explanation. Why is this the case, and what is the correct explanation?
A. Decreasing atomic radius is a result of the same cause of increasing ionization energy: increased nuclear charge with negligible electron shielding from samelevel electrons pulls valence electrons in more tightly, making it harder to remove them.
B. Atomic radius actually increases, not decreases across a row from left to right. The expansion of the atomic size makes it harder to remove the valence electrons.
C. Atomic radius neither increases nor decreases across a row of the periodic table. Increasing ionization energy from left to right is the result of the nucleus¡¯s decreasing pull on the valence electrons from left to right.
D. Both a and b are true.
E. None of the above are true.A.
ioniation energy: the energy required to remove an electron from an atom.
as you go across the periodic table, there are more protons in the nucleus of each atom and more electrons on the SAME ENERGY LEVEL. (each row of the periodic table represents an energy level of an atom.) since they are not getting any farther from the nucleus the attraction between the protons and electrons INCREASES because there are more of them so it is harder to pull them away from that attracton so higher energy is needed.
Atom size: same concept. since there is more attraction, the electrons come closer to nucleus so atom size decreases across the periodic table.