Chem Exam 3

catalyst

speeds up reaction

synthesis reaction

small molecules/atoms combine to create larger one

decomposition reaction

break apart larger molecules into smaller molecules

exchange reaction

synthesis and decomposition (single/double)

reversible reactions

forms product in either direction

chemical equilibrum

point where forward and reverse reaction are occuring at the same time

irreversible reactions

reactions that are highly exothermic and can’t be reversed

redox reactions

single replacement

oxidation

addition of oxygen, loss of energy/electrons

reduction

addition of hydrogens, energy/electrons

reducing agent

oxidized species

oxidizing agent

reduced species

cations

metals lose electrons (oxidized)

anions

nonmetals gain electrons (reduced)

condensation

two molecules joined, water is produced

hydrolysis

water is reactant and split into two molecules

carboxylation

addition of carboxyl

hydrogenation

2 hydrogens added, doubles bonds become single

trans fats

compounds where double bonds reform in energetically stable trans form

hydration

addition of H20 to alkene double bond, requires enzyme

markvnikov’s rule

H bonds to carbon with more hydrogen atoms and OH bonds to carbon with more carbon groups in an asymmetric alkene

monosaccharides

one sugar, cannot be broken down, C/O/H

generic monosaccharide formula

C_n(H₂O)_n

polysachharide

10+ monosaccharides joined together (continuous or branched)

aldose

monosaccharide containing aldehyde group

ketose

monosachharide containing ketone group

entantiometers

compound with single chiral center/ 2 stereoisomers

fischer projection

horizontal lines on chiral center represent wedges, vertica lines represent dashes

D-sugars

OH on chiral carbon farthest from carbonyl on the right

L-sugars

OH on chiral carbon farthest from carbonyl on the left

diastereomer

stereosiomers that are not exact mirror images (not all chirals flipped)

pressure

force exerted against a given area

atomsphere

unit for air pressure

pascal

SI unit

psi

pressure as a force

mmHG

blood pressure unit

gas properties

mostly empty, weak attractions, homogenous, easily compressed, unrestricted motion

ideal gas

gas that perfectly adheres to kinetic molecular theory

kinetic molecular theory

empty space, no attractive forces, constant random motion, kinetic energy proportional to temperature

boyles law

volume of fixed amount of gas is inversely proportional to pressure

charles law

volume of fixed amount of gas is directly proportional to absolute temp

gay-lussacs law

as temp increases, so does pressure

combined gas law

(P1xV1)/T1 = (P2xV2/T2)

vapor pressure

pressure of molecules above liquid