Ch.1-5 Biology

Front 1

deductive reasoning

Back 1

summarize the info at hand and draw conclusions from that information, proceeds from the general to the specific

Front 2

inductive reasoning

Back 2

drawing a generalization from several specific observations, proceeds from specific to general. it is IMPOSSIBLE to prove the accuracy of generalization

Front 3

the recursive nature

Back 3

experiments provide more observations, and at any time more observations may be added in and more testable models may be produced

Front 4

theory

Back 4

linnks together significant bodies of thought

Front 5

principle or law

Back 5

when a theory yields unvarying adn uniform predictions over a long period of time

Front 6

the goal of science is to

Back 6

understand nature

Front 7

the goal of technology is to

Back 7

apply scientific knowledge

Front 8

cell

Back 8

the basic structure adn functional unit of life consisting of living material bounded by a membrane. It is the smallest unit of life capable of growth and development

Front 9

growth

Back 9

increase in size and number

Front 10

development

Back 10

changes in roles of cells during the life cycle of an organism

Front 11

metabolism

Back 11

includes the chemical process essential to growth and repair. It is the sum of the chemical rxns adn energy transformations

Front 12

homeostasis

Back 12

the tendency of an organism to maintain a relatively constant interna or external environment. (Metabolism needs this).

Front 13

asexual reproduction

Back 13

copying; reprduction not involving sex, resulting from only cell division

Front 14

sexual reproduction

Back 14

reproduction involving sex, typically involves the formation of specialized egg and sperm cells and their fusion to produce a zygote which grows and develops into a new organism

Front 15

DNA

Back 15

responsible for information transfer from one generation to the next. Makes up genes.

Front 16

hormones

Back 16

chemical signals used for intercellular signaling

Front 17

what type of system do biologists use?

Back 17

binomial system for classifying organisms

Front 18

taxonomy

Back 18

the science of classifying adn naming of organisms

Front 19

Carolus Linnaeus

Back 19

swedish botanist who developed a system of classification that is the basis of what is used today

Front 20

species

Back 20

basic unit of classification.

Front 21

if species sexual

Back 21

can interbreed and produce fertile offspring

Front 22

if species asexual

Back 22

group based on similarities (DNA sequence based)

Front 23

Genus

Back 23

a gorup of closely related species

Front 24

binomial name

Back 24

made of genus and specific epithet. Genus is capitalized. ex. Homo sapiens

Front 25

order of taxonomic classification

Back 25

Dashing King Phillup Came Over For Great Sex
Family, Order, Class, Phylum, Kingdom, Domain

Front 26

domain

Back 26

the highest level of classification

Front 27

two domains of consist of prokaryotes

Back 27

archaea and bacteria
no true cellular nucleus

Front 28

archaea

Back 28

Kingdom Archaebacteria, typically found in extreme environments, distinguished by RNA

Front 29

Bacteria

Back 29

Kingdom Eubacteria, very diverse group of bacteria

Front 30

domain Eukarya

Back 30

consists of eukaryotes, organisms with a discrete cellular nucleus, it is divided into 4 kingdoms

Front 31

Kingdom Protista

Back 31

(domain eukarya) sinlge celled adn simple multicellular organisms having nuclei

Front 32

Kingdom Plantae

Back 32

(domain eukarya)plants are complex multicellular organisms having tissues and organs. Have cells walls containing cellulose. Have chlorophyll.

Front 33

Kingdom Fungi

Back 33

(domain eukarya)have cell walls containing chitin. most decomposers.

Front 34

Kingdom Animalia

Back 34

complex multicellular organisms that eat other organisms for nourishment. NO CELL WALLS. most forms of motile.

Front 35

producers

Back 35

autotrophs, manufacture their own food from simple materials

Front 36

photosynthesis

Back 36

CO2 + H2O + light energy = carbohydrate(food) + Oxygen

Front 37

respiration

Back 37

carbohydrate + oxygen = CO2 +H2O + energy

Front 38

consumers

Back 38

heterotrophs, obtain energy by eating other organisms (ultimate source of energy is producers) use food and oxygen and release CO2 and water

Front 39

decomposers

Back 39

obtain energy by breaking down the water products, and dead bodies of producers and consumers. Usually bacteria or fungi.

