Question

2. The element below sodium in the same group
would be expected to have a
(lower/higher) electronegativity than sodium and
the element above chlorine would be expected to
have a
(lower/higher) ionization
potential than chlorine.
3. On moving from left to right in a given period, the
number of shells
(remains the
same/increases/decreases)
4. On moving down a group, the number of valence
electrons
(remains the same/
increases/decreases)
5. The atomic size
(increases/
decreases) as we move from left to right across the
period because the
(number of
shells / number of valence electrons) increases but
the
(atomic number/ effective
nuclear change/ number of shells) remains the same.
6. Atomic radius of oxygen is
(smaller / greater) than neon.
7. Neon in period 2 is likely to have a
(larger / smaller) atomic radius than fluorine and its
electron affinity value would be
(greater/smaller / zero) compared to fluorine.
8. If an element has a high ionization potential, then, it
is likely to be a
(metal/non-metal)
​

Answer 1

Answer:

verrrrry big

Explanation: