ap chem unit 2

Electron negativity

An electrons tend echo to attract electrons in a covalent bond even closer to its nucleus

Polarity

the result of an electronegatity difference between bonded elements

Dipole movement

The presence of unequal electron sharing in a specific bond

Metals are good conductors because

They have delocalized electrons

Infrared spectroscopy

The entry required to change how a molecule vibrates or rotates depends based on a fixed amazing of energy only works in polar bonds

Hybridization

Atomic sub levels hybridize to form averaging sub levels

Molecular orbital theory

Helps to explain how atomic original overlap in molecules to form covalent bonds

In molecular orbitals

Electrons are assisted to be delocalized not restricted to one atom

Bonding orbitals

Primary molecular orbital form lower in energy electrons shared between atoms

Anti bonding orbitals

Secondary molecular orbital form higher in energy electrons shared but repelled

Sigma

S sublevel

Pi

p sublevel

In a triple bond

There are 2 pi bonds and 1 sigma

In a single bond

There is 1 sigma bond

In a double bond

There is one pi bond and one sigma bond

Bond order

Predicts Bob strength takes resonance structures into consideration

Bond order formula

Bonding electrons - anti bonding e/2

electron negativity

Increased side to side decreases downward

Why electron negativity increases across

Nuclear charge rises but shaking stays roughly constant bigger magnet atomic radius decreases

Why electronnegativty decrease downward

More Everton shells increased shielding larger radius

Formal charge

The charge assigned to an atom in a molecule assuming all electrons are shared equally regardless of electron negativity

Ideally

We want every atoms to have a formal charge of o

Boron

Bo inns most stable structure is comprised of of 3 single bonds not double bonds