memorize aice chem

(ch. 16) halogenoalkane + aqueous alkali

• nucleophilic substitution

• product: alcohol

(ch. 16) Hydrolysis of halogenoalkane

• Halogenoalkane + aqueous AgNO3

• the water in the silver nitrate solution acts as the nucleophile, forming alcohol

• can be used to test for halides: F (colorless) Cl (white solid) Br (cream solid) I (yellow solid)

(ch. 16) cyanide ions (CN-) in ethanol + halogenoalkane

• nucleophilic substitution

• reflux

• an extra carbon atom is added to the original halogenoalkane chain

(ch. 16) halogenoalkane + ammonia (NH3)(in ethanol)

• nucleophilic substitution

• Heated

• product: amine

(ch. 16) halogenoalkane + OH (ethanol)

• elimination

• products: alkene + HX

(ch. 17) combustion of alcohol

alcohol + oxygen —> carbon dioxide + water

(ch. 17) alcohol + HX

• nucleophilic substitution

• reflux

• products: halogenoalkane + water

• some reagents create gaseous HCl (misty fumes)

(ch. 17) reagents for nucleophilic substitution to form a halogenoalkane

• SOCl2 ( —> HCl)

• PCl5 (—> HCl)

• PCl3 ( + heat)

• PI3

• PBr3

(ch. 17) alcohol + Na (metal)

• products: sodium alkoxide + hydrogen

(ch. 17) primary alcohol oxidation

• products: aldehyde —> carboxylic acid

• reflux

• turns green

(ch. 17) secondary alcohol oxidation

• products: ketone

• reflux

• turns green

(ch. 17) tertiary alcohol oxidation

• No reactions

• turns orange

(ch. 17) alcohol passed over a hot catalyst

• elimination/dehydration

• products: alkene, water

• cats: Al2O3, Conc. H2SO4 + heat, P4O10, Conc. H3PO4 + heat, Pumice

(ch. 17) alcohol + carboxylic acids, with acid catalyst

• esterification

• products: water, ester

• heated under reflux with a concentrated strong acid

• reversible reaction

(ch. 17) hydrolysis of ester - acid hydrolysis

ester + water + (acid cat.)

• products: carboxylic acids, alcohol

• reversible

• both products & reactants are still present after the reaction

(ch. 17) hydrolysis of ester - base hydrolysis

ester + soluble base

• products: sodium salt of carboxylic acids, alcohol

• not reversible

(ch. 17) ketone reduction

• reducing agent: LiAlH4 or NaBH4

• product: secondary alcohol

(ch. 17) carboxylic acid reduction

• reducing agent: LiAlH4

• dry ether, room temperature

• product: primary alcohol

(ch. 17) aldehyde reduction

• reducing agent: LiAlH4, NaBH4

• product: alcohol

(ch. 15) Nitrogen oxides released in exhaust fumes - equation

N2 + O2 —> 2NO

(ch. 15/ch. 13) reactions in a catalytic converter

• the oxidation of carbon monoxide to form carbon dioxide

• the reduction of nitrogen oxides to form harmless nitrogen gas

• the oxidation of unburnt hydrocarbons to form carbon dioxide and water

(ch. 15) substitution reactions of alkanes - initiation step

Cl2 —> (UV light) 2Cl*

(ch. 15) substitution reactions of alkanes - propagation steps

CH3 + Cl2 —> CH3Cl + Cl*

(ch. 15) Substitution reactions of alkanes - termination step

CH3 + Cl* —> CH3Cl

(ch. 15) alkene + H2

• heat

• cat: Ni, Pd, Pt

• product: alkane

• used to manufacture margarine

(ch. 15) alkene + steam/H2O (g)

• heat

• cat: phosphoric acid (H3PO4)

• product: alcohol

(ch. 15) alkene + HX

• room temp

• electrophilic addition

• product: halogenoalkane

(ch. 15) alkene + X2 (aq)

• inert solvent & room temp

• electrophilic addition

• product: halogenoalkane

markovnikov’s rule

when compound HX is added to an unsymmetrical alkene, the hydrogen becomes attached to the carbon with the most hydrogens attached to it already

(ch. 15) oxidation of alkene with cold, dilute MnO4

• purple color of solution disappears

• Diol is formed

(ch. 15) oxidation of alkene with hot, concentrated manganate solution

product depends on what is bonded to the carbon atoms in the double bond

• Carbon with 2 hydrogens —> CO2

• Carbon with 1 hydrogen & 1 R group —> Carboxylic acid

• Carbon with 2 R groups —> ketone

(ch. 15) conditions for substitution reactions of alkane - free radical substitution mechanism

