name: homework
phosphorus trichloride is a slightly yellow fuming liquid with a pungent and irritating odor. when it comes into contact with water, it reacts violently with water. challenge why are actual covalent molecules like this when we draw them with the octet rule. phosphorus trichloride is an important reagent in the production of pesticides. phosphorus trichloride is used to produce pesticides such as parathion in the production of pesticides.
p₄ + 6cl₂→4pcl₃
17. *draw the lewis dot diagram for phosphorus trichloride.
18. *what is the shape of phosphorus trichloride according to the vsepr theory?
19. *is phosphorus trichloride a polar or nonpolar molecule? justify your response.
20. draw the lewis dot diagram for chlorine, cl₂.
21. draw the lewis dot diagram for calcium chloride.
when chlorine reacts with calcium, calcium chloride is formed.

Question

Accepted Answer

### 17.
# Explanation:
## Step1: Count total valence electrons
Phosphorus (P): 5 valence electrons; Each chlorine (Cl): 7 valence electrons. Total = $5 + 3	imes7 = 26$
## Step2: Place central atom, form bonds
Place P as central atom, form 3 P-Cl single bonds. Electrons used: $3	imes2=6$, remaining: $26-6=20$
## Step3: Assign lone pairs to outer atoms
Each Cl gets 3 lone pairs ($3	imes6=18$ electrons). Remaining electrons: $20-18=2$, assign to P as 1 lone pair.
# Answer:
Lewis dot diagram for $	ext{PCl}_3$:
```
      ..
:Cl:P:Cl:
      ..
      :Cl:
      ..
```
(Note: The central P has one lone pair, each Cl has three lone pairs, and single bonds connect P to each Cl.)

---

### 18.
# Explanation:
## Step1: Identify electron domains
$	ext{PCl}_3$ has 3 bonding pairs + 1 lone pair = 4 total electron domains.
## Step2: Apply VSEPR theory
4 electron domains correspond to tetrahedral electron geometry. With 1 lone pair, molecular shape is trigonal pyramidal.
# Answer:
Trigonal pyramidal

---

### 19.
# Explanation:
## Step1: Analyze molecular symmetry
$	ext{PCl}_3$ has a trigonal pyramidal shape. The P-Cl bonds are polar (Cl is more electronegative than P).
## Step2: Check dipole moment cancellation
The polar bonds are not symmetrically arranged; their individual dipole moments do not cancel out, creating a net molecular dipole moment.
# Answer:
$	ext{PCl}_3$ is a polar molecule. The trigonal pyramidal geometry means the polar P-Cl bond dipoles do not cancel, resulting in a net molecular dipole moment.

---

### 20.
# Explanation:
## Step1: Count total valence electrons
Chlorine (Cl): 7 valence electrons per atom. Total for $	ext{Cl}_2$: $2	imes7=14$
## Step2: Form bond and assign lone pairs
Form a single Cl-Cl bond (uses 2 electrons). Each Cl gets 3 lone pairs ($2	imes6=12$ electrons) to satisfy octet rule.
# Answer:
Lewis dot diagram for $	ext{Cl}_2$:
```
:Cl:Cl:
    ..
```
(Note: A single bond connects the two Cl atoms, and each Cl has three lone pairs of electrons.)

---

### 21.
# Explanation:
## Step1: Identify ion charges
Calcium (Ca) forms $	ext{Ca}^{2+}$; Chlorine (Cl) forms $	ext{Cl}^-$.
## Step2: Balance charges for neutral compound
2 $	ext{Cl}^-$ ions balance 1 $	ext{Ca}^{2+}$ ion.
## Step3: Draw ionic Lewis diagram
Show cation and anion with brackets, charge labels, and valence electrons on anion.
# Answer:
Lewis dot diagram for $	ext{CaCl}_2$:
$[	ext{Ca}]^{2+} \quad 2[:\ddot{	ext{Cl}}:]^-$

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QUESTION IMAGE

Question

Explanation:

17.

Step1: Count total valence electrons

Step2: Place central atom, form bonds

Step3: Assign lone pairs to outer atoms

Step1: Identify electron domains

Step2: Apply VSEPR theory

Step1: Analyze molecular symmetry

Step2: Check dipole moment cancellation

Answer:

18.