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N927:Chem/Physics > Exam 1 > Flashcards

Exam 1 Flashcards

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1
Q

How many mcg/mL in 1:1000 concentration of epinephrine (stock epi)?

A

1000mcg/mL

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2
Q

How many mcg/ml in 1:200,000 concentration epinephrine?

A

5mcg/mL

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3
Q

How many mcg/mL in 1:500,000 concentration Epinephrine?

A

2mcg/mL

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4
Q

How many mcg/mL in 1:400,000 concentration epinephrine?

A

2.5mcg/mL

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5
Q

Why do we give epi with LA?

A

1) epi vasoconstrict reducing blood flow thus reducing the dose of LA needed
2) epi vasoconstricts reducing blood flow so less chance of anesthesia leaking out into system

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6
Q

What is the recommended LA single injection doses for lidocaine?

A

7mg/kg with Epi

5mg/kg without

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7
Q

What is the LA single dose max for mepivacaine?

A

7 mg/kg with epi

5mg/kg without

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8
Q

Chlorprocaine LA single dose max?

A

14mg/kg with epi

12mg/kg without

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9
Q

LA single dose max for bupivacaine?

A

3 mg/kg with epi

2mg/kg without

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10
Q

What is single dose max for Levobupivacaine?

A
  1. 2 mg/kg with epi

2. 5 mg/kg without

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11
Q

What is the LA single dose max for ropivacaine?

A

3.5 mg/kg with epi

3 mg/kg without

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12
Q

What is single dose of LA max for tetracaine?

A

3 mg/kg with epi

1-2 mg/kg without

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13
Q

Matter is composed of discrete units called____

A

atoms

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14
Q

Atoms are composed of ____

A

subatomic particles (electrons, protons, neutrons)

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15
Q

Atoms are the smallest fraction of an element that can exist however they can still show _____ of an element.

A

characteristics

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16
Q

Electrons orbit in a ___ pattern around the nucleus d/t their electric charge

A

3D pattern (like a cloud)

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17
Q

Closer to the nucleus the electron is the ___ energy it is.

A

Lower energy. It is more stable the closer to the protons in the nucleus it is.

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18
Q

Why are electrons far apart?

A

They repel each others negativity.

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19
Q

Why do electrons spin in opposite directions?

A

So they can pair despite their repulsion.

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20
Q

What are the correct postulations of Dalton’s laws?

A

1) atoms of different elements have different properties
2) Atoms are neither created nor destroyed in chemical reactions (they obey the laws of conservation of matter)
3) Atoms of different elements form compounds in whole number ratios (H2O, H2O2)

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21
Q

What are the negated postulations of Dalton’s Laws?

A

1) All matter is made of tiny, indestructible particles called atoms–> fusion and fission reactions negated this postulate
2) All atoms of a given element are identical–> isotopes exist (different numbers of neutrons)

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22
Q

When you break an atom apart it is called? What happens with the energy? (Hint: atomic bomb, nuclear power industry)

A

Fission. HUGE amount of energy released. This is what is used in atomic bombs and nuclear power industry.

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23
Q

What happens when you put two elements together? What happens with the energy? (Hint: H-bomb)

A

Fusion. Production of ENORMOUS amounts of energy as seen in the H-bomb where isotopes of hydrogen combine under extremely high temperatures to create Helium.

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24
Q

The further away from the nucleus the ____ the electrons negative charge.

