A&p Chapter 2

Front 1

Matter

Back 1

Anything that has mass and occupies space

Front 2

Element

Back 2

Simple form of matter a substance that cannot be broken down into two or more different substances

Front 3

Ther are how many elements in the human body

Back 3

26

Front 4

There how 11 major elements 4 of which are

Back 4

carbon, oxygen, hydrogen, and nitrogen and they make up 96% of the human body.

Front 5

There are 15 trace elements that make up less than how much of body weight?

Back 5

2%

Front 6

Compound

Back 6

Atoms of 2 or more elements joined to form chemical combinations.

Front 7

The concept of an atom was proposed by a chemist named

Back 7

John Dalton

Front 8

Atoms contain several different kinds of subatomic particiles the most importan are

Back 8

Protons, nuetrons, electrons

Front 9

Protons

Back 9

are positively charged subatomic particles found in the nucleus

Front 10

Nuetrons

Back 10

have a neutral subatomic particles found in the nucleus

Front 11

Electrons

Back 11

Negatively charged subatomic particles found in the electron cloud

Front 12

Atomic Number and Atomic Weight

Back 12

The number of protons in an atom's nucleus and the atomic number is critically important; it identifies the kind of element

Front 13

Atomic Weight

Back 13

The mass of a single atom and it is equal tothe number of protons plus the number of neutrons in the nucleus (p+n)

Front 14

The total number of electorns in an atom equals the number of what in the nucleus?

Back 14

Protons

Front 15

The electrons form a what around the nucleus?

Back 15

Cloud

Front 16

Bohr Model

Back 16

A model resembling planets revolving around the sun, useful in visualizing the structure of atoms.

Front 17

Exhibits electrons in concentric circles showing relative distances of the electrons from the

Back 17

Nucleus

Front 18

Each ring or shell represents a specific energy level and can hold only a certain number of

Back 18

Electrons

Front 19

The number of arrangements of electrons determine whether a what is chemically stable?

Back 19

Atom

Front 20

An Atom with how many pairs of electrons in the outermost energy level is chemically inert?

Back 20

8 or 4 pairs

Front 21

An atom without a full outermost energy level is?

Back 21

Chemically active

Front 22

Atoms with fewer or more than eight electrons in the outer energy level will attempt to lose, gain, or share electrons with other atoms to achieve stability

Back 22

Octet Rule

Front 23

Isotopes of an element contain the same number of protons but differnt number of

Back 23

Neutrons

Front 24

Isotopes have the same atomic number and the same basic chemical properties as any other atom of the same element but they have different

Back 24

Atomic Weight

Front 25

An unstable isotope that undergoes nuclear breakdown and emits nuclear particles and radiation.

Back 25

Radioactive isotope

Front 26

Chemical Reaction

Back 26

Interaction between tow or more atoms that occurs as a result of activity between electrons in their outermost energy levels

Front 27

Molecule

Back 27

2 or more atoms joined together

Front 28

Compound

Back 28

Consists of molecules formed by atoms of 2 or more elements

Front 29

Chemical bonds

Back 29

2 types unite atoms into molecules

Front 30

Ionic Bond

Back 30

Formed by transfer of electrons; strong electrostatic force that binds positively and negatively charge ions together

Front 31

Formed by sharing of electron pairs between atoms

Back 31

Covalent Bond

Front 32

Much weaker than ionic or covalent bonds and results from unequal chage distribution on molecules

Back 32

Hydrogen Bonds

Front 33

Hydrogen Bonds

Back 33

Form when electrons are unequally shared For example water molecule

Front 34

Polar molecules have regions with partial electrical charges resulting fromm unequal sharing of electrons among atoms

Back 34

Hydrogen Bonds

Front 35

Area of different partial charges attract one another and form

Back 35

Hydrogen Bonds

Front 36

Involve the formation or breaking of chemical bonds

Back 36

Chemical Reactions

Front 37

Combining of 2 or more substances to form a more complex substance; formation of new chemical bonds: A+B=AB

Back 37

Synthesis

Front 38

Breaking down of a substance into 2 or more simpler substances; breaking of a chemical bonds AB = A+B

Back 38

Decomposition reaction

Front 39

Reversible reaction occur

Back 39

In both directions

Front 40

Metabolism

Back 40

All of the chemical reactions that occur in body cells

Front 41

Catabolism

Back 41

Chemical reactions that break down complex compounds into simpler ones and release energy; hydrolysis is a common catabolic reaction

Front 42

What are the end results of Catabolism?

