L . BF4 • 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: I XeF • 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: . HO* 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 :
Here’s the detailed breakdown of the given compounds:
1. BF₄⁻
- Chemical Formula: BF₄⁻
- Name of Chemical Formula: Tetrafluoroborate ion
- Total Number of Valence Electrons:
Boron (B): 3, Fluorine (F): 7 × 4 = 28, Additional electron for the negative charge: +1
Total = 32 electrons - Lewis Dot Structure:
Boron is the central atom bonded to four fluorine atoms. Each fluorine has three lone pairs, and all single bonds form a complete octet for fluorine and boron. - Formal Charges:
All atoms have a formal charge of 0 since boron shares four electrons and fluorine achieves octet. - VSEPR Electron Pair Geometry: Tetrahedral
- Molecular Geometry: Tetrahedral
- Polar or Non-Polar: Non-polar (symmetrical charge distribution)
- Hybridization of the Central Atom: sp³
- Resonance Structures: Not applicable (single, stable structure)
2. XeF₂
- Chemical Formula: XeF₂
- Name of Chemical Formula: Xenon difluoride
- Total Number of Valence Electrons:
Xenon (Xe): 8, Fluorine (F): 7 × 2 = 14
Total = 22 electrons - Lewis Dot Structure:
Xenon is the central atom with two single bonds to fluorine. Xenon also has three lone pairs. - Formal Charges:
All atoms have a formal charge of 0. - VSEPR Electron Pair Geometry: Trigonal bipyramidal (five regions of electron density)
- Molecular Geometry: Linear (lone pairs are equatorial)
- Polar or Non-Polar: Non-polar (linear geometry cancels dipole moments)
- Hybridization of the Central Atom: sp³d
- Resonance Structures: Not applicable
3. H₂O
- Chemical Formula: H₂O
- Name of Chemical Formula: Water
- Total Number of Valence Electrons:
Hydrogen (H): 1 × 2 = 2, Oxygen (O): 6
Total = 8 electrons - Lewis Dot Structure:
Oxygen is the central atom with two single bonds to hydrogen and two lone pairs. - Formal Charges:
All atoms have a formal charge of 0. - VSEPR Electron Pair Geometry: Tetrahedral
- Molecular Geometry: Bent
- Polar or Non-Polar: Polar (asymmetrical charge distribution)
- Hybridization of the Central Atom: sp³
- Resonance Structures: Not applicable
Explanation:
- Valence Electrons: Sum of valence electrons of each atom and charge contributions determine the total.
- Lewis Dot Structure: Arranged to satisfy octet rules and minimize formal charges.
- Formal Charges: Calculated using ( \text{Formal Charge} = \text{Valence Electrons} – (\text{Lone Electrons} + \frac{\text{Bonding Electrons}}{2}) ).
- VSEPR Theory: Electron pairs arrange to minimize repulsion, defining geometry.
- Polarity: Assessed by geometry and bond dipoles.
- Hybridization: Determined by the number of electron regions around the central atom.