Anatomy & Phisiology Chapter 2

Front 1

bio-

Back 1

life; biochemistry

Front 2

Biochemistry

Back 2

branch of science dealing with the chemistry of life forms.

Front 3

di-

Back 3

two

Front 4

disaccharide

Back 4

compound whose molecules are composed of two saccharide unit bound together

Front 5

glyc-

Back 5

sweet

Front 6

iso-

Back 6

equal

Front 7

isotope

Back 7

atom that has the same atomic number as another atom but a different atomic weight

Front 8

lip-

Back 8

fat

Front 9

lipids

Back 9

group organic compound that includes fats

Front 10

-lyt

Back 10

dissolvvable

Front 11

electrolyte

Back 11

substance that dissolves in water and releases ions

Front 12

mono-

Back 12

one

Front 13

monosaccharide

Back 13

compound whose molecule consists of a single saccharide unit

Front 14

poly-

Back 14

many

Front 15

polyunsaturated

Back 15

molecule that has many double bonds between its carbon atoms

Front 16

sacchar-

Back 16

sugar

Front 17

molecular formula

Back 17

abbreviation for the number of atoms of each element in a compound

Front 18

nucleus

Back 18

cellular organelle enclosed by a double layered porous membrance and containing DNA; the dense core of anatom thatis composed of protons and neutrons

Front 19

atomic number

Back 19

number of protons in an atom of an element

Front 20

atomic weight

Back 20

number of protons plus the number of neutrons in am atom of an element

Front 21

inert

Back 21

nonreactive with other elements

Front 22

ions

Back 22

atom or molecule with an electrical charge

Front 23

bond

Back 23

connection between atoms in a compound

Front 24

electron shells

Back 24

the path formed by an electron or several electrons encircling the nucleus of an atom at a particular energy level

Front 25

reactants

Back 25

substance entering a chemical reaction

Front 26

cations

Back 26

atom carrying a positve charge due to a deficiency of electrons

Front 27

anions

Back 27

atom carrying a negative charge due to one or more extra electrons

Front 28

products

Back 28

something produced as a result of a chemical reaction

Front 29

ionic bonds

Back 29

chemical bond formed between two ions by transfer of electrons; electrovalent bond

Front 30

structural formula

Back 30

representation of the way atoms bond to form a molecule, using symbols for each element and lines to indicate chemical bonds

Front 31

polar molecule

Back 31

combination of atoms in which the electrical charge is not distributed symmetrically

Front 32

hydrogen bond

Back 32

weak bond between a hydrogen atom and atom of oxygen or nitrogen

Front 33

syn-

Back 33

together

Front 34

synthesis

Back 34

process by which substances are united to form a new new type of substances

Front 35

-valent

Back 35

having power

Front 36

covalent bond

Back 36

chemical bond produced when two atoms share electrons

Front 37

atom

Back 37

smallest particle of an element that has the properties of that element

Front 38

electron (e-)

Back 38

extremely small particle with almost no weight; carried a negative electrical charge and is in constant motion around an atomin nucleus

Front 39

proton (p+)

Back 39

relatively large atomic particles; carries a postive electrical charge and is found within an atomic nucleus

Front 40

neutron (nO)

Back 40

particles with about the same weight as a protom; uncharged and thus electrically neutral; found within an atomic nucleus

Front 41

decomposition

Back 41

the breakdown of molecules into simpler compounds

Front 42

molecule

Back 42

particle formed by the chemical union of two or more atoms

Front 43

matter

Back 43

anything that has weight and occupies space

Front 44

element

Back 44

chemical substance with only one type of atom

Front 45

compound

Back 45

substanse composed of two or more chemically bonded elements

Front 46

bulk elements

Back 46

basic chemical subustance needed in a large quantity

Front 47

trace elements

Back 47

basic chemical substance needed in small quantity

Front 48

Ultratrace element

Back 48

basic element substance needed in very small quantity

Front 49

glycogen

Back 49

complex carbohydrate composed of sugar molecules bound together in a particular way

Front 50

exchange reaction (replacement reaction)

Back 50

parts of two diferent kinds of molecules trade positions as bond are bond and new bonds are formed.
AB + CD -> AD + CD

Front 51

reversible reaction

Back 51

the product or products can change back to the reactant or reactants.

A + B <=> AB

Front 52

Catalyst

Back 52

molecules that influence the rates (not the direction) of chemical reaction but are not consumed in the process.

