quantum chemistry

What is the total number of energy levels used by an atom of aluminum
(Al, atomic #13) in the ground state?

• 3
• 7
• 13
• 0

How many orbitals are available to hold electrons in the 6th energy level (n=6)?

• 9

• 16

• 26

• 36

This "rule" of Quantum Chemistry states that it is impossible to know both the position and velocity of an electron at the same time.

• Hund's Rule
• Heisenberg Uncertainty Principle
• Aufbau Principle
• Pauli Exclusion Principle

According to the Aufbau Principle, which sublevel should starting filling with electrons after 5s?

• 6s
• 5p
• 4d
• 3f

Identify the following element:
1s²2s²2p⁶3s²3p⁶4s²3d¹⁰

• nickel
• copper
• zinc
• gallium

The second energy level (n=2) contains a total of 5 electrons...how many more electrons can fit in the 2nd energy level?

• 0
• 3
• 5
• 7

Identify the element whose electron configurations ends with 5p³

• As
• Te
• Sb
• Sn

Which of the following statements is true about the 3s and the 4s sublevels?

• These sublevels have the same energy
• These sublevels are the same distance from the nucleus
• These sublevels hold different amounts of electrons
• These sublevels have the same shape

Which of the following quantum number sets is not allowed?

• { 3, 2, +1, -1/2 }
• { 5, 3, -1, +1/2 }
• { 12, 1, +2, +1/2 }
• { 7, 6, -5, -1/2 }

This "rule" of Quantum Chemistry states that no 2 electrons in an atom can be in the exact same state...each electron in an atom can be described by a unique set of quantum numbers.

• Hund's Rule
• Heisenberg Uncertainty Principle
• Aufbau Principle
• Pauli Exclusion Principle