A

Stronger

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25
Atomic weight=
proton+neutron
26
How many electrons in 1st orbital?
2 electrons
27
How many electrons in 2nd orbital?
8 electrons
28
The Nucleus of an atom is composed of what subatomic particles? What is the charge?
Proton and neutron. Proton is positively charged and the neutron is neutral so nucleus is positively charged.
29
The number of electrons=
the number of protons
30
What happens if the electrons do not equal the protons?
You have an ion.
31
Most of the mass is found where?
nucleus d/t the protons+ neutrons
32
The number of protons is the elements?
Atomic number
33
Atoms with the same number of protons and electrons are what in respect to charge?
neutral
34
If we give up protons we become?
An ion (cation/anion)
35
Electrons bestow?
electronegativity
36
Elements can lose or gain what subatomic particle?
electrons
37
Oxygens electronegativity would be?
Strong. Oxygen having 8 electrons distributes 2 to first shell and 6 to second shell making it close to the "octet". So it really wants to take other elements electrons.
38
Free radical is an...
Uncharged molecule (typically highly reactive and short lived) having an unpaired valence electron.
39
Free radicals can... (think electrons)
either donate or accept an electron from other molecules therefore behaving has oxidants or reductants.
40
Free radicals can.... ( think biologically)
damage biologically relevant molecules such as DNA, proteins, carbs, and lipids
41
How are free radicals produced?
normal metabolic processed (endogenous i.e metabolism) or from external sources (exogenous i.e. exposure to X-Rays, ozone, cigarette smoke, air pollutants, industrial chemicals.
42
What dampens the effects of Free radicials
antioxidants
43
Enzymatic reactions serve as a source for
free radicals
44
What enzymatic reactions are included in creating free radicals?
Those in the respiratory chain (ETC in the mitochondria), phagocytosis, prostaglandin synthesis, and in the cytochrome P-450 system.
45
How do antioxidants protect the cell from Free radicals?
They donate an electron to neutralize them.
46
How do we get homeostasis with free radicals?
We must balance production of free radicals and antioxidants
47
Electrons in energy level 1 have ___ energy.
Lower because they are closer to the nucleus.
48
Electrons in the farthest away energy level have ___ energy.
Higher because they are farther away from the nucleus.
49
Electrons want to orbit closer to which element?
The one closer to filling its valence electron shell (octet rule). The more electronegative element.
50
Polar molecules are
Electronegative
51
Electrons can ___ orbitals if enough energy is supplied.
jump
52
Element
cannot be separated into a simpler substance
53
A single atom has a
specific atomic number and atomic mass
54
Atomic number=
number of protons in the nucleus
55
atomic mass=
total number of protons and neutrons
56
Isotope=
different form of the element that has the same number of protons but DIFFERENT number of neutrons thus also a different atomic mass
57
atomic weight=
average mass of naturally occurring isotopes
58
Atomic mass/weight is of 1 atom is very small and is described as___
atomic mass unit (AMU)
59
1 mole=
6.02x10^23 atoms
60
AMU=
weight in grams
61
across the same row of elements what happens to electronegativity?
It increases.
62
What is matter?
has a mass (weight) and occupies space.
63
What gives matter its mass?
number of particles
64
Matter=
granular structure composed of molecules existing in three phases: solid, liquid, gas
65
mass=
given quantity of matter in an object
66
Mass is not the same as
weight
67
weight takes into account
gravitational force
68
Latent heat
amount of heat absorbed or released by a substance during a change in physical state
69
latent heat of vaporization
amount of energy a substance absorbs to overcome the attractive forces between molecules (S to L to Gas requires more heat respectively)
70
Less dense in which direction of phases of matter?
gas to liquid to solid (minus ice)
71
What is brownian motion?
random motion of particles suspended in a fluid (gas or liquid) resulting from their collision with the fast moving atoms or molecules in the gas or liquid.
72
Brownian motion is the basis of
diffusion
73
Molecular motion: molecules can move in what three ways?
translational (gas has highest form of this movement), rotational, vibrational
74
Translational movement=
all atoms/molecules from one place to another
75
rotational movement=
spinning around 3D axis
76
Vibrational movement=
bending/stretching/rotating bonds (change in shape)
77
when does molecular motion stop
absolute zero
78
What is the change in composition of matter?
atoms or molecules of 2 or more substances rearrange to form 2 or more new substances having different properties
79
Oxidation is the ___ of electrons
loss
80
Reduction is the ___ of electrons
gain
81
what is oxidized and reduced to form H2O?
hydrogen is oxidized giving its electron to oxygen which is reduced
82
if weight changed due to different forces exerted what stays the same
mass
83
Volume=
measure of the amount of space enclosed by a closes surface or space occupied by a given number of particles
84
Molecule=
2 or more atoms that are chemically joined, smallest unit that retains the physical and chemical properties of a substance
85
compound=
a molecule that contains at least two different elements
86
intramolecular forces=
attractions within a molecule ( i.e. covalent and ionic)
87
intermolecular forces=
attractions between molecules (i.e dipole-dipole, h-bonding, van der waals)
88
Molecular weight=
sum of all atomic weights of all the elements of a molecule or compound
89
Gram molecular weight
expression of MW of a substance in terms of grams, also known as a mole (1 mole= 6.02x10^23 at STP)
90
Gram molecular volume
one GMV( or mole) of a gas always 22.4L
91
Density =
mass of substance per unit of volume, measured in weight/volume in liquid (cm^3=mL) and MW/ gram molecular weight (gram/L)
92
Less dense gas = ___ flow of gas
easier
93
Specific gravity=
weight of a unit Volume of liquid or gas compared to a unit volume of H2O or dry air , ratio between the 2 densities
94
baricity=
density relative to CSF, if denser and patient is standing will go downward...positioning maters
95
Gravity=
every object attracts every other object with a force directed along the line of the center of the two objects, weak attractive force, force varies inversely with the square of the distance--> father away the objects are the less attracted
96
cohesion=
interaction between LIKE molecules (closer they are great force of attractions) (great in solids, least in gas)
97
decreased cohesion occurs with
added energy.
98
cohesive forces are ____ forces between molecules of like subtances/
INTERmolecular
99
adhesion =
interaction b/w UNLIKE molecules
100
adhesion and cohesion forces ___ with each other
compete
101
Properties of H2O because of its polar covalent bonds
1) dipolar nature of H2O makes it universal solvent 2) high latent heat-stores more heat per unit volume than most other substances and releases heat slowly 3) high heat of vaporization- large amount of heat required to break down hydrogen bonds and the heat is carried off at H2O vapor 4) water dissociates to H+ and 0H- thus contributing to the acid/base balance
102
van der waals=
weak, short range electrostatic attractive force (intermolecular force) between uncharged molecules, arising from the interaction of permanent or transient electric dipole moments
103
electric dipole moment=
measure of the separation of positive and negative electrical charges within a system, that is, a measure of the systems overall polarity (london dispersion forces)
104
% concentration
grams in a dL or in every 100mL (gm/dL=gm/100mL)
105
conversion of % concentration to mg/mL
move to right one decimal (2.5% is 25 mg/ml)
106
Converting mg/mL to %
move to left one decimal (2.5mg/ml is 0.25%)

N927:Chem/Physics (1 decks)

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