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Chem 103 > Unit 4 > Flashcards

Unit 4 Flashcards

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1
Q

What are London Dispersion forces and what are they present in

A

Very weak and temporary; found in everything

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2
Q

What is the relationship between IMF and KE

A

disproportinal. High IMF is low KE

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3
Q

When do dipole-dipole interactions occur

A

Between polar and nonpolar molecules (partial negative and partial positive)

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4
Q

When do H bonds occur and what are they

A

Very strong dipole-dipole interaction that occurs due to a very polar bond. Occurs between H and N, O, or F

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5
Q

What are ion-dipole interactions

A

occur when the partial positive or negative region of a polar molecule is attracted to an ion of hte opposite sign

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6
Q

What is the order of IMFs from weakest to strongest

A

London Dispersion, dipole-dipole, H bonds, ion-ion, and ion dipole bonds

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7
Q

What is viscosity

A

Resistance to flow

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8
Q

What are the three things that Viscosity depends on

A

IMFs, size/ shape of molecules, and temperature

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9
Q

What are cohesive forces

A

IMFs between identical molecules (Ie. water to water)

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10
Q

What is surface tension

A

E required to increase surface area of a liquid

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11
Q

What are adhesive forces

A

IMFs between different molecules

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12
Q

Are adhesive or cohesive forces stronger

A

Adhesive

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13
Q

What is vapor pressure and its symbol

A

The pressure above a liquid at equilibirum in a closed system and vap sub P

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14
Q

What does vapor pressure depend on and what are the relationships

A

Disproportional to IMF strength and proportional to temperature

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15
Q

What is boiling point

A

T at which a liquid’s vapor pressure is equal to atmospheric pressure

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16
Q

What is the relationship between vapor pressure and boiling point

A

disproportional

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17
Q

What is enthalpy of vaporization and its symbol

A

Heat necessary to vaporize one mole of liquid and Vap sub delta H

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18
Q

What is enthalpy of fusion and its symbol

A

E needed to melt one mole of stuff and fus sub delta H

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19
Q

Enthalpy of fusion is always slighlty smaller of bigger than enthalpy of vaporization

A

Smaller

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20
Q

What is sublimation

A

solid to gas

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21
Q

What is deposition

A

gas to solid

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22
Q

What is the triple point

A

Point where all three phases exist

23
Q

What is the critical point

A

Point where liquid/gas boundry no longer exists

24
Q

Why is the phase diagram of water different from others and how is it different

A

Because water is heavier than ice is thus, it has a negative slope for the liquid/solid boundary

25
Q

What is an ionic crystalline solid

A

forms crystal lattice only between metals and nonmetals

26
Q

What is a metallic crystalline solid

A

“sea of electrons” between metals only

27
Q

What is a molecular crystalline solid

A

forms only between nonmetals

28
Q

What is a covalent network crystalline

A

atomic solids only

29
Q

What is the relationship between temperature and solubility of gases

A

Increase in temperature causes a decrease in solubility

30
Q

What are miscible liquids

A

liquids that are soluble in each other at all concentrations

31
Q

What are immiscible liquids

A

Liquids that are not soluble in each other

32
Q

What is the relationship between temperature and solubility of solids

A

Decrease in temperature causes a decrease in solubility

33
Q

What is osmotic pressure and its symbol

A

pressure that a solution can exert and its symbol is small pi

34
Q

What is equilibrium

A

State where the concentration of reactants and products is constant

35
Q

What happens when the equilibrium constant is one

A

Reaction favors neither side

36
Q

What happens when the equilibrium constant is greater than one

A

The reaction favors products

37
Q

What happens when the equilibrium constant is less than one

A

Reaction favors reactants

38
Q

What does the equilibrium constant depend on

A

temperature

39
Q

What is the reaction quotient and its symbol

A

Way to determine if a system is at equilibrium or not and Q

40
Q

What is the equilibrium constant and its symbols

A

Describes concentrations of a system at equilibrium and K sub eq K sub C or K

41
Q

If Q is bigger than K what happens

A

There are too many reactants so system shifts right

42
Q

If Q is smaller than K what happens

A

There are too many products so system shifts left

43
Q

What is le Chatelier’s principle

A

if a system is perturbed at equilibrium, it returns to equilibrium by counteracting perturbation

44
Q

When at equilibrium and K > 1 what is Gibb’s free energy?

A

Negative thus, spontaneous

45
Q

When at equilibrium and K = 1 what is Gibb’s free energy?

A

Zero

46
Q

When at equilibrium and K < 1 what is Gibb’s free energy?

A

Postive thus, non spontaneous

47
Q

When are Kc and Kp equal

A

When there are an equal number of moles of gas on both sides

48
Q

When gases are in standard states, what is their pressure

A

1 atm

49
Q

What is the london dispersion trend?

A

Increases as electrons increase

50
Q

What is the relationship between boiling point and IMF

A

Proportional

51
Q

What is the relationship between viscosity and IMF

A

Proportional

52
Q

What is the relationship between surface tension and IMF

A

proportional

53
Q

What is the relationship between pressure and solubility of a gas

A

Proportional

Chem 103 (5 decks)

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