Atomic Orbitals And Quantum Numbers Flashcards
How do we find the principal quantum number (n) of an element?
Look at the row number
When is the f sub shell introduced?
At n=6
What is the electron configuration for Cr?
[Ar]4s^15d^6
(this is an exception!)
What happens to the atomic radii as we move across the periodic table?
It becomes smaller because the number of protons is greater
What happens to the atomic radii as we move down atomic groups?
It becomes greater because the number of shells increases
When does ionic radii increase?
When the number of electrons increases
When does ionic radii decrease?
When the number of protons increases
What is electron affinity?
Energy released when an electron is added
Smaller EA harder to add
Larger EA easier to add electrons
When are elements more likely to gain electrons?
As we move towards the right of the table (closer to the non-metallics)
Does electron affinity does increase or decrease as we move down the group?
It decreases
Higher on the group GREATER electron affinitiy
Do metallic elements lose or gain electrons?
Lose
Non-metallics GAIN electrons!
What is ionization energy?
Energy required to remove an electron
Larger IE harder to remove electrons
Smaller IE easier to remove
Why is ionization energy always positive?
We always apply energy to remove electrons
Do non-metallics have a high or low ionization energy?
High because they want to gain electrons, not lose them like metals
Metals have low ionization energy
As we move to the right of the table, does it take more energy to remove an electron?
Yes because the elements have more non-metallic characteristics
Between K and Na, which has a higher ionization energy?
K atomic number- 19, Na atomic number- 11
Na because it is higher on the group
Down groups, the metallic energy increases which means the IE decrease
Why does Be have a higher ionization energy than B?
Be: atomic number is 4, B: atomic number is 5
Be has a completely full s shell, so it requires more energy to remove an electron
This is an exception!
Why does O have a higher ionization energy than N?
The shells of O are more stable than that of N.
THIS EXCEPTION ALSO APPLIES TO P AND S
principal quantum number (n)
size and energy of the orbital (comes from row number)
Angular momentum quantum number (l)
shape of atomic orbital (l= 0, …, n-1)
Magnetic quantum number (ml)
orientation of the orbital in space relative to the other orbitals (ml= -l, …, 0,…,+l)
Electron spin quantum number (ms)
Electron spin quantum number (ms =+/- 1/2)
