Chem Phys Exam 2 Flashcards
(141 cards)
1
Q
Molecular interactions often occur in _____________
A
Solutions
2
Q
Solution
A
- Homogenous mixture in which one substance is dispersed in another as individual atoms or molecules
- liquid solution is transparent
3
Q
Clear Solution
A
- When you have a solution and you have a solute it disperses to individual atoms or molecules
- When this happens, molecules are so small they do NOT bend light, so solution is clear
4
Q
Cloudy Liquid
A
- Large particle that refract light
- Particles stick together- make cloudy liquid
- NOT considered a solution
5
Q
Sodium Chloride
A
Ion-Ion interaction
NaCl——> Na+ Cl-
6
Q
NaCl in solution
A
- Ion- diploe interaction
- Separates into anion and water molecules=partial positive
- Proton portion=partial positive charge
7
Q
Acid
A
Compound in which hydrogen ions are associated with an anion
Disassociates in solution:
1. Hydrogen ion (H+)
2. Anion
8
Q
Mixtures that are NOT Solutions
A
- Cloudy liquid (solutions are clear)
- gasoline and water
- oil and vinegar
- Diprivan (propofol)
- Maalox
- NPH insulin (mixture and solution)
9
Q
Gasoline and Water
A
-Most important of polar ends=do NOT mix
-oil is less dense, floats to top and water is on bottom
-Not enough interactions between these two for them to come
Together, react, and stay together
10
Q
Concentrations and Dilutions
A
- Molarity: best way to capture measurement
- Molality
- Normality
- Equivalents
- Osmolarity
11
Q
Concentrated Solution
A
- Color will give you idea about how concentrated a solution is
- Molecules are not bound together, but they are closer to each other
- More chemical reactions occur in concentrated solutions than in dilute solutions
12
Q
Dilute Solution
A
- Less chemical reactions occurring in this solution
- Molecules or atoms are farther apart
13
Q
Mole
A
- Amount of a substance equal to its formula weight in grams
- How we quantify all of the molecules and atoms we cannot see
14
Q
Example of Atomic Weight: 1 Mole of atoms
A
Hydrogen= Atomic weight 1 1gram (1 mole of atoms)
Carbon= Atomic weight 12: 12 grams (1 mole of atoms)
Nitrogen=atomic weight 14 14 grams (1 mole of atoms)
15
Q
Molecular weight of H2 & 1 mole of H2
A
Molecular weight= 2
1 mole of H2= 2 grams
16
Q
Molecular weight of N2 & 1 mole of N2
A
Molecular weight of N2= 28
1 mole of N2= 28 grams
17
Q
Mole
A
Weight in grams of a substance equal to its:
- Formula Weight
- Molecular Weight
- Gram molecular weight
- Atomic Mass Units
18
Q
Avogadro’s Number
A
- Number of atoms (for an element) or molecules (for a compound) in a mole
- 1 mole contains 6.02 X 10^23
- This number does NOT change
19
Q
Molarity
A
Means of expressing the concentration of a certain species in solution in units of moles per liter
20
Q
Molarity- How to calculate 1 Molar Solution
A
- 1 Molar Solution (1 M)
- Weight out solute as precisely as possible (molecular weight in grams)
- Add enough water to make 1 liter as precisely as possible
- want to make 1.000 M solution
21
Q
Molarity example: NaHCO3
A
- Molecular weight: (23+1+12+16x3)
- 84 gram/liter=1 M
- 84 mg/liter= 1mM - 1milimolar (1,000X less)
- Usually talk about milimolar in chemistry
22
Q
Calculations to Know: Molarity
A
Molarity=Moles per liter
23
Q
Calculations to know: Moles
A
Moles= weight/ weight per mole
24
Q
Calculations to know: Weight
A
Weight= moles X weight per mole
25
Calculations to know: Concentration
Concentration=moles/volume
26
Scientific Notation
Useful for expressing numbers that are very large and very small
27
Exponents: 10^0, 10^1, 10^2
```
10^0= 1 (zero zeros)
10^1= 10 (1 zero)
10^2= 100 (2 zeros)
```
28
To determine the exponent
- Count number of zeros after the 1
| - Count number of places decimal point has been displaced from 1
29
Determine 10,000= 10^?
