Chapter 2 Flashcards
Matter and its 3 forms
a substance that has mass and occupies space.
solid- bones
liquid- blood
gas- oxygen
atoms
the smallest particle that exhibits chemical properties of an element
elements
112 elements in the periodic table. Elements (92 occurring naturally) make up all things. Divided into Major, Minor, and trace elements.
subatomic particles
protons, neutrons, and electrons that compose atoms
What two subatomic particles determine the mass of an atom
protons and neutrons
What two subatomic particles define the charge of an atom
electrons and protons
Isotopes
atoms of the same element that have the same number of protons and electrons but differ in the number of neutrons. Isotopes of an element exhibit essentially identical chemical characteristics but have different atomic masses. e.g. Carbon12, carbon13, carbon14
radioisotopes
unstable forms of isotopes because their nuclei contain an excess # of neutrons. They are radioactive and release radiations as they decay into a more stable isotope.
Chemical compounds
stable associations between two or more elements combined in a fixed ratio. Classified as either ionic compounds or or molecular compounds
Ionic Compounds
structures composed of ions that are held together in a lattice by electrostatic interactions called ionic bonds
Ion
an atom or a group of atoms with an electrical charge, either positive or negative
cations
atoms with positive charge
anions
ions with negative charge
Antebrachial
forearm
antecubital
front of elbow
auricular
visible surfaces of the ear
major elements
oxygen
carbon
hydrogen
nitrogen
calcium
phosphorous
minor elements
sulfur, potassium, sodium, chlorine, magnesium, iron
valence shell
outer shell of an atom
chemical stability
when an atom has a complete outer shell they are relatively inert and exhibit low reactivity- they do not combine with other elements.
octet rule
the tendency for atoms to lose, gain, or share electrons to fill their outer shell and gain chemical stability
chemical compounds
stable associations between two or more elements combined in a fixed ratio.
ionic compounds
structures composed of ions that are held together in a lattice by electrostatic interactions called ionic bonds.
ion
an atom or group of atoms with an electrical charge, either positive or negative.
Types of bonds
Ionic: Transferringelectrons
Covalent: sharing electrons become molecules
Metabolism
chemical processes happening within the body
Catabolic process
Tearing things down
Anabolic process
Building things up
Covalent bond
The sharing of electrons between atoms form a covalent bond. Covalently bonded atoms forms a molecule. Both atoms need electrons to be stable.
Molecular formula
number and types of atoms forming molecules
e.g H2Co3 forms carbonic acid
structural formula
the molecular formula (number and types of atoms) plus their spacial arrangement within the molecule.
isomers
molecules composed of the same number and type of elements but arranged differently in space. e.g glucose, galactose, fructose
Types of Covalent Bonds
single: sharing one pair of electrons
double: sharing two pairs of electrons
triple: sharing 3 pairs of electrons
carbon skeleton
the arrangement of carbon atoms called the carbon backbone. 3 major arrangements: Straight, branched, ring
electronegativity
how atoms share electrons determines the attraction the atom has for electrons
nonpolar covalent bond
two atoms of the same type that share electrons equally. e.g two hydrogens
polar covalent bond
Type of bond where electrons are shared unequally resulting in a negative charge on one end and a positive charge on the other end.
non polar molecules
contain primarily nonpolar covalent bonds between atoms
amphipathic molecules
molecules that contain polar and non polar components. e.g phospholipid
intramolecular interactions
bonds, connections, etc that happen within a large molecule.
Organic molecules
molecules that contain carbon andhydrogenwhich are or have been components of living organisms
inorganic molecules
all other molecules that don’t have carbon. e.g water, acids, bases
4 primary organic macromolecules
lipids, carbohydrates, nucleic acids, proteins
water in the body functions in 4 ways
- transports
- lubricates
- cushions
- excretes waste
cohesion
the attraction between water molecules
surface tension
inward pulling of cohesive forces at the surface of water
adhesion
attraction between water molecules and substance other that water
solvent
a liquid that dissolves solutes
hydrophilic
water loving polar molecules that dissolve within water
electrolytes
subsstances that dissolve and dissociate in water can readily conduct an electric current
buffer
a molecules or molecular compound that helps prevent pH changes if either acid or base or added
mixtures
mixtures are formed from the combining or mixing of two different substances
3 types of water mixtures
Suspension: mixture composed of particles that are larger than 1 mm (Sand in water or blood) Only remain mixed while in motion
Colloid: mixture composed of smaller particles and remain mixed even while not in motion. (gelatin) scatters light but doesn’t settle
Solution: homogenous mixture of very small substances (soda, saltwater, simple syrup)
Mass/Volume
mass of solute per volume of solution (results from a blood test, like blood glucose levels)
Mass/volume percent
grams of solute per 100 ml of solution eg. IV solutions
molarity
measure of number of moles per liter of solution
molality
moles per kg of solvent
osmoles
reflects whether a substance dissolves, or dissolves and dissociates when placed into a solution
biological macromolecules
Lipids, carbohydrates, proteins, nucleic acids
polymers
polymers are molecules that are made up of repeating subunits called monomers and each monomer is either identical or similar in chemical structure.
dimer
two monomers bonded together
4 classes of Lipids
Phospholipids
Eicosanoids
Trigycerides
Steroids
Neutrons =
Atomic mass - protons
