AP Chem Unit 1

ElectroMagnetic Radiation

Form of Energy that Atoms Absorb

Photoelectron Spectroscopy

For Ionization Energy Values for all Electrons

Photoelectron Spectrum

Ionization Energy for all Electrons charted

Principal Quantum Number

Shell (Row: 1, 2, 3)

Angular Momentum Number

Subshell (Shape: S, P, D, F)

Magnetic Quantum Number

Individual Orbital within Subshell (1-s, 3-p, 5-d)

Spin Quantum Number

Differentiates 2 Electrons in Orbital (Top and Bottom Spin)A

Aufbau Principle

In Electron Configuration, electrons are placed in orbitals, subshells, and shells in order of increasing energy

Pauli Exclusion Principle

2 Electrons that share an orbital cannot have the same spin

Hund’s Rule

When Electron is added to Subshell, it will always occupy an empty orbital. If not, then it will occupy orbitals singly and only pair up if needed

What cation does Zinc form?

+2 Cation

What cation does Silver form?

+1 Cation

What electrons do Transition Metals lose?

Their highest-level s electrons before losing lower-shell d electrons

ElectroNegativity

Measure of how strongly an atom attracts valence electrons in a covalent bond

Electron Affinity

Change in Energy when a gas-phase atom gains an electron