CHEM final exam (grade 12)

SOme rules of naming compounds

-fINd the longest chain

-name so you have the smallest numbers possible

- //: -#- enes

- ///: - # - ynes

• alphabetical order (chaines)

naming format

cycloalkane

__ ,__- ____ylcyclo____

ex. 1-methyl-3-ethylcyclohexane

cycloalkane

_ ,__- _cyclo____yl ______

ex. 1-cyclobutylpentane

Aromatic hydrocarbon

_ ,__- ____ylbenzene

ex. 1-ethyl-3-methylbenze

Aromatic hydrocarbon

_ ,__- _phenyl______

ex. 1-phenylpentane

haloalkanes

__- _(F/Cl/Br/I)_____

• fluoro, chloro, bromo, iodo

ex. 3-bromo-6-chlorooctane

Alcohol (R-OH)

__- ____yl___- (c #0)- ol

ex. butan-2-ol

Carboxylic acid

__- ___yl_____oic acid

ex. pentanoic acid

Aldehyde

__- ____yl___al

• O= determines the root chain

• alwayd on the end so no numbers needed (At end)

ex. 2-methylbutanal

Ketone

• O= determines root chain

• O is prioritized

• drop the e at the end

__- ____yl___- (c #0)- one

ex. propanone

Ester

• root chain is determined by O=

short chain-_-____yl rootcahin oate

ex. ethyl-3-methylbutanoate

Ether

(the # C that O is attached too on the longest chain) short chain oxy-_-____yl root chain

• O is prioritized

ex. 1-methoxy-4-methylpentane

Amine

N-_chain_-N- chain root chain - (the # C that N is attached too on the longest chain) - amide

ex. N-ethyl-N-methylbutanamine

Amide

N-_____-__-______________________amide

ex. N,N-methylbutanamide

what happens in an addition reaction?

the double / triple bonds break

Alkenes

C=C + X-Y —> X-C-C-Y

Alkynes

• if limited ≡ —> =

• if excess ≡ —> -

Multiple Products

2 possible products

C=C-C + X-Y —> C^X-C^Y-C or C^Y-C^X-C

Markovmikov’s Rule

Unsymetrical:

Major (H is added to the carbon with the most H)

Minor (H is added to the carbon with the less H)

What happens in an elimination reaction?

forms double bonds

CH₂^X-CH₂^Y —> CH₂=CH₂ +X-Y

• Alcochols perform with strong acids (H₂SO₄)

• Haloalkanes preform under strong bases (NaOCH₂CH₃)

Major/Minor law / anti markovnikov rule

is the double bond can be formed in more then one place, then the H will be removed from the carbon with the most carbons attached to it (major)

what happens in a substituons reaction?

they swap

what happens in a condensation reaction?

2 molecules combine and form larger molecule + H2O

what happens in an estérification reaction

condensation reaction between carboxylique acid and alcohol

what happens in a hydrolysis reaction

ester + water —> carboxyic acid + alcohol

what happens in an oxidation reaction?

gains O lose H (alcohol + [O])

1^o. -OH + excess [O] —> aldehyde —> carboxylic acid

2^o. -OH + excess [O] —> ketone

3^o. -OH + [O] —> N.R.

what happens in a reduction reaction ?

• gains [H] lose O (K,A, or CA + [H] makes -OH)

what happens in combustion reactions?

• complete: hydrocarbon + O2 —> CO2 + H2O + energy

• incomplete: hydrocarbon + O2 (insufficient) —> C + CO + CO2 + H2O + energy

what happens in a polymer addition reaction?

reduces carbons double bond and makes a pattern

what happens in a polymer condensation reaction?

takes an OH off of one and H from the other to make H2O and a pattern

john dalton

described that matter is made up of small indestructible and indivisible shares (atoms)

JJ Thomson

used glass discharging tubes with trace amounts of gas and passed an electric current though it. rays appeared, which curved with a magnet showing they were negatively charged. (found out there was a + and - charge in a atom) (plum pudding boy)

Ernest Rutherford

Fired alpha particles at a thin sheet of gold surrounded by zinc sulfuric coated screen that light up when hit with alpha particles. some particles had a large particle deflection, meaning most of the mass and all positive charges surround a very dense center (nucleus) while electrons orbit around it.

