Biology Ch 2

Front 1

matter

Back 1

anything that occupies space and has mass

Front 2

mass

Back 2

the quantity of matter in an object

Front 3

weight

Back 3

the pull of gravity on an object

Front 4

elements

Back 4

pure substances that cant be broken down chemically into different kinds of matter

Front 5

atom

Back 5

basic unit of matter. smallest unit taht still contains properties of that element

Front 6

atom

Back 6

democritus came up with this and means unable to be cut

Front 7

protons neutrons

Back 7

what make up the nucleus or center of the atom

Front 8

isotope

Back 8

atoms fo the same element taht differe int eh number of neurtrons they contain and have the same chemical properties

Front 9

radioactive isotope

Back 9

the nuclei of an isotope that are unstable and break down at a constant rate over time

Front 10

valence electrons

Back 10

the electrons in the outer level thatare used to form bonds

Front 11

molecule

Back 11

the structure that results from atoms joining in covalent bonds and is the smallest unit of most compounds or two atoms of the same element taht join together

Front 12

compounds

Back 12

a substance formed by the chemical combination of two or more elements in definite proportions. and the physical and chemical properties are different from those of the elements from which it is formed

Front 13

isomer

Back 13

molecules with the same chemical formula but different structural fomulas

Front 14

stable atoms

Back 14

an atom with a filled outer shell

Front 15

covalent bnd

Back 15

when electrons are shared between atoms and the electrons travel about the nuclei of both atoms

Front 16

nonpolar bonding

Back 16

in a covalent bond if the sharing is equal it is...

Front 17

polar bonding

Back 17

in a covalent bond if the sharing is unequal it is..

Front 18

ionic bond

Back 18

when you transfer one or more electrons from one atom to another atom

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positive

Back 19

if an atom loses an electron it becomes

Front 20

negative

Back 20

if an atom gains an electron it becomes

Front 21

ions

Back 21

positively and negatively charged electrons that have different amounts of electrons

Front 22

cationp

Back 22

positve ion

Front 23

anion

Back 23

negative ion

Front 24

van der waals forces

Back 24

in an atom the rapid movement of electrons can create regions on a molecule taht have a tiny positive or negative charge and a slight attraction can develop between the regions . these intermolecular forces are

Front 25

polarity of water

Back 25

because oxygen has eight protons, the oxygen atom has a stronger attraction for the electrons in the covalent bond so the oxygen is on one end and the hydrogen atoms are on the other. the oxygen has a slight negative charge and the hydrogen end has a slightly positive charge

Front 26

hydrogen bonding

Back 26

when the polor molecules are attracted to each other. its the attraction of a hydrogen atom one one water molecule to an oxygen atom of another.

Front 27

intermolecular

Back 27

forms between molecules

Front 28

intramolecular

Back 28

froms insike a molecule (weak)

Front 29

cohesion

Back 29

an attraction between molecules fo the same substance

Front 30

cohesion

Back 30

causes water molecules to be drawn together(drops of water fomr beads) produces surface tension, reason why insects can wal on water

Front 31

adhesion

Back 31

an attraction between molecules of different substances

Front 32

adhesion

Back 32

makes the surface of water dip slightly in the center

Front 33

capillary action

Back 33

adhesion between water and glass causes water to rise in a narrow tube against the force of gravity

Front 34

capillary action

Back 34

helps draw water out of roots of a plant and up into its stems and leaves. ex solored water moving through caronation

Front 35

heat capacity

Back 35

it takes a large amount of heat energy to cause molecules to move faster and raise the temperature of water because of the hydrogen bonds between water

Front 36

heat capacity

Back 36

the amount of heat energy required to increase its temperature . waters is high

Front 37

mixtures

Back 37

a material composed of two or more elements or conpounds that are physically mixed together but not chemically combined

Front 38

solutions

Back 38

mixture in which one or more substances are uniformly distributed in another substance. all components are evenly distributed

Front 39

solution

Back 39

salt water is a blank

Front 40

solute

Back 40

the substance that is dissolved in amixture

Front 41

solvent

Back 41

water is an example of a

Front 42

solvent

Back 42

substance in which the solute is dissolved

Front 43

solute

Back 43

table salt and sugar in salt water are an example of

Front 44

aqueous solution

Back 44

a solution in which water is the solvent

Front 45

dissociation of waater

Back 45

when salt comes away from each other in water

Front 46

concentration of a solution

Back 46

measurement of the amount of solute dissolven in a fixed amount of the solution

Front 47

saturated solution

Back 47

when a given amount fo water has dissolved all of the solut it can. a solution in which no more solute can be added

Front 48

acidic solution

Back 48

solution with a ph below 7

Front 49

acidid

Back 49

a solution with more h plus ions than oh minus ions

Front 50

hydronium

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hydrogen ion

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hydroxide

Back 51

oh minus ion

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basic

Back 52

solutions with ph above 7

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basic

Back 53

a solution that has more oh minus ions that h plus ions

Front 54

neutral solution

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a solution with ph level 7

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neutral solution

Back 55

oh minus and h plus ions are equal

Front 56

buffers

Back 56

chemical substance that neutralizes small amounts of acid or base. prevent sharp sudden cahnges in the normal ph level

