Matter
Atom
Element

Isotopes


Pure substance

Compound
Molecule
Chemical Bond
Ionic bond
Ion
Covalent bond / THE CHEMISTRY OF LIFE
  • anything that has mass and takes up space.
  • basic unit of matter.
100 million atoms = 1 cm.
contains subatomic particles:
proton: + charge, found in nucleus.
neutron: no charge, found in nucleus.
electron: - charge, orbits nucleus.
atoms are neutral: #protons = #electrons.
atomic number = #protons = identity of element
atomic mass = #protons + #neutrons.

  • atoms of element with different # neutrons
all isotopes have same properties.
radioactive isotopes
unstable nucleus breaks down and gives off energy = radiation.
uses: medical tracers, kill bacteria,
cancer treatment, etc.
  • matter made up of 1 types of particle.
e.g. salt, gold, sugar, water.
  • formed by combination of 2 or more elements.
properties of compound differ from those of separate elements.
e.g. Na: explosive solid in water.
Cl: poisonous gas.
NaCl: table salt
  • smallest particle of a compound.
chemical formula (e.g. H2O)
tells # atoms of each element in compound.
  • energy that holds atoms together in molecules.
involves outermost electrons.
  • electrons are transferred from 1 atom to another.
oppositely charged atoms attract = bond.

  • atom with charge.
if atom loses electrons (+ charged ion).
if atom gains electrons (- charged ion).
  • electrons are shared between atoms.
shared electrons orbit both nuclei.
Water is important
Why??
Polar

Hydrogen bonds

Cohesion

Adhesion

capillary action
/ WATER: THE ELIXIR OF LIFE
  • 75% of earth is water.
  • 98% is in liquid state
  • liquid, solid and gas found on earth
  • life began in water.
living things are 50-95% water.
  • covalent bonds betw/ H and O atoms.
uneven sharing of electrons.
  • O has slight – charge.
  • H has slight + charge.
  • O of one H2O attracts H of another H2O.
weaker bond than ionic or covalent bond.
  • H2O molecules “stick” to each other.
due to hydrogen bonding betw/ water molecules.
causes surface tension, droplet formation.
  • wqter molecules “stick” to other substances.
meniscus: H2O to glass attraction.
  • water moves in tiny tubes.
due to cohesion betw/ water molecules AND
adhesion to another surface.
  • e.g plants, filter paper, paper towels.

“Universal” solvent
Hydrophilic
Hydrophobic
Solution
Suspension
Density
Heat /
  • dissolves many other polar substances.
separates ionic substances into ions
  • “water loving” molecules like sugars dissolve in water.
  • “water fearing” molecules like fats don’t dissolve.
  • even mixture of 2 or more substances.
solvent = substance with greatest amount.
solute = substance with lesser amount.
  • mixture of water and undissolved material.
e.g. blood = water, cells, ions, platelets.
  • ice is less dense than liquid water.
living things able to survive winter in ponds.
  • heats up and cools more slowly than surroundings.
helps keep temps. constant for living things.
pH scale
Acid
Base
Neutral
Buffers / Acids and Bases
  • measurement system from pH 0-14.
indicates concentration of H+ in solutions.
  • compound that forms H+ ions in solution.
high concentration of H+ ions.
pH below 7.
e.g. stomach acid, lemon juice, etc.
  • compound that forms OH- ions in solution.
low concentration of H+ ions.
pH above 7.
e.g. bleach, detergents, etc.
  • concentration H+ = concentration OH-.
pure water = pH 7.
  • weak acids or bases that react with strong acids or bases to prevent sudden pH changes.
pH in body fluids must be 7.35-7.45.
buffers in organisms to maintain pH.
Organic compounds
Why is carbon special?

Macromolecule
4 groups of macromolecules in living things.
Carbohydrates
monomer
function
/ Chemistry of Carbon
  • contain carbon (CO2 is INORGANIC)
  • has 4 valence electrons
  • forms covalent bonds with many other elements
  • can bond to other carbons
chains, rings, sheets (graphite), tubes, spheres
  • can form millions of different compounds.
  • large molecule made of smaller subunits.
monomer: small molecules (subunits).
polymer: chain of monomers bonded together.
polymerization: process of making polymer
from monomers.
  • proteins, lipids, carbohydrates, nucleic acids.
  • made of C, H, N, O, P, S
  • made of C, H, O (1:2:1 ratio)
  • made by plants
  • monosaccharide = simple sugar
glucose, fructose, galactose
  • polysaccharide = long chains of monosaccharides
  • energy source and structure.
glucose: quick energy source: plants/animals
glycogen: short-term energy storage: animals
starch: short term energy storage: plants
cellulose: cell walls: plants (“fiber”)
Lipids
made of

function
Proteins

monomer
function
/
  • made of C, H, O (mostly C, H )
  • not soluble in water
  • fatty acid (tails) and glycerol (backbone)
saturated fatty acid: max # C-H bonds.
unsaturated fatty acid: 1 C=H bond.
  • energy storage
saturated fat: long-term: animal
e.g. lard, butter, etc.
unsaturated fat: long-term: plants
e.g. olive oil, canola oil, corn oil, etc.
  • membranes
phospholipids: cell membranes: animals/plants
  • steroids
chemical signals: animals/plants
e.g. hormones, cholesterol, etc.
  • waxes: protective water-proof coverings.
fur, feathers, skin
plant leaves/fruit
insect exoskeletons
  • also called: polypeptide chains.
  • made of C, H, N, O S
  • amino acid: amino group, carboxyl group, R group
20 amino acids
  • depends on shape and amino acid sequence.
structures: muscle, bone, cartilage, hair.
enzymes: regulate reaction rates
immune system: fight disease
nutrient storage in cell:
chemical messengers
Nucleic acids
monomer

function
/
  • stores genetic information, codes for proteins.
made of C, H, N, O, P
2 types: deoxyribonucleic acid (DNA)
ribonucleic acid (RNA)
  • nucleotide (3 parts)
5-carbon sugar
phosphate group
nitrogen base
  • DNA: stores genetic information
  • RNA: transmits code to build proteins

News flash!!
Chemical reaction
Reactants
Products
Chemical Equation / Chemical Reactions
  • EVERY PROCESS IN LIVING THINGS INVOLVES CHEMICAL REACTIONS!!
  • process that changes 1 set of chemicals into another set of chemicals.
involves breaking and forming bonds.
compounds/elements entering into rxn.
compounds/elements produces by rxn.
HCl + NaOH  H2O + NaCl
Energy in reactions
Exothermic rxn
Endothermic rxn
Activation energy
Reactions in living things /
  • breaking/forming bonds releases/absorbs energy.
rxns that release energy
rxns that absorb energy: need energy to get started.
energy needed to get rxn started.
  • living things need to absorb energy to survive.
animals get energy from plants, animals.
plants get energy from sunlight.
Enzyme

Substrate
Active site
Product
How an enzyme works
Factors that affect enzyme /
  • biological catalyst that speeds up chemical rxn.
lowers activation energy.
  • uniquely shaped protein that helps break or build molecules.
  • reactant(s) that fit into enzyme’s active site.
  • place on enzyme where reaction happens.
  • result of reaction.
  1. substrate(s) fit into active site on enzyme.
  2. reaction occurs and products are released.
  3. reaction continues until substrate(s) are gone.
  4. enzyme is used and reused.
  • heat/abnormal pH denature (changes shape) enzyme.