Front 53

Acid

Back 53

substance that releases hydrogen ions (H+)

Front 54

base

Back 54

substance that release ions that can combine with hydrongen ions

Front 55

salt

Back 55

substance formed by the reaction between an acid and a base

Front 56

alkalosis

Back 56

pH of 7.5 to 7.8, makes one feel agitated and dizzy can be caused by breathing rapidly att high altitudes, taking too many antacids, high fever, anxiety, or mild to moderate vomiting.

Front 57

Acidosis

Back 57

pH 7.0 to 7.3, makes one feel disoriented, fatigues, breathing may become difficult.

Front 58

Buffers

Back 58

substance that can react with strong acid or base to form a weaker acid or base and thus resist a change in pH

Front 59

organic

Back 59

compounds have carbon and hydrogen

Front 60

inorganic

Back 60

chemical substances that lack carbon and hydrogen

Front 61

water

Back 61

h2o

Front 62

oxygen

Back 62

o2

Front 63

carbon dioxide

Back 63

co2

Front 64

electrolyte balance

Back 64

condition when the qualities of electrolytes entering the body equal those leaving it

Front 65

Distinguish between chemistry and biochemistry.

Back 65

Chemistry is the study of the composition of substances and how they change. Biochemistry is the chemistry of living organisms.

Front 66

Explain the relationship between elements and atoms.

Back 66

An element is a basic substance that other things are composed from. Each individual element is made up of tiny, invisible particles called atoms. The atom is the smallest complete unit of an element.

Front 67

Define compound.

Back 67

A compound is the product of two or more elements being combined.

Front 68

List the four most abundant elements in the human body.

Back 68

The four most abundant elements are hydrogen, oxygen, carbon, and nitrogen.

Front 69

Describe the major parts of an atom.

Back 69

Each atom is composed of a central portion, called a nucleus, and one or more electrons that are in constant motion around the nucleus. The nucleus contains one or more large particles called protons, and can also contain one or more similarly-sized particles called neutrons.

Front 70

Distinguish between protons and neutrons.

Back 70

Protons carry a single, positive electrical charge (p+). Neutrons are uncharged and thus are electrically neutral (n0).

Front 71

Define matter.

Back 71

Matter is anything that has weight and takes up space

Front 72

Explain why a complete atom is electrically neutral.

Back 72

The electron carries a single negative electric charge. The protons carry a single positive electric charge.
Neutrons carry no charge, thereby making them electrically neutral. The atom is electrically neutral because there is the exact same number of protons and electrons, which effectively cancel each other out.

Front 73

Distinguish between atomic number and atomic weight

Back 73

Atomic number represents the number of protons in an atom of a particular element. Since atoms are electrically neutral, it also tells you the number of electrons. Atomic weight represents the number of protons plus the number of neutrons in an atom of a particular element

Front 74

Define isotope

Back 74

Isotopes are elements with the same atomic number but different atomic weights

Front 75

Define atomic radiation

Back 75

Atomic radiation is the energy or atomic fragments that are given off by unstable isotopes

Front 76

Describe how electrons are arranged within atoms

Back 76

The electrons of an atom are found in one or more shells around the nucleus. The maximum number of
electrons that each of the first three inner shells can hold is as follows:
First shell (closest to the nucleus) 2 electrons
Second shell 8 electrons
Third shell 8 electrons

Front 77

Explain why some atoms are chemically inert

Back 77

An atom is chemically inert when the outermost electron shells are filled. These atoms cannot form chemical bonds

Front 78

Distinguish between an ionic bond and a covalent bond

Back 78

An ionic bond (electrovalent bond) is formed when atoms gain or lose electrons. A covalent bond forms when atoms share electrons

Front 79

Distinguish between a single covalent bond and a double covalent bond

Back 79

A single covalent bond occurs when atoms share one pair of electrons.
A double covalent bond occurs when atoms share two pairs of electrons.

Front 80

Explain the relationship between molecules and compounds

Back 80

A molecule is formed when two or more atoms of the same element bond together. A compound is formed when two or more elements of different atoms combine

Front 81

Distinguish between a molecular formula and a structural formula

Back 81

A molecular formula consists of the symbols of the elements in the molecule together with numbers to
indicate how many atoms of each element are present. It is essentially the recipe for that particular molecule or compound. A structural formula is drawn to represent how atoms are joined and arranged in various molecules. This is essentially the blueprint of how they fit together

Front 82

What are the three types of chemical reactions.

