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Light and Atomic Structure Review

Total questions: 42

Worksheet time: 42mins

Name
Class
Date
1.
For an electron to change from ground state to an excited stated it must...
a)
Absorb energy
b)
Release energy
2.

True or False: The ground state is the highest energy state of an atom.

a)

True

b)

False

3.

What is the light that you can see called?

a)

observatory light

b)

ultraviolet light

c)

visible light

d)

infrared light

4.

Which of the following is FALSE about electromagnetic spectrum?

a)

EM waves travel at the speed of light

b)

Long wavelengths of light have low frequencies

c)

High energy photon have long wavelength

5.

Diagram below shows

a)

Emission spectrum

b)

Absorption spectrum

c)

Line absorption spectrum

6.
When talking about energy levels in an atom, what is an "excited state"?
a)
The highest energy state of an atom.
b)
Any level higher than the ground state.
c)
The lowest energy state of an atom.
d)
When an atom loses an electron
7.
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
8.

A line spectrum is produced when an electron moves from one energy level

a)

into the nucleus

b)

to a higher energy level

c)

to another position in the same sublevel

d)

to a lower energy level

9.

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

a)

absorbs energy

b)

releases energy

10.

Emission spectra emitted by an element (or compound) will produce ___ through a spectroscope.

a)

bright lines

b)

a continuous rainbow

c)

dark lines

d)

white light

11.
What is the unknown spectra?
a)
beryllium
b)
copper
c)
manganese
d)
strontium
12.
Which elements are in the unknown sample?
a)
A and B
b)
B and C
c)
A and D
d)
B and D
13.
The blue section of the wave is measuring _________________.
a)
wavelength
b)
crest
c)
trough
d)
amplitude 
14.
What element has the following electron configuration? [Ar] 3d104s24p3
a)
As
b)
P
c)
Se
d)
Ga
15.

1. What is the shape of an s orbital?

a)

sphere

b)

peanut

c)

double peanut

d)

TOO COMPLEX TO KNOW IT.

16.
How many electrons can each p orbital hold?
a)
6
b)
3
c)
2
d)
4
17.
How many orbitals are in the f sublevel
a)
1
b)
3
c)
5
d)
7
18.
What is the correct electron configuration for Selenium
a)
1s22s22p63s23p64s24d104p4
b)
1s22s22p63s23p64s23d104p4
c)
1s22s22p63s23p64s23d104p3
d)
1s22s22p63s23p64s24d104p43
19.
Which is a particle of electromagnetic radiation with no mass that carries a quantum of energy?
a)
electron 
b)
neutron 
c)
microwave
d)
photon 
20.
Which model describes electrons as orbiting around a central nucleus?
a)
Bohr
b)
Rutherford
c)
Quantum Mechanical 
d)
Plum Pudding 
21.
What atom matches this electron configuration?
[Xe] 6s2 4f14 5d9
a)
Mercury
b)
Gold
c)
Platinum
d)
Thallium
22.
What is the maximum number of electrons that an orbital can have?
a)
1 electron
b)
2 electrons
c)
3 electrons
d)
4 electrons
23.
Bromine is found in which block?
a)
s
b)
p
c)
d
d)
f
24.

Which electron transition releases a photon with the greatest energy?

a)

n = 6 to n = 3

b)

n = 5 to n = 3

c)

n = 4 to n = 3

d)

n = 7 to n = 3

25.

Name the element- 1s2 2s2 2p6 3s2 3p6 4s2 3d5

a)

Manganese

b)

Magnesium

c)

Aluminum

d)

Boron

26.

Which "rule" explains why the two electrons in an orbital have opposite spin?

a)

Pauli Exclusion Principle

b)

Hund's Rule

c)

Heisenberg Uncertainty Principle

d)

Bohr's Rule

27.

How many valence electrons are in an atom of zinc?

a)

2

b)

10

c)

12

d)

8

28.

Which color has the shortest wavelength?

a)

Red

b)

Blue

c)

Yellow

d)

Violet

29.

What ground state element has this electron configuration? 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p1

a)

Gallium

b)

Indium

c)

Aluminum

d)

Germanium

30.

How many orbitals are there in the "d" sublevel?

a)

1

b)

3

c)

5

d)

7

31.

Which is the electron configuration for an oxygen atom?

a)

1s22s22p63s23p64s2

b)

1s22s22p4

c)

1s22s22p6

d)

1s22s22p63s23p6

32.
Hund’s rule states…
a)
Atomic orbitals have opposite spins and 2 electrons each
b)
Electrons occupy orbitals of highest energy first and energy level changes as you go up
c)
Electrons occupy orbitals of lowest energy first, starting with 1s
d)
Electrons occupy orbitals of equal energy, one electron enters EACH orbital ONE AT A TIME until orbitals of the entire energy level have one electron with the SAME SPIN.
33.
The Quantum Mechanical Model is the most recent/modern atomic model.
a)
True
b)
False
34.
What is the Pauli Exclusion Principle?
a)
An atomic orbital can only hold a maximum of 2 electrons, each with opposite spins
b)
An atomic orbital can hold a minimum of 6 electrons, each with opposite spins
c)
An atomic orbital can hold a maximum of 6 electrons, each with the same spin
d)
An atomic orbital can hold a minimum of 2 electrons, each with opposite spins
35.

JJ Thomson discovered what subatomic particle

a)

nucleus

b)

neutron

c)

proton

d)

electron

36.

First person to propose the concept of an atom

a)

Rutherford

b)

Democritus

c)

Dalton

d)

Bohr

37.

Thomson Experimented with ______

a)

Gold Foil

b)

alpha particles

c)

cathode rays

d)

protons

38.

Which model of the atom describes the location of electrons as probable within a dense "cloud" surrounding the nucleus of an atom?

a)

The Billiard Ball Model

b)

The Plum Pudding Model

c)

The Planetary Model

d)

The Quantum Mechanical Model

e)

The Nuclear Model

39.

The difference between 1s and 2s is ...

a)

the size of the sublevel

b)

the number of orbitals in each sublevel

c)

max amount of electrons the sublevel can hold

d)

ability of the electrons to make light

40.
True or false: as you move along the spectrum, radio to gamma waves, the wavelengths decrease in size (get smaller)
a)
true
b)
false
41.
Select the correct order of waves on the EMS from the longest wavelength to the shortest wavelength
a)
Radio, Micro, Infra, Visible, Ultra, X-ray, Gamma
b)
Gamma, X-ray, Ultra, Vis, Infra, Micro, Radio
c)
Vis, Micro, Infra, Ultra, X-ray, Gamma, Radio
d)
Micro, Radio, Vis, Infra, Ultra, X-ray, Gamma
42.
How much of the electromagnetic spectrum is visible?
a)
All of it
b)
None of it
c)
Most of it
d)
Only a small part

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