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Kennedy- Quarter 1 Final Exam review

Total questions: 161

Worksheet time: 8hrs 3mins

Name
Class
Date
1.

Which scientist discovered the electrons?

a)

Dalton

b)

Thomson

c)

Atristotle

d)

Bohr

2.

Bohr discovered that electrons are located in

a)

the nucleus

b)

inside protons

c)

electron cloud

d)

circular orbits around the nucleus

3.

What is a particle with one negative charge called?

a)

electron

b)

proton

c)

quark

d)

neutron

4.

The smallest particle of an element that still represents that element.

a)

Nucleus

b)

electron

c)

proton

d)

atom

5.

What is a particle with one positive charge called?

a)

proton

b)

electron

c)

neutron

d)

quark

6.

What is the center of an atom called?

a)

nucleus

b)

electron cloud

c)

proton center

d)

photon center

7.

What is the neutral particle found in the nucleus called?

a)

proton

b)

neutron

c)

electron

d)

quark

8.
Matter always has mass.
a)
true
b)
false
9.
In Dalton's Atomic Theory, all elements consist of __________ that cannot be divided.
a)
Atoms
b)
Parts
c)
Molecules
d)
Hydrogen
10.

Who was the Greek philosopher who called the smallest particle of matter an "atom"?

a)

Democritus

b)

Aristotle

c)

J.J Thompson

d)

Einstein

11.

Which of the following is/are conclusions based on Rutherford’s gold foil experiment?

a)

Atom is mostly empty space

b)

The nucleus is positively charged

c)

The atom has a small dense nucleus

d)

All answers are correct

12.
Who is the scientist who proposed the "solar system" model of an atom where the electrons orbit around the nucleus?
a)
Democritus
b)
Niels Bohr
c)
Ernest Rutherford
d)
Chadwick
13.
What is the number of protons that the element in this image contain?
a)
14
b)
7
c)
15
d)
18
14.
What number indicates the nucleus?
a)
1
b)
2
c)
3
d)
4
15.
Rutherford's gold foil experiment provided evidence that...
a)
negative and positive charges are spread evenly throughout the atom.
b)
alpha particles have a positive charge.
c)
gold is not a dense as previously thought.
d)
there is a dense positively charged nucleus at the center of an atom.
16.
J.J. Thomson provided evidence that an atom...
a)
is the smallest particle of matter
b)
contains negatively charged particles
c)
has an overall negative charge
d)
has an overall positive charge
17.
Which of the following is NOT a part of Dalton's atomic theory?
a)
All elements are composed of atoms.
b)
Atoms are alwyas in motion.
c)
Atoms of the same element are always identical.
d)
Atoms that combine do so in simple, whole-number ratios.
18.

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

19.

Which subatomic particle is not found in the nucleus of an atom?

a)

Proton

b)

Neutron

c)

Electron

d)

All of the above are found in the nucleus

20.

Isotopes of an element have a different number of...

a)

Protons

b)

Neutrons

c)

Electrons

d)

Mass

21.

Potassium-39 has how many neutrons?

a)

19

b)

18

c)

20

d)

21

22.

Nickel-59 has how many neutrons?

a)

30

b)

31

c)

32

d)

33

23.

Bromine-80 has how many neutrons?

a)

41

b)

42

c)

44

d)

45

24.

76 protons and 114 neutrons

a)

Osmium-114

b)

Osmium-76

c)

Osmium-190

d)

Osmium-190.23

25.

12 protons and 13 neutrons

a)

Mg-12

b)

Mg-13

c)

Mg-25

d)

Mg-24.305

26.

9 protons and 9 neutrons

a)

Fluorine-18

b)

Fluorine-9

c)

Fluorine-16

d)

Fluorine-18.998

27.

Rubidium has two common isotopes, 85Rb and 87Rb. If the abundance of 85Rb is 72.2% and the abundance of 87Rb is 27.8%, what is the average atomic mass of rubidium?

a)

85.468 amu

b)

37 amu

c)

85.6 amu

d)

86.4 amu

28.

