Chapter 15, Part 1- Review Exam #2

Front 1

What does an ampere measure?

Back 1

Electric current

Front 2

What does a candela measure?

Back 2

Luminous intensity

Front 3

Standard temp & pressure =

Back 3

100.00 kilopascals at 273 kelvin

Front 4

What resists changes in shape & volume?

Back 4

solid

Front 5

What are fluids that exhibit minimal to no compressibility & may change V with changes in P & T?

Back 5

liquid

Front 6

What are fluids that are compressible & easily change V with changes in P & T?

Back 6

gases

Front 7

What is plasma?

Back 7

mixture of ionized gas & free-floating electrons

Front 8

Elements are matter that possess?

Back 8

similar atoms containing same protons

Front 9

In a periodic chart, the vertical columns are called what? The horizontal columns are called what?

Back 9

groups, periods

Front 10

T or F. Atomic size increases from L to R?

Back 10

T

Front 11

These are much smaller than protons and neutrons?

Back 11

electrons, (-) charge outside

Front 12

# of protons =?

Back 12

atomic #

Front 13

What does the mass number or atomic mass equal?

Back 13

# protons + neutrons in atom

Front 14

Anions

Back 14

atom that gained an electron, (-) charged

Front 15

Cations

Back 15

atom that lost an electron, (+) charged

Front 16

Isotopes of same element have same # of and different #of?

Back 16

protons, but different # of neutrons

Front 17

Electron Configuration

Back 17

• K, L, M,N, O, P, Q
• 2, 8, 18,32,32,18,8

Front 18

Subshells, how many electrons in each?

Back 18

s(2), p(6), d(10), f(14), g(18)

Front 19

Subshells are divided into?

Back 19

orbitals

Front 20

Covalent bond

Back 20

physical sharing of electrons between atoms; stronger than electrostatic bonds
o Single- sharing of one pair of electrons
o Double- sharing of 2 pairs of electrons

Front 21

Electrostatic bond

Back 21

attraction of electrons between atoms; opposite attract, (+) to (-)

Front 22

Electrostatic bonds include? 3

Back 22

1. ion-ion: strongest electrostatic bond, high melting and boiling points (ex. NaCl)
2. ion-dipole: partial charges involved (ex. H20)
3. dipole-dipole (water surface tension): ex. H20

Front 23

Valence Electrons are?

Back 23

Electrons in the outermost shell

Front 24

London dispersion forces are?

Back 24

induced dipole bonding (oils), @ very low temps allow O2 and N2 to become liquids

Front 25

Isomers

Back 25

Same chemical formula but different structural formulas (# of atoms the same but arrangement is different)

Front 26

Steroisomers have?

Back 26

similar geometric arrangement but differ in their spatial position

Front 27

Enantiomers are ?

Back 27

mirror images of each other but can’t be superimposed, possess similar properties

Front 28

Diastereomers are?

Back 28

not mirror images and may have differing physical and chemical properties

Front 29

Racemic enantiomers are?

Back 29

50% levo & 50% dextro

Front 30

Structural isomers

Back 30

same molecular formula, atoms are located in different places

Front 31

Bond energy is the

Back 31

amount of energy needed to make or break a bond

Front 32

T or F. Short bonds, such as covalent bonds, tend to possess greater bond energies than longer, electrostatic bonds.

Back 32

True

Front 33

Bond energies are measured as an ________ change

Back 33

enthalpy

Front 34

Enthalpy

Back 34

is the total amount of energy possessed by a system

Front 35

Carbon has how many valence electrons available for bonding?

Back 35

4

Front 36

Hydrocarbons are molecules composed entirely of?

Back 36

carbon atoms with hydrogen atoms attached

Front 37

Saturated hydrocarbons

Back 37

are single-bonded carbon chains with all available carbon atoms attached to hydrogen

Front 38

Alkanes

Back 38

hydrocarbons containing only single-bonded carbon atoms

Front 39

Unsaturated hydrocarbons

Back 39

one or more double or triple bonds between carbon atoms

Front 40

Alkenes

Back 40

hydrocarbons containing double-bonded carbons

Front 41

Alkynes

Back 41

triple-bonded carbons

Front 42

Alkyls

Back 42

saturated and unsaturated hydrocarbons that have hydrogens omitted, are very reactive , and bond to functional groups

Front 43

Aryls

Back 43

cyclic hydrocarbons omitting a hydrogen on any carbon atom, are reactive, and also bind with functional groups

