WorksheetsHonors Chem: Atomic Model
Total questions: 50
Worksheet time: 2hrs 43mins
Name
Class
Date
1.
This was the first model of the atom ever proposed. It was simple and described atoms as tiny spheres that could not be broken down into smaller pieces.
a)
Democritus's model of the atom
b)
The "Plum Pudding Model" of the atom
c)
The "Rutherford Model" of the atom
d)
The "Solar System Model" of the atom
2.
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 "Solar System Model" of the atom
3.
This model added on to previous models by showing electrons existed at certain "energy levels". However is does not accurately show what those levels look like.
a)
The "Solar System Model" of the atom
b)
The "Rutherford Model" of the atom
c)
The "Plumb Pudding Model" of the atom
d)
The "Standard Model" of the atom
4.
What sub-atomic particle is this?
In the Nucleus
Positively Charged
Mass of 1 amu
In the Nucleus
Positively Charged
Mass of 1 amu
a)
proton
b)
electron
c)
nutron
5.
What sub-atomic particle is this?
Outside the Nucleus
Negatively Charged
Mass of 1/1000 amu
Outside the Nucleus
Negatively Charged
Mass of 1/1000 amu
a)
proton
b)
electron
c)
neutron
6.
What sub-atomic particle is this?
NeutronIn the Nucleus
No Charge
Mass of 1 amu
NeutronIn the Nucleus
No Charge
Mass of 1 amu
a)
proton
b)
electron
c)
neutron
7.
What is the atomic number of Chlorine (Cl)?
a)
17
b)
Cl
c)
35.453
d)
Chlorine
8.
The number of protons and electrons are the same as
a)
Atomic number
b)
Neutrons
c)
atomic mass
d)
Electron shells
9.
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.
10.
Ernest Rutherford discovered that atoms were mostly _________________.
a)
negatively charged
b)
positively charged
c)
electrons
d)
empty space.
11.
What does the nucleus of an atom contain?
a)
Electrons & Neutrons
b)
Protons & Neutrons
c)
Neutrinos & Positrons
12.
The majority of an atom's mass exists where?
a)
In the nucleus
b)
In the electron cloud
c)
In the space between the nucleus and the electrons
d)
In the neutrons
13.
How many protons are in this element?
a)
79
b)
196
c)
117
d)
Cannot be determined
14.
How many neutrons does this isotope of titanium have?
a)
48
b)
22
c)
26
d)
70
15.
What is the nuclear charge of this atom?
a)
+48
b)
+22
c)
0
d)
-22
16.
Who discovered the nucleus of an atom?
a)
JJ Thomson
b)
Ernest Rutherford
c)
John Dalton
d)
Democritus
17.
He proposed the "muffin" or "plum pudding model of the atom.
a)
John Dalton
b)
Niels Bohr
c)
Ernest Rutherford
d)
JJ Thomson
18.
How many neutrons does the isotope of lithium have?
a)
8
b)
3
c)
4
d)
5
19.
What was significant about the "gold foil" experiment, performed by Geiger and Marsden?
a)
It demonstrated that atoms contained a tiny positively charged nucleus at their centre
b)
It demonstrated that electrons were negatively charged
c)
It explained the Rydberg formula and the existence of emission spectra
d)
It demonstrated the existence of the neutron
20.
Which kind of wave has the greatest frequency?
a)
gamma rays
b)
infrared
c)
ultraviolet
d)
microwaves
21.
Determine the wavelength of this wave?
a)
1m
b)
2m
c)
3m
d)
4m
22.
What is the shortest wavelength of visible light?
a)
10-12m
b)
710nm
c)
390nm
d)
10m
23.
Which of the following regions of the electromagnetic spectrum has the lowest frequency?
a)
ultraviolet
b)
infrared
c)
visible
d)
x-ray
24.
An argon ion laser emits light at 488 nm. What is the frequency of this radiation?
a)
4.07 x 10^-19 Hz
b)
6.14 x 10^14 Hz
c)
1.46 x 10^2 Hz
d)
2.05 x 10^ 6 Hz
25.
If an AM radio station broadcasts at 995 kHz, what is the wavelength of this radiation?
a)
6.59 x 10^-28 m
b)
1.01 x 10^-6 m
c)
3.32 x 10^-3 m
d)
301 m
26.
