What atomic or hybrid orbitals make up the sigma bond between c1 and c2 in tetrafluoroethylene, c2f4?

hybrid sp2 -orbital make up the sigma bond between C1 and C2 in tetrafluoroethylene

Explanation:

The tetrafluoroethylene has a double bond between the carbons and single bonds between each fluor and carbon because each carbon requires a full octet and each fluor requires a pair of electrons.

In chemistry, hybridization is the interaction of atomic orbitals within an atom to form new hybrid orbitals. In sp2 hybridization, an s orbital and two orbitals are combined p. For this hybridization to occur, the carbon must be attached to three atoms as is the case in the carbon atom in this case. On the other hand, the sigma bond (σ) is formed when there is a front overlap of atomic orbitals; and the pi (π) bond is formed when there is superposition of parallel p orbitals.

Atoms that form sp2 hybridizations can form compounds with double bonds, as in this case between both carbons. Simple bonds are known as sigma bons (σ) and double bonds are composed of a sigma bond and a pi bond. So double bond between sp2 hybrid orbitals formed by one sigma-bond and one pi-bond.

In summary, hybrid sp2-orbital make up the sigma bond between C1 and C2 in tetrafluoroethylene

given:

mass of na = 115 g

excess cl2

to determine:

mass of nacl produced

explanation:

given reaction is-

2na(s) + cl2(g) → 2nacl(s)

since cl2 is in excess, na will be the limiting reagent

as per the reaction stoichiometry na: nacl = 1: 1

i.e. moles of na reacted = moles of nacl formed

now, # moles of na = mass of na/atomic mass

                                  = 115 g/23 g.mol-1 = 5 moles

therefore, moles of nacl = 5

molar mass of nacl = 58 g/mol

mass of nacl = 5 moles * 58 g.mol-1 = 290 g

ans: amount of nacl produced = 290 g