3.1-3.2 Bohr Model of the Atom

Multiple Choice

What is one key feature of the Bohr Model of the Atom?

• Electrons move randomly around the nucleus

• Electrons revolve in stable, quantized orbits

• Electrons are stationary in the nucleus

• Electrons have no defined energy

Multiple Choice

According to the Bohr Model, what happens to the energy of the shells as you move farther from the nucleus?

• The energy decreases

• The energy stays the same

• The energy increases

• The energy fluctuates

Multiple Select

Which of the following statements about ground and excited states are correct? Choose 3

• Ground state is the lowest energy state.

• Atoms and molecules can have multiple excited states.

• There is only one ground state for an atom or molecule.

• Excited states have lower energy than the ground state.

Multiple Choice

Consider swinging a rock on the end of a string in large circles. Even though you are constantly pulling on the string, the rock never collides with your hand. 

Why is this?

• The rock is moving so fast that the pull from your hand is not enough to pull the rock into your hand.

• Gravity is pulling the rock sideways away from your hand.

• The atmosphere is pulling the rock upwards away from your hand.

Multiple Choice

Even though the Earth is attracted to the sun by a very strong gravitational pull, what keeps the Earth from striking the sun?

• The fact that the Earth is moving keeps it from striking the sun.

• The fact that the Earth is huge keeps it from striking the sun.

• Mercury and Venus keep Earth from striking the sun.

Multiple Choice

Why doesn't the moon strike the Earth?

• The movement of the moon keeps it from colliding with the Earth, even though the Earth exerts a gravitational pull on the moon.

• The fact that the moon is twice as large as the Earth keeps it from striking the Earth

Multiple Choice

How could it be possible for the electrons to not "collapse" into the nucleus?

• The electrons must be orbiting so fast that the pull from the nucleus is not enough to cause the electrons to collide into the nucleus.

• The electrons are positive, and so is the nucleus, so the electrons aren't even attracted to the nucleus.

• The neutrons have one job: to keep the electrons from touching the nucleus.

Multiple Choice

As the frequency of light increases, what happens to the wavelength of the light?

• As the frequency increases, the wavelength must be smaller. This is because the frequency times the wavelength must always equal 3.00x10⁸ m/s

• As the frequency increases, the wavelength must also increase. This is because the frequency divided by the wavelength must always equal 3.00x10⁸ m/s

• As the frequency increases, the wavelength must be constant. This is because the wavelength must always equal 3.00x10⁸ m/s

Drag and Drop

What is the frequency of light that has a wavelength of 4.25 x 10^-8 m?

Frequency: ​ ​

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Units: ​ ​

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7.06 x 10^15

s^-1

0.706

1.42 x 10^-16

m

g

mol

m/s

s

1.42

Multiple Choice

What is the wavelength of light in meters that has a frequency of 3.85 x 10¹⁴ Hz?

• 7.79 x 10^-7 m

• 7.79 x 10²¹ m

• 1.28 x 10⁶ m

• 1.28 x 10²² m

​E = hv

Multiple Choice

Does an electron need to absorb energy or give off energy (release energy) to go from the 2nd to the 1st energy level?

• It needs to give off energy to go to a lower energy level.

• It needs to absorb energy to go to a lower energy level.

Multiple Choice

How is it possible for an electron to go from the 3rd to the 4th energy level?

• The electron must absorb energy to go to a higher energy level.

• The electron must release energy to go to a higher energy level.

• The electron must absorb energy to go to a lower energy level.

• The electron must jump multiple energy levels to go to one higher.

Drag and Drop

Red light of frequency 4.37 x 10¹⁴ Hz is required to excite a certain electron. What energy did the electron gain from the light?

Energy: ​ ​

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Units:​

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2.90 x 10^-19

J

m

s^-1

g

2.90 x 10^-47

1.52 x 10^-20

1.52 x 10^-48

6.60 x 10^47

6.60 x 10^-21

Multiple Choice

The energy difference between the 1st and 2nd energy levels in a certain atom is 5.01 x 10^-19 J. What frequency of light is necessary to excite an electron in the 1st energy level?

• 7.56 x 10¹⁴ Hz

• 3.32 x 10^-52 Hz

• 7.56 x 10^-54 Hz

• 1.32 x 10^-15 Hz

• 1.32 x 10^-53 Hz

Drag and Drop

An electron gives off a photon with 4.05 x 10^-19 J of energy. Determine the frequency, wavelength, and color of this light.

Frequency in Hz: ​

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Wavelength in m: ​

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Color: ​

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6.11 x 10^14

4.91 x 10^-7

blue

orange

green

2.68 x 10^-52

1.11 x 10^60

7.41 x 10^26

1.64 x 10^-15

violet

Multiple Choice

An electron released a photon with energy equal to 3.313 x 10^-19 J. What is the wavelength of this photon in nanometers (nm)?

• 600
• 500

• 313

• 906

• 400

Multiple Choice

An electron released a photon with energy equal to 3.313 x 10^-19 J. What is the color of this photon?

• orange

• red

• blue

• indigo

• yellow