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Unit 1 Atomic Structure & Light Review

Total questions: 65

Worksheet time: 3hrs 10mins

Name
Class
Date
1.

The nucleus of an atom contains which subatomic particles?

a)

protons and electrons

b)

protons and neutrons

c)

electrons and neutrons

d)

protons, electrons, and neutrons

2.

Which subatomic particle is counted to determine the type of element the atom represents?

a)

proton

b)

neutron

c)

electron

d)

boron

3.
Particles in an atom that are neutral and have no charge are 
a)
negatrons 
b)
electrons 
c)
neutrons 
d)
protons 
4.
Adding or subtracting neutrons (charge = 0, mass = 1) makes the element change into an...
a)
ion
b)
mixture
c)
isotope
d)
neutral atom
5.
The atomic mass is equal to _.
a)
the number of protons only
b)
the number of neutrons only
c)
the total number of protons and neutrons
d)
the number of protons, neutrons, and electrons.
6.
An atom becomes _________ when it gains electrons.
a)
Positive
b)
Negative
c)
Neutral
d)
Invinsible
7.
An atom that has gained or lost electrons is called ...
a)
a winner
b)
an isotope
c)
an ion
d)
a loser
8.

When an atom loses an electron, it becomes a

a)

positive ion

b)

negative ion

c)

neutral ion

d)

neutral atom

9.

What property determines if an atom is identified as Flourine?

a)

it has 10 neutrons

b)

it has an atomic mass of 19

c)

it has 9 protons

d)

Its element symbol is Fl.

10.

Which element is shown in the Bohr model?

a)

Helium because it has 2 valence electrons

b)

Magnesium because it has an atomic number of 12.

c)

Chromium because is has an atomic mass of 24.

d)

Argon because it has 18 total subatomic particles.

11.

An element has 5 protons, 6 neutrons, and 5 electrons. What is the mass number?

a)

5

b)

10

c)

11

d)

16

12.

An element has 5 protons, 6 neutrons, and 7 electrons. What is the charge of the atom?

a)

+2

b)

-1

c)

+1

d)

-2

13.

How many protons are in an average Chlorine atom?

a)

17

b)

35

c)

35.45

d)

18

14.

How many electrons are in an average Chlorine atom?

a)

17

b)

35

c)

35.45

d)

18

15.
How many electrons does a Copper atom have?
a)
63
b)
29
c)
92
d)
34
16.
What is the atomic number for an element with 41 neutrons and a mass number of 80?
a)
39
b)
41
c)
80
d)
121
17.
How many neutrons does this isotope of lithium have?
a)
8
b)
3
c)
4
d)
5
18.

A sodium atom with a +1 charge has 11 protons and ____ electrons.

a)

12

b)

23

c)

10

d)

11

19.

Isotopes of an element have a different number of...

a)

Protons

b)

Neutrons

c)

Electrons

d)

Mass

20.

Potassium-39 has how many neutrons?

a)

19

b)

18

c)

20

d)

21

21.
The formation of elements is known as _________.
a)
nucleotides
b)
Synthogenesis
c)
nuclear fission
d)
nucleosynthesis
22.
The two elements formed in Big Bang Nucleosynthesis where __________________.
a)
hydrogen and lithium
b)
hydrogen and helium
c)
hydrogen and oxygen
d)
helium and lithium
23.
________ nucleosynthesis happens in the center of stars and is where the elements helium through iron (Fe) are formed. 
a)
Big Bang
b)
Stellar
c)
Supernova
d)
Superdupernova
24.
All elements bigger than iron on the periodic table are formed in _________________.
a)
Big Bang Nucleosynthesis
b)
Stellar Nucleosynthesis
c)
Supernova Nucleosynthesis
d)
Genonucleosynthesis
25.
What can a scientist learn about a star from its spectrum
a)
its color
b)
its size
c)
its composition and temperature
d)
its age
26.

What does the electromagnetic spectrum show?

a)

The composition of stars only

b)

The different types of sound waves

c)

All forms of electromagnetic radiation in the order of increasing or decreasing wavelength

d)

Only the visible light spectrum

27.

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.

28.
Which elements are in the unknown sample?
a)
A and B
b)
B and C
c)
A and D
d)
B and D
29.

What does the picture below illustrate?

a)

Visible Light Spectrum

b)

Electromagnetic Spectrum

c)

Frequency Indicator

d)

Color Line

30.

Of the visible spectrum, what color has the longest wavelength?

a)

Blue

b)

Green

c)

Yellow

d)

Red

e)

Violet

31.

What color has the shortest wavelength and highest frequency?

a)

Violet

b)

Orange

c)

Red

d)

Blue

32.

Which color has the longest wavelength?

a)

Yellow

b)

Red

c)

Green

d)

Purple

33.
As the frequency of an electromagnetic wave increases, the amount of energy in that wave...
a)
increases.
b)
decreases.
c)
stays the same.
34.
Which has the SHORTEST wavelength and, therefore, the highest frequency/most energy
a)
Radio waves
b)
Ultraviolet Rays
c)
Gamma Rays
d)
X-rays
35.
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
36.

