Discussion Quiz 2 Flashcards

1
Q

Neutralization Reactions:

A

Special type of acid-base reaction
acid + base → salt + H2O(l)

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2
Q

The net ionic equation for strong acid – strong base:

A

H+ (aq) + OH−(aq) → H2 O(l)

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3
Q

Driving force for neutralization

A

formation of H2O, which has
very strong O-H bonds

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4
Q

Gas Forming Reactions:

A

Carbonates, sulfites, and sulfides react with acids:
CaCO3 (s) + 2 HCl(aq) → CaCl2 (aq) + H2O(l) + CO2 (g)

CaSO3 (s) + 2 HCl(aq) → CaCl2 (aq) + H2 O(l) + SO2 (g)

Na2S(s) + 2 HCl(aq) → 2 NaCl(aq) + H2 S(g)

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5
Q

Redox reactions

A

involve a species which is oxidized and another that is reduced

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6
Q

Redox Reactions example:

A

Cu2+ + Zn&raquo_space; Zn2+ + Cu
Cu 2+ is reduced to Cu. Cu 2+ is the oxidizing
agent. Redox is a battle for electrons.
24

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7
Q

Oxidation and Reduction Reactions

A

LEO says GER:
Loss of electrons: Oxidation
Gain of electrons: Reduction

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8
Q

Coulomb’s Law/ Potential Energy Results:

A

+/− attraction > +/+ and −/− repulsion

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8
Q

Why do salts dissolve in water?

A

Solvation Energy is greater than Lattice Energy

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8
Q

Coulomb’s Law

A

Potential = U = constant × (Q1Q2)/d
Q1: charge on cation Q2: charge on anion
d: distance between
the ions

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8
Q

Solvation Energy

A

Energy of
attractions between ions and
water.

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9
Q

Lattice Energy

A

Energy of attractions between cations
and anions in salt lattice

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10
Q

Driving Force of Precipitation Reactions:

A

The driving force is the formation of an insoluble solid

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11
Q

Energy Involved
in Salts Dissolving In Water

A
  • Breaking bonds requires energy (endothermic),
    such as disrupting ion-ion attractions in lattice.
    Coulomb’s Law predicts Lattice Energy

-Forming bonds releases energy (exothermic),
such as forming ion-water attractions
Solvation Energy

-The identity of the salt determines the magnitude of these energy changes and whether that salt is soluble in water (or not).

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12
Q

Strong Acids

A

Completely Ionize in Water
HBr hydrobromic acid
HCl hydrochloric acid
HI hydroiodic acid
HNO3 nitric acid
HClO4 perchloric acid
H2SO4 sulfuric acid

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13
Q

Weak Acids

A

Partially Ionize in Water
CH3COOH acetic acid
H2CO3 carbonic acid
H3PO4 phosphoric acid

14
Q

Strong Bases

A

Completely Ionize in Water
LiOH lithium hydroxide
NaOH sodium hydroxide
KOH potassium hydroxide
Ca(OH) 2 calcium hydroxide
Sr(OH) 2 strontium hydroxide
Ba(OH) 2 barium hydroxide

15
Q

Weak Bases

A

Weak bases leave a majority of dissolved base intact
and only generate a small number of hydroxide ions.:

NH3 ammonia

16
Q

Cation

A

Positively Charged Ion

17
Q

Anion

A

Negatively Charged Ion

18
Q

Polyatomic Ions

A

ammonium (NH4)+
hydronium (H3O)+
hydroxide (OH)−
acetate *CH3COO)−
nitrate (NO3)−
permanganate (MnO4)−
hydrogen carbonate (HCO3) −
carbonate (CO3) 2−
hydrogen sulfate (HSO4)−
sulfate (SO4) 2−
phosphate (PO4) 3−

19
Q

Naming Binary Molecular Compounds

A

Binary Compounds contain 2 different non-metal elements :
Name elements in formula order (the 2nd element’s name ends in “ide”
-prefixes show the number of each atom present

20
Q

Binary Molecular Compound Prefixes

A

1 -Mono
2 -Di
3 -Tri
4 -Tetra
5 -Penta
6 -Hexa
7 -Hepta
8 -Octa
9 -Nona
10 -Deca