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Chemistry Midterm Review

Total questions: 155

Worksheet time: 3hrs 45mins

Name
Class
Date
1.
A mixture that is NOT evenly distributed is called ....
a)
Compounded
b)
Homogenous
c)
Heterogenous
d)
Salty
2.
Are made from a combination of 2 or more elements in a constant ratio...
a)
Atome
b)
Mixture
c)
Compounds
d)
Elements
3.
What is the formula for density?
a)
density = mass x volume
b)
density = mass / volume
c)
density = mass + volume
d)
density = mass - volume
4.
What units can be used to express density?
a)
g/mL
b)
grams
c)
millimeters
d)
milliliters
5.
A bar of copper has a mass of 216g and a volume of 24cm3. What is the density of copper?  
a)
9g/cm3
b)
.11g/cm3
c)
5184g/cm3
d)
322mL
6.
What kind of properties can only be observed when a substance changes into a different substance?
a)
physical properties
b)
chemical properties
7.
Properties that can be observed without changing the identity of the substance.
a)
Physical
b)
Chemical
8.
Example for chemical property
a)
color
b)
hardness
c)
toxicity
d)
solubility
9.
Example for physical property
a)
melting point
b)
flammability
c)
reactivity 
d)
combustion
10.

Rutherford discovered what subatomic particle through his experimentation?

a)

The proton

b)

The neutron

c)

The electron

d)

The quark

11.

In his experiment, Rutherford concluded that atoms have a nucleus because

a)

most of the particles went straight through the foil.

b)

some of the particles were deflected near the front of the screen.

c)

some of the particles were deflected back towards the alpha source.

d)

not enough information is given.

12.
Isotopes of the same element have different ____________. 
a)
 numbers of protons  
b)
numbers of electrons
c)
 symbols 
d)
numbers of neutrons
13.
The atomic number of an atom or ion refers to the number of:
a)
neutrons
b)
protons
c)
nucleons
d)
electrons
14.
How many electrons does potassium K contain? (click to see image)
a)
19
b)
39
c)
20
d)
40
15.
How many neutrons does the isotope of lithium have?
a)
8
b)
3
c)
4
d)
5
16.

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

17.
Which particles are found in the nucleus
a)
electrons and protons
b)
neutrons and protons
c)
neutrons and electrons
d)
footballs and soccer balls
18.

Which statement is INCORRECT use of mole measurement?

a)

one mole of calcium is 40.01 grams.

b)

one mole of calcium is equals to 6.02 x 1023 atoms

c)

two moles of CaCl2 is equal to 6.02 x 1023 molecules

d)

two moles of KI is equals to 166g

19.

When compared, a mole of oxygen and a mole of sulfur, how many atoms each has?

a)

oxygen has 16 grams of atoms

b)

sulfur has 32.06 grams of atoms

c)

both contains 6.02 x 1023 atoms

d)

A

20.
What is the mass of 3.01 x 1022 atoms of magnesium?
a)
1.22 grams
b)
1.215 grams
c)
1.2 grams
d)
1.22x1046 grams
21.

When can atoms emit photons?

a)

When the electron is in the ground state

b)

When the electron is in the excited state

c)

When an electron is going from the ground state to the excited state

d)

When an electron is going from the excited state to the ground state

22.

Which energy state has more energy?

a)

Ground State

b)

Excited State

23.

What is happening in the picture

a)

An atom is absorbing energy to go to a higher state

b)

An atom is emitting a photon to go to a lower state

c)

The atom is losing an electron

d)

