solid to liquid

(ice to water)

liquid to solid

(water to ice)

liquid to gas

(water to steam)

gas to liquid

(steam to water)

metalic or non metalic

a substance composed of two or more elements chemically bonded together

H₂O

the least unit of a compound

(H₂O is one molecule of water)

smallest unit of an element

Hydrogen Atom

Matter (substances) is composed of Atoms, the smalles unit of an element.

3 subatomic particles:

protons, neutrons, electrons

have a positive charge

number of protons = atomic number

have no charge

Atomic weight - Atomic # = # of neutrons

Electrons

Have a negative charge

# of electrons = Atomic #

tiny central core located deep inside the atom

formed by protons and neutrons

electronically neutral

(the number of negatively charged electrons is always equal to the number of positively charged protons in a STABLE ATOM

an element whose atoms contain a different number of neutrons than most of that element

• Hydrogen (H): Atomic #1, Atomic Weight = 1 (No Neutron)

  • Deutrium (1N):  Atomic #1, Atomic Weight = 2 (1 Neutron)

  • Tritium (2N):  Atomic #1, Atomic Weight = 3  (2 Neutrons)

the emission of radiation from atoms' nucleus

Alpha Rays- heavy particles

Beta Rays- electrons formed in a neucleus by splitting a neutron into a proton and an electron

Gamma Rays- electromagnetic rays

stable isotopes

used in medicine

given by the number of "free electrons" in the outer shell

Outer Shell- 1+ single electrons (unpaired)- unstable/active

outer shell- 0 single electrons (only paired) chemically inactive or stable

formed when an atom loses or gains 1 or more electrons

"Transfer" of unpaired electron creates a chemical bond resulting in formation of a compound

Ex. Na+Cl > NaCl

Atoms cannot pull electrons away from other atom.  They end up "sharing" electrons

2 types

Atoms share electrons "equally" no difference in charge between two poles of bond

Example: Hydrogen Gas (H₂)

one atom exerts more pull on shared electron

Example H₂O

number of unpaired electrons in an atoms outer shell

number of chemical bonds it can form with other atoms

sum of all atomic weights of all the atoms found in the molecule

# of atoms x Atomic weight = molecular wt

water, H (1x2) 2 + 16 O (1x16) =18

in an aqueous solution give off hydrogen ions (H+)

ex. HCl (hydrochloric Acid) dissociates into H+ and Cl- ions

do not contain carbon, hydrogen and oxygen in chains

includes water and salts

give off hydroxide ions

Ex. NaOH (Sodium Hydroxide) dissociates into Na+ and OH- ions

soluble base

NaOH, KOH (alkali),

Ca(OH)₂ (Calcium Hydroxide), Base, Insoluble

compounds resulting from chemical interaction of an acid and a base

2HCL + Mg(OH)₂ > MgCl₂ +2H₂O

Process is called Neutralization

Type of reaction is "Exchange Reaction"

Partial Presure of H+ ions

designates the negative logarithm of H+ ion concentration

Gas (NH₃) when dissolved in water forms Ammonium Hydroxide (NH₄OH)

BI PRODUCT OF PROTEIN DECOMP

highly toxic .005% in blood is fatal

readily converted to non-toxic or substances of limited toxicity like urea or uric acid, which are excreted through the urine.

usually contain carbon, hydrogen, and oxgen

found in chains and occur naturally in living plants and animals

head: hydrophilic

-polar loves water

tail: hydrophobic

-non-polar, hates water

 bilipid membrane

"fluid mosaic model"

act as energy storage

contain high energy bonds

supply energy to cellular activities and help preform body functions

involved in the formation and maintenance of skin and fur

act as chemical messengers (hormones) that coordinate the metabolism of an organism

ex. cholesterol

Natural Fats

most abundant lipids in the body

MOST CONCENTRATED SOURCE OF ENERGY

CH₂O ratio

one is monosaccharide

occur in long chains or polymers of smaller units

most common sugars: glucose, fructose and galactose (Isomers)

glucose fructose galactose

same number of atoms, but the arangement differs (isomers)

Hexoses

Pentoses- monosaccharide, contain 5 carbon atoms (Ribose and Deoxyribose-not sweet)

two monosaccharides - one water molecule

sucrose (cane sugar)

maltose

lactose

many monosaccharides

removal of water to form straight chains or braided chains

large and complex

ex. Starch

animals, store starch in the form of glycogen in the liver

• glycogen has a molecular weight of several million

energy release

store energy

Glucose (simple sugar) <> Glycogen (animal starch stored in liver, temporary storage) <> Fat (permanent storage)

Nucleic Acid

Continued Existance-inheritance-heridity

information contained in the chromosomes is passed from generation to generation in the form of biochemical language of nucleic acids, called the genetic code, 

hetero-polymer, always linear

each nucleic acid-a monomer is called a nucleotide

composed of:

5 carbon sugar (ribose/deoxyribose)

phosphate ion

nitrogenous base

double ring

A (Adenine) & G (guanine)

single ring molecules

 C (cytosine) T (thymine only in DNA) U (uracil ONLY IN RNA)

DNA

2 strands, deoxyribose sugar, A=T, G=C, found in the nucleus, forms chromosomes during cell division

RNA

1 strand, ribose sugar, A=U, G=C, found in the ribosomes/cytoplasm, protein synthesis

a single very long molecule of DNA containing 100 million nucleotides

twists to form a double helix

46 per cell in humans

giant sized macromolecules found in the body abundantly

hormones, enzymes, structural proteins

Primary

Secondary

Tertiary

Quaternary

building blocks of proteins:

Carbon atom (C)

amino group (-NH₂)

acid group (-COOH) carboxyl

hydrogen atom (-H)

side chain with (-R)

amino acids frequently become linked by a (covalent) peptide bond

binds the carboxyl group of one amino acid to another amino acid

dipeptide- two amino acids linked

tripeptide- three amino acids linked

long sequences of amino acids linked together by peptide bonds

Protein hormone

insulin

hemoglobin

glycolisis

anaerobic respiration

Krebs Cycle or Citric Acid Cycle needs oxygen, occurs at mitochondria

electron transport chain

Enzymes

control the rate of chemical reaction in living organism

lipase

amylase

lactose dehydrogenase

creatine phosphokinase

enzymes with metalic elements

Hemoglobin: contains Iron, Manganese, Copper, Magnesium, Zinc

Molybdenum

lowers the activation energy

provides a surface for a reaction

substrate- brought together into close proximity to one another in the region of enzymes called Active Sites

provide a proper chemical enviornment

after reaction products split off leaving the enzyme free to act again

large complex molecules, very sensite to temperature, pH and other body changes

Chemical bond- a form of potential energy that may be used by the cell to do the owrk when the bond is broken

for stable molecules to be broken a certain amount of activation energy must be added to the system

once added, the reaction proceeds spontaneously

ex. combustible material > burst into flame when kindling temperature has been reached

Energy can neither be created nor destroyed

every transformation results in the usable or available energy to be lost

a constant source of energy is required, ultimate source of energy is the sun