A&p Ch.2 Lecture Notes

Front 1

the stuff of the universe

Back 1

matter

Front 2

anything that has mass and takes up space

Back 2

matter

Front 3

has definite shape and volume

Back 3

Solid

Front 4

has definite volume, changeable shape

Back 4

Liquid

Front 5

has changeable shape and volume

Back 5

gas

Front 6

the capacity to do work (put matter into motion).

Back 6

Energy

Front 7

energy in action

Back 7

kinetic

Front 8

energy of position; stored (inactive) energy.

Back 8

potential

Front 9

stored in the bonds of chemical substances

Back 9

Chemical

Front 10

Results from the movement of charged particles - Battery

Back 10

Electrical particles

Front 11

Directly involved in voving matter

Back 11

Mechanical

Front 12

Energy traveling in waves (visible light, ultraviolet light, and X-rays).

Back 12

Radiant or electromagnetic

Front 13

Energy is easily _____ from one form to another.

Back 13

Converted

Front 14

During ____ some energy is "lost" as heat.
The "lost" energy is not in a useable form to do work. It might be better to call it waste heat. It is this waste heat that keeps us warm.

Back 14

Conversion

Front 15

Unique substances that cannot be broke down by ordinary chemical means

Back 15

Elements

Front 16

More-or-less identical building blocks for each element

Back 16

Atoms

Front 17

one or two letter chemical shorthand for each element

Back 17

Atomic Symbol

Front 18

Each ____ has unique physical and chemical properties.

Back 18

element

Front 19

those detected with our senses and can be tested without changing the material

Back 19

physical properties

Front 20

pertain to the way atoms interact with one another

Back 20

Chemical properties

Front 21

Name the major elements of the human body

Back 21

* Oxygen
* Carbon
* Hydrogen
* Nitrogen

Front 22

____ elements that make up 3.9% of the body and include
* Calcium, phosphorus, potassium, sulfur, sodium, chlorine, magnesium, iodine, and iron.

Back 22

Lesser Elements

Front 23

____ elements make up less than 0.01% of the body
* they are required in minute amounts, and are found as part of enzymes.

Back 23

Trace Elements

Front 24

The ____ consists of neutrons and protons

Back 24

Nucleus

Front 25

____ have no charge and a mass of one atomic mass unit

Back 25

Neutrons

Front 26

_____ have a positive charg and a mass of 1 amu and are responsible for the identity of the element.

Back 26

Protons

Front 27

____ are found in regions surrounding the nucleus and are equal in number to protons in the nucleus of an element

Back 27

Electrons

Front 28

____ have a negative charge and negligible mass

Back 28

Electrons

Front 29

_____ model - electrons move around the nucleus in fixed, circular orbits.

Back 29

Planetary Model

Front 30

____ Model - regions around the nucleus in which electrons are most likely to be found.

Back 30

Orbital

Front 31

____ ____- equal to the number of protons (Ex: 75 protons)

Back 31

Atomic Number = 75

Front 32

Equal to the mass of the protons and neutrons

Back 32

Mass Number

Front 33

Average of the mass numbers of all isotopes.

Back 33

Atomic weight

Front 34

Atoms with same number of protons but a different number of neutrons

Back 34

Isotope

Front 35

Atoms that undergo spontaneous decay called radioactivity

Back 35

Radioisotopes

Front 36

two or more atoms held together by chemical bonds

Back 36

molecule

Front 37

two or more different kinds of atoms chemically bonded together by electrostatic attraction (a metal and a nonmetal)

Back 37

Ionic compound

Front 38

two or more components physically intermixed (not chemically bonded)

Back 38

Mixtures

Front 39

Homogeneous mixtures of components

Back 39

Solutions

Front 40

substance present in greatest amount

Back 40

solvent

Front 41

substance(s) present in smaller amounts

Back 41

Solute

Front 42

percent, or parts per 100 parts
* In biology ____ solutions are often preferred to molar ones. A 1% solution would have 1g of solute dissolved in a final volume of 100 ml of solution. this would be labeled as a weight/volume solution.

Back 42

percentage

Front 43

____, or moles per liter (M)

Back 43

Molarity

Front 44

A ___ of an element or compound is equal to its atomic or molecular weight (sum of atomic weights) in grams.

Back 44

Mole

Front 45

(emulsions) - heterogeneous mixtures whose solutes do not settle out.

