Discussion Quiz 2

Question 1

Neutralization Reactions:

Answer 1

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

Question 2

The net ionic equation for strong acid – strong base:

Answer 2

H+ (aq) + OH−(aq) → H2 O(l)

Question 3

Driving force for neutralization

Answer 3

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

Question 4

Gas Forming Reactions:

Answer 4

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)

Question 5

Redox reactions

Answer 5

involve a species which is oxidized and another that is reduced

Question 6

Redox Reactions example:

Answer 6

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

Question 7

Oxidation and Reduction Reactions

Answer 7

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

Question 8

Coulomb’s Law/ Potential Energy Results:

Answer 8

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

Question 8

Why do salts dissolve in water?

Answer 8

Solvation Energy is greater than Lattice Energy

Question 8

Coulomb’s Law

Answer 8

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

Question 8

Solvation Energy

Answer 8

Energy of
attractions between ions and
water.

Question 9

Lattice Energy

Answer 9

Energy of attractions between cations
and anions in salt lattice

Question 10

Driving Force of Precipitation Reactions:

Answer 10

The driving force is the formation of an insoluble solid

Question 11

Energy Involved
in Salts Dissolving In Water

Answer 11

• 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).

Question 12

Strong Acids

Answer 12

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

Question 13

Weak Acids

Answer 13

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

Question 14

Strong Bases

Answer 14

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

Question 15

Weak Bases

Answer 15

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

NH3 ammonia

Question 16

Cation

Answer 16

Positively Charged Ion

Question 17

Anion

Answer 17

Negatively Charged Ion

Question 18

Polyatomic Ions

Answer 18

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−

Question 19

Naming Binary Molecular Compounds

Answer 19

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

Question 20

Binary Molecular Compound Prefixes

Answer 20

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