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Electron configuration

Total questions: 52

Worksheet time: 2hrs 34mins

Name
Class
Date
1.
What atom matches this electron configuration?
1s2 2s2 2p6 3s2
a)
Neon
b)
Magnesium
c)
Aluminum
d)
Potassium
2.
Which is the electron configuration for an oxygen atom?
a)
1s22s22p63s23p64s2
b)
1s22s22p4
c)
1s22s22p6
d)
1s22s22p63s23p6
3.
What is the maximum number of electrons that an orbital can have?
a)
1 electron
b)
2 electrons
c)
3 electrons
d)
4 electrons
4.
How many valence electrons are represented here?
a)
7
b)
5
c)
2
d)
8
5.
How many d orbitals are there in a given sublevel?
a)
1
b)
3
c)
5
d)
7
6.
How many p orbitals are there in a sublevel?
a)
2
b)
1
c)
4
d)
3
7.
How many electrons can the d sublevel hold?
a)
8
b)
10
c)
2
d)
4
8.
What is this element? 
1s22s22p63s23p6
4s23d104p6
a)
Argon
b)
Krypton
c)
Selenium
d)
Bromide
9.
What atom matches this electron configuration?
[Xe] 6s2 4f14 5d9
a)
Mercury
b)
Gold
c)
Platinum
d)
Thallium
10.
What is the shorthand electron configuration for Sulfur atom?
a)
[Ar] 3p4
b)
[He] 3s23p4
c)
[Ne] 3s23p4
d)
[Na] 3s23p3
11.
How many electrons can the first energy level hold?
a)
1
b)
2
c)
8
d)
0
12.
Identify the element in Period 5 that has 1 valence electron?
a)
Rb
b)
Nb
c)
Ag
d)
Sb
13.
What do you start electron configuration with?
a)
1s2
b)
1d10
c)
1f14
d)
1p6
14.
There are 4 different types of subshells s,p,d,f
a)
true
b)
false
15.
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
16.
What does Pauli exclusion principle state ?
a)
states that each electron occupies the lowest energy orbital available
b)
states that a maximum of two electrons can occupy a single atomic orbital, but if only if the electros have opposite spins
c)
states that single electrons electrons with the same spin must occupy each-energy orbital before additional electrons with opposite spins can occupy the same orbitals
17.
What does Hund's rule states ?
a)
states that single electrons electrons with the same spin must occupy each-energy orbital before additional electrons with opposite spins can occupy the same orbitals
b)
states that each electron occupies the lowest energy orbital available
c)
states that a maximum of two electrons can occupy a single atomic orbital, but if only if the electros have opposite spins
18.
How many electron can be found in a s orbital?
a)
2
b)
3
c)
4
d)
1
19.
How many electron can be found in a p orbital?
a)
2
b)
3
c)
4
d)
6
20.
What atom matches this electron configuration?
1s22s22p63s23p64s23d10
a)
Zinc
b)
Copper
c)
Nickel
d)
Germanium
21.

Which area on the periodic table represents the electrons in the "d" sublevel?

a)

representative elements

b)

columns 3-8

c)

rare earth elements

d)

transition elements

22.

Each row on the periodic table represents:

a)

an energy level

b)

a sublevel

c)

an electron

d)

an orbital

23.
What's a valence electron?
a)
electrons in the second energy level
b)
electrons in the outermost energy level
c)
the atomic number
d)
electrons in the first level
24.
How many electrons are in the outer shell of Sodium (Na)?
a)
3
b)
1
c)
2
d)
4
25.
Electron arrangement that uses arrows
a)
Electron configuration
b)
Shorthand configuration
c)
Lewis dot structure
d)
Orbital diagram
26.

What are the shapes of p orbitals ?

a)

cloverleaf

b)

spherical

c)

dumbbell

27.

How many 4d orbitals are there in an atom?

a)

1

b)

3

c)

5

28.
Which of the waves shown below has the higher frequency?
a)
wave A
b)
Wave B
29.
True or False: Electrons are considered stable at their ground state.
a)
TRUE
b)
FALSE
30.
For an electron to change from ground state to an excited state it must...
a)
Absorb energy
b)
Release energy
31.

What is the shape of the d orbital?

a)

flat

b)

sphere

c)

dumbbell

d)

clover

32.

Light is emitted when an electron moves from the ________ state to the _________ state.

a)

excited, ground

b)

ground, excited

33.

Which color has the least amount of energy?

a)

Red

b)

Orange

c)

Green

d)

Blue

34.

This shape is that of a...

a)

s orbital

b)

d orbital

c)

p orbital

d)

f orbital

35.

This is a ____ orbital

a)

s

b)

d

c)

p

d)

d

36.

The principle quantum number, n, represents the:

a)

spin value

b)

suborbital value

c)

energy level

d)

magnetic value

37.

Orbital sublevels, or L, represents:

a)

orbital color

b)

orbital shape

c)

electron spin

d)

energy level

38.

How many electrons total are found in the f orbital?

a)

2

b)

6

c)

10

d)

14

39.
Which type of orbital is shaped like a sphere?
a)
s orbital
b)
p orbital
c)
d orbital
d)
f orbital
40.

Correctly pair the orbital with its "block" location

a)

s orbital, "gold" block

b)

p orbital, red block

c)

d orbital, darker green/brown block

d)

f orbital, blue block

41.

Which is shape is correctly paired with its sublevel

a)

sphere = d

b)

flower = s

c)

infinity or dumbbell = p

d)

clover = f

42.

What does the 1 in "1s" stand for?

a)

energy level

b)

s orbitals

c)

p orbitals

d)

the number of electrons

43.

Which of the following elements will be found in the. "p" block?

a)

sulfur

b)

sodium

c)

titanium

d)

plutonium

e)

copper

44.

Which quantum number tells you the shape of the orbitals?

a)

principal

b)

spin

c)

magnetic

d)

azimuthal/angular momentum

45.

Which quantum number shows the direction in which the electrons are traveling?

a)

spin

b)

magnetic

c)

angular mometnum

d)

principal

46.

Which quantum number shows the orientation of an electron's orbit on the "x", "y", "z" axis?

a)

spin

b)

magnetic

c)

angular momentum

d)

principal

47.

What is the name of the element whose electron configuration is 1s22s22p3?

a)

magnesium

b)

nitrogen

c)

carbon

d)

phosphorous

48.
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
49.
How can you tell how many energy levels an atom has? 
a)
APE MAN
b)
By the Group
c)
By the Period
d)
By the atomic mass
50.

Light acts like

a)

a wave.

b)

a particle.

c)

Both a wave and a particle

d)

neither a wave nor a particle.

51.

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

a)

Charm

b)

Photon

c)

Exciton

d)

Muon

52.

Which of the following is TRUE about the frequency and energy in electromagnetic waves?

a)

As the frequency of an EM wave increases, the energy also increases.

b)

As the frequency of an EM wave increases, the energy decreases.

c)

The Planck's constant increases when the frequency and energy of an EM wave increase.

d)

There is no relation between the energy and the frequency of an EM wave.

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