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Honors Science - Fall Interim Review Unit 2

Total questions: 187

Worksheet time: 2hrs 15mins

Name
Class
Date
1.
Smallest particle of an element that retains the element's properties
a)
atom
b)
molecule
c)
element
d)
compound
2.
A positively charged particle located in the nucleus of an atom
a)
proton
b)
neutron
c)
electron
d)
atom
3.
A small particle in the nucleus of the atom, with no electrical charge
a)
proton
b)
neutron
c)
electron
d)
atom
4.
A tiny, negatively charged particle that moves around the nucleus of an atom.
a)
proton
b)
neutron
c)
electron
d)
atom
5.
A particle that is electrically charged (positive or negative)
a)
atom
b)
ion
c)
isotope
d)
neutral
6.
Atoms of the same element with the same number of protons (atomic number) but a different atomic mass (number of neutrons).
a)
atom
b)
ion
c)
isotope
d)
neutral
7.
number of protons in an atom, its identity
a)
atomic number
b)
atomic mass
c)
chemical symbol
d)
element
8.
number of protons plus the number of neutrons
a)
atomic number
b)
atomic mass
c)
chemical symbol
d)
element
9.
positively-charged ion
a)
atom
b)
cation
c)
anion
d)
neutral
10.
negatively-charged ion
a)
atom
b)
cation
c)
anion
d)
neutral
11.
region of an atom containing protons and neutrons, where most of the mass of an atom is
a)
atom
b)
nucleus
c)
electron cloud
d)
atomic number
12.
region of an atom containing negatively charged particles, very little of the atom's mass is contained here
a)
atom
b)
nucleus
c)
electron cloud
d)
atomic number
13.
horizontal row on the periodic table
a)
atom
b)
period
c)
group
d)
family
14.
vertical column on the periodic table
a)
atom
b)
period
c)
group
d)
row
15.
the electrons in the outermost shell (main energy level) of an atom; these are the electrons involved in forming bonds
a)
atom
b)
valence e-
c)
orbit
d)
group
16.
a type of element that is shiny and conducts heat and electricity well
a)
metal
b)
nonmetal
c)
metalloid
17.
a type of element that conducts heat and electricity poorly
a)
metal
b)
nonmetal
c)
metalloid
18.
a type of element that has properties of both metals and nonmetals
a)
metal
b)
nonmetal
c)
metalloid
19.
a pure substance made up of only one kind of atom
a)
element
b)
compound
c)
homogenous mixture
d)
heterogenous mixture
20.
a pure substance made up of atoms of two or more different elements joined by chemical bonds
a)
element
b)
compound
c)
homogenous mixture
d)
heterogenous mixture
21.
a mixture in which the composition is uniform throughout
a)
element
b)
compound
c)
homogenous mixture
d)
heterogenous mixture
22.
a mixture that is not uniform in composition, components are not evenly distributed throughout the mixture
a)
element
b)
compound
c)
homogenous mixture
d)
heterogenous mixture
23.
an element found in group 17 of the periodic table, very reactive
a)
halogen
b)
noble gases
c)
alkali metals
d)
alkaline earth metals
24.
atoms that have completely filled energy levels or that have 8 electrons in their outermost energy level - do no easily lose electrons (group 8/18)
a)
halogen
b)
noble gases
c)
alkali metals
d)
alkaline earth metals
25.
group 1, only 1 electron in the outer level, very reactive, soft, silver, shiny, low density
a)
halogen
b)
noble gases
c)
alkali metals
d)
alkaline earth metals
26.
metallic elements in group 2 of the periodic table, harder than alkali metals and less reactive
a)
halogen
b)
noble gases
c)
alkali metals
d)
alkaline earth metals
27.

The vertical (up and down) columns in the Periodic Table are called

a)

groups

b)

towers

c)

periods

d)

atomic numbers

28.
The Modern Periodic Table of Elements is arranged by
a)
atomic mass
b)
atomic number
c)
valence electrons
d)
number of isotopes
29.
Which group of the periodic table is composed of inert (not reactive)  gases?
a)
alkali metals
b)
alkaline earth metals
c)
halogens
d)
noble gases
30.
Which is an alkali metal?
a)
Magnesium
b)
Iron
c)
Sodium
d)
Europium
31.
Which is a halogen?
a)
Helium
b)
Chlorine
c)
Oxygen
d)
Neptune
32.
Elements in a ..................have similar chemical properties.  
a)
period
b)
group
c)
row
33.

