Chapter 2 chemical level of organization

Question 1

Principle elements of human body

Answer 1

O2-oxygen, C-carbon, H-hydrogen, N-nitrogen. Secondary: Ca2+-calcium, Ch-chlorine, K-potassium, S-sulfur, P-phosphorus, Na+ sodium, Mg-magnesium, Fe-iron.

Question 2

atom

Answer 2

the smallest units of matter that retain the properties and characteristics of the element.

Question 3

nucleus, proton, neutron, electron

Answer 3

. The dense central core of an atom is its nucleus. Within the nucleus are positively charged protons (p+) and uncharged (neutral) neutrons (n). The tiny, negatively charged electrons (e-) move about in a large space surrounding the nucleus.

Question 4

electron shell (valence shell)

Answer 4

simple circles around the nu- cleus. Because each electron shell can hold a specific number of electrons, the electron shell model best conveys this aspect of atomic structure

Question 5

atomic number

Answer 5

number of protons

Question 6

atomic mass

Answer 6

number of protons +neutrons

Question 7

isotopes

Answer 7

are atoms of an element that have different numbers of neutrons and therefore different mass numbers.

Question 8

atomic mass

Answer 8

Dalton/atomic mass unit- average mass of its common occurring isotope

Question 9

Ion

Answer 9

is an atom that has a positive or negative charge because it has unequal numbers of protons and electrons

Question 10

Ionization

Answer 10

is the process of giving up or gaining electrons.

Question 11

molecule

Answer 11

2 atoms of same kind

Question 12

compound

Answer 12

2 or more atoms of different elements

Question 13

free radical

Answer 13

atom or group of atoms with unpaired electron in outermost shell- unstable, reactive and desctructive

Question 14

Octet rule

Answer 14

valence shell can only hold 8, stable, barely binds

Question 15

ionic bond

Answer 15

cation +, anion- bind by neg and pos charge, cation donates electron to anion.

Question 16

electrolyte

Answer 16

ionic compound that breaks apart into + & - ions in solution

Question 17

covalent

Answer 17

share electron

Question 18

single covalent bond, double covalent bond, triple covalent bond

Answer 18

2 atoms share one electron pair, share 2 pairs, share 3 pairs

Question 19

non-polar covalent bond

Answer 19

two atoms share the electrons equally—one atom does not attract the shared electrons more strongly than the other atom.

Question 20

electronegativity

Answer 20

power to attract electrons to itself. (greater pull=greater electronegativity)

Question 21

hydrogen bond

Answer 21

(weakest bonds), hydrogen bond forms when a hydrogen atom with a partial positive charge attracts the partial negative charge of neighboring electronegative atoms, most often larger oxygen or nitrogen atoms. hydrogen bonds result from attraction of oppositely charged parts of molecules

Question 22

surface tension

Answer 22

measure of difficulty of stretching or breaking the surface of liquid

Question 23

chemical reaction

Answer 23

occurs when new bonds form or old bonds break between atoms.

Question 24

products/reactants of chemical reaction

Answer 24

end substance=product, starting substance=reactant

Question 25

catalyst

Answer 25

enables a chemical reaction to produce faster, ex.enzyme

Question 26

synthesis reaction

Answer 26

anabolism- react for form a single product

Question 27

decomposition reaction

Answer 27

catabolism- break down molecules into two or more substances

Question 28

exchange reaction

Answer 28

weak electrolytes/ions, exchange products for one another HCL+ KOH = KCL + H2O

Question 29

reversible reaction

Answer 29

A reversible reaction is a chemical reaction where the reactants form products that, in turn, react together to give the reactants back

Question 30

oxidation/reduction reaction

Answer 30

Oxidation is loss of electron, reduction is gain of an electron

Question 31

inorganic/organic compound

Answer 31

usually lack carbon and are structurally simple/ always contain carbon, usually contain hydrogen, and always have covalent bonds

Question 32

water, water as a solution/solvent/solute

Answer 32

water an excellent solvent for other ionic or polar substances, gives water molecules cohe- sion (the tendency to stick together), and allows water to resist temperature changes.
/ In a solution, a substance called the sol- vent dissolves another substance called the solute

Question 33

hydrophilic/hydrophobic

Answer 33

water loving/water hating substances

Question 34

hydrolysis

Answer 34

decomposition reactions break down large nutrient molecules into smaller molecules by the ad- dition of water molecules

Question 35

dehydration synthesis reaction

Answer 35

when two smaller molecules join to form a larger mole- cule in a dehydration synthesis reaction (de- 􏰕 from, down, or out; hydra- 􏰕 water), a water molecule is one of the products formed

Question 36

heat capacity

Answer 36

water can absorb or release a relatively large amount of heat with only a modest change in its own temperature

