Chem unit 3

C6H12O6

Glucose

1 cal

energy required to raise temp of 1g of water by 1 degree Celsius

1 kilocall

1000 cal

In reactants

Bonds break, which requires energy

Energy absorbed (goes in)

In products

new bonds are formed, meaning energy is released

Enthalpy

ΔH total energy stored in a substance

Used to know how much heat is absorbed or released in a physical/chemical change

Endothermic

Hr>Hp

ΔH (+)

energy/heat goes in

Test tube cools

Energy to break reactant bonds > energy to form product bonds

Exothermic

heat exits

ΔH(-)

(Hr<Hp)energy to break reactant bonds < energy to form product bonds

Spontaneous

a reaction that can proceed without energy input

Gibbs free energy ΔG

predicting whether a chem reaction will happen naturally or is energy needed

ΔG(-)

the reaction is spontaneous/can happen on its own

ΔG(+)

reaction is non spontaneous/energy is needed

ΔG (0)

reaction is at equilibrium

Entropy Δ S

measure of disorder

entropy increases

more disorder

entropy decreases

less disorder

Exergonic reaction

releases free energy into the surroundings

spontaneous

ΔG(-)

Endergonic Reaction

requires a free energy input

nonspontaneous

ΔG(+)

faster reaction

lower activation energy means

catalyst

speeds up reactions by lowering the Ea

regenerated in reaction

Ketone

carbonyl in middle of chain

Aldehyde

carbonyl at the end of the chain

carbonyl

Carbon double bonded to oxygen

Oxidation (ORG CHEM)

increase in the number of C—O bonds

Reduction (ORG CHEM)

decrease in the number of C—O bonds

most oxidized carbon

has to be parent when naming molecules

more oxidized

more oxygen bonds

cellular respiration

exothermic

spontaneous

ΔS(+)

Matter

pure substance or mixture

concentration

solute to solvent ratio

isotonic

equal

hypotonic

swollen cell

concentration outside is lower

Hypertonic

shriveled cell

concentration outside higher

Equivalents

based on charge

Equilibrium

rate of forward + reverse reactions is equal, meaning concentration of products and reactants doesn’t change

equilibrium constant K

gives a measure of a reactions completeness

k=1

the concentration of reactants = concentration of products

k>1

equilibrium favors products

k<1

equilibrium favors reactants