Atomic Structure: Electron configuration. Flashcards
Different sub-shells have different what?
= energies.
As we move away from the nucleus what happens to the energy of the shells?
= Increases.
What are the rules for filling atomic orbitals?
= orbitals with the lowest energy are filled first.
= we can have 2 electrons in the same orbital but they must have opposite spins
= Electrons are filled in indiviudal orbitals before they are in pairs, as electrons in the same orbital repel.
What does electron configuration only show?
= subshells but not individual orbitals.
What is the electron configuration?
1s^2, 2s^2, 2p^6, 3s^2, 3p^6, 4s^, 3d^10.
Why is 3d after 4s?
= The energy of the 4s subshell is less than the energy of the 3d subshell.
= fill the 4s sub shell before the 3d sub shell.
What are the exceptions in electron configuration?
= Chromium and Copper.
Why does the 4s subshell only contain 1 electron in the circumstance of chromium and copper?
= 3d subshell is more stable when it is either half full or completly full.
Each block is named after the subshell containing what?
= highest energy electron.
What block is metals?
= sblock.
What block is the transition metals?
= d block.
WHat block is the non-metals?
= p block.
