A sample of seawater consists of water, sodium ions, chloride ions, and several other dissolved salts. These ions and salts are
1 answer:
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Answer:
B. BF₃
Explanation:
All the molecules have polar bonds, but a molecule will be nonpolar if the molecule has the symmetry that makes the bond dipoles cancel.
To make the decision, we must
- Draw the Lewis structure
- Assign the VSEPR electron geometry
- Determine the molecular shape.
- Examine the symmetry of the molecule
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<em>A. Water </em>
Lewis structure = H-O-H (2 bonding pairs, 2 lone pairs)
Electron geometry = AX₂E₂ tetrahedral
Molecular geometry = bent
Symmetry (see Figure A): The two O-H bonds are polar, with their negative ends pointing towards the O. The horizontal components of the bond dipoles cancel, but the vertical components reinforce each other and give an upward pointing molecular dipole. This is a <em>polar molecule with polar bonds</em>.
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<em>B. Boron trifluoride </em>
Lewis structure = BF₃ (3 bonding pairs)
Electron geometry = AX₃, trigonal planar
Molecular geometry = trigonal planar
Symmetry (see Figure B): The three B-F bonds are polar, with their negative ends pointing towards the F. The horizontal components of the bond dipoles cancel, but the vertical components of the two downward -pointing dipoles reinforce each other and give a resultant that is equal and opposite to the upward dipole. Thus, the bond dipoles cancel. This is a nonpolar molecule with polar bonds.
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<em>C. Ammonia</em>
Lewis structure = :NH₃ (3 bonding pairs, 1 lone pairs)
Electron geometry = AX₃E, tetrahedral
Molecular geometry = trigonal pyramidal
Symmetry (see Figure C): The three N-H bonds are polar, with their negative ends pointing towards the N. The horizontal components of the bond dipoles cancel, but the vertical components reinforce each other and give an upward pointing molecular dipole. This is a <em>polar molecule with polar bonds</em>.
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<em>D. Nitrogen trichloride </em>
Lewis structure = :NCl₃ (3 bonding pairs, 1 lone pair)
Electron geometry = AX₃E, tetrahedral
Molecular geometry = trigonal pyramidal
Symmetry (see Figure D): The three N-Cl bonds are polar, with their negative ends pointing towards the Cl. The horizontal components of the bond dipoles cancel, but the vertical components reinforce each other and give a downward pointing molecular dipole. This is a <em>polar molecule with polar bonds</em>.
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<em>E. Dichloromethane </em>
Lewis structure = H₂CCl₂ (4 bonding pairs)
Electron geometry = AX₄, tetrahedral
Molecular geometry = tetrahedral
Symmetry (see Figure E): The two C-H bonds are nonpolar, but the two C-Cl bonds are polar with their negative ends pointing towards the Cl. The horizontal components of the bond dipoles cancel, but the vertical components reinforce each other and give a downward pointing molecular dipole. This is a <em>polar molecule with polar bonds</em>.
Answer:
5. The mass of Na₂CO₃, that will produce 5 g of CO₂ is approximately 12.04 grams of Na₂CO₃
6. The mass of nitrogen gas (N₂) that will react completely with 150 g of hydrogen (H₂) in the production of NH₃ is 693. grams of N₂
Explanation:
5. The given equation for the formation of carbon dioxide (CO₂) from sodium bicarbonate (Na₂CO₃) is presented as follows;
(Na₂CO₃) + 2HCl → 2NaCl + CO₂ + H₂O
One mole (105.99 g) of Na₂CO₃ produces 1 mole (44.01 g) of CO₂
The mass, 'x' g of Na₂CO₃, that will produce 5 g of CO₂ is given by the law of definite proportions as follows;
The mass of Na₂CO₃, that will produce 5 g of CO₂, x ≈ 12.04 g
6. The chemical equation for the reaction is presented as follows;
N₂ + 3H₂ → 2NH₃
Therefore, one mole (28.01 g) of nitrogen gas, (N₂), reacts with three moles (3 × 2.02 g) of hydrogen gas (H₂) to produce 2 moles of ammonia (NH₃)
The mass 'x' grams of nitrogen gas (N₂) that will react completely with150 g of hydrogen (H₂) in the production of NH₃ is given as follows;
The mass of nitrogen gas (N₂) that will react completely with 150 g of hydrogen (H₂) in the production of NH₃, x = 693. grams