Chem & Phys CH 1,2&3 Flashcards
1
Q
What is the symbol and value for the following:
1) Tera
2) Giga
3) Mega
4) Kilo
5) Hecto
6) Deca
7) deci
8) centi
9) milli
10) Micro
11) Nano
A
1) Tera - T; 10^12
2) Giga - G; 10 ^9
3) Mega - M; 10^6
4) Kilo - K; 10^3
5) Hecto - H; 10^2
6) Deca - D; 10^1
7) deci - d; 10^-1
8) centi - c; 10^-2
9) milli - m; 10^-3
10) Micro - μ; 10^-6
11) Nano - n; 10^-9
2
Q
What are the 4 exponent rules?
A
1 When exponents are multiplied, you add them.
2) When exponents are divided, you subtract them
3) When parentheses are involved, you multiply
4) When adding or subtracting, convert exponent to the lowest common factor
3
Q
(2.68 x 10^-5) x (4.4 x 10^-8) = ?
A
11.8 x 10^-13 or 1.18 x 10^-12
4
Q
(1 x 10^3) + (1 x 10^2) = ?
A
(1 x 10^3) + (0.1 x 10^3) = 1.1 x 10^3
5
Q
Log (a x b) = ?
A
Log (a) + Log (b)
6
Q
Log (a/b) = ?
A
Log (a) - Log (b)
7
Q
Log (a^b)
A
b x log (a)
8
Q
Celcius to Farenheit
A
F = C x 1.8 + 32
9
Q
Farenheit to Celcius
A
C = (F-32) / 1.8
10
Q
Celcius to Kelvins
A
K = C + 273
11
Q
4 Rules or Significant Figures
A
1) Non-zero digits are always significant
2) Captive Zeros (zeros between non-zero digits) are always significant
3) Leading Zeros (zeros at the beginning of a number and located to the left of non-zero digits) are never significant
4) Trailing Zeros (Zeros at the end of a number and located to the right of non-zero digits) are only significant when the number contains a decimal point.
12
Q
How many significant digits in 2.30 x 10^3?
A
3
13
Q
Protons and neutrons have an atomic mass of 1 amu. How many kg in 1 amu?
A
1 amu = 1.66 x 10 ^-27kg
14
Q
Molecular vs. Ionic Compounds
A
1) Molecular compounds are composed of non-metals
2) Ionic Compounds are composed of a metal and a non-metal.
15
Q
How do you calculate atomic mass number?
A
of protons + # of neutrons
16
Q
How do you calculate Average Atomic Mass if Br-79 and Br-81 are the only naturally occurring isotopes that occur in equal amounts (50%)?
A
ATM is the weighted averages of the atomic masses of the isotopes of that element that occur naturally. (79 X .5) + (81 X .5) = 80
17
Q
How is the periodic table organized?
A
1) Groups - horizontal rows
2) Group Numbers - Columns
3) Groups - Metals, non-metals, and transitional metals.
18
Q
Is there a trend in the periodic table about what kind of ion an element is likely to form?
A
Metals (left side of the table) tend to form cations; non-metals (right side of the table) tend to form anions.
19
Q
How can you predict the charge of the ions derived from the representative elements?
A
For the Representative Metals, the cationic charge equals the group #; For representative non-metals, the anionic charge equals the group # - 8. Transition metals frequently for more than one cation.
20
Q
Define Hydrates? How are they used in anesthesia?
A
Hydrates are anhydrous ionic compounds that absorb water into their crystalline structure. Formation of a hydrate is generally reversible.
Used as desiccants in anesthesia.
21
Q
What charge are the following cations and anions likely to form:
1) Na
2) Phosphide
3) Barium
A
1) Na 1+
2) Phosphide 3-
3) Barium 2+
22
Q
Representative vs. Transition elements
A
1) Representative elements are those elements within the first two families (group 1 & 2 on the far left) and the sic families or groups (on the right) of the periodic table.
2) Transition metals are the elements in those groups in the middle of the table.
23
Q
is glucose (C6H12O6) an ionic or molecular compound?
A
Molecular because it contains no metals.
24
Q
What is the molar mass of nitrous oxide (N2O)?
A
(2 x 14) + 16 = 44g/mol
25
If a PT is given 20g of nitrous oxide, how many molecules of N2O have been given?