There are two primary isotopes found in any sample of copper: copper-63 and copper-65. The isotope 65Cu composes 69.2% of the sample and 63Cu comprises the other 30.8%. Based on this data, what is the atomic mass of copper?

a)

29 amu

b)

63.546 amu

c)

64.4 amu

d)

63.6 amu

29.

How do you calculate mass number?

a)

Mass x percent

b)

Protons + Electrons

c)

Protons + Neutrons

d)

Neutrons + Protons + Electrons

30.

What is the name of group number 2?

a)

transition metals

b)

halogens

c)

metaloids

d)

alkaline earth metals

31.

What is the name of group number 1?

a)

halogens

b)

noble gases

c)

alkali metals

d)

alkaline earth metals

32.

where are the metaloids found

a)

far left, vertical

b)

stair step/diagonal

c)

far right horizontal

d)

at the bottom

33.

What group number are the halogens found?

a)

18 (8A)

b)

1

c)

2

d)

17 (7A)

34.

Periodic law states that the elements are arranged according to their atomic ________ so that elements with similar chemical properties are in the same ________ and properties repeat periodically.

a)

numbers, rows

b)

masses, rows

c)

masses, column

d)

numbers, column

35.

A row on the Periodic Table of Elements

a)

family

b)

period

c)

row

d)

isotope

36.

Metals (select all that apply)

a)

are found on the right side of the periodic table.

b)

are found on the left side of the periodic table.

c)

are good conductors of heat and electricity.

d)

are brittle.

e)

are malleable and ductile.

37.

Nonmetals (select all that apply)

a)

are found on the right side of the periodic table.

b)

are found on the left side of the periodic table.

c)

are good conductors of heat and electricity.

d)

are brittle.

e)

can be solid, liquids, or gases at room temperature.

38.

Which element has similar chemical properties as sodium but has 7 energy levels?

a)

Francium (Fr)

b)

Cesium (Cs)

c)

Rubidium (Rb)

d)

Potassium (K)

39.

Elements that have the same number of energy levels are said to be in the same ______.

a)

group

b)

period

c)

family

d)

classification

40.

Element symbols have _____ capital letter(s).

a)

1

b)

2

c)

3

d)

4

41.

Match the following

a)

lithium

1.

2 energy levels

b)

helium

2.

1 energy level

c)

aluminum

3.

3 energy levels

d)

bromine

4.

4 energy levels

e)

strontium

5.

5 energy levels

42.

Match the following elements to the group they belong to.

a)

sodium

1.

alkali metal

b)

calcium

2.

alkaline earth metal

c)

chlorine

3.

halogen

d)

argon

4.

noble gas

43.

Put the groups of the periodic table in order from group 1A to group 8A (18).

a)

alkali metals

b)

alkaline earth metals

c)

halogens

d)

noble gases

1)
2)
3)
4)
44.

What do the periods (rows) represent?

a)

an additional energy level

b)

an additional proton

c)

an additional group

d)

an additional electron

45.
The atoms along the staircase are called 
a)
metals
b)
nonmetals
c)
metalloids
d)
noble gases
46.

The blue elements (left side) are called 

a)
metals
b)
nonmetals
c)
metalloids
d)
noble gases
47.

The yellow elements (right side) are called 

a)
metals
b)
nonmetals
c)
metalloids
d)
noble gases
48.
a)
Same group
b)
Same period
49.

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.

50.

Elements in the same group have : (2 correct answers)

a)

Similar chemical properties

b)

Similar names

c)

Same number of outer (valence) electrons)

d)

The same number of protons

51.

Mendeleev was the first person to arrange the elements into a table. How did he arrange the rows?

a)
alphabetical 
b)
density
c)
melting point
d)
atomic mass
52.

According to the Octet Rule, to achieve stability atoms attempt to fill the outer S and P orbitals. How many electrons are required to accomplish this?

a)

2

b)

4

c)

6

d)

8

53.

Which of the following elements will most likely form cations?

a)

Oxygen

b)

Iodine

c)

Magnesium

d)

Sulfur

54.

Which of the following has the greatest Atomic Radii?

a)

Rb

b)

In

c)

Sb

d)

Xe

55.

