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Unit 2 Test Review

Total questions: 41

Worksheet time: 54mins

Name
Class
Date
1.
Isotopes are elements with a different amount of
a)
protons
b)
neutrons
c)
electrons
d)
atoms
2.
an element will always have the same number of 
a)
neutrons
b)
protons
c)
isotopes
d)
atoms
3.
Which particle does not contribute mass to the atom?
a)
Proton
b)
Neutron
c)
Electron
d)
Nucleus
4.
An atom has 10 protons and a mass of 18. It has __ neutrons
a)
10
b)
18
c)
28
d)
8
5.
The mass number of an element that has18 protons, 18 electrons, and 19 neutrons is _____.
a)
12.5
b)
13
c)
25
d)
37
6.
How many neutrons does uranium-239 have
a)
92
b)
147
c)
239
d)
331
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.
What charge does an atom have if it GAINS an electrons?
a)
Positive (+)
b)
Negative (-)
9.

True or False: Electrons are found in the nucleus.

a)

True

b)

False

10.

Which scientist developed this model?

a)

Dalton

b)

Thomson

c)

Rutherford

d)

Bohr

11.

True or False: This model is considered the most modern of all the models we have discussed.

a)

True

b)

False

12.

What is the maximum number of electrons that can be found in the first shell?

a)

2

b)

8

c)

18

13.
Where electrons are likely to be found as they travel around the nucleus
a)
Nucleus
b)
Electron Cloud
c)
Within a Proton
d)
Within a Neutron
14.
Which electromagnetic waves have the highest frequencies and the shortest wavelengths?
a)
microwaves
b)
visible light
c)
gamma rays
15.
For waves in any medium, as the wavelength decreases, what happens to the frequency?
a)
It also decrease
b)
It stays the same
c)
It increases
16.
Which of the following has frequencies higher than ultraviolet rays?
a)
visible light
b)
infrared rays
c)
x-rays
17.
A certain photon of light has a wavelength of 4.22x10-7nm. What is the frequency? (v=c/λ)
a)
7.11x1014 Hz
b)
7.11Hz
c)
1.41x10-15
d)
-1.41x1015
18.
A wave with a large wavelength will have a ______ frequency and _____ energy
a)
high, low
b)
high, high
c)
low, high
d)
low, low
19.
What happens to the energy of a photon as the frequency of the wave increases? 
a)
The energy increases
b)
The energy decreases
c)
The energy stays the same 
20.
What is the energy of a quantum of light with a frequency of 7.39x1014Hz.(E=Hv)
a)
4.88x1019
b)
4.88x10-19
c)
2.22x1023
d)
2.22x10-23
21.
What is the wavelength for a quantum of light with energy of 7.56x10-19J? (λ=hc/E) 
a)
2.62x10-7m
b)
2.62x107m
c)
2.64x10-45m
d)
2.64x1045m
22.
A light has a wavelength of 5.06x10-7m. What is the frequency of the light? What is the color of light? (v=c/λ)
a)
16.87Hz, Red
b)
5.93Hz, Orange
c)
5.93x10-14Hz, Blue
d)
5.93x1014Hz, Green
23.
The energy for a quantum of light is 2.84x10-19J. What is the wavelength. (λ=hc/E)
a)
6.97x10-45m
b)
6.97x1045m
c)
6.97x10-7m
d)
6.97x107m
24.

Electromagnetic waves vary in

a)

the speed they travel in a vacuum.

b)

wavelength and frequency.

c)

the way they reflect.

d)

the orientation of their electric and magnetic fields.

25.

Infrared rays have a shorter wavelength than

a)

Ultraviolet ray.

b)

X-rays.

c)

radar waves.

d)

gamma rays

26.

The full range of frequencies of electromagnetic radiation is called

a)

visible light.

b)

radio waves.

c)

the electromagnetic spectrum.

d)

invisible radiation.

27.

Light in the form of a particle that has discrete amount of energy is called a

a)

Charm

b)

Photon

c)

Exciton

d)

Muon

28.

What is this element? Use a periodic table!

a)

Beryllium (atomic #4)

b)

Boron (atomic #5)

c)

Carbon (atomic #6)

d)

Nitrogen (atomic #7)

29.
What is the name of this element?
a)
Helium
b)
Hydrogen
c)
Argon
d)
Silver
30.
What is the name of this element?
a)
Lithium
b)
Boron
c)
Carbon
d)
Neon
31.

Which Bohr model represents Neon?

a)
b)
c)
d)
32.

Which model of the atom said that electrons circle the nucleus in orbits of a fixed radius?

a)

Bohr's model

b)

Thomson's plum pudding

c)

Rutherford's nuclear model

d)

Both Thomson's and Rutherford's model

33.
Absorption of energy by an electron results in 
a)
it moving from the ground to an excited state
b)
it moving from an excited to the ground state
c)
the emission of a photon
d)
it moving from an excited to the ground state and the emission of a photon
34.

The color of emitted light with the LONGEST wavelength is

a)

violet

b)

green

c)

red

d)

indigo

35.

The electron moves from position 1 to 2. How does the state of the electron shift during this reaction?

a)

The electron becomes less excited.

b)

The electron returns to the ground state.

c)

The electron becomes more excited.

d)

Light is emitted

36.

When atoms _____________ energy, their electrons move to higher energy levels. These electrons _____________ energy by emitting light when they return to lower energy levels.

a)

lose, absorb

b)

absorb, lose

c)

lose, lose

d)

absorb, absorb

37.
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.
38.
Which drawing represents the process by which an absorption line is formed?
a)
A
b)
B
c)
C
d)
D
39.
Why are line emission spectra of elements called "atomic fingerprints"?
a)
They are all the same
b)
They are all unique
c)
They are all similar
d)
They all contain colored light
40.

If an electron moves from n=4 to n=2 it ____

a)

absorbs energy

b)

releases energy

41.

Which type of spectrum is this?

a)

Emission Spectrum

b)

Absorption Spectrum

c)

Continuous Spectrum

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