Basic Chemistry - Final Notes

Charge 1+

Name Ammonium

NH

Hydronium

H30+

Bicarbonate

HCO3−

Bisulfate

HSO4−

Acetate

1−

Formula + 4

CH3CO2− or

C2H3O2−

Nitrite

NO2−

Nitrate

NO

Cyanide

CN−

Hydroxide

OH−

Dihydrogen phosphate

H2PO4−

− 3

Permanganate MnO4−

2−

3−

Carbonate

CO32−

Sulfate

SO42−

Hydrogen phosphate

HPO42−

Oxalate

C2O42−

Dichromate

Cr2O

Phosphate

PO43−

2− 7

Metal Li K Ca Na Mg Al Zn Cr Fe Cd Ni Sn Pb H2 Cu Ag Hg Au

Oxidized Li+ + e− K+ + e− Ca2+ + 2e− Na+ + e− Mg2+ + 2e− Al3+ + 3e− Zn2+ + 2e− Cr3+ + 3e− Fe2+ + 2e− Cd2+ + 2e− Ni2+ + 2e− Sn2+ + 2e− Pb2+ + 2e− 2H+ + 2e− Cu2+ + 2e− Ag+ + e− Hg2+ + 2e− Au3+ + 3e−

Acid

Equilibrium Reaction H2O ↔ H+ + OH– Inorganic Acids Nitrous acid HNO2 ↔ H+ + NO2– Hydroflouric acid HF ↔ H+ + F– Hypochlorous acid HOCl ↔ H+ + OCl– Hypobromous acid HOBr ↔ H+ + OBr– Hydrocyanic acid HCN ↔ H+ + CN– Carboxylic Acids Chloroacetic acid CH2ClCOOH ↔ H+ + CH2ClCOO– Formic acid HCOOH ↔ H+ + HCOO– Benzoic acid C6H5COOH ↔ H+ + C6H5COO– Acetic acid CH3COOH ↔ H+ + CH3COO– Inorganic Bases Ammonia NH3 + H2O ↔ NH4+ + OH– Hydrazine H2NNH2 + H2O ↔ H2NNH3+ + OH– Hydroxylamine HONH2 + H2O ↔ HONH3+ + OH– Amines Dimethylamine (CH3)2NH + H2O ↔ (CH3)2NH2+ + OH– Ethylamine CH3CH2NH2 + H2O ↔ CH3CH2NH3+ + OH– Methylamine CH3NH2 + H2O ↔ CH3NH3+ + OH– Pyridine C5H5N + H2O ↔ C5H5NH+ + OH– Aniline C6H5NH2 + H2O ↔ C6H5NH3+ + OH–

Reacts With

Water

Cold water, steam, or acids.

Steam or acids.

Acids.

Does not react with acids.

Table 3—Metal Activity (283) Equilibrium Constant Expression: c

K=

d

[C] ×[ D ] [ A]a ×[B] b

K a=

[ H ]×[ salt] [ acid ]

ò

ò

ò

ò

Acid Name

Anion

hydro__ic acid

__ide

hypo__ous acid

hypo__ite

__ous acid

__ite

__ic acid

__ate

per__ic acid

per__ate

Table 5—Naming

bcc: Fe, K, Na & W fcc: Al, Cu, Pb & Ag

Name 1 mol of any gas at 1 atm & 0°C (STP) Hydrochloric acid [salt ] occupies Sulfuric acid pH =−log K a log  [acid ] 22.4L Sodium hydroxide Sodium chloride • Oxidizing agents: O2, H2O2, K2Cr2O7 Calcium nitrate (alcohols), KMnO4, antiseptics Acetic acid • Reducing agents: coal (C), metals, H, Ammonia photo developer, antioxidants Methylamine electrode charge reaction electroplate Methyl alcohol cathode negative reduction spoon Ethyl alcohol Sucrose anode positive oxidation silver bar

1.4 x 10-3 1.8 x 10-4 6.3 x 10-5 1.8 x 10-5 1.8 x 10-5 8.5 x 10-7 9.1 x 10-9 5.9 x 10-4 4.3 x 10-4 4.2 x 10-4 1.5 x 10-9 4.2 x 10 -10

Formula

Type

HCl Strong acid H2SO4 Strong acid NaOH Strong base NaCl Salt Ca(NO3)2 Salt CH3COOH Weak acid NH3 Weak base CH3NH2 Weak base CH3OH Mol. liquid CH3CH2OH Mol. liquid C12H22O11 Mol. solid

Elec. Cond. Strong Strong Strong Strong Strong Weak Weak Weak None None None

Table 4—Some Electrolytes (274)

Intermolecular Melt. Elec. Particles Forces Point Cond. (l) Ionic Crystals Electrostatic / Ions High High Ionic (v strong) Covalent Network Crystals Covalent bonds Do not Atoms N/A (very strong) melt Metallic Crystals Positive ions & Metallic bonds Very High mobile electrons (very strong) High Molecular Crystals Hydrogen-bonded Molecules w/ H Hydrogen bonds Interm Very Low on N, O or F (interm) Polar Polar molecules Dipole forces Low Very Low w/o H bonds (weak) Nonpolar Atoms / nonpolar Dispersion forces Very Very molecules only (very weak) Low Very Low Table 6—Crystalline Solids

03/03/10

7.2 x 10-4 6.6 x 10-4 2.9 x 10-8 2.5 x 10-9 6.2 x 10 -10

Table 2—Ionization Data (255-6)

Definition of pH & pOH:

pH =−log[ H ] pOH =−log[OH ] Table 1—Polyatomic Ions (90) Oxidation: gain O, lose H, or lose e – Henderson-Hasselbalch Equation: Reduction: lose O, gain H, or gain e – O2

Ka/b/w 1.0 x 10 -14

Characteristics / Examples

Spec Heat

cal  g⋅° C

Al Cu Hard, polarsoluble; NaCl C2H5 OH Fe Very hard, insoluble; diamond HOC2 H4OH Insoluble malleable Mg conductors; Cu, Zn Hg S8 H2O Fragile; H2O, HF, NH3

0.216 0.0921

Fragile, soluble; HCl, H2S Soft, very soluble; Ar, H2, I2, CO2

• •

0.588 0.106 0.561

• • • • • •

0.245 • 0.0332 0.169 1.000 •

Strong acids Hydrochloric acid (HCl)

Boyle's Law

Hydrobromic acid (HBr)

Charles's Law

V 1 /T 1 =V 2 / T 2

Avogadro's Law

V 1 /n1 =V 2 /n 2

Combined Gas Law

P 1V 1 P 2 V 2 = T1 T2

Ideal Gas Law

PV =nRT

Hydriodic acid (HI) Nitric acid (HNO3) Sulfuric acid (H2SO4) Perchloric acid (HClO4) Strong bases Alkali metal hydroxides: LiOH, NaOH, KOH, RbOH, CsOH Alkaline earth metal hydroxides: Ca(OH) 2, Sr(OH)2, Ba(OH)2

1 atm = 101.325 kPa = 29.921 inHg = 760 torr = 760 mmHg = 14.696 lb/in 2 1 cal = 4.184 J

P1 V 1 =P 2 V 2

R=.0821 Acid

L⋅atm mol⋅K

Base

Salt

Strong Strong Neutral Strong

Weak

Acidic

•

° C=° F−32 /1.8 ° F =° C⋅1.832

Weak

Strong

Basic

•

Specific Gravity= D substance / D water

Weak

Weak

Any

•

∆ Heat=mass⋅specific heat⋅∆T

Note Sheet for Lecture Final

Table 7—Salts (257)

Jerry Goure