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Final Review

Total questions: 100

Worksheet time: 3hrs 42mins

Name
Class
Date
1.

Data that can be counted or measured is

a)

Qualitative data

b)

Quantitative data

c)

an Inference

d)

an Observation

2.

An act of using one or more of your senses to gather information and take note of what occurs is

a)

Qualitative data

b)

Quantitative data

c)

an Inference

d)

an Observation

3.

A logical explanation of an observation that is drawn from prior knowledge or experience is

a)

Qualitative data

b)

Quantitative data

c)

an Inference

d)

an Observation

4.

Match the statement below to the correct description:


The volume of water was 32 mL.

a)

Qualitative data

b)

Quantitative data

5.

Match the statement below to the correct description:

When we mixed water and calcium chloride together in the beaker, the beaker got very hot.

a)

Qualitative data

b)

Quantitative data

6.

Match the statement below to the correct description:

The dog is going to bite the cat.

a)

Inference

b)

Observation

7.

Match the statement below to the correct description:

That gorilla has sharp teeth!

a)

Inference

b)

Observation

8.
What is the formula for density?
a)
density = mass x volume
b)
density = mass / volume
c)
density = mass + volume
d)
density = mass - volume
9.
Frank has an eraser. It has a mass of 4g, and a volume of 2cm3. What is its density?
a)
8 g/cm3
b)
2 g/cm3
c)
1/2 g/cm3
d)
24 g/cm3
10.

What is the volume of 150 grams of lead if it has a density of 11.3 g/cm3?

a)

13.3 g

b)

13.3 cm3

c)

.075 g

d)

1695 cm3

11.

7,000 g = ____ kg

a)

70

b)

700

c)

7

d)

0.07

12.

648 g = ____ mg

a)

6,480

b)

64,800

c)

648,000

d)

64.8

13.

240 cm = ___________ m

a)

2400

b)

24

c)

2.4

d)

0.24

14.

68 cm = ___________ mm

a)

0.68

b)

6.8

c)

68

d)

680

15.

How many miles will a person run during a 10.0 kilometer race?

a)

6.2 miles

b)

6.21 miles

c)

1.61 miles

d)

1.6 miles

16.

How many kilograms of calcium are there in 173 pounds of calcium? (1 pound = 454 grams; 1 kg = 1000 g)

a)

1.10 kg

b)

78.5 kg

c)

110 kg

d)

78500 kg

17.

How many gallons are in a pool that holds 758,000 Liters?

(1 gallon = 3.79 Liters)

a)

200

b)

20,000

c)

200,000

d)

2,000,000

18.

How would you write 0.0005 in scientific notation?

a)

50 x 10-5

b)

5 x 10-4

c)

5 x 103

d)

.5 x 103

19.

Convert to scientific notation:


520,000,000

a)

52 x 107

b)

5.2 x 10-7

c)

5.2 x 108

d)

0.52 x 109

20.

Different isotopes of an element contain different numbers of ___.

a)

protons

b)

neutrons

c)

electrons

d)

elements

21.

If a proton is added or removed from an atom, what happens?

a)

It becomes a different element.

b)

It becomes a different isotope.

c)

Nothing happens.

22.

How many neutrons are in 1 atom of Carbon-13?

a)

6

b)

13

c)

7

d)

20

23.

How many protons are in an atom of Nitrogen-16?

a)

7

b)

9

c)

16

24.

What is the difference between Neon-20 and Neon-22?

a)

They have different numbers of electrons.

b)

They have different numbers of neutrons.

c)

Only 1 is radioactive.

d)

No difference.

25.

Which atom of these isotopes has 3 protons? The symbol for lithium is Li.

a)

Lithium-6

b)

Lithium-7

c)

All of them.

d)

Lithium-9

26.
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
27.
If the number of electrons in an atom changes you make a(n) __________________.
a)
ion
b)
isotope
c)
new element
d)
isomer
28.

How many electrons are in an atom with atomic number 34 mass number of 74, and a charge of -2?

a)

34

b)

36

c)

2

d)

40

29.

Which charge is POSITIVE?

a)

Proton

b)

Neutron

c)

Electron

d)

Cell

30.

Which charge is NEGATIVE?

a)

Proton

b)

Neutron

c)

Electron

d)

Cell

31.

Which particle is NEUTRAL - NO CHARGE?

a)

Proton

b)

Neutron

c)

Electron

d)

Cell

32.

How many PROTONS & ELECTRONS does Neon- Ne have?

a)

7

b)

8

c)

9

d)

10

33.

Carbon- C has an atomic MASS / WEIGHT of what?

a)

12.011

b)

6

c)

7

d)

14.007

34.

Which type of particle would you find floating around the nucleus, outside of the atom with its negative charges?

a)

Proton

b)

Neutron

c)

Electron

d)

Nucleus

35.

