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

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
``` For the heating curve the equations for: Q1 = Q2 = Q3 = Q4 = Q5 = ```
``` Q1 = mCpΔT Q2 = mΔHfus Q3 = mCpΔT Q4 = mΔHvap Q5 = mCpΔT ```
26
Dilute concentration is
solution that contains a small amount of solute
27
Concentrated concentration is
solution contain a lot of solute
28
Concentration is
the amount of solute present in a given amount of solvent or solution
29
Percent by Mass =
% by mass = mass solute/mass solution • 100%
30
Volume Percentage =
volume % = volume solute/mass solution • 100%
31
Molarity =
Molarity = moles solute/moles solution M=n/v
32
Equation for dilution of solutions
C1V1=C2V2
33
Ion-dipole forces
the interactions between ions and the dipoles of a polar molecule (like H2O)
34
Ionic compound dissolving: O (δ-) attracted to [charge] ions H (δ+) attracted to [charge] ions
O (δ-) attracted to + ions | H (δ+) attracted to - ions
35
MISCIBLE mixtures of 2 molecular (covalent) liquids are
two liquids that mix (solute and solvent) | e.g. alcohol and water
36
IMMISCIBLE mixtures are
two liquids that DO NOT mix | e.g. oil and water
37
Solubility is
maximum amt of solute that dissolves in a certain amount of solvent at a specific temperature
38
``` Polar compounds (dissolve/dissolve poorly) in water Nonpolar compounds (dissolve/dissolve poorly) in water ```
Polar compounds dissolve in water (because of dipole-dipole attractions) Nonpolar compounds dissolve POORLY in water
39
Solubility of solids/liquids | (increase/decrease) with (increasing/decreasing) temperature
Solubility of solids/liquids | increase with increasing temperature
40
Solubility of solids/liquids | are (affected/unaffected) by pressure
Solubility of solids/liquids | are unaffected by pressure
41
Solubility of gases | (increases/decreases) with (increasing/decreasing) temperature
Solubility of gases | decreases with increasing temperature
42
Solubility of gases | (increases/decreases) with (increasing/decreasing) pressure
Solubility of gases | increases with increasing pressure
43
Ionization is
dissolving SOLUBLE ionic compounds in WATER
44
Electrolyte is a
compound that when dissolved causes the solution to conduct electricity
45
A strong electrolytes conductivity is _ (High/low) # ions when dissolved (High/low) concentration (#M) of ion
A strong electrolytes conductivity is good High # ions when dissolved High concentration (#M) of ion
46
A weak electrolytes conductivity is _ (High/moderate/low) # ions when dissolved (High/moderate/low) concentration (#M) of ions
A weak electrolytes conductivity is good Moderate # ions when dissolved Moderate concentration (#M) of ions
47
``` A nonelectrolytes conductivity is _ #_ ions when dissolved ```
Insignificant | NO IONS WHEN DISSOLVED
48
Colligative property is a These properties are only for
Property that depends on the amount of particles in a solution (solute particles) These properties are only for SOLUTIONS
49
Adding a solute (increases/decreases) the vapor pressure Higher # solute particles or higher #M = (higher/lower) vapor pressure
Adding a solute decreases the vapor pressure Higher # solute particles or higher #M = lower v.p. (less escaping)
50
The higher # solute particles or higher #M = (higher/lower) Boiling Point
Higher # solute particles or higher #M = higher b.p. e.g. salt added to water for pasta
51
The higher # solute particles or higher #M = (higher/lower) Freezing Point
Higher # solute particles or higher #M = higher f.p. e.g. salting the roads
52
Osmotic pressure (Π) is Water flows from the _ to _ side
if pure water and dissolution are separated by a semipermeable membrane Water flows from the solvent to solution side
53
Higher # solute particles or higher #M = (higher/lower) Π
Higher # solute particles or higher #M = higher Π
54
Isotonic solutions are
solutions with the SAME Π as another solution
55
Hypotonic solutions have
lower Π than a particular solution
56
Hypertonic solutions have
higher Π than a particular solution
57
Collision theory is
the assumption that chemical reactions are caused by the collisions of molecules
58
``` Collisions with: High temperature = _ reactions High concentration = _ reactions Large particles = _ surface area More surface area = _ reactive Larger the particles = _ reaction ```
``` 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
A reversible reaction is Generally take place in _ phase
a reaction where both the forward (forming products) and backward (reforming reactants) rxns are possible Generally take place in the SAME phase
60
Increase pressure, shift to _ moles of gas
Increase pressure, shift to FEWER moles of gas
61
Decrease pressure, shift to _ moles of gas
Decrease pressure, shift to MORE moles of gas
62
Rxns that have a change in temperature are _ and _ is a product
Exothermic and HEAT is a product
63
Equilibrium constant Keq =
Keq = [C]c[D]d/ [A]a[B]b