Back 82

synthesis reaction
decomposition reaction
exchange reaction

Front 83

synthesis reaction

Back 83

occurs when two or more reactants bond together to make a new and more complex product. It can be symbolized as follows:
A + B = AB

Front 84

decomposition reaction

Back 84

occurs when a more
complex substance is broken apart into smaller, simple substances. It can be symbolized as follows:
AB = A + B

Front 85

exchange reaction

Back 85

occurs when parts of two molecules change positions. It can be symbolized as follows: AB + CD = AD + CB

Front 86

Explain what is meant by reversible reaction

Back 86

A reversible reaction is one in which the end product (or products) of the reaction can changed back to the
reactant (or reactants) that originally underwent the reaction A + B = AB

Front 87

Explain what pH measures

Back 87

pH measures the concentration of hydrogen ions found in substances

Front 88

Distinguish between organic and inorganic substances

Back 88

An organic substance contains both carbon and hydrogen atoms. An inorganic substance lacks carbon atoms

Front 89

Describe the roles played by water and by oxygen in the human body

Back 89

Water is the most abundant substance in the human body. It is a major component of blood and other body fluids. It is an important solvent. It also has an important role in the transportation of chemicals in the body.
Additionally, water can absorb and transport heat. Oxygen is used by cellular organelles in the process of releasing energy from glucose and certain other molecules. The resultant energy is used to drive the cell’s metabolic activities

Front 90

List several ions that cells require, and describe their general functions

Back 90

Sodium (Na+), chlorine (Cl-), potassium (K+), calcium (Ca+), magnesium (Mg+2), phosphate (PO4-3), carbonate (CO3-2), bicarbonate (HCO3-), and sulfate (SO4-2) are the ions that play important roles in metabolic processes. These processes include maintenance of proper water concentrations and nerve functions, in body fluids, pH, blood clotting, bone development, energy transfer within cells, and muscle function

Front 91

Define electrolyte balance

Back 91

Electrolyte balance is the condition where the electrolytes are present in certain concentrations, both inside and outside cells, to maintain homeostasis

Front 92

Describe the general characteristics of carbohydrates

Back 92

Carbohydrates supply much of the energy for the cells. They supply building materials for certain cell
structures and are often stored as reserve energy. These molecules contain atoms of carbon, hydrogen, and oxygen. Carbohydrates usually have twice as many hydrogen as oxygen atoms. The carbon atoms are joined in chains that vary in length with the specific kinds of carbohydrates

Front 93

Distinguish between simple and complex carbohydrates

Back 93

Simple carbohydrates are the six-carbon sugars known as simple sugars. Complex carbohydrates are
formed when a number of simple sugar molecules are bound together to form molecules of varying size.

Front 94

Describe the general characteristics of lipids.

Back 94

Lipids are organic substances that are insoluble in water but soluble in certain organic solvents. They supply more energy, gram for gram, than carbohydrates. They contain carbon, hydrogen, and oxygen. Lipids contain a much smaller proportion of oxygen than carbohydrates

Front 95

Distinguish between saturated and unsaturated fats

Back 95

A saturated fat contains no double bonds between carbon atoms. An unsaturated fat contains one or more double bonds between carbon atoms

Front 96

Describe the general characteristics of proteins

Back 96

Proteins can be used as structural materials, energy sources, hormones, and receptors on cell surfaces that are specialized to bond to particular kinds of molecules. Others act as antibodies against foreign substances that can enter the body. Still others act as enzymes in metabolic processes. Proteins contain atoms of carbon, hydrogen, and oxygen. In addition, they always contain nitrogen atoms, and sometimes contain sulfur atoms as well.

Front 97

Describe the function of an enzyme

Back 97

An enzyme is a molecule that acts as a catalyst in living systems. That is, it speeds specific chemical reactions without being consumed or changed in the process.

Front 98

Explain how protein molecules may become denatured

Back 98

When protein molecules lose their unique shape and become disorganized, they become denatured. This can be a result of exposure to excessive heat, radiation, electricity, or various chemicals. When they become denatured, it is a permanent change and they are therefore nonfunctional

Front 99

Describe the general characteristics of nucleic acids

Back 99

Nucleic acid molecules are generally very large and complex. They contain atoms of carbon, hydrogen, oxygen, nitrogen, and phosphorus. These are bound into building blocks called nucleotides

Front 100

Explain the general functions of nucleic acids

Back 100

These control all cell activities. They store information that is used by cell parts to construct specific kinds of protein molecules, including enzymes