Front 40

evolution

Back 40

the core unifying theme thst explains much of the observations connected with the other themes

Front 41

elements

Back 41

substances that cannot be further broken down. 92 naturally occuring elements

Front 42

4 elements that make 96% of the mass of living things

Back 42

O H C N

Front 43

8 other elements present in small amounts

Back 43

Ca, P, K, S, Na, Mg, Cl, Fe

Front 44

atom

Back 44

smallest unit of an element that still retains the properties of that element

Front 45

electron

Back 45

contributes no significant mass to the atom, but carries a (-1) electrical charge

Front 46

proton

Back 46

contributes a mass of 1 mass unit, carries a (+1) charge

Front 47

neutron

Back 47

contributes a mass of 1 mass unit, carries no charge

Front 48

protons and neutrons are found in the

Back 48

nucleus

Front 49

elements differ from

Back 49

different number of protons

Front 50

atomic number

Back 50

protons + nucleus

Front 51

isotopes

Back 51

atoms that have the same number of protons but have different number of neutrons

Front 52

atomic nuclei can undergo

Back 52

change/decay

Front 53

most unstable isotopes are

Back 53

radioisotopes

Front 54

when an atom is neutral

Back 54

electrons = protons

Front 55

orbitals

Back 55

energy levels

Front 56

valence electrons

Back 56

the outer electrons

Front 57

chemical properties of an atom are determined by

Back 57

valence electrons

Front 58

molecule

Back 58

two or more atoms held together by covalent bonds, may be composed of one or more elements. molecule differs in its physical and chemical properties from the elements that make it up

Front 59

compound

Back 59

a specific combination of two or more DIFFERENT elements chemically combined in a fixed ration. have unique physical and chemical properties that differ from those of the elements use to make it. some held by covalent bonds - making it molecular

Front 60

chemical formula

Back 60

showing the number of atoms of each element present. often called molecular formula.

Front 61

structural formula

Back 61

shows the arrangement of atoms in a molecule

Front 62

molecular mass

Back 62

the sum of the atomic masses of the atoms in the molecule

Front 63

a chemical bond is a

Back 63

reduced energy state

Front 64

bond energy

Back 64

is the amount of energy required to break a particular chemical bond

Front 65

covalent bond

Back 65

electrons shared b/w two atoms. result in filled valence shells, electrons are shared in pairs, carbon forms 4 covalent bonds

Front 66

ionic bond

Back 66

one atom completely gives up an electron to another atom. formed by the attraction b/w cation and anion

Front 67

nonpolar

Back 67

equal sharing of electrons

Front 68

polar

Back 68

unequal sharing of electrons. result if one nuclues holds a stronger attraction on the electron pair. partial charge

Front 69

ion

Back 69

an atom gains or gives one or more electrons

Front 70

cation

Back 70

lost one or more electrons, has a positive charge

Front 71

anion

Back 71

gains one or more electrons, has a negative charge. suffix -ide indicates an anion

Front 72

polyatomic ions

Back 72

only they can lose or gain PROTONS

Front 73

hydration

Back 73

surrounding the ions with the ends water molecules w/ the opposite charge

Front 74

hydrogen bonds

Back 74

weak interactions involving partially charged hydrogen atoms, more common and important in living things. very weak compared to cov. bonds.

Front 75

strength of covalent, hydrogen, and ionic bonds

Back 75

covalent bond stronger than ionic, and ionic stronger than hydrogen, hydrogen is the weakest

Front 76

double arrow in an equation indicates

Back 76

equilibrium

Front 77

oxidation

Back 77

a chemical process in which an atom, molecule, or ion LOSES an electron(s). oxygen is most common oxidizing agent

Front 78

reduction

Back 78

an elecctron is GAINED (charge is reduced)

Front 79

oxidation and reduction are always

Back 79

paired, hence redox reactions

Front 80

look for movement of what in redox reactions

Back 80

electrons

Front 81

what percentage of cells is made of water?

Back 81

70%

Front 82

about what percentage of the earrth's surface is covered in water?

Back 82

75%

Front 83

electronegative

Back 83

electron seeking, oxygen atoms are electronegative

Front 84

the polar character of water allows it to form what type of bonds?

Back 84

hydrogen

Front 85

four properties of water that are critical to life

Back 85

1. it is the principle solvent
2. exhibits both cohesive and adhesive forces
3. helps maintain stable temp
4. ice floats in liquid water

Front 86

water makes a good solvent because?

