Phosphine is a very toxic gaseous compound. In phosphine (PH3) lewis structure, there are three sigma bonds and one lone-pair around phosphorous atom. No charges on phosphorous atom and hydrogen atoms. Shape of PH3 is trigonal pyramidal. Molecular geometry around phosphorous atom is tetrahedral. Total valence electrons pairs around phosphorous atom is four. In this tutorial we will learn how to draw the lewis structure of PH3 and determining the shape and molecular geometry of the molecule.
According to the lewis structure shown above, you will understand phosphine's structure is a simple. Therefore, we can draw the lewis structure of phosphine easily.
There are several steps to draw the lewis structure of PH3. But, because phosphine is a simple molecule, these steps are not complex and do not require all general steps which are used to draw lewis structures of complex molecules and ions. Those steps are explained in detail in this tutorial.
There are two elements in PH3; hydrogen and phosphorous. Hydrogen is a group IA element and has only one electron in its last shell (valence shell). Phosphorus is a group VA element in the periodic table and contains five electrons in its last shell. Now we know how many electrons are includes in valence shells of hydrogen and phosphorus atom.
To find out total valence electrons given by a particular element, you should multiply number of electrons of the valance shell by the number of atoms of that element.
Total valance electrons pairs = σ bonds + π bonds + lone pairs at valence shells
Total electron pairs are determined by dividing the number total valence electrons by two. For, PH3, Total pairs of electrons are 4.
To be the center atom, ability of having greater valance is important. Then, from hydrogen and phosphorus, which atom has the highest valence? Maximum valence of phosphorus is five. Hydrogen's only valence is one. Therefore, phosphrus atom should be the center atom of PH3. Now, we can draw the sketch of PH3 to describe how atoms are attached with each other.
After determining the center atom and sketch of PH3 molecule, we can start to mark lone pairs on atoms. Remember that, there are total of four electron pairs.
There are no charges on phosphorus atom and hydrogen atoms. Also, remember that PH3 is a molecule which does not have a overall charge.
Because there is no charges on atoms, no need to reduce charges as a step of obtaining the best lewis structure. So, we have got the best lewis structure for PH3.
There are three sigma bonds and one lone-pair around phosphorus atom . Therefore, shape of PH3 is trigonal pyramidal.
Summation of number of sigma bonds and lone-pairs around phosphorus atom is four. Therefore geometry should be tetrahedral.
Questions
Both structures have three sigma bonds and one lone pair on center atom. So, shape of both ammonia and phosphine is trigonal pyramidal.
There are no direct charges such as -1,+1 on atoms. But, due to electronegativity difference, phosphorus and hydrogen atoms are slightly polarized. Phosphorus is negatively polarized and hydrogen is positively polarized.