Which TWO particles are found housed in the nucleus of the atom?

a)

Protons and Electrons

b)

Protons and Neutrons

c)

Electrons and Neutrons

d)

Protons, Neutrons, and Electrons

36.

How many valence electrons does this element have?

a)

12

b)

8

c)

2

d)

10

37.

What is the atomic mass for this element? (Round to the nearest WHOLE number.) (This information for this element can be found on the periodic table!)

a)

11

b)

19

c)

24

d)

23

38.

How many valence electrons does this element have?

a)

1

b)

2

c)

3

d)

4

39.

What element does this Bohr model represent?

a)

Carbon

b)

Boron

c)

Neon

d)

Nitrogen

40.

How many electrons can the first energy level hold?

a)

1

b)

2

c)

8

d)

Unlimited

41.

What element is this the Bohr model of?

a)

Fluorine (F)

b)

Potassium (K)

c)

Aluminum (Al)

d)

Boron (B)

42.
What is the name of this element?
a)
Helium
b)
Hydrogen
c)
Argon
d)
Silver
43.

An atom has a full first and second energy level and 8 electrons in its third level. This atom is neutral. What element is this atom?

a)

Chromium (Cr)

b)

Argon (Ar)

c)

Magnesium (Mg)

d)

Need mor information

44.

Which is the correct molecular structure for carbon dioxide?

a)
b)
c)
d)
45.

What is the correct Lewis Dot Structure for ammonia NH3

a)
b)
c)
d)
46.
Which of the following is the correct Lewis dot structure for the molecule fluorine (F2)?
a)
A
b)
B
c)
C
d)
D
47.

Which Lewis Dot Model drawing correctly shows an O2 molecule?

a)
b)
c)
d)
48.

which two elements have the same number of valence electrons?

a)

C and O

b)

Cl and F

c)

Ga and Ge

d)

Na and Mg

49.

What is the correct lewis dot diagram for Boron?

a)
b)
c)
d)
50.

What type of bonding does this picture show?

a)

Ionic

b)

Covalent

51.

What type of bonding does this picture show?

a)

Ionic

b)

Covalent

52.

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

53.

Valence electrons are shared

a)

Ionic bonds

b)

Covalent bonds

54.

Valence electrons are transferred

a)

Ionic bonds

b)

Covalent bonds

55.
Where are the nonmetals located on the periodic table? 
a)
Blue
b)
Red
c)
Green
56.

The chemical bond between a non-metal and another non-metal will be a ________ bond.

a)

metal

b)

ionic

c)

covalent

d)

polar

57.

The chemical bond between a metal and a non-metal will be a _____ bond.

a)

metal

b)

ionic

c)

covalent

d)

polar

58.

Sodium and Bromine will make a _____ bond.

a)

ionic

b)

covalent

c)

metallic

59.

Carbon and Oxygen will make a ___________ bond.

a)

ionic

b)

covalent

c)

metallic

60.

MgO

a)

ionic

b)

covalent

c)

metallic

61.

If two fluorine atoms bond they will make a _____ bond.

a)

ionic

b)

covalent

c)

metallic

62.

Hydrogen and Chlorine will from a _________ bond

a)

ionic

b)

covalent

c)

metallic

63.

How do you name this base NaOH

a)

Sodium (I) hydroxide

b)

Sodium hydro oxogen

c)

Sodium hydroxide

d)

Sodium monohydroxide

64.

What is the name for MnO2MnO_2  

a)

Manganese oxogen

b)

Manganese oxide

c)

Manganese (I) oxide

d)

Manganese (IV) oxide

65.

Name the covalent compound SO3

a)

Monosulfur Trioxide

b)

Silver Trioxide

c)

Sulfur Trioxide

d)

Sulfur Oxide

66.

What is the formula for the covalent compound Sulfur dioxide?

a)

SiO2

b)

SO2

c)

S2O

d)

S2O2

67.
__Al + __Fe3N2 -->__AlN + __Fe
a)
already balanced
b)
4,2,4,6
c)
2,1,2,3
d)
1,2,1,3
68.
__Na + __Cl2 --> __NaCl
a)
1,1,2
b)
2,1,2
c)
2,1,1
d)
already balanced
69.
How many Hydrogen are in 4H2O?
a)
6
b)
8
c)
2
d)
4
70.
The following is what type of reaction:
PbCl2 + AgNO3 → Pb(NO3)2 + AgCl
a)
Synthesis
b)
Decomposition
c)
Single Replacement
d)
Double Replacement
71.
The following is what type of reaction:
NH3 + HCl  → NH4Cl
a)
Synthesis
b)
Decomposition
c)
Single Replacement Replacement
d)
Double Replacement Replacement
72.
Consider the equation 4 Fe+3 O2 → 2 Fe2O3 . In this equation, 3 O2 is a
a)
product
b)
reactant
c)
compound
73.
Which generalized equation represents a synthesis reaction?
a)
A + BC → AC+ B
b)
A + B → AB
c)
AB → A + B
74.
Which generalized equation represents a decomposition reaction?
a)
A + BC → AC+ B
b)
A + B → AB
c)
AB → A + B
75.
Which generalized equation represents a single displacement reaction?
a)
A + BC → AC+ B
b)
A + B → AB
c)
AB → A + B
76.