1mol/44g = xmols/20g --> x= .45mols --> .45 x (6.02 x 10^23) = 2.7 x 10^-23
26
Which of the following in an UNLIKELY compound:
1) Al3O2
2) BeO
3) NaF
4) FeS
Al3O2 - because of valence electrons. Al = +3 and O =-2
27
What cation are the following metals likely to form:
1) Al
2) Rb
3) Mg
4) Li
5) Ga
1) Al 3+
2) Rb +
3) Mg 2+
4) Li +
5) Ga 3+
28
What anion are the following non-metals likely to form:
1) S
2) I
3) N
4) P
5) Se
1) S 2-
2) I -
3) N -3
4) P -3
5) Se -2
29
Name the following compounds:
1) MgN
2) AlS
3) LiI
4) KO
5) CaC
1) MgN - Magnesium nitride
2) AlS - Aluminum sulfide
3) LiI - Litium iodide
4) KO - Potassium oxide
5) CaC - Calcium carbide
30
Define and Electrolyte? How are strong electrolyte mixtures mad compared to non-electrolyte mixtures?
Electrolytes are compounds that dissolve in water to give a solution that conducts electricity.
Ionic compounds that dissolve in water are strong electrolytes. Molecular compounds that dissolve in water are normal non-electrolytes. c
31
Which of the following aqueous solutions of the substances below, do you expect to be a strong electrolyte:
1) NacL
2) Ethanol (C2H6O)
3) Glycerin (C3H8O3)
4) Lithium Pyruvate (LiC3H3O3)
5) Ammonium Carbonate ((NH4)2CO3)
1) NacL -Yes
2) Ethanol (C2H6O) - No
3) Glycerin (C3H8O3) - No
4) Lithium Pyruvate (LiC3H3O3) - Yes
5) Ammonium Carbonate ((NH4)2CO3) - Yes
32
What is an Isoptope?
Elements with the same amount of protons but a different number of neutrons, which changes the atomic mass. This can make them unstable and reactive.
33
Example of nuclear isotope and its purpose?
Iodine-123: scan used to evaluate for thyroid cancer
34
What is an ion?
When an atom or molecule gains or loses an electron, giving it a net positive or negative charge.
35
How are the following elements commonly used in the body:
1) Ca
2) Cl
3) Cu
4) H
5) I
6) Fe2+
7) Mg
1) Ca - bones/teeth, muscle contractions, nerve impulses and blood clotting.
2) Cl - HCl stomach, Nacl in ECF, KCl in ICF, helps balance fluids and pH.
3) Cu - Erythrocyte production, absorption of Fe++, helps form collagen, act as antioxidant.
4) H - acid base balance, stomach HCl
5) I - Thyroid hormones T3 & T4
6) Fe2+ - HgB (280 million molecules HgB per RBC)
7) Mg - Co-factor for 300+ enzymes, helps regulate metabolic functions. Can be used to slow uterine contractions.
36
How are the following elements commonly used in the body:
1) N
2) O2
3) P
4) K
5) Na
6) S
1) N - N20 is an important anesthetic gas
2) O2 - ATP production in cellular respiration
3) P - DNA, RNA, ATP
4) K - Muscle contration
5) Na - Fluid Balance
6) S - Component of vital amino acids for protein synthesis
37
What are Polyatomic Ions?
Ionic compounds formed from two or more non-metals bonded in a way that results in a net electrical charge.
i.e. SO3^2- & HCO3-
38
(T/F?) The net charge on an Ionic compound must be zero?
True
39
What happens if the the ionic charges in an ionic compound aren't equal?
Seek the least common multiple between the absolute values of the charges: use the criss-cross method.
i.e. Al3+ & O2- --> Al2O3
40
Complete the following reactions:
1) Na+ and CO3^2- -->
2) Mg2+ and PO4^3- -->
3) NH4+ and SO4^2- -->
1) Na+ and CO3^2- --> Na2CO3
2) Mg2+ and PO4^3- -->Mg3(PO4)2
3) NH4+ and SO4^2- --> (NH4)2SO4
41
How are Hydrates written?
Written as: ionic compound * # of water molecules
i.e. CuSO4 * 5 H2O (Copper Sulfate Pentahydrate)
MgSO4 * 7 H2O (Magnesium Sulfate Heptahydrate)
42
Define Avogadro's Number?
