2) read the following graduated cylinders in milliliters. be specific!
a. ______ ml

b. ______ ml

use the periodic table to determine what charge the following elements have. (include a charge (+/-) and a number!) example sodium +1 oxygen -2

______ i

4) al ______

5) p ______

6) kr ______

7) k ______

draw the lewis dot model of each of the following elements.

______ ba

13) rn

14) te

15) k

16) he (crossed out)

draw the ionic bond that forms between the following atoms. use arrows to show the transfer of electrons. include charges after the transfer of electrons.

$\ce{al_{2}s_{3}}$

Question

2) read the following graduated cylinders in milliliters. be specific!
a. ______ ml

b. ______ ml

use the periodic table to determine what charge the following elements have. (include a charge (+/-) and a number!) example sodium +1 oxygen -2

______ i

4) al ______

5) p ______

6) kr ______

7) k ______

draw the lewis dot model of each of the following elements.

______ ba

13) rn

14) te

15) k

16) he (crossed out)

draw the ionic bond that forms between the following atoms. use arrows to show the transfer of electrons. include charges after the transfer of electrons.

$\ce{al_{2}s_{3}}$

Accepted Answer

### Part 2: Reading Graduated Cylinders

#### a.
# Explanation:
## Step1: Identify the scale
The graduated cylinder has markings at 60 and 70 mL. The space between 60 and 70 is divided into 10 equal parts (since it’s a typical graduated cylinder), so each small division is $ \frac{70 - 60}{10} = 1 $ mL.
## Step2: Read the meniscus
The bottom of the meniscus (the curved surface of the liquid) is at the 68 mL mark (counting 8 divisions above 60, as each division is 1 mL: $ 60 + 8 = 68 $).
# Answer:
68

#### b.
# Explanation:
## Step1: Identify the scale
The graduated cylinder has markings at 5, 10, 15, 20 mL. The space between 5 and 10, 10 and 15, 15 and 20 is divided into 5 equal parts, so each small division is $ \frac{10 - 5}{5} = 1 $ mL.
## Step2: Read the meniscus
The bottom of the meniscus is at the 9 mL mark (4 divisions above 5, since each division is 1 mL: $ 5 + 4 = 9 $).
# Answer:
9

### Part 3: Determining Element Charges (Using Periodic Table)

#### 3) Iodine (I)
# Explanation:
Iodine is in Group 17 (halogens) of the periodic table. Elements in Group 17 typically gain 1 electron to achieve a stable octet, so their charge is $ -1 $.
# Answer:
-1

#### 4) Aluminum (Al)
# Explanation:
Aluminum is in Group 13. Elements in Group 13 typically lose 3 electrons to achieve a stable octet, so their charge is $ +3 $.
# Answer:
+3

#### 5) Phosphorus (P)
# Explanation:
Phosphorus is in Group 15. Elements in Group 15 typically gain 3 electrons to achieve a stable octet, so their charge is $ -3 $.
# Answer:
-3

#### 6) Krypton (Kr)
# Explanation:
Krypton is a noble gas (Group 18). Noble gases are stable and do not typically form ions, so their charge is $ 0 $.
# Answer:
0

#### 7) Potassium (K)
# Explanation:
Potassium is in Group 1. Elements in Group 1 typically lose 1 electron to achieve a stable octet, so their charge is $ +1 $.
# Answer:
+1

### Part 4: Lewis Dot Models (Brief Explanations)

#### 12) Barium (Ba)
# Brief Explanations:
Barium is in Group 2, so it has 2 valence electrons. The Lewis dot model shows Ba with 2 dots (representing valence electrons) around it: $ \text{Ba} \cdot \cdot $ (or $ \dot{\text{Ba}}\dot{} $).
# Answer:
$ \text{Ba} \cdot \cdot $ (or equivalent Lewis dot notation with 2 valence electrons)

#### 13) Radon (Rn)
# Brief Explanations:
Radon is a noble gas (Group 18), so it has 8 valence electrons (a stable octet). The Lewis dot model shows Rn with 8 dots (or 4 pairs) around it: $ \text{Rn} : : : : $ (or $ \ddot{\text{Rn}}\ddot{} $ with 8 dots).
# Answer:
$ \text{Rn} : : : : $ (or equivalent Lewis dot notation with 8 valence electrons)

#### 14) Tellurium (Te)
# Brief Explanations:
Tellurium is in Group 16, so it has 6 valence electrons. The Lewis dot model shows Te with 6 dots (2 lone pairs and 2 unpaired electrons) around it: $ \text{Te} : : \cdot \cdot $ (or $ \ddot{\text{Te}}\cdot \cdot $).
# Answer:
$ \text{Te} : : \cdot \cdot $ (or equivalent Lewis dot notation with 6 valence electrons)

#### 15) Potassium (K)
# Brief Explanations:
Potassium is in Group 1, so it has 1 valence electron. The Lewis dot model shows K with 1 dot around it: $ \text{K} \cdot $
# Answer:
$ \text{K} \cdot $

#### 16) Helium (He) (Note: The “X” in the image might be a mistake, but He is a noble gas)
# Brief Explanations:
Helium is a noble gas with 2 valence electrons (a stable duet). The Lewis dot model shows He with 2 dots around it: $ \text{He} : $
# Answer:
$ \text{He} : $

### Part 5: Ionic Bond in $ \text{Al}_2\text{S}_3 $

# Explanation:
1. **Aluminum (Al)**: Group 13, loses 3 electrons → $ \text{Al}^{3+} $ (valence electrons: 3, donates 3).
2. **Sulfur (S)**: Group 16, gains 2 electrons → $ \text{S}^{2-} $ (valence electrons: 6, accepts 2).
3. **Electron Transfer**:
   - Each Al atom donates 3 electrons (total for 2 Al: $ 2 \times 3 = 6 $ electrons).
   - Each S atom accepts 2 electrons (total for 3 S: $ 3 \times 2 = 6 $ electrons).
   - Use arrows to show Al donating electrons to S:
     - $ \text{Al}
ightarrow \text{S} $ (3 arrows from Al to each S, but for simplicity, show the transfer leading to $ \text{Al}^{3+} $ and $ \text{S}^{2-} $, then form $ \text{Al}_2\text{S}_3 $ with charges $ (\text{Al}^{3+})_2 (\text{S}^{2-})_3 $).

# Answer:
- Aluminum atoms ($ \text{Al} $) lose 3 electrons each, forming $ \text{Al}^{3+} $ ions.
- Sulfur atoms ($ \text{S} $) gain 2 electrons each, forming $ \text{S}^{2-} $ ions.
- Electron transfer: $ 2 \text{Al} $ donate $ 6 $ electrons ( $ 2 \times 3 $ ) to $ 3 \text{S} $ ( $ 3 \times 2 $ electrons gained), resulting in the ionic compound $ \text{Al}_2\text{S}_3 $ with ions $ \text{Al}^{3+} $ and $ \text{S}^{2-} $.
(Visually, draw arrows from Al’s valence electrons to S’s valence electrons, then show the charged ions: $ \text{Al}^{3+} $ (with no valence electrons) and $ \text{S}^{2-} $ (with 8 valence electrons).)

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QUESTION IMAGE

Question

Explanation:

Part 2: Reading Graduated Cylinders

a.

Step1: Identify the scale

Step2: Read the meniscus

Step1: Identify the scale

Step2: Read the meniscus

Answer:

b.