Ionization Energy and Quantum Number ?? Please briefly explain the first questio

Question

Ionization Energy and Quantum Number ??

Please briefly explain the first question's answer.

For the second question Please explain why and why not for EACH choice for full points. The professor wants us to explain our answers.

Why does ionization energy decrease as you move down a group in the periodic table? because the atoms get closer to noble gas configuration because shielding decreases because effective nuclear charge increases because the outer electrons get further from the nucleus because nuclear charge decreases Consider the quantum numbers n = 4 and l= 2. Which of the following statements are correct regarding these quantum numbers? More than one may be correct. corresponds to a p-orbital can hold up to 4 electrons ml can only equal -1,0, +1 has 5 orbitals ms can only equal 1/2 an electron with these quantum numbers could have an electron configuration of [Kr] 5s2 4d3 an electron at these quantum numbers has more energy than an electron at n = 5,l = 0 when the last electron in the ground state has these quantum numbers, the atom is between Scandium and Zinc on the Periodic Table

Explanation / Answer

1.beacause oter electrons get farther from nucleas

2.           for this part 4,5,6,7 options are correct

l = 2 means d orbital, for l =2, ml = -2,-1,0,1,2, means 5 orbitals
by pauli's exclusion principle ms can be + or - 2
n = 5 , l=0 meaans 5s orbital, which have lower energy than 4d orbital
6th option also correct coz [kr]5s34d3 can have electrons with configration n=4, l=2

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