Write the Lewis structure for O 2 F 2 . Predict the bond angles and hybridization of the two central oxygen atoms. Assign oxidation states and formal charges to the atoms in O 2 F 2 . The compound O 2 F 2 is a vigorous and potent oxidizing and fluorinating agent. Are oxidation states or formal charges more useful in accounting for these properties of O 2 F 2 ?

Interpretation: The Lewis structure, bond angle of O2F2 and hybridization of two central atom of oxygen in O2F2 is to be stated. The formal charge and oxidation state of each atom is to be assigned. If oxidation state or formal charge more useful in accounting for the given properties of O2F2 is to be stated.

Concept introduction: The following steps are to be followed to determine the molecular structure of a given compound,

• The central atom is identified.

• Its valence electrons are determined.

• The value 1 e− is added to the total number of valence electrons for each monovalent atom present.

• The total number obtained is divided by 2 to find the number of electron pairs.
• This further gives the hybridization of the given compound.

Formal charge is a charge given to an atom with assumption that electrons are shared equally between atoms in all chemical bonds irrespective of their electro negativity.

To determine: The Lewis structure, bond angle of O2F2 and hybridization of two central atom of oxygen in O2F2 ; the formal charge and oxidation state of each atom; If oxidation state or formal charge more useful in accounting for the given properties of O2F2 .

Explanation

The Lewis structure, bond angle of O2F2 and hybridization of two central atom of oxygen in O2F2 is as follows.

The first step in determining the Lewis structure is to determine the number of valence electrons. The atomic number of oxygen (O) is 8 and its electronic configuration is,

1s22s22p4

The valence electron of oxygen is 6 .

The atomic number of fluorine (F) is 9 and its electronic configuration is,

1s22s22p5

The valence electron of fluorine is 7 .

The molecule O2F2 is made of two fluorine atoms and two oxygen atoms; hence, the total number of valence electrons is,

2O + 2F =( 2×6 + 2×7)= 26

The formula of number of electron pairs is,

X=V+M±C2

Where,

• X is the number of electron pairs.
• V is the valence electrons of central atom.
• M is the number of monovalent atoms.
• C is the charge on compound.

The number of electron pairs is,

X=V+M±C2X=82=4

This means that the central atom shows sp3 hybridization and should have a tetrahedral geometry. The bond angle is 109.5° .

The Lewis structure of O2F2 is