Chemical Bonding

A chemical bond is a lasting attraction between atoms, ions or molecules that enables the formation of chemical compounds. The bond may result from the electrostatic force of attraction between oppositely charged ions as in ionic bonds or through the sharing of electrons as in covalent bonds.

Ionic bonding

Ionic bonding is the complete transfer of valence electron(s) between atoms. It is a type of chemical bond that generates two oppositely charged ions. In ionic bonds, the metal loses electrons to become a positively charged cation, whereas the nonmetal accepts those electrons to become a negatively charged anion

Covalent bonding

A covalent bond is a chemical bond that involves the sharing of electron pairs between atoms. These electron pairs are known as shared pairs or bonding pairs, and the stable balance of attractive and repulsive forces between atoms, when they share electrons, is known as covalent bonding.

Single covalent

A single covalent bond is when only one pair of electrons is shared between atoms. A sigma bond is the strongest type of covalent bond, in which the atomic orbitals directly overlap between the nuclei of two atoms.

Multiple covalent

Covalent bonding is the sharing of one or more electron pairs. In many covalent bonding situations, multiple chemical bonds exist — more than one electron pair is shared. ... A nitrogen atom can fill its octet by sharing three electrons with another nitrogen atom, forming three covalent bonds, a so-called triple bond.

Co-ordinate dative

A coordinate covalent bond, also known as a dative bond, dipolar bond, or coordinate bond is a kind of two-center, two-electron covalent bond in which the two electrons derive from the same atom. The bonding of metal ions to ligands involves this kind of interaction. This type of interaction is central to Lewis theory.

Comparison

Ionic bonding

1.Electrostatic force of attraction between oppositely-charged ions formed by the complete transfer of electrons from an atom to another atom

2.An atom that loses electrons will form a positive ion that is then transferred to another atom, the atom that gains the electron will form an negative ion and the cations and anions are then attracted by a strong electrostatic force of attraction.

3.The bond is relatively very strong

THEY DISSOLVE IN WATER

Covalent bonding

1.Electrostatic force of attraction that two neighbouring nuclei have for a localized air of electrons shared between them

2.The atoms share their valence electrons to achieve duplet electronic configuration

3.The bond is relatively weak

THEY HYDROLYSE IN WATER

Dot and cross diagram

A dot and cross diagram is a diagram used to show how electrons from the outer shells of atoms are shared or transferred in a chemical bond.

Ionic compound

Covalent compound

Shape of molecules

VSPER theory

VSEPR theory is based on the idea that the geometry (shape) of a molecule is mostly determined by repulsion among the pairs of electrons around a central atom. The pairs of electrons may be bonding or non-bonding (also called lone pairs).

Bond angles

Bond angles also contribute to the shape of a molecule. Bond angles are the angles between adjacent lines representing bonds. The bond angle can help differentiate between linear, trigonal planar, tetraheral, trigonal-bipyramidal, and octahedral

Sigma and Pie bonds(σ and π bonds)

SP orbital is 2 bonds

Sp4 is 3 bonds

Lone pair of electrons counts as 1

Double bond and triple bond counts as 1 bond

Sigma bonds(σ )

Formed by orbitals from two atoms overlapping end to end

Pie bonds(π )

Formed by the P orbitals from two atoms overlapping sideways

Metallic bonding

Metallic bonding is a type of chemical bonding that rises from the electrostatic attractive force between conduction electrons and positively charged metal ions. It may be described as the sharing of free electrons among a structure of positively charged ions.

MP and BP

Most metals have high melting and boiling points due to their strong intermolecular forces

Electrical conductivity

Metals can conduct electricity due to the movement of delocalized electron

Heat conductivity

Metals can also conduct heat due to the movement of delocalized electron as well

Electronegativity

It is the ability of a particular atom, which is covalently bonded to another atom, to attract the bond pair of electron towards itself.

Allotropes

Graphite and Graphene have giant structure
Buckyball/c60 and nanotube have simple structure and can conduct electricity as well as graphite and graphene

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Chemical Bonding

Chemical Bonding

Ionic bonding

Covalent bonding

Single covalent

Multiple covalent

Co-ordinate dative

Comparison

Ionic bonding

Covalent bonding

Dot and cross diagram

Ionic compound

Covalent compound

Shape of molecules

VSPER theory

Bond angles

Sigma and Pie bonds(σ and π bonds)

Sigma bonds(σ )

Pie bonds(π )

Metallic bonding

MP and BP

Electrical conductivity

Heat conductivity

Electronegativity

Allotropes

The topic after this is very difficult to explain words thus I will be using videos from BBSpikschemistry which is extremely helpful

General

VDW and Volatility

Intermolecular forces

Polarity

CO-ORDINATE DATIVE BONDING

Why ice floats

Hydrogen bond

Hydrogen bond comparison