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CHEM 120 SUMR'DONE > Unit 3: Ch 8, 10, 11 - Definitions & Equations > Flashcards

Unit 3: Ch 8, 10, 11 - Definitions & Equations Flashcards

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1
Q

covalent bonds are _ + _

A

nonmetals + nonmetals

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2
Q

covalent bonds in molecules are the sharing of

A

electrons between 2 ATOMS

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3
Q

A single bond is the sharing of

Length and strength:

A

2 bonding electrons; (1 pair)

longest and weakest

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4
Q

A double bond is the sharing of

Length and strength:

A

4 bonding elections; (2 pairs)

medium

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5
Q

A triple bond is the sharing of

Length and strength:

A

6 bonding elections; (3 pairs)

shortest and strongest

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6
Q

Intramolecular interactions are

A

inside molecules

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7
Q

Intermolecular interactions are

rhyme; inter-vene

A

between molecules

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8
Q

Electronegativity is the

The highest is

A

ability of an atom to attract electrons to itself

F!!!

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9
Q

An ionic interaction is the

A

Transfer of electrons

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10
Q

A polar covalent bond is the

A

Unequal-sharing of electrons

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11
Q

A nonpolar covalent bond is the

A

Equal-sharing of electrons

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12
Q

Bond polarity is found by the

A

difference between the 2 electronegativity values

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13
Q

Nonpolar molecules shapes are

slide 41

A

Symmetrical shape (NO lone pairs on central atoms with the exterior atoms all the SAME)

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14
Q

Polar molecules shapes are

slide 41

A
  1. Symmetrical geometry (NO lone pairs) with different exterior atoms all the SAME
  2. ANY combination of atoms with a NONsymmetrical geometry (lone pairs)
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15
Q

Dipole-Dipole Forces are present in (polar/nonpolar) molecules

A

polar

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16
Q

ionic compounds are _ + _

A

metal + nonmetal

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17
Q

Hydrogen bonding is (strength)

Present ONLY between molecules with _, _ and _ bonds

A

VERY STRONG

N-H, O-H, H-F bonds

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18
Q

London Forces are present in

A

Everything

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19
Q

Heat of Fusion is the

A

amount of heat needed to melt or freeze 1 g of a substance

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20
Q

Heat of Vaporization is the

A

amount of heat needed to boil/condense 1 g of a substance

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21
Q

Heat of Sublimation is the

A

same for sublimation and deposition

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22
Q

Equation for Heat of Fusion

A

Q = m•Hf

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23
Q

Equation for Heat of Vaporization

A

Q = m•HV

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24
Q 
For the heating curve
Q1 is
Q2 is
Q3 is 
Q4 is  
Q5 is
A 
Q1 - ice melting
Q2 - ice melting into water
Q3 - water heating
Q4 - water boiling into steam
Q5 - steam heating
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25
Q 
For the heating curve the equations for:
Q1 =
Q2 = 
Q3 = 
Q4 = 
Q5 =
A 
Q1 = mCpΔT
Q2 = mΔHfus
Q3 = mCpΔT
Q4 = mΔHvap
Q5 = mCpΔT
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26
Q

Dilute concentration is

A

solution that contains a small amount of solute

27
Q

Concentrated concentration is

A

solution contain a lot of solute

28
Q

Concentration is

A

the amount of solute present in a given amount of solvent or solution

29
Q

Percent by Mass =

A

% by mass = mass solute/mass solution • 100%

30
Q

Volume Percentage =

A

volume % = volume solute/mass solution • 100%

31
Q

Molarity =

A

Molarity = moles solute/moles solution

M=n/v

32
Q

Equation for dilution of solutions

A

C1V1=C2V2

33
Q

Ion-dipole forces

A

the interactions between ions and the dipoles of a polar molecule (like H2O)

34
Q

Ionic compound dissolving:
O (δ-) attracted to [charge] ions
H (δ+) attracted to [charge] ions

A

O (δ-) attracted to + ions

H (δ+) attracted to - ions

35
Q

MISCIBLE mixtures of 2 molecular (covalent) liquids are

A

two liquids that mix (solute and solvent)

e.g. alcohol and water

36
Q

IMMISCIBLE mixtures are

A

two liquids that DO NOT mix

e.g. oil and water

37
Q

Solubility is

A

maximum amt of solute that dissolves in a certain amount of solvent at a specific temperature

