Answer:
The number of lone pairs = 0
The number of single bonds = 4
The number of double bonds = 0
Explanation:
The first step to draw a Lewis structure is to find the total number of valence electrons. To do this we need to find the number of valence electrons in all the atoms in the molecule. In this case, we have 1 nitrogen that has a valence number of 5 and 4 hydrogens with a valence number of 1.
Second, we need to find the number of electrons that are shared in the bond, to do this we add the valence atoms of all the atoms in the molecule. Since this molecule is a cation (positive charge), we have to take away one electron from the molecule. Taking this into account we have:
5*1 (nitrogen) + 1*4(hydrogens) -1 (cation) = 8 electrons shared
Third, we need to determine the number of bonds. Since each bond needs two electrons. To get the number of bonds we need to divide the number of electrons shared by 2. By doing this we get 4 bonds for this molecule.
Finally, we draw the structure. See picture.
The octet rule says that atoms are stable when they have 8 electrons in the outer electron shell. There are some exceptions like hydrogen that just have 2 electrons in its outer shell. In this case, we see that each hydrogen has 2 electrons and that the nitrogen has 8 electrons around it, so they follow the octet rule.
2. Number of lone pairs: this is the electrons that don’t participate in bonding. Looking at the structure, you can see that all the valence electrons in the molecule participate in bonds, so this number is 0.
3. We have 4 single bonds in the structure. 2 electrons are shared. One single line.
4. There are cero double bonds in this structure. 4 electrons are shared. Two single lines.
