91影视

To draw the Lewis structures of these three species, we need to follow some basic steps: - Count the total available valence electrons. - Assign pairs of electrons to the central atom to fulfill the octet rule. - Arrange the remaining electrons around the outer atoms to also satisfy the octet rule.

1. The total valence electrons are \[5 (N) + 3 \times 1 (H) = 8\text{ electrons}\]. 2. Nitrogen is the central atom, surrounded by three Hydrogen atoms. 3. Distribute the remaining valence electrons: Nitrogen shares three pairs of electrons with three Hydrogen atoms, forming three single bonds (N-H). Nitrogen also has one lone pair of electrons left. The structure is: ``` H | H--N--H ```

1. The total valence electrons are \[5 (As) + 5 \times 7 (Cl) = 40\text{ electrons}\]. 2. Arsenic (As) is the central atom, surrounded by five Chlorine (Cl) atoms. 3. Distribute the remaining valence electrons: Each Chlorine atom shares a pair of electrons with Arsenic, forming five single bonds (As-Cl). Each Chlorine atom also has three lone pairs of electrons. The structure is: ``` Cl | Cl--As--Cl / \ Cl Cl ```

1. The total valence electrons are \[5 (P) + 6 \times 7 (F) + 1 (\text{extra e鈦粆) = 48\text{ electrons}\]. 2. Phosphorus (P) is the central atom, surrounded by six Fluorine (F) atoms. 3. Distribute the remaining valence electrons: Each Fluorine shares one pair of electrons with Phosphorus, forming six single bonds (P-F). Each Fluorine atom also has three lone pairs of electrons. The structure is: ``` F | F--P--F / \ F F \ F ```

Now that we have the Lewis structures, we can predict the molecular geometries using the VSEPR theory, which states that electron pairs repel each other to get their geometry. - 狈贬鈧�: Nitrogen is surrounded by three bonding pairs and one lone pair, which gives it an electron geometry of tetrahedral. However, considering only bond pairs, the molecular shape is trigonal pyramidal. The hybridization would be sp鲁 since there are four electron pairs. - 础蝉颁濒鈧�: Arsenic is surrounded by five bonding pairs. Thus, the electron geometry is trigonal bipyramidal. The molecular shape is also trigonal bipyramidal, and the hybridization would be sp鲁d. - 笔贵鈧嗏伝: Phosphorus is surrounded by six bonding pairs, giving it an electron geometry of octahedral. The molecular shape is octahedral as well, and the hybridization would be sp鲁d虏.

- NF鈧�: Nitrogen is a very small atom, with a valence electron shell (n=2) that can accommodate only four orbitals: one s and three p orbitals. In order to form five bonds with Fluorine (F), Nitrogen would need five orbitals (sp鲁d), which is not possible for Nitrogen since it lacks available d orbitals. Furthermore, F is highly electronegative, which would lead to increased electron repulsion in such a compact structure. - NCl鈧嗏伝: Similar to NF鈧�, Nitrogen's valence shell doesn't have enough orbitals to form six bonds with Chlorine (Cl) atoms, as it would require six orbitals (sp鲁d虏) and Nitrogen lacks d orbitals.