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### Question 5 (Electron Dot Structures)
#### a. Argon
# Explanation:
## Step1: Determine valence electrons
Argon (Ar) is a noble gas with atomic number 18. Its electron configuration is $1s^2 2s^2 2p^6 3s^2 3p^6$, so it has 8 valence electrons.
## Step2: Draw electron dot structure
Represent the symbol (Ar) and place 8 dots (4 pairs) around it: $	ext{Ar:} \overset{..}{..} \overset{..}{..}$ (or simply $	ext{Ar} \cdot\cdot\cdot\cdot \cdot\cdot\cdot\cdot$ with 8 dots, 2 on each side).
# Answer: $	ext{Ar} \cdot\cdot\cdot\cdot \cdot\cdot\cdot\cdot$ (8 dots, 2 on each of the four sides)

#### b. Calcium
# Explanation:
## Step1: Determine valence electrons
Calcium (Ca) has atomic number 20, electron configuration $[Ar] 4s^2$, so 2 valence electrons.
## Step2: Draw electron dot structure
Place 2 dots next to the Ca symbol: $	ext{Ca} \cdot\cdot$
# Answer: $	ext{Ca} \cdot\cdot$

#### c. Iodine
# Explanation:
## Step1: Determine valence electrons
Iodine (I) has atomic number 53, electron configuration $[Kr] 4d^{10} 5s^2 5p^5$, so 7 valence electrons.
## Step2: Draw electron dot structure
Place 7 dots around I, with 1 unpaired dot: $	ext{I} \cdot\cdot\cdot\cdot \cdot\cdot\cdot$ (7 dots, 3 pairs and 1 single)
# Answer: $	ext{I} \cdot\cdot\cdot\cdot \cdot\cdot\cdot$

#### d. Strontium
# Explanation:
## Step1: Determine valence electrons
Strontium (Sr) has atomic number 38, electron configuration $[Kr] 5s^2$, so 2 valence electrons.
## Step2: Draw electron dot structure
Place 2 dots next to Sr: $	ext{Sr} \cdot\cdot$
# Answer: $	ext{Sr} \cdot\cdot$

#### e. Xenon
# Explanation:
## Step1: Determine valence electrons
Xenon (Xe) is a noble gas with atomic number 54, electron configuration $[Kr] 4d^{10} 5s^2 5p^6$, so 8 valence electrons.
## Step2: Draw electron dot structure
Place 8 dots around Xe: $	ext{Xe} \cdot\cdot\cdot\cdot \cdot\cdot\cdot\cdot$
# Answer: $	ext{Xe} \cdot\cdot\cdot\cdot \cdot\cdot\cdot\cdot$

#### f. Tin
# Explanation:
## Step1: Determine valence electrons
Tin (Sn) has atomic number 50, electron configuration $[Kr] 4d^{10} 5s^2 5p^2$, so 4 valence electrons.
## Step2: Draw electron dot structure
Place 4 dots around Sn, with 2 unpaired (or arranged as 2 pairs and 2 singles, but typically 4 dots: $	ext{Sn} \cdot\cdot\cdot\cdot$)
# Answer: $	ext{Sn} \cdot\cdot\cdot\cdot$

### Question 6 (Octet Rule)
# Brief Explanations:
The octet rule states that atoms tend to gain, lose, or share electrons to achieve a stable electron configuration with 8 valence electrons (like noble gases, except H/He which follow a duet rule).
# Answer: Atoms tend to gain, lose, or share electrons to have 8 valence electrons (a stable octet, like noble gases).

### Question 7 (Metallic and Nonmetallic Atoms)
# Explanation:
## Step1: Metallic atoms behavior
Metallic atoms (like metals) have low electronegativity and few valence electrons, so they tend to **lose** valence electrons to form positive ions (cations).
## Step2: Nonmetallic atoms behavior
Nonmetallic atoms (nonmetals) can achieve an octet by gaining electrons (to form anions) or **sharing** electrons (in covalent bonds, e.g., in molecules like $	ext{H}_2	ext{O}$ or $	ext{CO}_2$).
# Answer: First blank: lose; Second blank: sharing

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QUESTION IMAGE

Question

Explanation:

Question 5 (Electron Dot Structures)

a. Argon

Step1: Determine valence electrons

Step2: Draw electron dot structure

Step1: Determine valence electrons

Step2: Draw electron dot structure

Step1: Determine valence electrons

Step2: Draw electron dot structure

Answer:

b. Calcium