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### A. Electron Configuration of a Neutral Phosphorus Atom
The atomic number of phosphorus is 15, indicating it has 15 electrons in a neutral state. The electron configuration of phosphorus is:
Electron Configuration:
[tex]\[ \text{1s}^2 \text{2s}^2 \text{2p}^6 \text{3s}^2 \text{3p}^3 \][/tex]
### B. Lewis Diagram of the Hydrogen Phosphate Ion (HPO₄²⁻)
To draw the Lewis structure of the hydrogen phosphate ion (HPO₄²⁻), follow these steps:
1. Central Atom: Place the phosphorus (P) atom in the center.
2. Bonding: Arrange one oxygen (O) atom to form a double bond and three other oxygen atoms to form single bonds with the phosphorus atom.
3. Hydrogen: Attach a hydrogen (H) atom to one of the single-bonded oxygen atoms (forming an OH group).
4. Charges: The ion should also show that two of the oxygens have a negative charge (since it's a 2- charge ion).
The Lewis structure is represented as:
- P is located at the center bonded with:
- One O via a double bond
- Two Os via single bonds (each carrying a negative charge)
- One OH group via a single bond
### C. Potassium Dihydrogen Phosphate (KH₂PO₄) Analysis
(i) Molar Mass
To determine the molar mass (molecular weight) of potassium dihydrogen phosphate (KH₂PO₄), sum the atomic masses of all elements in the compound:
- Potassium (K): 39.10 g/mol
- Hydrogen (H): 1.01 g/mol (since there are two hydrogen atoms, it’s [tex]\(2 \times 1.01\)[/tex])
- Phosphorus (P): 30.97 g/mol
- Oxygen (O): 16.00 g/mol (since there are four oxygen atoms, it’s [tex]\(4 \times 16.00\)[/tex])
[tex]\[ \text{Molar Mass of } \text{KH₂PO₄} = 39.10 + 2(1.01) + 30.97 + 4(16.00) = 136.09 \, \text{g/mol} \][/tex]
(ii) Percentage Composition of Oxygen
The percentage composition of oxygen in potassium dihydrogen phosphate (KH₂PO₄) is calculated using the total molar mass of the compound and the mass of oxygen present:
[tex]\[ \text{Total mass of Oxygen} = 4 \times 16.00 = 64.00 \, \text{g/mol} \][/tex]
[tex]\[ \text{Percentage of Oxygen} = \left( \frac{64.00}{136.09} \right) \times 100 \approx 47.03 \, \% \][/tex]
(iii) Mass of Phosphorus in 150 g of KH₂PO₄
Given 150 grams of potassium dihydrogen phosphate, calculate the mass of phosphorus:
[tex]\[ \text{Mass of Phosphorus in KH₂PO₄} = \left( \frac{30.97}{136.09} \right) \times 150 \approx 34.14 \, \text{g} \][/tex]
### Summary
1. Electron Configuration of Phosphorus:
[tex]\[ \text{1s}^2 \text{2s}^2 \text{2p}^6 \text{3s}^2 \text{3p}^3 \][/tex]
2. Lewis Diagram of Hydrogen Phosphate (HPO₄²⁻):
- Central P bonded with:
- One double-bonded O
- Two single-bonded Os with negative charges
- One single-bonded OH group
3. Potassium Dihydrogen Phosphate Analysis:
- Molar Mass: 136.09 g/mol
- Percentage of Oxygen: 47.03%
- Mass of Phosphorus in 150 g: 34.14 g
### A. Electron Configuration of a Neutral Phosphorus Atom
The atomic number of phosphorus is 15, indicating it has 15 electrons in a neutral state. The electron configuration of phosphorus is:
Electron Configuration:
[tex]\[ \text{1s}^2 \text{2s}^2 \text{2p}^6 \text{3s}^2 \text{3p}^3 \][/tex]
### B. Lewis Diagram of the Hydrogen Phosphate Ion (HPO₄²⁻)
To draw the Lewis structure of the hydrogen phosphate ion (HPO₄²⁻), follow these steps:
1. Central Atom: Place the phosphorus (P) atom in the center.
2. Bonding: Arrange one oxygen (O) atom to form a double bond and three other oxygen atoms to form single bonds with the phosphorus atom.
3. Hydrogen: Attach a hydrogen (H) atom to one of the single-bonded oxygen atoms (forming an OH group).
4. Charges: The ion should also show that two of the oxygens have a negative charge (since it's a 2- charge ion).
The Lewis structure is represented as:
- P is located at the center bonded with:
- One O via a double bond
- Two Os via single bonds (each carrying a negative charge)
- One OH group via a single bond
### C. Potassium Dihydrogen Phosphate (KH₂PO₄) Analysis
(i) Molar Mass
To determine the molar mass (molecular weight) of potassium dihydrogen phosphate (KH₂PO₄), sum the atomic masses of all elements in the compound:
- Potassium (K): 39.10 g/mol
- Hydrogen (H): 1.01 g/mol (since there are two hydrogen atoms, it’s [tex]\(2 \times 1.01\)[/tex])
- Phosphorus (P): 30.97 g/mol
- Oxygen (O): 16.00 g/mol (since there are four oxygen atoms, it’s [tex]\(4 \times 16.00\)[/tex])
[tex]\[ \text{Molar Mass of } \text{KH₂PO₄} = 39.10 + 2(1.01) + 30.97 + 4(16.00) = 136.09 \, \text{g/mol} \][/tex]
(ii) Percentage Composition of Oxygen
The percentage composition of oxygen in potassium dihydrogen phosphate (KH₂PO₄) is calculated using the total molar mass of the compound and the mass of oxygen present:
[tex]\[ \text{Total mass of Oxygen} = 4 \times 16.00 = 64.00 \, \text{g/mol} \][/tex]
[tex]\[ \text{Percentage of Oxygen} = \left( \frac{64.00}{136.09} \right) \times 100 \approx 47.03 \, \% \][/tex]
(iii) Mass of Phosphorus in 150 g of KH₂PO₄
Given 150 grams of potassium dihydrogen phosphate, calculate the mass of phosphorus:
[tex]\[ \text{Mass of Phosphorus in KH₂PO₄} = \left( \frac{30.97}{136.09} \right) \times 150 \approx 34.14 \, \text{g} \][/tex]
### Summary
1. Electron Configuration of Phosphorus:
[tex]\[ \text{1s}^2 \text{2s}^2 \text{2p}^6 \text{3s}^2 \text{3p}^3 \][/tex]
2. Lewis Diagram of Hydrogen Phosphate (HPO₄²⁻):
- Central P bonded with:
- One double-bonded O
- Two single-bonded Os with negative charges
- One single-bonded OH group
3. Potassium Dihydrogen Phosphate Analysis:
- Molar Mass: 136.09 g/mol
- Percentage of Oxygen: 47.03%
- Mass of Phosphorus in 150 g: 34.14 g
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