Which property describes the measure of an atom's attraction for another atom's electrons?

a)

atomic radii

b)

electronegativity

c)

electron affinity

d)

ionization energy

56.

Which of the following groups of elements have the highest ionization energy?

a)

alkali metals

b)

alkaline earth metals

c)

halogens

d)

noble gases

57.

Definition of ionization energy is

a)

The energy required to remove an electron

b)

The energy required to add an electron

c)

The ability to attract an electron

d)

The distance from the nucleus to the outermost electron

58.

What group contains elements with 7 valence electrons

a)

Noble Gasses

b)

Alkali Earth Metals

c)

Halogens

d)

Transition Metals

59.

Select the element that has 3 valence electrons

a)

Calcium

b)

Sodium

c)

Aluminum

d)

Sulfur

60.

Select the element below that is least reactive

a)

Hydrogen

b)

Chlorine

c)

Lithium

d)

Neon

61.

Select the group that is the most reactive metals

a)

Transition Metals

b)

Alkali Earth Metals

c)

Alkali Metals

d)

Halogens

62.

What is a negatively charged atom called?

a)

Anion

b)

Cation

63.

The element with the highest electronegativity is -

a)

At

b)

F

c)

Cl

d)

Br

64.

How does electronegativity change from top to bottom in a group in the periodic table?

a)

It decreases

b)

It remains constant

c)

It increases

d)

It fluctuates randomly

65.

How does electronegativity change from left to right within a period in the periodic table?

a)

It decreases

b)

It increases

c)

It fluctuates randomly

d)

It remains constant

66.

What is electronegativity?

a)

The number of protons in an atom

b)

The measure of an atom's attraction to electrons

c)

The amount of energy needed to remove an electron from an atom

d)

The size of the atom

67.

If an electron is closer to the nucleus, it will be (harder, easier) to remove that electron and its ionization energy will be (high, low )

a)

Easier, High

b)

Easier, Low

c)

Harder, High

d)

Harder, Low

68.

How does ionization energy change from top to bottom in a group in the periodic table?

a)

It remains constant

b)

It decreases

c)

It increases

d)

It fluctuates randomly

69.

How does ionization energy change from left to right within a period in the periodic table?

a)

It fluctuates randomly

b)

It increases

c)

It decreases

d)

It remains constant

70.

What is ionization energy?

a)

The measure of an atom's attraction to electrons

b)

The number of protons in an atom

c)

The amount of energy needed to remove an electron from an atom

d)

The size of the atom

71.
Which atom has the largest atomic radius?
a)
potassium
b)
rubidium 
c)
francium
d)
cesium
72.

Atomic radius decreases from left to right across a period because from left to right there is

a)

increasing number of valence electrons

b)

increasing shielding

c)

increasing effective nuclear charge (from increasing protons in the nucleus)

d)

increasing number of electron shells

73.

What happens to the atomic radius as you go from left to right within a period in the periodic table?

a)

It fluctuates randomly

b)

It increases

c)

It remains constant

d)

It decreases

74.
As you move down the periodic table atoms get bigger.  This is because ____________.
a)
The atoms have more mass.
b)
The atoms have more protons.
c)
The atoms have more energy levels
d)
The atoms have more nuetrons
75.

What is atomic radius?

a)

The number of protons in an atom

b)

The amount of energy needed to remove an electron from an atom

c)

The size of the atom

d)

The measure of an atom's attraction to electrons

76.

Ionic Bonding involves...

a)

the transfer of protons

b)

the transfer of neutrons

c)

the transfer of electrons

d)

none of these choices

77.

What do atoms that form positive ions tend to do?

a)

tend to lose electrons

b)

tend to lose protons

c)

tend to gain electrons

d)

tend to gain protons

78.

What elements generally compose a covalent bond?

a)

metal and nonmetal

b)

2 or more nonmetals

c)

metal

d)

none of the above

79.

Magnesium Bromide is a (an) ________ compound

a)

metallic

b)

covalent

c)

ionic

d)

organic

80.

