Chemistry and physics Flashcards

1
Q

An ion is an

A

atom that carries a positive or negative charge

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2
Q

A ___________________________- involves the complete transfer of valence electron(s) from one atom to another. This leaves one atom with a negative charge and the other with a positive charge.

A

ionic bond

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3
Q

_______ tend to form ionic bonds.

A

Metals
acids & bases

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4
Q

____________ involves the equal sharing of electrons.

A

Covalent bonds

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5
Q

A single bond is created when

A

one pair of electrons is shared

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6
Q

A double bond is created when

A

two pairs of electrons are shared

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7
Q

__________ describes a very weak intermolecular force that holds molecules of the same type together

A

Van der Waals’ forces

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8
Q

_______________ are when atoms share electrons, but the electrons tend to remain closer to one atom than the other

A

Polar covalent bonds

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9
Q

A key example of a polar covalent bond is

A

water
the region near the oxygen atom is relatively negative and the region near each hydrogen atom is relatively positive

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10
Q

Molecular bonds in decreasing order of strength are

A

covalent>ionic>polar covalent

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11
Q

The atom consists of the following three components:

A

protons (+ charge)
neutrons (no charge)
electrons (negative chrage)

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12
Q

What parts form the nucleus of the atom?

A

protons and neutrons

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13
Q

The number of ____________ in the nucleus determines the atom’s atomic number

A

protons

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14
Q

The electrons in the outermost shell are called

A

valence electrons

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15
Q

An incomplete shell allows

A

an atom to react with another atom

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16
Q

Two or more atoms bonded together is called a

A

molecule

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17
Q

A full shell makes the atom

A

non-reactive (inert)

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18
Q

An atom will have a neutral charge if

A

electrons= # protons

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19
Q

An atom will have a positive charge if

A

electrons <# protons

20
Q

An atom will have a negative charge if

A

electrons> #protons

21
Q

An atom with a positive charge (it has lost electrons) is called a

A

cation

22
Q

An atom with a negative charge (it has gained electrons) is called an

A

anion

23
Q

Dalton’s law is about

A

gas pressures; it says that the total pressure is equal to the sum of the partial pressures exerted by each gas in the mixture

24
Q

Dalton’s law equation is

A

Ptotal= P1+ P2 + P3

25
Q

Applications of Dalton’s law:

A

calculate the pressure of an unmeasured gas
calculate the total pressure of a gas mixture
convert partial pressure to volumes percent
convert volumes to partial pressure

26
Q

What is the equation to convert a partial pressure to volumes percent with a liquid?

A

volume of solute/volume of solution x100

27
Q

What is the equation to convert a partial pressure to volumes percent of a gas?

A

partial pressure/total pressure x 100

28
Q

At sea level, the agent monitor measures the end-tidal isoflurane as 8 mmHg. Convert this to volumes percent.

A

8 mmHg/760 mmHg x100= 1%

29
Q

What is the equation to convert volumes percent to a partial pressure?

A

partial pressure = (volumes %/ 100) x total pressure

30
Q

At sea level the agent monitor measures the end-tidal sevoflurane as 2%. What is the partial pressure of sevoflurane in the exhaled tidal volume?

A

15.2 mmHg

31
Q

Which component of the oxygen delivery equation is MOST affected by Henry’s law?
a. cardiac output
b. hemoglobin
c. arterial oxygen saturation
d. PaO2

A

PaO2

32
Q

Henry’s law is about

A

gas solubility

33
Q

Henry’s law states that at

A

a constant temperature, the amount of gas that dissolves in a solution is directly proportional to the partial pressure of that gas over the solution

34
Q

Applications of Henry’s Law includes

A

anesthetic emergence is prolonged in the hypothermic patient
overpressuring the vaporizer
increasing the FiO2 increases the PaO2

35
Q

Fick’s law of diffusion describes the

A

transfer rate of a gas through a tissue medium

36
Q

Applications of Fick’s law include

A

cardiac output calculation
placental drug transfer
diffusion hypoxia
a patient with severe OCPD has a slower rate of inhalation induction

37
Q

Graham’s law says that the

A

molecular weight of a gas determines how fast it can diffuse through a membrane

38
Q

___________ molecules tend to diffuse faster than ________ molecules

A

smaller; larger

39
Q

The higher the gas pressure the

A

more it will dissolve into a liquid

40
Q

How does temperature affect solubility?

A

increased temperature decreases solubility
lower temperature increases solubility

41
Q

What is the solubility coefficient of oxygen?

A

0.003 mL/dL/mmHg

42
Q

What is the solubility coefficient of carbon dioxide?

A

0.067 mL/dL/mmHg

43
Q

CO2 is ________times more soluble than O2

A

20x

44
Q

What is the oxygen delivery equation?

A

Do2= Co x [(1.34 x Hgb x SpO2)] + (PaO2 x 0.003)] x 10

45
Q

The rate of transfer of gas in directly proportional to

A

partial pressure difference (driving force)
diffusion coefficient (solubility)
membrane surface area

46
Q

The rate of transfer of gas is inversely proportional to

A

membrane thickness
molecular weight

47
Q

Applications of Graham’s law include

A

second gas effect- using N2O to hasten the onset of a volatile anesthetic (the second gas)
high fresh gas flow is turbulent as it passes through the annular space (determined by the gas’s density)