Back 86

of its highly polar character

Front 87

hydrophilic substances

Back 87

interact readily with water

Front 88

water does not readily dissolve. . .

Back 88

nonpolar(hydrophobic) substances, thus, hydrophobic substances are good compounds for membranes

Front 89

cohesive forces

Back 89

are caused by the attraction of water molecules to other water molecules, and give water a high surface tension

Front 90

surface tension

Back 90

the ability of a water surface to withstand some stress

Front 91

adhesive forces

Back 91

cause water molecules to be attracted to other kinds of molecules, it is how things are made wet

Front 92

capillary action

Back 92

the tendency of water to move up narrow tubes even against gravity, results from cohesion and adhesion, living organisms take advantage of this

Front 93

specific heat

Back 93

the amount of energy required to raise the temperature of a specific amount of a substance one degree celsius. (for water, 1g og water to raise by one degree of celsius

Front 94

the specific heat of water is. . .

Back 94

much higher than most other substances, due to hydrogen bonding. It cools down slowly b/c of the formation of hydrogen bonds

Front 95

in order to change temp of water. . .

Back 95

requires gain or loss of more energy than it does other substances

Front 96

what helps cool the ecosphere?

Back 96

the high heat of vaporization

Front 97

heat vaporization

Back 97

the amount of energy required to convert one gram of liquid into the gaseous state

Front 98

water has an extremely high vaporization b/c?

Back 98

of the hydrogen bonds in liquid water

Front 99

calorie

Back 99

the amount of heat(energy) required to cause the temperature of one gram of pure water to rise one degree celsius

Front 100

how many calories does it take to convert 1g of liquid water into water vapor

Back 100

540 calories

Front 101

as liquid water cools, it becomes?

Back 101

denser, but only up to a point

Front 102

at 4 degrees celsius

Back 102

water begins to expand as it cools further

Front 103

zero degrees celsius

Back 103

ice freezes into a crystal based on the placement of hydrogen bonds

Front 104

acids

Back 104

proton donors. a substance that dissociates in solution to yield hydrogen ions (H+)

Front 105

any substance that yields a proton is a?

Back 105

acid

Front 106

base

Back 106

proton acceptors, eaither dissociate in water to produce hydroxide ions and a cation, or split water to form a cation and hydroxide ion

Front 107

water tends to slightly dissociate into?

Back 107

hydrogen adn hydroxide ions (H+ and OH-)

Front 108

in pure water, the concentrations of these ions are?

Back 108

equal
H+ = OH- = 10^-7
ten more times = 10^-6

Front 109

acidic solutions

Back 109

have an elevated H+, and thus reduced OH-

Front 110

basic solutions

Back 110

have an elevated OH-, and thus reduced H+

Front 111

pH scale

Back 111

to express the proton concentration of a solution

Front 112

pure water has a pH of?

Back 112

7
so ten times more = 10^6 or pH 6
ten times less = 10^8 or pH 8

Front 113

a pH below 7 is

Back 113

acidic

Front 114

a pH above 7 is

Back 114

basic

Front 115

the pH of most living things is?

Back 115

7.2 to 7.4

Front 116

buffers

Back 116

minimize pH changes

Front 117

weak acids and weak bases serve as?

Back 117

buffers

Front 118

solvent

Back 118

a liquid into which a substance dissolves

Front 119

solute

Back 119

the dissolved substance

Front 120

solution

Back 120

solvent + solute

Front 121

salts

Back 121

form from acids adn bases

Front 122

electrolytes

Back 122

are salts, acids, or bases that form ions in water and thus can conduct an electrical current when dissolved in water. (pure water is poor conductor, but put salt in and it is)

Front 123

nonelectrolytes

Back 123

are substances like sugar that dissolve in water do not become ionic

Front 124

mixture

Back 124

a mixture of 2 or more elements and/or more elements and/or compounds

Front 125

heterogenous

Back 125

mixtures that are not uniform composition throughout - a living organism is a good ex.

Front 126

homogeneous

Back 126

mixtures that are completely uniform thorughout, a salt water is a good ex.

Front 127

organic chemistry

Back 127

have at least one carbon covalently bonded to another carbon atom or to hydrogen, the chemistry of organic molecules is organized around the carbon atom

Front 128

single carbon cardon bonds allow?

Back 128

rotation around them and lend to flexibility to molecules

Front 129

the shape of a molecule is important in determining?

