CHEMMMMMMMMMMMMMMMMMMMMMMMMMM (conversion factors)

FIVE BIG BOOMS FOR TYSOEE

Celsius to Farenheit

add 32

Farenheit to Celsius

subtract 32

1 Kelvin

273.4 C

1 Kilometer

0.6214 miles

1 Liter

0.264 gallons

1 cm

0.393701 in

AVOGADRO’S NUMBER

6.022 × 10²³

Properties of Ionic Compounds

1. Contain positive and negative ions

2. Sum of cations = sum of anions

3. Formula reflects smallest whole number ratio of ions

4. Usually form between a metal (cation) and nonmetal (anion)

5. Named using (name of first compound)+(second compound prefix + ate, ide, ite)

Properties of Covalent Bonds

1. Between a metal and a nonmetal

2. Electrons are shared between elements

3. Uses prefixes that indicate number of each element

Rules for Acid Naming

1. Begins with H = acid

2. ite becomes ous

3. acid at end

Relationship between wavelength and frequency

smaller wavelength = greater frequency

Relationship between wavelength and energy

shorter wavelength = greater energy

energy from photons

E=hc/(wavelength)

Relationship between velocity and wavelength

shorter wavelength = greater velocity

equation to find wavelength from velocity

(wavelength) = h/mv

Rydberg Formula (1/(wavelength)(1/n1² - 1/n2²)

used to find the wavelength from one orbital to another

Energy Difference

hc/(wavelength)

Coulomb’s Law (F=k((q1q2/r²)

1. Similar charges repel, opposite charges attract

2. Repulsion varies inversely with the distance between the particles

3. Greater charge magnitude results in stronger attraction

4. Potential energy is proportional to the product of the two charges divided by the distance between them.

Nuclear Charge

1. Valence electrons are more shielded from nuclear charge than core electrons

2. Overall determined by # of electrons

Quantum number assignments

n = 1,2,3,4,5,6,7 (corresponds to principal level)
l = maximum value is (n-1), 0=s,1=p,2=d,3=f

number of orbitals = 2l+1
ml = range is (-l to +l)
ms = spin number - spin up (1/2) or spin down (-1/2)

diamagnetic atom

all orbitals are full

trends for metallic character

decreases as we move to the right, increases as we move down.
Decreases with increasing ionization energy.

what happens when a second-column atom loses two electrons?

full octet! full octet! Used when drawing Lewis structure!!!!!!

Elements that do not always follow octet rule?

Boron, Aluminum, Beryllium

Difference in ionic and covalent bonding

covalent - typical Lewis structure
ionic - transfers electrons, usually have different charges

For sequences that define where an electron is

a positive charge means that the corresponding number of electrons is subtracted from the orbital of the highest value.
A negative charge means the corresponding number of electrons are added to the current orbital or the next one.

Rules for lattice energy

Magnitude increases with increase in ionic charge, decreases with increasing ionic radius

molecular geometry

shape of electrons around central atom

What is one way to determine polarity?

ELECTRONEGATIVITY; higher difference in electronegativity means more polarity

exothermic

more energy is released (negative hrxn)

endothermic

more energy used to break bonds than form them (positive hrxn)

2 bonding points, no lone pairs

linear

3 bonding points, no lone pairs

trigonal planar

3 bonding points, one lone pair

bent

four bonding points, no lone pairs

Tetrahedral

four bonding points, one lone pair

trigonal pyramidal

four bonding points, two lone pairs

bent

5 bonding points, no lone pairs

trigonal bipyramidal

five bonding points, one lone pair

seesaw

five bonding points, two lone pairs

t-shaped

five bonding points, three lone pairs

linear

six bonding points, no lone pairs

octahedral

six bonding points, one lone pair

square pyramidal

six bonding pairs, three lone pairs

square planar

Determining Redox Reactions in an acid

1. Assign oxidation states (charge)

2. Separate the halves to form two separate reactions

3. Balance the elements besides H and O, then balance H and O.

4. Balance with respect to charge - make the charges equal by adding electrons to both sides.

5. Make the numbers of electrons equal on both sides by multiplying by a small whole number.

6. Add the reactions together and verify that it is balanced.

Balancing redox reactions in a base

1. Assign oxidation states

2. Separate the overall reaction into two half-reactions

3. Balance each half-reaction with respect to mass

4. Balance each half reaction with respect to charge. Balance O by adding H2O, and H by adding H+, and add as many OH- ions as H+ so they cancel out.

5. Make the number of electrons equal in both half-reactions

6. Add together and verify.

NIO PIR

More Negative is Oxidation
More Positive is Reduction

1 mmHg

1 torr

1 atm

760mmHg

1 atm

1.01325 bar

1 Pa

10^-5 bar

1 in

2.54 cm

1 cm

10 mm

q = C(T)

q = constant of proportionality
C = Heat capacity
T = change in temperature

C = q/T = j/C

calculating heat capacity

Relationship between mass, heat capacity, heat, and temp.

q = mCT

Fix for a gaseous cylinder: w = F X D

F = Pext X A X D(or h)

qcal = ccal X T

H = E + PV

=qp

exothermic reaction

-H

endothermic

+H

Boyle’s Law

V = 1/P

P1V1 = P2V2

Relationships between pressure 1 and pressure 2

v1/t1 =

v2/t2

v1/n1 =

v2/n2

P = n(RT/V)

Part of partial pressure equation

Law of partial pressures

Directly related to molarity

Add them all together

Kp

Kc(RT)^(c+d-(a+b))

Qc = (molesA)(molesB)/moles(C)moles(D)

How to find Q

Q<K

reaction goes towards right

Q>K

reaction goes to the left

Q=K

Reaction is at equilibrium

Effects of temperature change on Equilibrium

Increasing the temperature causes an exothermic reaction to shift left.
Decreasing causes it to shift right.

Effect of Volume change on equilibrium

Decreasing volume causes reaction to shift in the direction of fewer moles.

Increasing the volume causes the reaction to shift in the direction that has the greater number of moles of gas particles.

Acid

Donor

Base

Acceptor

Relationship between the acid and base

Stronger acid = weaker conjugate base

pH

-log[H3O] [concentration]

Ratings for acidity

pH>7 - acidic
pH<7 - basic
pH = 7 - neutral

p[OH]

-log[OH-]

Kw

[OH-][H3O+]

paramagnetic

unpaired electron

What do we place in the Ka and Kc equations?

Molar concentration you absolute buffoon

Alkanes

Single C-C bonds

Alkenes

Double C-C bonds

Alkynes

Triple C-C bonds

CH3

methyl

CH2CH3

Ethyl

CH2CH2CH3

Propyl

CH2CH2CH2CH3

Butyl

CHCH3-CH3

Isopropyl

CH2CHCH3-CH3

Isobutyl

CHCH2CH3

CH3

CH3-CCH3-CH3

tert-butyl

Alcohols

ROH

Ethers

ROR

Aldehydes

RCHO

Ketones

RCOR

Carboxylic Acids

RCOOH

Esters

RCOOR