1. identify each property below as more typical of a metal or a nonmetal.
a. gas at room temperature
b. brittle
c. malleable
d. poor conductor of electric current
e. shiny
2. to which group in the periodic table does each of the following elements belong? how many valence electrons do atoms of each element have?
a. nitrogen
b. lithium
c. phosphorus
d. barium
e. bromine
f. carbon
3. write electron dot structures for each of the following elements:
a. cl
b. s
c. al
d. li
4. describe two ways that an ion forms from an atom.
5. explain why ionic compounds are electrically neutral.

Question

1. identify each property below as more typical of a metal or a nonmetal.
   a. gas at room temperature
   b. brittle
   c. malleable
   d. poor conductor of electric current
   e. shiny
2. to which group in the periodic table does each of the following elements belong? how many valence electrons do atoms of each element have?
   a. nitrogen
   b. lithium
   c. phosphorus
   d. barium
   e. bromine
   f. carbon
3. write electron dot structures for each of the following elements:
   a. cl
   b. s
   c. al
   d. li
4. describe two ways that an ion forms from an atom.
5. explain why ionic compounds are electrically neutral.

Accepted Answer

### Question 1
#### Part a
# Explanation:
## Step1: Recall metal/nonmetal states
Metals are solid (except Hg), nonmetals often gas.
## Step2: Determine category
Gas at room temp: nonmetal (most nonmetals like O, N are gas; metals solid except Hg).
# Answer: nonmetal

#### Part b
# Explanation:
## Step1: Recall metal/nonmetal brittleness
Metals are malleable, nonmetals brittle.
## Step2: Determine category
Brittle: nonmetal (nonmetals break easily, metals deform).
# Answer: nonmetal

#### Part c
# Explanation:
## Step1: Recall metal malleability
Malleable means can be hammered into sheets, a metal property.
## Step2: Determine category
Malleable: metal (metals are malleable, nonmetals brittle).
# Answer: metal

#### Part d
# Explanation:
## Step1: Recall metal/nonmetal conductivity
Metals are good conductors, nonmetals poor.
## Step2: Determine category
Poor conductor: nonmetal (nonmetals don’t conduct well, metals do).
# Answer: nonmetal

#### Part e
# Explanation:
## Step1: Recall metal luster
Metals are shiny (lustrous), nonmetals dull (mostly).
## Step2: Determine category
Shiny: metal (metals have metallic luster).
# Answer: metal

### Question 2
#### Part a: Nitrogen (N)
# Explanation:
## Step1: Locate N on periodic table
Nitrogen is in group 15 (VA).
## Step2: Calculate valence electrons
Group 15 elements have 5 valence electrons (group number - 10 for groups 13 - 18: 15 - 10 = 5).
# Answer: Group 15 (VA), 5 valence electrons

#### Part b: Lithium (Li)
# Explanation:
## Step1: Locate Li on periodic table
Lithium is in group 1 (IA).
## Step2: Calculate valence electrons
Group 1 elements have 1 valence electron.
# Answer: Group 1 (IA), 1 valence electron

#### Part c: Phosphorus (P)
# Explanation:
## Step1: Locate P on periodic table
Phosphorus is in group 15 (VA).
## Step2: Calculate valence electrons
Group 15: 15 - 10 = 5 valence electrons.
# Answer: Group 15 (VA), 5 valence electrons

#### Part d: Barium (Ba)
# Explanation:
## Step1: Locate Ba on periodic table
Barium is in group 2 (IIA).
## Step2: Calculate valence electrons
Group 2 elements have 2 valence electrons.
# Answer: Group 2 (IIA), 2 valence electrons

#### Part e: Bromine (Br)
# Explanation:
## Step1: Locate Br on periodic table
Bromine is in group 17 (VIIA).
## Step2: Calculate valence electrons
Group 17: 17 - 10 = 7 valence electrons.
# Answer: Group 17 (VIIA), 7 valence electrons

#### Part f: Carbon (C)
# Explanation:
## Step1: Locate C on periodic table
Carbon is in group 14 (IVA).
## Step2: Calculate valence electrons
Group 14: 14 - 10 = 4 valence electrons.
# Answer: Group 14 (IVA), 4 valence electrons

### Question 3
#### Part a: Cl (Chlorine)
# Explanation:
## Step1: Determine valence electrons
Cl has 7 valence electrons (group 17).
## Step2: Draw electron dot structure
Place 7 dots around Cl, one on each side (up, right, down, left) then pair: $\cdot \underset{\cdot \cdot}{\overset{\cdot \cdot}{Cl}} \cdot$
# Answer: $\cdot \underset{\cdot \cdot}{\overset{\cdot \cdot}{Cl}} \cdot$

#### Part b: S (Sulfur)
# Explanation:
## Step1: Determine valence electrons
S has 6 valence electrons (group 16).
## Step2: Draw electron dot structure
Place 6 dots: $\cdot \underset{\cdot \cdot}{\overset{\cdot \cdot}{S}} \cdot \cdot$
# Answer: $\cdot \underset{\cdot \cdot}{\overset{\cdot \cdot}{S}} \cdot \cdot$

#### Part c: Al (Aluminum)
# Explanation:
## Step1: Determine valence electrons
Al has 3 valence electrons (group 13).
## Step2: Draw electron dot structure
Place 3 dots: $\cdot 	ext{Al} \cdot \cdot$
# Answer: $\cdot 	ext{Al} \cdot \cdot$

#### Part d: Li (Lithium)
# Explanation:
## Step1: Determine valence electrons
Li has 1 valence electron (group 1).
## Step2: Draw electron dot structure
Place 1 dot: $\cdot 	ext{Li}$
# Answer: $\cdot 	ext{Li}$

### Question 4
# Explanation:
## Step1: Define ion formation
Ions form when atoms gain or lose electrons.
## Step2: Explain two ways
1. **Losing electrons**: Metals (low ionization energy) lose valence electrons to form positive ions (cations, e.g., $	ext{Na}
ightarrow 	ext{Na}^+ + e^-$).
2. **Gaining electrons**: Nonmetals (high electron affinity) gain electrons to form negative ions (anions, e.g., $	ext{Cl} + e^-
ightarrow 	ext{Cl}^-$).
# Answer: An ion forms when an atom (1) **loses electrons** (forming a cation, e.g., $	ext{Na}
ightarrow 	ext{Na}^+ + e^-$) or (2) **gains electrons** (forming an anion, e.g., $	ext{Cl} + e^-
ightarrow 	ext{Cl}^-$).

### Question 5
# Explanation:
## Step1: Define ionic compound
Ionic compounds are made of cations (positive) and anions (negative).
## Step2: Explain charge balance
The total positive charge from cations equals the total negative charge from anions. For example, in $	ext{NaCl}$, 1 $	ext{Na}^+$ ( +1) and 1 $	ext{Cl}^-$ ( -1) balance to zero. In $	ext{CaCl}_2$, 1 $	ext{Ca}^{2+}$ ( +2) and 2 $	ext{Cl}^-$ ( 2×-1 = -2) balance.
# Answer: Ionic compounds are electrically neutral because the **total positive charge of cations** equals the **total negative charge of anions** in the compound. For example, $	ext{NaCl}$ has 1 $	ext{Na}^+$ (+1) and 1 $	ext{Cl}^-$ (-1), so net charge = 0.

Sovi.AI - AI Math Tutor

QUESTION IMAGE

Question

Explanation:

Question 1

Part a

Step1: Recall metal/nonmetal states

Step2: Determine category

Step1: Recall metal/nonmetal brittleness

Step2: Determine category

Step1: Recall metal malleability

Step2: Determine category

Answer:

Part b