Back 129

its chemical and biological properties

Front 130

isomers

Back 130

molecules that have same molecular formula but different structures

Front 131

stereoisomers

Back 131

substances with the same arrangement of covalent bonds, but the order in which the atoms are arranged in space is different

Front 132

structual isomers

Back 132

substances w/ the same molecular formula that differ in the covalent arrangement of their atoms

Front 133

two kinds of stereo isomers

Back 133

cis-trans isomers - associated w/ compounds that have carbon carbon double bonds
enantiomers - substances that mirror images of each other and that cannot be superimposed on each other

Front 134

functional groups

Back 134

groups of atoms covalently bonded to a carbon backbone that give properties different from a C-H bond

Front 135

hydroxly group

Back 135

OH
polar, found in alcohols, interacts w/ water

Front 136

carbonyl group

Back 136

CO
polar, found in aldehydes and ketones, interacts w/ water

Front 137

carboxyl group

Back 137

CO HO
weally acidic, found in organic acids, iteracts w/ water

Front 138

amino group

Back 138

NH2
weakly basic, found in such things as amino acids, interacts w/ water

Front 139

sulfhydryl group

Back 139

SH
essentiallu nonpolar, found in some amino acids, does not interact w/ water

Front 140

phosphate group

Back 140

PO4H2
weakly acidic, found in such things as phospholipids and nucleic acids. interacts w/ water

Front 141

methyl group

Back 141

CH - chomp down on meth
nonpolar(thus hydrphobic), found in such things as lipids, other membrane components

Front 142

polymers

Back 142

are long chains or branching chains based on repeating subunits (monomers)
ex. proteins(polymer) made from amino acids (monomer)

Front 143

macromolecules

Back 143

very large polymers

Front 144

polymers are degraded into monomers by?

Back 144

hydrolysis

Front 145

condensation

Back 145

monomers are covalently linked to form polymers

Front 146

the four major classes of biologically important organic molecules are

Back 146

carbohydrates, lipids, proteins, and nucleic acids

Front 147

carbohydrates

Back 147

include sugars, starches, and cellulose. contain only 3 elements - C, H, O = CH20
created for energy storage and consumed for energy production

Front 148

carbohydrates are grouped into?

Back 148

monosaccharides, disaccharides, and polysaccharides

Front 149

monosaccharides

Back 149

simple sugars(a single monomer).

Front 150

pentose

Back 150

include ribose and deoxyribose

Front 151

hexoses

Back 151

include GLUCOSE, fructose, and galactose

Front 152

pentose and hexose sugars form what kind of structure?

Back 152

ring structures in solution -this often creates diastereomers

Front 153

disaccharides

Back 153

consist of two monosaccharide
units. formed when the equivalent of a water molecule is removed from the 2 monosaccharides

Front 154

two monomers are joined by a

Back 154

glycosidic linkage

Front 155

common disaccharides

Back 155

maltose, sucrose, lactose

Front 156

maltose

Back 156

(malt sugar)has 2 glucose subunits

Front 157

sucrose

Back 157

(table sugar) glucose + fructose

Front 158

lactose

Back 158

(milk sugar) glucose + galactose

Front 159

polysaccharides

Back 159

marcomolecule made of repeating monosaccharides units linked together by glycosidic bonds

Front 160

starch

Back 160

the main storage carbohydrate of plants. polyer made from alpha-glucose units

Front 161

amylose

Back 161

unbranched starch chain

Front 162

amylopectin

Back 162

branched starch chain. plants store starch in organelles called amyloplasts

Front 163

glycogen

Back 163

the main storage carbohydrate for animals. highly branched and more water-soluble. mostly found in liver and muscle cells, NOT found in organelle

Front 164

cellulose

Back 164

the major structural componet of most plant cell walls. polymer made from beta-glucose.

Front 165

most organisms cannot digest?

Back 165

cellulose

Front 166

cellulose contains what percentage of the carbon found in plants

Back 166

50%

Front 167

chitin

Back 167

structural component in fungal cell walls and arthropod exoskeletons

Front 168

lipids

Back 168

fata and fat like substances. are a heterogeneous group of compounds defined by solubility NOT structure.

Front 169

lipids are principally

Back 169

hydrophobic

Front 170

lipids consist of

Back 170

carbon and hydrogen

Front 171

roles of lipids are

Back 171

serving membrane as structural components, signaling molecules, and as energy storage

Front 172

major classes of lipids are?

