chem mistakes

attractive forces among molecules cause increases/decreases in P in ideal gas law

lower P (not as many collision)

nonzero volume of molecules cause increases/decreases in P in ideal gas law

increase (more collisions, less volume means up P)

ideal gas conditions

high temp and low pressure

a larger surface area of reactants = faster/slower rxn

faster since more of reactant is exposed to the rxn

smaller pieces or ribbon react faster

smaller pieces bc more exposed surface area

when titrating a polyprotic acid, which H comes off first

the more acidic one (attached to a more electronegative atom)

stronger acid = stronger/weaker bond with H

weaker bond

strength of oxoacids depends on

1.number of oxygens per H (more=stronger) and 2. the electronegativity of the other atom.

if an acid has more oxygens, it is more/less stable

more

electronegativity and bases

more electroneg = weaker bc more electroneg means it attracts e- more/not as willing to let go and thus not as willing to grab onto protons = weaker base

the more stable an anion, the stronger/weaker the acid (what makes an acid stable?)

more oxygens = more pull on O-H bonds = weaker = less stable acid = stronger acid

delta G

G standard + RtlnQ

what makes an acid stronger?

weaker and more polar bonds

bond order

number of bonds/ number of location