chemistry predicting products rules

metals and oxygen

metallic oxides

metallic oxides and carbon dioxide

metallic carbonates

metal oxides and sulfur dioxide

metallic sulfites

nonmetal oxides and water

acids

soluble metallic oxides and water

bases (metallic hydroxides)

ammonium carbonate

ammonia, water, and carbon dioxide

ammonium hydroxide

ammonia and water

binary ionic compounds

electrolyze into metal and nonmetal components

carbonic acid

water and carbon dioxide

hydrogen peroxide

water and oxygen

metallic carbonates

metallic oxides and carbon dioxides

metallic chlorates

metallic chlorides and oxygen

oxyacids

water and nonmetallic oxides

sulfurous acid

water and sulfur dioxide

hydrocarbon

use excess oxygen to form carbon dioxide and water

all aqueous

no solution

metals and acids

metal replaces hydrogen in acid to make metallic ions and hydrogen gas

metals and water

metals replace hydrogen in water to make metallic hydroxides and hydrogen gas

metals and less active metals

metals and metal ion solutions

halogens and halides

halogens replace less active halide to make a halide ion and halogen

two soluble ions (aq)

insoluble precipitate

metal sulfides and acid

hydrogen sulfide gas and salt

metal carbonates and acid

carbon dioxide gas, water, and salt

metal sulfites and acid

sulfur dioxide gas, water, and salt

ammonium salt heated with strong soluble hydroxide

ammonia gas, water, and salt

acid and base

salt and water

HCl (hydrochloric acid)

strong acid

HBr (hydrobromic acid)

strong acid

HI (hydroiodic acid)

strong acid

HNO3 (nitric acid)

strong acid

HClO4 (perchloric acid)

strong acid

H2SO4 (sulfuric acid)

strong acid

LiOH (lithium hydroxide)

strong base

NaOH (sodium hydroxide)

strong base

KOH (potassium hydroxide)

strong base

Ba(OH)2 (barium hydroxide)

strong base

Sr(OH)2 (strontium hydroxide)

strong base

HF (hydrofluoric acid)

weak acid

H3PO4 (phosphoric acid)

weak acid

H2CO3 (carbonic acid)

weak acid

CH3CO2H (acetic acid)

weak acid

H2C2O4 (oxalic acid)

weak acid

H2C4H4O6 (tartaric acid)

weak acid

H3C6H5O7 (citric acid)

weak acid

HC9H7O4 (aspirin)

weak acid

NH3 (ammonia)

weak base

net ionic seperation

no solid liquid gases or weak acids

acids

proton donor

bases

proton acceptor

H2CO3

H2O+CO2

H2SO3

H2O+SO2

NH4OH

H2O+NH3

equilibrium always proceeds

towards the weaker substances

salts

ionic compounds

oxidation number of pure elements

0

oxidation number of fluorine

-1

oxidation number of oxygen

-2

oxidation number of hydrogen

+1

oxidation number of charged ions

the charge

oxygen is -2 UNLESS

is a peroxide or paired w fluorine

oxidation number of Cl, Br, and I

-1

Cl, Br, and I are -1 UNLESS

paired with oxygen or fluorine

hydrogen is -1 UNLESS

part of a metal hydride

oxidation

losing electrons

reduction

gaining electrons

same redox on both sides means

NO REDOX REACTION

acids in water

H3O- and an anion

bases in water

hydroxide and an anion

acids and ammonia

NH4+ and water