Count number of zeros=4
| 10,000= 10^4
30
Exponents of numbers
-exponents of numbers
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Negative Exponents:
.1
.01
.001
```
.1= 10 ^-1= 1/10
.01= 10^-2= 1/100
.001= 10^-3= 1/1000
```
32
Kilo (k)
Thousand
| 10^3= 1,000
33
Milli (m)
One- thousandth
| 10^-3= 1/1000
34
Mega (M)
Million
| 10^6= 1,000,000
35
Micro
One-millionth
| 10^-6= 1/1,000,000
36
Giga
Billion
| 10^9
37
Tera
10^12
| Trillion
38
Deci
10^-1= 1/10
39
Centi
10^-2= 1/100
40
Nano
10^-9
41
Pico
10^-12
42
Femto
10^-15
43
Atto
10^-18
44
F degree is _________ than C degree
Small
| Difference is factor of 100/180= 5/9
45
32 degree F= ___________ C
0 degree Celsius
46
Conversion from F to C
C= (F-32) X 5/9
47
Conversion from C to F
F= C X 9/5 + 32
48
Conversion from C to Kelvin
K= C + 273
49
0 degree Celsius= _______ K
273. 15 K
50
180 C=__________ K
372.15 K
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Pressure:
1 atm=________ mmHG
1 atm= _______ torr
1 atm= 760 mmHG, 760 torr
52
1 mmHG= _______ torr
1 torr
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760 torr= _______ atm
1 atm
54
1 atm= ________ psi
1 atm= ________ ft water
1 atm= ________ inches Hg
1 atm= ________ kPa
14. 7 PSI
33. 9 ft water
29. 92 inches HG
101. 325 kPa
55
Weight: 1 kg= ____ pounds
2.2 pounds
56
Weight: 1 pound=______ grams
454 grams
57
Volume: 1 liter=_______ ml
1000
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1 ml= ____ cc
1 cc
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1000ml=________ kg
1 kg
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1 liter= ____ quarts
1.06 quarts
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1 quart= ________ ml
946 ml
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20 drops= ________ cc
1 TB= _______ ml
1 ounce= ________ ml
1 cc
15 ml
29.6 ml
63
```
Distance:
1 cm= _____ inches
1 inch= ______ cm
1 kilometer= ______ miles
1 mile= ________ kilometers
```
1 cm= .39 inches
1 inch= 2.54 cm
1 kilometer= .62 miles
1 mile= 1.61 kilometers
64
Don't round off a calculated Quantity When all of the Numbers in your equation are _________________
- Precise
- If you can measure out 2.19 grams with your measuring device then do that
- Know when it's appropriate to be precise (weighing out NaCl) and when it's okay to not be (baking a cake)
65
When solving for Molarity what units should your answer be in?
- Moles/liter= M
| - if asked for a concentrated in mM, then you must convert from M to mM
66
Molality
-Means of expressing the concentration of a certain species in solution in terms of moles per KG of water
-1 Molal solution: weight out MW in grams
-add exactly 1kg (1 Liter) of water.
