6 posts • Page 1 of 1
Could someone explain why in 2.B.9 in the 7th edition, the Lewis structure for potassium phosphide has the P in the center with 8 electrons, and the K does not have any electrons and isn't attached to the P, but instead just floats around the P?
The fact that the potassium ions just float around the phosphorus indicate that the bonds between the atoms are considered ionic, therefore the phosphorus atoms possesses all of the atoms in the model. The way the potassium atoms are floating around the phosphorus I think is pretty arbitrary, they could be any orientation as long as they stay the correct number of degrees apart due to their electrostatic repulsion from each other. Hope that helps!
K3P is an ionic compound, so it is going to be a transfer of electrons. K has 1 valence electron and P has 5 valence electrons. K wants to lose its 1 valence electron so it will have a full, stable electron configuration that resembles [Ar]. P wants to gain 3 electrons in order to have a full, stable electron configuration that resembles [Ar]. There are three K atoms in this compound, so each one will donate an electron for a total of 3 electrons transferred to P. K does have electrons, but because the lone pairs in the drawing of ionic compounds only represent the valence electrons, and K's one valence electron has been transferred to the P ion, so K has no electrons around it but it is denoted with a + to represent that it has lost one electron. K is not attached to P because there is no sharing of electrons, and therefore no bonds formed. It is a complete transfer of electrons between the two.
Who is online
Users browsing this forum: No registered users and 1 guest