Draw The Electron Do Formula For Selenium Oxide, SeO2, And State The Type Of Bonds In A Selenium Dioxide Molecule.
A 1 Double Bond And 1 Triple Bond
B 1 Single Bond And 1 Double Bond
C 1 Single Bond And 1 Triple Bond
D 2 Double Bonds
E 2 Single Bonds
The correct answer and explanation is :
The correct answer is:
D) 2 Double Bonds
Explanation:
Selenium dioxide (SeO₂) consists of one selenium (Se) atom and two oxygen (O) atoms. To determine its electron dot (Lewis) structure and bonding type, follow these steps:
Step 1: Count the Valence Electrons
- Selenium (Se) belongs to Group 16 and has 6 valence electrons.
- Oxygen (O) also belongs to Group 16, with 6 valence electrons each.
- Total valence electrons: 6 (Se) + 2 × 6 (O) = 18 electrons.
Step 2: Determine the Central Atom
Since selenium is less electronegative than oxygen, it will be the central atom. The oxygen atoms will bond with selenium.
Step 3: Assign Bonds and Distribute Electrons
- Selenium forms two double bonds with each oxygen atom to complete their octets.
- Each oxygen gets 4 non-bonding electrons (lone pairs).
- Selenium has a formal charge of 0, meaning the structure is stable.
Step 4: Molecular Shape and Bond Type
- The molecule adopts a linear shape (O=Se=O) due to sp² hybridization and VSEPR theory.
- The Se–O bonds are both double bonds, meaning each consists of one sigma (σ) bond and one pi (π) bond.
Conclusion:
Selenium dioxide contains two double bonds (O=Se=O), making option D) 2 Double Bonds the correct choice. This structure is consistent with experimental data, showing strong covalent bonding between selenium and oxygen.