Front 44

Amines

Back 44

derivatives of ammonia; NR3; only 1 or 2 of R groups can be H; all have lone electron pair on N

Front 45

Alcohols

Back 45

ROH, where R is any alkyl (contains C & H) group; OH (hydroxyl group) very polar

Front 46

Phenols

Back 46

similar to alcohols with ROH general formula but R is aryl group (benzene); propofol is a pheno

Front 47

Ethers

Back 47

ROR’ where R & R’ are alkyl groups attached by O; inert but highly flammable;

Front 48

Aldehydes

Back 48

RCHO

Front 49

Ketones

Back 49

RCOR’

Front 50

Carboxylic acid

Back 50

RCOOH

Front 51

Esters

Back 51

RCOOR

Front 52

Amides

Back 52

RCONH2; RCONHR; RCONR2

Front 53

Solubility is defined as?

Back 53

max amt of 1 substance (solute) that can dissolve into another (solvent)

Front 54

Solubility is enhanced by?

Back 54

intermolecular interactions between substances with similar electron configurations (“like dissolves like”)

Front 55

endothermic rx

Back 55

rx requires more energy than it produces (consumes heat)

Front 56

In a endothermic rx, increased temp = ________solubility.

Back 56

increased

Front 57

Exothermic rx

Back 57

produces more energy than required to break bonds

Front 58

In a exothermic rx, increased temp=_______ solubility.

Back 58

decreased

Front 59

What has little influence on solubility of solids & liquids?

Back 59

pressure

Front 60

Gas solubility in liquids is ________ related to temp

Back 60

inversely

Front 61

Henry’s Law

Back 61

constant temp, amt of gas dissolved in liquid is directly proportional to the partial P of that gas at equilibrium above the gas-liquid interface

Front 62

Henry's law equation

Back 62

p = kc
p = partial P of solute above soln; k = Henry’s constant; c = concentration of solute in soln

Front 63

Increasing gas partial P above liquid will?

Back 63

increase gas amt dissolved in liquid

Front 64

Diffusion

Back 64

process of net movement of 1 type of molecule thru space as a result of random motion intended to minimize a concentration gradient

Front 65

The process of diffusion by?

Back 65

Brownian motion, which is driven by inherent kinetic E of molecules

Front 66

Temp directly proportional to?

Back 66

Kinetic E

Front 67

The velocity at which a molecule may distribute is determined by its?

Back 67

MW

Front 68

Molecules with smaller mass will diffuse?

Back 68

fASTER

Front 69

Graham’s Law

Back 69

rate of effusion (gas diffusion thru an orifice) of a gas is inversely proportional to square root of molecular wt (describes faster diffusion of smaller molecules compared to larger)

Front 70

Fluids (gas or liquid) diffusion thru membrane is dependent on? 5

Back 70

concentration gradient, tissue area, fluid tissue solubility, membrane thickness & mw

Front 71

Diffusion directly proportional to?

Back 71

conc gradient, tissue area & fluid tissue solubility

Front 72

Diffusion inversely proportional to?

Back 72

membrane thickness & mw

Front 73

Osmosis

Back 73

water movement across semipermeable membrane to equilibrate conc gradient

Front 74

Semipermeable membranes are permeable to?

Back 74

water only and not to solute

Front 75

Osmotic pressure

Back 75

force needed to stop osmosis from occurring

Front 76

Oncotic pressure

Back 76

osmotic P caused by plasma proteins & electrolytes in capillaries, balances the hydrostatic pressure tendency to push water out of capillaries

Front 77

Normal oncotic P =

Back 77

28 mm Hg

Front 78

Our vascular system is a?

Back 78

semipermeable membrane that responds to IV delivery of colloids by sequestering fluids

Front 79

Fick’s Law

Back 79

diffusion of gases across biological tissues

Front 80

Ficks law accounts for? 4

Back 80

mw, concentration gradient, solubility & membrane interactions

Front 81

Fick’s Law allows for determination of?

Back 81

pulmonary gas exchange

Front 82

In ficks law diffusion across a semipermeable membrane is directly related to? and indirectly related to?

Back 82

o Directly proportional to partial pressure gradient, membrane solubility of gas & membrane area
o Inversely proportional to membrane thickness & mw

Front 83

The equation for Fick's law is?

