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Unit 2 Review Game

Total questions: 67

Worksheet time: 2hrs 14mins

Name
Class
Date
1.

Which has the longest wavelength?

a)

Radio Waves

b)

Red Visible Light

c)

Infrared Light

d)

Gamma Rays

2.

How do electrons become excited?

a)

Emitting light/energy

b)

Absorbing light/energy

c)

Going down an orbital/energy level

d)

Going up an orbital/energy level

3.

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

a)

active

b)

inactive

c)

excited

d)

ground

4.

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

5.

What form of energy is emitted when an excited electron returns to the ground state?

a)

Photon (light)

b)

Heat

c)

Kinetic

d)

Potential

6.

An atom in the ______________ is more stable.

a)

Ground state

b)

Excited State

7.
An example of a wave with a short wavelength, high frequency, and high energy is a 
a)
X-ray
b)
Microwave
c)
Visible light wave
d)
Infrared wave
8.

Which color has the longest wavelength?

a)

Yellow

b)

Red

c)

Green

d)

Purple

9.

The distance between 2 neighboring peaks or troughs is called _____________________.

a)

Speed

b)

Frequency

c)

Wavelength

d)

Amplitude

10.

The most dangerous waves which are short and can be caused from radioactivity or nuclear reactions.

a)

Gamma Rays

b)

X-Rays

c)

UV Rays

d)

Microwaves

11.

Hot objects give off this type of wave.

a)

Gamma

b)

UV

c)

Radiowaves

d)

Infrared

12.

Match the following descriptions to the correct form of electromagnetic radiation

a)

The waves we can see

1.

Visible light

b)

Used to cook food and in cell phones

2.

Microwaves

c)

Detected as heat, used in remote controls

3.

Infrared

d)

The highest frequency waves, very dangerous to humans

4.

Gamma

e)

Produced by the sun & can cause sunburns

5.

Ultraviolet

13.

Which wave has the highest frequency?

a)

A

b)

B

c)

C

14.

S orbitals hold a maximum of (a)   electrons, p orbitals hold a maximum of ​ (b)   electrons, d orbitals hold a maximum of ​ (c)   electrons, and f orbitals hold a maximum of ​ (d)   electrons.

Choose from the below words
2
6
10
14
8
12
18
15.

When are photons of light released?

a)

When electrons move from the ground state to the excited state

b)

When electrons move from the excited state to the ground state

c)

When electrons stay in the same orbital.

d)

When the distance to the nucleus increases.

16.

Match the following elements to the correct Lewis Dot diagram

a)

1.

Ca

b)

2.

Se

c)

3.

F

d)

4.

Xe

e)

5.

B

17.

Click on the transition metal

A
B
C
D
E
F
G
18.

Match the following to the correct oxidation number

a)

O

1.

-2

b)

Cl

2.

-1

c)

Al

3.

+3

d)

Na

4.

+1

e)

PO4

5.

-3

19.

Find the frequency of an electromagnetic wave with a wavelength 2.75 × 10–8 m.

a)

1.10 Hz

b)

1.09 × 1016 Hz

c)

9.17 × 1015 Hz

d)

9.17 × 1016 Hz

20.
How many valence electrons are in an atom of Ar?
a)
2
b)
8
c)
4
d)
1
21.
How many valence electrons are in an atom of Ba?
a)
2
b)
8
c)
4
d)
1
22.

What happens to the energy absorbed by excited electrons as they return to ground state?

a)

energy turns into visible light

b)

electrons move to higher energy level

c)

electrons will be added

d)

electrons will be removed

23.
What atom matches this electron configuration?
1s2 2s2 2p6 3s2
a)
Neon
b)
Magnesium
c)
Aluminum
d)
Potassium
24.
Which is the electron configuration for an oxygen atom?
a)
1s22s22p63s23p64s2
b)
1s22s22p4
c)
1s22s22p6
d)
1s22s22p63s23p6
25.
What is the maximum number of electrons that an orbital can have?
a)
1 electron
b)
2 electrons
c)
3 electrons
d)
4 electrons
26.
How many valence electrons are represented here?
a)
7
b)
5
c)
2
d)
8
27.
How many d orbitals are there in a given sublevel?
a)
1
b)
3
c)
5
d)
7
28.
How many p orbitals are there in a sublevel?
a)
2
b)
1
c)
4
d)
3
29.
How many electrons can the d sublevel hold?
a)
8
b)
10
c)
2
d)
4
30.
What is this element? 
1s22s22p63s23p6
4s23d104p6
a)
Argon
b)
Krypton
c)
Selenium
d)
Bromide
31.
How many valence electrons does Chlorine have?
a)
5
b)
2
c)
7
d)
5
32.
How many valence electrons does phosphorus have?
a)
5
b)
2
c)
8
d)
15
33.
Which element is pictured?
a)
neon
b)
fluorine
c)
magnesium
d)
argon
34.
Which of the following is a p block element?
a)
Ca
b)
Ar
c)
Re
d)
Au
35.
Electron arrangement that uses arrows
a)
Electron configuration
b)
Shorthand configuration
c)
Lewis dot structure
d)
Orbital diagram
36.
The electron configuration of an atom is 1s22s22p6.  The number of electrons in the atom is 
a)
3
b)
6
c)
8
d)
10
37.

