Metals
1. Electron configuration.
Metals typically have 1 to 3 electrons in their outer shell , which they can easily lose to form positive ions (cations).
2. Reactivity.
Metals tends to react with non -metals and acids.for example alkali metals like sodium react with vigorously with water , while transition metal can react with acids to release hydrogen gas .
3. Oxides formation .
Metals oxides are generally basic in nature . For instance , sodium acid react with water to form sodium hydroxide (a strong base).
4. Tendency to form compounds
Metal often form ionic compounds by transferring electron to nonmetal. for examples sodium chloride (Nacl) forms sodium and chlorine.
5. Conductivity.
Metals are good conductors odf electricity and heat due to the presence of free- moving electrons .
Non metals.
1. Electron configuration .
Non-metal usually have 4 to 8 electron in outer shell and tends to gain or share electrons to form negative ions ( anions) or covalent compounds
2. Reactivity.
Non metal can react with metals to form ionic compounds and with other nonmetals to form covalent compounds. For example chlorine can react with sodium to form sodium chloride.
3. Oxides formation .
Nonmetals oxides are typically acidic or neutral. For instance , sulfur dioxide react with water form sulfurous acid.
4. Tendency to form compound.
Non metal often form covalent compounds by sharing electrons . For example Water is formed by the sharing of electron between hydrogen and oxygen.
5. Conductivity.
Non metal are generally poor conductors of electricity and heat, with exception like graphite.
Important points of metals and non- metals.
*Metals tends to lose electron and form cation, while non-metals gain or share electron to form anions or covalent bonds.
* Metals generally form basic oxides , whereas nonmetal form acidic or neutral oxides.
* Metals are typically good conductors of electricity, while non-metals are not, it is poor conductors of electricity.
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