and nonmetals?
a)
A
b)
B
c)
C
d)
D
15.

The electron cloud is divided in to energy levels or shells. The first level will hold _____ electrons and the second level will hold ______ electrons.

a)

8, 2

b)

2,8

c)

1, 8

d)

8,18

16.

_____________ transfer electrons from a metal to a nonmetal.

a)

Covalent Bonds

b)

Ionic Bonds

c)

James Bonds

d)

Savings Bonds

17.

___________ share electrons between nonmetals and nonmetals.

a)

Ionic bonds

b)

Covalent bonds

c)

Polar covalent bonds

d)

Diatomic bonds

18.

Polar covalent is when the electrons are shared ___________

a)

equally

b)

unequally

c)

between metals and nonmetals

d)

in diatomic molecules

19.
When two atoms share electrons, a chemical bond is formed.  This type of bond is called:
a)
covalent bond
b)
ionic bond
c)
crystal bond
d)
polyatomic bond
20.

Which of these is covalent?

a)

NaCl

b)

KBr

c)

CO2

d)

AlCl3

21.

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

a)

They have very high melting points

b)

They conduct electricity when in solution

c)

They have high boiling points

d)

They will not dissolve in water

22.

Which of the following is NOT formed by a covalent bond?

a)

K2S

b)

H2O

c)

I2

d)

CO2

23.

What is the correct name for this formula: BeI2?

a)

beryllium (II) iodide

b)

beryllium diiodide

c)

beryllium iodine

d)

beryllium iodide

24.

Which structures conduct electricity as a liquid but not as a solid?

a)

Metallic

b)

Covalent

c)

Ionic

d)

All of the above

25.
Which is the correct formula for dinitrogen monoxide?
a)
H2O
b)
NO2
c)
N2O
d)
N2O2
26.

Name the following compound: AlCl3

a)

Aluminum trichloride

b)

Aluminum chloride

c)

monoaluminum chloride

d)

monoaluminum trichloride

27.

What is the formula for lithium nitride

a)

LiN

b)

LiN3

c)

Li3N

d)

LiN2

28.

What is the correct name for PCl3?

a)

monophosphorus trichloride

b)

triphosphorus monochloride

c)

triphosphorus chloride

d)

phosphorus trichloride

29.

What is the correct formula for N2Br4?

a)

dinitrogen tetrabromide

b)

tetranitrogen dibromide

c)

dineon tetrabromide

d)

dinitrogen tetraboride

30.

What is the correct formula for calcium nitride?

a)

CaN

b)

Ca3N2

c)

Ca2N3

d)

C3N2

31.

What is the formula for disulfur heptafluoride?

a)

SF

b)

S7F2

c)

S2F6

d)

S2F7

32.

In order for sulfur to reach an octet, sulfur will...

a)

Gain 2 electrons

b)

Lose 2 electrons

c)

Gain 1 electron

d)

Lose 1 electron

33.

Is this ionic bond drawn correctly?

a)

Yes

b)

No

c)

Maybe

d)

Why are you asking ME?

34.
What is the correct formula for this molecule?
a)
NH
b)
N3H
c)
NH3
d)
NH4
35.

A burning candle is covered by a jar as shown in the picture. The whole arrangement has a mass of 500g. What will be the approximate mass of the arrangement when the candle is completely burnt, after four minutes?

a)

0g

b)

50g

c)

250g

d)

500g

36.

Which chemical equation shows that the total mass during a chemical reaction stays the same?

a)

Mg + Cl2 → MgCl2

b)

NaOH + MgCl2 → NaCl + MgOH

c)

2Na + 2H2O → NaOH + H2

d)

H2O + O2 → H2O

37.

In the picture, which box on the right shows the correct products according to the Law of Conservation of Mass?

a)

A

b)

B

c)

C

d)

D

38.

Which chemical equation is balanced?

a)

CH₄ + O₂ → CO₂ + 2H₂O

b)

H₂ + O₂ → 2H₂O₄

c)

4Al + 3O₂ → 2Al₂O₃

d)

None are balanced

39.
Students react baking soda & vinegar.
Which of the following would provide the evidence that the number of atoms present before a chemical reaction is equal to the number of atoms present after the chemical reaction?
a)
The mass of the plastic bag, baking soda, and vinegar before the reaction was equal to the mass after the reaction.
b)
Bubbles were produced during the reaction, which meant that a gas was being produced.
c)
The plastic bag did not change in any way, indicating that it was not involved in the reaction.
d)
The mass of the baking soda was exactly equal to the mass of the vinegar used to create the chemical reaction.
40.