The letter, C, is a ... of carbon.

a)

Name

b)

Nickname

c)

Chemical Symbol

d)

Pseudonym

34.

Which of the following are physical properties of metal?

a)

Luster

b)

Conductivity

c)

Malleability

d)

Ductility

35.

True or False: The reactivity of metals tends to decrease as you move from left to right across the periodic table.

a)

True

b)

False

36.

Name this group: These metals are the most reactive.

a)
b)
c)
d)
37.

Name this group: These metals are the second most reactive.

a)
b)
c)
d)
38.

Name this group: These metals are the second most reactive.

a)
b)
c)
d)
39.

Name this group: These metals contain familiar metals such as gold, iron, and copper.

a)
b)
c)
d)
40.

Name this group: These metals, located near the nonmetals, are never found uncombined in nature.

a)
b)
c)
d)
41.

Find these groups: Locate Lanthanides and Actinides.

a)
b)
c)
d)
42.

Which of the following could be properties of nonmetals?

a)

Poor electrical conductivity

b)

Poor thermal conductivity

c)

Dullness

d)

Brittleness

43.

I am a metal


I am in group 2


I am in period 6


I am…

a)

Mo

b)

Re

c)

S

d)

Ba

44.

I am a nonmetal


I am in period 2


I am in group 16/6A

a)

Ba

b)

Si

c)

Ba

d)

O

45.

Find an element with similar chemical properties to Barium (Ba).

a)

Ca an Ra, because they are in the same group and have similar chemical properties.

b)

Cs and La, b/c they are in the same period number.

c)

Ca and Y, b/c they are 90 degree angle and have similiar properties.

46.
Atoms gain or lose electrons to get a full outermost energy level.
a)
Octet Rule
b)
Law of Conservation
c)
Cation
d)
Anion
47.
They normally lose electrons during chemical reactions. Usually, form positive ions.
a)
Metals
b)
Nonmetals
c)
Metalloids
d)
Anion
48.
They normally gain electrons during chemical reactions. Usually form negative ions.
a)
Metals
b)
Nonmetals
c)
Metalloids
d)
Cation
49.
An atom that has an electrical charge from losing or gaining electrons.
a)
Isotope
b)
Ion
c)
Nucleus
d)
Electron Cloud
50.
An ion with a positive charge. Formed by losing electrons. Usually metals or Hydrogen become this way.
a)
Cation
b)
Anion
c)
Ion
d)
Atom
51.
An ion with a negative charge. Formed by gaining electrons. Usually nonmetals become this way
a)
Cation
b)
Anion
c)
Ion
d)
Atom
52.
The force that holds atoms together.
a)
Octet Rule
b)
Law of Conservation
c)
Chemical bonding
d)
nucleus
53.
a chemical bond between oppositely charged ions - metal bonded to non metal
a)
Octet Rule
b)
Ionic Bond
c)
Covalent Bond
d)
Atomic Bond
54.
A shorthand representation of the valence electrons in an atom.
a)
Octet Rule
b)
Electron dot diagram
c)
chemical formula
d)
chemical bonding
55.
Chemical symbols that show the ratio and amount of elements in a compound.
a)
Chemical formula
b)
Reactants
c)
Products
d)
Subscripts
56.
tell the amount of atoms in an element or compound; immediately follows what it is describing
a)
Chemical formula
b)
Reactants
c)
Subscripts
d)
Coefficients
57.
the numbers that appear before the formulas to represent the number of molecules or elements there are
a)
Chemical formula
b)
Reactants
c)
Subscripts
d)
Coefficients
58.
A starting material in a chemical reaction
a)
Chemical formula
b)
Reactants
c)
Subscripts
d)
Coefficients
59.
The elements or compounds produced by a chemical reaction.
a)
Chemical formula
b)
Reactants
c)
Products
d)
Coefficients
60.
Shows how many electrons can be shared, lost or gained to become stable; you cancel out the valence numbers to make the compound
a)
Lewis dot structure
b)
Oxidation numbers
c)
Periods
d)
Coefficients
61.
substance dissolved in water
a)
malleability
b)
ductility
c)
aqueous solution (aq)
d)
heterogenous mixture
62.
metal being hammered into a thin sheet
a)
malleability
b)
ductility
c)
chemical property
d)
density
63.
metal that can be drawn into a thin wire
a)
malleability
b)
ductility
c)
chemical property
d)
density
64.
outermost electrons which will determine bonding.
a)
valence electrons
b)
covalent bond
c)
ionic bond
d)
Electron Cloud
65.
a chemical bond that results from the sharing of electrons - non metal bonded to non metal
a)
ionic bond
b)
covalent bond
c)
chemical reaction
d)
cation
66.
Matter is not created nor destroyed in any chemical or physical change
a)
Octet Rule
b)
Law of Conservation
c)
Cation
d)
Anion
67.
A+B-->AB
a)
synthetic reaction
b)
decomposition reaction
c)
single replacement reaction
d)
double replacement reaction
68.
AB --> A + B
a)
synthetic reaction
b)
decomposition reaction
c)
single replacement reaction
d)
double replacement reaction
69.
AB+C->AC+B
a)
synthetic reaction
b)
decomposition reaction
c)
single replacement reaction
d)
double replacement reaction
70.
AB + CD --> AD + CB
a)
synthetic reaction
b)
decomposition reaction
c)
single replacement reaction
d)
double replacement reaction
71.
A compound that consists of positive and negative ions; typically a metal and nonmetal
a)
ionic compound
b)
covalent compound
c)
cation
d)
anion
72.
a chemical compound formed by the sharing of electrons
a)
ionic compound
b)
covalent compound
c)
Cation
d)
Anion
73.
A measure of the extra positive or negative particles that an object has.
a)
atom
b)
isotope
c)
charge
d)
valence electron
74.