Which element has a configuration of 1s2 2s2 2p6?

a)

Neon

b)

Helium

c)

Argon

d)

Krypton

38.

Which element has electronic configuration of 1s2 2s2 2p6 3s2 3p2

a)

C

b)

Si

c)

Mg

d)

Be

39.
This orbital diagram represents:  
a)
C
b)
B
c)
N
d)
O
40.

What element has the electron configuration 

1s22s22p31s^22s^22p^3  

a)

Nitrogen

b)

Oxygen

c)

Magnessium

d)

Carbon

41.

What atom matches this electron configuration?

1s22s22p63s23p64s23d10

a)

Zinc

b)

Copper

c)

Nickel

d)

Germanium

42.

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

43.

According to the octet rule, most elements need _______ valence electrons.

a)

2

b)

8

c)

6

d)

18

44.

Hydrogen needs _____ electrons to be stable.

a)

4

b)

6

c)

8

d)

2

45.

If electrons are shared unequally then the bond is ___.

a)

non-polar covalent

b)

ionic

c)

non-polar ionic

d)

polar covalent

46.

If electrons are shared equally, the bond is ____.

a)

non-polar covalent

b)

ionic

c)

non-polar ionic

d)

polar covalent

47.

Which of the following is the correct Lewis dot structure for a molecule of fluorine, F2?

a)
b)
c)
d)
48.

When drawing Lewis structures, only __________ electrons are used.

a)

inner shell

b)

core

c)

valence

d)

stable

49.

Each line in a Lewis structure represents __________ electron(s).

a)

3

b)

2

c)

1

d)

4

50.

What is the correct Lewis structure for ammonia, NH3?

a)
b)
c)
d)
51.

Which is the correct Lewis structure for carbon dioxide?

a)
b)
c)
d)
52.

What is the total number of valence electrons in the Lewis structure of the NO2- polyatomic ion?

a)

8

b)

19

c)

18

d)

24

53.

Three pairs of electrons are shared in a ____.

a)

single bond

b)

double bond

c)

triple bond

54.

Which of the following has bond angles of 120 degrees?

a)

tetrahedral

b)

bent

c)

trigonal planar

d)

trigonal pyramidal

55.

Which of the following molecular geometries has bond angles of 109.5 degrees?

a)

bent

b)

tetrahedral

c)

octahedral

d)

linear

56.
According to VSEPR, molecules adjust their shapes to keep which of the following as far away as possible?
a)
Pairs of valence electrons
b)
Inner shell electrons
c)
Mobile Electrons
d)
Electrons closest to the nucleus
57.

What is the shape? Hint: Draw the Lewis dot structure for NH3.

a)

tetrahedral

b)

trigonal pyramidal

c)

trigonal planar

d)

bent

58.
What is the shape of H2O?
a)
linear
b)
tetrahedral
c)
bent
d)
trigonal pyramidal
59.

SiCl4 has what shape?

a)

trigonal planar

b)

pyramidal

c)

tetrahedral

d)

trigonal pyramidal

60.

3 atoms bonded and 0 lone pairs

a)

linear

b)

trigonal planar

c)

bent

d)

tetrahedral

e)

trigonal pyramidal

61.

3 atoms bonded and 1 lone pairs

a)

true linear

b)

trigonal planar

c)

bent

d)

tetrahedral

e)

trigonal pyramidal

62.
What is the correct formula for this molecule?
a)
Si4F
b)
SiF4
c)
SiF
d)
Si4F4
63.

What name is given to the shape shown in the picture?

a)

bent

b)

trigonal planar

c)

triangular

d)

trigonal pyramidal

64.

What is the name of the molecular geometry for this Lewis Structure?

a)

trigonal planar

b)

trigonal pyramidal

c)

tetrahedral

d)

bent

65.

Which is the 3D picture of this molecule?

a)
b)
c)
d)
66.

This molecule has 2 bonds and 2 lone pairs around the central atom. What shape is it?

a)

bent

b)

trigonal pyramidal

c)

tetrahedral

d)

linear

67.

In the following lewis structure, how many bonds are around the central atom?

a)

1 bond

b)

2 bonds

c)

3 bonds

d)

4 bonds

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