Back 42

Carbon dioxide, water, and other waste products

Front 43

More than half the energy release during Catabolism is transferred to what whcih is then used to do cellular work?

Back 43

ATP

Front 44

Chemical reactions that join simple molecules together to form more complex molecules

Back 44

Anabolism

Front 45

Chemical reactions responsibile for anabolism is

Back 45

Dehydration Synthesis

Front 46

Molecule

Back 46

2 or more atoms joined together

Front 47

Compound

Back 47

molecules formed by atoms of 2 or more elements

Front 48

Chemical bonds

Back 48

2 types unite atoms into molecules

Front 49

Ionic or electrovalent bonds

Back 49

formed by transfer of electrons; strong electrostatic force that binds positively and negatively charged ions together

Front 50

Covalent Bond

Back 50

formed by sharing of electron pairs between atoms

Front 51

Hydrogen bond

Back 51

Much weaker that inoic or covalent bonds; result from unequal charge distribution on molecules

Front 52

Hydrogen bonds from when

Back 52

electrons are unequally shared like WATER molecule.

Front 53

Polar molecules have regions

Back 53

with partial electrical charges resulting from unequal sharing of electons amoung atoms

Front 54

Chemical Reactions involve the formation or breaking of

Back 54

Chemical bonds

Front 55

3 types of chemial reactions involved in physiology

Back 55

Synthesis reaction, Decomposition reaction, exchange reaction

Front 56

Synthesis Reaction

Back 56

combining 2 or more substances to form a more complex substance fromation of new chemical bonds; A+B=AB

Front 57

Decomposition reaction is

Back 57

Breaking down of a substance into 2 or more simplier substances; breaking of chemical bonds AB=A+B

Front 58

Exchange Reaction is

Back 58

decomposition of 2 substances and in exchange synthesis of 2 new compounds for them: AB+CD=AD +CB

Front 59

Metabolism

Back 59

all of the chemical reactions that occur in body cells

Front 60

Catabolism

Back 60

chemical reactions that break down complex compounds into simpler ones and release energy; hydrolysis is a common catabolic reaction

Front 61

Ultimately the end porducts of what are carbon dioxide, water, and other waste products

Back 61

Catabolism

Front 62

Catabolism involves more than half of the energy released in transferred to what which is used to do cellular work

Back 62

ATP

Front 63

Anabolism is

Back 63

Chemical reaction that join simple molecules together to form more complex molecules

Front 64

What chemical reaction is responsibile for anabolism

Back 64

dehydration synthesis

Front 65

These have few carbon atoms and none have C-C or C-H bonds

Back 65

Inorganic compounds

Front 66

These have at least 1 carbon atom and at least one C-C or C-H bond in each molecule

Back 66

Organic Molecules

Front 67

Organic Molecules often have

Back 67

Functional groups attached to the carbon containing core of the molecule

Front 68

Inorganic molecules are properties of

Back 68

Water

Front 69

The body's most abundant and important compound is

Back 69

Inorganic molecules

Front 70

This allows water to act asw an effective solvent

Back 70

Polarity

Front 71

This solvent allows transportation of essential materials throughout the body

Back 71

Inorganic molecules

Front 72

Water can loose and gain large amounts of heat with little change in its own temperature; enables the body to maintain a relatively constant temperature

Back 72

High specific heat

Front 73

water requires the absorption of significant amounts of heat to change it from a liquid to a gas allows the body to sissipate excess heat

Back 73

High heat of vaporization

Front 74

Required to complete decomposition reactions necessary for the release of energy in the body

Back 74

Oxygen

Front 75

Carbon Dioxide

Back 75

Produced as a waste product and also helps maintain the appropriate acid-base balance in the body

Front 76

Large group of inorganic compounds that includes acids bases and salts

Back 76

Electrolytes

Front 77

Substances that dissociate in solution to form ions

Back 77

Electrolytes

Front 78

Postively charged ions are

Back 78

cations

Front 79

Negatively charged ions are

Back 79

anions

Front 80

Any substances that releases a hydrogen ion (H+) when in solution; "proton donor"

Back 80

Acid

Front 81

Level of what depends on the number of hydrogen ions a particular acid will relaease

Back 81

Acidity

Front 82

Electrolytes that dissociate to yield hydroxide ions (OH-) or other electrolytes that combine with hydrogen ions (H+)

