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Chemistry Test 1

Total questions: 132

Worksheet time: 5hrs 4mins

Name
Class
Date
1.
Isotopes are atoms of the same element with different #’s of __________ & therefore different __________.
a)
n0 ;  atomic #’s
b)
p+ ; atomic #’s
c)
e- ; atomic masses
d)
n0 ; atomic masses
2.
How many neutrons does the isotope below have?     89 36Kr
a)
53
b)
36
c)
89
d)
125
3.
If X is the symbol for an element, which of the following two symbols represent    isotopes of the same element?     I. 7735X  II. 7733X  III. 8137X  IV. 8135 X
a)
I and II
b)
III and IV
c)
I and IV
d)
I and III
4.
How many neutrons does an atom of the isotope Neon-22 have?
a)
12
b)
10
c)
22
d)
20
5.
If the number of electrons in an atom changes you make a(n) __________________.
a)
ion
b)
isotope
c)
new element
d)
isomer
6.
Ions are: 
a)
atoms with a positive or negative charge
b)
atoms with no charge
c)
atoms with ONLY a positive charge
d)
atoms with ONLY a negative charge
7.
How many electrons are in an atom that has an atomic number of 34, an atomic mass of 74 and a charge of -2?
a)
34
b)
36
c)
2
d)
40
8.
How many protons does this isotope of titanium have?
a)
48
b)
22
c)
26
d)
70
9.
How many neutrons does the isotope of lithium have?
a)
8
b)
3
c)
4
d)
5
10.
In a correctly written symbol what would be located in the "A" position?
a)
number of neutrons
b)
atomic number
c)
number of electrons 
d)
mass number
11.
What quantities vary between isotopes of an element?
a)
protons, electrons, and atomic mass
b)
protons, electrons, and atomic number
c)
neutrons and electrons
d)
neutrons and atomic mass
12.
which atom has  4 neutrons?
a)
Li-6
b)
Li-7
c)
Li-8
d)
they have the same # of neutrons
13.
How many neutrons does the isotope below have?     89 36Kr
a)
53
b)
36
c)
89
d)
125
14.
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
15.
What is the name of the pictured isotope?
a)
Chlorine-Schmorine
b)
Chlorine-17
c)
Chlorine-35
d)
Chlorine-18
16.
What is the name of the pictured isotope?
a)
Copper-29
b)
Copper-63
c)
Copper-34
d)
CopperWopperHopperBopper
17.
What is the name of the pictured isotope?
a)
Carbon-12
b)
Carbon-13
c)
Carbon-14
d)
Carbon-15
18.
How many neutrons does B (Boron) contain?
a)
5
b)
11
c)
6
d)
10.811
19.
Adding or subtracting neutrons (charge = 0, mass = 1) makes the element change into an...
a)
ion
b)
mixture
c)
isotope
d)
neutral atom
20.
If an atom gains an electron it is a(n)
a)
Positive ion
b)
Negative ion
c)
Isotope
d)
Neutral Atom
21.
If an atom loses an electron it is a(n)
a)
Positive ion
b)
Negative ion
c)
Isotope
d)
Neutral Atom
22.
Ca+ is an example of a(n)
a)
Positive ion
b)
Negative ion
c)
Isotope
d)
Neutral Atom
23.
Carbon-14 is an example of a(n)
a)
Positive ion
b)
Negative ion
c)
Isotope
d)
Neutral Atom
24.
Which answer choice describes the subatomic particles and their respective charges?
a)
p-    e+    n
b)
p+    e     n-
c)
p+    e-    n
d)
p-     e+    n
25.
Has the symbol
a)
Alpha
b)
Beta 
c)
Gamma
26.
When an atom loses this particle, the atomic number of the product atom is lower by the two and its mass number is lower by four. 
a)
Alpha 
b)
Beta
c)
Gamma
27.
Has a mass of 0 and a charge of 0
a)
Alpha
b)
Beta
c)
Gamma
28.
Has the symbol
a)
Alpha
b)
Beta
c)
Gamma
29.
Has a moderate penetrating power.  It can penetrate 4 mm into body tissue and can be stopped by metal foil.
a)
Alpha
b)
Beta
c)
Gamma
30.
Electromagnetic radiation made of high-energy photons.
a)
Alpha 
b)
Beta
c)
Gamma
31.
Has the symbol
a)
Alpha
b)
Beta
c)
Gamma
32.
Has the lowest penetrating power.  Can only penetrate 0.05 mm into the body and can be stopped by a piece of paper or clothing.
a)
Alpha
b)
Beta
c)
Gamma
33.
This individual accidentally discovered a process when working with uranium salts on a photographic plate.  Who is this scientist?
a)
Marie Curie
b)
Antoine Henri Becquerel
c)
Pierre Curie
34.
This individual won the 1911 Nobel Peace Prize for Chemistry.
a)
Marie Curie
b)
Antoine Henri Becquerel 
c)
Pierre Curie
35.
What was one of the draw backs of Marie Curie's work?
a)
She missed out on valuable family time
b)
She died from leukemia caused by  her long term exposure to radiation
c)
She was limited in diet and wasn't able to eat chicken
36.