The atom is losing a proton

24.
Why did the alpha particle (positively charged particle) sometimes bounce back when hitting the gold foil.
a)
hit neutron in nucleus and they repelled alpha particle
b)
hit proton in nucleus and they repelled alpha particle
c)
hit electrons in electron shells and they repelled alpha particle
25.
What atom matches this electron configuration?
1s22s22p63s23p64s23d10
a)
Zinc
b)
Copper
c)
Nickel
d)
Germanium
26.
What atom matches this electron configuration?
1s22s22p63s2
a)
Neon
b)
Magnesium
c)
Aluminum
d)
Potassium
27.
What electron configuration matches an oxygen atom?
a)
1s22s22p63s2, 3p64s23d104p5
b)
1s22s22p4
c)
1s22s22p6
d)
1s22s22p63s23p64s23d1
28.
What is the name of Groups 17?
a)
Alkali Metals
b)
Alkali Earth Metals
c)
Transition Metals
d)
Halogens
29.
Where are the metals on the Periodic Table?
a)
To the left
b)
In the upper right hand corner
c)
On the zigzag line
d)
At the bottom
30.
Where are the nonmetals on the Periodic Table?
a)
To the left
b)
In the upper right hand corner
c)
On the zigzag line
d)
At the bottom
31.

Which 3 are the correct examples of extensive properties?

a)

mass, length, density

b)

mass, length, volume

c)

length, density, color

32.

What is the Molar Mass of KOH?

a)

40

b)

16

c)

1

d)

57

33.

A substance that is tightly packed together is most likely in what state of matter?

a)

solid

b)

liquid

c)

gas

34.

How many nuetrons are in the atom Ag-109?

a)

62

b)

109

c)

47

35.

According to the Electromagnetic Spectrum, what has a greater frequency than visible light?

a)

Microwaves

b)

UV rays

c)

Radiowaves

36.

Which color has the longest wavelength?

a)

Purple

b)

Red

c)

Green

d)

Blue

37.

Which elements are examples of Alkali Earth Metals?

a)

Lithium, Sodium

b)

Beryllium, Magnesium

c)

Boron Aluminum

38.

Label #4

a)

wavelength

b)

crest

c)

trough

d)

frequency

39.

Label #3

a)

wavelength

b)

crest

c)

trough

d)

frequency

40.

Label #1

a)

wavelength

b)

crest

c)

amplitude

d)

frequency

41.

Electronic configurations of atoms: no exceptions. What is the electronic configuration of Titanium, Ti?

a)

[Ar]4s²3d²

b)

[Ar]3s²3d²

c)

[Ar]3s²4d²

d)

[Kr]4s²3d²

42.

The principal quantum number, n, describes:

a)

Orbital shape

b)

Orbital size and energy level

c)

Electron spin

d)

Orientation of the orbital

43.

What is demonstrated by electron diffraction patterns?

a)

Electrons behave as particles.

b)

Electrons behave as waves.

c)

Electrons have no mass.

d)

Electrons are unaffected by energy.

44.

Which group in the periodic table contains the alkali metals?

a)

Group 1

b)

Group 2

c)

Group 17

d)

Group 18

45.

How many grams are in 3.45 kilograms?

a)

34.5 grams

b)

345 grams

c)

3450 grams

d)

.00345

46.

Which of the following is a pure substance?

a)

egg

b)

gold

c)

sea water

d)

bronze

47.

A cube has a known volume of 21.0cm^3. A student uses a graduated cylinder and obtains measurements of 21.1, 20.9, and 21.2. Which of the following best fits the measurements of the student?

a)

precise

b)

accurate

c)

both

d)

neither

48.

Which state of matter has a definite volume but no definite shape?

a)

solid

b)

liquid

c)

gas

d)

none of the above

49.

Which scientist said that negatively charged electrons orbit a positive charged nucleus, much like the planets orbit the sun?

a)

Dalton

b)

Mendeleev

c)

Pauling

d)

Bohr

50.

A student needs to report the average mass of a sample of 7.2785 grams of sodium chloride. Round this number to three significant figures.

a)

7.3 g

b)

7.279 g

c)

7.28

d)

7.27 g

51.

How many neutrons would be in the isotope Nitrogen-15?

a)

7

b)

8

c)

15

d)

14

52.

Which group on the period table is considered to be the most stable and unreactive because they have a full valence shell?

a)

Akali metals

b)

Alkaline metals

c)

Noble Gases

d)

Halogens

53.

Which element does Sodium share similar physical and chemical properties with?

a)

Carbon

b)

Potassium

c)

Silver

d)

Chlorine

54.

