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Semester 1 Final Exam

Total questions: 100

Worksheet time: 3hrs 43mins

Name
Class
Date
1.
What SI unit is used to measure length?
a)
meters
b)
liters
c)
candelas
d)
kilograms
2.
What SI unit is used to measure volume?
a)
meters
b)
liters
c)
candelas
d)
kilograms
3.
What SI unit is used to measure mass?
a)
meters
b)
liters
c)
candelas
d)
kilograms
4.
What SI unit is used to measure time?
a)
seconds
b)
amperes
c)
Kelvin
d)
mole
5.
What SI unit is used to measure temperature?
a)
seconds
b)
amperes
c)
Kelvin
d)
mole
6.
What SI unit is used to measure the amount of a substance?
a)
seconds
b)
amperes
c)
Kelvin
d)
mole
7.
Convert the following SI Units:  3.2 km to meters
a)
32
b)
320
c)
3200
d)
32000
8.
Convert the following SI Units: 5 cm to meters
a)
5
b)
0.5
c)
0.05
d)
0.005
9.
What is the metric prefix for kilo?
a)
h
b)
he
c)
k
d)
m
10.
28 °C = __?__ K
a)
301
b)
245
c)
401
d)
345
11.
-123 °C = __?__ K
a)
150
b)
396
c)
496
d)
250
12.
The measure of matter in an object.
a)
mass
b)
length
c)
weight
d)
ton
13.
A graduated cylinder is used to measure the __________ of a liquid.
a)
temperature
b)
mass
c)
volume
d)
length
14.

Which of the following would be considered a physical change?

a)

Cutting paper

b)

pH test

c)

Burning marshmellow

d)

Roasting a Turkey

15.

Which of the following would be considered a physical property?

a)

Colour

b)

Flammability

c)

pH

d)

Reactivity

16.
Which of the following is represented by point 3 on the graph above. 
a)
Gas heating
b)
Sublimation
c)
Liquid Heating
d)
Evaporation
17.
Which of the following is a Physical Property 
a)
Toxicity
b)
Flammability
c)
Malleability
d)
Reactivity
18.
Which of the following would be considered a homogeneous mixture
a)
Sweet Tea
b)
Vegetable soup
c)
24 Karat Gold
d)
Distilled water
19.
A block of metal has a mass of 14.0 Kg and a volume of 2.0 Liters what is the density?
a)
14.0 kg/L 
b)
7.0 Kg/L
c)
2.0 Kg/L 
d)
0.5 Kg/l
20.
Phase change from a solid to a gas.
a)
sublimation
b)
deposition
c)
condensation
d)
evaporation
21.
When the temperature of matter decreases the particles ...
a)
speed up and move farther apart
b)
speed up and move closer together
c)
slow down and move farther apart
d)
slow down and move closer together
22.
A gas
a)
has a definite shape but no definite volume
b)
has a definite volume but no definite shape
c)
has fast-moving particles
23.
Which is a quality that only gasses display
a)
Spread out to fill all available space
b)
Take the shape of their container
c)
Can't be compressed
d)
All of these
24.
Which of the following has the lowest density?
a)
Gasses
b)
Solids
c)
Liquids
d)
All mater is the same density
25.
If you increase the pressure of a constant volume of gas, what will happen to the temperature?
a)
Increase
b)
Decrease
c)
Stay the same
d)
It will Blow Up
26.
What will happen to the volume of a gas under constant temperature if the pressure increases?
a)
Increase
b)
Decrease
c)
Nothing
d)
Explosion!
27.
How are pressure and volume related?
a)
Directly
b)
Indirectly
c)
They aren't related
28.
Which of the following would increase the pressure on a system?
a)
Increase the Temperature
b)
Pump in more gas
c)
Decrease the volume
d)
All of these
29.
The molecules of a gas are in constant and random motion.
a)
TRUE
b)
FALSE
c)
DEPENDS UPON THE KIND OF MOLECULE
30.
What happen to the energy of the system when the molecules collide with each other?
a)
Energy increases
b)
Energy decreases
c)
Energy remains the same
31.
What will happen to the volume of the gas when the temperature is increased? 
a)
volume decreases
b)
volume increases
32.
What will happen to the size of the balloon when it is placed inside the refrigerator? 
a)
Its size decreases.
b)
Its size increases.
33.
Gas molecules can easily be compressed  because ___________. 
a)
gas molecules are soft
b)
gas molecules are far apart
c)
gas molecules follow the shape of the container
34.
Among the following gases, which one is the heaviest?
a)
hydrogen gas
b)
nitrogen gas
c)
oxygen gas
d)
chlorine gas
35.
Entropy increases from solid, liquid to gas. Why?
a)
Molecular disorder increases
b)
Molecular randomness decreases
c)
Molecules are more energetic
d)
Molecules are more reactive
36.

