Chapter 8 Homework Attempt 2 Flashcards

Calculate the wavelength of light (in nm) if the light has a frequency of (4.60x10^14) s^-1. Use a value of (3.0000x10^8) for the speed of light.

Remember 1 m = (1.000x10^9) nm

Do not include units with your answer.

Note: Your answer is assumed to be reduced to the highest power possible.

Calculate the wavelength of light (in nm) if the light has a frequency of (3.400x10^14) s^-1. Use a value of (3.00x10^8) for the speed of light.

Remember 1 m = (1.0000x10^9) nm

Do not include units with your answer.

Note: Your answer is assumed to be reduced to the highest power possible.

Calculate the frequency of light (in s^-1 also known as Hz) with a wavelength of (4.00x10^2) nm. Use a value of (3.0000x10^8) for the speed of light.

Remember 1 m = (1.000x10^9) nm

Do not include units with your answer.

Note: Your answer is assumed to be reduced to the highest power possible.

Calculate the frequency of light (in s^-1 also known as Hz) with a wavelength of (6.70x10^2) nm. Use a value of (3.0000x10^8) for the speed of light.

Remember 1 m = (1.000x10^9) nm

Do not include units with your answer.

Note: Your answer is assumed to be reduced to the highest power possible.

Rank the following types of radiation from lowest energy to highest energy.

1 being the lowest energy and 7 being the highest energy

Remember: E_photon = hν

Calculate the energy of a photon of light (in Joules) with a wavelength of (6.1000x10^2) nm. Use a value of (3.00x10^8) for the speed of light.

Remember 1 m = (1.0000x10^9) nm

h = (6.6260x10^-34) Js

Do not include units with your answer.

Note: Your answer is assumed to be reduced to the highest power possible.

Calculate the energy of a photon of light (in Joules) with a wavelength of (4.30x10^2) nm. Use a value of (3.000x10^8) for the speed of light.

Remember 1 m = (1.0000x10^9) nm

h = (6.6260x10^-34) Js

Do not include units with your answer.

Note: Your answer is assumed to be reduced to the highest power possible.

An electron transitions from the n = (5.0000x10^0) energy level to the n = (2.0000x10^0) energy. Calculate the energy, in Joules, associated with this energy transition. If the transition is exothermic be sure to include the appropriate sign.

Use the equation:

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This is for administrative purposes only.

Rydberg Constant = (2.18x10^-18)

Note: Your answer is assumed to be reduced to the highest power possible.

An electron transitions from the n = (5.00x10^0) energy level to the n = (2.000x10^0) energy. Calculate the energy, in Joules, associated with this energy transition. If the transition is exothermic be sure to include the appropriate sign.

Use the equation:

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This is for administrative purposes only.

Rydberg Constant = (2.1800x10^-18)

Note: Your answer is assumed to be reduced to the highest power possible.

An s orbital has what shape?

A p orbital has what shape?

How many electrons does the s sublevel contain?

How many electrons can the p sublevel hold?

How many orbitals are in a d sublevel?

Consider the list of quantum numbers below:

n = 4; l = 1; m_l = -1; m_s = +1/2

(OR n = 4; l = 1; m sub _l = minus 1; m sub _s = +1/2)
In which orbital subshell will this electron be located?

Consider the list of quantum numbers below:

n = 4; l = 1; m_l = -1; m_s = +1/2

(OR n = 4; l = 1; m sub _l = minus 1; m sub _s = +1/2)
Is this a valid set of quantum numbers?

• Yes
• No

Consider the list of quantum numbers below:

n = 6; l = 1; m_l = 0; m_s = -1/2

(OR n = 6; l = 1; m sub _l = 0; m sub _s = minus 1/2)
In which orbital subshell will this electron be located?

Consider the list of quantum numbers below:

n = 4; l = 2; m_l = -3; m_s= -1/2

(OR n = 4; l = 2; m sub _l = minus 3; m sub _s = minus 1/2)
Is this a valid set of quantum numbers?

• Yes
• No

An electron is located in the 5d orbital. Quantum numbers for this electron would be: <p>n = ______</p> <p>l = ______</p>