Module 2

Front 1

Density

Back 1

mass per unit volume D=M/V
the amount of matter in a particular volume the "compactness"
examples: g/dl, g/cm, mg/L

Front 2

Element

Back 2

building blocks of matter
example: iron, calcium, oxygen

Front 3

atom

Back 3

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

Front 4

Hydrogen

Back 4

H

Front 5

Carbon

Back 5

C

Front 6

Oxygen

Back 6

O

Front 7

Calcium

Back 7

Ca

Front 8

Potassium

Back 8

K

Front 9

sodium

Back 9

Na

Front 10

Nitrogen

Back 10

N

Front 11

Chlorine

Back 11

Cl

Front 12

Flourine

Back 12

F

Front 13

Sulfur

Back 13

S

Front 14

Magnesium

Back 14

Mg

Front 15

Iron

Back 15

Fe

Front 16

Iodine

Back 16

I

Front 17

Lithium

Back 17

Li

Front 18

Silver

Back 18

Ag

Front 19

Phosphorous

Back 19

P

Front 20

Lead

Back 20

Pb

Front 21

Copper

Back 21

Cu

Front 22

Mercury

Back 22

Hg

Front 23

Calcium function in body

Back 23

bone, teeth, muscle contraction

Front 24

Phosphorus function in body

Back 24

ATP,protein, DNA

Front 25

chlorine function in body

Back 25

NaCl(salt), water balance

Front 26

sulfur function in body

Back 26

proteins

Front 27

potassium function in body

Back 27

nerve transmission, muscle contraction

Front 28

sodium function in body

Back 28

NaCl, water balance, nerve transmission

Front 29

magnesium

Back 29

enzymes

Front 30

iodine

Back 30

thyroid function

Front 31

iron function in body

Back 31

blood hemoglobin

Front 32

oxygen function in body

Back 32

part of water

Front 33

carbon function in body

Back 33

structural framework

Front 34

atomic number

Back 34

equal to the number of protons in an atom's nucleus. It is also equal to the number of electrons in an uncharged atom

Front 35

atomic weight

Back 35

the mass of an average atom of an element

Front 36

Mass number

Back 36

number of protons plus number of neutrons, or ,round off the atomic weight

Front 37

Isotopes

Back 37

atoms with the same number of protons, different number of neutrons,different mass number

Front 38

group numbers indicate what

Back 38

how many electrons in the outer shell

Front 39

elements near the left side of the chart tend to _ electrons

Back 39

give away

Front 40

elements near the right of the chart tend to _ electrons

Back 40

take

Front 41

Ion

Back 41

charged atoms, or charged particles, examples K+, Na+, Mg++,

Front 42

cation

Back 42

positively-charged ion

Front 43

anion

Back 43

negatively-charged ion

Front 44

elements that tend to give away electrons, are left with a net _ charge

Back 44

positive

Front 45

elements that tend to take electrons, are left with a net _ charge

Back 45

negative

Front 46

describe ionic

Back 46

an ionic bond occurs between metal and nonmetal. it involves giving away and taking electrons. it results when a cation and an anion attract each other.

Front 47

describe covalent

Back 47

occurs between two non metals
it involves sharing electrons
it results when neutral atoms share electrons

Front 48

describe polar covalent

Back 48

a polar covalent bond exist when the sharing of electrons between two nonmetal atoms is unequal

Front 49

nonpolar covalent

Back 49

a nonpolar covalent bond exists when two nonmetal atoms share electrons equally.

Front 50

describe hydrogen bond

Back 50

usually occurs between a hydrogen atom and oxygen or nitrogen. it involves unequal sharing of electrons, which leaves hydrogen with a partial + charge and the oxygen or nitrogen with a partial - charge

Front 51

dexcribe Compound

Back 51

a substance formed from the chemical combination of 2 or more elements

Front 52

describe molecule

Back 52

smallest piece of any compound or pure substance

Front 53

molecular weight

Back 53

1. mass of molecule
2. round atomic weights of each atom to the nearest whole number.
3. add them together.

Front 54

formula for bicarbonate

Back 54

HCO3

Front 55

formula for carbonate

Back 55

(CO3-)2

Front 56

formula for Phosphate

Back 56

PO4

Front 57

formula for Nitrate

Back 57

NO3

Front 58

Nitrite

Back 58

NO2

Front 59

Sulfate

Back 59

SO4

Front 60

Sulfite

Back 60

SO3

Front 61

formula for Hydroxide

Back 61

OH-

Front 62

formula for Ammonium

Back 62

NH4

Front 63

size of particles in solutions

Back 63

very small(crystalloids)

Front 64

size of particles in colloids

Back 64

medium size (large molecules)

Front 65

size of particles in suspensions

Back 65

large (sand)

Front 66

describe solution

Back 66

a homogeneous(Of uniform structure or composition throughout) mixture of two or more substances

Front 67

describe solute

Back 67

the substance that is put into the liquid technically the substance(s) prestent in a solution in the smaller amount

Front 68

solvent

Back 68

the liquid technically the material present in a solution in the largest amount

Front 69

a solution is said to be a dilute if

Back 69

there is only a small amount of solute per unit volume of solution

Front 70

concentrated solutions have what?