Why do all bonds form?

a)

so the number of protons equals the number of electrons

b)

so an atom can become unstable

c)

to fill the outermost energy level

75.
Ionic bonds are between...
a)
Metal and Non-metal
b)
Non-metal and Non-metal
c)
Metal and Metal
76.

What is a cation's charge?

a)

positive

b)

negative

c)

neutral

d)

depends on the element

77.

What is an anion's charge?

a)

positive

b)

negative

c)

neutral

d)

depends on the element's charge

78.

Is potassium a cation or an anion?

a)

cation

b)

anion

79.

How many atoms are there in the compound MgCO3?

a)

3

b)

4

c)

5

d)

6

80.

How many atoms of sulfur are in each molecule of H2SO4?

a)

1

b)

4

c)

2

d)

7

81.
Atoms are most stable when their outer shell is complete.
a)
true
b)
false
82.
How are ionic bonds formed?
a)
Transfer of electrons
b)
Sharing of electrons
83.
Why do elements bond?
a)
To be friends
b)
To create a new element
c)
To become stable
84.
Atoms that gain electrons become...
a)
negatively charged
b)
positively charged
c)
remain neutrally charged
d)
21
85.
octet rule
a)
atoms are most stable when surrounded by eight valence electrons
b)
Electrons on the outermost energy level of an atom
c)
An atom with the same number of protons but a different number of neutrons.
d)
the sum of the number of neutrons and protons in an atomic nucleus
86.

Lithium is in group 1 of the periodic table, which ion would it form?

a)

Li-

b)

Li2-

c)

Li+

d)

Li2+

87.

Generally, atoms form bonds so that _______________.

a)

Each atom loses its electrons

b)

Each atom has a stable electron configuration

c)

Each atom has an unstable electron configuration

d)

Each atom gains electrons

88.
Where are the nonmetals located on the periodic table? 
a)
Blue
b)
Red
c)
Green
89.

Which statements about the formation of ionic bonds in sodium chloride are true?

a)

A sodium atom transfers its valence electron to a chlorine atom.

b)

The oppositely charged ions attract each other in an ionic bond.

c)

A chlorine atom accepts a valence electron from a sodium atom.

d)

The chlorine atoms become positive ions.

e)

The sodium atoms become negative ions.

90.
electron dot diagram
a)
A model of an atom in which each dot represents a valence electron
b)
A particle in the nucleus that has a positive charge
c)
positively charged central part of an atom
d)
A pure substance made of only one kind of atom
91.

