1) Chemical Bond :- The attractive force which holds various constituents ( atoms, ions, etc) together in different chemical species
2) Electrovalent bond aka Ionic Bond :- The bond formed, as a result of the electrostatic attraction betweeen the positive and negative ions
3) Octet Rule :- Atoms can combine either by transfer of valence electrons from one atoms to another (gaining or losing) or by sharing of valence electrons in order to have an octet in their valence shell
4) Formal Charge :- The formal charge of an atom in a polyatomic molecule or ion may be defined as the difference between the number of valence electron of that atom in an isolated or free state and the number of electrons assigned to that atom in the Lewis structure
5) Lattice Enthalpy :- The Lattice enthalpy of an ionic solid is defined as the energy required to completely seperate on mole of a solid ionic compound into gaseous constituent ions.
6) Bond Length :- The equilibrium distance between the nuclei of two bonded atoms in a molecule.
7) Covalent Radius :- It is measured approximately as the radius of an atom's core which is in contact with the core of an adjacent atom in a bonded situation. (Leave it to our textbook to give a complicated definition even for a simple concept (ง •_•)ง)
It is also given as the half of the distance between two similar atoms joined by a covalent bond in the same molecule
8) Van der waals radius :- It is half of the distance between two similar atoms in seperate molecules in a solid
9) Bond Angle :- It is defined as the angle between the orbitals containing bonding electron pairs around the central atoms in a molecule/complex ion.
10) Bond Enthalpy :- It is defined as the amount of energy required to break one mole of bonds of a particular type between two atoms in a gaseous state.
11) Bond Order :- It is given by the number of bonds between the two atoms in a molecule
12) Structure of Resonance :- Whenever a single Lewis structure cannot describe a molecule accurately, a number of structures with similar bond energy, positions of nuclei, bonding and non-bonding pairs of electrons are takes as canonical structures of the hybrid which describes the molecule accurately
13) Dipole Moment :- It is defined as the product of the magnitude of the charge and the distance between the centres of positive and negative charge
14) Hybridisation :- The process of intermixing of the orbitals of slightly different energies so as to redistribute their energies, relsulting in the formation of new set of orbitals with equivalent energies and shape.
15) Bonding molecular orbital :- Addition of atomic orbitals
16) Antibinding molecular orbitals :- Subtraction of atomic orbitals
17) Hydrogen Bond :- The attractive forces which binds hydrogen atoms of one molecule with the electronegative atom (F,O or N) of another molecule.
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