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Chapter 8 Homework Attempt 2

front 1

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.

back 1

6.52 x 102

front 2

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.

back 2

8.82 x 102

front 3

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.

back 3

7.50 x 1014

front 4

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.

back 4

4.48 x 1014

front 5

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

1 being the lowest energy and 7 being the highest energy

Remember: Ephoton = hν

back 5

front 6

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.

back 6

3.2587 x 10-19

front 7

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.

back 7

4.62 x 10-19

front 8

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:

-------------------------------

This is for administrative purposes only.

Rydberg Constant = (2.18x10^-18)

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

back 8

-4.5780 x 10-19

front 9

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:

-------------------------------

This is for administrative purposes only.

Rydberg Constant = (2.1800x10^-18)

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

back 9

-4.58 x 10-19

front 10

An s orbital has what shape?

back 10

sphere

front 11

A p orbital has what shape?

back 11

dumbbell

front 12

How many electrons does the s sublevel contain?

back 12

2 electrons

front 13

How many electrons can the p sublevel hold?

back 13

6 electrons

front 14

How many orbitals are in a d sublevel?

back 14

5 orbitals

front 15

Consider the list of quantum numbers below:

n = 4; l = 1; ml = -1; ms = +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?

back 15

4p

front 16

Consider the list of quantum numbers below:

n = 4; l = 1; ml = -1; ms = +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

back 16

Yes

front 17

Consider the list of quantum numbers below:

n = 6; l = 1; ml = 0; ms = -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?

back 17

6p

front 18

Consider the list of quantum numbers below:

n = 4; l = 2; ml = -3; ms= -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

back 18

No

front 19

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

back 19

n = ___ 5 ___

l = ___ 2 ___