Tables

Question 1

Table 4.2: Strong and weak acids and bases.

Answer 1

Strong acids: Hydrochloric acid (HCl), Hydrobromic acid (HBr), Hydriodic acid (HI), Nitric acid (HNO3), Sulfuric acid (H2SO4), Perchloric acid (HClO4)
Weak acids: Hydrofluoric acid (HF), Phosphoric acid (H3PO4), Acetic acid (CH3COOH or HC2H3O2)
Strong bases: Group 1A(1) hydroxides: Lithium hydroxide (LiOH), Sodium hydroxide (NaOH), Potassium hydroxide (KOH), Rubidium hydroxide (RbOH), Cesium hydroxide (CsOH), Heavy Group 2A(2) hydroxides: Calcium hydroxide (Ca(OH)2), Strontium hydroxide (Sr(OH)2), Barium hydroxide (Ba(OH)2).
Weak bases: Ammonia (NH3)

Question 2

Table 4.1: Solubility rules for ionic compounds in water.

Answer 2

Soluble Ionic Compounds

1. All common compounds of Group lA(1) ions (Li+, Na+, K+, etc.) | (exceptions) None
2. All common compounds of ammonium ion (NH4+) | None
3. All common nitrates (NO3-), acetates (CH3COO- or C2H3O2-), and perchlorates (ClO4-) | None
4. All common chlorides (Cl-), bromides (Br-), and iodides (I-) | Chlorides, bromides, and iodides of Ag+, Pb(2+), Cu+, and Hg2(2+)
5. All common fluorides (F-) | PbF2 and fluorides of Group 2A(2)
6. All common sulfates (SO4(2-)) | CaSO4, SrSO4, BaSO4, Ag2SO4, PbSO4

Insoluble Ionic Compounds

1. All common metal hydroxides | Group 1A(1) hydroxides and Ca(OH2), Sr(OH)2, and Ba(OH)2
2. All common carbonates (CO3(2-)) and phosphates (PO4(3-)) | Carbonates and phosphates of Group 1A(1) and NH4+
3. All common sulfides | Sulfides of Group 1A(1), Group 2A(2), and NH4+

Question 3

Table 1.3 Meaning of the following prefixes: hecto, deka, mega, milli, pico, tera, femto, nano, micro, giga, kilo, deci, centi.

Answer 3

tera (T) 10¹²
giga (G) 10⁹
mega (M) 10⁶
kilo (k) 10³
hecto (h) 10²
deka (da) 10
-
deci (d) 10⁻¹
centi (c) 10⁻²
milli (m) 10⁻³
micro (μ) 10⁻⁶
nano (n) 10⁻⁹
pico (p) 10⁻¹²
femto (f) 10⁻¹⁵

Question 4

Table 1.4 Common SI-English equivalent quantities:
1 mile = _ km
1 in = _ cm
1 kg = _ lb

Answer 4

1. 1.609
2. 2.54
3. 2.205

Question 5

Table 2.3 Common monatomic ions. List the formulas for the following: barium, calcium, hydrogen, lithium, zinc, magnesium, sodium, strontium, potassium, aluminum, cadmium, cesium, silver.

Give the formulas for the following: hydride, fluoride, chloride, bromide, iodide, oxide, sulfide, nitride.

Answer 5

Ba²⁺, Ca²⁺, H⁺, Li⁺, Zn²⁺, Mg²⁺, Na⁺, Sr²⁺, K⁺, Al³⁺, Cd²⁺, Cs⁺, Ag⁺

H⁻, F⁻, Cl⁻, Br⁻, I⁻, O²⁻, S²⁻, N³⁻

Question 6

Table 2.4 List the common charge states for the following: Cr, Co, Cu, Fe, Pb, Hg, Sn

Associate the trivial names with a charge state: chromous, chromic, cupric, cuprous, mercurous, mercuric, stannous, stannic, ferric, ferrous.

Answer 6

Cr: 2, 3. Co: 2, 3. Cu: 1, 2. Fe: 2, 3. Pb: 2, 4. Hg: 1 (as Hg₂²⁺), 2. Sn: 2, 4.

2, 3, 2, 1, 1, 2, 2, 4, 3, 2.

Question 7

Table 4.4 Rules for assigning oxidation numbers

Answer 7

General rules:
1. For an atom in its elemental form (Na, C, or O2) ON = 0
2. For a monatomic ion: ON = ion charge
3. Sum of ON values for the atoms in a molecule or formula unit equals 0.
Specific boys:
1. Group 1: +1 in compounds
2. Group 2: +2 in all compounds
3. H: +1 in combination with nonmetals, -1 in combination with metals and boron
4. F: -1 in all compounds
5. O: -1 in peroxides, -2 in everything else except with F.
6. Group 7: -1 in combination with metals, nonmetals (except O), and other halogens lower in the group.