Chemical formula: Name of chemical formula: Total number of valence electrons: Lewis dot structure: Calculate formal charges: VSEPR Electron Pair Geometry: Molecular Geometry: Polar or Non-polar: Hybridization of the central atom(s): Resonance structures when applicable:
The Correct Answer and Explanation is:
Sure! Let’s use the example of carbon dioxide (CO₂) to answer the questions:
- Chemical Formula:
The chemical formula of carbon dioxide is CO₂. - Name of Chemical Formula:
The name of the chemical formula CO₂ is Carbon Dioxide. - Total Number of Valence Electrons:
To calculate the total number of valence electrons:- Carbon (C) is in group 14 of the periodic table and has 4 valence electrons.
- Oxygen (O) is in group 16 and has 6 valence electrons.
- Since there are two oxygen atoms, the total valence electrons are:
- Lewis Dot Structure:
In the Lewis dot structure of CO₂:- Carbon is the central atom with two double bonds to the two oxygen atoms.
- The oxygen atoms have two lone pairs of electrons each.
- The structure looks like this: O=C=O.
- Formal Charges:
The formal charge is calculated as: Formal Charge=Valence electrons−(Lone pair electrons+12×Bonding electrons)\text{Formal Charge} = \text{Valence electrons} – (\text{Lone pair electrons} + \frac{1}{2} \times \text{Bonding electrons})Formal Charge=Valence electrons−(Lone pair electrons+21×Bonding electrons)- For carbon: 4−(0+2×4)=0 (formal charge on carbon).4 – (0 + 2 \times 4) = 0 \text{ (formal charge on carbon)}.4−(0+2×4)=0 (formal charge on carbon).
- For each oxygen: 6−(4+2×2)=0 (formal charge on oxygen).6 – (4 + 2 \times 2) = 0 \text{ (formal charge on oxygen)}.6−(4+2×2)=0 (formal charge on oxygen).
- VSEPR Electron Pair Geometry:
In CO₂, the central atom carbon has two regions of electron density (double bonds to two oxygens), so the electron pair geometry is linear. - Molecular Geometry:
The molecular geometry of CO₂ is also linear, as there are no lone pairs on the central carbon atom. - Polar or Non-polar:
CO₂ is non-polar because the molecule is symmetrical, and the dipoles cancel each other out. - Hybridization of the Central Atom(s):
The central carbon atom in CO₂ is sp hybridized. This is because it has two regions of electron density (two double bonds), which suggests an sp hybridization. - Resonance Structures (When Applicable):
In the case of CO₂, there are no resonance structures. The Lewis structure with double bonds between carbon and oxygen is the only valid structure.
Explanation (300 words):
Carbon dioxide (CO₂) is a linear, non-polar molecule with a central carbon atom bonded to two oxygen atoms by double bonds. The total number of valence electrons is 16, calculated by adding the valence electrons of carbon (4) and oxygen (6 each for two oxygen atoms). In the Lewis structure, each oxygen atom has two lone pairs, and the carbon atom forms two double bonds, one with each oxygen.
The formal charges for all atoms in CO₂ are zero, as shown by the formal charge calculation for carbon and oxygen. This means that the structure is well-formed and stable.
According to VSEPR theory, the electron pair geometry around the central carbon atom is linear, as there are two electron regions (double bonds) around it. The molecular geometry is also linear, and since there is no asymmetry in the distribution of charge, CO₂ is non-polar.
The central carbon atom in CO₂ is sp hybridized. This hybridization arises from the two electron regions (two double bonds), leading to a linear arrangement.
Since CO₂ does not have multiple valid resonance structures, it has a simple, stable structure with no need for resonance. The bond angles between the carbon and oxygen atoms are approximately 180°, confirming the linear geometry.