How is the bond in F2 different from the bond in KCl ?

a)

F2 is covalent and KCl is ionic

b)

F2 is ionic and KCl is covalent

c)

F2 is ionic and KCl is ionic

d)

F2 is ionic and KCl is ionic

81.

When naming COVALENT/MOLECULAR compounds, you use ______ to indicate the amount of each element in the name.

a)

prefixes

b)

coefficients

c)

subscripts

d)

superscripts

82.

Phosphorous trichloride

a)

PCl3

b)

P3Cl

c)

P3Cl3

d)

PCl

83.

The formula for the ionic compound of magnesium and nitrogen would be

a)

MgN2

b)

MgN

c)

Mg3N2

d)

MgN3

84.

What is the formula for magnesium phosphide?

a)

Mg3P2

b)

Mg2P3

c)

Mg2PO4

d)

Mg3(PO4)2

85.

What is the chemical name for NI3 ?

a)

Nitrogen hydroxide

b)

Nitrogen trinitride

c)

Nitrogen triiodide

d)

Triiodide mononitrogen

86.

Why do elements bond?

a)

To be friends

b)

To create a new element

c)

To become stable

d)

To get bigger

87.
If an atom gains two electrons what charge will it have?
a)
-2
b)
-1
c)
+1
d)
+2
88.
Nitrogen will ____ valence electrons when forming an ionic bond.
a)
gain 1
b)
lose 1
c)
gain 3
d)
lose 3
89.
Beryllium will ____ valence electrons when forming an ionic bond.
a)
lose 4
b)
gain 4
c)
lose 2
d)
gain 2
90.

What is the reason why Noble gases are so stable?

a)

They have an even number of electrons

b)

They have no electrons

c)

They have a full outer shell of electrons

d)

They bond with other atoms

91.

Covalent bonds are formed between...

a)

2 non-metals

b)

a metal and a non-metal

c)

2 metals

d)

2 ions

92.

Why are there two sodiums (Na), in the formation of this ionic compound?

a)

There always has to be 2 metals

b)

The overall charge needs to add up to 4

c)

The overall charge has to be 0

d)

It needs to have more metal atoms than nonmetal

93.

Using the model for the formation of Scandium Fluoride (an ionic compound), write the chemical formula.

a)

Sc3F

b)

Sc3F3

c)

Sc+3F-1

d)

ScF3

94.

Using the model, write the chemical formula for an ionic compound that has Mg and Cl.

a)

MgCl2

b)

Mg2Cl2

c)

Mg+2Cl-1

d)

Mg2Cl2

95.

Contrast polar and nonpolar bonds.

a)

A polar bond will unequally share electrons and a nonpolar bond will equally share electrons

b)

A polar bond will share electrons equally and a nonpolar bond will unequally share electrons

c)

Polar bonds are covalent and nonpolar bonds are ionic

d)

None of the above

96.

A student wants to combine Zn and HCl to form NEW compound. What would likely form?

a)

ZnH2 + Cl2

b)

ZnCl2 + H2

c)

There will be no reaction

d)

CuH2 + Cl2

97.

Water is a polar covalent molecule. Which of the following applies

a)

Sugar dissolves easily in water. Polar substances dissolve in other polar substances

b)

Sugar DOESN'T dissolve in water. Polar substances dissolve in other polar substances.

c)

Sugar dissolves easily in water. Polar substances DON'T dissolve easily in other polar substances

d)

Sugar DOESN'T dissolve in water. Polar substances dissolve in nonpolar substances.

98.

What makes a covalent bond polar?

a)

One atom has a HIGHER electronegativity than the other- so it hogs electrons

b)

One atom has a LOWER electronegativity than the other- so it hogs electrons

c)

The are the same element and have the same electronegativity

d)

They are found at the North Pole

99.

There are 3 substances on the table. Substance A is a white powder with a high melting point and conducts in a solution. Substance B is a silver gray solid with a high melting point. Substance C is a white solid with a low melting point that doesn't conduct. Based on the properties, what are the bonds of each material.

a)

A has covalent bonds, B has ionic bonds, and C has metallic bonds

b)

B has covalent bonds, C has ionic bonds, and A has metallic bonds

c)

C has covalent bonds, A has ionic bonds, and B has metallic bonds

d)

Not enough information

100.

