Light, Electrons, and Periodic Table

Which of the following elements make up the unknown sample?

• A and B

• B and C

• C and D

Which of the following electron jumps would be responsible for the MOST energetic light emitted?

• 5th to the 2nd energy level

• 3rd to the 2nd energy level

Solve this problems using the equation: 
C = λν
If an AM radio station broadcasts at
9.95 x 10⁵ Hz, what is the wavelength of this radiation?

• 6.59 x 10^-28 m
• 1.01 x 10^-6 m
• 3.32 x 10^-3 m
• 302 m

The electron configuration of an atom is 1s²2s²2p⁶. How many electrons are in this atom?

• 3

• 6

• 8

• 10

 The diagram above represents two electrons with 

• a. opposite spins.
•  b. the same spin.
• c. different energies.
• d. different energy levels.

What is the electronic configuration of iron?

• 1s²2s²2p⁶3s²3p⁶4s²3d⁶
• 1s²2s²2p⁶3s²3p⁶3d⁸
• 1s²2p⁶3s²3p⁶4s²3d⁶
• 1s²2s²2p⁶3s²3p⁶4s¹3d⁶

Which of the following is the correct electron dot structure for nitrogen?

• 
• 
• 
• 

In the model shown, if an electron jumps from n=3 to n=4, which of the following is true?

• 0.66 eV of energy were absorbed by the electron

• 0.66 eV of energy were released by the atom

• The electron has relaxed to a lower energy state

• Light is given off in the form of a photon

In the model shown, if an electron in n=2 is given energy of 1.5 eV, what will happen?

• It will jump up to the n=3 level, since the energy is large enough

• The electron will stay in n=2, since the energy is too small

• The electron will relax down to n=1, since the energy pushes it to a lower level

• It will jump to some location between n=2 and n=3

If a photon is emitted with an energy of 9.61 x 10^-20 J, calculate the frequency of the light. (E=hv; h = 6.63x10^-34Js)

• 1.45 x 10^14 Hz

• 6.89 x 10^13 Hz

• 6.37 x 10^15 Hz

• 1.32 x 10^13 Hz