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SRNAChem&Physics > State of Matter > Flashcards

State of Matter Flashcards

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1
Q

States of matter, SOLID

A

Molecules made up of solid are arranged in regular repeating patterns, held firmly in place, can vibrate within a limited area

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2
Q

Liquids

A

Volume no shape
takes on shape of container
Molecules are also touching but have more movement

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3
Q

In liquids

A

intermolecular forces are weaker and allow the molecules to slid past one another

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4
Q

Are liquid compressible

A

NO

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5
Q

Gases

A

Has no definite volume or shape
Expand to fill container
Molecules are not touching ahd have more common movement

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6
Q

Liquid to gas

A

eVaporization

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7
Q

Gas to liquid

A

COndensation

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8
Q

Gas to solid

A

Deposition

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9
Q

Solid to gas

A

Sublimation

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10
Q

Liquid to solid

A

Freezing

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11
Q

Solid to liquid

A

melting

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12
Q

Heat of fusion

A

Amount of energy to melt a solid into liquid phase

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13
Q

Heat of vaporization

A

amount of energy necessary to vaporize a liquid into a gas phase

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14
Q

Heat is the amount of________? is heat the same as temperature?

A

energy flowing into an object not the same as temperature.

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15
Q

Melting - SOLID to LIQUID, As more heat energy is added,

A

Solid: vibration between particles become greater until the movement overcome the intermolecular forces holding the molecules together, causing dissociation into a liquid state.

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16
Q

Intermolecular forces

A

Determine how molecules interact with one another
Are electrostatic in nature
Based on electron organization

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17
Q

Atoms tends to either

A

gain, lose or share electrone in order to achieve a toltal of 8 valence electron - like noble gases.

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18
Q

The close an element is to noble gas

A

the more reactive it is (electronegative)

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19
Q

Dipole dipole interaction examples

A

Acetone; delta means partial

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20
Q

Acetone is

A

polar molecule

boiling point is 56 C, liquid at room temperature

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21
Q

Hydrogen bonding ex

A

Water

Polar molecure

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22
Q

What is the strongest dipole bond

A

Hydrogen bonding

Boling point 100C liquid at room temperature

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23
Q

London dispersion forces ex

A

CH4
Non polar molecues
weakest type of intermoleculs bond
boiling point -164C gas at room temp

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24
Q

Lewis structure

A

used in chemistry to describe chemical bonds using valence electrons
Straight lines represent shared pairs of electrons
Dots represent lone pair of electros
Oxygen has 6 valence but gains 2 more from 2 hydrogens for a total of 8, its nearest noble gas NE.

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25
Q

Hydrogen has

A

one valence electron, but gaisn another from oxygen for a total of 2 its nearest noble gas.

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26
Q

Ionic bond:

Examples:

A

one atom donates electron to another

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27
Q

what is the strongest type of bond

A

IOnic

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28
Q

Covalent

A

Not as strong as ionic

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29
Q

In covalent, atoms

A

share electrons

30
Q

Usually a metal donating

A

an electron to a non-metal

31
Q

Covalent bond

A

Shared electrons spend more time around the more electronegative atom, leading to a polar covalent bond

32
Q

Surface tension

A

Water molecules are attracted to other water molecules
STick together.
poses potential problem in the lungs

33
Q

Surface tension

A

On a surface this causes side to side and downward attraction forces , but no balancing attractions from above the surface of the liquid,

34
Q

Surfactants does what

A

Lower surface tension

35
Q

Without surfactant

A

Collapsed alveoli

36
Q

Inhaled anesthetics come in a

A

Liquid form

Changes states from liquid to vapor via VAPORIZERS

37
Q

Vapor pressure

A

when molecules of a liquid escape into the gas phase, they collide with the walls of the container, exerting force on the wall. This is called vapor pressure.

38
Q

An increase temperatures

A

Causes an increase in vapor pressure and volatility

39
Q

Ethanol is more

A

volatile than water at the same temperatures

40
Q

Relates vapor pressure to temperature

A

Clausius Capeyron Equation

41
Q

Clausius Capeyron Equation

A

logP = A + B / T

42
Q

A and B depends

A

On the particular fluid

43
Q

What is the vapor pressure of enflurance at 25 C?