6.02 x 10^23 and represents one mole of anything.
43
How do you calculate pH when given the hydrogen concentration?
pH = -log [H+]
44
How many pounds in a kilogram?
2.2lbs = 1kg
45
How can you determine the mg/mL in a % solution?
1) 1% solution = ?mg/mL
2) 2% solution = ?mg/mL
3) 10% solution = ?mg/mL
Move the decimal place one to the right. i.e.
1) 1% solution = 10mg/mL
2) 2% solution = 20mg/mL
3) 10% solution = 100mg/mL
46
What is the percentage in grams/100mL of 1% lidocaine? In other words, how many grams of lidocaine in 100mL of a 1% solution?
Since 1% lidocaine = 10mg/mL, then
| 1000mg/100mL or 1g/100mL
47
What is the max dose you can give of lidocaine with epi and lidocaine without epi?
1) Lidocaine with epi max dose = 7mg/kg
| 2) Lidocaine without epi max dose = 4.5mg/kg
48
Calculate the max dose of 1% lidocaine with epi that can be given to a patient that weighs 100kg?
7mg/1kg = Xmg/100kg --> x=700mg;
since 1% lido = 10mg/1mL
10mg/1mL = 700mg/xmL --> x = 70mLs max dose
49
What are the concentrations in mcg/mL of the following drug ratios:
a) 1:200,000
b) 1:100,000
c) 1: 10,000
Just divide 1 million by the second number -->
a) 1:200,000 = 5mcg/mL (1,000,000/200,000 = 5)
b) 1:100,000 = 10mcg/mL (1,000,000/100,000 = 10)
c) 1: 10,000 = 100mcg/mL (1,000,000/10,000 = 100)
50
What is the final concentration in mcg/mL when 4mg is placed in 250mL?
Since you have 4mg/250mL, this is the same as 4000mcg/250mL. When simplified = 16mcg/mL
51
What is the percent O2 being administered when 2L/min of O2 and 2L/min of Air are flowing?
*Remember that air has 21% breathable oxygen
2,000mL O2 + (.21 x 2000mL Air) = 2420mL O2
2420/4000 (total flow) = .605 or 60.5%
52
What is the percent O2 being administered when 1L/min of O2 and 2L/min of N20 are flowing?
*Remember there's no breathable oxygen in N2O; Therefore,
1,000mL O2 + 0 = 1000mL O2
1000/3000 (total flow) = .33 0r 33%
53
What is the percent O2 being administered when 2L/min of O2 and 2L/min of N20 are flowing?
*Remember there's no breathable oxygen in N2O; Therefore,
2,000mL O2 + 0 = 2000mL O2
2000/4000 (total flow) = .5 0r 50%
54
Given that a full E-cylinder contains 660L O2 @ 2000 psi, how long can O2 flow @ 2L/min if the gauge reads 1000psi?
Duration of flow = O2 tank conversion factor (.28) x remaining tank pressure (psi) / Continuous flow rate
i.e. 330L O2 / 2Lper min = 165 mins
55
How is Estimated Blood Volume (EBV) calculated?
EBV = Body Weight (kg) x ABV (mL/kg)
56
What are the Average Blood Volumes for the following populations:
1) Premature Neonates
2) Neonates
3) Infants
4) Men
5) Women
1) Premature Neonates - 96
2) Neonates - 85
3) Infants - 80
4) Men - 75
5) Women - 65
57
How is Allowable Blood Loss (ABL) calculated?
ABL = ((Original Hct -Final Hct) / Original Hct) x EBV
58
Given: initial HgB = 14; Male blood volume 75mL/kg; weight 70kg; minimum HgB = 8; determine EBV and ABL
1) EBV = 70kg x 75 = 5250mL
| 2) ABL = ((14-8)/14) x 5250 = 2250mL
59
If you have Neosynephrine 10mg/mL and you mix it with 249 mL of 0.9% normal saline, what is the final concentration in mcg/mL?
Since 10mg/1mL = 1000mcg/1mL, after adding 0.9% NaCl, we have 1000mcg/250ml, which when simplified = 40mcg/ml
60
You have Dopamine 200mg/250mL and a 100kg patient. If given an order to start Dopamine 3mcg/kg/min, how many mL/min should be infused?
