q2 chemistry: u4l11 covalent lewis dot diagram day 2
5. **nitrogen triiodide
a. ionic or covalent?
b. formula:
c. lewis dot diagram:
6. *lithium sulfide
a. ionic or covalent?
b. formula:
c. lewis dot diagram:
7. **explain the bond from question 5 in terms of electron movement and electronegativity.
8. explain the bond from question 6 in terms of electron movement and electronegativity.

Question

q2 chemistry: u4l11 covalent lewis dot diagram day 2
5. **nitrogen triiodide
  a. ionic or covalent?
  b. formula:
  c. lewis dot diagram:
6. *lithium sulfide
  a. ionic or covalent?
  b. formula:
  c. lewis dot diagram:
7. **explain the bond from question 5 in terms of electron movement and electronegativity.
8. explain the bond from question 6 in terms of electron movement and electronegativity.

Accepted Answer

### Question 5: Nitrogen triiodide
#### a. Ionic or covalent?
# Brief Explanations:
Nitrogen (N) and iodine (I) are both nonmetals. Covalent bonds form between nonmetals as they share electrons.
# Answer:
Covalent

#### b. Formula:
# Explanation:
## Step1: Identify elements and prefixes
Nitrogen (N) has no prefix (implies 1), triiodide means 3 iodine (I) atoms.
## Step2: Combine symbols with subscripts
Formula is $NI_3$.
# Answer:
$NI_3$

#### c. Lewis dot diagram:
# Explanation:
## Step1: Valence electrons
Nitrogen has 5 valence electrons, each iodine has 7. Total valence electrons: $5 + 3	imes7 = 26$.
## Step2: Bonding structure
N is central. Single bonds between N and each I (3 bonds, using 6 electrons). Remaining electrons: $26 - 6 = 20$. N has 2 non - bonding electrons (lone pair), each I has 6 non - bonding electrons (3 lone pairs).
## Step3: Draw the diagram
N in the center, 3 I atoms around it. Each N - I is a single bond (2 electrons). N has a lone pair (2 electrons), each I has 3 lone pairs (6 electrons each).
# Answer:
```
    ..
: I - N - I :
    ..   ..
: I :
    ..
```
(Note: The dots are arranged as lone pairs around each atom. The N has one lone pair, each I has three lone pairs, and there are single bonds between N and each I.)

### Question 6: Lithium sulfide
#### a. Ionic or covalent?
# Brief Explanations:
Lithium (Li) is a metal, sulfur (S) is a nonmetal. Ionic bonds form between metals and nonmetals as electrons are transferred.
# Answer:
Ionic

#### b. Formula:
# Explanation:
## Step1: Determine charges
Li has a +1 charge ($Li^+$), S has a - 2 charge ($S^{2 - }$).
## Step2: Balance charges
To balance, we need 2 $Li^+$ for 1 $S^{2 - }$. So formula is $Li_2S$.
# Answer:
$Li_2S$

#### c. Lewis dot diagram:
# Explanation:
## Step1: Ions and electrons
$Li^+$ has no valence electrons (lost 1), $S^{2 - }$ has 8 valence electrons (gained 2).
## Step2: Draw the diagram
Two $Li^+$ ions (represented as $Li^+$) and one $S^{2 - }$ ion. The $S^{2 - }$ has 8 electrons (4 lone pairs) around it, and the $Li^+$ ions are associated with the $S^{2 - }$ ion.
## Step3: Representation
$[Li^+] \quad [: \ddot{S}:]^{2 - } \quad [Li^+]$ (the dots around S represent the 8 valence electrons in the stable octet).
# Answer:
$[Li^+] \quad [: \ddot{S}:]^{2 - } \quad [Li^+]$ (with the dots around S arranged as four lone pairs)

### Question 7: Explain bond in $NI_3$ (question 5)
# Brief Explanations:
- Electronegativity: N (3.04) and I (2.66) have similar electronegativities.
- Electron movement: Since electronegativities are close, they share electrons. The bonding electrons are shared between N and each I atom, forming covalent bonds. The difference in electronegativity is small, so electron sharing is relatively equal (polar covalent, but still sharing).
# Answer:
Nitrogen and iodine have relatively similar electronegativities (N: ~3.04, I: ~2.66). In the covalent bond of $NI_3$, electrons are shared between the nitrogen and each iodine atom. Since the electronegativity difference is small, the bonding electrons are not fully transferred but are shared, with a slight pull towards the more electronegative nitrogen, resulting in a polar covalent bond.

### Question 8: Explain bond in $Li_2S$ (question 6)
# Brief Explanations:
- Electronegativity: Li (0.98) is much less electronegative than S (2.58).
- Electron movement: Lithium atoms (metals) transfer their valence electrons (1 each) to the sulfur atom (nonmetal). Each Li loses 1 electron (becomes $Li^+$), and S gains 2 electrons (becomes $S^{2 - }$). The electrostatic attraction between the positive $Li^+$ ions and negative $S^{2 - }$ ion forms the ionic bond.
# Answer:
Lithium is a metal with low electronegativity (0.98) and sulfur is a nonmetal with higher electronegativity (2.58). In $Li_2S$, each lithium atom transfers its single valence electron to the sulfur atom. Two lithium atoms (each losing 1 electron to form $Li^+$) and one sulfur atom (gaining 2 electrons to form $S^{2 - }$) are involved. The electrostatic attraction between the positively charged $Li^+$ ions and the negatively charged $S^{2 - }$ ion creates the ionic bond.

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QUESTION IMAGE

Question

Explanation:

Question 5: Nitrogen triiodide

a. Ionic or covalent?

Step1: Identify elements and prefixes

Step2: Combine symbols with subscripts

Step1: Valence electrons

Step2: Bonding structure

Step3: Draw the diagram

Answer:

b. Formula: