The Lewis structure of PF3 shows that the central phosphorus atom has __________ nonbonding and __________ bonding electron pairs.
Is the answer 1, 3
Is it 1 because it asked for PAIRS- so there are two electrons not bonded- so one pair?
Yes, I think so. The person making the question could have made it clearer by writing "phosphorus atom has ???? non-bonding electron pairs and ?????bonding electron pairs."
https://www.google.com/search?q=lewis+structure+PF3&hl=en&client=firefox-a&hs=deY&tbo=u&rls=org.mozilla:en-US:official&tbm=isch&source=univ&sa=X&ei=70fzUNzgFbP02wXQtoDIDA&ved=0CEsQsAQ&biw=846&bih=468
Thank you sir.
Sorry for the confusion, but the correct answer is actually 1 nonbonding and 3 bonding electron pairs. In the Lewis structure of PF3, phosphorus atom is surrounded by three fluorine atoms. Each fluorine contributes one electron to form a covalent bond with phosphorus, resulting in three bonding electron pairs. Phosphorus also has one lone pair of electrons, which are nonbonding. So, there is one nonbonding electron pair and three bonding electron pairs around the central phosphorus atom.
The Lewis structure of PF3 shows that the central phosphorus atom has 1 nonbonding and 3 bonding electron pairs.
To determine this, you need to know the Lewis structure of PF3. Here's how you can construct it:
1. Start by counting the total number of valence electrons for each atom. Phosphorus (P) is in Group 15 of the periodic table, so it has 5 valence electrons. Fluorine (F) is in Group 17, so each fluorine atom contributes 7 valence electrons. In total, you have 5 valence electrons (from P) + 3(7) valence electrons (from F) = 26 valence electrons.
2. Place the least electronegative atom (phosphorus) at the center and connect the other atoms (fluorine) to it using single bonds. In this case, there are three fluorine atoms bonded to phosphorus, so you will have three single bonds between P and F.
3. Distribute the remaining valence electrons around the atoms to satisfy the octet rule (except for hydrogen, which can only accommodate 2 electrons). In this case, each fluorine atom has 8 electrons around it, and phosphorus has 10 electrons around it.
4. If there are any remaining valence electrons, place them on the central atom as lone pairs until the octet rule is satisfied for the central atom. In this case, you have 6 remaining valence electrons that need to be placed on the central phosphorus atom.
By following these steps, you will find that the Lewis structure of PF3 has one lone pair of electrons on the phosphorus atom. Therefore, the answer is 1 nonbonding and 3 bonding electron pairs.