Question

1. true (a) or false (b): the quantum mechanical model treats electrons as waves.
2. which diagram best shows the quantum mechanical model of the atom?

for questions 21 - 23, use the image to the right and the options below to answer the questions.
a. orbital type/shape b. energy level c. number of electrons d. aufbau

1. the \1\ represents the
2. the \s\ represents the
3. the \2\ represents the
4. an atom having an electron configuration of (1s^{2}2s^{2}2p^{6}3s^{1}) would be an atom of

a. al b. mg c. na d. ar

1. a chemistry student at calvert hall wrote the orbital diagram for carbon (c) in the following way.

the rule he did not correctly follow is:
a. aufbau principle b. pauli exclusion principle c. hunds rule

Explanation:

• Question 19: The Quantum Mechanical Model treats electrons as waves. This is a fundamental concept in quantum mechanics.
• Question 20: Diagram a shows different orbitals (1s, 2s, 2p, 3s) which is characteristic of the Quantum Mechanical Model. Diagram b shows electrons in circular - like paths (more like the Bohr model).
• Question 21: In the notation \(1s^{2}\), the number \(1\) represents the energy level.
• Question 22: The letter \(s\) represents the orbital type/shape.
• Question 23: The superscript \(2\) represents the number of electrons.
• Question 24: For an atom with electron configuration \(1s^{2}2s^{2}2p^{6}3s^{1}\), the total number of electrons is \(2 + 2+6 + 1=11\). Sodium (\(Na\)) has an atomic number of \(11\).
• Question 25: Hund's Rule states that electrons will fill degenerate orbitals (same - energy orbitals) singly before pairing up. In the given orbital diagram for carbon (\(C\), atomic number \(6\), electron configuration \(1s^{2}2s^{2}2p^{2}\)), the two \(2p\) electrons should be in separate \(2p\) orbitals with parallel spins. But in the given diagram, one \(2p\) orbital is filled with one electron before the other \(2p\) orbitals are singly occupied.

Answer:

1. A. True
2. a
3. b. energy level
4. a. orbital type/shape
5. c. number of electrons
6. c. Na
7. c. Hund's Rule