Question

DQuestion 4 1 pts As you go horizontal the effective nuclear charge [Select) therefore the atomic radius and Select ] . Even though you are [Select ] electrons D Question 5 1 pts The higher the positive charge the [ Select ] the ion/element. The more negative a charge is, the the ion/element I Select ) aarod nt 11-28nm

Answer 1

question 4:

As you go horizontal the effective nuclear charge increases and therefore the atomic radius decreases even though you are increasing electrons.

Along a period in a periodic table the atomic radius of elements decreases. As for example atomic radius order of different elements in second period is Li>Be>B>C>N>O>F. The reason is that as we increase the number of protons in nucleus the effective nuclear charge increases. This effect of increasing nuclear charge (by adding protons) can not be compensated completely by adding same number of electrons (which is a negative charge).

question 5:

The higher the positive charge smaller the ion/element. The more negative a charge is, the larger the ion/element.

For positive ion the number of protons in the nucleus is greater than the number of electrons in the orbits. So effective nuclear charge increases and radius decreases as attractive force will be more than repulsive force. Again for negative charge the number of electrons exceed the number of protons. So, effective nuclear charge decreases and atomic or ionic radius increases as more repulsive force among electrons arises due to presence of extra electrons.