Chemistry Unit 2

Principle Quantum Number

Indicates the main energy level occupied by an electron

s block

first two groups; hold 2 electrons, reactive and always in compounds

d block

groups 3-12 Transition metals, shiny, good conductors of heat and electricity, holds 10 electrons

p block 

Group 13-18, metals, nonmetals, and metalloids very different in terms of properties holds 6 electrons

F block

bottom part, magnetic, reactive to a lot of things, holds 14 electrons

Aufbau Principle

An electron occupies the lowest energy orbital before filling any others

Pauli Exclusion Principle

An orbital can hold two electrons of opposite spin

Hund’s Rule 

Orbitals of equal energy are each occupied by one electron before any orbital is occupied by a second electron, and all electrons in singly occupied orbitals must have the same spin

Atomic Radii

The size of the atoms themselves

Atomic Radii sizing

Left to right- smaller

Decrease across the periods

Ion

An atom or group of atoms that has a positive or negative charge

Something with a charge 

Ionization

The process of gaining or losing electrons resulting in the formation of ions

Ionization Energy

The amount of energy required to remove one electron from a neutral atom of an element

Valence Electrons 

The electrons available to be lost, gained, or shared in the formation of a chemical compound 

Outer Shell Electrons 

Electronegativity

Measure of the ability for an electron or chemical compound to attract electrons

Angular Momentum Quantum Number

Symbolized by l and indicated the shape of the orbital

Magnetic Quantum Number

Symbolized by m and indicates the orientation of the orbital around the nucleus

Spin Quantum Number

Does the orbital have a positive or negative spin