orgo test 1

organic chemistry

living things, carbon containing

molecular formula

tells you what atoms and how many (NOT connectivity)

constitutional isomers

same molecular formula, different connectivity

how many valence electrons and bonds are in carbon

4

how many valence electrons and bonds are in nitrogen

5 and 3

how many valence electrons and bonds are in oxygen

6 and 2

lone pair

electron pairs not in a bond

valence electrons

outermost electrons used in bonds and reactions

octet rule

elements are stable with 8 electrons (hydrogen is an exception)

single bond

bond with 2 electrons

double bond

bond with 4 electrons

triple bond

bond with 6 electrons

electronegativity

how much an atom draws electrons towards it, increase as you go up and to the right

polarized bond

electrons are not shared equally, EN 0.5-0.7

nonpolar covalent bond

electrons are shared equally, EN <0.5

ionic bond

EN >0.7

atomic orbital

the 3d plot of a wave function, cloud of electron density

electron density

probability of finding an electron

aufbau principle

electron fill atomic orbitals from lowest to highest energy

pauli exclusion principle

electrons don’t have the same spin

hunds rule

every orbital has to have 1 electron before it can have 2

charge of carbon with 3 bonds and a lone pair

negative 1

charge of carbon with 3 bonds

positive 1

charge of nitrogen with 2 bonds and 2 lone pairs

negative 1

charge of nitrogen with 4 bonds

positive 1

charge of oxygen with 1 bond and 3 lone pairs

negative 1

charge of oxygen with 3 bonds and 1 lone pair

positive 1

induction

induction

where are carbons in bond line drawings

where lines meet and end

sigma bonds

when sp2 orbitals overlap, single bonds

pi bonds

when p orbitals overlap, double bond, weaker than sigma bond (by itself)

sp3

connected to 4 things, 1 s-character and 3 p-characters

sp2

connected to 3 things, s-character and 2 p-character

molecular geometry

only for atoms bonded to central atom

dipole moment

amount of partial charge x the distance of partial charges

debye (D)

units for dipole movements

dipole-dipole

when polar molecules line up their opposite charges

hydrogen bond

strong dipole-dipole, when hydrogen is bonded with N, O, F

London-dispersion forces

induced transient dipole moment, produces a weak fleeting attachment, higher mass has ahigher

functional groups

collection of atoms in a molecule that have a particular reaction and properties

Alkyl halide group

R-X (Cl, Br, I)

Alkene

Alkyne

alcohol

keytone

aldehyde

carboxylic acid

acyl halide

ether

thiol

sulfide

aromatic/benzene ring

anhydride

ester

amide

amine

localized electrons

belong to one atom, can’t create resonance structures

delocalized

electrons that can be spread across multiple atoms, used in resonance structure

resonance structures should not

break sigma bounds, have different overall charges, or break octet rule

allylic position

electron pair next to a carbon double bond

what makes a resonance more significant

more octects, negative charge on EN atom, positive charge on less EN atom