Bisc104 Chapter 2

Front 1

the four elements that dominate; and the trace elements

Back 1

Oxygen, Carbon, Hydrogen, Nitrogen; we contain relative high quantities of calcium, phosphorous, sulfur, sodium, chlorine, magnesium

Front 2

describe an atom, its pieces and about them

Back 2

protons (+) neutrons (/) and electrons in the orbitals (-).
-protons and neutrons have a mass of 1 dalton.
-number of electrons = number of protons in an uncharged/neutral atom

Front 3

isotope

Back 3

substance with the same number of protons as the original element but a different number of neutrons. they are chemically identical but have different masses.

Front 4

how to find the number of neutrons:

Back 4

atomic mass - atomic number

Front 5

atomic mass, atomic number

Back 5

a. mass: mass of the atom, different for different isotopes
a. number: the number of protons in the nucleus of an atom. The a. number can tell an elements reactivity because it tells the number of electrons in the valence shell and when it will become a positive or a negative ion.

Front 6

radioactive decay

Back 6

happens when new elements are formed. the nucleus divides and releases energy. the energy is helpful or harmful.

Front 7

valence shell

Back 7

outermost ring of electrons, where atoms are bonded together.
elements in the same column have the same number of valence electrons.

Front 8

ion

Back 8

charged atom

Front 9

an atom with 1-3 electrons in valence

Back 9

can lose them and become positive

Front 10

an atom with 5-7 electrons in valence

Back 10

can gain more and become negtive

Front 11

atom with 8 electrons in valence

Back 11

noble gas

Front 12

ionic bond

Back 12

ionic bond: strong, like magnets + and -, many things form this bond. example: element with 1 valence give it to element with 7 valence so have - and + charges and attract.

Front 13

covalent bond

Back 13

more common and more important than ionic to living tissue, electrons are shared. example: hydrogen with 1 valence electron is attracted to oxygen which shares 2 of its 8 valence electrons. Often involve carbon, oxygen, nitroge, hydrogen.
single covalent bond: H-H
double: 2 pairs shared like in O2: O=O
triple: 3 pairs shared like N2 cause has 5 valence in outside

nonpolar molecule: when the electrons are shared evenly and charge is same on each end
polar covalent: unequal electron sharing where one end has stronger pull than other

Front 14

hydrogen bond

Back 14

weak
-when hydrogen is part of a polar covalent bond (unequal), the hydrogen end tends to be more positive.

Front 15

van der Waals force

Back 15

atoms vibrate and electrons whirl around and carious regions randomly become more positive or negative . van der Waals occurs when these intermittent molecules brifly attract one another.

Front 16

bonds and their endothermic, exothermic reactions

Back 16

endo: absorb energy when formed, used to store energy in the body for later release
exo: energy is released wen the bond is formed

Front 17

hydrophilic, hydrophobic

Back 17

philic: have an affinity for water and seperate in it
phobic: lack affinity for water, not soluble in water

Front 18

water is:

Back 18

necesary for digestion, excretion, respiration and circulation...
liquid at room, dissolves other substances so good solvent, cohesive and adhesive( sicks to itself, others), high specific heat: lots of energy to raise/lower temp, high heat of vaporation: takes alot to vaporize: as core temp rises, body sweats to increase heat loss;, ice floats

Front 19

pH

Back 19

-measures acidity, alkalinity
-ranges from 0-14. lower numbers=higher acidity
litmus: a pH indicator. veggie dye that changes color in prsence of acid or base.
-body needs stable acidity: a helper to keep homeostasis is a buffer: compounds that stabilize pH by absorbing excess H+ or OH- ions

Front 20

compound

Back 20

molecule with unlike atoms

Front 21

functional group

Back 21

determinds the compound's reactivity and how it reacts with other chemicals

Front 22

4 categories of organic compounds

Back 22

carbohydrates, lipids, proteins, and nucleic acids

Front 23

acidity/alkalinity (pH)

Back 23

they affect the rate and energetic properties of many chemical reactions..
Common acids—lemon juice, orange juice, cranberry juice, vinegar and coffee.
Common bases—soap, milk of magnesia, ammonia.

Front 24

cholesterol, estrogen, testosterone

Back 24

choles: a calss of steroids found in animals, aids in membraine fluidity
estrogen.testosterone:steroids

Front 25

peptide bonds

Back 25

bond between carboxyl group of one amino acid and the amino group of the adjacent amino acid
Make long chains of amino acids called polypeptides (bond between 2 is a dipeptide) and when more than 100 bonds called a protein.

Front 26

proteins and their structure

Back 26

primary structure, secondary, tertiary, quarternary, globular

the shape of protein determines its function

when protein radically alters its folding pattern or unfolds, call it denaturing.

Front 27

enzyme

Back 27

special class of functional proteins, serve as catalysts (facilitate reactoion) for biochemical reactions

Front 28

active site of a protein

Back 28

shaped to bind to one specific substrate/reactant...this is to provide the substrate with an environment for a specific chemical reaction

Front 29

ATP, adipocytes, ADP

Back 29

the primary energy molecule that an be used to perform cellular functions...stores energy, Short-term energy storage uses a high-energy system that is reversible and instantly available.

adipocytes: specialized fat cells that store large quantities of lipid, long term storage of energy

ADP: what results when ATP loses phosphate

Front 30

amino acid

Back 30

building blocks of proteins, create chain and once get to mor ethan 100 called a protein