You are investigating the reactivity of oxygen with other non-metals

You are investigating the reactivity of oxygen with other non-metals.

a) Draw a box diagram to show the electron configuration of oxygen.

b) Give the symbol and charge of an oxygen ion.

c) Draw the box diagram to show the electron configuration of the oxygen ion.

d) Silicon dioxide can form a beautiful crystal known as quartz. Draw the Lewis dot structure. Show all steps and charges.

e) Determine the geometry of silicon dioxide.

f) What is the hybridisation of the central atom in silicon dioxide?

The correct answer and explanation is :

Here are the answers to your questions:

a) Box Diagram of Oxygen Electron Configuration

Oxygen has an atomic number of 8, meaning it has 8 electrons. The electron configuration is 1s² 2s² 2p⁴. Below is the box diagram representation:

1s  ↑↓   
2s  ↑↓   
2p  ↑↓ ↑  ↑

Each box represents an orbital, and the arrows represent electrons (↑↓ for paired electrons and ↑ for unpaired).

b) Symbol and Charge of an Oxygen Ion

When oxygen gains two electrons to complete its octet, it forms an oxide ion (O²⁻).
Symbol: O²⁻
Charge: -2

c) Box Diagram of the Oxygen Ion (O²⁻)

The oxygen ion has two additional electrons, making its electron configuration 1s² 2s² 2p⁶, the same as neon (Ne):

1s  ↑↓   
2s  ↑↓   
2p  ↑↓ ↑↓ ↑↓

All electrons are now paired.

d) Lewis Dot Structure of Silicon Dioxide (SiO₂)

Silicon dioxide consists of one silicon (Si) atom covalently bonded to two oxygen (O) atoms. Since oxygen needs two bonds to complete its octet, each oxygen forms a double bond with silicon.

Steps:

Valence Electrons:

Si: 4 valence electrons
O: 6 valence electrons × 2 = 12
Total: 16 valence electrons

Bond Formation:

Silicon forms two double bonds with oxygen to satisfy the octet rule.

Final Structure:

   O═Si═O

Each oxygen has four lone electrons (..), and Si has a full octet.

e) Geometry of Silicon Dioxide

SiO₂ is a linear molecule due to the double bonds and sp hybridization of the silicon atom. The bond angle is 180°.

f) Hybridization of Silicon in SiO₂

The central Si atom is sp hybridized.

Explanation (300 words)

Silicon dioxide (SiO₂) has a linear molecular geometry due to the bonding between silicon and oxygen. To determine the hybridization, we analyze the valence electrons and bonding.

Silicon belongs to group 14 and has four valence electrons (3s²3p²). Oxygen belongs to group 16 with six valence electrons. Each oxygen forms a double bond with silicon to satisfy the octet rule.

In bonding, silicon needs to form two sigma (σ) bonds with oxygen. The number of sigma bonds determines hybridization. Since silicon forms two σ bonds, its steric number is 2 (number of sigma bonds + lone pairs).

Using the steric number rule:

Steric Number 2 → sp hybridization
Steric Number 3 → sp² hybridization
Steric Number 4 → sp³ hybridization

Since SiO₂ has a steric number of 2, silicon undergoes sp hybridization. This means one s orbital and one p orbital mix to form two sp hybrid orbitals, aligning in a linear shape (180° bond angle). The remaining two p orbitals remain unhybridized and participate in π bonds with oxygen.

Thus, SiO₂ has an sp hybridized silicon atom. The linear structure is due to sp hybridization and the double bonds between Si and O.

Image Representation

Here is an image of the SiO₂ Lewis structure and molecular geometry:

Here is the diagram illustrating the Lewis dot structure, molecular geometry, and hybridization of silicon dioxide (SiO₂). Let me know if you need any modifications or further explanations!