What is happening to the electrons during a covalent bond?

a)

The electrons are being shared

b)

One element is taking electrons, another is giving away electrons

c)

The electrons don't move

d)

Both atoms give away electrons

101.

What is happening to the electrons during an ionic bond

a)

They are sharing electrons

b)

The electrons don't move

c)

One atom takes the electrons, one gives them away

d)

They both give away electrons

102.

Which is of the following is NOT true about ionic compounds?

a)

Ionic compounds are brittle

b)

Ionic compounds melt easily

c)

Ionic compounds conduct electricity in water

d)

Ionic compounds are made of positive and negative ions

103.

Why do ionic bonds form?

a)

They share electrons

b)

The two anions have the same change, so they are attracted to each other

c)

The two cations have an opposite charge, so they are attracted to each other

d)

The cation and anion have opposite charges, and opposite charges attract.

104.

What is the definition of a covalent bond?

a)

A covalent bond is a chemical bond that involves the repulsion of like charges between atoms.

b)

A covalent bond is a chemical bond that involves the attraction of opposite charges between atoms.

c)

A covalent bond is a chemical bond that involves the transfer of electron pairs between atoms.

d)

A covalent bond is a chemical bond that involves the sharing of electron pairs between atoms.

105.

What is a synthesis reaction?

a)

A synthesis reaction is a type of chemical reaction in which two or more complex substances combine to form a simpler substance.

b)

A synthesis reaction is a type of chemical reaction in which two or more substances combine to form a substance with the same properties as the original substances.

c)

A synthesis reaction is a type of chemical reaction in which two or more simple substances combine to form a more complex substance.

d)

A synthesis reaction is a type of chemical reaction in which two or more substances break down into simpler substances.

106.

What is a decomposition reaction?

a)

A decomposition reaction is a type of chemical reaction where a compound releases energy in the form of heat and light.

b)

A decomposition reaction is a type of chemical reaction where a compound breaks down into simpler substances or elements.

c)

A decomposition reaction is a type of chemical reaction where a compound combines with other substances to form a more complex compound.

d)

A decomposition reaction is a type of chemical reaction where a compound undergoes a phase change from solid to liquid.

107.

What is a double replacement reaction?

a)

A double replacement reaction is a chemical reaction where two compounds exchange atoms to form two new compounds.

b)

A double replacement reaction is a chemical reaction where two compounds break down into multiple compounds.

c)

A double replacement reaction is a chemical reaction where two compounds combine to form a single compound.

d)

A double replacement reaction is a chemical reaction where two compounds exchange ions to form two new compounds.

108.

The difference in electronegativity affects the type of bond will be formed. What type of bond would be formed with a difference of 0.8?

a)

Nonpolar Covalent

b)

Polar Covalent

c)

Ionic

109.

__________ bonds involve an unequal sharing of electrons, while __________ bonds involve an equal sharing of electrons.

a)

Nonpolar, polar

b)

Polar, metallic

c)

Metallic, nonpolar

d)

Polar, nonpolar

110.

Which electrons are involved in a chemical bond?

a)

Valence electrons

b)

Inner shell electrons

c)

Electrons are not involved in bonding

111.

If sodium and oxygen formed a bond, it would be classified as --

a)

polar covalent

b)

nonpolar covalent

c)

ionic

d)

metallic

112.

Which bond involves an unequal sharing of electrons?

a)

Ionic bond

b)

Nonpolar covalent bond

c)

Polar covalent bond

d)

Metallic bond

113.
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
114.
How are covalent bonds formed?
a)
Sharing of electrons
b)
Transfer of electrons
115.

Which one of the following statements is true?

a)

The salt solution conducts electricity.

b)

The sugar solution conducts electricity.

c)

The pure water conducts electricity.

116.

Which of the following statements describes a polar molecule? 

a)

because electrons are transferred between atoms, the molecule conducts electricity

b)

electrons are equally shared between atoms, giving them a negative charge

c)

molecule has unequal sharing of electrons, atoms have slightly positive or negative charge

d)

a polar molecule is perfectly symmetrical, electrons travel freely around atoms

117.