What is an atomic electron transition?

a)

A change in the number of protons in an atom

b)

A change in the number of neutrons in an atom

c)

A change in the number of electrons in an atom

d)

A change of an electron from one energy level to another within an atom

37.

What happens during absorption in electron transitions?

a)

An electron emits energy and jumps to the next orbital

b)

An electron absorbs energy and jumps to the next orbital

c)

An electron emits energy and returns to its regular resting state

d)

An electron absorbs energy and returns to its regular resting state

38.

What determines the frequency and color of the emitted light during electron transitions?

a)

The number of protons in the atom

b)

The number of neutrons in the atom

c)

The energy level of the electron

d)

The speed of the electron

39.

Which image shows the lower energy light released?

a)

b)

40.

In which state does an electron have the least amount of energy?

a)

Excited state

b)

Ground state

c)

Orbital

d)

Bohr model

41.

What evidence led Niels Bohr to believe that electrons occupy specific energy levels in atoms?

a)

Excited electrons emit colored light at every possible wavelength.

b)

Excited electrons emit colored light at only certain wavelengths.

c)

Electrons emit colored light only when in an excited state.

d)

Electrons emit colored light only when in ground state.

42.

Which principal energy level change by the electron of a

hydrogen atom will cause the greatest amount of energy to be absorbed?

a)

n = 2 to n = 4

b)

n = 2 to n = 5

c)

n = 4 to n = 2

d)

n = 5 to n = 2

43.
Light is emitted when an electron moves from the ________ state to the _________ state
a)
excited, ground
b)
ground, excited
44.
Every element has its own unique atomic spectra.
a)
True
b)
False
45.
The electron configuration of an atom is 1s22s22p6.  The number of electrons in the atom is 
a)
3
b)
6
c)
8
d)
10
46.
What atom matches this electron configuration?
1s22s22p63s23p64s23d10
a)
Zinc
b)
Copper
c)
Nickel
d)
Germanium
47.
What is the noble gas shorthand electron for Sulfur atom?
a)
[Ar] 3p4
b)
[He] 3s23p4
c)
[Ne] 3s23p4
d)
[Na] 3s23p4
48.
How many electrons can the first energy level hold?
a)
1
b)
2
c)
8
d)
0
49.

An electron transitions from n = 6 to n = 3. Which wavelength is released?

a)

410 nm

b)

1875 nm

c)

1282 nm

d)

1094 nm

50.

Oxygen is perhaps the most important atom on Earth. Which of the following electronic transitions in the oxygen atom will result in light emission?

a)

n=1→n=2n=1\rightarrow n=2  

b)

n=1→n=3n=1\rightarrow n=3  

c)

n=3→n=2n=3\rightarrow n=2  

d)

n=2→n=3n=2\rightarrow n=3  

51.

Which carries the highest energy?

a)
b)
c)
52.
Which electron configuration belongs to Copper (Cu)?
a)
1s2 2s2 2p6 3s2 3p6 4s2 3d8
b)
1s2 2s2 2p6 3s2 3p6 4s2 3d9
c)
1s2 2s2 2p6 3s2 3p6 4s2 3d10
53.
How many valence electrons does Chlorine have?
a)
5
b)
2
c)
7
d)
5
54.
How many valence electrons are represented here?
a)
7
b)
5
c)
2
d)
8
55.
Identify the Electron Configuration for Aluminum (Al)
a)
1s2 2s2 2p6 3s2 3p1
b)
1s2 2s2 2p6 3s2 3p3
c)
1s2 2s2 2p6 3s2 4p1
56.

Calculate the wavelength of the yellow light emitted by the street light, if the frequency of the radiation is 5.10x1014Hz.

a)

5.12 x 10-7m

b)

5.88 x 10-7 m

c)

4.20 x 1014m

d)

3.0 x 108m

57.

Energy is measured in........

a)

Wavelength

b)

Meters

c)

Joules

d)

Frequency

58.

The symbol for wavelength Is?

a)

nu

b)

lambda

c)

vi

d)

meters

59.

What is the frequency of light with a wavelength of

4.8 x 10-7 meters?

a)

5.34 x 10-9 Hz

b)

3.0 x 108 Hz

c)

3.21 x 1017 Hz

d)

6.25 x 1014 Hz

60.

The unit of measure for frequency is?

a)

Seconds

b)

Meters

c)

Hertz

d)

Liters

61.

The symbol for a frequency of a wave is?

a)

Hertz

b)

v

c)

lambda

d)

meters/second

62.

What does "h" stand for?

a)

Speed of Light

b)

Plank's Constant

c)

Speed of Sound

d)

Constant Energy

63.

What is the energy of a quantum of light with a frequency of 7.39x1014Hz.(E=Hv)

a)

4.88x1019 J

b)

4.88x10-19 J

c)

2.22x1023 J

d)

2.22x10-23 J

64.

A certain photon of light has a wavelength of 4.22x10-7nm. What is the frequency?

a)

7.11x1014 Hz

b)

7.11Hz

c)

1.41x10-15 Hz

d)

-1.41x1015 Hz

65.
Which color has the longest wavelength?
a)
Orange
b)
Green
c)
Blue
d)
Indigo

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