Back 83

J = (alpha)D/x(PaO2 – PcapO2)

J = diffusion flux;  solubility constant for O; D = diffusivity;
x = membrane thickness;
(PaO2 – PcapO2) = alveolar-cap O2 partial P difference

Front 84

Gravity

Back 84

9.81m/sec/sec (32ft/sec/sec) per Sir Isaac Newton “each particle of matter attracts every other particle with a force which is directly proportional to the product of their masses and inversely proportional to the square of the distance between them”

Front 85

Gravitational force =

Back 85

(G x m1 x m2)/(d2)
G = grav constant; m1 & m2 = masses of objects; d = distance

Front 86

Weight =

Back 86

mass x force of gravity

Front 87

Newton’s 1st Law of Motion

Back 87

(law of inertia)—a body in motion tends to stay in motion unless acted upon by another force

Front 88

Newton’s 2nds Law of Motion

Back 88

(law of acceleration)—acceleration of a body is in the direction of and proportional to the force (F), and that acceleration (a) is inverse to the mass (m) of the body.
F = ma.
If multiple forces exist, the direction & acceleration are proportional to the sum of all forces. These are called vectors.

Front 89

Newton’s 3rd Law of Motion

Back 89

(law of reciprocal action)—for every action there is an equal and opposite reaction. It states that objects exert equal but opposite forces on one another.

Front 90

Force is the amount of?

Back 90

E required to move objects

Front 91

Newton

Back 91

force required to accelerate 1 kg weight 1 meter per second (std measure of force derived from force of gravity)
o Newton = 1 meter/sec/sec
o 1 newton equivalent to 1/9.81 kg weight or 102 g weight

Front 92

Force = ____ x ____?

Back 92

mass multiplied by acceleration
F = ma
m = mass; a = acceleration

Front 93

Dyne=

Back 93

1/1000th of Newton; force required to move 1 g weight 1 cm per sec

Front 94

Pulmonary vascular resistance is measure of?

Back 94

pulm vascular system’s resistance to flow from RV

Front 95

Normal PVR

Back 95

100-200 dyne sec/cm5

Front 96

Formula for calc SVR

Back 96

= 80 x (MAP-CVP)/CO; normal values 900-1200 dyne sec/cm5

Front 97

What 2 types of values describe physical world?

Back 97

Scalar values and vectors

Front 98

Scalar values described by?

Back 98

magnitude alone; possess no motion & include mass, energy & work

Front 99

Vector described by?

Back 99

magnitude & direction; express motion & described by force, speed, velocity, acceleration, distance & displacement

Front 100

Normal axis of electrical flow is between?

Back 100

-30 & +90 degrees

Front 101

Positive deflection in leads I & II is?

Back 101

normal

Front 102

Negative deflection in leads I & II is?

Back 102

deviation

Front 103

Pressure is defined as

Back 103

force over area
P = f/a

Front 104

Increasing area in which given force is applied will result in?

Back 104

lower pressure

Front 105

Std unit of P measurement is?

Back 105

Pascal

Front 106

pascal is?

Back 106

force of 1 newton (N) over 1 square meter
Pa = 1 N/1 m2
Pa = 102 g/m2

Front 107

kPa =

Back 107

102 kg/m2

Front 108

Will a TB syringe or a 10 mL syringe generate more pressure when 20N of force is applied?

Back 108

TB syringe

Front 109

Atmopheric P

Back 109

cumulative effect of gravity on atmospheric gases gives rise to atmospheric P

Front 110

Atmospheric gases are less concentrated @ ?

Back 110

altitude and more concentrated at sea level

Front 111

1 kPa = ____ cm = ____ mm Hg

Back 111

10.2, 7.5

Front 112

1 atm = ____ mm Hg = ____ torr = ___ bar = ____ kPa = ____ cm H2O = _____ lb/inch2

Back 112

760, 760, 1, 100, 1020, 14.7

Front 113

manometer is?

Back 113

simplest measuring device, open to atmospheric pressure on one end and exposed to a pressure for measurement on the other end

Front 114

Invasive BP monitors use a?

Back 114

piezoelectric transducer that converts pressure waves into electrical signals

Front 115

absolute P= ______ pressure + _____ pressure

Back 115

atmospheric, gauge

Front 116

gauge P = _______ P - ________ P

Back 116

absolute, atmospheric

Front 117

gauge P reads zero at?

Back 117

760 mm Hg at sea level

Front 118

The ASTMI mandates that the zero reading of Bourdon gauges lie between the?

Back 118

6 o’clock and 9 o’clock positions