Total volume will be greater than 1L
67
Normality
-means of expressing the concentration of an acid in terms of hydrogen ion equivalents
68
HCl= _________ normality
1 molar= 1 normality
| Only one Hydrogen ion
69
H3PO4= __________ Normality
1 molar= 3 normality
| 3 Hydrogen ions
70
Equivalents
-Means of expressing the concentration of a species in terms of the number of ions released
71
Equivalents:
100 mM of NaCl:
1 liter= ___________ mEq Cl-
1 liter= 100 mEq of Cl-
| Because there is only one Cl- ion
72
Equivalents:
100 mM of FeCl3
1 liter= _________ mEq of Cl-
1 Liter= 300 mEq of Cl-
| Because there is 3 Cl- ions
73
Osmolarity
-Means of expressing the overall number of particles in solution
Without regard to their identity
-Represents the total concentration of all species
74
Osmolarity Example:
| NaCL: 1 mM= _________ mOsm/liter
1mM= 2 mosm/liter
| Na+ & Cl= 2 separate ions
75
Osmolarity Example:
| 1 mM of MgSO4= ________ mOsm/liter
1 mM of MgSO4= 2 mOsm/liter
| Mg 2+ & SO4-2
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1:1
- Basic unit on which others are based
| - 1 gram/ml
77
1%
1 gram/100 ml (w/v)
| 1 ml/100 ml (v/v)
78
Mg %
- mg/DL
| - mg/100 ml
79
Definition of a Solution
- Homogenous mixture in which one substance is dispersed in another as individual atoms or molecules
- Liquid Solution:
1. Transparent
2. Passes through filter
3. Does not settle upon standing
80
Solvent
-Substance in which a solute dissolve to form a solution
81
Solute
-Substance that dissolves in a solvent to form a solution
82
Saturated Solution
- solution in which solvent is unable to hold any more solute
- solvent may be in equilibrium with an excess of undissolved solute
83
Suspension
- Finely divided solid particles dispersed in a liquid
- Particles will settle upon standing under the influence of gravity
- Must shake or mix before using
- Particle size > 1 um trapped by filter
84
Tyndall Effect
- to distinguish solution from suspension which contains excess undissolved solute
- particles not in solution scatter light
- solvent will not be transparent to beam of light
85
La Chatelier's Principle
-if a system at equilibrium is perturbed, the system moves to counteract the effects of the change
86
Crystalloid
- Soltuion: particles are distributed as individual molecules
- Particles are small enough to diffuse through a semi-permeable membrane
- Particles are not trapped by a filter
87
Examples of Crystalloids
- LR
- NS
- D5W
88
Colloid
- Finely divided particles dispersed in a liquid (or gas)
| - Particles are too small to settle under the influence of gravity
89
Colloid
- Particles are too large to diffuse through semi-permeable membrane
- Particles not trapped by a filter
- Particle size is 2-1,000 nm
90
Examples of colloids
- milk
- dextran
- hespan
- albumin
- fog
- smoke
91
Emulsion
- Particles or globules of one liquid dispersed in another liquid
- Liquids are immiscible
- Layers may separate on standing
- May contain emulsifier to prevent separation
92
Micelle
- Hydrophilic head
- Aqueous solution
- Hydrophobic tail
93
Examples of emulsions:
- Diprivian
- TPN
- Mayonnaise
- Butter
- Detergent on dirty clothes
94
Soap
Ionic end= polar and hydrophilic
Hydro carbon Chain= non polar and hydrophobic
Cleaning action*
95
Examples of suspensions:
- NPH insulin
- Maalox
- Blood
- Oral Antibiotics
96
Density
- mass per volume
| - gram/ml
97
Density of Water
- maximum at 3.98 degree C
- by definition, 1 gram/cc
- 1 gram/ml
- 1 kg/liter
98
Specific Gravity
- Weight of a substance compared to the weight of the same volume of a reference compound
- Reference compound is usually water at its maximum density
- Equivalent to density of substance in gram/ml without units
- Ratio that has no units
99
Ethanol:
Density= 0.789 grams/ml
Spec gravity=_____________?
Spec gravity= .789 (NO UNIT)
100
Accuracy
Does the measurement give you the "right" answer
| Think of darts and Bulls eye
101
Reliability
- Reproductibility
| - extent to which a measurement gives the same answer every time
102
Can a measurement be reliable but not accurate?