You have 200mg/250mL or 200,000mcg/250mL or 800mcg/1mL of Dopamine.
Your rate is 3mcg/kg/min and your PT is 100kg which = 300mcg/min.
Since 800mcg/1mL = 300mcg/XmL --> x = 0.375mL/min
61
If you have an epinephrine solution of 1:20,000 and need to make a mixture of 1:100,000, using saline as a dilutant, how many ml's of 1:20,000 are required to make a dilution factor of 10mcg/ml and how many mL of Nacl will you use?
Since 1:20,000 = 50mcg/ml and 1:100,000 = 10mcg/ml
50mcg/Xml = 10mcg/1mL --> X = 5mL of solution
Since solution = 5mL and epi is 1mL, then there is 4mL Nacl in solution.
62
What is the 4/2/1 Rule?
Per hour, give:
1) 4ml.kg for the first 10 kg of PT's weight
2) 2ml/kg for the next 10 kg of PT's weight
3) 1ml/kg for the rest of the PT's weight
63
Apply the 4/2/1 rule to a 70kg man?
(4 x 10) + (2 x 10) + (1 x 50) = 110ml/hr
64
Numerical value of pi?
3.1415297
65
Speed of Light?
6.626 x 10^-34J/sec
66
Acceleration due to gravity?
2.998 x 108m/sec
67
Charge on an electron?
1.602 x 10^-19 Coulombs
68
Universal Gas Constant?
8.314 J/mol-K
69
What is Newton's First law?
An object at rest or moving at constant speed in a straight line will continue in that state until a net external force acts upon it.
70
What is Newton's Second Law?
Force is equal to mass times acceleration (F = M x A)
71
What is Newton's Third Law?
For every action, there is an equal and opposite reaction.
72
Define Force?
Force is the weight of an object
73
What is the acceleration gravity?
The force of gravity accelerates all objects on earth to 9.81 m/sec^2
74
Scalar vs.Vector
Scalar values have magnitude only (i.e. distance, height, mass, age, etc.)
Vector quantities have magnitude and direction (velocity, force, torque, etc).
75
How many newtons in 1 kg?
1 kg = 9.81 N
76
How many newtons in 1 lb?
1 lb = 4.45 N
77
Define Mass?
Mass is defined as the amount of matter in an object (in physics, it's the resistance of an object to acceleration).
78
What is the unit of measurement for acceleration?
m/s^2 = meters per seconds squared
79
Mass vs. Weight
Mass is the amount of matter in an object while weight is the gravitational force exerted on an object by earth. (i.e. our weight is different on earth than it is on the moon).
80
Define Velocity? What is the formula?
Velocity is displacement divided by time. V = Δr/Δt. where r is displacement and t is time.
81
How is Speed calculated?
Speed (s) = d/t
82
Difference between distance and displacement?
Distance is linear (a scalar measurement) and displacement is directional and can be positive, negative or zero.
83
Define Resultant?
When two or more vectors are added, the sum is called a resultant.
84
You are walking 5 mph east on a train going 30 mph east. What is your resultant velocity?
35 mph east
85
You are walking 5 mph west on a train that is going 30 mph east. What is your resultant vector?
25 mph east
86
You are in a boat traveling east at 3.0 m/s and the current is going north at 1.0 m/s. What is your resultant velocity?
For vectors with different directionality, draw a third arrow to connect heads and tails. The vectors draw a right triangle, so the resultant can be calculated using the pythagorean theorem: c^2 = a^2 + b^2
3^2 + 1^2 = 3.16
87
What is acceleration? how is it calculated?
Acceleration is a vector that describes how velocity changes with time. A = Δv/Δt.
88
What is pressure? What is the unit of measurement for pressure? How is it calculated?
Pressure is defined as force per unit area. The SI unit of measurement for pressure = Pascal. P = force/area
89
What are the five different units of measurements for pressure?
1) Atmosphere (atm)
2) mmHg
3) kPa
4) Psi
5) cmH20
90
What is the value of 1 atm in mmHg? kPa? psi? cmH20? and torr?
1 atm = 760mmHg = 101.325 kPa = 14.7 psi = 1033.23 cmH20 = 760 torr
91
What is hydrostatic pressure?
The pressure exerted as a result of a liquid's weight.
92
Describe the law of Laplace?
In spheres and cylinders, the law of Laplace illustrates the relationship between wall tension, internal pressure and radius.
