Reaction Types

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Slide 1

Reaction Types

Slide 2

Combination (Synthesis) Reactions

Two or more substances combine to form a new compound.

A + X  AX

Reaction of elements with oxygen and sulfur

Reactions of metals with Halogens

Synthesis Reactions with Oxides

There are others not covered here!

Slide 3

Decomposition Reactions

A single compound undergoes a reaction that produces two or more simpler substances

Decomposition of:

Binary compounds H2O(l )  2H2(g) + O2(g)

Metal carbonates CaCO3(s)  CaO(s) + CO2(g)

Metal hydroxides Ca(OH)2(s)  CaO(s) + H2O(g)

Metal chlorates 2KClO3(s)  2KCl(s) + 3O2(g)

Oxyacids H2CO3(aq)  CO2(g) + H2O(l )

AX  A + X

Slide 4

Single Replacement Reactions

Replacement of:

Metals by another metal

Hydrogen in water by a metal

Hydrogen in an acid by a metal

Halogens by more active halogens

A + BX  AX + B

BX + Y  BY + X

Slide 5

The Activity Series of the Metals

Lithium

Potassium

Calcium

Sodium

Magnesium

Aluminum

Zinc

Chromium

Iron

Nickel

Lead

Hydrogen

Bismuth

Copper

Mercury

Silver

Platinum

Gold

Metals can replace other metals provided that they are above the metal that they are trying to replace

Metals above hydrogen can replace hydrogen in acids.

Metals from sodium upward can replace hydrogen in water

Slide 6

The Activity Series of the Halogens

Fluorine

Chlorine

Bromine

Iodine

Halogens can replace other halogens in compounds, provided

that they are above the halogen that they are trying to replace.

2NaCl(s) + F2(g) 

2NaF(s) + Cl2(g)

MgCl2(s) + Br2(g) 

???

No Reaction

???

Slide 7

Double Replacement Reactions

The ions of two compounds exchange places in an aqueous solution to form two new compounds.

AX + BY  AY + BX

One of the compounds formed is usually a precipitate, an insoluble gas that bubbles out of solution, or a molecular compound, usually water.

Slide 8

Combustion Reactions

A substance combines with oxygen, releasing a large amount of energy in the form of light and heat.