Water is polar. Which bonds will it dissolve (more than 1 must be checked)?

a)

ionic

b)

metallic

c)

nonpolar

d)

polar

118.

How is a chemical change different from a physical change?

a)

there is no difference

b)

a physical change creates a new substance

c)

a chemical change creates a new substance

119.

A precipitate is a ___________ that forms when 2 liquids react together.

a)

solid

b)

liquid

c)

gas

d)

plasma

120.
Is burning wood a chemical or physical change?
a)
chemical
b)
physical
121.
Is a a rusting bicycle a chemical or physical change?
a)
chemcial
b)
physical
122.
Is melting ice a chemical or physical change?
a)
chemical
b)
physical
123.
Is spoiling food a physical or chemical change?
a)
phyiscal
b)
chemical
124.
Salt dissolves in water
a)
physical Change
b)
chemical change
125.
Which is a chemical change?
a)
freezing fruit juice
b)
slicing a potato
c)
boiling water
d)
copper metal turning green
126.

Which of the following observations would indicate a chemical change has happened? Select ALL correct answers.

a)

a solid precipitate forms

b)

heat energy is released

c)

breaks into smaller pieces

d)

folded in half

e)

a gas is produced

127.

Bubbles form when water boils. Is this evidence of chemical change?

a)

Yes, because water is changing.

b)

Yes, because the water is reacting.

c)

No, because the vapor is still water.

d)

No, because water doesn't react with anything.

128.

Every chemical change involves __________.

a)

dissolving substances

b)

the release of light and heat

c)

an increase in density

d)

the formation of a new substance

129.

What is the Law of Conservation of matter?

a)

Matter is created in a chemical reaction

b)

Matter is created in a physical change

c)

New chemicals formed from a chemical reaction have a larger overall matter than the original reactants

d)

Matter is never created or destroyed

130.
An oreo cookie weighs 20 grams.  It gets crushed into crumbs for a recipe.  How much do its crumbs weigh?
a)
15 grams
b)
25 grams
c)
20 grams
131.

If the mass of a chemical reaction's product is 15 grams, what would the mass of the reactants be?

a)

20 g

b)

15 g

c)

10 g

d)

3 g

132.

Why does this picture demonstrate the Law of Conservation of Matter?

a)

the number of atoms of each element are the same on both sides

b)

they start out separate and end up combined

c)

the same elements are used

d)

it doesn't demonstrate the Law of Conservation of Matter

133.

Is the following reaction balanced?

H2 + O2 ⟶ H2OH_2\ +\ O_2\ \longrightarrow\ H_2O  

a)

Yes

b)

No

134.

Is the following reaction balanced?

2KClO3 ⟶ 2KCl + 3O22KClO_{3\ }\longrightarrow\ 2KCl\ +\ 3O_2  

a)

Yes

b)

No

135.

Is the following reaction balanced?

10P + 4O2 ⟶ 2P2O510P\ +\ 4O_{2\ }\longrightarrow\ 2P_2O_5  

a)

Yes

b)

No

136.

Which number is needed to balance the following equation?


2K + MgBr2 ⟶ …KBr + Mg2K\ +\ MgBr_2\ \longrightarrow\ \ldots KBr\ +\ Mg  

a)

3

b)

1

c)

2

d)

4

137.

Which number is needed to balance the following equation?


2Na + 2H2O ⟶ 2NaOH +…H22Na\ +\ 2H_2O\ \longrightarrow\ 2NaOH\ +\ldots H_2  

a)

2

b)

1

c)

3

d)

4

138.

Classify:

2H2 + O2 ---->2H2O

a)

synthesis reaction

b)

decomposition reaction

c)

single replacement reaction

d)

double replacement reaction

139.

Classify:

2KClO3 ---->2KCl + 3Os

a)

synthesis reaction

b)

decomposition reaction

c)

single replacement reaction

d)

double replacement reaction

140.