All elements with atomic number greater than _____ are radioactive.

a)

14

b)

84

c)

90

37.

In beta decay, a neutron is

a)

turned into an electron.

b)

is gained.

c)

turned into a proton and a high speed electron.

38.

If Lead-214 undergoes beta decay, the element goes through a transmutation to

a)

mercury

b)

bismuth

c)

polonium

39.

If Polonium-218 undergoes alpha decay, it becomes

a)

lead

b)

Astatine

c)

mercury

40.

During beta-particle emission, a neutron splits into a____________________.

a)

proton and electron

b)

neutron and electron

c)

neutron and proton

41.
The process of nuclear change in an atom of radioactive material is called... 
a)
nuclear decay
b)
nuclear mass
c)
isotopes
d)
radon
42.
Radioactive materials have unstable...
a)
electrons
b)
protons
c)
nuclei
d)
neutrons
43.
This is an example of...
a)
Fission  reaction
b)
Fusion reaction
c)
Decomposition reaction
d)
Decay
44.
Which process involves the joining of small nuclei?
a)
Beta decay
b)
Alpha decay
c)
Nuclear fission
d)
Nuclear fusion
45.

How many grams of Carbon-14 will remain after 17,100 years?

a)

32 g

b)

16 g

c)

8 g

d)

4 g

46.

What percentage of Rubidium-87 will remain after 4 half-lives?

a)

25%

b)

12.5%

c)

6.25%

d)

3.125%

47.
The length of time required for half of the radioactive atoms in a sample to decay is its...
a)
era
b)
age
c)
half-life
d)
eon
48.

In the equation, 146C --> 147N + 0-1B, the _______ decay of radioactive carbon-14 results in the creation of a new nitrogen-14 atom.

a)

Gamma

b)

Beta

c)

Alpha

49.
Uranium-238  decays into  Thorium-234  by emitting .........
a)
an alpha particle
b)
a beta particle
c)
gamma rays
d)
visible light
50.
A helium nucleus with two protons and two neutrons is called a(n) ____.  
a)
alpha particle
b)
electroscope
c)
beta particle
d)
gamma ray
51.
Which type of nuclear radiation is being emitted here?
a)
Alpha
b)
beta
c)
gamma 
d)
none
52.
If we start off with element 24X50 after an alpha decay we get another element Y that looks like
a)
22Y50
b)
22Y46
c)
20Y48
d)
26Y54
53.
Solve this equation for alpha decay.
85209At = ___ + 24He
a)
83205Bi
b)
86209Rn
c)
81207Tl
d)
85208At
54.
Balance the following equation:
146C --> 0-1e + ________
a)
145B
b)
146C
c)
147N
d)
42He
55.
Solve this equation for alpha decay.
85209At = ___ + 24He
a)
83205Bi
b)
86209Rn
c)
81207Tl
d)
85208At
56.

Gamma rays have

a)

no mass

b)

a huge mass

c)

a small mass

d)

an average mass

57.
Solve this equation for beta decay.
614C = ___ + -10e
a)
410Be
b)
714N
c)
210He
d)
613C
58.
The diagram shows the path of radioactive rays, S and T. Which of the following shows the type of ray S and ray T?
a)
ray S= alpha.  ray T=beta
b)
ray S= alpha   ray T=gamma
c)
ray S= beta.    ray T=gamma
d)
ray S= gamma.  ray T= beta
59.

