Do PCl5 have 3 lone pairs for each Cl? and 1 lone pair for P ??
Each Cl has 3 lone pairs but P has no lone pairs.
P has 5 e.
Cl has 5 x 7 = 35
total e = 40
Count the 6 around each Cl and that accounts for 30 electrons. Then count 10 more for the 5 bonds for each P-Cl and that is the 40 electrons available.
To determine the number of lone pairs in PCl5, let's first look at the Lewis structure of PCl5.
In the Lewis structure of PCl5, phosphorus (P) is the central atom, and it forms bonds with five chlorine (Cl) atoms. Each chlorine atom is bonded to phosphorus by a single covalent bond. The total number of valence electrons can be calculated as follows:
Phosphorus (P) has 5 valence electrons (group 15 element).
Chlorine (Cl) has 7 valence electrons each (group 17 element).
So, the total number of electrons for PCl5 would be:
5 + (7 x 5) = 40 valence electrons.
For each covalent bond, two electrons are shared between the participating atoms. Since there are five covalent bonds in PCl5, a total of 10 electrons would be used to form these bonds.
To distribute the remaining 30 electrons, we start by placing one electron around each atom, and then pairing up the remaining electrons. After distributing all the electrons, the Lewis structure of PCl5 would look like:
PCl5 Lewis structure:
:Cl: :Cl: :Cl: :Cl: :Cl:
P
In this Lewis structure, each chlorine atom has 3 lone pairs (6 electrons), and phosphorus has 1 lone pair (2 electrons).
So, to answer your question:
- Yes, each chlorine atom has 3 lone pairs in PCl5.
- And PCl5 has 1 lone pair on the phosphorus atom.
To determine the number of lone pairs on each atom in PCl5, we need to examine the Lewis structure of the molecule.
The Lewis structure of PCl5 consists of one phosphorus atom (P) bonded to five chlorine atoms (Cl). Since each chlorine atom forms a single bond with phosphorus, we have a total of five bonds.
Next, we need to determine the number of lone pairs.
The valence electron configuration of chlorine (Cl) is [2s2 2p6 3s2 3p5], and the valence electron configuration of phosphorus (P) is [3s2 3p3]. For all the chlorine atoms, they each form a single bond with phosphorus by sharing a pair of electrons. This accounts for 10 electrons (5 pairs) in total.
Now, in order to complete the octet around phosphorus, it needs a total of 5 more electrons. These electrons can be obtained from lone pairs. Since each lone pair consists of two electrons, phosphorus requires 2.5 lone pairs, which is not physically possible. Therefore, PCl5 does not have any lone pairs on phosphorus.
In summary, PCl5 has no lone pairs on phosphorus (P), and each chlorine atom (Cl) does not have three lone pairs either.