Question

Consult your textbook and lecture notes and review the concepts of hybridization, hybrid orbital, polar and non-polar either in a bond or molecule, σ bond, π bond, London dispersion forces, dipole-dipole forces, and hydrogen bonding. 

Answer 1

ANS-1:In chemistry, the electron domain refers to the number of lone pairs or bond locations around a particular atom in a molecule. Electron domains may also be called electron groups.   

ANS-2: orbital hybridisation (or hybridization) is the concept of mixing atomic orbitals into new hybrid orbitals (with different energies, shapes, etc., than the component atomic orbitals) suitable for the pairing of electrons to form chemical bonds in valence bond theory. Fr example ,the hybridisation of the carbon atom is based on the number of bonds to other carbons or identical atoms. sp3 = single bond. sp2 = double bond. sp = triple bond

ANS-3:the hybrid orbitals form from the mixing of two or more atomic orbitals. In the chemical bond formation of simple molecules, we can simply consider the overlapping of atomic orbitals.example-When four atomic orbitals are mixed to form hybrid orbitals, 4 x sp3 hybrid orbitals are formed

ANS-4 chemical species in which the distribution of electrons between the covalently bonded atoms is not even. Polarity is a description of how different the electrical poles of a molecule are. If they are highly different, it can be said that the species is a highly polar molecule.[SEPERATION OF CHARGE]

ANS-5:A nonpolar molecule has no separation of charge, so no positive or negative poles are formed. In other words, the electrical charges of nonpolar molecules are evenly distributed across the molecule[ NO SEPERATION OF CHARGE]

ANS-6:Sigma bond are formed by the overlap of atomic orbitals. Sigma bonds are formed by end-to-end overlapping and . acquired their names from the Greek letters and the bond when viewed down the bond axis.

ANS-7: pi bonds are formed by the overlap of atomic orbitals.  Pi bonds are when the lobe of one atomic orbital overlaps another. acquired their names from the Greek letters and the bond when viewed down the bond axis.

ANS-8:The London dispersion force is the weakest intermolecular force. The London dispersion force is a temporary attractive force that results when the electrons in two adjacent atoms occupy positions that make the atoms form temporary dipoles. This force is sometimes called an induced dipole-induced dipole attraction. Example- HOMOATOMIC MOLECULES

ANS-9:Dipole-dipole forces are attractive forces between the positive end of one polar molecule and the negative end of another polar molecule. Dipole-dipole forces have strengths that range from 5 kJ to 20 kJ per mole.The partially positive end of a polar molecule is attracted to the partially negative end of another. An example of a dipole–dipole interaction can be seen in hydrogen chloride (HCl): the positive end of a polar molecule will attract the negative end of the other molecule and influence its position.

ANS-10:A hydrogen bond is an attraction between two atoms that already participate in other chemical bonds. One of the atoms is hydrogen, while the other may be any electronegative atom, such as oxygen, chlorine, or fluorine. Hydrogen bonds may form between atoms within a molecule or between two separate molecules.water (H₂O)Water is an excellent example of hydrogen bonding.

Answer 2