93
In which biological structures is the Law of Laplace perfectly demonstrated?
1) Alveoli
2) Cardiac Ventricle
3) Saccular Aneurysm
94
Pressure vs. Tension as it applies to the Law of Laplace?
Pressure is the pushing force. It pushes the walls of the object apart.
Tension is the pulling force. It holds the walls of the object together.
95
How is wall stress (sigma/σ) calculated?
σ = (P*r)/2h
96
In the heart, what contributes to σ or wall stress? What happens as a result of an increase in wall stress?
In the heart, increases in σ increase oxygen consumption as each myocyte uses more energy when developing greater tension. Hypertrophy is the compensatory response to elevated wall stress.
97
How much pressure is created when you apply 5.00 N of force on a syringe plunger that has a diameter of 1.00 cm?
Since P = F/A;
Area of a circle = πr^2 or 3.14(0.5cm)^2
convert cm to m and you get 3.14(.005)^2 = 7.854 x 10^-5
divide force by area: 5N/7.854 x 10^-5 = 63.66kPa
98
How much pressure is created when you apply a 5.00 N force on a syringe plunger that has a diameter of 2.00cm?
3.134(.01m)^2 = .000314
| 5 / .000314 = 15.9 kPa
99
(T/F?) Smaller syringes have the capacity to develop very high pressures? Doubling the diameter of the syringe decreases the pressure by a factor of 4?
True - this is why it is easier to unclog a clogged picc line with the smaller syringes
100
What is the area of a 3mL and a 20mL syringe?
3mL syringe area = 5.89 x 10 ^ -5
| 20mL syringe area = 28.7 x 10 ^ -5
101
How much pressure is created from a 3mL and 20ml syringe when you apply 25 N of force?
1) 3mL syringe: P = 25 / 5.89 x 10^-5 = 424 kPa
2) 20mL syringe: P = 25 / 28.7 x 10^-5 = 87.1 kPa
* 3mL syringe generates 4.9X higher pressure than a 20mL syringe.
102
How do you calculate Absolute Pressure and Bourdon Pressure?
1) Absolute Pressure = Atmospheric pressure + gauge pressure
| 2) Bourdon Pressure = Gauge pressure - atmospheric pressure
103
What is the total absolute pressure in a tank of 02 that reads 45 psi?
59 psi
104
What are the gasses that compose the barometric pressure? what % of atmosphere are they and what are their partial pressures?
1) Nitrogen - 78.08% atmosphere & 593mmHg
2) Oxygen - 20.95% atmosphere & 159mmHg
3) Argon - 0.93% atmosphere & 7mmHg
4) Carbon Dioxide - 0.03% atmosphere & 0.2mmHg
105
What is the total partial pressure of of the atmosphere at sea level?
760mmHg
106
Calculate the partial pressures for nitrogen and oxygen at sea level (1 atm)?
1) Nitrogen - .78 x 760mmHg = 593mmHg (79kPa)
| 2) Oxygen - .21 x 760mmHg = 159mmHg (21.2kPa)
107
What is the partial pressures of N2O and O2 during a 70:30 induction at an atmospheric pressure of 635mmHg?
1) N20 - 0.7 x 635 = 445mmHg (59.3 kPa)
| 2) O2 - 0.3 x 635 = 191mmHg (25.5 kPa)
108
What is the partial pressure of oxygen at atmospheric pressure of 253mmHg?
0.21 x 253 = 53mmHg (7.1 kPa)
109
How is density calculated?
Density = mass/volume
110
How many feet in a mile?
5280 feet
111
How many km in a mile?
1.609 km
112
How many liters in 1 gallon?
1 gallon = 3.785 liters
113
How many mg in 1 grain?
1 grain = 64.799mg
114
How many inches^3 in 1 cm^3?
1 cm^3 = 0.061 inches^3
115
How many km^2 in 1 mile^2?
1 mile ^2 = 2.59km^2
116
How many lbs/ft^3 in 1 gm/cm^3?
1 gm/cm^3 in 62.43lbs/ft^3
117
What is the SI Unit of measurement for weight?
Weight is a force, which is measured in Newtons
118
What is the SI Unit of measurement for mass?
Kilograms
119
What is the SI Unit of measurement for force?
kPa measured in N/m^2
