DNAP Chem/Physics Exam 1

Accuracy

refers to how close experimental data is to the actual “true” data. For example, pulse ox correlating with the ABG.

Precision

represents agreement between repeated measures of the same target measure.

Baracity

The ratio of the density of a local anesesthetic to the density of cerebral spinal fluid (CSF). Correlates with specific gravity. One of the most important factors that determine the spread of a local anesthetic in the subarachnoid space.

Hypobaric Solution

 will rise, less dense than CSF, usually local anesthetic and sterile water

Isobaric Solution

spread is minimal, 1:1 ratio of CSF to local anesthetic

Hyperbaric Solution

will sink, more dense than CSF, usually local anesthetic and dextrose

Halogens

highly reactive, have 7 valence electrons, easier to gain 1 to make 8 than remove 7

Alkali Metals

highly reactive, valence shell only contains 1 electron, easy to remove/share (low ionization energy)

nonmetals

will gain electrons when reacting with metals, but will share electrons when reacting with other nonmetals

Noble Gases

Group 18; lack of chemical reactivity, extremely high ionization energy due to complete valence shells (octet rule)

3 primary particles from which atoms are built?

neutrons, protons, electrons

Neutron

neutral charge, in the nucleus, help stabilize the repulsive forces in the nucleus of the positively charged protons and negatively charged electrons

Protons

positive charge, in the nucleus, larger/heavier than electrons, carry an equal but opposite charge to electrons

Electrons

negative charge, form a “cloud” around the nucleus, organized into “fixed” energy levels

meter (m)

International System (SI) unit for distance

kilogram (kg)

International System (SI) unit for weight

second (sec)

International System (SI) unit for time

ampere (A or amp)

International System (SI) unit for electrical current

kelvin (K)

International System (SI) unit for temperature

mole (mol)

International System (SI) unit for amount of substance

candela (cd)

International System (SI) unit for light intensity

newton (N)

International System (SI) unit for force

pascal (Pa)

International System (SI) unit for pressure

joule (J)

International System (SI) unit for energy or work

watt (W)

International System (SI) unit for power

specific gravity

the ratio of an object’s density to that of a reference, usually water

matter

object or material that has both mass and occupies space

Standard Temperature and Pressure (STP): Temperature

273 kelvin

Standard Temperature and Pressure (STP): Pressure

1 atm

what makes up all matter?

atoms

What states can matter exist in?

liquid, solid, gaseous, plasma

Liquid

state of matter that has definite volume and assumes shape of container

Solid

state of matter that has both shape and volume

Gas

state of matter that has neither definite shape or volume, will easily change volume with changes in temperature and pressure

Plasma

state of matter that is a mixture of ionized gas and free-floating electrons

Enthalpy

measure of the amount of energy associated with substances in a reaction

Examples of endothermic changes of state

sublimation (dry ice to CO2), melting (ice to water), vaporization (water to steam)

Examples of exothermic changes of stae

condensation (steam to water), freezing/crystallization (ice formation)

Physical properties

color or odor

Chemical properties

flammability

pure substance

matter that can’t be separated physically and the chemical and physical properties are uniform throughout with regard to chemical and physical properties are classified as:

mixture

matter that contains two or more pure substances is classified as:

homogeneous

mixture that is uniform throughout and can’t be separated

heterogeneous

mixture that is non-uniform and may be separated into component parts

Atomic number

the number of protons in the nucleus

Mass number

total number of protons + neutrons in the nucleus

Isotopes

atoms with identical atomic numbers but different mass numbers & different number of neutrons. how most elements in nature occur

horizontal rows on periodic table

periods (1-7)

vertical columns on periodic table

groups (18)

Cation

a positively charged ion due to the loss of electron(s)

-will be smaller than the parent atom because the excessive positive charge "pulls" the electrons closer to the nucleus (there is no longer a balance between attractive and repulsive forces)

Anion

-negatively charged ion due to the gain of electron(s)

-larger than the parent atom since the "pull" of the nucleus on any given electron is reduced

Monoatomic gases

completely full valence shells, most stable

halogens and alkali metals

the halogens (F, Cl, Br, I…) have 7 valence electrons, so it is much easier to gain 1 electron to make 8 rather than remove 7; this is why they are highly reactive. The alkali metals are similarly highly reactive as their valence shell only contains 1 electron, making it easy to remove/share.

