In a water molecule, two hydrogen atoms bind to one oxygen atom. How many lone pairs of electrons will be shown around each hydrogen atom in the Lewis structure of water?
There are no non bonding pairs (lone pairs) on each Hydrogen atom. The one pair shown, is a bonding pair.
To determine the number of lone pairs of electrons around each hydrogen atom in the Lewis structure of water, we first need to understand the structure of a water molecule.
A Lewis structure represents the arrangement of atoms and electrons in a molecule. In water (H₂O), there is one oxygen atom (O) and two hydrogen atoms (H). Oxygen has six valence electrons (electrons in its outermost energy level), while hydrogen has one valence electron.
In the Lewis structure of water, we distribute the valence electrons around the atoms to satisfy the octet rule (in which atoms seek to have eight valence electrons). Oxygen needs two more electrons to complete its octet, whereas each hydrogen atom needs one more electron.
To satisfy these requirements, we show two lone pairs of electrons around the oxygen atom (represented by two pairs of dots) and no lone pairs around each hydrogen atom. This gives the oxygen atom a total of eight valence electrons and each hydrogen atom two electrons.
So, in the Lewis structure of water, there are no lone pairs of electrons around the hydrogen atoms.