(nuclear model)

what happens to element when they are energized

they give off specific wavelength of light

Niels Bohr

• electrons orbit like planetary orbits

• the force that holds electrons together is electrostatic force betweent and - charges on electrons

• electrons only exist in energy levels

• electrons can jump between energy levels by absorbing or emitting energy

• planetary model (didn't explain larger atoms)

what are the quantum numbers and do they describe

• n, 1, ml,: describes the distribution of electrons in atoms

• n: energy levels and size

• I : shape

• ml: 3D orientation

• ms: behaviour of specific electron

charaistics of n

• tells you the energy level and size of orbital

* (all orbitals with the same value of n are in the same shell/energy level)

• greater value of n means greater probability of finding an electron farther from the nucleus

• electrons can jumps to different levels of n (absorlos energy when it goes up, and releases it when goes down)

stuff about I

• shape of orbital

• also callEd sublevels or subshells

• 1 = n-1 (possible values)

• 0=5, 1=p, 2=d, 3=f

stud about ml

• Choose from -I to +l, indicating the 3D orientation of orbitals. The total number of orbitals for an energy level n is n²

pauli exclusion principle

• no 2 electrons around an atom can have the same 4 Q numbers (electrons in the same orbital have same 3 Q's but different spins)

Aufbau principle

electrons occupied the lowest energy orbitals first

hunds rule

the lowest energy level of a atom has the max amount of unpaired allowed

ionic bonds

• metal + non-metal

• metals lose there electrons and non metals gain

• opposites attract and form a crystal lattice

covalent bonds

non metal + no metal

metallic bonds

• metal + metal

• since 2 metals have a valance shell that are less then 8, they create a sea of valence electrons

• low EN

• valence electrons move freely from one atom to the next

Valance bond theory

a covalent bond (share electrons) forms when the orbitals of 2 atoms overlap and share a common region in space where a pair of electrons are

Hybrid orbitals

formed by the combination of 2 or more orbitals in the valence shell of an atom.

PI bonds

covalent bonds formed by the overlap of P orbitals/formed from double bonds

VSEPR Theroy

• valance shall electron pair repulse theory

• electron groups around an atom are positioned as far away from each other

(electron groups are lone pairs, single, double and triple bonds)

first law of thermodynamics

energy cannot be created or destroyed only transferred

second law of thermodynamics

when objects are in thermal contact that heat will be transferred from the object will the higher temperature to the object with the lower infill both objects have the same temperature and reach thermal equilibrium

what are the 6 Factors Affecting Reaction Rate

• Nature of the reactants

• Concentration of solution

• Temperature

• Pressure of Gases

• Surface area of the particles of a solid

• Presence of a catalys

Keq’s relation to one

Keq >1 favoris products

Keq < favours reactants

change in concentration (product up and down)

product ⬆ more reactents formed

product ⬇ more product formed

change in pressure

pressure ⬆ more/shift towards side with fewer particles

pressure ⬇ shift to side with more particles

Temperature increase

Toward endothermic reaction → Endothermic forward reaction Keq Increases

Temperature decrease

Toward exothermic reaction → exo increase keq

Properties of Ionic compounds

◼ Crystal Lattices

◼ High MP and BP (In the range of metals [some above some below])

◼ Soluble (positive and negitve meds of ploles)

◼ Hard and Brittle (With enough force, the ions can “shift” and now repel.)

◼ Conductive if dissolved in water (so ions to move and conduct electricity)

Intramolecular bonds

exist within a molecule.

Intermolecular forces

Dipole-Dipole

Dipole induced dipole

Dispersion forces aka Van der Waals forces

Dipole-Dipole

When a covalent molecule is polar it has a permanent dipole

These dipoles can line up and cause attraction to each other

Induced Dipole

Bringing a polar molecule near a non-polar one can induced a dipole.

The molecules than have a small attraction to each other.

Dispersion Forces

Attractive forces between non-polar molecules.

Electrons orbit nuclei and cause brief momentary (but ongoing) moments of slight polarity.

Temporary dipole.

Very weak, but when many occur at the same time, can have a significant effect.

structure isomère

same formula diff shape

distereomer

same formula different properties

anti imores

mirror images