calcium (Ca)2+

blood clotting, muscle contraction, nerve impulse transmission

Iron (Fe)2+

oxygen transport

Potassium (K+)

regulate cellular ion concentrations

Sodium (Na+)

muscle contraction, nerve impulse transmission

Hydrogen carbonate (bicarbonate) (HCO3)-

acid-base balance

Hydrogen Phospate (HPO4)2-

acid-base balance

Ionization potential

the energy required to removal an electron from a neutral atom. the stronger the bond, the higher the ionization potential

Ionization potential

as you move down in a particular group on the periodic table, the atom size increases, so the outer most electron is progressively further and further away from the nucleus and the ionization energy decreases. It will require less and less energy to remove the outermost electron(s) (low hanging fruit kind of thing) As you move across the table in periods, the atom size decreases, the outermost electrons are therefore closer to the nucleus and harder to remove, so the ionization energy increases. (more tightly held by nucleus) This energy is low for the alkali metals that have one valence electron and extremely high for the noble gases that have complete valence shells. Remember, the removal of an electron results in a positive ion.

electron affinity

the ease with which a neutral atom gains an electron, represents the energy released when a single electron is added to a neutral atom in the gaseous state resulting in a negative ion

Electronegativity

the ability of an atom in a molecule to attract electrons to itself in a chemical bond (how strongly the atoms pull on the electons in a bond)

electron affinity & electronegativity

both generally decrease as you move down a group on the table and increase as you move left to right across periods

First Law of Therodynamics

(the law of conservation of energy): energy is not created or destroyed, just converted to another form or transferred to another part of the system

Second Law of Thermodynamics

A system and its surroundings tend towards increasing disorder or randomness

Entropy

The measure of disorder or randomness (think second law of thermodynamics)

catalyst

presence of this will increase the rate of reaction

Kids Have Dropped Over Dead Converting Metrics

K=Kilo, H=Hecto, D=Deca, O= Base Unit (Liter, Meter, or Gram), D=Deci, C=Centi, M=Milli

percent concentrations

X amount % concentration = X g/100mL

To easily convert X% concentration to mg/mL simply move the decimal point to the right one spot (i.e 0.9% NaCl = 9mg NaCl/mL)

1% Lidocaine

10mg/ml

2% Lidocaine

20mg/ml

0.5% Bupivacaine

5mg/ml

3% Nesocaine

30mg/ml

7.5% Bupivacaine

75mg/ml

¼ or .25

2.5mg/ml

1/8 or 0.125

1.25mg/ml

1/10 or 0.1

1mg/ml

1/16 or 0.0625

0.625mg/ml

1/32 or 0.03125

0.3125mg/ml

Epi 1:1000 (most common preparation)

1mg/ml or 1000mcg/ml

Epi 1:10,000 (ACLS dose)

100mcg/ml

Epi 1:100,000

10mcg/m

Epi 1:200,000

5mcg/ml

Epi 1:400,000

2.5mcg/ml

Epi 1:500,000

2mcg/ml

Lidocaine with epi max dose

7 mg/kg (300mg max single dose)

Lidocaine without epi max dose

4.5mg/kg (300mg max single dose)

Mepivacaine with epi max dose

7mg/kg (400mg max single dose)

Mepivacaine without epi max dose

5mg/kg (400mg max single dose)

Chloroprocaine with epi max dose

14mg/kg (1000mg max single dose)

Chloroprocaine without epi max dose

11mg/kg (800mg max single dose)

Bupivacaine with epi max dose

2.5mg/kg (225mg max single dose)

Bupivacaine without epi max dose

2mg/kg (175mg max single dose)

Levobupivacaine with epi max dose

3.2mg/kg (no max single dose)

Levobupivacaine without epi max dose

2.5mg/kg (no max single dose)

Ropivacaine with epi max dose

3.5mg/kg (no max single dose)

Ropivacaine without epi max dose

3mg/kg (no max single dose)

Tetracaine with epi max dose

3mg/kg (200mg max single dose)

Tetracaine without epi max dose

1-2mg/kg (200mg max single dose)