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WorksheetsAtomic Theory and Structure (Honors)
Total questions: 41
Worksheet time: 2hrs 44mins
Name
Class
Date
1.
Electrons can be found in
a)
The protons
b)
The nucleus
c)
Electron Clouds
2.
This is the SI unit used for the masses of atomic particles
a)
ion
b)
amu
c)
moles
d)
grams
3.
This contains most of the mass of an atom
a)
Electron Cloud
b)
Nucleus
c)
Electron
d)
Ions
4.
The weighted average of the masses of all naturally occurring isotopes of an element is
a)
Atomic number
b)
Atomic mass
c)
Mass number
d)
Neutrons
5.
The first person to ever talk about an atom was
a)
Democritus
b)
Rutherford
c)
Dalton
d)
Bohr
6.
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
7.
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.
c)
He discovered that atoms had nuclei.
d)
He discovered that atoms could be divided into smaller parts.
8.
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
9.
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.
10.
What is the smallest particle of an element?
a)
atom
b)
proton
c)
electron
d)
neutron
11.
What scientist first developed 4 rules for atomic theory, and helped kick start modern chemistry?
a)
J.J. Thomson
b)
Ernest Rutherford
c)
John Dalton
d)
Democritus
12.
Niels Bohr suggested that electrons.......
a)
are found in specific orbits
b)
electrons are scattered throughout the atom
c)
electrons move according to their energy level
d)
electrons are positive
13.
True or False: The majority of an atom is made up of empty space
a)
True
b)
False
14.
What element is pictured?
a)
Hydorgen
b)
Boron
c)
Beryllium
d)
Arsenic
15.
How many neutrons are in an atom with an atomic number of 20, an atomic mass of 45, and a charge of +2?
a)
20
b)
25
c)
45
d)
18
16.
How many electrons are in an atom with an atomic number of 20, an atomic mass of 45, and a charge of +2?
a)
20
b)
22
c)
18
d)
2
17.
What characteristic of an element's atoms ALWAYS determines the element's identity?
a)
the number of neutrons
b)
the number of protons
c)
the atomic mass
d)
the number of valence electrons
18.
Calculate the average atomic mass of silver. (answers are not to correct sig figs)
a)
106.38649amu
b)
111.91896amu
c)
107.8677amu
d)
121
19.
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
20.
What is the biggest difference between an atom of cobalt (Co) and an atom of nickel (Ni) as shown in the periodic table entries?
a)
An atom of nickel has more protons.
b)
An atom of cobalt has more electrons.
c)
An atom of cobalt has a lower number of neutrons.
d)
An atom of nickel has a higher value for atomic mass.
21.
A neutral atom of Carbon-13 has ________ electrons and _________ neutrons
a)
13, 13
b)
6, 6
c)
7, 7
d)
6, 7
22.
What is the RELATIVE mass of a proton?
a)
basically zero
b)
1.67 x 10-24 g
c)
1 amu
d)
unknown
23.
In a correctly written symbol what would be located in the "Z" position?
a)
number of neutrons
b)
atomic number
c)
number of electrons
d)
mass number
24.
The mass of an atom is located in the ___________ and the volume of an atom is made of the ____________
a)
electron cloud, nucleus
b)
electron cloud, energy levels
c)
nucleus, electron cloud
d)
nucleus, neutrons
25.
The number in Kr-84 represents what about Krypton?
a)
The number of electrons
b)
The number of neutrons
c)
The mass number
d)
The atomic number
26.
The mass of a proton or neutron is equal to __________ g.
a)
1.67 x 10-24
b)
6.02 x 1023
c)
6.626 x 10-34
d)
3.00 x 108
27.
The speed of light is equal to __________ m/s.
a)
1.67 x 10-24
b)
6.02 x 1023
c)
6.626 x 10-34
d)
3.00 x 108
28.
Light with high energy has...
a)
high wavelength and frequency
b)
high wavelength and low freqency
c)
low wavelength and high frequency
d)
low wavelength and frequency
29.
True or False: A mole of copper atoms has more particles than a mole of carbon atoms
a)
True
b)
False
30.
Calculate the energy of a 6.67 x 1012 Hz wave.
a)
4.42 x 10-21 J
b)
4.50 x 10-5 J
c)
9.93 x 10-47 J
d)
1.01 x 1046 J
31.
Calculate the wavelength of a 6.67 x 1012 Hz wave.
a)
4.42 x 10-21 m
b)
4.50 x 10-5 m
c)
2.23 x 104 m
d)
2.00 x 1021 m
32.
The actual mass of a carbon-12 atom is __________. (You can calculate it or some of you may have it memorized)
a)
1.67 x 10-24 g
b)
2.00 x 10-23 g
c)
12 amu
d)
12 g
33.
What part of the spectrum does a wave fall on if its frequency is 2.4 x 1013 Hz?
a)
infrared
b)
gamma rays
c)
microwaves
d)
visible light
34.
Calculate the atomic mass of copper-62.
a)
62.4 amu
b)
1.04 x 10-22 g
c)
63.5 amu
d)
29 g
35.
Dalton's law that stated elements combine in whole number ratios.
a)
Law of conservation of mass
b)
Law of definite proportions
c)
Law of multiple proportions
d)
Law of gravity
36.
The particle that determines how reactive an element will be is the _____.
a)
Proton
b)
Neutron
c)
Electron
d)
Nucleus
37.
What subatomic particles have the SAME mass?
a)
protons and neutrons
b)
protons and electrons
c)
neutrons and electrons
d)
protons, neutrons & electrons
38.
Is this atom neutral?
a)
Yes, because the protons = neutrons
b)
Yes, because the protons = electrons
c)
No, because the outside ring is not full
d)
No, it is missing electrons
39.
How many valence electrons does this atom have?
a)
2
b)
4
c)
5
d)
9
40.
What is the identity of this element based on this Bohr model?
a)
Magnesium (Mg)
b)
Aluminum (Al)
c)
Iron (Fe)
d)
Chromium (Cr)
41.
How many valence electrons are in this atom?
a)
3
b)
13
c)
14
d)
27
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