Chemistry of Life Ch. 2,3,4,5

matter

takes up space and has mass

compounds

2 or more elements in a fixed ratio

matter made up of elements _____ be broken up by chemical reaction

cannot

trace elements

minute quantities

element

unique atomic structure

atom

smallest unit of matter

radioactivity

neutrons split up into proton and electron

isotope

same # protons different # neutrons

groups

# valence electrons

periods

electronegativity

4th group

contains carbon and shares electrons forming chain

groups 5-8

accept electrons (to form anions -)

groups 1-3

donate electrons (to form cations +)

radioactive isotope

high energy/randomly give off particles and energy

rule for atom’s electrons (and what is n)

2n² (energy level #)

energy

capacity to bring about change

potential energy

energy stored in bonds/passed by matter due to structure

covalent bonds

sharing electrons

H+

proton/hydrogen without its electron

molecule

2 or more atoms held by covalent bonds

what bonds can hydrogen and carbon form (they are different)

H - single, C - up to quadruple

electronegativity

wanting electrons more or less

polar covalent bonds

electrons shared unequally (different electronegativity)

non-polar covalent bonds

electrons shared equally (same electronegativity)

electrostatic attraction

attraction between a cation (+) and an anion (-)

salts

ionic compounds

weak chemical bonds

attraction between molecules

hydrogen bond

H atoms covalently bonded to electronegative atom and attracted to electronegative atom

van der waals

transiently ± regions of molecules attract

shape of molecule determines ________

function

chemical reaction

making and breaking bonds

catabolic

big to small energy released (+)

anabolic

small to big energy stored in bonds (-)

equillibrium

forward and backward reaction at the same rate

sun is ______

expanding

water is a _____ molecule

polar

cohesion

attraction of like/same molecules

water moderate temperature by ______ heat and ______ it

absorbing/releasing

kinetic energy

energy of motion

heat

total kinetic energy due to molecular motion

temperature

measures of heat

specific heat

heat absorbed or lost for 1g to change temperature by 1C

evaporation

liquid to gas

water has _____ heat of evaporation

high

insulation

lower density of ice allows for it to float and form a crust on top insulating bodies of water

water is a ______ solvent due to its _______

versatile/polarity

acids

donate H+

bases

accept H+ or donate OH-

pH determined by _______ of ________ ions

concentration/hydrogen

buffers

limit changes in OH- and H+ concentration

mass number/atomic mass

sum of protons and neutrons

atomic number

number of protons

atomic weight

average mass of an element’s isotope

ionic bonds

electronegativity of interacting elements is drastically different so one rips an electron away from the other (now attract to each other because they are oppositely charged)

hydrocarbon

found in cell molecules

isomers can differ in three ways

structural, geometric, enantiomers

isomer

molecules (differ in properties)

isotope

elements (same properties)

hydroxyl

OH (alcohol)

Carbonyl

CO (sugar)

Carboxyl

COOH (organic acid)

Amino

NH3 (protein)

Sulfhydryl

SH (protein)

Phosphate

PO4 (nucleotides)

adhesion

water clings to cell walls resisting gravity

surface tension

measure of how difficult it is to stretch or break the surface of a liquid

heat of vaporization

quantity of heat a liquid must absorb for 1g of it to be converted from liquid to gas

evaporative cooling

water’s ability to cool a surface because fastest moving molecules evaporate leaving slower ones behind causing cooling

solute

substance that is dissolved

solvent

substance that dissolves another substance

aqueous solution

water is the solvent

hydrophilic

aphinity for water

hydrophobic

with no aphinity for water

colloid

stable suspension of fine particle in a liquid

hydration shell

sphere of water molecules around each dissolved molecule

molarity

number of moles for solute per liter of solution

carbonic acid buffer system equation and how it works

H2CO3 →← HCO3- + H+

when blood is too acidic (too much OH-) carbonic acid breaks apart to form carbonate ion and hydrogen ion that binds with OH- to form H2O

brackets indicate _____ concentration

molar

macromolecule

polymers built out of monomers

lipids are ______ polymers because they are ________ made of _______ ________

not/macromolecules/finite/subunits

polymers

long molecules made up of monomers

dehydration synthesis/condensation reaction

process that joins monomers through combining the H+ and OH- of two monomers

endothermic/anabolic/endogonic

reaction resulting in energy storage of making a bond

hydrolysis

breaking bonds by adding water and releasing energy

catabolic/exothermic/exergonic

reaction resulting in energy release and breaking of bonds

carbohydrates H:O ratio

2:1 always

empirical formula of carbohydrates

CH2O (monosaccharides)

monosaccharide

sugar whos name ends in “os“ derived from carbon 

n=3 trios

n=4 quantos

n=5 pentose etc.

types of carbohydrates

monosaccharide:

• trios

• quantose

• pentose

• hexose

oligosaccharide:

• di

• tri

• tetra

• penta

polysaccharide

• glycans

sugars can be in _____ or _______ form

straight/ring

pyran

hexagonal

furan

pentagonal

— O —

ester bond

starch flag placement

6th c

cellulose flag placement

6th and 4th c

glycogen flag placement

non-linear

flag molecule

CH2OH

protein monomer

amino acid

amino acid make up

amino group and carboxyl

protein structures

primary, secondary, tertiary, quartery