General Chemistry

1.6 x 10^{-19 C}

• same # of protons
• different # of neutrons

reducing agents

tend to lose e^-

family

• n = energy level
• l = shape of orbital

• - ide
• - ite
• -ate

• "hypo" = first
• "per" = last

increases size and energy of e^- orbital

• same 1st 3 numbers, different 4th:
• same shell (n), subshell (l), orbital
• different spin (+1/2) or (-1/2)

amt. of energy released when an e^- is gained

ability of atom to draw in e^- from a bond

increases right to left, bottom to top

diagonally left and right

increases left to right, bottom to top

increases left to right, top to bottom

(right diagonal down)

van der Waals

larger atoms - further away

temporary dipole-dipole moment

• H bonding
• dipole-dipole
• van der Waals

• 0^oC (273K)
• 1 atm (760 torr)

22.4L

• 1. zero volume
• 2. no forces other than repulsive in collision
• 3. elastic collisions
• 4. avg. KE proportional to temperature

no

8.314 J

avg. KE is proportional to temperature

ideal

when molecules are close together

high temperature and low pressure

(so molecules are far apart)

monoatomic

monoatomic

pinhole - spreading from high to low pressure

gases with higher rms velocity

spreading into another gas or empty space

P_A = X_A times P_total

KE = ³/₂ RT

increase PE

molecules bind together more

no, only their average kinetic energies

they have different molecular weights

velocity₁/velocity₂ = sq. root (mass₂/mass₁)

reversed subscripts

reversed subscripts

inversely proportional to sq. root of their mass

H₂ because it's lighter

weak intermolecular forces

[reactants] increases

temperature increases

constant

• kinetics = rate (getting to state)
• thermodynamics = G, S, H (prop. of this state)

• conduction
• convection
• radiation

molecular collisions

• conducts heat from hot to cold reservoir
• (higher energy to lower energy)

• doesn't matter -
• same regardless of length

increase distance = increase temperature difference

constant

fluid movement

electromagnetic waves

energy transfer that is not heat

W = -P x change in V

0

no work is done

E = q + W

since no work, E = q

W = -q

E = 0 because E is proportional to T

• into (-)
• out of (+)

H = change U + P changeV

H = E

change in enthalpy when a compound is formed from raw elements

H = change U + P change in V

H = W + U

H = 0 J/mol

• endothermic (+) - absorbs heat
• exothermic (-) - releases heat

greater in endothermic

standard state elements - O₂ H₂

positive

delta S = Q/T

energy transfer/temperature

hot = negative (energy is leaving system)

cold = positive (energy is entering system)

positive

entropy of universe must always be > 0

increases entropy

increase in entropy

universal entropy (not entropy of system)

positive (more disorder)

• exergonic = spontaneous
• endergonic = non-spontaneous

• (-) = spontaneous
• (+) = non-spontaneous

energy available to do work

delta G = delta H - Tdelta S

negative free energy = spontaneous

because universe tends towards greater disorderedness

delta G = -RT lnK

K = 1

products and reactants are equal

• (-) G = K > 1
• (+) G = K < 1

reactants are favored

products are favored

moles/Liter

moles/kg

1L = 1kg of water

55.5 moles

solution = more disordered = inc. entropy = decrease G

• [products]^coefficients /
• [reactants]^coefficients

leave them out

# moles/ L

increases solubility

increases solubility of salts

decreases solubility

measure of energy change needed to change temperature of substance

no work (W=P change in V)

yes because substance can expand, so substance absorbs energy

q = C x change in T

q = mc change T

Yes

1 cal/g^oC

1 calorie = 4 joules

yes, but either temperature or heat, not both

decreases vapor pressure

decreases boiling point

iMRT

Molarity x 0.8 x T x i

delta G = H - TS

not much influence

electrolytes,

able to conduct electricity

yes, polar conductor

unless it contains electrolytes

completely

will produce 0.2 moles of Na+ 0.2 mol of Cl-

intermolecular forces

have enough KE (for a gas)

force some mol. to crash back down

eq. = same # leaving and returning

negative = stronger bonds are formed

positive = weaker bonds are formed

strong = lowers vapor pressure

weaker = raises vapor pressure

concentration of dissolved salt reaches maximum

increased vapor pressure = decrease in boiling point

strength of intermolecular forces

melting

boiling

endothermic

heat is being added, temperature increases

solid to gas

gas to solid

solid to liquid (melting

liquid to solid (freezing)

exists in equilibrium as a solid, liquid, gas

temp. where a substance cannot be liquefied

pressure required for liquidification at critical temp.

critical temperature and critical temperature

boiling point

accepts/donates e^-

donate/accept H+

acts as either acid or base

diprotic acid

acids that can donate more than one proton

all strong bases

completely dissociate

decreasing polarity

decreasing bond strengh

increasing acidity

stronger acids

O draws e^- to one side, increasing polarity

• left = basic
• right = acidic

increases right and down

binary compounds = only 2 elements

pH = -log[H⁺]

pOH = -log[OH^-]

pH + pOH = 14

strong acids and bases dissociate completely in solution -

[H⁺] and [OH^-] are the same as original conentrations

requires K_a

pH = 0

because [H⁺] = 1 and 10⁰ = 1

K_a = [H⁺][A^-] / [HA]

strong acid

pK_a = -log[K_a]

small pKa = large K_a

small pK_a = strong acid

acids and bases combine exothermically to from water + salt

M_initialV_initial = M_finalV_final

look at conjugates of ion

conjugates = NaOH and HCl

both strong, so Na⁺ and Cl^- is neutral

flat plateu

all acid has been converted to base

100% A^-

7

EP < 7

pH > 7

[acid] = [base]

have more than 1 EP and more than 1 1/2 EP

once the 1st proton has completely dissociated

no change in pH upon addition of acid or base

1/2 equivalence point

because [HA] = [A^-]

pH = pK_a + log[A^-]/[HA]

[HA] = [A^-] so pH = pK_a

mix equal amounts of acid with conjugate base

basic = red to blue

acidic = blue to red

when indicator changes color

loss of e^-

gain of e^-

LEO the lion says GER

• F = -1
• H = +1
• O = -2

poor oxidizing and reducing agent

• balance other elements
• H₂O - balance O
• H⁺ - balance H
• e^- - balance charge

chemical energy to electrical energy

• T = terminals
• E = electrodes
• I = ionic conductor

ionic conducting phase

carries current (in the form of ions)

electric potential difference from T to T

• anode = (-)
• cathode = (+)

RED CAT - AN OX

reduction cathode - anode oxidation

positive cell potential (E)

potential difference between terminals when they're connected

reduces potential difference

Anode l Anoic solution ll Cathodic solution l Cathode

delta F = -nFE

number of moles

Faraday's constant:

100,000 C/mol

E = E^o (RT/nF) lnQ

E = 0

because no rxn is favored

identical electrodes whose half cells have different ion concentation

toward greater entropy

require force by outside power source

2H⁺ + 2e^- > H₂ E = 0

position and momentum

photon is released

(energy is released in form of a photon)

E = hf

e^- is bumped to a higher energy state