Question

which of the following statements is false?

1. “shielding” reduces the full nuclear charge to an “effective nuclear charge” (Z eff)

2. For a given n value, the lower the l value, the higher the sub shell energy

3. Higher nuclear charge lowers orbital energy (stabilizes the system) by increasing nucleus-electron attractions

4. Inner electrons shield outer electrons much more effectively than do electrons in the same subshell, so shielding by inner electrons greatly lowers the Z eff felt by outer electrons

5. “Penetration” by an ns electron increases its overall attraction to the nucleus relative to that for an np electron, thereby rendering sub shells be and np with different energies

Answer 1

Answer:

The false statement will be (2), where written 'given n value, the lower the l value, the higher the subshell energy', This statement is false because if n=1, which shows the shell "K", having l value be 0. Here if the value of l=0 that doesn't mean the system has higher energy but it shows that electrons are in S Subshell. Higher energy indicates instability but in other words, if we are talking about energy, it should in terms of ionization energy or electron affinity. Then only we can say that if the value of n is lower electrons in the Subshell held tightly under the influence of nuclear charge.