Statement -1 : Each carbon in ethylene molecule is ${\mathrm{sp}}^2$ hybridized.

Statement -2:  The $\mathrm{H}-\mathrm{C}-\mathrm{H}$ bond angle in ethylene molecule is $120°C$

Each carbon atom in ethylene is attached to two hydrogen atoms by single covalent bonds and to another carbon atoms by a double bond. Since each carbon is attached to three other atoms. it uses ${\mathrm{sp}}^2$ hybrid orbitals and an unhybridized ${\mathrm{p}}_{\mathrm{x}}$ orbital to form its bond. Each $\mathrm{C}-\mathrm{H}$ bond is a $\mathrm{\sigma }$ bond resulting from the overlap of $1s$ orbital of hydrogen atom and ${\mathrm{sp}}^2$ orbital of a carbon atom. One $\mathrm{C}-\mathrm{C}$ bond results from the linear overlap of ${\mathrm{sp}}^2$ orbitals one from each carbon atom. $\mathrm{One} \mathrm{\pi }$ bond results from the lateral overlap of two unhybridized ${\mathrm{P}}_{\mathrm{z}}$ orbitals. one from each carbon atom.