An isotope that undergoes B- decay has

a)

too few protons

b)

too many protons

c)

too few neutrons

d)

Too many neutrons

60.

Solve this equation for beta decay.

614C = ___ + -10e

a)

410Be

b)

714N

c)

210He

d)

613C

61.

Which of these is a use of alpha radiation?

a)

Sterilising food

b)

Smoke detectors

c)

Monitoring paper thickness

d)

Industrial tracers

62.
For which of the following problems would a scientist most likely use carbon-14? 
a)
to calculate the age of the Earth's oldest rocks
b)
to calculate the age of a piece of bone 
c)
to identify the elements that make up a rock 
d)
to identify the elements that make up a bone
63.
Where does radioactivity have application in our lives?
a)
Medicine
b)
Energy (electricity)
c)
Agriculture
d)
All of the above
64.

How is radiation used to treat cancer?

a)

Radiation is used to stimulate the growth of cancer cells

b)

Cancer cells are bombarded with radiation and become inactive

c)

Cancer cells are burned up by radiation

d)

Radiation melts cancer cells

65.

Nuclear medicine (like radiation used in cancer treatment) is used to both diagnose and treat different diseases.

a)

True

b)

False

66.

beneficial uses of radiation include

a)

irradiating food

b)

causing cancer

c)

death

d)

poisoning

67.
If 10 mg of iodine 131 is given to a patient, how much is left after 24 days? The half-life of iodine-131 is 8 days.
a)
1.25mg
b)
1.25g
c)
10g
d)
10mg
68.
The half-life of strontium-90 is 25 years. How much strontium-90 will remain after 100 years if the initial amount is 4.0 g?
a)
3.0g
b)
0.25mg
c)
0.3g
d)
0.25g
69.
What is the half-life of iodine-131?
a)
32 days
b)
8 days
c)
16 days
d)
24 days
70.
The word "atom" is from the _____
a)
Latin for "three parts"
b)
Greek for "indivisible"
c)
Gaelic for "uncuttable"
d)
French for "tiny"
71.
The proton is _____
a)
heavy and neutral
b)
heavy and negatively charged
c)
heavy and positively charged
d)
light and negatively charged
72.
The electron is _____
a)
heavy and positively charged
b)
light and positively charged
c)
light and neutral
d)
light and negatively charged
73.

Which subatomic particles determine the identity of an element?

a)

electrons

b)

protons

c)

neutrons

d)

photons

74.
The number of protons in an element is its _____
a)
atomic weight
b)
relative atomic mass
c)
atomic number
d)
mass number
75.
Neutrons serve as a kind of _____
a)
charge carrier
b)
shock absorber for collisions
c)
shield for radiation
d)
buffer between the protons
76.
Which term is basically the weighted average of the number of nucleons found in nature?
a)
atomic weight
b)
relative atomic mass
c)
relative atomic number
d)
mass number
77.
Which term represents just the total number of nucleons in the nucleus of an atom?
a)
atomic weight
b)
relative atomic mass
c)
atomic number
d)
mass number
78.
Variants of an element, with different masses but the same chemical properties, are called _____
a)
isotropics
b)
isotherms
c)
isomers
d)
isotopes
79.

Compared to the rest of the atom the nucleus is

a)

small and contains most of the mass

b)

Large and contains no mass

c)

small and contains little mass

d)