Back 82

Bases

Front 83

Bases are described as

Back 83

Proton Acceptors

Front 84

PH Scale

Back 84

Assigns the value to measure of acidity or alkalinity of a solution

Front 85

PH indicates

Back 85

The degree of acidity or alkalinity of a solution

Front 86

PH of 7 indicates

Back 86

Neutrality; equal amounts of H+ and OH-;

Front 87

a pH less than 7 indicates

Back 87

Acidity

Front 88

A pH of higher than 7 indicates

Back 88

Alkalinity

Front 89

Buffers

Back 89

maintain constancy of pH and minimize changes in the concentrations of h+ and OH- ions

Front 90

These act as a reservior for hydrogen ions

Back 90

Buffers

Front 91

Compunds that result from chemical interaction of an acid and a base

Back 91

Salts

Front 92

Reaction between an acid and a base to form a salt and water is called a

Back 92

Neutralization reaction

Front 93

This describes compounds that contain C-C or C-H bonds

Back 93

Organic

Front 94

Organic compounds containing carbon hydrogen, and oxygen commonly called sugars and starches

Back 94

Carbohydrates

Front 95

Monosaccharides are

Back 95

Simple sugars with short carbon chains those with 6 carbons are hexoses whereas those with 5 are pentoses

Front 96

2 (di) or more (poly) simple sugars that are bonded together through a synthesis reaction

Back 96

Disaccharides and Polysaccharides

Front 97

Water-insoluble organic molecules that are critically important biological compounds are

Back 97

Lipids

Front 98

Lipids major roles:

Back 98

Energy source, structural role, and Integral parts of cell membranes

Front 99

Triglycerides or fats

Back 99

Most abundant lipids and most concentrated source of energy

Front 100

The building blocks of Triglycerides are

Back 100

Glycerol and fatty acids

Front 101

Types of fatty acids

Back 101

saturated fatty acid and unsaturated fatty acid

Front 102

Triglyerides are formed by a

Back 102

Dehydration synthesis

Front 103

Fat compounds similar to triglyceride

Back 103

Phospholipids

Front 104

One end of phospholipids is water soluble

Back 104

Hydrophilic

Front 105

The other end of a phosphilipids

Back 105

is fat soluble-- hydrophobic

Front 106

These can join 2 different chemical environments

Back 106

Phospholipids

Front 107

Phospholipids can form double layers called bilayers that make up

Back 107

Cell Membrane

Front 108

Main component is steroid nucleus

Back 108

Steroids

Front 109

Steriods are involved in many

Back 109

Structural and functional roles

Front 110

Commonly called tissue hormones produced by cell membranes throughout the body

Back 110

Prostaglandins

Front 111

Most abundant organic compounds; chain like polmers

Back 111

Proteins

Front 112

These are building blocks of proteins

Back 112

Amino acids

Front 113

8 amino acids that cannot be produced by the human body

Back 113

Essential amino acids

Front 114

Nonesssential amino acids

Back 114

12 amino acids can be produced from molecules available in the numan body

Front 115

Amino acids consist of

Back 115

carbon atom, an amino group, a carboxyl group a hydrogen atom and a side chain

Front 116

There are 4 levels of proten organization

Back 116

Primary structure, Secondary Structure, Tertiary Structure, and Quaternary Structure

Front 117

Functional shape of the protein molecules is called the

Back 117

Native state

Front 118

Structional proteins form the structures of the

Back 118

Body

Front 119

Funtional proteins cause chemical changes in the

Back 119

Molecules

Front 120

Denatured proteins have lost their shape and therefore their

Back 120

Function

Front 121

Proteins can be denatured by changes in pH, temperature, radiation and

Back 121

Other chemicals

Front 122

If the chemical environment is restored proteins may be renatured and

Back 122

Funtion normally

Front 123

DNA funtions as the molecule of

Back 123

Heredity

Front 124

Base pairs holds how many chains of DNA molecule together?

Back 124

2 chains

Front 125

DNA is composed of

Back 125

deoxyribonucleotides, that is, structural units composed of the pentose sugar, phosphate group, and notrogenous base

Front 126

RNA is composed of

Back 126

pentose sugar, phosphate group, and a nitrogenous base

Front 127

Some RNa molecules are temporary copies of the

Back 127

DNA code

Front 128

These are regulatory and act as enzymes

Back 128

Some RNA molecules

Front 129

Nucleotides have important roles in the body such as

Back 129

ATP, 3 phosphate subunits

Front 130

Energy stored in ATP is used to

Back 130

Do the body's work

Front 131

ATP is often called the

Back 131

Energy Currency of cells