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Honors Chem Chapter 6

Total questions: 112

Worksheet time: 6hrs 36mins

Name
Class
Date
1.

Which of the following has the shortest wavelength?

a)

microwaves

b)

UV rays

c)

Infrared

d)

the color blue

e)

radio waves

2.

Which of the following has the most energy?

a)

Red

b)

Blue

c)

Green

d)

Violet

e)

IR (infrared)

3.

Which of the following has the most energy?

a)

X-rays

b)

The color green

c)

Microwaves

d)

UV (ultraviolet)

e)

IR (infrared)

4.

Which of the following has the least amount of energy?

a)

UV rays

b)

The color yellow

c)

infrared

d)

Gamma rays

5.

Which of the following has the lowest energy?

a)

The color yellow

b)

The color blue

c)

The color purple

d)

The color orange

6.

Which of the following has the lowest frequency?

a)

The color blue

b)

The color green

c)

The color yellow

d)

The color violet

7.

Which of the following is directly related to the energy of the photons of EMR?

a)

speed

b)

wavelength

c)

frequency

d)

Planck constant

8.

Calculate the energy of the photons in a type of electromagnetic radiation if the frequency is 4.50 x 1018 Hz.

a)

2.98 x 1015 joules

b)

1.47 x 10-52 joules

c)

6.79 x 1051 joules

d)

2.98 x 10-15 joules

e)

6.67 x 10-11 joules

9.

Liam, Avery, and Noah are discussing the properties of electromagnetic waves. They all agree that all electromagnetic waves have the same...

a)

frequency

b)

speed

c)

wavelength

d)

energy

10.

Which of the following EMR carries the greatest amount of energy?

a)

x-rays

b)

gamma rays

c)

infrared rays

d)

visible light

e)

microwaves

11.

Sophia is observing ocean waves and notices that a wave with a large wavelength will have a ______ frequency and _____ energy.

a)

high, low

b)

high, high

c)

low, high

d)

low, low

12.

During a physics class, David, Luna, and Elijah are studying waves. They notice that the blue section of a wave diagram is measuring _________________.

a)

wavelength

b)

crest

c)

trough

d)

amplitude

13.

_____ have the longest wavelengths and lowest frequencies of all electromagnetic waves.

a)

Microwaves

b)

Radio waves

c)

Gamma rays

d)

Ultraviolet

14.

What is a photon?

a)

When radiation bursts through electric waves

b)

The emission of electrons from a metal caused by light striking the metal

c)

The rate at which a wave's energy flows through a given unit of area

d)

Particles of light, also called packets of light energy

15.

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

a)

excited, ground

b)

ground, excited

16.

Calculate the wavelength of light that has the following frequency:

5.2 x 1012 s-1

a)

5.8 x 10-5 m

b)

5.8 x 10-7 m

c)

5.19 x 1014 m

d)

1.56 x 1023 m

e)

1.73 x 104 m

17.

Which wave has the highest frequency?

a)

A

b)

B

c)

C

d)

None (same frequency)

e)

Not enough info

18.

Charlotte, Henry, and Zoe are comparing the energy of different colored lights in their science project. Which color of light has the smallest energy in this group?

a)

red

b)

yellow

c)

green

d)

blue

e)

purple

19.

When atoms _____________ energy, their electrons move to higher energy levels. These electrons _____________ energy by emitting light when they return to lower energy levels.

a)

lose, absorb

b)

absorb, lose

c)

lose, lose

d)

absorb, absorb

20.

A radio station broadcasts at a frequency of 89.4 MHz. What is the radio wavelength in meters?

(MHz = 106 Hz)

a)

3.36 m

b)

0.298 m

c)

2.98 x 10-7 m

d)

3.36 x 106 m

21.

A beam of light has a wavelength of 615 nm. What is the color of this light?

a)

purple

b)

blue

c)

green

d)

yellow

e)

red

22.

A beam of light has a wavelength of 560 nm. What is the color of this light?

a)

purple

b)

blue

c)

green

d)

yellow

e)

red

23.

A beam of light has a wavelength of 465 nm. What is the color of this light?

a)

purple

b)

blue

c)

green

d)

yellow

e)

red

24.

A beam of light has a wavelength of 408 nm. What is the color of this light?

a)

purple

b)

blue

c)

green

d)

yellow

e)

red

25.

A beam of light has a wavelength of 615 nm. What is the frequency of this light?

a)

4.88 x 1014 Hz

b)

4.88 x 10-4 Hz

c)

0.0488 Hz

d)

2.05 x 10-15 Hz

e)

4.88 x 105 Hz

26.