Given A= 7.967 Torr, B = -1678 torr/K

A

log P = 217 mmHg

44
Q

X enflurane =

A

Vapor pressure of enflurane / Total pressure

45
Q

Boiling point of a liquid

A

will increase if the pressure on the liquid is increased

46
Q

Phase diagram

A

Shows Triple state of water or other l

47
Q

States of matter: Liquid, the molecules flow

A

Easily around one another
Kept from flying around by attractive forces between them
Assume shape of their container

48
Q

States of matter: GAS the molecules fly

A

in all direction at GREAT SPEED, they are so far apart that the attractive forces between them are INSIGNIFICANT

49
Q

Solid are held by

A

INTERMOLECULAR FORCES

50
Q

Are solids compressible

A

NO

51
Q

Vaporization – Liquid to GAS state

A

If we continue to add more heat energy, the movement continues to increase overwhelming the intermolecular forces and particles begin to escape the liquid surface vaporizing into a gas

52
Q

What are the 3 types of INTERMOLECULAR FORCES

A
  1. Dipole-dipole
  2. Hydrogen bonding
  3. London-Dispersion Forces
53
Q

What is the weakest types of intermolecular bonds?

A

London dispersion forces

54
Q

The thin film of fluid lining the aveloli could

•Surfactant reduces

A
  • cause the walls to stick together and collapse

- the surface tension so this does not happen.

55
Q

Volatility is the

A

tendency of a liquid to change into gas

56
Q

Higher volatility = __________

Higher volatility = ___________

A

Higher evaporation

Higher Vapor pressure

57
Q

This equation is used to calculate the Vapor

Pressure of a liquid

A

logP = A + B/T

58
Q

If O2 is sent through a vaporizer with liquid enflurane,
the composition of the O2 enflurane mixture will depend
on

A

the temp. of the vaporizer and the pressure of the O2.

59
Q

Vapor Pressure determines

A

the (mole fraction, or) Partial Pressure of a volatile anesthetic in a gas mixture

60
Q

Boiling point is the

A

Boiling point is the temperature at which the vapor
pressure is equal to the ambient pressure (normally one
atmosphere).

61
Q

Boiling point of a liquid will_________ if the

pressure on the liquid is increased. Ex:

A

increase ; Water normally boils into steam at 100C, but in a sealed pressurized autoclave, the boiling point increases to 120C or more.

62
Q

PHASE DIAGRAM

A

Shows the combined effects of temperature and pressure on the state of matter.

63
Q

Explain why water is liquid at room temperature while CO2 is a gas

A

Water can form hydrogen bonds that can hold the water molecules into a liquid state even when the average kinetic energy of the molecule is relatively high.

64
Q

Why does NACL dissolves in water and not in covalent solvent?

A

When NACL dissociates in water, it separates into Na+ and Cl- ions. Organic solvents are not polar enough to solvate the ions and keep them away from each other.

65
Q

How does vapor pressure depend on temperature?

A

At temperature INCREASES, VAPOR PRESSURE INCREASES

AS intermolecular FORCES DECREASE, Vapor PRESSURE INCREASES.

66
Q

What is a surfactant and how do they break surface tension? examples when useful..

A

Surface active agents , known as soaps and detergents, have an ionic, hydrophillic end that allows the surfactant to interact with water molecules. The surfactant also haas a HYDROPHOBIC tail that prevents the water molecules from interacting with each other. This reduces the surface tension and cohesion of the water. Cleaning and preventing the collapse of a premature baby’s lungs are 2 applications of surfactants.

67
Q

Do you expect nitrous oxide to be more soluble in the adipose tissue or in the blood? Explain.

A

Nitrous oxide has a small molecule dipole but is not very polar compared to water. Therefore nitrous oxide is expected to be preferentially soluble in adipose tissue.

68
Q

Which state of matter (solid, liquid or gas) do you expect to be the least dense? Explain.

A

The gas state. Since the molecules are not in contact with each other, the volume of the gas will be greater and as the volume of a SAMPLE INCREASES, the DENSITY DECREASES

69
Q

The constants in the modified Clausius-Clapeyron equation for sevoflurane are A= 8.083 torr and B= -1.726torr. K. remember that temperature expressed in Kelvin
Calculate the vapor pressure at temperature of 20.0C?
Calculate the vapor pressure at temperature of 25C?
Calculate the vapor pressure at temperarture of 35C?

A

log (P) = A + B/ T

a. 156 torr
b. 195 torr
c. 301 torr

70
Q

The boiling points of Sevoflurane and Desflurane are 59C and 23C, respectively.

a. which compound has the greater amount of intermolecular forces?
b. Which compound do you believe is more polar?
c. Based on your answer earlier, which compound is more soluble in a polar solvent, like water?

A

a. In order to boil, the temperature must be great enough for the kinetic energy of the molecules to overcome the attractions due to intermolecular forces. In this case, sevoflurane has more intermolecular forces.
b. Greater polarity results in more intermolecular attractive forces, which suggests sevoflurane is the more polar substance
c. Following from the previous answer, sevoflurane appears to be more polar, so it should be more soluble in a polar solvent, such as water.

SRNAChem&Physics (13 decks)

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