Quantum Numbers, Atomic Orbitals, and Electron Configurations
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These flashcards cover key concepts related to quantum numbers, atomic orbitals, and electron configurations, helping to reinforce understanding of the material.
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15 Terms
What are quantum numbers?
A set of four numbers that describe the unique quantum state of an electron in an atom.
What does the principal quantum number (n) indicate?
The principal quantum number specifies the energy level and size of the orbital.
How are subshells designated according to the angular momentum quantum number (l)?
Subshells are designated by letters: 0 is s, 1 is p, 2 is d, 3 is f, and so on.
What does the magnetic quantum number (ml) specify?
The orientation of an orbital in space for a given energy and shape.
What does the spin quantum number (ms) represent?
The orientation of the spin axis of an electron, either +½ (up) or -½ (down).
What is the Pauli exclusion principle?
No two electrons in the same atom can have identical values for all four quantum numbers.
What is electron configuration?
The distribution of electrons among the orbitals of an atom.
What is the Aufbau principle?
The principle that electrons occupy the lowest energy orbitals available.
What is Hund's rule?
When electrons occupy orbitals of equal energy, they spread out to minimize pairing.
What type of elements form cations by losing electrons from the outermost shell?
Alkali metals (Group I) and alkaline earth metals (Group IIA).
What is an isoelectronic configuration?
An ion's electron configuration that matches that of the nearest noble gas.
How do transition metals typically form ions?
Transition metals usually lose valence s electrons first to form +2 charges, but can also lose d electrons.
What happens to electrons when they absorb energy?
They can be excited to higher energy orbitals.
Define paramagnetic substances.
Substances with unpaired electrons that are weakly attracted to magnets.
Define diamagnetic substances.
Substances with all paired electrons that are not attracted to magnets.
Note 
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