Bob puts 200 grams of ice into a pitcher with 900 grams of water. He gets distracted and comes back later to find that the ice has melted in the water. How many grams of water does Bob now have in the pitcher?

a)

200 g

b)

700 g

c)

1,100 g

d)

900 g

41.

Is this balanced?

Al + O2 → 2Al2O3

a)

Yes

b)

No

c)

Depends on the scale

d)

Who knows?

42.

In a reaction A + B ----> C, reactant A has a mass of 5g and product C has 9g. How many grams must reactant B have?

a)

4g

b)

5g

c)

9g

d)

14g

43.

Valence electrons are found by looking at which __________ the atom is located in on the periodic table.

a)

group

b)

column

c)

row

d)

box

44.

_________ are located to the right of the stair-step line.

a)

Metals

b)

Nonmetals

c)

Metalloids

d)

Black holes

45.

Metals are _________ at room temperature with the exception of mercury.

a)

solids

b)

gas

c)

liquid

d)

invisible

46.

Nonmetals are generally ________ at room temperature.

a)

solids

b)

liquids

c)

gases

d)

Adele fans

47.

The _____ phase is one in which intermolecular forces hold the atoms or molecules loosely together but do not force them into a rigid structure.

a)

solid

b)

liquid

c)

gas

d)

plasma

48.

In the ________ phase, atoms and molecules experience their greatest freedom. The forces attracting gas molecules are almost non-existent. As a result, these molecules are much farther apart and can move freely about.

a)

Solid

b)

Liquid

c)

Gas

d)

Plasma

49.

_____________ are gases that have been so energized that their atoms have been stripped of some or all electrons. Solar flares are great examples of plasma. Solar flares eject extremely hot hydrogen ions (H+) away from the Sun and toward Earth.

a)

Solids

b)

Liquids

c)

Gases

d)

Plasmas

50.
What is the phase change of sublimation?
a)
Liquid to solid
b)
Gas to liquid
c)
Liquid to gas
d)
Solid to gas
51.
One reactant into several products.
a)
Decomposition
b)
Synthesis
c)
Combustion
d)
Single Replacement
52.

Usually starts with a hydrocarbon that reacts with oxygen and produces carbon dioxide and water.

a)

Decomposition

b)

Synthesis

c)

Combustion

d)

Single Replacement

53.
Two Reactants and One Product
a)
Decomposition
b)
Synthesis
c)
Combustion
d)
Single Replacement
54.

This picture of a football is here for no reason.

Click CONTINUE to move on.

a)

CONTINUE

b)

I don't follow directions.

c)

What if I don't like football?

d)

Is this for a grade?

55.

Which two of the following are chemical reactions?

a)

sugar dissolving in water

b)

water turning into steam

c)

burning wood

d)

mixing baking soda and vinegar

e)

tearing paper

56.

How many hydrogens are on the product side of this chemical equation?

a)

1

b)

2

c)

3

d)

4

57.

How many carbons are present on the reactant side?

a)

1

b)

2

c)

3

d)

4

58.

Why are chemical equations always balanced? Select ALL that apply.

a)

Matter cannot be created.

b)

Matter cannot be destroyed.

c)

Matter can only be rearranged/conserved.

d)

Matter doesn't matter.

59.

2NH3 states that there are how many of each atom?

a)

2 Nitrogen and 3 Hydrogen

b)

6 Nitrogen and 2 Hydrogen

c)

2 Hydrogen and 6 Nitrogen

d)

2 Nitrogen and 6 Hydrogen

60.

This pictures simulates which type of reaction?

a)

Synthesis

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

61.

Identify the type of reaction:

ZnCl2 + Mg → Zn + MgCl2

a)

Synthesis

b)

Single Replacement

c)

Double Replacement

d)

Decomposition

62.

Identify the reaction type:

NaCl + KOH → KCl + NaOH

a)

Double replacement

b)

Combustion

c)

Synthesis

d)

Decomposition

63.

Group 1 of the periodic table is called the...

a)

Halogens

b)

Noble Gases

c)

Transition Metals

d)

Alkali Metals

64.

Group 17 of the periodic table is called the...

a)

Halogens

b)

Noble Gases

c)

Transition Metals

d)

Alkaline Earth Metals

65.

Elements on the periodic table are arranged by...

a)

relative atomic mass

b)

date of discovery

c)

atomic number

d)

number of electrons

66.

