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Quantum Model & E- Configuration

Total questions: 40

Worksheet time: 31mins

Name
Class
Date
1.

What is the shape of s orbitals?

a)

Dumbbell shaped

b)

Peanut shaped

c)

Spherical shaped

d)

Hybrid structure

2.
How many electrons can the first energy level hold?
a)
1
b)
2
c)
8
d)
0
3.
Electrons occupy orbitals of lowest energy first is part of what electron configuration rule?
a)
Hund’s Rule
b)
Aufbau Principle
c)
Pauli Exclusion Principle
4.
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.
5.

How many orbitals are in each sublevel?

a)

s:1 p:3 d:5 f:7

b)

s:2 p:6 d:10 f:14

c)

s:1 p:6 d:5 f:14

d)

s:2 p:3 d:10 f:7

6.

Which sublevel has the highest energy?

a)

3s

b)

3d

c)

3p

d)

1s

7.

Which main energy level is furthest from the nucleus ?

a)

1

b)

2

c)

3

d)

4

8.
What is the maximum number of orbitals on the 2nd main energy level?
a)
8
b)
9
c)
4
d)
2
9.
Which scientist developed the Quantum Mechanical
a)
E. Schroedinger
b)
W. Heisenberg
c)
J. Dalton
d)
N. Bohr
10.
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
11.
What is this element?
1s22s22p63s2
a)
Neon
b)
Magnesium
c)
Aluminum
d)
Potassium
12.
Which orbital has the least amount of energy? 
a)
p orbital
b)
d orbital
c)
s orbital 
d)
What is an orbital?
13.
An area of high probability of finding an electron 90% of the time is called a(n)
a)
nucleus
b)
sublevel
c)
orbital
d)
energy level
14.
The exponent or superscript in an electron configuration tells us
a)
the number of positions of that orbital.
b)
the distance from the nucleus or level.
c)
the number of electrons in that orbital.
d)
the number of electrons in the atom.
15.
How many valance electrons are in 1s22s22p63s2
a)
4 ve
b)
2 ve
c)
8 ve
d)
6 ve
16.
What shape are D Orbitals?
a)
Hybrid structure
b)
Spherical shaped
c)
Dumbell shaped
d)
Cloverleaf shaped
17.
The Heisenberg Uncertainty Principle states:
a)
You cannot measure the momentum and exact position of an electron at the same time
b)
electrons occupy the orbitals of lowest energy first
c)
an atomic orbital may describe at most 2 electrons
d)
No two electrons can have the same set of quantum numbers
18.

What is the correct order of the visible light spectrum starting with the longer wavelength?

a)

Red, yellow, orange, blue, violet, indigo

b)

Violet, indigo, blue, green, yellow, orange, red

c)

Green, yellow, blue, indigo, red, orange

d)

Red, orange, yellow, green, blue, indigo, violet

19.
What gases are in the unknown mixture?
a)
Gas B & Gas D
b)
Gas C & Gas B
c)
Gas A & Gas D
d)
Gas D & Gas C
20.
What waves have the lowest energy? 
a)
Gamma rays
b)
Visible light waves
c)
Radio waves
d)
X rays
21.

A wave with a large wavelength will have a ______ frequency and _____ energy

a)

high, low

b)

high, high

c)

low, high

d)

low, low

22.
The distance from one point to the next corresponding point on a wave is called the ________________.
a)
waveform
b)
peak
c)
amplitude
d)
wavelength
23.

The number of waves that pass a fixed point in a given amount of time is...

a)

frequency

b)

wave speed

c)

amplitude

d)

wavelength

24.

When an electron returns to ground state from an excited state, the atom will

a)

emit energy

b)

absorb energy

c)

rotate

d)

wiggle

25.

In order to go from ground state to an excited state, an electron must

a)

emit energy

b)

absorb energy

c)

rotate

d)

wiggle

26.

Ground state means that an electron is...

a)

at its lowest possible potential energy

b)

in the first shell of an atom

c)

laying low for the weekend

d)

removed from an atom

27.
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
28.

What is incorrect about this orbital diagram?

a)

Both arrows in the 2p box should be pointing up : Pauli Exclusion

b)

There is nothing incorrect with this diagram

c)

In the 2p sublevel, there should only be 1 electron in the first orbital and one in the second orbital : Hund's Rule

d)

All the arrows should be pointing up.

29.
Which element is pictured?
a)
neon
b)
fluorine
c)
magnesium
d)
argon
30.

This shape is that of a...

a)

s orbital

b)

d orbital

c)

p orbital

d)

f orbital

31.

How many orbitals are available to hold electrons in the 6th energy level (n=6)?

a)

9

b)

16

c)

26

d)

36

32.
According to the Aufbau Principle, which sublevel should starting filling with electrons after 5s?
a)
6s
b)
5p
c)
4d
d)
3f
33.
The second energy level (n=2) contains a total of 5 electrons...how many more electrons can fit in the 2nd energy level?
a)
0
b)
3
c)
5
d)
7
34.
Which of the following statements is true about the 3s and the 4s sublevels?
a)
These sublevels have the same energy
b)
These sublevels are the same distance from the nucleus
c)
These sublevels hold different amounts of electrons
d)
These sublevels have the same shape
35.

The number of possible different orbital shapes for the second energy level is

a)

1

b)

2

c)

3

d)

4

36.

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

37.

An orbital that can never exist according to the quantum description of the atom is

a)

3f

b)

6d

c)

3d

d)

8s

38.

The letter designations for the first four sublevels with the maximum number of electrons that can be accommodated in each sublevel are

a)

s:1, p:2, d:3, and f:4.

b)

s:1, p:3, d:5, and f:7.

c)

s:2, p:4, d:6, and f:8.

d)

s:2, p:6, d:10, and f:14.

39.

If n is the principal quantum number of a main energy level, the number of electrons in that energy level is

a)

n2

b)

2n

c)

n

d)

2n2

40.
What is this element?
1s22s22p63s23p64s23d10
a)
Zinc
b)
Copper
c)
Nickel
d)
Germanium

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