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Review Flashcards

(50 cards)

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1
Q

6 Common Strong Acids

A

HCl (hydrochloric acid)

HBr (hydrobromic acid)

HI (hydroiodic acid)

HNO3 (nitric acid)

H2SO4 (sulfuric acid)

HClO4 (perchloric acid)

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2
Q

6 Common Strong Bases

A

LiOH (lithium hydroxide)

NaOH (sodium hydroxide)

KOH (potassium hydroxide)

Ca(OH)2 (calcium hydroxide)

Sr(OH)2 (strontium hydroxide)

Ba(OH)2 (barium hydroxide)

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3
Q

Strong acids have what kind of base?

A

Weaker but more stable

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4
Q

Strong acids ______ __________ when dissolved in water

A

ionize completely

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5
Q

Bronsted-Lowry Acid

A

Proton Donor

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6
Q

Bronsted-Lowry Base

A

Proton Acceptor

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7
Q

Lewis Acid

A

Electron Pair Acceptor

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8
Q

Lewis Base

A

Electron Pair Donor

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9
Q

Strong acids are what?

A

molecular compound

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10
Q

Strong bases are what?

A

ionic compounds

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11
Q

Proton

A

H+

Cation

1 proton

0 electrons

positive

Acid

1s0

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12
Q

Hydrogen Atom

A

H

Atom

0 Nutrons

1 proton

1 electrons

Neutral

LIKE radical

1s1

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13
Q

Hydride Ion

A

H-

Anion

1 proton

2 electrons

negative

base

1s2

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14
Q

What are intermolecular forces

A

force that mediates interaction BETWEEN molecules

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15
Q

3 types of IMF

A

Weakest: Dispersion Forces

Dipole-Dipole Interaction

Strongest: Hydrogen bonding

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16
Q

What are intramolecular forces

A

interactions WITHIN 1 molecule of a substance

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17
Q

Dispersion Forces

A

“Temporary” attractive forces resulting from instantaneous, momentary, transient, induced dipoles

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18
Q

Dipole-Dipole Interactions

A

Electrostatic forces between partially (+) end of one polar molecule and the partially (-) end of another molecule; results from permanent dipoles

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19
Q

Hydrogen Bonding

A

Occurs between a hydrogen atom bound to a small electronegative atom and a lonepair of electrons on another small electronegative atoms (N, O, F)

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20
Q

Most volatile (fumes/gas)

A

escape liquid phase to gas
lowest boiling point

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21
Q

highest boiling point

Study These Flashcards
A

means strongest intermolecular forces (least volatile)

22
Q

Solution

Study These Flashcards
A

Solute in the solvent

23
Q

Solute

Study These Flashcards
A

Substance dissolved in solvent

24
Q

Solvent

Study These Flashcards
A

Substance in which the solute is dissolved

25
Miscible Liquids
Mix to form homogeneous solution
26
Immiscible Liquids
Don't mix, heterogeneous mix, different polarities
27
Characteristics of Solutions
Homogeneous; uniform composition State of solution typically same as solvent Solution particles dispersed among solvent particles Dissolved particles will not seperate from solution Concentration can be varied within limits
28
Alloys
Solid solutions of different metals dissolved in another metal
29
Air
gaseous solution of O, N, etc
30
Rubbing Alc
Solution of H2O in isopropanol is a liquid
31
Enthalpy
Heat of reaction absorbed or evolved
32
Nonelectrolytes
Not ionized when dissolved in water Not form conduction solution
33
Electrolytes
Ionize when dissolved in water Strong Acid, Strong Bases
34
Strong Electrolytes
Ionize completely when dissolved in water Form strongly conduction solution Strong Acids, Strong Bases
35
Weak Electrolytes
Ionize incompletely when dissolved in water Form weakly conduction solution Weak Acids, Weak Bases
36
Solubility
Max concentration that can be achieved under given conditions when the dissolution process is at equilibrium
37
Saturated Solution
Solute's concentration = solubility
38
Unsaturated Solution
Solute's concentration is less than solubility
39
Dilute Solution
Low solute concentration
40
Concentrated Solution
High solute concentration
41
Supersaturated Solution
Solute concentration is higher than solubility (by heating a solution)
42
Miscible Liquids
Have infinite mutual solubility Can be mixed in any proportions to yields solutions Have similar polarities
43
Immiscible Liquids
Do not mix to a great degree Form separate layers when placed in the same container
44
Partially miscible liquids
Have moderate mutual solubility Two layers form but each layer is saturated with the other substance
45
Solubility of a solid in a liquid tends to do what with temperature
increase
46
Molarity
chemical amount(mol) / Volume of solution (L)
47
Mole Fraction
Moles of A / Total moles
48
Molality
mol solute / Kg solvent (mass of solvent
49
Raoult's Law
Partial pressure exerted by any component of an ideal solution is equal to the vapor pressure of that component multiplied by its mole fraction in the solution
50
Vapor Pressure
Pressure exerted by a gaseous phase when vaporization and condensation are at equilibrium or are occurring at the same rate

Chem 2 (3 decks)

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