Complete the following table: Formula Lewis Structure Data Wedge and Dash Drawing 1. CF3Cl Bonding electrons 4 Nonbonding electrons 0 Hybridization sp3 AXE notation AX4E0 Molecular geometry tetrahedral Polar or nonpolar polar Resonance no Isomers none 2. NH3 Bonding electrons Nonbonding electrons Hybridization AXE notation Molecular geometry Polar or nonpolar Resonance Isomers 3. H2O Bonding electrons Nonbonding electrons Hybridization AXE notation Molecular geometry Polar or nonpolar Resonance Isomers
The Correct Answer and Explanation is:
Let’s break down the table for each of the molecules:
1. CF3Cl (Chlorotrifluoromethane)
- Bonding electrons: 12 (Each C-F bond contributes 2 bonding electrons, and there are 3 C-F bonds. 1 C-Cl bond contributes 2 bonding electrons.)
- Nonbonding electrons: 0 (Carbon has no lone pairs; each fluorine and chlorine atom satisfies its valence requirement of 8 electrons.)
- Hybridization: sp³ (The central carbon atom forms four bonds, so it adopts sp³ hybridization.)
- AXE notation: AX₄ (A = central atom, X = bonded atoms, E = lone pairs)
- Molecular geometry: Tetrahedral (There are four bonding regions around the central carbon atom: 3 C-F bonds and 1 C-Cl bond.)
- Polar or nonpolar: Polar (CF3Cl has different atoms attached, which causes a dipole moment, making the molecule polar.)
- Resonance: No (There are no resonance structures in CF3Cl.)
- Isomers: None (There are no isomers for CF3Cl due to its simple structure.)
2. NH3 (Ammonia)
- Bonding electrons: 6 (3 N-H bonds, each contributing 2 bonding electrons.)
- Nonbonding electrons: 2 (The nitrogen atom has one lone pair.)
- Hybridization: sp³ (Nitrogen forms three bonds and has one lone pair, so it adopts sp³ hybridization.)
- AXE notation: AX₃E (A = nitrogen, X = hydrogen atoms, E = lone pair)
- Molecular geometry: Trigonal pyramidal (There are three bonding pairs and one lone pair, which pushes the hydrogen atoms down, resulting in a trigonal pyramidal shape.)
- Polar or nonpolar: Polar (The lone pair on nitrogen and the different electronegativities between nitrogen and hydrogen lead to a polar molecule.)
- Resonance: No (Ammonia does not exhibit resonance.)
- Isomers: None (Ammonia is a simple molecule with no isomers.)
3. H2O (Water)
- Bonding electrons: 8 (2 O-H bonds, each contributing 2 bonding electrons.)
- Nonbonding electrons: 4 (Oxygen has two lone pairs.)
- Hybridization: sp³ (Oxygen forms two bonds and has two lone pairs, so it adopts sp³ hybridization.)
- AXE notation: AX₂E₂ (A = oxygen, X = hydrogen atoms, E = lone pairs)
- Molecular geometry: Bent (Due to the two lone pairs, the molecule adopts a bent geometry with an ideal bond angle of 104.5°.)
- Polar or nonpolar: Polar (Water is a highly polar molecule due to the bent geometry and the large electronegativity difference between oxygen and hydrogen.)
- Resonance: No (Water does not exhibit resonance.)
- Isomers: None (There are no isomers for water.)
Explanation:
- Hybridization: Hybridization refers to the mixing of atomic orbitals to form new hybrid orbitals that can bond with other atoms. The type of hybridization (sp³, sp², sp) depends on the number of bonds and lone pairs around the central atom. For example, in CF3Cl, the central carbon is sp³ hybridized due to the four bonds it forms.
- AXE Notation: This is a shorthand used in VSEPR theory to describe the electron domain geometry of molecules. “A” is the central atom, “X” represents the surrounding atoms, and “E” represents lone pairs on the central atom. In NH3, the AXE notation is AX₃E because nitrogen has three bonds and one lone pair.
- Molecular Geometry: The molecular geometry describes the 3D arrangement of atoms in a molecule. For example, the geometry of NH3 is trigonal pyramidal due to the lone pair pushing down on the bonding atoms.
- Polarity: A molecule is polar if it has a net dipole moment, which occurs when the distribution of charge is uneven. This happens when atoms with different electronegativities are bonded together and the molecule has an asymmetrical shape. Water is polar because of its bent shape and the difference in electronegativity between oxygen and hydrogen.
