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Chapter 1: Problem 68

Phosphorus is immediately under nitrogen in the Periodic Table. Predict the molecular formula for phosphine, the compound formed by phosphorus and hydrogen. Predict the H-P-H bond angle in phosphine.

Short Answer

Expert verified
Answer: The molecular formula of phosphine is PH3, and the approximate H-P-H bond angle within this compound is 107.3 degrees.

Step by step solution

01

Identify the group number for elements

Identify the group number of phosphorus in the periodic table. Phosphorus is in Group 15, right below nitrogen.
02

Determine the number of valence electrons

Since phosphorus is in Group 15, it has 5 valence electrons. Hydrogen, on the other hand, has only 1 valence electron (as it is in Group 1).
03

Determine the molecular formula of phosphine

To form a compound, the atoms will share electrons to achieve a stable electron configuration. In the case of phosphorus, it needs 3 more valence electrons to complete its octet (eight electrons in the valence shell, except for hydrogen which only needs a duet - two electrons). Hydrogen, being in Group 1, needs one more electron to form a duet for stability. As a result, one phosphorus atom will bond with three hydrogen atoms, each sharing one electron pair with phosphorus. Thus, the molecular formula for phosphine is PH3.
04

Predict the H-P-H bond angle

In phosphine (PH3), the central atom (phosphorus) is surrounded by three hydrogen atoms. To minimize electron repulsion between bonding pairs, the hydrogen atoms will arrange themselves in a trigonal pyramidal geometry around the phosphorus atom. In a trigonal pyramidal molecular geometry, the H-P-H bond angle will be approximately 107.3 degrees.

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