Table of contents

1. Intro to General Chemistry3h 48m
2. Atoms & Elements4h 16m
3. Chemical Reactions4h 10m
4. BONUS: Lab Techniques and Procedures1h 38m
5. BONUS: Mathematical Operations and Functions48m
6. Chemical Quantities & Aqueous Reactions3h 53m
7. Gases3h 49m
8. Thermochemistry2h 37m
9. Quantum Mechanics2h 58m
10. Periodic Properties of the Elements3h 9m
11. Bonding & Molecular Structure3h 29m
12. Molecular Shapes & Valence Bond Theory1h 57m
13. Liquids, Solids & Intermolecular Forces2h 23m
14. Solutions3h 1m
15. Chemical Kinetics2h 53m
16. Chemical Equilibrium2h 29m
17. Acid and Base Equilibrium5h 1m
18. Aqueous Equilibrium4h 47m
19. Chemical Thermodynamics1h 50m
20. Electrochemistry2h 42m
21. Nuclear Chemistry2h 36m
22. Organic Chemistry5h 7m
23. Chemistry of the Nonmetals2h 39m
24. Transition Metals and Coordination Compounds3h 16m

10. Periodic Properties of the Elements

The Electron Configuration

General Chemistry

10. Periodic Properties of the Elements

The Electron Configuration

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Multiple Choice

A ground state atom of Mg could not have any electrons with which of the following electron configurations?

n = 1, l = 0, m_l = 0, m_s = +1/2

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

n = 2, l = 1, m_l = -1, m_s = -1/2

n = 3, l = 0, m_l = 0, m_s = -1/2

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Verified step by step guidance

Step 1: Understand the quantum numbers and their meaning. The four quantum numbers are: principal quantum number $n$, azimuthal (angular momentum) quantum number $l$, magnetic quantum number $m_l$, and spin quantum number $m_s$. Each electron in an atom is described by a unique set of these numbers.

Step 2: Recall the electron configuration of a ground state magnesium (Mg) atom. Magnesium has 12 electrons, and its ground state electron configuration is $1s^2 2s^2 2p^6 3s^2$. This means electrons fill up to $n=3$, $l=0$ (the 3s orbital) in the ground state.

Step 3: Analyze the given quantum numbers for each electron configuration option to determine if they correspond to an allowed electron in the ground state of Mg. Check if the quantum numbers correspond to orbitals that are occupied in the ground state or if they violate any quantum rules.

Step 4: Specifically, check the option $n=3$, $l=2$, $m_l=0$, $m_s=+1/2$. Here, $l=2$ corresponds to a d orbital. Since Mg's ground state electron configuration does not include any electrons in the 3d orbitals (which would be $n=3$, $l=2$), this configuration cannot be present in the ground state.

Step 5: Confirm that the other options correspond to orbitals that are occupied in the ground state or are allowed by the quantum numbers for Mg's electrons. Thus, the configuration with $n=3$, $l=2$, $m_l=0$, $m_s=+1/2$ is the one that cannot exist for a ground state Mg atom.