What is the energy of a photon emitted by a light source with a frequency of 6.00 x 1014 Hz?

a)

3.97 x 10-19 joules

b)

2.50 x 10-34 joules

c)

5.45 x 1014 joules

d)

1.20 x 10-25 joules

e)

4.00 x 10-15 joules

27.

Calculate the wavelength of light that has the following frequency:

6.0 x 1014 s-1

a)

2.0 x 10-7 m

b)

5.0 x 10-7 m

c)

3.0 x 1014 m

d)

2.0 x 1023 m

e)

4.0 x 104 m

28.

A broadcasting station emits a signal at a frequency of 102.5 MHz. What is the wavelength of this signal in meters?

(MHz = 106 Hz)

a)

2.93 m

b)

0.293 m

c)

2.93 x 10-7 m

d)

2.93 x 106 m

29.

A light wave travels with a wavelength of 700 nm. Determine the frequency of this light wave.

a)

4.29 x 1014 Hz

b)

5.71 x 10-15 Hz

c)

700 x 106 Hz

d)

2.85 x 105 Hz

e)

0.285 Hz

30.

Write the electron configuration for Be

a)

1s2 2s2

b)

1s2 2s1

c)

1s1 2s2

d)

1s2 2s3

31.

Write the electron configuration for B

a)

1s2 2s2 2p1

b)

1s2 2s2

c)

1s1 2s2 2p2

d)

1s2 2s3

32.

Write the electron configuration for C

a)

1s2 2s2 2p2

b)

1s2 2s2

c)

1s1 2s2 2p1

d)

1s2 2s4

33.

Write the complete electron configuration for N

(a)  

34.

Write the complete electron configuration for O

(a)  

35.

Write the complete electron configuration for F

(a)  

36.

Write the complete electron configuration for Ne

(a)  

37.

Write the complete electron configuration for Na

(a)  

38.

Write the complete electron configuration for Mg

(a)  

39.

Write the complete electron configuration for Al

(a)  

40.

Write the complete electron configuration for Si

(a)  

41.

Write the complete electron configuration for P

(a)  

42.

Write the complete electron configuration for S

(a)  

43.

Write the complete electron configuration for Cl

(a)  

44.

Write the complete electron configuration for Ar

(a)  

45.

Write the complete electron configuration for K

(a)  

46.

Write the complete electron configuration for Ca

(a)  

47.

Write the complete electron configuration for V

(a)  

48.

Write the complete electron configuration for Fe

(a)  

49.

Write the complete electron configuration for As

(a)  

50.

Which element does this orbital diagram represent?

Hint: Type the element symbol with proper upper and lower case letter(s). DO NOT type the full name of the element.

(a)  

51.

Which element does this orbital diagram represent?

Hint: Type the element symbol with proper upper and lower case letter(s). DO NOT type the full name of the element.

(a)  

52.

Which element does this orbital diagram represent?

Hint: Type the element symbol with proper upper and lower case letter(s). DO NOT type the full name of the element.

(a)  

53.

Which element does this orbital diagram represent?

Hint: Type the element symbol with proper upper and lower case letter(s). DO NOT type the full name of the element.

(a)  

54.

Which element does this orbital diagram represent?

Hint: Type the element symbol with proper upper and lower case letter(s). DO NOT type the full name of the element.

(a)  

55.

Which element does this orbital diagram represent?

Hint: Type the element symbol with proper upper and lower case letter(s). DO NOT type the full name of the element.

(a)  

56.

Which element does this orbital diagram represent?

Hint: Type the element symbol with proper upper and lower case letter(s). DO NOT type the full name of the element.

(a)  

57.

Which element does this orbital diagram represent?

Hint: Type the element symbol with proper upper and lower case letter(s). DO NOT type the full name of the element.

(a)  

58.

Which element does this orbital diagram represent?

Hint: Type the element symbol with proper upper and lower case letter(s). DO NOT type the full name of the element.

(a)  

59.

Which element does this orbital diagram represent?

Hint: Type the element symbol with proper upper and lower case letter(s). DO NOT type the full name of the element.

(a)  

60.

Which element does this orbital diagram represent?

Hint: Type the element symbol with proper upper and lower case letter(s). DO NOT type the full name of the element.

(a)  

61.

Which element does this orbital diagram represent?

Hint: Type the element symbol with proper upper and lower case letter(s). DO NOT type the full name of the element.