Front 57

suspensions

Back 57

mixtures of water and nondissolved particles that separate into small pieces and dont settle out

Front 58

chnops

Back 58

elements of life

Front 59

4

Back 59

how many valence electrons do carbon atoms have

Front 60

carbon compound

Back 60

when two carbon atoms covalently bond form

Front 61

hydrocarbons

Back 61

molecules containing only carbon and hydrogen atoms

Front 62

carbon bonds

Back 62

when the carbon atoms do this it gives carbon the ability to form chains that are almos unlimited in length and can form millions of different large and complex structures

Front 63

functional groups

Back 63

when clusters of atoms are added to a hydrocarbon and it influences the prperties of the molecule and determines characteristics of the compound

Front 64

monomer

Back 64

the smaller simpler molecues that are bound together to make polymers

Front 65

polymers

Back 65

large complex molecules with the repeating units(monomers)

Front 66

condensation reaction

Back 66

when a monomer goes to a polymer

Front 67

dehydration synthesis

Back 67

which uses endergonic

Front 68

dehydration synthesis

Back 68

which uses anabolic

Front 69

hydrolosis

Back 69

goes from a polymer to a monomer

Front 70

hydrolosis

Back 70

which is exergonic

Front 71

hydrolosis

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which is catabolic

Front 72

macromolecules

Back 72

made from thousands of smaller molecules or large molymers

Front 73

inorganic molecules

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water and carbon dioxide

Front 74

inorganic molecules

Back 74

what we need to live

Front 75

inorganic molecules

Back 75

smaller simpler molecues

Front 76

organic molecules

Back 76

large complex carbon containing molecules

Front 77

organic

Back 77

carbohydrates, lipids, nucleic acids, proteins

Front 78

sugars starches cellulose glycogen

Back 78

what are examples of carbohydrates

Front 79

monosaccharides

Back 79

what are the monomers of carbohydrates

Front 80

monosaccharides

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single or simple sugars

Front 81

glucose fructose galactose ribose deoxyribose

Back 81

what are examples of monosaccharides

Front 82

disaccharides

Back 82

double sugars

Front 83

disaccharides

Back 83

what are the dimers of carbohydrates

Front 84

glucose and glucose

Back 84

what makes up maltose( malt sugar)

Front 85

glucose fructose

Back 85

what makes up sucrose

Front 86

glucose galactose

Back 86

what makes up lactose

Front 87

maltose sucrose lactose

Back 87

examples of disaccharides

Front 88

polysaccharides

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polymers of carbohydrates

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polysaccharides

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many complex sugars 3 or mor sugars linked together byteh process of dehydration synthesis

Front 90

glycogen starch cellulose

Back 90

examples of polysaccharides

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glycogen

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animal starch

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starch

Back 92

in plants

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cellulose

Back 93

in plant cell walls

Front 94

carbon and hydrogen a little oxygen

Back 94

what elements do lipids contain

Front 95

store energy

Back 95

lipids are large and nonpolar( wont dissolve in water and are used to blank blank

Front 96

glycerol fatty acid chains

Back 96

monomers of lipids

Front 97

fats oils waxes steriods

Back 97

polymers of lipids

Front 98

saturated fatty acids

Back 98

when it holds the max number of hydrogen atoms, mo double bonds between the carbons

Front 99

saturated fatty acids

Back 99

solid at room temperature

Front 100

unsaturated fatty acids

Back 100

dont hold max number of hydrogen atomes, and have one or more double bonds between carbons

Front 101

unsaturated fatty acids

Back 101

liquid at room temperature

Front 102

triglycerides

Back 102

3 molecules of fatty acids to one glycerol

Front 103

phospholipid

Back 103

2 fatty acid chains and one phosphorous group linked to one glycerol

Front 104

nucleic acids

Back 104

store and transmit hereditary or genetic information

Front 105

nucleotides

Back 105

monomers of nucleic acids

Front 106

5 carbon sugar phosphate group nigrogenous base

Back 106

what do nucleotides contain

Front 107

deoyribonucleic ribonucleic

Back 107

polymers of nucleic acids

Front 108

nitrogen carbon hydrogen oxygen

Back 108

what elements do proteins contain

Front 109

enzymes horomones blood muscles membrane proteins toxins

Back 109

examples of proteins

Front 110

amino acids

Back 110

monomers of proteins

Front 111

proteins

Back 111

polymers of proteins

Front 112

peptide bond

Back 112

bond that holds to amino acids together

Front 113

amino and carboxyl

Back 113

amino acids can be joined together by bonding what two groups

Front 114

polypeptides

Back 114

many amino acids are linked together. the functional groups of the individual amino acids influences the shape and the shape determines the function

Front 115

primary structure

Back 115

sequence of a proteins amino acids.

Front 116

secondary structure

Back 116

folding or coiling ofthe polypeptide chains

Front 117

tertiary structure

Back 117

complete three dimensional arrangement of a polypeptide chain gives globular shape