# To which part of a water molecule would Li^+ be attracted?

Jun 29, 2017

The oxygen part.

#### Explanation:

A simple way to explain this concept is with something called electronegativity.

If you were to take a look at the Oxygen atom's electronegativity value, you would be able to tell that it is a very electronegative element. Therefore, it will draw the electrons away from the Hydrogen atoms.

The result will be that the Oxygen will acquire a partial negative charge, and the two Hydrogens will receive a partial positive charge (the sum of the charges would be $0$).

Now, lets think about $L {i}^{+}$. We know from common knowledge that "opposites attract." After taking a look at the water molecule above, we can tell that the positive Li would be attracted to the negative O atom. This is because the oxygen has a minus sign (as explained) and the Hydrogens have a plus sign.

Therefore, we can say that the $L {i}^{+}$ atom would be attracted to the Oxygen atom of the water molecule.

I hope that helps!

Jun 29, 2017

Well, which part of the water molecule is most electron-rich?

#### Explanation:

Clearly we speak of the oxygen centre. When we represent the dissolution of a lithium salt in water, we often write.......

$L i C l \left(s\right) \stackrel{{H}_{2} O}{\rightarrow} L i C l \left(a q\right)$

Where $L i C l \left(a q\right)$ specifies the aquated ions, i.e. ${\left[L i {\left(O {H}_{2}\right)}_{4 - 6}\right]}^{+}$ and ${\left[C l {\left({H}_{2} O\right)}_{6}\right]}^{+}$. And thus in aqueous solution each lithium ion is associated with, i.e. solvated by, several water molecules, and likewise for the chloride ion.