(a)  

62.

Which element does this orbital diagram represent?

Hint: Type the element symbol with proper upper and lower case letter(s). DO NOT type the full name of the element.

(a)  

63.

Which element does this orbital diagram represent?

Hint: Type the element symbol with proper upper and lower case letter(s). DO NOT type the full name of the element.

(a)  

64.

Write the abbreviated electron configuration for Si

(a)  

65.

Write the abbreviated electron configuration for Cl

(a)  

66.

Write the abbreviated electron configuration for Ca

(a)  

67.

Write the abbreviated electron configuration for Cr

(a)  

68.

Write the abbreviated electron configuration for Ni

(a)  

69.

Write the abbreviated electron configuration for Ge

(a)  

70.

Write the abbreviated electron configuration for Tc

(a)  

71.

Write the abbreviated electron configuration for Ag

(a)  

72.

Write the abbreviated electron configuration for Br

(a)  

73.

Write the abbreviated electron configuration for Cs

(a)  

74.

Write the abbreviated electron configuration for Eu

Eu = europium atomic # is 63

(a)  

75.

Write the abbreviated electron configuration for W

W = tungsten atomic # is 74

(a)  

76.

Write the abbreviated electron configuration for Bi

Bi = bismuth atomic # is 83

(a)  

77.

Categorize the following elements by how many valence electrons they have.

Categorize the following

boron

aluminum

carbon

silicon

nitrogen

phosphorus

oxygen

sulfur

3 valence electrons
4 valence electrons
5 valence electrons
6 valence electrons
78.

Categorize the following elements by how many valence electrons they have.

Categorize the following

boron

gallium

germanium

silicon

arsenic

phosphorus

selenium

sulfur

3 valence electrons
4 valence electrons
5 valence electrons
6 valence electrons
79.

Categorize the following elements by how many valence electrons they have.

Categorize the following

boron

indium

tin

silicon

arsenic

antimony

magnesium

calcium

3 valence electrons
4 valence electrons
5 valence electrons
2 valence electrons
80.

Categorize the following elements by how many valence electrons they have.

Categorize the following

tellurium

fluorine

nitrogen

zinc

6 valence electrons
7 valence electrons
5 valence electrons
2 valence electrons
81.

Categorize the following elements by how many valence electrons they have.

Categorize the following

sodium

chlorine

neon

copper

potassium

iron

argon

bromine

1 valence electron
7 valence electrons
8 valence electrons
2 valence electrons
82.

Which element has the largest atomic radius?

a)

C

b)

N

c)

O

d)

F

83.

Which element has the largest ionization energy?

a)

C

b)

N

c)

O

d)

F

84.

Which element has the largest atomic radius?

a)

Si

b)

P

c)

S

d)

Cl

85.

Which element has the largest ionization energy?

a)

Si

b)

P

c)

S

d)

Cl

86.

Which element has the largest atomic radius?

a)

Ge

b)

As

c)

Se

d)

Br

87.

Which element has the largest ionization energy?

a)

Ge

b)

As

c)

Se

d)

Br

88.

Which element has the largest atomic radius?

a)

Na

b)

Mg

c)

S

d)

Cl

89.

Which element has the largest ionization energy?

a)

Na

b)

Mg

c)

S

d)

Cl

90.

Which element has the largest atomic radius?

a)

K

b)

Ca

c)

Se

d)

Br

91.

Which element has the largest atomic radius?

a)

I

b)

Br

c)

Cl

d)

F

92.

Which element has the largest ionization energy?

a)

I

b)

Br

c)

Cl

d)

F

93.

Which element has the largest atomic radius?

a)

Te

b)

Se

c)

S

d)

O

94.

Which element has the largest ionization energy?

a)

Te

b)

Se

c)

S

d)

O

95.

Which element has the largest atomic radius?

a)

Sb

b)

As

c)

P

d)

N

96.

Which element has the largest atomic radius?

a)

Sn

b)

Ge

c)

Si

d)

C

97.

Arrange the following elements in order of increasing atomic radius.

(This means start with the smallest to the largest)

a)

F

b)

O

c)

N

d)

C

e)

B

1)
2)
3)
4)
5)
98.

Arrange the following elements in order of increasing atomic radius.

(This means start with the smallest to the largest)

a)

Zn

b)

Cu

c)

Ni

d)

Co

e)

Fe

1)
2)
3)
4)
5)
99.

Arrange the following elements in order of increasing atomic radius.

