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Unit 4 Review - Electrons

Total questions: 51

Worksheet time: 1hrs 2mins

Name
Class
Date
1.
According to _______, an electron occupies the lowest-energy orbital that can receive it.
a)
the Aufbau principle
b)
the Pauli exclusion principle
c)
Hund's rule
d)
Conservation of Energy
2.
What's the electron configuration for vanadium?
a)
1s22s22p63s23p64s23d3
b)
1s22s22p63s23p63d5
c)
1s22s22p63p64s24p3
3.

What's the electron configuration for Neon (Ne)?

a)

1s22s22p6

b)

1s22s22p23s23p2

c)

1s10

d)

n=10

4.
The first orbital can hold a maximum of how many electrons?
a)
2
b)
3
c)
8
d)
6
5.
There are 4 different types of subshells s,p,d,f
a)
true
b)
false
6.
How many valence electrons are represented here?
a)
7
b)
5
c)
2
d)
8
7.
What is the shorthand electron configuration for Sulfur atom?
a)
[Ar] 3p4
b)
[He] 3s23p4
c)
[Ne] 3s23p4
d)
[Na] 3s23p3
8.
What noble gas should be used to write the shorthand configuration for Te?
a)
Ar
b)
Kr
c)
Xe
d)
Sb
9.
Which of the following is a p block element?
a)
Ca
b)
Ar
c)
Re
d)
Au
10.

What is the state when electrons move to a higher energy level upon absorption of energy?

a)

active

b)

inactive

c)

excited

d)

ground

11.

What particles in the heated compounds are responsible for the production of the colored light?

a)

proton

b)

neutron

c)

electron

d)

proton and neutron

12.
How many electrons should Flourine have around its Lewis dot model?
a)
5
b)
6
c)
7
d)
8
13.
How many electrons should Magnesium have around its Lewis dot model?
a)
1
b)
2
c)
3
d)
4
14.
How many electrons should Chlorine have around its Lewis dot model?
a)
5
b)
6
c)
7
d)
8
15.
Why are ions formed?
a)
To make our lives difficult
b)
Because atoms want 8 valence electrons
c)
Because atoms have the same number of protons and electrons
d)
Because atoms gained neutrons
16.
Cations are...
a)
Positive
b)
Negative
c)
Neutral
d)
Purring
17.
Anions are...
a)
Positive
b)
Negative
c)
Neutral
d)
Crying
18.
An atom becomes _________ when it gains electrons.
a)
Positive
b)
Negative
c)
Neutral
d)
Invinsible
19.
An atom becomes _______ when it loses electrons.
a)
Positive
b)
Negative
c)
Neutral
d)
Invinsible
20.
A Radium atom wants...
a)
One more electron
b)
One less electron
c)
Two more electrons
d)
Two less electrons
21.
Make sure you get enough Potassium in your diet!
a)
Huh?
b)
K
c)
I <3 bananas
d)
Sure
22.
Valence electrons are: 
a)
Electrons farthest away from the nucleus
b)
Electrons closest to the nucleus
c)
Electrons that just come and go - they don't stay with the atom
23.
What charge will an Oxygen ion have? 
a)
+1
b)
-1
c)
+2
d)
-2
24.
If an element has 3 valence electrons, what charge will likely form on its ion ?
a)
+3
b)
+5
c)
-3
d)
-5
25.
Which of the following has a -3 charge?
a)
Boron
b)
Fluorine
c)
Nitrogen
d)
Neon
26.
How many electrons can the 3rd energy level hold?
a)
2
b)
8
c)
16
d)
18
27.
What does the following ion mean
              Na +1
a)
sodium gains an electron
b)
sodium loses an electron
c)
sodium gains a proton
d)
sodium loses a proton
28.
What does the following ion mean 
                      S-2
a)
sulfur gains 2 electrons
b)
sulfur loses 2 electrons
c)
sulfur gains 2 protons
d)
sulfur loses 2 protons
29.

The maximum number of electrons that can fit into the 2nd energy level is

a)

2

b)

8

c)

18

d)

32

30.

An atom has electrons in the 1s orbital which is closest to the nucleus. The same atom also has electrons in the 2s orbital. Which electrons are higher energy?

a)

1s

b)

2s

31.

How many energy levels does Calcium have? Hint - it has to do with what period Ca is in.

a)

1

b)

2

c)

3

d)

4

32.

What is the maximum number of energy levels an atom can have?

a)

1

b)

7

c)

5

d)

3

33.

What does the 2 in sublevel 1s2 represent?

a)

The number of electrons in the suborbital

b)

The shape of the suborbital

c)

The number of neutrons in the suborbital

d)

The energy level of the electrons.

34.

What does the 1 in sublevel 1s2 represent?

a)

The number of electrons in the suborbital

b)

The shape of the suborbital

c)

The number of neutrons in the suborbital

d)

The energy level of the electrons.

35.

Which element is this? 1s22s22p63s23p64s23d104p65s24d105p6

a)

Fr

b)

U

c)

Xe

d)

Lr

36.

Which element is this? 1s22s22p63s23p2

a)

Fr

b)

Si

c)

Xe

d)

Ca

37.

What is the correct electron configuration of Carbon?

a)

1s22s22p2

b)

1s22s22p63s23p5

c)

1s22s2

d)

1s22s22p6

38.
What is the noble gas shorthand electron for Sulfur atom?
a)
[Ar] 3p4
b)
[He] 3s23p4
c)
[Ne] 3s23p4
d)
[Na] 3s23p4
39.
How many electron can be found in a s orbital?
a)
2
b)
3
c)
4
d)
1
40.
How many electron can be found in a p orbital?
a)
2
b)
3
c)
4
d)
6
41.
Family 3A
a)
has 3 valence electrons
b)
+3 oxidation number
c)
loses 3 electrons
d)
all of these
42.
The oxidation for sulfur is
a)
+2
b)
-2
c)
+6
d)
-6
43.

The only family that can be cations or anions (hint: "skip")

a)

Transitions

b)

1A

c)

4A

d)

8A

44.

What is the charge of an ion with 17 protons, 16 neutrons, and 18 electrons?

a)

0

b)

+1

c)

-1

d)

+9

45.

The change of an atom from an excited state to the ground state always requires

a)

release of energy

b)

absorption of energy

c)

release of an electron

d)

absorption of green light

46.
In a stable atom, the atomic number is equal to...
a)
neutrons
b)
electrons
c)
atomic mass
d)
what is a stable atom?
47.
What is this element?
1s22s22p63s2
a)
Neon
b)
Magnesium
c)
Aluminum
d)
Potassium
48.
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
49.
Valence electrons are the...
a)
Innermost electrons
b)
Middle electrons
c)
Outermost electrons
d)
Any electrons
50.

USE THE PERIODIC TABLE

How many valence electrons does carbon have?

a)

4

b)

12

c)

6

d)

14

51.

USE THE PERIODIC TABLE

How many valence electrons does sodium have?

a)

1

b)

2

c)

3

d)

4

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