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faust18 [17]
3 years ago
6

Using VSEPR theory which of the following would be the correct shape for nitrogen trifluoride?

Chemistry
1 answer:
RUDIKE [14]3 years ago
6 0

Answer:

trigonal pyramidal

Explanation:

In NF3, the nitrogen atom is sp3 hybridized. Now we must remember that according to the VSEPR theory, the number of electron pairs in the valence shell of the central atom in a molecule determines its shape.

Here, the nitrogen atom is the central atom and its outermost shell is surrounded by four electron pairs - one lone pair and three bond pairs. This means that it has a tetrahedral electron pair geometry.

However, due to the lone pair, the three fluorine atoms are arranged in a  trigonal pyramidal geometry. Hence the correct shape of the molecule is trigonal pyramidal.

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Answer:

436.8 mmHg.

Explanation:

From the question given above, the following data were obtained:

Total pressure (Pₜ) = 0.93 atm

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Pressure of O₂ (Pₒ₂) =?

Next, we shall convert the total pressure to mmHg . This can be obtained as follow:

1 atm = 760 mmHg

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0.93 atm = 0.93 × 760 mmHg / 1 atm

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Finally, we shall determine the pressure of the O₂. This can be obtained as follow:

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Pₜ = Pₙ₂ + Pₒ₂

706.8 = 270 + Pₒ₂

Collect like terms

706.8 – 270 = Pₒ₂

436.8 = Pₒ₂

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