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Unit 4 Chemistry Review

Total questions: 43

Worksheet time: 2hrs 9mins

Name
Class
Date
1.
What atom matches this electron configuration?
1s22s22p63s2
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.
What is the electron configuration for nitrogen?
a)
1s2 2s2 2p3
b)
1s2 2s3 2p2
c)
1s2 2s3 2p1
d)
1s2 2s2 2p2 3s1
4.
The distance traveled between two successive peaks of a waves is the
a)
speed
b)
frequency
c)
wavelength
d)
energy
5.
If electrons in an atom have the lowest possible energies, the atom is in the
a)
ground state.
b)
inert state.
c)
excited state.
d)
radiation-emitting state.
6.

What element has this electron configuration?

a)

hydrogen

b)

helium

c)

lithium

d)

beryllium

7.

What element has this orbital notation?

a)

lithium

b)

beryllium

c)

boron

d)

carbon

8.

What element has this electron configuration?

a)

boron

b)

carbon

c)

nitrogen

d)

oxygen

9.

Which element is represented by this orbital notation?

a)

carbon

b)

nitrogen

c)

oxygen

d)

fluorine

10.
All orbitals of equal energy are occupied by one electron before any single orbital is occupied by a second electron.
a)
Aufbau principle
b)
Pauli exclusion principle
c)
Hund’s rule
d)
Core Notation
11.
Electrons are paired based on their spin directions, clockwise and counterclockwise, is what electron configuration rule?
a)
Hund’s Rule
b)
Aufbau Principle
c)
Pauli Exclusion Principle
12.

Which is not an orbital

a)

S

b)

P

c)

K

d)

F

13.

The shape of S orbital is

a)

Sphere

b)

Dumbell

c)

oval

d)

there is no certain shape

14.

The "d" sublevel can hold a maximum of ________ electrons.

a)

2

b)

5

c)

6

d)

10

e)

14

15.

What is a quanta?

a)

a French soda

b)

a packet of energy or light

c)

an area where an electron may be found 90% of the time

d)

a description of the atom in its ground state

16.

3.0x108 ms3.0x10^8\ \frac{m}{s}  is

a)

Planck's constant

b)

the number of complete wave cycles per second

c)

the speed of light

d)

an excited state

17.

6.62x10−34 J s6.62x10^{-34}\ J\ s  is

a)

Planck's constant

b)

total valence electrons in the whole periodic table

c)

the speed of light

d)

principal energy level

18.

Frequency is measured in

a)

m/s

b)

J

c)

Hz

d)

cubic meters

19.

An electron is in a(n) ______________ when it is in the lowest principal energy level possible.

a)

excited state

b)

orbital

c)

ground state

d)

sublevel

20.

An electron is in a(n) _____________ when it has absorbed energy and jumped to a higher principal energy level than is typical.

a)

excited state

b)

s-orbital

c)

ground state

d)

unpaired

21.

________ principal energy levels are closer to the nucleus while __________ principal energy levels are farther away from the nucleus.

a)

Lower, higher

b)

Higher, lower

22.

The shape of S orbital is

a)

Sphere

b)

Dumbell

c)

oval

d)

there is no certain shape

23.

What orbital is this an image of?

a)

s

b)

p

c)

d

d)

f

24.

How many valence electrons does Hydrogen have?

a)

1

b)

2

c)

3

d)

4

e)

5

25.

How many valence electrons does Helium have?

a)

1

b)

2

c)

3

d)

4

e)

5

26.

How many valence electrons does Lithium have?

a)

1

b)

2

c)

3

d)

4

e)

5

27.

The electrons in the highest principal energy level in an atom are known as

a)

unpaired

b)

valence

c)

snooty

d)

f-orbitals

28.

Electrons that occupy an orbital alone are known as

a)

sad

b)

unpaired

c)

valence

d)

electron configurations

29.

When an atom becomes an cation, the _________ electrons are lost first.

a)

unpaired

b)

valence

c)

d-orbital

d)

f-orbital

30.

How are electrons represented in an orbital diagram?

a)

as happy faces

b)

as dots

c)

as arrows

d)

as boxes

31.

Writing the noble gas of the previous principal energy level and then the sublevels that follow is known as

a)

electron configuration

b)

abbreviated electron configuration

c)

quanta

d)

photon tracking

32.

Astronomers use emission spectra to evaluate the different elements contained within stars. Why?

a)

Astronomers aren't real scientists.

b)

Each element has a unique "fingerprint" based on their electrons' excited and ground states.

c)

Stars can only be seen with the human eye.

d)

Some species of bacteria produce bioluminescence, so stars do also.

33.

Which color has the higher frequency?

a)

red

b)

orange

c)

yellow

d)

green

34.

Which color has the higher energy?

a)

yellow

b)

green

c)

blue

d)

violet

35.

Which radiation travels the fastest?

a)

radio waves

b)

microwaves

c)

visible light

d)

they all travel at the same speed

36.

Which color has the longest wavelength?

a)

red

b)

orange

c)

yellow

d)

green

37.

Why might the bottom of your pots and pans at home "glow" when heated over the stovetop?

a)

They are not built to withstand the heat

b)

Manufacturers error

c)

The electrons in the metal are excited and then emit light when falling back to ground state.

d)

The electrons are in their ground state and emit light in order to get excited.

38.

Is quantized energy more like a staircase or an elevator?

a)

staircase

b)

elevator

39.

When writing electron configurations for a cation, electrons are ______

a)

added

b)

subtracted

40.

When writing electron configurations for anions, electrons are ________

a)

added

b)

subtracted

41.

Aufbau Principle states that

a)

the electrons must ride the bus

b)

electrons occupy lowest available energy levels first

c)

only two electrons spinning in opposite directions are allowed in an orbital

d)

each orbital of equal energy must have one electron before a second electron is added

42.

Pauli Exclusion Principle states that

a)

the electrons must ride the bus

b)

electrons occupy lowest available energy levels first

c)

only two electrons spinning in opposite directions are allowed in an orbital

d)

each orbital of equal energy must have one electron before a second electron is added

43.

Hund's Rule states that

a)

the electrons must ride the bus

b)

electrons occupy lowest available energy levels first

c)

only two electrons spinning in opposite directions are allowed in an orbital

d)

each orbital of equal energy must have one electron before a second electron is added

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