How many significant figures are in the following number?

9.56 x 10^-8

a)

5

b)

3

c)

2

d)

6

55.

An isotope of Nitrogen contains 7 protons and 8 neutrons. What is the mass number of the isotope?

a)

7

b)

8

c)

15

d)

14

56.

What experiment was responsible for discovering the electrons, a negatively charged particle?

a)

Gold-Foil Experiement

b)

Cathode-Ray Tube Experiment

c)

Plum Pudding Model

d)

Quantum Mechanics

57.

Isotopic notation for an element includes:

a)

The number of protons only.

b)

The number of neutrons only.

c)

The mass number and atomic number.

d)

The chemical symbol and atomic mass.

58.

In the periodic table, elements in the same vertical column are called:

a)

Periods

b)

Rows

c)

Groups

d)

Families

59.

Which of the following elements is a noble gas?

a)

Oxygen (O)

b)

Neon (Ne)

c)

Sodium (Na)

d)

Carbon (C)

60.

Elements in the same period on the periodic table have the same number of:

a)

Protons

b)

Electrons

c)

Neutrons

d)

Energy levels

61.

Tungsten (W) would be classified as a(n):

a)

element

b)

compound

c)

heterogeneous mixture

d)

homogeneous mixture

62.

Which atom below would be an isotope of sodium with a mass number of 23?

a)

atomic number: 12, # of neutrons: 11, # of electrons: 6

b)

atomic number: 11, # of neutrons: 6, # of electrons: 6

c)

atomic number: 11, # of neutrons: 11, # of electrons: 12

d)

atomic number: 11, # of neutrons: 12, # of electrons: 11

63.

Lithium is a(n):

a)

alkali metal and very reactive

b)

halogen and very reactive

c)

alkali earth metal and reactive

d)

noble gas and very unreactive

64.

When experimenting with the growth of a plant, a scientist uses three (of the same type of) plants, two different fertilizers, equal light, and equal water. What type of variable is the fertilizer?

a)

Dependent

b)

Independent

c)

Control

d)

Compound

65.

Which particle has a mass so small, it is considered to be 0 amu?

a)

proton

b)

hydrogen nucleus

c)

neutron

d)

electron

66.

(8 x 10-23) - (2 x 10-25)

a)

7.98 x 10-23

b)

6 x 10-23

c)

6 x 10-25

d)

7.98 x 10-25

67.

Multiply (1.23 x 104) x (.52 x 102)

a)

6.396 x 107

b)

0.6396 x 107

c)

6.396 x 105

d)

6.396 x 108

68.
Express the following in scientific notation:
.000457
a)
457 x 106
b)
457 x 10-6
c)
4.57 x104
d)
4.57 x 10-4
69.

What is the variable the scientist wants to measure or observe?

a)

Amount of light

b)

Amount of moisture

c)

Number of seeds

d)

# of seeds germinated

70.

You know that 12 inches = 1 foot. Convert 72 inches to feet.

a)

864 feet

b)

6 feet

c)

5 inches

d)

72 feet

71.
When using dimensional analysis, the conversion  fact has to equal _____.
a)
100
b)
0.01%
c)
multiples of 10
d)
1
72.

The conversion factor that should be used to when finding how many inches are in 48.93 cm is ___.

a)

2.54 cm/1 inch

b)

100 cm/ 2.54 inches

c)

1 inch/2.54 cm

d)

2.54 cm/ 2.54 inches

73.

A student measures her heart rate after each of the activities listed. Based on this information, which is a constant in the student's investigation?

a)

Energy expended during activity

b)

Length of activity time

c)

Equipment needed for activity

d)

Activity performed

74.

Which of following is the experimental group in this experiment?

a)

The seeds covered with water and the dry seeds

b)

The dry seeds only

c)

The moist seeds and the seeds covered with water

d)

The dry seeds and the moist seeds

75.
The purpose of the control group is:
a)
Used for comparisons
b)
Application of the I.V.
c)
Application both the I.V. and D.V.
d)
Application of all constants.
76.

