By Katie Gordon, Nicolas Graham,
Brittany Melanson, and Mitchell Travis
Introduction


Compounds with
small ions tend to be
less soluble than
compounds with large
ions.
This is because small
ions bond more
closely together than
large ions, and they
are harder to break
apart- this makes
them less soluble.

The size of the ion is
a direct result from
when an atom gives
up or gains an ion,
the size after the
electron Is gained or
lost is different than
the original size of
the atom.

Ions of metals tend
to be smaller than
their original neutral
atoms. For the ions
of non-metals tend
to be bigger than
their original neutral
atoms.

The size of the ions
increases as you go
down a family in the
periodic table
Questions



Which would you
expect to be less
soluble?
Sodium or tin
Chlorine or barium



Which would you
expect to be more
soluble?
Krypton or lithium
Oxygen or iodine
Questions

If sodium has a
neutral charge, then
loses an electron
and becomes Na1+,
would you expect
the ion to be bigger
or smaller?

Smaller
Questions

If chlorine has a
neutral charge then
gains an electron
and becomes Cl 1-,
would you expect
the ion to be bigger
or smaller?

Bigger