METALS & NON METALS

 

SCIENCE CLASS 10TH CHAPTER-METAL AND NON-METAL FORMULA & IMPORTANT POINTS

Science Formulas

Class-10 for chapter-Metal and non-metal 

Metals: The elements, which have the properties of luster, malleability and ductility, high thermal and electrical conductivities. The metals have a good tendency to loose. electrons.

Non-metals: The elements, which do not have the above, mentioned properties.These have a good tendency to gain electrons.

Metalloids: The elements having the properties of metals as well as non-metals.

Difference between metals and non-metals    

PropertiesMetalsNon-metals
Physical Properties  
1. StateMetals are solids at ordinary temperature.

(except mercury, which is a liquid.)

Non-metals exist in all the three states,

that is, solid, liquid and gas.

2. LustreThey possess lustre of shine.They possess no lustre.

(except lodine and graphite.)

3. Malleability and DuctilityMetals are generally malleable and ductile.Non-metals are neither malleable nor ductile.
4. HardnessMetals are generally hard.

Alkali metals are exception.

Non-metals possess varying hardness.

Diamond is an exception.

It is the hardest substance known to occur in nature.

5. DensityThey have high densities.They generally possess low densities.
6. Conductivity (Heat & Electricity)Metals are good conductors of heat and electricity.Non-metals are poor conductors of heat and electricity.

The only exception is graphite which is

a good conductor of electricity.

7. Melting and boiling pointThey usually have high melting and boiling point.Their melting and boiling point are usually low. carbon and silicon.

The exceptions are boron,

carbon and silicon.

Main Group Metals

Group IA, IIA, and IIIA metals form cations by losing all of their outermost electrons. The charge on the cation is same as group number. The cation is given same name as the neutral metal atom. 

GroupElementCationIon name
IAHH+hydrogen ion
 LiLi+lithium ion
 NaNa+sodium ion
 KK+potassium ion
 CsCs+cesium ion
IIAMgMg2+magnesium ion
 CaCa2+calcium ion
 SrSr2+strontium ion
 BaBa2+barium ion
IIIAAlAl3+aluminum ion

Transition and Post Transition Metals

The elements usually form ionic compounds; many of the elements can form more than one cation. (The charges of the expected transition metals must be memorized; Group IV and V metal cations tend to be either group number or the group number minus two.

MetalIonSystematic nameCommon name
CadmiumCd2+cadmium ion 
ChromiumCr2+Chromium (II) ionchromous ion
 Cr3+Chromium (III) ionchromic ion
CobaltCo2+Cobalt (II) ioncobaltous ion
 Co3+Cobalt (III) ioncobaltic ion
CopperCu+copper(I) ioncuprous ion
 Cu2+Copper (II) ioncupric ion
GoldAu3+Gold (III) ion 
IronFe2+Iron (II) ionferrous ion
 Fe3+Iron (III) ionferric ion
ManganeseMn2+Manganese (II) ionmanganous ion
 Mn3+Manganese (III) ionmanganic ion
MercuryHg2+mercury (I) ionmercurous ion
 Hg2+Mercury (II) ionmercuric ion
NickelNi2+Nickel (II) ionnickelous ion
SilverAg+silver ion 
ZincZn2+zinc ion 
TinSn2+Tin (II) ionstannous ion
 Sn4+Tin (IV) ionstannic ion
LeadPb2+Lead (II) ionplumbous ion
 Pb4+Lead (IV) ionplumbic ion
BismuthBi3+Bismuth (III) ion 
 Bi5+bismuth (V) ion 

Main Group Non-Metal

Group IVA, VA, VIA, and VIIA nonmetals form anions by gaining enough electrons to fill their valence shell with eight electrons. The charge on anion is the group number minus eight. The anion is named after taking the element stem name and adding the ending -ide. 

GroupElementAnionIon name
IVACC4-carbide ion
 SiSi4-silicide ion
VANN3-nitride ion
 PP3-phosphide ion
 AsAs3-arsenide ion
VIAOO2-Oxide ion
 SS2-sulfide ion
VIASeSe2-selenide ion
 TeTe2-telluride ion
VIIAFF-fluoride ion
 ClCl-chloride ion
 BrBr-bromide ion
 II-iodide ion
IAHH-hydride ion

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