UV light

(ch. 13) NO2 catalyzing the oxidation of SO2 in the making of acid rain

SO2 + NO2 —> SO3 + NO

(ch. 13) NO2 is regenerated as NO reacts w/ oxygen in the atmosphere

NO + ½ O2 —> NO2

(ch.13) SO3 reacting with water to cause acid rain

SO3 + H2O —> H2SO4

(ch. 12) color of F2

pale yellow

(ch. 12) color of Cl2

green/yellow

(ch. 12) color of Br2

orange/brown

(ch. 12) color of I2

grey/black solid, purple vapor

(ch. 12) trend of melting point and boiling points of the halogens

Increases going down the group

(ch. 12) volatility

the ease at which the halogens evaporate

(ch. 12) volatility trend of the halogens + why

decreases down the group, because a greater number of e- = greater chance for induced dipoles = stronger the van der Waals forces

(ch. 12) reactivity trend of the halogens

decreases down the group

(ch. 12) chlorine in cold alkali

Cl2 + 2NaOH —> NaCl + NaClO + H2O

(ch. 12) chlorine in hot alkali

3Cl2 + 6NaOH —> 5NaCl + NaClO3 + 3H2O

(ch. 12) Cl ion (NaCl) reaction with sulfuric acid (reaction + observations)

• NaCl + H2SO4 —> NaHSO4 + HCl

• HCl produces misty white fumes

(ch. 12) Br ion (NaBr) reaction with sulfuric acid (reaction (two parts) + observations)

• initial reaction: NaBr + H2SO4 —> NaHSO4 + HBr

• oxidation of HBr: 2HBr + H2SO4 —> Br2 + SO2 + 2H2O

• HBr produces misty white fumes

• Br produces a reddish brown gas

(ch. 12) I ion (NaI) with sulfuric acid, and subsequent oxidations (reaction + observation)

• Initial reaction: NaI + H2SO4 —> NaHSO4 + HI

• oxidation of HI:

  • 2HI + H2SO4 —> I2 + SO2 + 2H2O

  • 6HI + H2SO4 —> 3I2 + S(s) + 4H2O

  • 8HI + H2SO4 —> 4I2 + H2S + 4H2O

• Sulfur is a yellow solid

• Hydrogen sulfide (H2S) has a strong smell of bad eggs

• Iodine is a purple gas

• HI produces misty white fumes

(ch. 12) chlorine:

1. color of silver halide precipitate on addition of silver nitrate solution

2. effect on precipitate of adding dilute ammonia solution

3. effect on precipitate of adding concentrated ammonia solution

1. white

2. dissolves/colorless

3. still dissolved/colorless

(ch. 12) bromide:

1. color of silver halide precipitate on addition of silver nitrate solution

2. effect on precipitate of adding dilute ammonia solution

3. effect on precipitate of adding concentrated ammonia solution

1. cream

2. remains cream

3. dissolves

(ch. 12) Iodide:

1. color of silver halide precipitate on addition of silver nitrate solution

2. effect on precipitate of adding dilute ammonia solution

3. effect on precipitate of adding concentrated ammonia solution

1. pale yellow

2. remains pale yellow

3. remains pale yellow

(ch. 12) bleach components

NaCl & NaClO

(ch. 12) oxidizing agent power down the halogen group

decreases down the group

(ch. 11) color of Mg during flame test

bright white

(ch. 11) color of Ca during flame test

brick red

(ch. 11) color of Sr during flame test

scarlet red

(ch, 11) color of Ba during flame test

apple green

(ch. 11) CaO reaction with water

• CaO(s) + H2O(l) —> Ca(OH)2 (s)

• vigorous reaction

• some of Ca(OH)2 dissolves, giving a weakly basic solution

(ch. 11) magnesium reaction with cold water

• Mg (s) + 2H2O (l) —> Mg(OH)2 (s/aq) + H2(g)

• reacts slowly

• forms a weakly basic solution

(ch. 11) hot magnesium reaction with water (as steam)

• Mg(s) + H2O (g) —> MgO (s) + H2 (g)

• reacts vigorously with water

(ch. 11) calcium reaction with water

• Ca(s) + 2H2O (l) —> Ca(OH)2 + H2

• forms a cloudy white suspension

(ch. 11) Barium reaction with water

reacts vigorously

(ch. 11) solubility of group 2 hydroxides trend

increases going down the group

(ch. 11) solubility of group 2 sulfates trend

decreases going down the group

(ch. 11) solubility of group 2 carbonates

Mg, Ca, Sr, Ba are insoluble

(ch. 11) Group 2 carbonate solubility with dilute acids

reactions with dilute NHO3 & dilute HCl form soluble salts

(ch. 11) Thermal decomposition of group 2 carbonates trend

the temperature at which thermal decomposition takes place increases going down group 2

(ch. 11) thermal decomposition of group 2 nitrates trend

the temperature at which thermal decomposition takes place increases going down group 2

(ch. 11) cement + sand & rock =

concrete

(ch. 11) what is slaked lime made of? what is it used for?

• Ca(OH)2

• raise pH of soil

(ch. 11) what is limestone made of?

CaCO3