Back 45

Colloids

Front 46

_____ - heterogeneous mixtures with visible solutes that tend to settle out (Big Pieces)

Back 46

Suspensions

Front 47

No chemical bonding takes place in ____

Back 47

mixtures

Front 48

Most ____ can be separated by chemical means

Back 48

Mixtures

Front 49

____ can be heterogeneous (not uniform) or homogeneous (uniform)

Back 49

Mixtures

Front 50

____ cannot be separated in to their elemental components by physical means (like filtering)

Back 50

Compounds

Front 51

All ____ are homogeneous uniform through out

Back 51

Compounds

Front 52

____ ____, or energy levels, surround the nucleus of an atom

Back 52

Electron shells

Front 53

____ are formed using the electrons in the outermost energy level (valance electrons)

Back 53

Bonds

Front 54

____ ____- outermost energy level containing chemically active electrons

Back 54

Valence shell

Front 55

___ ___, except for the first shell which is full with two electrons, atoms interact in a manner to have eight electrons in their valence shell.

Back 55

Octet rule

Front 56

___ elements have their outermost energy level fully occupied by electrons

Back 56

Inert

Front 57

Chemically inert elements (valence shell ____)

Back 57

Complete

Front 58

_____ elements do not have their outermost energy level fully occupied by electrons

Back 58

Reactive

Front 59

Chemically ____ elements (valence shell incomplete)

Back 59

Active

Front 60

Two or more different kinds of atoms chemically bonded together by electrostatic attraction (a metal and a nonmetal) form crystals.

Back 60

Ionic

Front 61

Two or more different kinds of atoms chemically bonded together by electrostatic attraction (a metal and a nonmetal) form molecules

Back 61

Covalent

Front 62

A ___ bond is a special type of dipole-dipole bond that exists between an electronegative atom and a hydrogen atom bonded to another electronegative atom.

Back 62

Hydrogen

Front 63

IONIC BONDS
have gained one or more electrons negative (ions formed from nonmetals or groups of elements carrying extra electrons) - negative ion, Chloride

Back 63

Anions

Front 64

IONIC BONDS
___ are charged atoms resulting from the gain or loss of electrons.

Back 64

Ions

Front 65

IONIC BONDS
____ have lost one or more electrons (ions formed from metals or groups of atoms imissing one or more electrons) positive ion - Sodium.

Back 65

Cation
(cats are positive)

Front 66

Electrons shared equally between atoms produce ____ molecules

Back 66

nonpolar

Front 67

Unequal sharing of elctrons produces ___ molecules

Back 67

Polar
(polar bears don't share)

Front 68

Atoms with six or seven valence shell electrons are _____

Back 68

Electronegative (nonmetals)

Front 69

Atoms with one or two valence shell electrons are _____

Back 69

Electropositive (metals)

Front 70

____ bonds are too weak to bind atoms together

Back 70

Hydrogen

Front 71

* Common in dipoles such as water
* Responsible for surface tension in water
* Important as intramolecular bonds, giving the molecule a three-dimentional shape very important in protein structure and bond between the strands in DNA

Back 71

Hydrogen Bonds

Front 72

____ reactions occur when chemical bonds are formed, rearranged, or broken.

Back 72

Chemical

Front 73

Written in symbolic form using chemical equations

Back 73

Chemical Reactions

Front 74

____ equations contain:
* Number and type of reacting substances, and products produced
* Relative amounts of reactants and products.

Back 74

Chemical

Front 75

EXAMPLES OF CHEMICAL REACTIONS
H + H =

Back 75

H2

Front 76

EXAMPLES OF CHEMICAL REACTIONS
4H + C =

Back 76

CH4 methane

Front 77

_____ reactions: Synthesis reactions which always involve bond formation
A + B = AB

Back 77

Combination

Front 78

____ reactions: Molecules are broken down into smaller molecules
AB = A + B

Back 78

Decomposition

Front 79

____ reactions: bonds are both made and broken
AB + C = AC + B
(can I dance with your partner)

Back 79

Exchange

Front 80

Reactants losing electrons are electron donors and are ____

Back 80

Oxidized

Front 81

Reactants taking up electrons are electron acceptors and become ____

Back 81

reduced

Front 82

Reactions that release energy

Back 82

Exergonic reactions

Front 83

Reactions whose products contain more potential energy than did its reactants

Back 83

Endergonic

Front 84

All chemical reactions are theoretically ____
A + B = AB
AB = A + B
if neaigher a forward nor reverse reaction is dominant, chemical equilibrium is reached.

Back 84

Reversible

Front 85

Name the factors influencing Rate of Chemical Reactions/

Back 85

* Temperature
* Particle Size
* Concentration
* Catalysts
* Enzymes

Front 86

Chemical reactions proceed quicker at higher ____.

Back 86

Temperature

Front 87

The smaller the ___ ___ the faster the chemical reaction

Back 87

Particle Size

Front 88

Higher reacting particle _____ produce faster reactions

Back 88

Concentration

Front 89

_____ increase the rate of a reaction without being chemically changed.

Back 89

Catalysts

Front 90

_____ Biological Catalysts

Back 90

Enzymes