Looking for trustworthy answers? Westonci.ca is the ultimate Q&A platform where experts share their knowledge on various topics. Discover detailed answers to your questions from a wide network of experts on our comprehensive Q&A platform. Discover in-depth answers to your questions from a wide network of professionals on our user-friendly Q&A platform.
Sagot :
To determine which of the given ions is isoelectronic with \( P^{3-} \), we need to find the number of electrons in each ion and compare them with the number of electrons in \( P^{3-} \).
### Step-by-Step Solution:
1. Identify the atomic number of phosphorus (P):
- Phosphorus (P) has an atomic number of 15, which means a neutral phosphorus atom has 15 electrons.
2. Determine the number of electrons in \( P^{3-} \):
- The \( P^{3-} \) ion results when a neutral phosphorus atom gains 3 electrons. Therefore:
[tex]\[ 15 \text{ (original electrons)} + 3 \text{ (gained electrons)} = 18 \text{ electrons} \][/tex]
3. Calculate the number of electrons in each given ion:
- Ion: \( N^{3-} \)
- Nitrogen (N) has an atomic number of 7, so a neutral nitrogen atom has 7 electrons.
- As \( N^{3-} \), it gains 3 electrons:
[tex]\[ 7 \text{ (original electrons)} + 3 \text{ (gained electrons)} = 10 \text{ electrons} \][/tex]
- Ion: \( K^{+} \)
- Potassium (K) has an atomic number of 19, so a neutral potassium atom has 19 electrons.
- As \( K^{+} \), it loses 1 electron:
[tex]\[ 19 \text{ (original electrons)} - 1 \text{ (lost electron)} = 18 \text{ electrons} \][/tex]
- Ion: \( Na^{+} \)
- Sodium (Na) has an atomic number of 11, so a neutral sodium atom has 11 electrons.
- As \( Na^{+} \), it loses 1 electron:
[tex]\[ 11 \text{ (original electrons)} - 1 \text{ (lost electron)} = 10 \text{ electrons} \][/tex]
- Ion: \( O^{2-} \)
- Oxygen (O) has an atomic number of 8, so a neutral oxygen atom has 8 electrons.
- As \( O^{2-} \), it gains 2 electrons:
[tex]\[ 8 \text{ (original electrons)} + 2 \text{ (gained electrons)} = 10 \text{ electrons} \][/tex]
4. Compare the number of electrons:
- \( P^{3-} \) has 18 electrons.
- \( N^{3-} \) has 10 electrons.
- \( K^{+} \) has 18 electrons.
- \( Na^{+} \) has 10 electrons.
- \( O^{2-} \) has 10 electrons.
Only \( K^{+} \) has the same number of electrons (18) as \( P^{3-} \).
Therefore, the ion that is isoelectronic with [tex]\( P^{3-} \)[/tex] is [tex]\( K^{+} \)[/tex], which corresponds to option 2.
### Step-by-Step Solution:
1. Identify the atomic number of phosphorus (P):
- Phosphorus (P) has an atomic number of 15, which means a neutral phosphorus atom has 15 electrons.
2. Determine the number of electrons in \( P^{3-} \):
- The \( P^{3-} \) ion results when a neutral phosphorus atom gains 3 electrons. Therefore:
[tex]\[ 15 \text{ (original electrons)} + 3 \text{ (gained electrons)} = 18 \text{ electrons} \][/tex]
3. Calculate the number of electrons in each given ion:
- Ion: \( N^{3-} \)
- Nitrogen (N) has an atomic number of 7, so a neutral nitrogen atom has 7 electrons.
- As \( N^{3-} \), it gains 3 electrons:
[tex]\[ 7 \text{ (original electrons)} + 3 \text{ (gained electrons)} = 10 \text{ electrons} \][/tex]
- Ion: \( K^{+} \)
- Potassium (K) has an atomic number of 19, so a neutral potassium atom has 19 electrons.
- As \( K^{+} \), it loses 1 electron:
[tex]\[ 19 \text{ (original electrons)} - 1 \text{ (lost electron)} = 18 \text{ electrons} \][/tex]
- Ion: \( Na^{+} \)
- Sodium (Na) has an atomic number of 11, so a neutral sodium atom has 11 electrons.
- As \( Na^{+} \), it loses 1 electron:
[tex]\[ 11 \text{ (original electrons)} - 1 \text{ (lost electron)} = 10 \text{ electrons} \][/tex]
- Ion: \( O^{2-} \)
- Oxygen (O) has an atomic number of 8, so a neutral oxygen atom has 8 electrons.
- As \( O^{2-} \), it gains 2 electrons:
[tex]\[ 8 \text{ (original electrons)} + 2 \text{ (gained electrons)} = 10 \text{ electrons} \][/tex]
4. Compare the number of electrons:
- \( P^{3-} \) has 18 electrons.
- \( N^{3-} \) has 10 electrons.
- \( K^{+} \) has 18 electrons.
- \( Na^{+} \) has 10 electrons.
- \( O^{2-} \) has 10 electrons.
Only \( K^{+} \) has the same number of electrons (18) as \( P^{3-} \).
Therefore, the ion that is isoelectronic with [tex]\( P^{3-} \)[/tex] is [tex]\( K^{+} \)[/tex], which corresponds to option 2.
We appreciate your time on our site. Don't hesitate to return whenever you have more questions or need further clarification. We hope you found what you were looking for. Feel free to revisit us for more answers and updated information. Discover more at Westonci.ca. Return for the latest expert answers and updates on various topics.