Ionic bonds are formed from a combination of metal elements and __________________ elements.

a)

non-metal

b)

receive

c)

metal

d)

donate

92.

In the formation of ionic bonds, the electrons will be ____________ from metal elements to non-metal elements.

a)

oppositely

b)

receive

c)

transferred

d)

donate

93.

Atoms form ions because they want to have a (a)   outer shell.

94.

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

95.

Oxygen is in group 6 of the periodic table, which ion would it form?

a)

O-

b)

O+

c)

O2-

d)

O2+

96.

What two types of atoms make a covalent bond?

a)

2 non-metals

b)

1 metal and 1 non-metal

c)

2 metals

97.
In chemical compounds, covalent bonds form when
a)
the electronegativity difference between two atoms is very large.
b)
electrons are completely transferred between two metals.
c)

pairs of electrons are shared between two non-metal atoms.

d)

two non-metal atoms are attracted to each other by opposite charges.

98.

Identify the following compound as ionic or covalent: SO2

a)

ionic

b)

covalent

99.

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

a)

ionic

b)

covalent

100.

Identify the following compound as ionic or covalent: CH3COOH

a)

ionic

b)

covalent

101.
What is it called when atoms share one pair of electrons?
a)
A double bond
b)
A triple bond
c)
A quadruple bond
d)
A single bond
102.
What is it called when atoms share two pairs of electrons?
a)
A double bond
b)
A single bond
c)
A triple bond
d)
A quadruple bond
103.

What is it called if there are three pairs of electrons being shared?

a)
Triple bond
b)
Bond length
c)
Tribond
d)
Chocolate Mousse
104.
In a covalent bond, one or more electrons are? 
a)
shared 
b)
lost 
c)
gained 
d)
transferred 
105.

What do we call the number of valence elctrons that most atoms need to become stable?

a)

triplet

b)

quartet

c)

octet

d)

heptet

106.

What group of elements does not tend to form compounds because they already have an octet?

a)

metalloids

b)

halogens

c)

noble gases

d)

metals

107.

What kind of bond forms when nonmetal/metalloid atoms share electrons with each other?

a)

metallic bond

b)

ionic bond

c)

covalent bond

108.
CO2
a)
Ionic
b)
Covalent
c)
Polyatomic Ion 
d)
Metallic 
109.
Ionic bonds form between metals and ____.
a)
metalloids
b)
metals
c)
nonmetals
110.

Nitrogen and Oxygen will make a ____________ bond

a)

ionic

b)

covalent

c)

metallic

111.
The chemical formula shows one carbon atom bonded to __________ oxygen atoms.
a)
one
b)
two
c)
three
d)
four
112.
Which of the following is the correct Lewis dot structure for the molecule fluorine (F2)?
a)
A
b)
B
c)
C
d)
D
113.

What type of bond does nitrogen gas form?

a)

ionic

b)

single covalent

c)

double covalent

d)

triple covalent

114.

What type of bond does oxygen gas form?

a)

ionic

b)

single covalent

c)

double covalent

d)

triple covalent

115.
What is the correct formula for this molecule?
a)
NH
b)
N3H
c)
NH3
d)
NH4
116.
Molten compound conducts electricity.
a)
ionic compound
b)
covalent compound
117.
Some are solids, some are liquids, and some are gases at room temperature.
a)
ionic compounds
b)
covalent compounds
118.
Molten compound does NOT conduct electricity.
a)
ionic compound
b)
covalent compound
119.

Have a low melting point (< 200°C)

a)
ionic compounds
b)
covalent compounds
120.
usually soft
a)
ionic compounds
b)
covalent compounds
121.

Which of the following describes covalent bonds?

a)

Bonds form because of opposite charges

b)

electrons are shared to fill outer electron shells

c)

Electrons are transferred between atoms

d)

Covalent bonds are magical

122.

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

123.

A material that has a low boiling point

a)

Ionic

b)

Covalent

c)

Both

124.

Cl2

a)

Ionic

b)

Covalent

c)

Both

125.