Yes
Example: tape measure if it's been stretched
Example: non calibrated thermometer
103
Precision
- Extent to which a measurement can distinguish between 2 closely spaced values
- Directly related to a number of significant digits in a measurement
- Number of significant digits in value should be appropriate for the context: Measurment device, use of measurement
104
Validity
-Extent to which a measurement provides a true indication of the parameter of interest
-A measurement can be accurate, reliable and precise but NOT valid
Example: IQ test as a measure of intelligence
105
Questionable Validity
- blood pH as a measure of acid/base status
- pulse oximetry to monitor organ perfusion
- pupillary size as an indicator of ICP
- arterial line to monitor fluid status
106
Gas
- No definite shape or volume, conforms to container, fills container, flows and is easily compressible
- gases that do NOT react chemically= homogenous mixture
- Molcules high kinetic energy, large distances, do not interact with each other or container
- Ideal gas= no intermolecular forces
107
Liquids
- Definite Volume
- Conforms to shape of container
- Flows, not compressible
- Molecular distance small, medium kinetic energy, inter-molecular forces hold condensed state but allow molecules to slide against each other
108
Solids
- Definite volume, definite shape
| - Molecules are densely packed, minimal kinetic energy, ordered structure
109
Common Gases
- O2
- N2
- CO2
- CO
110
Force
F= pressure/area
111
Volume cylinder
V=area base X height
112
Area of a circle
PiR(2)
113
Volume of a cube
Side(3)
114
Volume of a circle
4/3 Pi r (3)
115
Temperature Conversions:
Boiling H20= F____=C______=K_________
Freezing H20= F______=C______=K________
O degree K=_________C=________F
Boiling H20= 212F= 100C= 373.15K
Freezing H20= 32F=0C-273.15K
O K= -273 C= -524 F
116
1 atm=_____mmHg=_______ PSI=_____ kPa
1 atm= 760 mmHG= 14.7PSI=101 kPa
117
Measuring Pressure
- Atmospheric pressure exists
- Gauge pressure is pressure within vessel (tank) ABOVE atmospheric pressure
- Bourdon spring gauge (Pressure causes coiled copper to straighten) 02 tank gauges
118
Avogadro's Number and Hypothesis
```
#= 6.02 X 10(23) the number of molecules in one mole of a substance
Hypothesis= one mole of gas at standard temperature (O degree C or 273.15K) and pressure (1 atm/1bar or 100 kPa) (STP) occupies a volume of 22.4 liters
-at equal temperature and pressure, equal volumes of gas contain equal numbers of gas particles
```
119
How much volume is occupied by 2 moles of oxygen?
2 moles X 22.4L/mole= 44.8 liters of oxygen
120
How much volume is occupied by a 2 mole of 50:50 mixture of O2/N2O?
2 moles X 22.4L= 44.8 Liters of O2/N2O
121
Charles' Law
-Volume of a gas is proportional to its absolute temperature as long as the pressure and amount of gas are held constant
VI/T1=V2/T2
NOTE: no p in this equation because pressure is constant
Temperature must be in Kelvin
Kelvin= C + 273.15
122
Charles' Law
-If you have a certain molar amount of gas and increase its temperature, the volume of space occupied by that gas will increase and vice versa.
123
Boyles' Law
-Volume of a gas is proportional to its pressure as long as the TEMPERATURE is held constant
P1V1=P2V2
Note: No T because temperature is constant
-decreased volume= increased pressure
-increased volume=decreased pressure
-Units of pressure and volume do not matter as long as they match on both sides
124
Boyles' Law:
| What happens when we contract our diaphragm?
1. Contract our diaphragm, the pressure inside the lungs drops below atmospheric pressure and air flows into our lungs
2. When we release our diaphragm, pressure inside the lungs increase and volume of gas flows out of the lungs
125
Gay-Lussac's Law
-Pressure is proportional to absolute temperature (Kelvin) if volume is constant
-As temperature increases, pressure increases and vice versa
P1/T1=P2/T2
NOTE: no V because volume is constant
126
The "Universal" or "Ideal" Gas Law
PV=nRT
Pressure (atm) X volume (L)= n (number of moles per gas) X R (universal gas constant (8.314 J/mol K)X T (temperature in K)
127
Kinetic Molecular Theory: first 3?
1. Ideal gases consist of a large number of tiny particles
2. Gas particles are in constant, random motion
3. Gas particles are small compared to the distance b/t them
128
Kinetic Molecular Theory: 4-6?
4. Volume of particle sis negligible
5. Gas particles do not react chemically with the other container or each other
6. No forces of attraction or repulsion b/t gas molecules or the container
129
Kinetic Molecular Theory 7-9?