The group number tells you

a)

the number of electron shells an element has

b)

the number of electrons in the outer shell of an atom

c)

the number of electrons needed to fill the outer electron shell

d)

the ion that an atom will make

67.

The period number tells you how many

a)

outer electrons there are in an atom

b)

electron shells an atom has

c)

ions an atom can form

d)

bonds an atom can make

68.

Elements from group 2 will form with a charge of

a)

+1

b)

+2

c)

-2

d)

-1

69.

Atoms from group 16 will generally form ions with a charge of

a)

+1

b)

+2

c)

-2

d)

-1

70.

Isotopes of an element have the same atomic number but different mass numbers

a)

True

b)

False

71.

What is the maximum number of electrons in the first shell?

a)

8

b)

4

c)

6

d)

2

72.

What is the optimum number of electrons an atom likes in its outer shell?

a)

2

b)

6

c)

4

d)

8

73.

What is the atomic number of nitrogen?

a)

7

b)

14.007

c)

N

d)

28

74.

What is the atomic mass of nitrogen?

a)

7

b)

15

c)

14.007

d)

.007

75.

The groups of a periodic table are the

a)

Horizontal rows

b)

Vertical columns

76.

Periods in the periodic table are

a)

rows

b)

columns

77.

An element is shiny, solid, but brittle.

Which element would that description best describe?

a)

Na

b)

Cl

c)

Te

d)

Cu

78.

Where are electrons likely to be found on an atom?

a)

Nucleus

b)

Electron Clouds

c)

Neutrons

d)

Everywhere

79.

Which of the following subatomic particles has the smallest Atomic Mass Unit or AMU?

a)

Proton

b)

Neutron

c)

Electron

d)

Nucleus

80.

Which elements share similar chemical properties?

a)

Na + Mg

b)

Na + K

c)

O + F

d)

Na + F

81.

Which of the following elements has a full outer energy level and is in the group identified as the Noble Gases?

a)

Li

b)

O

c)

B

d)

Ne

82.

Which of the following is a property of Alkali Metals (Group 1)?

a)

They are so hard they cannot be cut.

b)

They are very, very reactive.

c)

They are stored in water.

d)

They have few uses.

83.

When a Halogen (G17) reacts with an Alkali Metal (G1), what is formed?

a)

Salt

b)

Liquid

c)

Nonmetal

d)

Electron

84.

The Atomic Number of an atom is the total number of what in the nucleus?

a)

Protons + Electrons

b)

Protons

c)

Neutrons

d)

Protons + Neutrons

85.

Three elements are listed below:

Atom 1: 15 protons, 15 neutrons, 15 electrons

Atom 2: 23 protons, 23 neutrons, 23 electrons

Atom 3: 23 protons, 24 neutrons, 23 electrons.

Which two atoms are isotopes of the same element?

a)

Atom 1

Atom 2

b)

Atom 1

Atom 3

c)

Atom 2

Atom 3

d)

None

86.

Which Group carries a +2 Ionic Charge?

a)

Group 1

b)

Group 2

c)

Group 16

d)

Group 17

87.

What charge does an atom have when it GAINS electrons?

a)

Positive

b)

Negative

c)

Neutral

88.

What is the mass number of this Neon atom?

a)

10

b)

11

c)

21

d)

20

89.

How many electrons does this magnesium ion have?

a)

24

b)

12

c)

10

d)

14

90.
Which atom has  4 neutrons?
a)
Li-6
b)
Li-7
c)
Li-8
d)
they have the same # of neutrons
91.

How many valence electrons does carbon have?

a)

4

b)

5

c)

6

d)

7

92.

USE THE PERIODIC TABLE

How many valence electrons does Neon have?

a)

18

b)

8

c)

10

d)

2

93.
Which of the following tables correctly lists the physical properties of metals and nonmetals?
a)
A
b)
B
c)
C
d)
D
94.
Silicon is a semiconductor and has properties of both metals and nonmetals. What type of element is Silicon? 
a)
Metal
b)
Nonmetal
c)
Metalloid
d)
Pretty
95.

Non-metals are located on the...

a)

Right side of the periodic table

b)

left side of the periodic table

c)

top row of the dinner table

d)

along the zig-zag line

96.

Metals are found on this side of the Periodic Table:

a)

Left side

b)

Right side

c)

On the stair-step line

d)

Below

97.
A student is given a sample of an unknown substance. He is asked to determine if it is classified as a metal, a metalloid, or a nonmetal. He discovered that the unknown element conducted some heat and electricity, had a shiny luster, and broke easily. This element is most likely a 
a)
metal
b)
nonmetal
c)
metalloid
d)
cannot be determined
98.