Back 172

triacyglycerols(fats), phopholipids, and terpenes

Front 173

triaclyglycerols

Back 173

contain glycerol joined to three fatty acids

Front 174

saturated fatty acids contain

Back 174

no carbon-carbon double bonds
usually solid at room temp

Front 175

unsaturated fatty acids contain

Back 175

one or more double bonds
usually liquid at room temp

Front 176

monosaturated

Back 176

one double bond

Front 177

polysaturated

Back 177

more than one double bond

Front 178

condensation results in

Back 178

ester linkage b/w a fatty acid and the glycerol

Front 179

phospholipids

Back 179

consist of diacylglycerol molecule, a phosphate group esterfied to the 3rd OH group of glycerol, and an organic molecule esterfied to the phophate

Front 180

phospholipids are

Back 180

amphipathic, they have a nonpolar end(tail -hydrophobic)) and a polar end(head)

Front 181

terpenes

Back 181

long chained lipids built from 5-carbon isoprene units

Front 182

steroids

Back 182

are terpene derivatives that contain four rings of carbon atoms

Front 183

proteins

Back 183

macromolecues that are polymers formed from amino acids. have structural diversity.

Front 184

roles of proteins

Back 184

enzyme catalysis, defense, transport, structure/support, motion, regulation

Front 185

proteins are made from amino acids and amino acids are linked by?

Back 185

peptide bonds

Front 186

amino acids

Back 186

consist of a central or aloha carbon, bound to that carbon is a hydrogen atom

Front 187

the R group of an amino acid determines?

Back 187

the identity and much of the chemical properties of the amino acid

Front 188

plants and bacteria usually make their own?

Back 188

amino acids

Front 189

peptide bond

Back 189

joins the carboxyl group of one amino acid to the amino group of another, is formed by a condensation reaction

Front 190

dipeptide

Back 190

two amino acids fastened together by a peptide bond

Front 191

what determines the structure of a protein?

Back 191

the sequence of amino acids

Front 192

proteins have 4 levels of organization

Back 192

primary structure (1 degree)
secondary structure(2 degree)
tertiary structure(3 degree)
quaternary structure(4 degree)

Front 193

primary structure of a protein

Back 193

the sequence of amino acids in the peptide chain

Front 194

secondary structure of a protein

Back 194

results from hydrogen bonds involving the backbone, where the peptide chains is hld in structures, either a coiled aloha-helix or folded pleated sheet

Front 195

quaternary structure of a protein

Back 195

results from interactions between two or more seperate polypeptide chains. it is the 3-dimensional structure(the protein conformation)

Front 196

protein conformation

Back 196

the final three dimensional structure. this determines the function

Front 197

enzymes

Back 197

biological substances that regulate the rates of the chemical reactions in living organisms, most are proteins

Front 198

nucleic acids

Back 198

transmit hereditary info by determining what proteins a cell makes. are polymers made of nucleotide monomers

Front 199

two classes of nucleic acids

Back 199

DNA and RNA

Front 200

DNA

Back 200

carries the genetic info cells use to make proteins

Front 201

RNA

Back 201

functions in protein synthesis according to mechanisms

Front 202

a nucleotide consists of

Back 202

a 5-carbon sugar(ribose or deoxyribose), one or more phosphate groups, and a nitrogen base

Front 203

purines

Back 203

double-ringed nitrogen bases

Front 204

pyrimidines

Back 204

single-ringed nitrogen bases

Front 205

DNA typically contains the purines. . .
and the pyrimidines

Back 205

adenine(A) and guanine(G)

cytosine(C) and thymine(T)
A-T C-G

Front 206

RNA typically contains the purines. . .
and the pyrimidines

Back 206

adenine(A) and guanine(G)

cytosine(C) and uracil(U)

Front 207

nucleotides are fastened together by

Back 207

phosphodiester bonds

Front 208

DNA's structure is

Back 208

double helix, it is the hydrogen bonds hold strands together

Front 209

the two stralnds of DNA are

Back 209

antiparellel

Front 210

adenosine triphosphate(ATP)

Back 210

an important energy carrying compound in metabolism

Front 211

cyclic adenosine monophosphate(cAMP)

Back 211

is a hormone intermediary compound

Front 212

nicotinamide adenine dinucleotide(NAD+)

Back 212

an electron carrier which is oxidized or reduced in many metabolic reactions