White phosphorous has the chemical formula p4(s). a p4 molecule has 20 valence electrons. draw a lewis formula for a white phosp
horous molecule in which none of the atoms violates the octet rule and the formal charge on each atom is zero. there are no pi bonds in the structure.
1 answer:
The Lewis structure of P₄ is shown in 3-D form. The two bottom corner P atoms are facing right in front of us, one P atom behind the two, and one P above it. Each line represents 2 electrons. When you add the lone electrons, you get a total of 20 valence electrons.
Formal charge of each P: 5 - (2 +1/2*6) = 0
Formal charge of each P: 5 - (2 +1/2*6) = 0
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Answer:
640.32 g
Explanation:
2KClO₃ → 2KCl + 3O₂
First we <u>convert KClO₃ moles to O₂ moles,</u> using the <em>stoichiometric coefficients</em>:
- 13.34 mol KClO₃ *
= 20.01 mol O₂
Then we <u>convert O₂ moles to grams</u>, using its <em>molar mass</em>:
- 20.01 mol O₂ * 32 g/mol = 640.32 g
So 640.32 g of O₂ are formed from 13.34 moles of KClO₃.