Which represents a decrease in entropy?

a)

sublimation of CO2

b)

boiling water

c)

condensation of steam on cold glass

d)

NaCl dissolving in water

37.

The entropy will usually increase when

a)

a molecule is broken into two or more smaller molecules

b)

a reaction occurs that results in an increase in the number of moles of gas

c)

a solid changes to a liquid

d)

all of these

38.
The amount of energy required to raise the temperature 1ºC for every kilogram is called____?
a)
Thermal Energy
b)
Specific Heat
c)
Temperature
d)
Kinetic Energy
39.
What unit do you use to measure Thermal Energy?
a)
J/Kg ºC
b)
Kg
c)
ºC
d)
J
40.
What is the equation to measure change in Thermal Energy?
a)
Q=mc∆t
b)
Q=mc
c)
Q= ∆mct
d)
m=QC
41.
Water has a specific heat of 4184 J/KgºC.  Wood has a specific heat of 1760 J/KgºC.  What material needs more energy to raise the temperature 1ºC
a)
Wood
b)
Water
c)
Both are the same
42.
Copper, Stainless Steel, Carbon Steel, and Zinc were all heated using the same thermal energy.  What material would be the coolest after being heated?
a)
Copper
b)
Carbon Steel
c)
Zinc
d)
Stainless Steel
43.
What does temperature measure?
a)
Heat
b)
ºC
c)
Kinetic Energy
d)
Thermal Energy
44.
How does heat flow?
a)
Always from cold to warm
b)
Always from warm to cold
c)
Both warm to cold & cold to warm
d)
It depends on the temperature
45.
Which particle contributes the negative charge to the atom?
a)
proton
b)
electron
c)
neutron
d)
nucleus
46.
Which particle does not contribute mass to the atom?
a)
Proton
b)
Neutron
c)
Electron
d)
Nucleus
47.
The three main subatomic particles are electrons, protons and ____________.
a)
photons
b)
neurons
c)
neutrons
d)
quarks
48.
What are the two main parts of the atom?
a)
nucleus and cytoplasm
b)
nucleus and electron cloud
c)
core and electron cloud
d)
protons and neutrons
49.
Most of the mass in an atom is made up of _____________________?
a)
protons and electrons
b)
protons and neutrons
c)
neutrons and electrons
d)
electrons and quarks
50.
What is the electrical charge of a proton?
a)
1+
b)
1-
c)
neutral
d)
2-
51.
Water is an element
a)
true
b)
false
52.
DIFFERENT kinds of atoms chemically combined to form a substance are
a)
Mixture
b)
Element
c)
Compound
d)
Substance
53.
Salt water is a mixture.
a)
True
b)
False
54.
A mixture that does not look the same throughout:
a)
heterogeneous mixture
b)
homogeneous mixture
c)
the periodic table
d)
water
55.
How many valence electrons are represented here?
a)
7
b)
5
c)
2
d)
8
56.
How many electrons can the first energy level hold?
a)
1
b)
2
c)
8
d)
0
57.
How many valence electrons does phosphorus have?
a)
5
b)
2
c)
8
d)
15
58.
Identify the element in Period 5 that has 1 valence electron?
a)
Rb
b)
Nb
c)
Ag
d)
Sb
59.
What element in Period 4 has 5 valence electrons?
a)
Zr
b)
As
c)
V
d)
Sb
60.
Ionization energy is...
a)
the energy required to add an electron to a specific atom
b)
how much energy it takes to remove an electron from an atom
c)
the energy required to shield the outer electrons from the nucleus
d)
a measure of the ability of an atom to attract electrons
61.
Atomic radius generally increases as we move __________.  
a)
down a group and from right to left across a period 
b)
up a group and from left to right across a period 
c)
down a group and from left to right across a period 
d)
up a group and from right to left across a period 
62.
Which atom has the largest atomic radius?
a)
potassium
b)
rubidium 
c)
francium
d)
cesium
63.

