Complete & Condensed
Write the full form of Aluminum (Al)
1s² 2s² 2p⁶ 3s² 3p¹
An electron in a hydrogen atom jumps from the n=2 level to the n=3 level. Is this ground or excited state?
Excited State
For a 4p electron, what is the angular momentum quantum number (l)
l = 1
How many electrons can the p-sublevel hold in any principal energy level?
6
What is the electron configuration of Na⁺?
1s² 2s² 2p⁶
Write the full form of Phosphorus (P)
1s² 2s² 2p⁶ 3s² 3p³
Write the electron configuration for an excited state of Boron (B: 1s² 2s² 2p¹) where one 2s electron is promoted to 2p.
1s² 2s¹ 2p²
An electron has quantum numbers n = 2, l = 1. What sublevel is it on?
2p
How many electrons are in the 3d sublevel [Ar] 4s² 3d⁶?
6
Which element has 5 electrons in the 3p sublevel?
Chlorine
Write the full form of Titanium (Ti)
1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d²
True or False: The ground state of an atom always has the lowest possible energy configuration.
True
An electron has quantum numbers n = 2, l = 1. What are the possible values of mₛ for this electron?
Which sublevel can hold a maximum of 2 electrons?
s
True or False: All atoms of the same element always have the same ground-state electron configuration.
True
Write the condensed form of Gold (Au)
[Xe] 6s¹ 4f¹⁴ 5d¹⁰
Write an excited state configuration for Oxygen (O) where one 2p electron moves to the 3s orbital.
1s² 2s² 2p³ 3s¹
For a 3d electron, list all possible magnetic quantum numbers (mₗ).
-2, -1, 0, 1, 2
Which sublevel contains 3 orbitals and can hold up to 6 electrons?
3p
Are ground state or excited state configurations more stable?
Ground State
Write the condensed form of Uranium (U)
[Rn] 7s² 5f³ 6d¹
Explain why an excited state of an atom is less stable, and describe what happens to the electrons when it returns to the ground state.
Electrons in an excited state are at higher energy than necessary, making the atom less stable. When they return to the ground state, they release energy, often as light or heat.
A electron has n = 3. List all possible sets of quantum numbers (n, l, mₗ, mₛ) for this electron.
n = 3
l = 0, 1, 2
mₗ = -2, -1, 0, 1, 2
mₛ = +½ or -½
What is the highest energy level of Nickel at ground state?
4s²
Explain why F has a smaller radius that Li.
They have the same number of orbitals but F has 7 electrons on it and Li only has 1 on it. F's nucleus more strongly hold to those electrons, causing a smaller radius.