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Bonding and structure: Chapter 3 Part- 1 - Coggle Diagram
Bonding and structure:
Chapter 3
Part- 1
Ionic bonding:
Ionic bonds are formed when
there is give or take of electrons between atoms/ ions.
Ionic bonds are usually found in compounds that contain
metals combined with non- metals
. When a bond is formed in this way,
electrons are transferred from metal atoms to the non- metal atoms during the chemical reactions.
Atoms that give electrons are called as
cations
(+) ve charged.
Atoms that take electrons are called as
anions
(-) ve charged.
E.g. Reaction between Sodium chloride
Sodium + Chlorine ---> Sodium chloride
Sodium has one extra electron in it's outermost shell, while chlorine needs one electron to complete its outermost shell (has 7 e-). When these 2 elements react, outer electron of each sodium atom is transferred to the outer shell of chlorine. Both sodium and chlorine are in their ionic forms in the compound.
In this way,
both of the atoms obtain full outer shells
and become like the noble gases. One way of showing the electron transfer is by using a
dot and cross diagram
. Only outer electrons are important in bonding so diagrams can be simplified by missing out the inner shells:
Reactions:
Na (s) ---> Na+ (s) + e-
Cl (g) + e- ---> Cl- (g)
Na (s) + Cl (g) ---> NaCl (s)
An ionic bond is a strong electrostatic force between oppositely charged ions.
Also known as '
Electrovalent bonding
'.
Oxidation and reduction:
Oxidation involved loss of electrons.
Reduction involves gain of electrons.
A
redox
reaction involves
simultaneous oxidation and reduction.
More about Ionic compounds:
Ionic compound structure:
Ions are arranged in a
lattice
. The giant lattice structure of ionic compounds is a
regular arrangement of alternating positive and negative ions.
In a lattice,
oppositely charged ions attract each other
.
To see the structure of an ionic compound, we use x- ray diffraction.
This lattice structure is present due to the electrostatic energy.
Properties of an ionic compound:
High melting and boiling point (due to strong electrostatic forces).
Solid at room temperature.
Cannot conduct electricity when solid
; conducts in molten/ aqueous form.
Can mainly dissolve in water easily.