Chem Exam 2

constitutional isomers (structural)

same chemical formula but atoms connected in different ways

geometric isomers

compounds have the same formula but their arrangement is different

conformers

sp³ # p orbitals

0

sp² # p orbitals

1

sp # p orbitals

2

sp³ shape

tetrahedral

sp² shape

trigonal planar

sp shape

linear

sp³ bond angle

109 degrees

sp² bond angle

120 degrees

sp bond angle

180 degrees

formal charge equation

# valence electrons - # nonbonding electrons - # bonds

neutral molecule formal charge

0

what does a higher electronegativity mean

an atom has a stronger pull towards electrons

what happens to the bond length when the bond order increases

it decreases

if a bond is lower does that mean it has more or less strength

less

bond lengths

internuclear distance when potential energy well hits minimum

constructive overlap

destructive overlap

bond order formula

(# bonding electrons - # antibonding electrons) / 2

molecular orbital theory

valence bond theory

atomic orbitals combine to form hybridized orbitals which then lets them form covalent bonds w/ atoms next to them

cis isomers

same group on same side of molecule

trans isomers

same group diagonal on molecule

bonding orbitals

created by in phase combination and makes lower energy orbitals

antibonding orbitals

created by out of phase combination and makes higher energy orbitals and have the star

if you add electrons to bonding orbitals what happens to the bond order

inc it

if you add electrons to antibonding orbitals what happens to the bond order

dec it

unsaturated

has a double bond, triple bond, or a ring

sigma bond

formed by head on orbital overlap + every bond has ONE

pi bond

formed by side to side overlap of 2 p orbitals + happen in double + triple bonds + stop rotation from happening bc it’d break the side to side overlap

whats the longest bond

single bond

whats the strongest bond

triple bond