38
Q 
Polar compounds (dissolve/dissolve poorly)  in water 
Nonpolar compounds (dissolve/dissolve poorly)  in water
A

Polar compounds dissolve in water (because of dipole-dipole attractions)
Nonpolar compounds dissolve POORLY in water

39
Q

Solubility of solids/liquids

(increase/decrease) with (increasing/decreasing) temperature

A

Solubility of solids/liquids

increase with increasing temperature

40
Q

Solubility of solids/liquids

are (affected/unaffected) by pressure

A

Solubility of solids/liquids

are unaffected by pressure

41
Q

Solubility of gases

(increases/decreases) with (increasing/decreasing) temperature

A

Solubility of gases

decreases with increasing temperature

42
Q

Solubility of gases

(increases/decreases) with (increasing/decreasing) pressure

A

Solubility of gases

increases with increasing pressure

43
Q

Ionization is

A

dissolving SOLUBLE ionic compounds in WATER

44
Q

Electrolyte is a

A

compound that when dissolved causes the solution to conduct electricity

45
Q

A strong electrolytes conductivity is _
(High/low) # ions when dissolved
(High/low) concentration (#M) of ion

A

A strong electrolytes conductivity is good
High # ions when dissolved
High concentration (#M) of ion

46
Q

A weak electrolytes conductivity is _
(High/moderate/low) # ions when dissolved
(High/moderate/low) concentration (#M) of ions

A

A weak electrolytes conductivity is good
Moderate # ions when dissolved
Moderate concentration (#M) of ions

47
Q 
A nonelectrolytes conductivity is _
 #_ ions when dissolved
A

Insignificant

NO IONS WHEN DISSOLVED

48
Q

Colligative property is a

These properties are only for

A

Property that depends on the amount of particles in a solution (solute particles)

These properties are only for SOLUTIONS

49
Q

Adding a solute (increases/decreases) the vapor pressure

Higher # solute particles or higher #M = (higher/lower) vapor pressure

A

Adding a solute decreases the vapor pressure

Higher # solute particles or higher #M = lower v.p. (less escaping)

50
Q

The higher # solute particles or higher #M = (higher/lower) Boiling Point

A

Higher # solute particles or higher #M = higher b.p.

e.g. salt added to water for pasta

51
Q

The higher # solute particles or higher #M = (higher/lower) Freezing Point

A

Higher # solute particles or higher #M = higher f.p.

e.g. salting the roads

52
Q

Osmotic pressure (Π) is

Water flows from the _ to _ side

A

if pure water and dissolution are separated by a semipermeable membrane

Water flows from the solvent to solution side

53
Q

Higher # solute particles or higher #M = (higher/lower) Π

A

Higher # solute particles or higher #M = higher Π

54
Q

Isotonic solutions are

A

solutions with the SAME Π as another solution

55
Q

Hypotonic solutions have

A

lower Π than a particular solution

56
Q

Hypertonic solutions have

A

higher Π than a particular solution

57
Q

Collision theory is

A

the assumption that chemical reactions are caused by the collisions of molecules

58
Q 
Collisions with:
High temperature = _ reactions
High concentration = _ reactions
Large particles = _ surface area
More surface area = _ reactive
Larger the particles = _ reaction
A 
High temperature = faster reaction
High concentration = faster reactions
Large particles = small surface area
More surface area = more reactive
Larger the particles = slower reaction will proceed
59
Q

A reversible reaction is

Generally take place in _ phase

A

a reaction where both the forward (forming products) and backward (reforming reactants) rxns are possible

Generally take place in the SAME phase

60
Q

Increase pressure, shift to _ moles of gas

A

Increase pressure, shift to FEWER moles of gas

61
Q

Decrease pressure, shift to _ moles of gas

A

Decrease pressure, shift to MORE moles of gas

62
Q

Rxns that have a change in temperature are _ and _ is a product

A

Exothermic and HEAT is a product

63
Q

Equilibrium constant Keq =

A

Keq =
[C]c[D]d/
[A]a[B]b

CHEM 120 SUMR'DONE (9 decks)

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