Chem 106 Final Exam

Front 1

more readily form pi bonds

Back 1

first element of each group

Front 2

making hydrogen

Back 2

Strong acid and metal
Methane and water
Carbon and Water at 1000 C
Electrolysis of water
Electrolysis of brine

Front 3

Strong acid and metal

Back 3

2M+2HX->2MX+H2

Front 4

Methane and water

Back 4

CH4+H2O->3H2+CO
CO+H2O->CO2+H2

Front 5

Carbon and Water at 1000 C

Back 5

C+H2O->CO+H2

Front 6

Electrolysis of water

Back 6

2H2O->2H2+O2

Front 7

Electrolysis of brine

Back 7

NaCl+H2O->NaOH+Cl2+H2

Front 8

Halogens are good reductants or oxidants?

Back 8

Oxidants

Front 9

Hydrogen Isotopes

Back 9

Protium 1/1H
Deuterium 2/1H
Tritium 3/1H

Front 10

How noble gases form compounds

Back 10

Unfilled d-orbitals

Front 11

How do inner halogen compounds react

Back 11

oxidizes the anions of the halogens below it on the periodic table
Br2 +2I- -> 2Br - +I2

Front 12

Are inner halogen compounds reactive?

Back 12

yes highly reactive

Front 13

How to make halogen hydrides
including exceptions

Back 13

salt + H2SO4 -> H-halide + XSO4
exceptions: I, Br
use H3PO4 instead

Front 14

How to make oxygen

Back 14

Photosynthesis:
CO2+H2O+light -> C6H12O6 + 6O2
Lab prep
KClO3 -> KCl + O2

Front 15

Naming oxyacids

Back 15

HClO hypo- -ous +1
HClO2 -ous +3
HClO3 -ic +5
HClO4 per- -ic +7

Front 16

Nonmetal reactivity
Metal reactivity

Back 16

Nonmetals form covalent oxides
Most metals form ionic oxides

Front 17

Peroxides

Back 17

H2O2
-1 Oxidation state

Front 18

Superoxides

Back 18

NaO2
-1/2 Oxidation state

Front 19

Ostwald process

Back 19

4 NH3 (g) + 5 O2 (g) -> 4 NO (g) + 6 H2O (g)
2 NO (g) + O2 -> 2 NO2 (g)
2 NO2 (g) + H2O (l) -> 2 H+ + 2 NO3- (aq) + NO (g)

Front 20

Ammonia with bleach

Back 20

NH3 + OCl- -> NH2Cl

Front 21

PCl3
PCl5

Back 21

P+Cl2 -> PCl3
PCl3+ Cl2 -> PCl5

Front 22

CO2 production

Back 22

Carbon combustion
C (s) + O2 (g) -> CO2 (g)
Baking
Solubility in water

Front 23

Baking- CO2 production

Back 23

NaHCO3 (s) + H+ (aq) -> Na+ (aq) + CO2 (g) + H2O (l)

Front 24

Solubility in water- CO2 production

Back 24

CO2 (g) + H2O (l) -> H2CO3 (aq)

Front 25

Carbonate reactivity

Back 25

Dissolving minerals with acids:
CaCO3 (s) + 2 H+ (aq) -> Ca2+ (aq) + H2O (l) + CO2 (g)

Front 26

Metallurgy

Back 26

the science of extracting metals from their natural sources and preparing them for practical use.

Front 27

pyrometallurgy

Back 27

add heat
using heat to alter minerals to reduce metals.

Front 28

electrometallurgy

Back 28

use of electric and electrolytic processes to purify metals or reduce metallic compounds to metals.

Front 29

hydrometallurgy

Back 29

Using aqueous reactions to extract metal

Front 30

blast furnace

Back 30

Iron oxide ores in
Coke (carbon) = fuel
Limestone facilitates slag

Front 31

Calcination –

Back 31

using heat to release volatiles
PbCO3(s) -> PbO(s) + CO2(g)

Front 32

Roasting –

Back 32

using heat and reducing gases
PbO(s) + CO(g) -> Pb(l) + CO2(g)

Front 33

Smelting
equation

Back 33

Process of producing molten metal & slag
CaO (i) + SiO2 (l) -> CaSiO3 (l)

Front 34

Slag

Back 34

molten silicate materials

Front 35

Down's cell

Back 35

liquid Na, gaseous Cl2

Front 36

Hall Process

Back 36

makes molten aluminum
electrometallurgy

Front 37

Electron-Sea Model

Back 37

Metals can be thought of as cations suspended in a “sea” of valence electrons.
Attractions hold electrons near cations, but not so tightly as to impede their flow.

Front 38

3 types of magnetism

Back 38

diamagnetism
paramagnetism-unpaired d electrons
ferromagnetism-iron

Front 39

alloy

Back 39

mixtures of two metals