Chapter 8 Homework Attempt 1 Flashcards

Calculate the wavelength of light (in nm) if the light has a frequency of (5.5000x10^14) s^-1. Use a value of (3.00x10^8) 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 (3.300x10^14) s^-1. Use a value of (3.000x10^8) for the speed of light.

Remember 1 m = (1.00x10^9) 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 (5.800x10^2) nm. 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 (5.50x10^2) 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 (7.0000x10^2) nm. Use a value of (3.000x10^8) for the speed of light.

Remember 1 m = (1.000x10^9) nm

h = (6.63x10^-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 (6.200x10^2) nm. Use a value of (3.000x10^8) for the speed of light.

Remember 1 m = (1.00x10^9) nm

h = (6.626x10^-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 = (5.00x10^0) energy level to the n = (1.0000x10^0) 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 = (2.180x10^-18)

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

An electron transitions from the n = (4.00x10^0) 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 = (2.180x10^-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 = 2; l = 0; m_l = 0; m_s = +1/2

(OR n = 2; l = 0; m sub _l = 0; m sub _s = +1/2)
What element has the outermost electron represented by this set of quantum numbers? (Symbol, please)

Consider the list of quantum numbers below:

n = 3; l = 0; m_l = 0; m_s = +1/2

(OR n = 3; l = 0; m sub _l = 0; m sub _s = +1/2)
What element has the outermost electron represented by this set of quantum numbers? (Symbol, please)

Consider the list of quantum numbers below:

n = 5; l = 0; m_l = 0; m_s = +1/2

(OR n = 5; l = 0; m sub _l = 0; m sub _s = +1/2)
What element has the outermost electron represented by this set of quantum numbers? (Symbol, please)

An electron is located in the 5f orbital. Quantum numbers for this electron would be:

n = ______

l = ______

Consider the list of quantum numbers below:

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

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

• Yes
• No