The valence electrons are shared when the outermost orbitals overlap.

a)

Ionic

b)

Covalent

c)

Both

126.
How many valence electrons does nitrogen have?
a)
3
b)

2

c)
5
d)
1
127.
How many valence electrons does hydrogen have?
a)
3
b)
2
c)
5
d)
1
128.
Low melting point and low solubility in water are general properties of ______________________ compounds
a)
ionic
b)
covalent
c)
chemical
d)
glucose
129.
The chemical formula shows one carbon atom bonded to __________ oxygen atoms.
a)
one
b)
two
c)
three
d)
four
130.

Can be brittle or hard

a)

ionic

b)

covalent

131.

Oppositely-charged ions attract each other

a)

ionic

b)

covalent

132.

Electrons are equally shared

a)

non-polar covalent

b)

polar covalent

c)

ionic

133.

Electrons are unequally shared

a)

non-polar covalent

b)

polar covalent

c)

ionic

134.

Which has the greater electronegativity:  H or F?

a)
H
b)
F
135.
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. 
136.
What elements have zero electronegativity?
a)
metals
b)
nonmetals
c)
metalloids
d)
noble gases
137.

LiBr is called

a)

lithium bromine

b)

lithium (I) bromine

c)

lithium bromide

d)

lithuim (I) bromide

138.

Which of these combinations is an ionic compound made of?

a)

Metal and Metal

b)

Nonmetal and Nonmetal

c)

Metal and Nonmetal

d)

Cation and Cation

139.

Name the following ionic compound: BeCl2

a)

beryllium chlorine

b)

beryllium II chloride

c)

beryllium chloride

d)

beryllium dichloride

140.

Name the following ionic compound: Cs2S

a)

cesium sulfide

b)

cesium sulfate

c)

cesium II sulfate

d)

cesium II sulfide

141.

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

a)

Metal

b)

Nonmetal

c)

Anion

d)

Cation

142.

The number that tells you if an ion has lost or gained electrons

a)

atomic number

b)

oxidation number

c)

mass number

d)

electron number

143.

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

144.

Name for NaH

a)

sodium hydrogen

b)

potassium hydride

c)

sodium hydride

d)

potassium hydrogen

145.

Formula for barium sulfide

a)

B2S3

b)

BaS

c)

Ba2S

d)

BaS2

146.

Name for PBr2

a)

phosphorus bromide

b)

phosphorus dibromide

c)

phosphorus dibromine

d)

phosphorus bromine

147.

Formula for Disilicon Heptasulfide

a)

SiS6

b)

SiS7

c)

Si2S6

d)

Si2S7

148.

Name for SrBr2

a)

strontium bromine

b)

strontium bromide

c)

strontium dibromide

d)

strontium dibromine

149.

Name for BaO

a)

Barium oxide

b)

Barium monoxide

c)

Monobarium oxide

d)

Monobarium monoxide

150.

Name for CO

a)

carbon monoxide

b)

carbon oxide

c)

monocarbon oxide

d)

carbide monoxide

151.

When cations and anions join, they form what kind of chemical bond?

a)

ionic

b)

Metalic

c)

Covalent

152.

Which of the following sets of elements will MOST LIKELY form an ionic bond?

a)

He, O

b)

Na, F

c)

Na, K

d)

Cl, F

153.

Which compound is MOST LIKELY formed using covalent bonds?

a)

K2O

b)

CaBr₂

c)

SiO₂

d)

KBr

154.

Which pair of elements would MOST LIKELY bond to form a covalently bonded compound?

a)

Na and F

b)

P and O

c)

Ba and Cl

d)

Mg and S

155.

Which of the following sets of elements will MOST LIKELY form an ionic bond?

a)

He, F

b)

Na, Cl

c)

Na, K

d)

Cl, He

156.

When two or more different elements are chemically combined, it forms a ___.

a)

mixture

b)

element

c)

solution

d)