As you move from left to right on the periodic table, the number of valence electrons.......

a)

Increases

b)

Decreases

c)

Remains the same

64.

As you move down a group on the periodic table, the number of valence electrons....

a)

Increases

b)

Decreases

c)

Remains the same

65.

Which of the following would be most similar to Phosphorus? (select all that apply)

a)

Nitrogen

b)

Sulfur

c)

Silicon

d)

Germanium

e)

Antimony

66.

Which of the following reasons explains why there is a decimal for most atomic masses?

a)

The mass of one atom can have a fraction.

b)

Since electrons are very small mass they only add a little bit, usually only a decimals worth.

c)

It is the average mass of all the potential isotopes of an atom.

d)

Neutrons have a mass of 1.1 meaning that fractions are common.

67.
Which of the following will have a higher electronegativity than arsenic (As)?
a)
Carbon (C)
b)
Neon (Ne)
c)
Antimony (Sb)
d)
Germanium (Ge)
68.
Which of the following will have a lower ionization energy than Scandium (Sc)?
a)
Helium (He)
b)
Titanium (Ti)
c)
Calcium (Ca)
d)
Magnesium (Mg)
69.
As you move across the periodic table atoms tend to get smaller because, ______________.
a)
the atoms have more mass.
b)
the atoms have less mass
c)
the atoms have more protons.
d)
the atoms have less electrons.
70.
The atom with the largest atomic radius in Group 18 is - 
a)
Ar
b)
He
c)
Kr
d)
Rn
71.
Which statement correctly and completely identifies a trend?
a)
Atomic radius decreases across a period and increases down a group.
b)
Electronegativity decreases across a period and decreases down a group.
c)
Ionization energy increases across a period and increases down a group.
d)
Ionic radius increases across a period and increases down a group.
72.
What is the number of valence electrons for Oxygen?
a)
8
b)
6
c)
2
d)
1
73.
What is the number of valence electrons for Beryillum?
a)
1
b)
4
c)
2
d)
7
74.
What type of diagram is this?
a)
Electron Dot Diagram
b)
Bohr Model
c)
Alkali Diagram
d)
Chemical Diagram
75.
How many valence electrons in this structure?
a)
6
b)
5
c)
4
d)
7
76.
What is a diatomic element?
a)
a metal bonded with a nonmetal
b)
2 or more nonmetals bonded together
c)
2 or more metals bonded together
d)
2 atoms of the same element bonded together
77.
The number of bonds an element will form in a covalent compound will be equal to
a)
the number of valence electrons
b)
eight electrons
c)
the number of electrons needed to reach an octet
d)
the group number
78.
Which element below is not diatomic?
a)
hydrogen
b)
oxygen
c)
nitrogen
d)
sulfur
79.

Why does the melting point of metals increase across period 3, from Sodium (Na) to Aluminium (AI)?

a)

Size of atoms gets smaller

b)

Attraction force between nuclei and free electron increases

c)

Increased space between the valence electrons in the "sea"

d)

Increased number of valence electrons contributed to the "sea"

80.

Why do metals conduct electricity?

a)

They are shiny

b)

The electrons are delocalised and able to move

c)

The electrons are held tightly within the lattice

d)

The electrons are shared between two metal ions

81.
A mixture of two or more metals is called:
a)
mixture
b)
solution
c)
compound
d)
alloy
82.

Water has an unusually high boiling point for a molecular compound because it has

a)

hydrogen bonding

b)

ion-ion attractions

c)

a high density

d)

a large gram formula mass

83.
The substances listed on the right side of a chemical equation are the
a)
Yields
b)
Reactants
c)
Products
d)
Precipitates
84.
CaCO3 represents a chemical
a)
Symbol
b)
Formula
c)
Subscript
d)
Reaction
85.
The substances listed on the left side of a chemical equation are the
a)
Products
b)
Coefficients
c)
Precipitates
d)
Reactants
86.