7. Collisions b/t particles and container are perfectly elastic (no energy is lost)
8. Pressure is caused by collisions b/t particles and container walls
9. Average kinetic energy of a collection of gas particles depends on their absolute temperature and NOTHING else
130
At STP (O degree C) and 1 atm (760mmhg) 1 mole of an ideal case will occupy how much space?
1. 22.4 liters of space
| At room temp (68 degree, 1 mole of ideal gas occupies 24L of space)
131
Dalton's Law of Partial Pressures
-The total pressure in a mixture of gases is equal to the sum of the partial pressures of the individual gases in the mixture
P (total)= PO2 + PCO2 + PN2O
The partial pressure of a gas is equal to the (Fi% X atmospheric pressure)
Need to know Fi% of the gas to make this law work
132
What is the partial pressure of O2 in room air?
- RA FiO2 is 21%
- Atmospheric pressure is 760
.21 X 760= 159.6 mmHG
NOTE: pO2 and PCO2 is the partial pressure of Oxygen and CO2 in the blood.
133
Composition of Dry Room Air
Nitrogen: 78%= 593 mmHG
Oxygen: 21%= 159 mmHG
Argon: 1%= 8 mmHG
CO2: .03%= .2 mmHG
134
Anesthetic partial pressures: Iso, Sevo, Des
1. 1% Isoflurance= 1 volume ISO/ 100 volume of carrier gas, Partial Pressure= 240 mmhg
2. 2% Sevoflurance= 2 volumes SEVO/ 100 volume of carrier gas, Partial Pressure= 170 mmhg
3. 6% Des= 6 cc des fluorane/100 cc oxygen/air, 669 mmhg
135
Mole Fraction
- Mole fraction of each component is the number of moles compared to the total number of moles of gas present
- P1+P2= (N1+N2) RT/v
The partial pressure of each gas is directly related to the # of moles of the gas
136
Law of LaPlace-Cylinders
T= P X R (T= wall tension, P= pressure, R= radius of cylinder)
- As cylinder expands, the radius increases. As radius increases, wall tension increases.
- As blood vessel dilates from increased fluid, wall tension in the vessel increases. Greater likelihood of rupture
- Capillaries withstand high pressure better than large vessels especially veins because their radius is smaller and therefore the wall tension is lower
137
Law of LaPlace- Spheres (alveoli)
T=Pr/2, or 2T= Pr, or P=2T/r
Alevoli without surfactant: P= 2T/r
-when R decreases, pressure in the alveoli increases if wall tension is the same
-When pressure increases in small alveoli (small R), P in small alveoli is higher than larger alveoli and air moves from small to large, and small alveoli collapse
-Result= atelectasis & ARDS. Premature infants born without surfactant
138
Law of LaPlace- Spheres- Alveoli with surfactant
P=2T/r
- surfactant allows for the surface tension to increase as radius increases
- maintaining T keeps pressure within the alveoli the same
- when P1=P2, gas does not move from A1 to A2
139
Henry's Law
- amount of gas that dissolves in a liquid is directly proportional to the partial pressure of the gas in the gas phase over/around that liquid.
- Blood is a liquid. O2, Co2, and Anesthetic agents=gas
140
Oxygen Carrying Capacity Equation
CaO2= (1.34 X Hgb X SaO2) + 0.003 (PaO2)
-Answer is in ml/DL?
Note:
PAO2= alveolar oxygen partial pressure= 6X FiO2
PaO2= arterial oxygen partial pressure= 5X FiO2
141
Graham's Law
-Rate of diffusion through an office of a gas is inversely proportional to the square root of the molecular weight
R=1/ (square root of MW)
-Smaller molecules diffuse through membranes faster, larger slower
-Large molecules have higher molecular weight.
-This relates to second gas effect w/ Nitrous Oxide: rapid uptake of smaller molecule leaves higher concentration of large molecules that are left behind).
-this relates to diffusion hypoxia which can occur w/ N2O: reverse of
Second gas effect. Smaller molecules rush out and reduce concentration of the larger molecules.