(This means start with the smallest to the largest)

a)

Mo

b)

Nb

c)

Zr

d)

Y

e)

Sr

1)
2)
3)
4)
5)
100.

Arrange the following elements in order of increasing atomic radius.

(This means start with the smallest to the largest)

a)

F

b)

O

c)

N

d)

P

e)

As

1)
2)
3)
4)
5)
101.

Arrange the following elements in order of increasing atomic radius.

(This means start with the smallest to the largest)

a)

Ar

b)

Cl

c)

S

d)

Se

e)

Te

1)
2)
3)
4)
5)
102.

The data in the table shows the first 6 ionization energies for an unknown element. Of the following elements, which one could have the data presented in the table?

a)

Na

b)

Mg

c)

Si

d)

Al

e)

Cl

103.

The data in the table shows the first 6 ionization energies for an unknown element. Of the following elements, which one could have the data presented in the table?

a)

Li

b)

Be

c)

B

d)

C

e)

O

104.

The data in the table shows the first 6 ionization energies for an unknown element. Of the following elements, which one could have the data presented in the table?

a)

Na

b)

Mg

c)

Al

d)

P

e)

S

105.

The data in the table shows the first 6 ionization energies for an unknown element. Of the following elements, which one could have the data presented in the table?

a)

S

b)

Mg

c)

Al

d)

P

e)

Si

106.

The data in the table shows the first 6 ionization energies for an unknown element. Of the following elements, which one could have the data presented in the table?

a)

N

b)

F

c)

O

d)

B

e)

C

107.

The data table shows the first 6 ionization energies for Na, sodium. Why is there a very large difference between the 1st and 2nd ionization energy?

a)

Sodium has 1 valence electron. The 2nd electron removed is a core electron.

b)

Sodium has 2 valence electrons. The 3rd electron removed is a core electron.

c)

Sodium has 1 total electron, therefore the remaining ionization energies are hypothetical.

d)

Sodium has 1 core electron, the 2nd electron removed is a valence electron.

108.

The data table shows the first 6 ionization energies for Al, aluminum. Why is there a very large difference between the 3rd and 4th ionization energy?

a)

Aluminum has 3 valence electrons. The 4th electron removed is a core electron.

b)

Aluminum has 4 valence electrons. The 5th electron removed is a core electron.

c)

Aluminum has 3 electrons in the 3p subshell, and the rest are in the 6s subshell.

d)

Aluminum has 3 core electrons, the 4th electron removed is a valence electron.

109.

The data table shows the first 6 ionization energies for Si, silicon. Why is there a very large difference between the 4th and 5th ionization energy?

a)

Silicon has 4 valence electrons. The 5th electron removed is a core electron.

b)

Silicon has 5 valence electrons. The 6th electron removed is a core electron.

c)

Silicon has 4 electrons in the 4p subshell, and the rest are in the 2s subshell.

d)

Silicon has 4 core electrons, the 5th electron removed is a valence electron.

110.

Why does fluorine have a higher ionization energy than iodine?

a)

Fluorine's valence e- are closer to its nucleus than iodine's, making it harder to remove an electron from fluorine.

b)

Fluorine's valence e- are further from its nucleus than iodine's, making it harder to remove an electron from fluorine.

c)

Fluorine's valence e- are further from its nucleus than iodine's, making it easier to remove an electron from fluorine.

d)

Fluorine's valence e- are closer to its nucleus than iodine's, making it easier to remove an electron from fluorine.

111.

Why does sulfur have a higher ionization energy than tellurium?

a)

Sulfur's valence e- are closer to its nucleus than tellurium's, making it harder to remove an electron from sulfur.

b)

Sulfur's valence e- are further from its nucleus than tellurium's, making it harder to remove an electron from sulfur.

c)

Sulfur's valence e- are further from its nucleus than tellurium's, making it easier to remove an electron from sulfur.

d)

Sulfur's valence e- are closer to its nucleus than tellurium's, making it easier to remove an electron from sulfur.

112.

Why does nitrogen have a higher ionization energy than arsenic?

a)

Nitrogen's valence e- are closer to its nucleus than arsenic's, making it harder to remove an electron from nitrogen.

b)

Nitrogen's valence e- are further from its nucleus than arsenic's, making it harder to remove an electron from nitrogen.

c)

Nitrogen's valence e- are further from its nucleus than arsenic's, making it easier to remove an electron from nitrogen.

d)

Nitrogen's valence e- are closer to its nucleus than arsenic's, making it easier to remove an electron from nitrogen.

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