Symbol of Micro-

a)

π\pi  

b)

η\eta  

c)

MM  

d)

μ\mu  

77.

3 km = ___________ mm

a)

30

b)

300

c)

3,000

d)

3,000,000

78.

240 cm = ___________ m

a)

2400

b)

24

c)

2.4

d)

0.24

79.

6 kg = _____ g

a)

6

b)

6000

c)

600

d)

.006

80.

A physical blend of 2 or more components is called a ____.

a)

type of element

b)

mixture

c)

chemical reaction

d)

physical property

81.

How many significant figures are there in 1008 grams?

a)

1

b)

2

c)

3

d)

4

82.

How many significant figures are there in 10 liters?

a)

1

b)

2

c)

3

d)

4

83.

If an atom has no charge, which of the following must be true?

a)

It has more neutrons than protons or electrons.

b)

There are only neutrons inside the atom.

c)

Its number of protons is equal to its number of electrons.

d)

The neutrons in the atom outnumber the electrons and protons.

84.
This happens naturally due to an unstable nucleus.
a)
fission
b)
fusion
c)
radioactive decay
d)
K-capture
85.

These are found in the nucleus and have a neutral charge.

a)

proton

b)

electron

c)

neutron

86.

In an atom, an orbital represents

a)

the most probably location of a proton

b)

the most probable location of an electron

c)

the least probably location of a neutron

d)

photons emitted as electrons move to lower energy levels

87.
True or False: The majority of an atom is made up of empty space
a)
True
b)
False
88.

During a flame test, sodium chloride produces an intense yellow flame. This yellow color is produced when electrons in excited atoms

a)

are gained by the atoms

b)

are lost by the atoms

c)

move to higher energy states within the atoms

d)

move to lower energy states within the atoms

89.
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
90.

The unknown emissions spectra belongs to the element

a)

Hydrogen

b)

Mercury

c)

Neon

d)

Helium

91.

Which energy level of Calcium has the most energy?

a)

1st

b)

2nd

c)

3rd

d)

4th

92.

Which accurately describes nonmetals?

a)

Poor conductors of electricity

b)

Often used in computer parts

c)

Both malleable and ductile

d)

Both dull and brittle

93.

What does the unit Liters, L, measure?

a)

Volume

b)

Pressure

c)

Temperature

d)

Moles

94.
When experimenting with the growth of a plant, a scientist uses three (of the same type of) plants, two different fertilizers, equal light, and equal water. What type of variable is the fertilizer?
a)
Dependent
b)
Independent
c)
Control
d)
Compound
95.
Ms. S set up an experiment to see how the mass of a ball affects the distance it rolls off a ramp. What is the dependent variable?
a)
Distance traveled by the ball
b)
Height of the ramp
c)
Mass of the ball
d)
Where the experiment took place.
96.

How close a measurement is to the true value is called..

a)

Accuracy

b)

Precision

c)

Significant

d)

Estimate

97.
When a measurement is repeatable and consistent it is said to have...
a)
High precision
b)
Low precision
c)
High accuracy
d)
Low accuracy
98.
This bullseye demonstrates...
a)
High Accuracy & High Precision
b)
High Accuracy & Low Precision
c)
Low Accuracy & High Precision
d)
Low Accuracy & Low Precision
99.

The attendance for the basketball game was estimated to be 18,000 people but 16,500 people attended. What was the percent error?

a)

10%

b)

9.09%

c)

8.3%

d)

90%

100.

Zed went to the store and bought a bag of chips. He estimated there would be 450 chips in the package, but realized there were only 320 chips in that package. What was his percent error?

a)

29%

b)

41%

c)

85%

d)