What physical state symbol should be included for water?

a)

(s) - solid

b)

(l) - liquid

c)

(g) - gas

d)

(aq) - aqueous

87.

Why does oxygen's symbol have a subscript "2"?

a)

Because it is monoatomic.

b)

Because it is diatomic.

c)

Because it is triatomic.

88.

If two objects have different temperatures, heat will flow from the warmer object to the cooler one UNTIL ____________

a)

one reaches a temperature of zero

b)

they both have an equal temperature

c)

one runs out of energy

89.
What would be the effect on the particles if more heat is supplied to the system?
a)
They would slow down
b)
They would stop moving
c)
They would speed up
d)
There would be no effect
90.
Which direction will the heat flow while this person holds a hot cup of tea?
a)
from the cup to her hand
b)
from her hand to the cup
c)
no heat is transferred
91.
A metal cube at temperature of 10°C immersed in a liquid at temperature of 70°C.
What is the temperature of the metal cube when thermal equilibrium is achieved between the cube and the liquid?
a)
Between 10°C and 70°C
b)
More than 70°C
c)
Less than 10°C
d)
Same as the room temperature
92.

What is the direction of thermal energy flow (in general)?

a)

High to low.

b)

Low to high.

93.

100 g of ice cold water (0 C) is mixed with 50 g of boiling water (100 C). What best describes the outcome of this process?

a)

The final temperature will be 50 C because this is the average temperature.

b)

The final temperature will be less than 50 C because the 100g sample has more mass.

c)

The final temperature will be greater than 50 C because the 100 C water has a higher temperature.

d)

The final temperature can not be determined with the given information.

94.

When a substance increases in temperature, what describes the motion of the particles?

a)

They move more rapidly.

b)

They expand in size.

c)

They change their phase.

d)

They decrease their entropy.

95.

How can temperature be described?

a)

Heat flow from a substance.

b)

How fast (on average) the particles are moving.

c)

The average size of the particles.

d)

The arrangement of the particles.

96.

The units of heat capacity are ________.

a)

 KJ\frac{K}{J}  or  °CJ\frac{\degree C}{J}  

b)

 JK\frac{J}{K}  or  J°C\frac{J}{\degree C}  

c)

 Jg−K\frac{J}{g-K}  or  Jg−°C\frac{J}{g-\degree C}  

d)

 Jmol\frac{J}{mol}  

e)

 g−KJ\frac{g-K}{J}   or  g−°CJ\frac{g-\degree C}{J}  

97.

The units of specific heat (specific heat capacity) are ______.

a)

KJ\frac{K}{J} or °CJ\frac{\degree C}{J}

b)

JK\frac{J}{K} or J°C\frac{J}{\degree C}

c)

Jg−K\frac{J}{g-K} or Jg−°C\frac{J}{g-\degree C}

d)

Jmol\frac{J}{mol}

e)

g−KJ\frac{g-K}{J} or g−°CJ\frac{g-\degree C}{J}

98.

The specific heat of liquid bromine is 0.226  Jg−K\frac{J}{g-K}  . How much heat (in Joules) is required to raise the temperature of 10.0 ml of bromine from 25.00 °C\degree C   to 27.30 °C\degree C ? The density of liquid bromine is 3.12  gml\frac{g}{ml}  .

a)

5.20

b)

16.2

c)

300

d)

32.4

e)

10.4

99.

A sample of aluminum metal absorbs 11.2 J of heat, upon which the temperature of the sample increases from 23.2  °C\degree C  to 30.5  °C\degree C . Since the specific heat capacity of aluminum 0.90  Jg−K\frac{J}{g-K}  , the mass of the sample is _______ grams.

a)

72

b)

1.7

c)

10

d)

65

e)

7.3

100.

What is the final temperature of a 35.1 g sample of iron, having an initial temperature of 24.5  °C\degree C , when it absorbs 115 J of heat? The specific heat capacity of iron is 0.450  Jg−K\frac{J}{g-K} .

a)

26.3

b)

27.9

c)

38.6

d)

31.8

e)

34.9

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