A pure element unbound or in a diatomic state, such as CL2, always has an oxidation number of . a. magnitude equal to its valence number
b. 2
c. 1
d. 0

120,630,890

step-by-step explanation:

110+10=120,620+10=630,880+10=890

c is having 4 valence electrons and is bonded to three hydrogens and one sulphur atom, therefore, the number of bond pair is equal to four. as all the valence electrons are used in forming the bonds so, there is no lone pair left on carbon.

s is having 6 valence electrons and is bonded to one other sulfur atom and one carbon atom, therefore, the number of bond pair is equal to 2. as only two valence electrons are used in forming the bonds so, four electrons are left. therefore, two lone pairs are present on s.