92%

101.
What is the correct SI unit for mass?
a)
Kilograms
b)
newtons
c)
pounds
d)
grams
102.
The amount of matter or stuff in an object
a)
volume
b)
mass
c)
force
d)
matter
103.
820 mg = _____ cg
a)
82,000
b)
82
c)
0.82
d)
0.0082
104.
Is 20 g greater than, less than, or equal to 2 kg?
a)
greater than
b)
less than
c)
equal to
105.
How many Significant Figures in the number below?
4.56 x 103
a)
5
b)
4
c)
6
d)
3
106.
How many significant figures does the following number have: 1740200
a)
2
b)
1
c)
3
d)
5
107.
What is 0.000328 rounded to 1 significant figure?
a)
0
b)
0.0003
c)
0.00033
d)
0.000328
108.
Solve. Round using SigFig math rules.
12.5-mL + 20.05-mL + 2.69-mL
a)
35-mL
b)
35.2-mL
c)
35.24-mL
d)
35.240-mL
109.
Calculate 1.23 m x 0.89 m and give your answer with the correct number of significant figures.
a)
1.0 m2
b)
1.1 m2
c)
1.0947 m2
d)
1.095 m2
110.
Calculate 923 g ÷ 20312 cm3 and give your answer with the correct number of significant figures.
a)
0.04 g/cm3
b)
0.045 g/cm3
c)
0.0454 g/cm3
d)
0.05 g/cm3
111.

Which of the following measurements is expressed to three significant figures?

a)

0.007 m

b)

7077 mg

c)

7.30 × 10^−7 km

d)

0.070 mm

112.
Different isotopes have...
a)
different masses
b)
different atomic numbers
c)
different electrons
d)
different protons
113.
How many neutrons does a Flourine-14 isotope have?
a)
4
b)
5
c)
9
d)
14
114.
In the modern periodic table elements are arranged by:
a)
atomic mass
b)
atomic number
c)
valence electrons
d)
number of isotopes
115.

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

116.

Which family(group) of metals have two electrons in the outer most energy level?

a)

Lanthanides

b)

Halogens

c)

Oxygen family

d)

Alkaline earth metals

117.
[Ne]3s23p1 is the noble gas configuration for which element?
a)
scandium
b)
boron
c)
nitrogen
d)
aluminum
118.

Which of the following is not a correct designation for a sublevel?

a)

zz

b)

p

c)

d

d)

f

119.
All orbitals of equal energy are occupied by one electron before any single orbital is occupied by a second electron.
a)
Aufbau principle
b)
Pauli exclusion principle
c)
Hund’s rule
d)
Core Notation
120.
Which guideline, Hund’s rule or the Pauli exclusion principle, is violated in the following orbital diagrams?
a)
Hund's
b)
Aufbau's
c)
Pauli's Exclusive
121.
Which guideline, Hund’s rule or the Pauli exclusion principle, is violated in the following orbital diagrams?
a)
Aufbau's
b)
Hund's
c)
Pauli exclusive
122.
Electrons occupy orbitals of lowest energy first is part of what electron configuration rule?
a)
Hund’s Rule
b)
Aufbau Principle
c)
Pauli Exclusion Principle
123.
Name groups 3B - 12B on the periodic table.
a)
noble gases
b)
halogens
c)
metalloids
d)
transition metals
124.
Which group has the most reactive nonmetals?
a)
alkali metals
b)
noble gases
c)
metalloids
d)
halogens
125.

Which of the following is not part of the atomic theory?

a)

All matter is composed of tiny, invisible, indivisible particles called atoms

b)

Atoms of different elements are different.

c)

Atoms have a neutral charge

d)

Atoms of the same element are the same.

e)

Atoms cannot be created or destroyed, just rearranged.

126.

Who discovered the neutron?

a)

Chadwick

b)

Thompson

c)

Rutherford

d)

Dalton

127.

Who first coined the word, "Atomos"?

a)

Democritus

b)

Dalton

c)

Mendeleev

d)

Thompson

128.

True or False: Mendeleev knew the properties of the elements that weren't discovered yet.

a)

True

b)

False

129.

True or False: Elements that are known as metalloids share the same characteristics as both metals and nonmetals.

a)

True

b)

False

130.

Most metals are NOT:

a)

ductile

b)

malleable

c)

good conductors

d)

liquid at room temperature

131.
A pure substance containing only one kind of atom.
a)
element
b)
mixture
c)
compound
132.
The ability of a substance to be pounded or rolled into thin sheets
a)
State
b)
Ductility
c)
Malleability
d)
Thermal Conductivity
133.
How many electrons can the d sublevel hold?
a)
8
b)
10
c)
2
d)
4
134.

