WorksheetsCP Unit 5 Review (Electron Configuration)
Total questions: 20
Worksheet time: 31mins
Name
Class
Date
1.
What atom matches this electron configuration?
1s2 2s2 2p6 3s2
1s2 2s2 2p6 3s2
a)
Neon
b)
Magnesium
c)
Aluminum
d)
Potassium
2.
How many electrons can the first energy level hold?
a)
1
b)
2
c)
8
d)
0
3.
How many valence electrons does Chlorine have?
a)
5
b)
2
c)
7
d)
5
4.
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
5.
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
6.
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
7.
Which electron configuration belongs to Chlorine (Cl)?
a)
1s2 2s2 2p6 3s2 3p5
b)
1s2 2s2 2p6 3s2 3p6
c)
1s2 2s2 2p6 3s2 3p7
8.
Which of the following is a p block element?
a)
Ca
b)
Ar
c)
Re
d)
Au
9.
How many electron can be found in a p orbital?
a)
2
b)
3
c)
4
d)
6
10.
The electron configuration of an atom is 1s22s22p6. The number of electrons in the atom is
a)
3
b)
6
c)
8
d)
10
11.
How many atomic orbitals are there in the p sublevel?
a)
2
b)
3
c)
4
d)
5
12.
Is the following electron configuration correct? Why or why not?
1s22s22p63s23p64s24d104p65s1
a)
No. 4p6 should be after 5s1.
b)
No. It should be 3d10 not 4d10
c)
Yes. All electrons are represented properly.
d)
Yes.
13.
Electron arrangement that uses arrows
a)
Electron configuration
b)
Shorthand configuration
c)
Lewis dot structure
d)
Orbital diagram
14.
1. What is the shape of an s orbital?
a)
sphere
b)
dumbbell
c)
double dumbbell
d)
TOO COMPLEX TO KNOW IT.
15.
This orbital diagram represents:
a)
Carbon
b)
Boron
c)
Nitrogen
d)
Oxygen
16.
What is incorrect about this orbital diagram?
a)
Both arrows in the 2p box should be pointing up
b)
There are too many electrons in the 1s orbital
c)
In the 2p boxes, there should only be 1 electron in the first 2p box and one in the 2nd 2p box
d)
All the arrows should be pointing up
17.
In an orbital diagram, an arrow represents:
a)
an electron
b)
an orbital
c)
an element
18.
What do the coefficients represent in this diagram?
a)
electrons
b)
Sublevels
c)
Orbitals
d)
energy levels
19.
Which rule is violated in the following orbital diagrams?
a)
Aufbau Principle
b)
Hund's Rule
c)
Pauli's Exclusion Principle
20.
How many unpaired electrons would lithium have?
a)
1
b)
2
c)
3
d)
0
100 %