Large and contains most of the atoms mass

80.
What atom matches this electron configuration?
1s22s22p63s23p64s23d10
a)
Zinc
b)
Copper
c)
Nickel
d)
Germanium
81.
What electron configuration matches an oxygen atom?
a)
1s22s22p63s2, 3p64s23d104p5
b)
1s22s22p4
c)
1s22s22p6
d)
1s22s22p63s23p64s23d1
82.
How many electrons does Si contain? (click to see image)
a)
14
b)
28
c)
2
d)
4
83.
How many electrons can the first energy level hold?
a)
1
b)
2
c)
8
d)
0
84.
The electron configuration of an atom is 1s22s22p6.  The number of electrons in the atom is 
a)
3
b)
6
c)
8
d)
10
85.
Which electron configuration belongs to Chlorine (Cl)?
a)
1s2 2s2 2p6 3s2 3p5
b)
1s2 2s2 2p6 3s2 3p6
c)
1s2 2s2 2p6 3s2 3p7
86.
There are 4 different types of subshells s,p,d,f
a)
true
b)
false
87.
What is the maximum number of electrons that an orbital can have?
a)
1 electron
b)
2 electrons
c)
3 electrons
d)
4 electrons
88.
What is the shorthand electron configuration for Sulfur atom?
a)
[Ar] 3p4
b)
[He] 3s23p4
c)
[Ne] 3s23p4
d)
[Na] 3s23p3
89.
Which element is pictured?
a)
neon
b)
fluorine
c)
magnesium
d)
argon
90.
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
91.

What does Pauli exclusion principle state ?

a)

states that each electron occupies the lowest energy orbital available

b)

states that -no two electrons in the same orbital can have the same spin

c)

states that single electrons electrons with the same spin must occupy each-energy orbital before additional electrons with opposite spins can occupy the same orbitals

92.

Horizontal (SIDE TO SIDE) rows on the periodic table are

a)

groups

b)

periods

93.

The period number tells you the number of

a)

protons

b)

energy levels

c)

valence electrons

94.

How many energy levels does Au have? Just give me the number.

(a)  

95.

How many energy levels does Co have? Just give me the number.

(a)  

96.

Db and Ru have the same number of energy levels.

a)

True

b)

False

97.

H and He have the same number of energy levels.

a)

True

b)

False

98.

JJ Thomson discovered what subatomic particle

a)

nucleus

b)

neutron

c)

proton

d)

electron

99.

Rutherford discovered what part of the atom

a)

nucleus

b)

neutron

c)

proton

d)

electron

100.

First person to propose the concept of an atom

a)

Rutherford

b)

Democritus

c)

Dalton

d)

Bohr

101.

Who proposed the theory that atoms orbit the nucleus in specific orbits.

a)

Bohr

b)

Democritus

c)

Rutherford

d)

Chadwick

102.

This particle balances the charges from the protons to make the atom neutral

a)

proton

b)

electron

c)

neutron

d)

nucleus

103.

These particles are found in the nucleus

a)

protons and electrons

b)

nucleus and neutrons

c)

protons and neutrons

d)

electrons and neutrons

104.

Which of the following shows the correct order of Atomic Theory Timeline

a)

Rutherford, Bohr, Dalton, Democritus, Thomson

b)

Bohr, Democritus, Thomson, Rutherford, Dalton

c)

Dalton, Thomson, Rutherford, Bohr, Democritus

d)

Democritus, Dalton, Thomson, Rutherford, Bohr

105.

Thomson Experimented with ______

a)

Gold Foil

b)

alpha particles

c)

cathode rays

d)

protons

106.

Rutherford experimented with ____

a)

Gold foil and alpha particles

b)

Cathode rays and alpha particles

c)

electron and alpha particles

d)

gold foil and cathode rays

107.

Which Scientist created this model

a)

Democritus

b)

Chadwick

c)

Bohr

d)

Rutherford

108.
Who stated that atoms cannot be divided?
a)
Democritus
b)
Dalton
c)
Thomson
d)
Bohr
109.
What scientist is best known for his "Plum Pudding" model of the atom?
a)
J.J. Thomson
b)
Ernest Rutherford
c)
John Dalton
d)
Democritus
110.
What contribution did John Dalton make to atomic theory? 
a)
He discovered that every atom was positively charged. 
b)
He discovered that every element consisted of one type of atom that couldn't be divided. 
c)
He discovered that atoms had nuclei. 
d)
He discovered that atoms could be divided into smaller parts. 
111.
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.
112.
The first person to propose a theory about an atom called the Atomos Theory was
a)
Democritus
b)
Rutherford
c)
Dalton
d)
Aristotle
113.
His atomic model was depicted similar to a planetary/solar system
a)
Niels Bohr
b)
Joseph Thomson
c)
Ernest Rutherford
d)
Democritus
114.
Who's model is this? 
a)
Millikan
b)
Rutherford
c)
Thomson
d)
Bohr
115.
How did each model of the atom help to develop the atomic theory? 
a)
Each model provided opinions that were added.
b)
Each model showed different properties of the same structure. 
c)
Each model showed new particles that had been discovered.
d)
Each model built upon the other to show new particles or properties of previously discovered particles. 
116.
Electron cloud is based on
a)
Quantum Mechanics
b)
Gold Foil Experiment
c)
Matter is made up of small particles called atoms
d)
Nuclear Theory
117.
James Chadwick discovered the ________.
a)
proton
b)
neutron
c)
electron
d)
nucleus
118.

