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Spring 2020 - Chemistry & Physics > States of Matter & Changes of State - Quiz 4 > Flashcards

States of Matter & Changes of State - Quiz 4 Flashcards

1
Q

Characteristics of

Solid:

Liquid:

Gas:

A
  • Solid: Definite Volume & Shape
  • Liquid: Definite Volume
  • Gas: No Definite Shape or Volume
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2
Q

Liquid Intermolecular forces can and can’t do what?

A

Can hold molecules together, but cant prevent them from sliding past each other

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3
Q

What are the Intermolecular Forces for Gas Molecules?

A

Zero

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4
Q

What is Deposition?

A

Gas to Solid

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5
Q

What is Sublimation?

A

Solid directly into Gas

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6
Q

Cations

A

Metals that tend to give up electrons

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7
Q

Anions

A

Non metals that tend to acquire electrons

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8
Q

What is an Ionic Bond?

A

Attraction between oppositely charged ions

Stronger than Covalent Bonds

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9
Q

What are Covalent Bonds?

A

Sharing of Electrons by overlapping electron clouds of two atoms

Weaker than Ionic Bonds

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10
Q

Valence Electrons

A

Electrons on the Outer Most Shell

Number of Valence electrons = Group Number

They all want eight (octet rule)

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11
Q

VSEPR Theory

A

Valence Shell Electron Pair Repulsion

The groups connected to central atoms want to get away from eachother

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12
Q

What is Pauling’s concept of Electronegitivity?

A

More Electronegative atoms will tend to pull electrons towards themselves

Flourine is the most Electronegative

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13
Q

What is a Non-Polar Bond?

A

When two bonded atoms have the same electronegativity

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14
Q

What is a Polar Bond?

A

When two bonded atoms have different electronegativity.

The electrons are closer to the more electronegative atom

Creates Partial Charge

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15
Q

What are the main types of Intermolecular Forces?

A

Dipolar

Hydrogen Bonding

London Forces

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16
Q

Dipole-Dipole Attraction

A

Only happens between Polar Molecules or those of Opposite Partial Charges

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17
Q

Hydrogen Bonding

A
  • Type of Dipolar Interation
  • Only when directly bonded to F, O, N
  • Stronger than Dipole-Dipole
  • So when Hydrogen is bonded to F/O/N, that same Hydrogen highly attracts other things w/ partial negative charge
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18
Q

How is Hydrogen Bonding Important to the body?

A
  • Keeps water in liquid state
  • Holds DNA together
  • Maintain Enzymes
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19
Q

Ion Dipole Attraction

A
  • Attraction b/t Ionic & Polar Molecule
  • Allows ionic solids to dissolve in water
  • Strength depends on dipole moment
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20
Q

What are London Forces?

A
  • Weakest, but Most Important and found Everywhere
  • Occurs with uneven distribution of e- –> instant dipole
  • Bigger molecules have bigger London Forces d/t more e-
  • AKA Vander Waal Forces
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21
Q

What changes with more Intermolecular Forces?

A

↑Boiling & ↑Melting

↑Heat of Fusion & Vaporization

↑Viscosity

↓Vapor Pressure

Solubility

22
Q

How does Intermolecular Forces relate to Surface Tension?

A

Greater Intermolecular Forces = Greater Surface Tension

23
Q

According to LaPlace’s Law, what is the relationship between surface tension and radius?

A

In a blood vessel, the surface tension is directly proportional to the radius of the vessel.

Tension = Pressure x Radius (Cylindrical)

24
Q

LaPlace states in a blood vessel, the smaller the radius. the ________ pressure it can withstand

A

Smaller the radius of blood vessel, the more pressure it can withstand

25
Q

How does surface tension act in a spherical shape?

A

Tension = Pressure x (Radius/2)

26
Q

What are Surfactants?

A

Surface Active Agent, like soap, that reduces surface tension

27
Q

What is Saponification?

A

Chemical Process of making soap from fats/oils

Soap is the salt of Fatty Acid

28
Q

What is the Form of Soaps and Surfactants?

A

Polar head with Non-Polar (Hydrophobic) tail.

29
Q

What are Micelles?

A

When the Non-Polar, Hydrophobic tails come together and form a sphere. This traps other greasy, water-insoluble things in the center.

30
Q

Increase Intermolecular forces _______ viscosity

A

Increasing IM forces increases Viscosity

31
Q

The greater the Intermolecular Force, the __________ the Vapor Pressures

A

Greater IM Forces = Lower Vapor Pressures

32
Q

What is Vapor Pressure?

A

The pressure exerted by the most energetic molecules when they escape and become free gas

33
Q

What is the relationship of Temperature to Vapor Pressure & Volatility of a liquid?

A

Increased Temperature = Increased Vapor Pressure & Volatility

34
Q

What is the Heat of Vaporization?

A

The Amount of Energy needed to free one mole of liquid, at its boiling point, into the gas phase

(AKA Molar Enthalpy of Vaporization)

35
Q

What is Dynamic Equilibrium?

A

When the amount of molecules escaping liquid and the amount of molecules going back into liquid are the same.

(Balance between Vaporization & Condensation)

36
Q

What is Liquid Volatility?

A

The tendency of a liquid to Evaporate

37
Q

The higher the Vapor Pressure, the _________ volatile the liquid.

The lower the Vapor Pressure, the _______ volatile the liquid.

Vice Versa

A

Higher Vapor Pressure = More Volatility

Lower Vapor Pressure = Less Volatility

38
Q

Inside a Gas Vaporizer, what are the factors that determine the concentration of Gas Delivered?

A

Temperature

and

Amount of O2

39
Q

What is the Vapor Pressure of Isoflurane?

40
Q

What is the Vapor Pressure of Enflurane?

41
Q

What is the Vapor Pressure of Halothane?

42
Q

What is the Vapor Pressure of Desflurane?

43
Q

What is the Vapor Pressure of Sevoflurane?

44
Q

What is a Boiling Point?

A

The Temperature when Vapor Pressure = Ambient Pressure

45
Q

The more the Intermolecular forces, the ______ the Boiling Point

and the ______ Melting Point

A

More IM forces =

Higher Boiling Point & Higher Melting Point

46
Q

What kind of effect does Evaporation have?

A

Cooling effect d/t Endothermic Process

EX: Sweating

47
Q

What kind of effect does Consendation have?

A

Heating effect because it releases energy.

EX: Hot steam burning you

48
Q

What is the Molar Enthalpy of Fusion?

A

Heat needed to convert 1 mole of solid to liquid at its normal meltin point.

49
Q

What is the Triple Point on a Phase Diagram?

A

The Pressure and Temperature at which a substance exists in all three phases (solid, liquid, gas) in equilibrium

50
Q

What is the Critical Point in a Phase Diagram?

A

The point at which there is no phase boundaries.

Spring 2020 - Chemistry & Physics (8 decks)

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