compound

157.
This is used to represent the number of each atom being represented. 
a)
A Exponent
b)
The Coefficient
c)
A Molecule
d)
The Subscript
158.
This appears on the left side of a chemical formula, and represents how many molecules there are. 
a)
An Atom
b)
The Subscript
c)
A Molecule
d)
The Coefficient
159.
How many hydrogen atoms are in this chemical formula: 
a)
4 hydrogen atoms
b)
1 hydrogen atom
c)
2 hydrogen atoms
d)
3 hydrogen atoms
160.
How many oxygen atoms are in this chemical formula?
a)
7 oxygen atoms
b)
4 oxygen atoms
c)
3 oxygen atoms
d)
1 oxygen atoms
161.
How many oxygen atoms are in this chemical formula?
a)
6 oxygen atoms
b)
2 oxygen atoms
c)
3 oxygen atoms
d)
4 oxygen atoms
162.
Is this balanced?
2HgO → 2Hg + O2
a)
Yes
b)
No
163.
Is this balanced?
Al + O2 → 2Al2O3
a)
Yes
b)
No
164.
Law of conservation of mass states that 
a)
matter is created
b)
matter is destroyed
c)
matter is neither created nor destroyed
d)
matter does not change
165.
True or false.  Law of conservation of mass means that the number of atoms of the products is more than the number of atoms in the reactants. 
a)
True
b)
False
166.
What is the law of conservation of mass?
a)
The part of the universe being studied
b)
The rest of the universe that interacts with the system
c)
Within a closed system, mass does not change
d)
A system that freely exchanges matter and energy
167.
Can matter be created or destroyed?
a)
Yes, it can be created.
b)
Yes, it can be destroyed.
c)
No, matter is always conserved
d)
None of these
168.
The total amount of matter (atoms) before and after a chemical reaction (change), remains the same.
a)
True
b)
False
169.
What is the law of conservation of mass?
a)
Matter changes when reacted or changed.
b)
The mass of all reactants are changed during a physical or chemical change
c)
The mass of the reactants is the same as the mass of the products
d)
The mass of the products is different than the mass of the reactants.
170.
What is the Law of Conservation of mass?
a)
Mass is created in a chemical reaction
b)
Mass is created in a physical change
c)
New chemicals formed from a chemical reaction have a larger overall mass than the original reactants
d)
Mass is never created or destroyed
171.
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
172.
If four hydrogen atoms react with two hydrogen atoms, how many atoms will be in the product?
a)
6
b)
4
c)
8
d)
2
173.
What does the principle of conservation of mass mean?
a)
The total mass of the reactants is more than the products
b)
Matter is not created or destroyed
c)
The total mass of the reactants is less than the products
174.
The total amount of matter (atoms) before and after a chemical reaction (change), remains the same.
a)
True
b)
False
175.
During a chemical reaction, matter (mass) can change states (solid, liquid, gas) ...
a)
and CAN be created or destroyed
b)
but can NOT be created or destroyed
176.
The Law of Conservation of Matter is the reason a chemical equation MUST be:
a)
balanced
b)
unbalanced
177.
No atoms are gained or lost in a chemical reaction. The number of atoms:
a)
fluctuates (goes up and down)
b)
increases
c)
remains constant
d)
decreases
178.
The amount of matter you start with CAN BE DIFFERENT than the amount of matter you end with.
a)
True, it can be different
b)
False, it remains the same
179.

The chemical reaction AgNO3 + NaCl --> AgCl + NaNO3 is a

a)

single displacement

b)

double displacement

c)

composition

d)

decomposition

180.
A decomposition reaction can be represented as _____________________.
a)
AB  → A + B
b)
A + B → AB
c)
AB + CD → AC + BD
d)
A + BC → B + AC
181.
A chemical change in which a single compound breaks down into two or more simpler products is called a ______________________.
a)
single-replacement reaction
b)
synthesis reaction
c)
double-replacement reaction
d)
decomposition reaction
182.
This chemical equation for mercury oxide is an example of what type of reaction?
2HgO  → 2Hg + O2
a)
decomposition reaction
b)
synthesis reaction
c)
combustion reaction
d)
Marvin the Martian reaction
183.
A synthesis reaction can be represented as ________________________.
a)
AB + CD → AC + BD
b)
AB → A + B
c)
A + B → AB
d)
A + BC → B + AC
184.
This chemical equation for magnesium oxide is an example of what type of reaction?
2Mg + O2  → 2MgO
a)
decomposition reaction
b)
synthesis reaction
c)
single displacement reaction
d)
combustion reaction
185.

In an endothermic reaction, heat is ...

a)

taken in

b)

given out

186.
In an exothermic reaction, heat is ...
a)
taken in
b)
given out
187.

A substance that increases the rate of a reaction without being used up during the reaction is called a

a)

catalyst

b)

product

c)

reactant

d)

solute

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