Back 70

much more solute per unit volume of solution

Front 71

a 5% soultion of glucose has how much glucose disolved into how much water to make how much volume

Back 71

5 grams and 100ml (5g/100ml or 5 g/dl)

Front 72

solutions contain very small what? such as ?

Back 72

particles, ions and small molecules

Front 73

particles small enough to form soultions are called what?

Back 73

crystalloids

Front 74

crystalloids do what in solutions?

Back 74

remain evenly dispersed, they do not settle out.

Front 75

what types of filters will crystalloids pass through?

Back 75

very large pores of filter paper and through the smaller pores of a semipermeable membrane

Front 76

semipermeable membrane is used for what

Back 76

dialysis

Front 77

suspensions include what size of particles? such as?

Back 77

large particles such as sand and clay if you let stand particles will settle to the bottom

Front 78

colloid include what? what type of filter will they pass though? what type will they not?

Back 78

larger molecules or groups of molecules such as proteins. the particles don not settle out.they pass through a paper filter but too large to pass through a semipermiable membrane

Front 79

our blood is a suspension of cells and a crystalloid solution, and a colloid why?

Back 79

because it has a suspension of cells, colloid because protiens are dissolved in it, and crystalloid solution because of dissolved salts,etc.

Front 80

describe protoplasm. is it a solution?

Back 80

the living matter in a cell. yes

Front 81

describe cytoplasm.

Back 81

the cellular protoplasm bounded by the cellular and nuclear membrane, is a water solution of colloids and crystalloids. suspended in the solution are the cellular organelles such as mitochondria, lysosomes, and free ribosomes.

Front 82

give 4 properties of a solution.

Back 82

1. clear
2. not filterable
3. do not settle out.
4. small crystolloid solutes.

Front 83

give 4 properties of suspensions.

Back 83

1. translucent or opaque(not clear; not transmitting or reflecting light or radiant energy; "opaque windows of the jail"; "opaque to X-rays")
2. filterable
3. settle out
4. large particles

Front 84

define acid

Back 84

substances that dissociate in water and produce hydrogen ions (H+)

Front 85

define base

Back 85

substances that dissociate in water and produce hydriate ion (OH-)

Front 86

define salts

Back 86

substances that dissociate in water and produce and anion and a cation neither of which is H+ or OH-

Front 87

ph values that differ by 3 units means that they differ by

Back 87

10 to the third

Front 88

distinguish between "neutral" pH and the "average" pH of the blood.

Back 88

average pH is 7.35-7.45
neutral pH is 7.00

Front 89

define strong acid

Back 89

strong acids dissociate COMPLETELY

Front 90

define weak acid

Back 90

weak acids DO NOT dissociate completely.

Front 91

which acid has a more disruptive effect on physiology

Back 91

strong acids

Front 92

which acids are buffers?

Back 92

weak acids

Front 93

define buffers

Back 93

chemical compounds that can convert strong acids or bases into weak ones

Front 94

give an example of buffers

Back 94

HCO3(weak base) and H2CO3(weak acid)

Front 95

define physical processes

Back 95

usually change the physical appearance of the substance.

Front 96

define chemical processes

Back 96

these are processes that form new substances, as in burning wood and rust formation. major bonds are changed.

Front 97

describe oxidation

Back 97

removal of an electron during chemical reaction.
loses electron, energy, and H+

Front 98

describe reduction

Back 98

gain of an electron during a chemical reaction.
gains electron, energy, and H+

Front 99

describe decompostion

Back 99

catabolism, exergenic (energy out) 2 H20 -> 2 H2 + O2

Front 100

describe synthesis

Back 100

anabolism, endergonic (energy in) 2 H2 + 02 -> 2 H20

Front 101

describe exchange (replacement)

Back 101

HCL(acid) + NaOH(base) -> H20(water) + NaCl(salt)

Front 102

describe reversible

Back 102

NaCl <--> Na+ + Cl-

Front 103

name the four most abundant elements in living systems

Back 103

1. carbon
2. hydrogen
3. oxygen
4. nitrogen

Front 104

by number of atoms and by mass C

Back 104

9.5 number 18 mass percent

Front 105

by number of atoms and by mass H

Back 105

63 number 10 mass percent

Front 106

by number of atoms and by mass O

Back 106

25.5 number 65 mass percent

Front 107

by number of atoms and by mass N

Back 107

1.4 number 3 mass percent

Front 108

describe 5 properties of inorganic compounds

Back 108

1. do not(usually) contain carbon
2. are small
3.include mainly ionic bonds
4. are not very flammable
5. are usually water soluble(hydrophilic)

Front 109

dexcribe 5 properties of organic compounds

Back 109

1. contain carbon
2. are frequently large
3. include mainly covalent bonds
4. usually flammable
5. may not be water soluble (hydrophobic)

Front 110

describe 5 properties of water and provide example of how property is utilized in the human body.

Back 110

1. solvent/suspending medium
2. participates in chemical reactions
3. heat buffer
4. evaporative cooling
5. lubricant

Front 111

water is composed of what type of bonds

Back 111

polar covalent bonds which makes it a versatile solvent

Front 112

water participates in _ reactions

Back 112

chemical

Front 113

in _ _ reactions adding water breaks or "lysis" bonds

Back 113

hydrolysis chemical

Front 114

in _ _ reactions water is removed

Back 114

dehydration synthesis reactions

Front 115

water has a very _ surface tension and is a great _

Back 115

high, lubricant