States of Matter & Changes of State - Quiz 4 Flashcards

(50 cards)

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
How does surface tension act in a spherical shape?
Tension = Pressure x (Radius/2)
26
What are Surfactants?
Surface Active Agent, like soap, that reduces surface tension
27
What is Saponification?
Chemical Process of making soap from fats/oils Soap is the salt of Fatty Acid
28
What is the Form of Soaps and Surfactants?
Polar head with Non-Polar (Hydrophobic) tail.
29
What are Micelles?
When the Non-Polar, Hydrophobic tails come together and form a sphere. This traps other greasy, water-insoluble things in the center.
30
Increase Intermolecular forces _______ viscosity
Increasing IM forces **increases** Viscosity
31
The greater the Intermolecular Force, the __________ the Vapor Pressures
Greater IM Forces = **Lower** Vapor Pressures
32
What is Vapor Pressure?
The pressure exerted by the most energetic molecules when they escape and become free gas
33
What is the relationship of Temperature to Vapor Pressure & Volatility of a liquid?
**Increased** Temperature = **Increased** Vapor Pressure & Volatility
34
What is the Heat of Vaporization?
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
What is Dynamic Equilibrium?
When the amount of molecules escaping liquid and the amount of molecules going back into liquid are the same. (Balance between Vaporization & Condensation)
36
What is Liquid Volatility?
The tendency of a liquid to Evaporate
37
The higher the Vapor Pressure, the _________ volatile the liquid. The lower the Vapor Pressure, the _______ volatile the liquid. Vice Versa
Higher Vapor Pressure = **More** Volatility Lower Vapor Pressure = **Less** Volatility
38
Inside a Gas Vaporizer, what are the factors that determine the concentration of Gas Delivered?
Temperature and Amount of O2
39
What is the Vapor Pressure of Isoflurane?
239 mmHg
40
What is the Vapor Pressure of Enflurane?
175 mmHg
41
What is the Vapor Pressure of Halothane?
243 mmHg
42
What is the Vapor Pressure of Desflurane?
669 mmHg
43
What is the Vapor Pressure of Sevoflurane?
157 mmHg
44
What is a Boiling Point?
The Temperature when Vapor Pressure = Ambient Pressure
45
The more the Intermolecular forces, the ______ the Boiling Point and the ______ Melting Point
More IM forces = **Higher** Boiling Point & **Higher** Melting Point
46
What kind of effect does Evaporation have?
Cooling effect d/t Endothermic Process EX: Sweating
47
What kind of effect does Consendation have?
Heating effect because it releases energy. EX: Hot steam burning you
48
What is the Molar Enthalpy of Fusion?
Heat needed to convert 1 mole of solid to liquid at its normal meltin point.
49
What is the Triple Point on a Phase Diagram?
The Pressure and Temperature at which a substance exists in all three phases (solid, liquid, gas) in equilibrium
50
What is the Critical Point in a Phase Diagram?
The point at which there is no phase boundaries.