What results did Rutherford expect to see if the Plum-Pudding model is correct?

a)

He expected that most of alpha particles would go through a gold-foil and small number of particles would deflect sightly

b)

He expected that most of alpha particles would not go through a gold-foil and will stop on one side of a foil.

c)

He expected that most of alpha particles would ricochet back after hitting a gold-foil

119.

What results did Rutherford observe in his Gold-Foil experiment?

a)

He observed that all alpha particles did go through a gold-foil in straight lines

b)

He observed that most alpha particles did not go through a gold-foil and stopped on one side of the gold foil.

c)

He observed that a small number of alpha particles bounced off the gold-foil at very large angles

d)

He observed that all alpha particles slightly deflected from the straight line when going through a gold-foil

120.

Choose one of the conclusions that Ernest Rutherford made based on the experimental results of his Gold-Foil experiment

a)

He concluded that the atom is indivisible

b)

He concluded that the atom is mostly empty space

c)

He concluded that the atom has neutrons

d)

He concluded that the atom is tightly packed with subatomic particles all mixed together

121.
He found that atoms have smaller parts and found negative electrons that he theorized were surrounded in a sphere of positive charges
a)
J.J. Thomson
b)
Ernest Rutherford
c)
Niels Bohr
d)
James Chadwick
122.
He found the positively charged protons in the nucleus and said that electrons moved around the nucleus
a)
J.J. Thomson
b)
Ernest Rutherford
c)
Niels Bohr
d)
James Chadwick
123.
He first measured the mass and charge of an electron using the oil drop experiment.
a)
Joseph Thomson
b)
Robert Millikan
c)
John Dalton
d)
Niels Bohr
124.

The color of emitted light with the LONGEST wavelength is

a)

violet

b)

green

c)

red

d)

indigo

125.

Each element produces its own pattern of emission spectra lines because each element has its own distinct

a)

Speed of light

b)

Electron configuration

c)

Number of neutrons

d)

None of these

126.

The color of emitted light with the SHORTEST wavelength is

a)

violet

b)

green

c)

red

d)

indigo

127.

This device is a

a)

telescope

b)

spectrascope

c)

microscope

d)

prism

128.

How many of the following substances are elements?

 SS   N2O4N_2O_4   FeFe   O2O_2   LiFLiF   SrSr   AlAl  

a)

5

b)

3

c)

4

d)

6

129.

All stars are composed of a mixture of elements. When these elements are heated they emit specific amounts of electromagnetic radiation, known as an emission spectrum. Each element emits a unique, identifiable, spectrum.


Using the Bright-line emission spectrum chart below, identify the elements present in this modeled star (found in the line labeled “mixture”).

a)

Lithium and cadmium are in the mixture. Strontium is not in the mixture.

b)

Lithium and strontium are in the mixture. Cadmium is not in the mixture

c)

Cadmium and strontium are in the mixture. Lithium is not in the mixture

d)

All of the shown elements are present in the mixture.

130.
Emission of light from an atom occurs when an electron
a)
drops from a higher to a lower energy level.
b)
   jumps from a lower to a higher energy level.   
c)
   moves within its atomic orbital.
d)
falls into the nucleus.
131.

How many electrons can each sublevel hold?

a)

s-1, p-2, d-3, f-4

b)

s-2, p-2, d-2, f-2

c)

s-2, p-6, d-10, f-14

132.
Which of these is the electron?
a)
A
b)
B
c)
C
d)
D

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