Highest oxidation state of Mn in the fluoride is +4 but in their oxides it is +7. This is because :
1) fluorine always stabilise lower oxidation state
2) fluorine possess no d - orbitals
3) fluorine is more electronegative than oxygen
4) fluorine can form single bond, oxygen can form double bond

Higher oxidation state of manganese in fluoride is +4 (MnF_(4)) but highest oxidation state in oxides is +7(Mn_(2)O_(7)) because

Higher oxidation state of manganese in fluoride is +4 (MnF_(4)) but highest oxidation state in oxides is +7(Mn_(2)O_(7)) because

The oxidation state of fluorine can also be + 2. The given statement is true or false?

Assertion: In some cases oxygen shows positive oxidation number though it is an electronegative element. Reason: Fluorine is more electronegative than oxygen.

Write the correct form of the following statement: The fluorine atom is more electronegative than H atom, therefore, the H-F bond is formed by gain and loss of electrons.

Although fluorine is more electronegative than oxygen, but the ability of oxygen to stabilise higher oxidation states exceeds that of fluorine. Why?

A : Oxides of carbon in higher oxidation state is more acidic than in lower oxidation state . R : Both CO_(2) and CO can exist .

Fluorine has -1 oxidation state while iodine exhibits oxidation states of -1, +1, +3 ,+5 and +7. This is due to

Assertion: Fluorine exists only in -1 oxidation state. Reason: Fluorine has 2s^(2)2p^(5) configuration.

The reactivities of C Cl_(4) and SiCl_(4) are different. For example SiCl_(4) can be easily hydrolysed and is prone to substitution reactions, whereas C Cl_(4) is inert. The observed difference is because (a)carbon atom has smaller size than hence substitution is not possible (b)carbon is more electronegative than silicon ( c)silicon has low lying unoccupied orbitals (d) C-Cl bond is stronger than Si-Cl bond