How many atoms are present in a 13.5 gram sample of beryllium?

a)

1.5 particles

b)

9 particles

c)

4.03 x1023 particles

d)

9.02 x1023 particles

77.

A sample of silver contains 5.71 x 1022 atoms. How many moles of silver are present?

a)

3.43 x 1046 moles

b)

0.0529 moles

c)

0.0948 moles

d)

10.5 moles

78.

Determine the mass of 2.40 moles of C6H12

a)

201 g

b)

115 g

c)

230. g

d)

353 g

79.

How does heat move?

a)

from a warmer to a cooler object

b)

from a cooler to a warmer object

c)

toward a hot object

d)

away from a cold object

80.

Energy transmitted by electromagnetic waves

a)

conduction

b)

convection

c)

radiation

81.

__________ is the transfer of heat by the movement of a fluid.

a)

Conduction

b)

Convection

c)

Radiation

82.

When you touch hot sand, heat is transferred by _________ to your skin.

a)

conduction

b)

convection

c)

radiation

83.
The specific heat of aluminum is 0.21 cal/g°C.  How much heat(Q) is released when a 10 g piece of aluminum foil is taken out of the oven and cools from 100° to 50°?
a)
105 J
b)
10.5 J
c)
1.05 J
84.
The specific heat(c) of copper is 0.39 J/g °C. What is the temperature change(∆t) when 100 Joules of heat(Q) is added to 20 grams?
a)
12.82 °C
b)
24.12°C
c)
351 °C
85.

A 15.75-g piece of iron absorbs 1086.75 joules of heat energy, and its temperature changes from 25°C to 175°C. Calculate the specific heat capacity of iron.

a)

0.46 J/goC

b)

1.654 J/goC

c)

2,567,446.875 J/goC

86.

The specific heat(c) of copper is 0.38 J/g °C. What is the temperature change(∆t) when 100.0 Joules of heat(Q) is added to 20.0 grams?

a)

6.5 °C

b)

133°C

c)

13.16 °C

87.
In an exothermic reaction, heat is ...
a)
taken in
b)
given out
88.

In an endothermic reaction, heat is ...

a)

taken in

b)

given out

89.
Baking bread and cooking an egg are examples of....?
a)
Endothermic processes
b)
Exothermic processess
c)
None of these 
90.
What type of reaction is shown in the photo?
a)
Exothermic
b)
Isothermic
c)
Endothermic
d)
None of the  above
91.

What type of reaction occurs in a hand warmer?

a)

exothermic

b)

endothermic

92.

Two objects with different temperature in thermal contact will reach thermal equilibrium when.....

a)

both object becomes hotter

b)

both objects become colder

c)

both object reach the same final temperature

d)

net heat transfer other than zero

93.
Increase in temperature of the reactants can do one of the following
a)
Slow collision frequency
b)
Allow less effective collision between the particles
c)
Neutralise the reaction
d)
increase collision between the particles thus increasing the rate.
94.

Increasing pressure causes the reacting particles

a)

to bond together

b)

to repel from each other

c)

gain more kinetic energy

d)

to move closer together

95.

2SO2(g)+O2(g) ⇌ 2SO3(g) + Heat


Adding SO2(g) will

a)

shift equilibrium right

b)

shift equilibrium left

c)

increase rate of reaction

d)

have no change

96.

2SO2(g)+O2(g) ⇌ 2SO3(g) + Heat


Increasing the temperature will...

a)

shift equilibrium right

b)

shift equilibrium left

c)

increase pressure

d)

have no change

97.

2SO2(g) + O2(g) ⇌ 2SO3(g) + Heat


Removing O2(g) will

a)

shift equilibrium right

b)

shift equilibrium left

c)

increase pressure

d)

have no change

98.

2SO2(g)+1O2(g) ⇌ 2SO3(g) + Heat


Increasing the volume of the container will...

a)

shift equilibrium right

b)

shift equilibrium left

c)

slow rate of reaction

d)

have no change

99.

2SO2(g)+1O2(g) ⇌ 2SO3(g) + Heat


Increasing the pressure on the system will...

a)

shift equilibrium right

b)

shift equilibrium left

c)

slow rate of reaction

d)

have no change

100.

What is the ion formed from Sulfur? If it has 6 valence electrons.

a)

S+2

b)

S-2

c)

S+6

d)

S-6

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