In a covalent bond, electrons are shared between atoms, leading to a concentration of electron density between the nuclei.

sp3 hybridization involves one s and three p orbitals, resulting in a tetrahedral geometry.

Bond order = (Number of bonding electrons - Number of antibonding electrons) / 2 = (3 - 1) / 2 = 1.

O2 has 12 total electrons, with 10 in bonding orbitals and 2 in antibonding orbitals. Bond order = (number of bonding electrons - number of antibonding electrons) / 2 = (10 - 2) / 2 = 4 / 2 = 2.

Increasing temperature generally increases the kinetic energy of molecules, leading to more frequent and effective collisions, thus increasing the reaction rate.

Molecules with sp2 hybridization have bond angles of approximately 120 degrees due to trigonal planar geometry.

A trigonal bipyramidal electron geometry with one lone pair results in a T-shaped molecular geometry.

sp2 hybridization results in a trigonal planar shape due to the arrangement of three electron groups around the central atom.

CH4 has four bonding pairs of electrons and no lone pairs, resulting in a tetrahedral molecular geometry.

H2O has a bent shape and significant electronegativity difference between H and O, resulting in a higher dipole moment compared to CO2, CH4, and NH3.

Ionic bonds result from the transfer of electrons from one atom to another, typically between metals and nonmetals.