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Chemistry Final Practice (fall 2024)

Total questions: 107

Worksheet time: 2hrs 36mins

Name
Class
Date
1.

A pure substance made of only one type of atom (e.g., O₂)

a)

Heterogeneous Compound

b)
Mixture
c)
Element
d)

Homogeneous Mixture

2.

  • Two or more atoms chemically bonded (e.g., H₂O).

a)

Mixture

b)

Element

c)

Compound

d)

Homogeneous Mixture

3.

  • Uniform composition (e.g., saltwater)

a)

Heterogeneous Mixture

b)

Element

c)

Homogeneous Mixture

d)

Compond

4.

  • Non-uniform composition (e.g., sand and water)

a)

Heterogeneous Mixture

b)

Element

c)

Homogeneous Mixture

d)

Compond

5.
a)
heterogeneous mixture
b)
homogeneous mixture
6.

  • Definite shape and volume, particles vibrate but don’t move.

a)

Solid

b)

Liquid

c)

Gas

7.

  • Definite volume, but indefinite shape, particles can move past each other.

a)

Solid

b)

Liquid

c)

Gas

8.

  • Indefinite shape and volume, particles move freely

a)

Solid

b)

Liquid

c)

Gas

9.

Change in appearance (e.g., freezing, dissolving).

a)

Chemical Change

b)

Physical Change

10.

  •  New substance is formed (e.g., combustion, rusting).

a)

Chemical Change

b)

Physical Change

11.

Which is an example of separating a mixture?

a)
evaporation
b)

chromatography

c)
sublimation
d)
condensation
12.

Independent of amount (e.g., density, boiling point) is known as the ----- property.

(a)  

13.

The Dependent on the amount (e.g., mass, volume) is known as a ----- property.

(a)  

14.

Which image shows Distillation?

a)

b)

c)

.

15.

Define Filtration:

4 lines
16.

What is Chromatography?

a)
A method for measuring temperature changes in liquids.
b)
A process for mixing different gases together.
c)
A technique for analyzing the color of substances.
d)

The separation of mixtures based on their movement through a medium

17.

What is the order of units? (smallest to largest)

a)
inch, foot, yard, mile, light year
b)
millimeter, centimeter, decimeter, meter, kilometer
c)
centimeter, meter, hectare, kilometer, mile
d)
millimeter, centimeter, meter, kilometer, mile
18.

What is the name of the conversion of different units in our curriculum?

a)
Unit measurement
b)
Unit analysis
c)

Dimensional Analysis

d)
Unit conversion
19.
You know 1000 mg = 1 g.  Convert 2.5 grams into milligrams.
a)
25 mg
b)
25,000 mg
c)
250 mg
d)
2500 mg
20.

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

21.

What are the rules for significant figures?

a)

Non-zero digits are always significant.

b)

Zeros between non-zero digits are significant.

c)

Leading zeros are not significant.

d)

Trailing zeros are significant in decimals.

e)

All of the above

22.
How many significant figures in 10,097?
a)
3
b)
5
c)
2
d)
0
23.

What is the equation for Percent Error?

a)

Percent Error = |(Experimental Value - True Value)| /

|True Value| * 100

b)

Percent Error = (Experiment Value + True Value) /

(True Value) * 100

c)

Percent Error = |(True Value - Experimental Value)| /

|Experimental Value| * 100

d)

Percent Error = (Experimental Value - True Value) / (Experimental Value) * 100

24.

Density

a)
Density = Mass + Volume
b)
Density = Volume / Mass
c)
Density = Mass x Volume
d)
Density = Mass / Volume
25.

  • How close a measurement is to the true value



(a)  

26.

  • How consistent repeated measurements are



(a)  

27.

What are the forms of energy?

a)
Magnetic, gravitational, sound
b)
Static, mechanical, elastic
c)
Kinetic, potential, thermal, chemical, electrical, nuclear, radiant.
d)
Hydraulic, pneumatic, thermal energy
28.
What is the boiling point for this substance?
a)
60 °C
b)
40 °C
c)
120 °C
d)
100 °C
29.
Describe the substance between letters A and B. 
a)
Solid
b)
Liquid
c)
Melting
d)
Evaporating
30.

Heat needed to change the temperature

a)
Q = mΔT
b)

Q = mHv

c)

q = mHf

d)
Q = mcΔT
31.