Question 37

mixture, colloid, solution, suspension

Answer 37

mixture: blend together but not bonded by chemical bonds,
colloid: large particles (appear translucent or opaque)
solution: remain evenly dispersed among solvent
suspension: may mix for a bit but will settle out (blood)

Question 38

concentration (and moles)

Answer 38

mol/L, solute/solution
1 mol=atomic mass of molecule
1 mol of NACL=58.44 grams as atomic mass is 58.44

Question 39

Acid (hydrogen ion)

Answer 39

disassociate into one or more hydrogen ions (proton donor)

H+

Question 40

base

Answer 40

remove H+ from solutions (proton accept)

hydroxide ion OH-

Question 41

salt

Answer 41

NACL,

Question 42

Define the term pH, and explain the role of buffer systems in homeostasis

Answer 42

This scale is based on the concentration of H􏰑 in moles per liter. A pH of 7 means that a solution contains one ten-millionth (0.0000001) of a mole of hydrogen ions per liter.
which function to convert strong acids or bases into weak acids or bases. Strong acids (or bases) ionize easily and contribute many H􏰑 (or OH􏰒) to a solution. Therefore, they can change pH drastically, which can disrupt the body’s metabolism. Weak acids (or bases) do not ionize as much and contribute fewer H􏰑 (or OH􏰒). Hence, they have less effect on the pH. The chemical compounds that can convert strong acids or bases into weak ones are called buffers

Question 43

carbonic acid bicarbonate buffer system

Answer 43

Carbonic acid (H2CO3) can act as a weak acid, and the bicarbonate ion (HCO3-) can act as a weak base. 
 buffer system can compensate for either an excess or a shortage of H+.

Question 44

macromolecules
polymers
monomers
isomers

Answer 44

Small organic molecules can combine into very large mole- cules that are called macromolecules.
A polymer is a large molecule formed by the covalent bonding of many identical or similar small building-block molecules called monomers.
Molecules that have the same molecular formula but different structures are called isomers.

Question 45

carbohydrate-
monosaccharide
disaccharide
polysaccharide; starches; cellulose
glycogen

Answer 45

monosaccharide/disaccharide (2 monosaccharides)-simple sugars.
Cells throughout the body break down the hexose (6 carbon) glucose to produce ATP.
polysaccharide- ten to millions of monosaccharides joined by dehydrated synthesis

Question 46

lipid

Answer 46

insoluble in h2o and hydrophobic.

Question 47

lipoprotien

Answer 47

lipid molecules join with hydrophilic protein

Question 48

fatty acid; saturated and unsaturated

Answer 48

fatty acid-simplest lipid, building blocks of triglycerides
A saturated fatty acid contains only single cova- lent bonds between the carbon atoms of the hydrocarbon chain. Because they lack double bonds, each carbon atom of the hy- drocarbon chain is saturated with hydrogen atoms.
An unsaturated fatty acid contains one or more double covalent bonds between the carbon atoms of the hydrocarbon chain. Thus, the fatty acid is not completely saturated with hydrogen atoms (kink or bend in chain)

Question 49

triglyceride =triacylglycerol

glycerol

Answer 49

most plentiful lipids in your body and in your diet
A triglyceride consists of two types of building blocks: a single glycerol molecule and three fatty acid mole- cules. A three-carbon glycerol molecule forms the backbone of a triglyceride

Question 50

Phospholipid

amphipathic

Answer 50

Phospholipid- have a glyc- erol backbone and two fatty acid chains attached to the first two carbons,

amphipathic-Molecules that have both polar and nonpolar parts are said to be amphipathic

Question 51

steroid

cholesterol

Answer 51

steroid-four ring carbon atom- slightly ampipathic

cholesterol-Body cells synthesize other steroids from cholesterol, needed for cell membrane structure

Question 52

eicasanoids:
prostaglandins
leukotrienes

Answer 52

eicasanoids: lipids derived from a 20-carbon fatty acid called arachidonic acid.
eicasanoids subclasses:
They modify responses to hormones, contribute to the inflammatory response (Chapter 22), prevent stomach ulcers, dilate (enlarge) airways to the lungs, regulate body temperature, and influence formation of blood clots, to name just a few. Leukotrienes participate in allergic and inflammatory responses.

Question 53

function of protien

Answer 53

1) (structural) Form structural framework of various parts of body
2) (regulatory)Function as hormones that regulate various physiological processes; control growth and development; as neurotransmitters, mediate responses of nervous system.
3) (contractile) Allow shortening of muscle cells, which produces movement.
4) (immunologic)- Aid responses that protect body against foreign substances and invading pathogens.
5) (transport)-carry vital substances around the body
6) (catalytic)-Act as enzymes that regulate biochemical reactions.