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CHEMICAL BONDINGS (Alloys (Can keep its shape more than pure elements…
CHEMICAL BONDINGS
Alloys
Homogeneous mixture of elements of which one of them is a pure metal
Can keep its shape more than pure elements
Stronger, more resistent and hard to bend, but more brittle
Bigger atoms make the districation of atoms (sliding) more difficult
They disturb they orderly arrangement of atom in the metals
The interaction of atoms involving the outer electrons of each atom
The Number of the Group of an element corresponds to the number of electrons in the outer shell
Every atom needs to have 8 electrons in their outer shell
Lewis Configuration
Different types of bonding
Bondings in elements
Metallic bondings (metallic elements)
metallic lattice
The atoms become positive ions because they have lost electrons (sea of delocalized electrons), but the number of protons in the nucleus has remained unchanges
Positive ions --> more stable electron arrangement
Covalent bondings (non-metallic elements)
Bondings in compounds
Covalent bondings (non-metallic elements)
simple molecules or giant molecular lattices
The bond is formed by the sharing electrons between two atoms and each atom contributes one electron to each bond
Polar: the cloud of electrons is more shifted towards the atom with the highest electronegativity (0.5≤Δe<1.7)
Non-polar: the cloud is distributed symmetrically (Δe<0.5)
Ionic bonding (metal + non-metal)
giant ionic lattices
It involves the transfer of electrons from one atom to another
The oppositely charged ions are attracted to each other by electrostatic forces
Δe≤1.7
Properties of bondings
Ionic compounds
Crystalline solids at room temperature
High melting and boiling points
Often soluble in water
Conduct electricity
Covalent compounds
Liquid or gases at room temperature
Low melting and boiling point
Soluble in organic solvents (ex: ethanol)
Do not conduct electricity
Electronegativity: the capability of an element to attract the electrons shared in a bonding