An anion will be a ____ ion.

a)

negative

b)

positive

c)

neutral

d)

synchronous

99.

An atom that has become charged by gaining or losing electrons.

a)

Ion

b)

Isotope

c)

Electron

d)

Valence Electron

100.

An atom's atomic mass comes from its

a)

Electrons

b)

Protons

c)

Electron Cloud

d)

Nucleus

101.

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

a)

covalent bond

b)

ionic bond

c)

metallic bond

d)

transfer bond

102.

What type of bond involves the transfer of electrons between atoms?

a)

covalent bond

b)

ionic bond

c)

metallic bond

d)

transfer bond

103.
When two atoms share electrons, a chemical bond is formed.  This type of bond is called:
a)
covalent bond
b)
ionic bond
c)
crystal bond
d)
polyatomic bond
104.

Which of these is covalent?

a)

NaCl

b)

KBr

c)

CO2

d)

AlCl3

105.

Which of the following is NOT formed by a covalent bond?

a)

K2S

b)

H2O

c)

I2

d)

CO2

106.

Select all properties of METALS.

a)

good conductors of heat and electricity

b)

brittle

c)

malleable and ductile

d)

lustrous

e)

semiconductor

107.

Select all properties of NONMETALS.

a)

good conductors of heat and eletricity

b)

good insulators; poor conductors

c)

brittle

d)

malleable and ductile

e)

form cations or no ions

108.
How many valence electrons are in an atom of Ar?
a)
2
b)
8
c)
4
d)
1
109.

Why is the atomic number important?

a)

It tells you the mass of the element

b)

It determines which isotope an atom is

c)

It determines the properties and locatation of an element.

d)

They are gained and lost to form ions.

110.
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
111.
Carbon 14 has
a)
6P 6N 6E
b)
6P 8N 6E
c)
8P 6N 6E
112.
Carbon 12 has 
a)
6 P 6 N 6E
b)
6P 8N 6E
c)
8P 6N 6E
113.

Metals tend to be ​ (a)   at room temperature.

Choose from the below words
solids
gases
liquids
plasma
invisible
not enough info to answer
solids and gases
114.

Nonmetals tend to be​ (a)   at room temperature.

Choose from the below words
gases
liquids
plasma
invisible
not enough info to answer
solids and gases
solids
115.

The only metal that is liquid at room temperature is (a)   .

116.

The only nonmetal that is liquid at room temperature is (a)   .

117.

What is the formula for calcium sulfide?

(a)  

118.

What is the formula for tetranitrogen decoxide?

(a)  

119.

What is the formula for lithium sulfide?

(a)  

120.

What is the formula for aluminum oxide?

(a)  

121.

What is the formula for dinitrogen pentachloride?

(a)  

122.

What is the forumula for dinitrogen pentoxide?

(a)  

123.

What is the name of CaCl2

​ (a)  

124.

What is the name of P2O5

(a)  

125.

What is the name of Li2O

(a)  

126.

What is the name of N2O

(a)  

127.

Identify the common substance that is very soluble in water.

a)

Oil

b)

Copper

c)

Salt

d)

Sand

128.

If a substance has a high melting point, dissolves in water and conducts electricity, it is probably which type of compound?

a)

Covalent

b)

Ionic

129.

Why do chemical bonds form?

a)

to exchange protons

b)

to be more stable

c)

to share nuclei

d)

to have 4 valence electrons

130.

Identify the following compound as ionic or covalent: SO2

a)

ionic

b)

covalent

131.

Identify the following compound as ionic or covalent: Ca(OH)2

a)

ionic

b)

covalent

132.

Is the formula S4N4 an ionic or covalent compound?

a)

ionic

b)

covalent

133.
Which is most likely to form a negative ion...
a)

an element from Group 7

b)
a metal
c)
an element from Group 1
d)
an element with atoms that have eight valence electrons
134.
When an atom loses a valence electron, it becomes a(n) _________ion.
a)
positive 
b)
negative
135.

Why do ionic bonds form?

a)

so the number of protons equals the number of electrons

b)

to fill the outermost energy level to make the atom stable

c)

so an atom can become unstable

136.

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

137.

Ca and Cl

a)

Ionic

b)

Covalent

138.

C and S

a)

Ionic

b)

Covalent

139.

Mg and F

a)

Ionic

b)

Covalent

140.

Is this atom stable or unstable?

a)

Stable

b)

Unstable

141.

