Chapter 1: Structure of the Atom

Electromagnetic radiation

is defined by wavelength and frequency.

Pauli Exclusion Principle

The states that no two electrons in an atom can have the same set of four quantum numbers.

Momentum

is correlated to the size of the electrons orbit.

Wavelength

is the distance between to repeating points (minima to minima or maxima to maxima)

Heisenberg Uncertainty Principle

The states that it is impossible to simultaneously determine the exact position and momentum of a particle.

indivisible particles

All matter is made up of tiny, called atoms.

Electrons

will fill the lowest energy orbitals first before moving to higher energy orbitals.

Frequency

is the number of waves per second.

Bohr radius

The is the distance between the nucleus and the electron in a hydrogen atom in its ground state.

Electron orbitals

are regions of space around the nucleus of an atom where electrons are likely to be found.

arrangement of orbitals

The number and in an atom is determined by its electron configuration.

Valence electrons

are represented by dots in Lewis dot structures.

hund's rule

Electrons fill orbitals one by one with parallel spins before pairing up

neutron charge

0

proton charge

+1

electron charge

-1

max electrons in the first principal energy level

2

max electrons in the second principal energy level

8

max electrons in the third principal energy level

18

max electrons in the fourth principal energy level

32