Nitrogen has two isotopes. One isotope has a mass of 14.003 amu and a relative abundance of 99.63%, while the other has a mass of 15.000 amu and a relative abundance of 0.37%. What is the average atomic mass for nitrogen?

a)

14.993 amu

b)

14.456 amu

c)

14.778 amu

d)

14.007 amu

135.
Four isotopes of lead include lead-204, lead-206, lead-207, and lead-208.  The average atomic mass of lead is 207.2.  Which isotope of lead is likely to be the most abundant.
a)
204
b)
206
c)
207
d)
208
136.
Do the following atoms belong to the same element? Explain
       Aluminum-27
       An atom with 14 protons and 13 neutrons
a)
Yes because they have the same number of protons
b)
Yes because they have the same mass
c)
No because they have different number of protons
d)
No because they have different number of neutrons
137.

Give the answer to the correct number of significant figures to

3.419 + 3.912 + 7.0518 + 0.00013

a)

14.383

b)

14.382

c)

14.3829

d)

14.38293

138.

35,400 mg = ________g

a)

3.5400 g

b)

3,540 g

c)

35.4 g

d)

354,000 g

139.

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

140.

Choose the correct shortcut configuration for iodine.

a)

[Ar]4s24d104p5

b)

[Kr]5s24d105p5

c)

[Xe]5s25d105p5

d)

none of the above

141.

Each row on the periodic table represents:

a)

an energy level

b)

a sublevel

c)

an electron

d)

an orbital

142.

Which area on the periodic table represents the electrons in the "d" sublevel?

a)

representative elements

b)

columns 3-8

c)

rare earth elements

d)

transition elements

143.
Chemistry
a)
D=m/v
b)
Neutral group of atoms held by covalent bonds, like C,P,N,H,S,I,Br,Cl,O,F
c)
Study of the composition of matter, A PHYSICAL SCIENCE
d)
energy in crystals for ionic bond
144.
homogeneous mixture example
a)
the energy needed to remove an electron or ion
b)
Ab^2
c)
air, alike throughout mixture
d)
sodium chloride
145.
Problems using Sig Figs - 14 X 2 =
a)
30
b)
all have same atomic number
c)
9 grams X
d)
Protons + Neutrons
146.
Photon
a)
quantum of light
b)
Sea of electrons
c)
An electron occupies the lowest-energy level
d)
another name for an isotope
147.
How many electrons in the 4th main energy level?
a)
unequal positive 2 negative charge like H-Cl-H^+
b)
frequency
c)
32 total
d)
weighted average of the atomic masses for the isotopes of an element
148.

Which best explains why different elements emit different colors of light when they are burned?

a)

Every element has a different arrangement of electrons that get excited in different ways to release different types of light.

b)

They get hot.

c)

Every element has the same arrangement of electrons that get excited in the same ways to release different types of light.

d)

Every element has light always stored in its electrons.

149.

When an electron goes up an energy level in a atom, we say that the electron is_______.

a)

pretty neat

b)

hot

c)

cold

d)

excited

150.

Light is emitted by

a)

electrons gaining energy and going up to a higher energy level

b)

electrons giving off energy as a photon and going down to a lower energy level

c)

little gremlins inside lightbulbs

d)

tractors

151.

What sublevel is this?

a)

p

b)

d

c)

s

d)

f

152.
All matter is made of what?
a)
energy 
b)
atoms 
c)
electrons 
d)
compounds 
153.
What happens in ALL chemical changes?
a)
Change in state of matter
b)
A new substance is formed
c)
Bubbles are produced
d)
An explosion
154.
Molar mass is in units of ________.
a)
grams
b)
grams/mole
c)
mole
d)
moles/gram
155.
What is the molar mass of Mg(NO3)2
a)
148.313g/mol
b)
134.306g/mol
c)
54.311g/mol

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