How many valance electrons does this atom have?

a)

1

b)

2

c)

5

d)

8

142.

Atoms involved in a covalent bond are not charged, while atoms involved in an ionic bond are charged (negative or positive)

a)

true

b)

false

143.

Nitrogen, N, will form which of the following ions?

a)

N

b)

N-3

c)

N-5

d)

N+5

144.
Write the formula for barium + nitrogen
a)
Ba2N3
b)
Ba3N2
c)
BaN
d)
BaN3
145.
Write the correct chemical formula for Ag +  and  Br -
a)
AgBr
b)
silver bromide
c)
Ag2Br2
d)
gold bromide
146.

What will be the charge of a bromine ion?

a)

+7

b)

-7

c)

-1

d)

+1

147.
Which is the correct name for CaBr2?
a)
Calcium Bromine
b)
Bromine Calcium
c)
Calcium Bromide
148.
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
149.
How do the following two elements bond together?
Al3+  O2-         
a)
AlO
b)
Al2O3
c)
Al3O6
d)
Al3O2
150.

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

151.
Which of the following is a characteristic property of ionic compounds?
a)
They form hard, brittle crystals with characteristic shapes
b)
They have low melting points
c)
They have low boiling points
d)
They contain no charged particles
152.
Which of the following is NOT true of ionic compounds?
a)
Metal ions have a + charge
b)
Non-metal ions have a - charge
c)
They conduct electricity when they are solid
d)
They are arranged in a giant lattice
153.
Which of the following is NOT formed by a covalent bond?
a)
K2S
b)
H2O
c)
I2
d)
CO2
154.
Dense and poor conductors
a)
Ionic Bonds
b)
Covalent Bonds
c)
Both bonds
d)
Neither bond
155.
Low melting point
a)
Ionic Bonds
b)
Covalent Bonds
c)
Both bonds
d)
Neither bond
156.
Polar or Nonpolar types
a)
Ionic 
b)
Covalent
157.

A polar bond will share it's electrons

a)

twice.

b)

equally.

c)

unequally.

d)

never.

158.
Which side of a chemical equation is the reactant side?
a)
Left (before the yields sign)
b)
Right (after the yields sign)
159.

Si + S8 →Si2S4

a)

Synthesis

b)

Decomposition

c)

Single replacement

d)

Double replacement

160.

Pb(NO3)2 →PbO + NO2 + O2

a)

Synthesis

b)

Decomposition

c)

Single replacement

d)

Combustion

161.
AB + CD →AD + CB
a)
Double Replacement
b)
Single Replacement
c)
Synthesis
d)
Decomposition
162.

Cu + 2Ag(NO3) → 2Ag + Cu(NO3)

a)

Synthesis Reaction

b)

Decomposition Reaction

c)

Single Replacement Reaction

d)

Double Replacement Reaction

163.
This pictures simulates what type of reaction?
a)
Synthesis
b)
Decomposition
c)
Single Replacement
d)
Double Replacement
164.
Always starts with a hydrocarbon that reacts with oxygen and produces carbon dioxide and water. 
a)
Decomposition
b)
Synthesis
c)
Combustion
d)
Single Replacement
165.
The number in front of a compound or element is a 
a)
Subscript
b)
Coefficient
c)
Superscript
d)
Charge
166.

The Coefficient (3) in the Chemical Formula, 3H2O, tells you how many _____________ there are.

a)

Atoms of Hydrogen

b)

Atoms of Oxygen

c)

Atoms of Water

d)

Molecules of Water

167.
A chemical reaction is balanced when
a)
both sides have the same elements
b)
Both sides have the same  number of atoms
c)
Same subscripts
d)
Same coefficients
168.
If a reaction starts with a total 75g of reactants it should produce 
a)
a total of 40g of products
b)
a total of 75g of products
c)
a total of 180 g of products
d)
None of the above
169.
24 g of magnesium reacts with 38 g of fluorine to produce _____ g magnesium fluoride
a)
62 
b)
38
c)
24
d)
14
170.
Which equation best represents the law of conservation of mass? 
a)
A
b)
B
c)
C
d)
D
171.
Is this balanced?
2HgO → 2Hg + O2
a)
Yes
b)
No
172.

Is this equation balanced or unbalanced?

CH4 + 2O2--> CO2+ 2H2O

a)

balanced

b)

unbalanced

173.
Is this equation balanced or unbalanced? 
H2 + O2 --> H2O
a)
balanced
b)
unbalanced
174.

What are the reactants in the following chemical equation?

a)

CH4 and 2O2

b)

CO2 and 2H2O

175.