  • Heat for fusion (melting)

a)
Q = mΔT
b)

Q = mHv

c)

q = mHf

d)
Q = mcΔT
32.

  • Heat for vaporization (boiling)

a)
Q = mΔT
b)

Q = mHv

c)

q = mHf

d)
Q = mcΔT
33.

According to the reference table, what is the boiling point of ethanoic acid at 80 kPa?

a)

28 oC

b)

100oC

c)

111oC

d)

125oC

34.

At which temperature is the vapor pressure of ethanol equal to the vapor pressure of propanone at 35oC?

a)

35oC

b)

60oC

c)

82oC

d)

95oC

35.
How do you convert Celsius to Kelvin?
a)
Add 273
b)
Subtract 273
c)
You can't convert those
d)
They are the same thing
36.
How do gas molecules move?
a)
In an orderly fashion
b)
Constantly and randomly
c)
In straight-line paths
d)
In a circular motion
37.
A gas is heated from 263K to 298K. The volume is increased from 24.0L to 35.0L. If the original pressure was 1.00 atm, what is the new pressure?
a)
0.78 atm
b)
1.65 atm
c)
1.28 atm
d)
0.61 atm
38.
When Pressure increases then the Volume must...
a)
Increase
b)
decrease
39.
What is the formula for Boyle's Law?
a)
P1V1=P2V2
b)
P1V1/P2V2
c)
P1V2=P2V1
d)
P1/V1=P2/V2
40.
Which container will have a lower pressure?
a)
left
b)
right
c)
they both have the same pressure
d)
I don't know
41.

Charle's Law states that the ______________of a gas is directly proportional to its ______________.

a)

pressure and temperature

b)

volume and pressure

c)

volume and temperature

d)

temperature, volume, and pressure

42.

What is the formula for Charle's Law?

a)

P1V1/ P2V2

b)

P1V2 = P2 V1

c)

P1/V1=P2/V2

d)

P1V1=P2V2

43.

Which one of these is NOT an Ideal Gas Assumption?

a)

Gas particles are hard, round spheres.

b)

Gas particles are strongly attracted to one another.

c)

Gas particles do not take up space.

d)

Gas particles collide perfectly elastically.

44.

A hypothetical gas that perfectly fits all the assumptions of the kinetic molecular theory is known as

a)

real gas

b)

ideal gas

c)

imaginary gas

d)

perfect gas

45.

Why does ice float on liquid water?

a)

Ice does not float on liquid water.

b)

It has a higher density than liquid water.

c)

It floats because it has lower density than liquid water.

d)

adhesion and cohesion

46.

Collisions in which particles transfer all their kinetic energy to other particles are called ___.

a)

elastic

b)

inelastic

47.

Fill in the blank: Postulate #2 of the KMT states that the particles of a gas are in constant rapid ________.

a)

degeneration

b)

deceleration

c)

acceleration

d)

motion

48.

Fill in the blank: Postulate #1 of the KMT states that gases consist of large numbers of tiny particles that are _________ in comparison to their size.

a)

far apart

b)

close together

c)

heavy

d)

light

49.

Which gas is least likely to obey the ideal gas laws at very high pressures and very low temperatures?

a)

He

b)

Ne

c)

Kr

d)

Xe

50.

Which of the following is NOT a factor in the ideal gas law?

a)

pressure

b)

temperature in Kelvins

c)

amount of a substance in moles

d)

type of container

51.

What does the variable "n" represent in the ideal gas law?

a)

pressure

b)

volume

c)

moles

d)

temperature

52.

Choose the correct set of variables to solve the following problem: What is the volume of a balloon if it contains 3.2 moles of helium at a temperature of 20⁰C and 1.2 atm?

a)

P = x (unknown), V = 3.2 mol, n = 1.2 atm, T = 20⁰C K

b)

P = 1.2 atm, V = 3.2 mol, n = 20⁰C, T = x (unknown)

c)

P = 293 K, V = 3.2 mol, n = x (unknown), T = 1.2 atm

d)

P = 1.2 atm, V = x (unknown), n = 3.2 mol, T = 293 K

53.

What is the difference between Real and Ideal Gases?

4 lines
54.

Draw an atom.

Include the 3 types of particles.

55.

Chadwick found the nucleus through the gold foil experiment.

a)

True

b)

False

56.

Aristotle and other early Greek philosophers thought that matter was composed of four elements: air, earth, fire, and water.

a)

True

b)

False

57.

