Chapter 2 Basic Chemistry

matter is made up of

atoms that contain protons, neutrons, electrons

proton

1 positive charge, 1 mass unit

neutron

no charge, 1 mass unit

electron

1 negative charge, tiny mass

the nucleus contains

protons and neutrons, all mass and positive charges

the electron shell contains

all negative charges, not all are complete

atoms with incomplete energy levels are

reactive

atomic number

number of protons, identifies element

atomic mass

average number of protons plus number of neutrons

common atoms found everywhere in the body

carbon, hydrogen, oxygen, nitrogen, phosphorus, sulfur

calcium (Ca)

in bone, cell signaling

sodium (Na), potassium (K), chlorine (Cl) are

important electrolytes

magnesium (Mg)

a co-factor

iron (Fe)

to transport oxygen

iodine (I)

in thyroid hormone

chemical bonds involve

sharing, gaining, losing of electrons in the valance shell

types of chemical bonds

ionic, covalent, hydrogen

ionic bonds

attraction between cations and anions, creates compounds

cation

electron doner

anion

electron acceptor

covalent bonds

strong electron bonds involving shared electrons, creates molecules

hydrogen bonds

weak polar bonds based on partial electrical attraction

sodium chloride (NaCl) is a

compound from ionic bonding

transient interactions

atoms can move

common cations

sodium, potassium, calcium, magnesium

common anions

chloride, phosphate, bicarbonate, sufate

covalent bonds involve

sharing of pairs of electrons between atoms

covalent bonds share

electrons that make single, double, or triple bonds depending on the number of paired electrons

nonpolar covalent bonds

involve equal sharing of electrons

polar covalent bonds

involve unequal sharing of electrons, form polar molecules

water has

polar covalent bonds, hydrogen bonds

hydrogen bonds

involve slightly positive and slightly negative parts of polar molecules being attracted to each other

hydrogen bonds produce

transient interactions only

molecular weight

sum of the atomic weights of the atoms in a molecule

formula weight

sum of the atomic weights in a compound

hydrogen bonds between H2O cause

surface tension

moles

1 mole of any substance contains Avogadro’s number of molecules

molar concentration (M) equals

amount/volume or mol/L

what are moles written as

g/mol

inorganic molecules (compounds)

are not based on carbon and hydrogen

organic molecules

are based on carbon and hydrogen

nutrients are

essential molecules obtained from food

metabolites

molecules made or broken down in the body

reactants

materials going into a reaction

products

materials coming out of a reaction

metabolism

all the reactions that are occurring at one time into an organism

decomposition reaction (catabolism)

breaks chemical bonds

hydrolysis

water is a reactant and broken down in the product

synthesis reaction (anabolism)

forms chemical bonds

dehydration synthesis

water is broken down in the reactant and formed as a product

reversible reaction

a reaction that occurs simultaneously in both directions

at the equilibrium

the amounts of chemicals do not change even though the reactions are still occurring

reversible reactions seek

equilibrium

if reactants are added or removed, the reaction rates

adjust to reach a new equilibrium