What are the products in the following chemical equation?

a)

CH4 and 2O2

b)

CO2 and 2H2O

176.

How many carbon atoms are on both sides of the equation?

a)

1

b)

2

c)

3

177.

Is the equation balanced?: 2H2O + O2 --> 4MgO + 3Fe

a)

yes

b)

no

178.

Balance this equation:

___H2 +___ Cl2 --->___ HCl

a)

It is balanced.

b)

H2 + Cl2 ---> 2HCl

c)

3H2 + Cl2 ---> 6HCl

d)

H2 + 3Cl2 ---> 6HCl

179.
How many HCl molecules do you need to balance this equation? 
Mg +  __HCl --->  MgCl2 + H2
a)
1
b)
2
c)
3
d)
4
180.

How does a balanced chemical equation satisfy the Law of Conservation of Mass?

a)

During a chemical reaction, matter is destroyed.

b)

During a chemical reaction, the total number of atoms increases.

c)

 During a chemical reaction, one or more new substances are formed.

d)

During a chemical reaction, the total amount of matter stays the same.

181.
Maria fills a bowl with 200 g of water. She puts the bowl of water in the freezer, and the water freezes. Which will most likely be the mass of the frozen water?
a)
50 g
b)
100 g
c)
200 g
d)
400 g
182.
What is a closed system?
a)
a system where none of the reactants or products are allowed to escape
b)
compounds made of thousands of repeating smaller molecules
c)
the output, or result of a chemical reaction
d)
occurs when the atoms and molecules of two or more substances rearrange to form new substances
183.
In a chemical reaction, the mass of the reactants was 15g.  The mass of the products was 12g.  Did this chemical reaction follow the law of conservation of mass?
a)
Yes 
b)
No
c)
You can't tell with the given infomation 
184.
A boiling pot of water on a stove is what type of system
a)
Closed System
b)
Open System
185.

Mr. Brady did an experiment. He started with 15 grams of mass. At the end, he had 13 grams of mass. What happened?

a)

His experiment was in an open system, so some mass escaped.

b)

His experiment was in a closed system so the mass did not change.

186.

How can the law of conservation of mass apply to a burning log, if all that remains of it is ash?

a)

The ash has the same mass as the log, although a large percentage of it blows away.

b)

The law of conservation of mass applies to changes of state but not to chemical reactions.

c)

The law of conservation of mass applies to substitution and displacement reactions, but not to combustion reactions.

d)

The masses of the gases released into the air plus the mass of ash equal the mass of the log before burning.

187.

Look at the following chemical equation. 2As + 6NaOH → 2Na3 AsO3 + 2H2

Does this equation follow the law of conservation of matter?

a)

Yes, because the mass of the reactants is equal to the mass of the products

b)

No, because the reactants contain more oxygen (O) atoms than the products.

c)

No, because the reactants contain more hydrogen (H) atoms than the products.

d)

Yes, because the reactants contain the same number of arsenic (As) atoms as the products.

188.

Chemical X has a mass of 5 grams, and chemical Y has a mass of 10 grams. If the two chemicals are mixed and a complete chemical reaction takes place, what is most likely the mass of the product?

a)

5g

b)

10g

c)

15g

189.
A student notices that an inflated balloon gets larger when it is warmed by a lamp. Which best describes the mass of the balloon as a result of this change?
a)
The mass of the balloon increases because the size of the balloon has increased.
b)
The mass of the balloon increases because the temperature of the balloon has increased.
c)
The mass of the balloon stays the same because the gas inside the balloon still has the same mass after it warms up.
190.

In a reaction A + B ----> C, reactant A has 5g and product C has 9g. How many grams does reactant B have?

a)

4g

b)

5g

c)

9g

d)

14g

191.
What will weigh more when a chemical change is complete?  The reactants before the chemical reaction, or the product after the reaction is complete?
a)
They both will weigh the same
b)
The product always weighs more than the reactant
c)
The reactant will weigh more than the product
d)
They both will loose mass after the reaction
192.
In the reaction AB-----> A + B reactant AB has 12g and product B has 5g. How many grams should product A have?
a)
17g
b)
2g
c)
7g
d)
None of the above

Similar Resources on Wayground

18.1 P Rates of Reaction

190 questions

18.1 P Rates of Reaction

quiz

Worksheet

•

9th Grade

Chemistry Regents review

192 questions

Chemistry Regents review

quiz

Worksheet

•

9th - 12th Grade