Metal and Non-metal Oxides. An oxide is a compound of oxygen and one or more other elements.

Metal and Non-metal

Oxides

An oxide is a compound of oxygen and one or more other elements.

An oxide is a compound of oxygen and one or more other elements.Examples of oxides are carbon dioxide, CO2,

An oxide is a compound of oxygen and one or more other elements.Examples of oxides are carbon dioxide, CO2, sulfur trioxide, SO3,

An oxide is a compound of oxygen and one or more other elements.Examples of oxides are carbon dioxide, CO2, sulfur trioxide, SO3, and sodium oxide, Na2O.

In Science 10, you are given this Periodic Table:

METALS NON-METALS

An oxide formed by a metal and oxygen is called a metal oxide.

An oxide formed by a metal and oxygen is called a metal oxide.Some examples are:


Li2O


Li2OMgO


Li2OMgO

CaO

An oxide formed by a non-metal and oxygen is called a non-metal oxide.

An oxide formed by a non-metal and oxygen is called a non-metal oxide.Some examples are:


CO2


CO2

NO2


CO2

NO2

Cl2O

Metal oxides, and non-metal oxides have quite different properties.

Metal oxides, and non-metal oxides have quite different properties.One very important difference is what they produce when they are dissolved in water.

Metal oxides dissolve in water to form BASIC

solutions.

Metal oxides dissolve in water to form BASIC

solutions.

Non-metal oxides dissolve in water to form

ACIDIC solutions.

Metal oxides dissolve in water to form BASIC solutions.

Non-metal oxides dissolve in water to form ACIDIC solutions.

Na2O(s) + H2O(l)



Na2O(s) + H2O(l) 2NaOH(aq)




sodium hydroxide




sodium hydroxide(a base)



MgO(s) + H2O(l)



MgO(s) + H2O(l) Mg(OH)2(aq)




magnesium hydroxide




magnesium hydroxide(a base)



CO2(g) + H2O(l)



CO2(g) + H2O(l) H2CO3(aq)




Carbonic acid



SO2(g) + H2O(l)



SO2(g) + H2O(l) H2SO3(aq)




Sulfurous acid



SO3(g) + H2O(l)




Sulfuric acid



2NO2(g) + H2O(l)



2NO2(g) + H2O(l) HNO2(aq)



2NO2(g) + H2O(l) HNO2(aq)

Nitrous acid



2NO2(g) + H2O(l) HNO2(aq) + HNO3(aq)




Nitric acid




Nitric acidNitrous Acid



Cl2O(g) + H2O(l) 2



Cl2O(g) + H2O(l) 2HOCl(aq)




Hypochlorous Acid

Acid Precipitation



CO2(g)

Naturally occurs in Earth’s

atmosphere



Carbonic acid



Carbonic acidA weak acid

Carbon dioxide dissolves in rainwater to form weak carbonic acid. CO2(g) + H2O(l) H2CO3(aq)

Natural rainwater has a pH of about 5.6

Carbon dioxide dissolves in rainwater to form weak carbonic acid. CO2(g) + H2O(l) H2CO3(aq)


Rainwater with a pH of 5.6 and above is NOT called Acid

Rain


Rainwater is a pH lower than 5.6 is called Acid

Rain



Thermal power generating plants burn large amounts of coal.


Thermal power generating plants burn large amounts of coal.Coal and other fossil fuels contain small amounts of sulfur.

S(s) + O2(g)

S(s) + O2(g) SO2(g)

SO2 is a non-metal

oxide

S(s) + O2(g) SO2(g)

S(s) + O2(g) SO2(g)


Sulfurous acid

S(s) + O2(g) SO2(g)


Dissolved sulfurous acid causes Acid Precipitation



Many industrial processes release SO2 and SO3 into the atmosphere


Aqueous sulfurous acid and sulfuric acid cause

Acid Precipitation



Vehicle exhaust releases nitrogen oxides like NO2 to the atomosphere.


Nitric acidNitrous Acid

Acid precipitation can have serious effects on freshwater organisms, crops, and forests.

Acid precipitation can have serious effects on freshwater organisms, crops, and forests.Acid precipitation can also damage buildings and statues made of limestone or marble.

Limestone and marble are made up of calcium carbonate, CaCO3(s).

Limestone and marble are made up of calcium carbonate, CaCO3(s). When calcium carbonate is exposed to sulfuric acid (H2SO4(aq)), the following reaction occurs:


CaCO3(s) + H2SO4(aq)


CaCO3(s) + H2SO4(aq) CaSO4(s)


CaCO3(s) + H2SO4(aq) CaSO4(s) + H2O(l)


CaCO3(s) + H2SO4(aq) CaSO4(s) + H2O(l) + CO2(g)


CaCO3(s) + H2SO4(aq) CaSO4(s) + H2O(l) + CO2(g)

This slowly dissolves the CaCO3 which makes up limestone or marble.

Metal and Non-metal Oxides. An oxide is a compound of oxygen and one or more other elements.

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