Which scientist developed the model of the atom shown?

a)

Chadwick

b)

Thomson

c)

Rutherford

d)

Bohr

58.

Which scientist developed the model of the atom shown?

a)

Chadwick

b)

Thomson

c)

Rutherford

d)

Bohr

59.

What were the main flaws in Dalton’s atomic theory? (choose all that apply)

a)

All elements are composed of tiny indivisible particles called atoms that cannot be broken down further.

b)

Atoms of different elements differ in their physical and chemical properties.

c)

All atoms of a given element are identical.

d)

In chemical reactions, atoms are combined, separated or rearranged, but not created nor destroyed.

e)

Atoms of different elements combine in simple, whole number ratios to form compounds.

60.

How many protons does krypton have?

a)

84

b)

36

c)

48

d)

8

61.

How many electrons are in Nitrogen? Use the picture to the left.

(a)  

62.

Who proposed that electrons move around the nucleus in circular orbits?

a)

Dalton

b)

Thomson

c)

Rutherford

d)

Bohr

63.

Which of the following has the atomic models in the correct Chronological order?

a)

Solid sphere, Plum pudding, Nuclear, Planetary, Quantum Mechanic/Electron Cloud

b)

Solid sphere, Plum pudding, Nuclear, Quantum Mechanic/Electron Cloud, Planetary,

c)

Plum pudding, Nuclear, Planetary, Quantum Mechanic/Electron Cloud,Solid sphere

d)

Nuclear, Planetary, Solid sphere, Quantum Mechanic/Electron Cloud,Plum pudding,

64.
This model was developed after J.J. Thompson discovered electrons, a particle smaller than an atom. Is shows electrons floating freely in a positive space.
a)
The "Plum Pudding Model" of the atom
b)
The "Rutherford Model" of the atom
c)
Democritus's model of the atom
d)
The "Quantum Mechanical Model" of the atom
65.
This model this model was the first to show a nucleus, consisting of protons and neutron.  Electrons surround the nucleus but are not shown in distinct energy levels. 
a)

The "Nuclear Model" by Rutherford

b)

The "Plum Pudding Model" of the atom by Thomson

c)

The "Quantum Mechanical Modell" of the atom by Heisenberg

d)
Democritus's model of the atom
66.

This model added on to previous models by showing electrons existed at certain "energy levels". It is often called the Planetary Model.

a)
The "Bohr Model" of the atom
b)
The "Rutherford Model" of the atom
c)
The "Plumb Pudding Model" of the atom
d)
The "Quantum Mechanical Model" of the atom
67.

In an atom, there are three types of subatomic particles. ______ are positively charged, ______ are negatively charged, and ______ are neutral.

a)

Protons, Electrons, Neutrons

b)

Electrons, Protons, Neutrons

c)

Neutrons, Protons, Electrons

d)

Electrons, Neutrons, Protons

68.

_______ is the average mass of all the isotopes of an element.

a)

Atomic Mass

b)

Atomic Number

c)

Chemical Symbol

d)

Element Name

69.

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

70.

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

71.
How many neutrons does the isotope of lithium have?
a)
8
b)
3
c)
4
d)
5
72.
What do these isotopes of carbon all have in common?
a)
neutrons & mass number
b)
atomic number and neutrons
c)
atomic number and electrons
d)
protons, atomic number, and mass number
73.
which atom has  4 neutrons?
a)
Li-6
b)
Li-7
c)
Li-8
d)
they have the same # of neutrons
74.

What is the chemical symbol for iron?

a)

I

b)

Ir

c)

Fe

d)

R

75.

What is iron's atomic number?

a)

12

b)

26

c)

55.85

d)

55

76.

What family is copper in?

a)

alkali metals

b)

alkaline earth metals

c)

noble gases

d)

transition metals

77.

What is silver's chemical symbol?

a)

S

b)

Ag

c)

Si

d)

I

78.

Group 1: These metals are extremely reactive. They all have one valence electron. They are shiny and silver in color. They are soft and can be cut with a knife.

a)

Transition Metals

b)

Alkali Metals

c)

Alkaline Metals

d)

Lanthanides

79.

Group 2: Slightly less reactive because they have 2 valence electrons. They are silver colored and more dense that Group 1 metals.

a)

Transition Metals

b)

Alkali Metals

c)

Alkaline-earth Metals

d)

Actinides

80.