A microwave oven emits radiation at a wavelength of 0.500 cm. What is the frequency of this radiation?
a)
6.67 x 10^-7 Hz
b)
2.00 Hz
c)
1.50 x 10 ^ 6 Hz
d)
6.00 x 10^10 Hz
27.
An radium-266 atom may emit a photon of light with a frequency of 4.50 x 1019 Hz when it undergoes nuclear fission. What is the wavelength (in pm) of this photon?
a)
0.0298 pm
b)
6.66 pm
c)
15.0 pm
d)
29.8 pm
28.
The ________ of a photon of light is ________ proportional to it frequency and ________ proportional to its wavelength.
a)
amplitude, directly, inversely
b)
energy, inversely, directly
c)
energy, directly, inversely
d)
velocity, inversely, directly
29.
High frequency waves have _________ wavelength.
a)
varying
b)
high
c)
the same
d)
low
30.
Look carefully at the waves. Which carries the most energy?
a)
microwave
b)
infrared
c)
ultraviolet
d)
x-ray
31.
Which part of the electromagnetic spectrum has high enough energy to cause damage to eyes and skin, and sometimes even cancer?
a)
Infrared Rays
b)
Radio Waves
c)
Microwaves
d)
Ultraviolet Rays
32.
A wave with a large wavelength will have a ______ frequency and _____ energy
a)
high, low
b)
high, high
c)
low, high
d)
low, low
33.
The unit of frequency is ___.
a)
meters
b)
nanometers (nm)
c)
m/s
d)
Hertz
34.
What is the frequency of a wavelength at 0.75 meters?
a)
30 Hz
b)
60 Hz
c)
80 Hz
d)
1000 Hz
35.
A common infrared laser operates at 1.06 x 103 nm. What if the energy of a photon with this wavelength?
a)
7.02 x 10^-40 J
b)
6.25 x 10^-28 J
c)
3.54 x 10^-15 J
d)
1.87 x 10^-19 J
36.
What do we call a massless bundle (particle) of concentrated electromagnetic energy?
a)
proton
b)
electron
c)
wave
d)
photon
37.
Light behaves as both a(n) __________ and a(n) __________
a)
photon, sound
b)
wave, photon
c)
wave, particle
d)
wavicle, photon
38.
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
39.
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
40.
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
41.
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
42.
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
43.
What is the RELATIVE mass of a proton?
a)
basically zero
b)
1.67 x 10-24 g
c)
1 amu
d)
unknown
44.
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
45.
The speed of a wave is its wavelength multiplied by its ___________
Or the formula
C = λ x ν
Or the formula
C = λ x ν
a)
amplitude
b)
vibration
c)
frequency
d)
reflection
46.
Put the visible light colors in order from longest wavelength to shortest wavelength
a)
Violet, Indigo, Blue, Green, Orange, Yellow, Red
b)
Red, Yellow, Green, Orange, Violet, Blue, Indigo
c)
Red, Orange, Yellow, Green, Blue, Indigo, Violet
47.
Solve this problems using the equation: C = λ x ν
A microwave oven emits radiation at a wavelength of 5.00 x 10^-1cm. What is the frequency of this radiation?
(Convert to m first).
A microwave oven emits radiation at a wavelength of 5.00 x 10^-1cm. What is the frequency of this radiation?
(Convert to m first).
a)
6.67 x 10^-7 Hz
b)
2.00 Hz
c)
1.50 x 10 ^ 6 Hz
d)
6.00 x 10^10 Hz
48.
Violet light has a wavelength of 4.10 x 10^-12 m. What is the frequency?
a)
1.23 x 10^ -3 Hz
b)
7.31 x 10^ 19 Hz
c)
1.37 x 10^12 Hz
d)
3.0 x 10^ 8 Hz
49.
Calculate the energy of red light.
a)
2.82 x 10^ -28 J
b)
2.84 x 10^ -19 J
c)
2.11 x 10^11 J
d)
4.29 x 10^12 J
50.
Calculate the wavelength of EM radiation that has energy of 3.98 ^10-19 J. What color is this EM radiation?
a)
499 nm. Violet
b)
499 km. Radio waves; no visible color to humans
c)
499 nm. Orange
d)
119 A. UV ranage
100 %
