Using three dimensional model you have drawn, describe the shape of methane molecule. How many bonds are there and what kind of bonds is found there?
The shape of a methane molecule (CH4) can be described as a tetrahedron. In a tetrahedral shape, there are four bonding pairs of electrons surrounding the central carbon atom, pushing the four hydrogen atoms as far apart as possible.
Each hydrogen atom is bonded to the central carbon atom through a single covalent bond. Covalent bonds consist of the sharing of a pair of electrons between two atoms. In the case of methane, four covalent bonds are formed between the carbon atom and each of the four hydrogen atoms.
The bonds found in methane are categorized as sigma bonds, which are formed by the overlap of orbitals directly between the bonding atoms. Specifically, in methane, each hydrogen atom forms a sigma bond by overlapping its s orbital with one of the four sp3 hybrid orbitals of the central carbon atom. These sigma bonds are strong and hold the molecule together.
The shape of a methane molecule can be described as a tetrahedron. The central carbon atom is bonded to four hydrogen atoms, with each bond extending outward from the carbon atom in a three-dimensional space.
There are a total of four bonds in a methane molecule. These bonds are covalent bonds, specifically single covalent bonds. Each bond involves the sharing of one pair of electrons between the carbon atom and one of the hydrogen atoms. These covalent bonds result in a stable methane molecule.