Groups 3-12: These metals have a moderate range of reactivity and a wide range of properties. They are shiny and good conductors of heat and electricity. They have higher densities and melting points than Groups 1 and 2. These have 1 or 2 valence electrons.

a)

Transition Metals

b)

Alkali Metals

c)

Alkaline-earth Metals

d)

Lanthanides

81.

Elements with atomic numbers 57-70 and 89-102: These metals were taken out and placed at the bottom of the table so the table wouldn't be so wide. Some are shiny and reactive. Others are radioactive and unstable. Elements 95-103 do not exist in nature but have been manufactured in the lab.

a)

Alkali Metals

b)

Alkaline-earth Metals

c)

Lanthanides and Actinides

d)

Boron Group

82.

Group 17: All nonmetals. Very reactive. Poor conductors of heat and electricity. Tend to form salts with metals. Example NaCl: sodium chloride which is known as table salt. These elemtns have 7 valence electrons (Group # minus 10).

a)

Boron Group

b)

Oxygen Group

c)

Nitrogen Group

d)

Halogens

83.

Group 18: Unreactive nonmetals. All are colorless, odorless gases at room temperature. These elements have a full outer energy level, usually 8 valence electrons, except for Helium which only has 2 valence electrons.

a)

Nitrogen Group

b)

Oxygen Group

c)

Noble Gases

d)

Halogens

84.

The elements on the right side of the Periodic Table are classified as ________________.

a)

Metals

b)

Nonmetals

85.
The atom with the largest atomic radius in Group 18 is - 
a)
Ar
b)
He
c)
Kr
d)
Rn
86.
As you move down a group, atomic radius increases because - 
a)
you add more and more neutrons
b)
you add more and more protons
c)
you add more and more shells (energy levels)
d)
you add more atomic mass
87.

Which of the following halogens has the greatest electronegativity?

a)

Chlorine (Cl)

b)

Bromine (Br)

c)

Iodine (I)

d)

Astatine (At)

88.

What is a vertical (up and down) column in the periodic table?

a)

group or family

b)

period

c)

periodic law

d)

octet rule

89.
Which atom has the largest atomic radius?
a)
potassium
b)
rubidium 
c)
francium
d)
cesium
90.
Electronegativity is...
a)
the ability of an atom to attract/ accept 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. 
91.
Electronegativity __________ from left to right within a period and __________ from top to bottom within a group.
a)
decreases, increases 
b)
increases, increases
c)
increases, decreases 
d)
stays the same, increases
92.
Atomic Radius is...
a)
the relative size of the atom's nucleus
b)
the relative size of the atom's electron cloud
c)
the energy required to shield the outer electrons from the nucleus
d)
a measure of the ability of an atom to attract electrons
93.
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.
94.
Atoms that have a high electronegativity, _______________.
a)
give up their electrons more easily.
b)
hold on to their electrons more tightly.
c)
have more electron shells.
95.

This could be the dot diagram of

a)

Mg

b)

Cl

c)

C

d)

O

96.

What is the goal of the Lewis Dot Structure?

a)

To determine the electron position.

b)

To show the element's valence electrons & bonding capabilities.

c)

To find the atomic mass of an element.

d)

To search for the number of electrons in an individual atom.

97.

How many valence electrons should Lithium have in its Lewis dot model?

a)

1

b)

2

c)

3

d)

4

98.

Which of these is correct?

a)
b)
c)
99.
What's a valence electron?
a)
electrons in the second energy level
b)
electrons in the outermost energy level
c)
the atomic number
d)
electrons in the first level
100.

How would you draw a Lewis dot diagram for Magnesium?

a)
b)
c)
d)
101.

Which of the following shows a correct Lewis dot structure?

a)
b)
c)
d)
102.

Where are metals located on the periodic table?

a)

right side of the staircase

b)

on the staircase

c)

left side of the staircase

103.

Which of these is incorrect?

a)
b)
104.

Which of these is the correct Lewis Dot diagram for the element Neon (Ne)?

a)
b)
c)
d)
105.

Which of the following is the a correct Lewis dot diagram for nitrogen (N)?

a)
b)
c)
d)
106.
How many electrons does potassium K contain? 
a)
19
b)
39
c)
20
d)
40
107.

Draw the Lewis Dot Diagram for Nickel (Ni).

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