Classify:

Mg + 2HCl ----> MgCl2 + H2

a)

synthesis reaction

b)

decomposition reaction

c)

single replacement reaction

d)

double replacement reaction

141.

Classify:

2HCl + 2NaOH -----> NaCl + H2O

a)

synthesis reaction

b)

decomposition reaction

c)

single replacement reaction

d)

double replacement reaction

142.

Classify:

CH4 + O2 → CO2 + H2O

a)

single replacement

b)

double replacement

c)

synthesis

d)

combustion

143.
What are the products of this reaction?
Cu+ AgNO3--> 
a)
Cu(NO3)2+Ag
b)
CuNO3 + Ag
c)
CuAg+NO3
d)
Cu+ AgNO3
144.
Predict the products for the this reaction:
K + HCl --> 
a)
KCl + H2
b)
KHCl 
c)
KH + Cl2
d)
KCl + H
145.
Predict the products for the this reaction:
Mg + CuCl2 --> 
a)
MgCl2 + Cu
b)
MgCl + Cu
c)
MgCu + Cl2
d)
CuMg + Cl2
146.

Predict the products for the this Double Replacement reaction:

AgNO3 + KCl →

a)

AgCl + KNO3

b)

AgK + ClNO3

c)

KAg + NO3Cl

d)

AgCl + 3 KNO

147.

If an element is diatomic it should have a subscript of___

a)

1, always

b)

2, only when it is an element

c)

it shouldn't have a subscript, it should have a coefficent

d)

2, when bonded in a compound

148.

For the following equation, identify the reaction and predict the products: (SELECT TWO ANSWERS)

Be(NO3)2+RbF⟶Be\left(NO_3\right)_2+RbF_{ }\longrightarrow  

a)

Single Replacement

b)

Decomposition

c)

Double Replacement

d)

BeF2 +RbNO3BeF_2\ +RbNO_3  

e)

BeRb2 +F(NO3)2BeRb_{2\ }+F\left(NO_3\right)_2  

149.

Which box has a higher density?

a)

A

b)

B

c)

They are the same

150.
What is the formula for density?
a)
density = mass x volume
b)
density = mass / volume
c)
density = mass + volume
d)
density = mass - volume
151.
Frank has a paper clip. It has a mass of 9g and a volume of 3cm3. What is its density?
a)
3 g/cm3
b)
1/3 g/cm3
c)
27 g/cm3
d)
39 g/cm3
152.
A piece of copper has a mass of 89g and a volume of 10 cm3.  What would be the density of the copper?
a)
0.89 g/cm3
b)
89 g/cm3
c)
8.9 g/cm3
d)
890 g/cm3
153.

An object has a volume of 6 cm3 and a mass of 42 g. What's it's density?

a)

7 g/cm3

b)

48 g/cm3

c)

42 g/cm3

d)

6 g/cm3

154.
In the picture, the mass of the block is 200 g, the dimensions of the block are 6 cm by 4 cm by 5 cm.  What is its density?
a)
1.67g/cm3
b)
13.33 g/cm3
c)
0.60 g/cm3
d)
 24000 g/cm3
155.
Which liquid is the least dense?
a)
oil
b)
water
c)
syrup 
d)
plastic bottle
156.

Which has the greatest density?

a)

A

b)

B

c)

C

d)

All the same density

157.
An object with which of the following densities will float on water?
a)
0.7 g/cm3
b)
1.2 g/cm3
c)
3.5 g/cm3
d)
11.4 g/cm3
158.

Let's practice! Before reads 50 mL. After we drop in the object, the new water level goes up to 60 mL. What is the volume of the blocks?

a)

8 mL

b)

10 mL

c)

60 mL

d)

5 mL

159.
Which of the following would float on water? Remember, water has a density of 1.0g/cm3 . 
a)
Honey 1.30 g/cm3
b)
Lamp Oil .80 g/cm3
c)
Pepsi 1.04 g/cm3 
160.
Which liquid is the most dense?
a)
corn syurp
b)
water
c)
glycerine
d)
corn oil
161.
What is the volume of the rock?
a)
30cm3
b)
10cm3
c)
40cm3
d)
20cm3

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