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This presentation talks about the physical properties of metals which you can see and feel, and also about the chemical properties which arise on reactions
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Properties of Metals
Properties of Metals
Maria Vincent
-The Adroit 6
Maria Vincent
-The Adroit 6
PROPERTIES OF METALS
Physical Properties
Determining the Chemical Properties of Metals
Those features of metals which can be seen or felt.
Physical Properties
State of Existence
Conduct-ivity
Hardness
Lustre
Sonorosity
Malleabilty
Ductility
Melting/ Boiling
Allotropy
Tensile Strength
State of ExistenceSolids at room temperature
Exception: Mercury- Liquid
LustreHave a shiny surface (lustre)
when freshly cut.
ConductivityGood conductor of heat and
electricity.
Silver is the best conductor of heat and electricity.
HardnessUsually hard
Exception: Sodium, Potassium- soft
SonorisityThey are sonorous.
Malleability and Ductility
Metals are malleable and ductile.
Gold, silver and platinum are highly malleable and ductile.
Melting and Boiling Point
High melting and boiling point.
Exception: Gallium, cesium have low mp and bp.
AllotropyMetals do not exist in
allotropic forms.
Tensile StrengthHigh tensile strength (do not
break easily).
PROPERTIES OF METALS
Chemical Properties
Determining the Chemical Properties of MetalsDetermining the Chemical Properties of Metals
The tendency of metals to lose electrons from their valence shells.
CHEMICAL PROPERTIES OF METALSReaction of Metals with Oxygen
Metals reacting with Oxygen
What happens when a piece of magnesium ribbon is burnt
2Mg + O2 -----g2MgO(Grey colore
d)
(White powdery
substance)
Metals reacting with Oxygen
What happens when 1 gram of copper powder is heated?
2Cu + O2 -----g2CuO(Brow
n colore
d)
(BlackColored)
Metals reacting with Oxygen
What happens when sodium is left in the open?
4Na + O2 -----g2Na2O(Silvery-
white colored)
(GreyColored)
Metals reacting with Oxygen
We can have a generalized equation:
Metal + Oxygen ----g Metal Oxide
Nature of Metal Oxides
Oxides of metals like Na, K, Mg dissolve in water to form soluble hydroxides called alkalis.
These react with acids to form salt and water.
Na2O + H2O ----g 2NaOH
NaOH + HCl ----g NaCl + H2O
Nature of Metal Oxides
Oxides of metals like Ca, Fe react with water to form insoluble hydroxides called bases.
These react with acids to form salt and water.
CaO + H2O ----g Ca(OH)2
Ca(OH)2 + HCl ----g CaCl2 + H2O
Nature of Metal Oxides
Oxides of Al and Zn show basic as well as acidic behaviour- amphoteric oxides.
These react with acids and to form salt and water.
Al2O3 + 6HCl ----g 2AlCl3 + H2O
Al2O3 + 2NaOH ----g 2NaAlO2 + H2O
CHEMICAL PROPERTIES OF METALS
Reaction of Metals with Water
Metals reacting with Water
Highly reactive metals- Na, K- react violently in cold water and catch fire.
2Na + H2O -----g2NaOH + H2 + Heat
Metals reacting with Water
Calcium reacts with water less violently and magnesium reacts with water on heating.
+
Mg + 2H2O -----g Mg(OH)2 + H2
Metals reacting with Water
In general:
Metal + Water ----g Metal Hydroxide + Hydrogen
Metals reacting with WaterMetals of lower reactivity- Fe,
zn, Al- react with water only when steam is passed over heated metals.
3Fe + 4H2O -----g Fe3O4 + 4H2 (steam)
Metals reacting with Water
In general:
Metal + Steam ----g Metal Oxide + Hydrogen
CHEMICAL PROPERTIES OF METALS
Reaction of Metals with Acids
Metals reacting with Acids
Recall these reactions:
NaCl + H2
MgCl2 + H2
FeSO4 + H2
ZnSO4 + H2 Zn + H2SO4
Fe + H2SO4
Mg+ 2HCl
Na + HCl
-----g-----g-----g-----g
Metals reacting with Acids
Metals placed above hydrogen react with dilute acids to form salt and release hydrogen gas.
Metal + Acid ----g Salt+ Hydrogen
Metals reacting with Acids
Note: Metals do not evolve hydrogen gas when they react with dilute nitric acid. Nitric acid is a strong oxidizing agent and oxidizes the hydrogen evolved to water and it self gets reduced to an oxide of nitrogen.Zn+4HNO3 ----g Zn(NO)3 + 2H2O +
2NO2
CHEMICAL PROPERTIES OF METALSReaction of Metals with Solutions of Other Metallic Salts
Metals reacting with Other Metallic Salt Solutions
Metals placed higher in the reactivity series can displace the metal which occupies a lower position from its aqueous solution of its salt.
Metals reacting with Metallic Salt Solutions
Recall these reactions:
ZnSO4 + Fe
Al2(SO4)3 + 3Zn
Na2SO4 + Mg Na + MgSO4
2Al+ 3ZnSO4
Zn+ FeSO4
-----g
----g
-----g
Metals reacting with Other Metallic Salt Solutions
Metal + Other Metal’s Salt Solution ----g First Metal’s Salt Solution+ Metal from the Salt
Solution