sublevels and orbitals

• How many electrons on each energy level ?

  2, 8, 18, 32
• Each energy level is made up of what

  Sub levels
• What are sub levels split into?

  Orbitals
• How many electrons can each orbital hold up to?

  2 electrons
• The 4 sub levels

  s, p, d, f
• What shape is the s sub level

  spherical
• What shape is the p sublevel

  peanut (8)
• Number of orbitals for s sublevel

  1 orbital
• Number of orbitals for p sublevel

  3 orbitals
• Number of orbitals for d sublevel

  5 orbitals
• Number of orbitals for f sublevel

  7 orbitals
• Number of electrons for s sublevel

  2
• Number of electrons for p sublevel

  6
• Number of electrons for d sublevel

  10
• Number of electrons for f sublevel

  14
• Hund's Rule

  If possible electrons are unpaired in the same orbital
• Why do we fill orbitals singly first and then pair them up

  due to electron repulsion
• s-block elements

  groups 1 and 2
• d-block elements

  transition metals
• p-block elements

  the elements consists of the last six groups minus helium
• Why is 4s2 filled first

  This is because 4s2 is lower in energy and closer to the nucleus than 3d10
• Transition metals

  -After 4s2 you fill 3d electrons

  -lose their 4s electrons before their 3d electrons (even thought 4s is filled before 3d)
• Exception to the rule of 4s2

  Chromium (Cr) and copper (Cu) have 4s1 before 3d instead of 4s2
• Why do chromium and copper have 4s1

  Because an atom is more stable if it has a half-filled or filled set of 3d orbital and a single electron in the 4s orbital
• S and p block ions

  Lose or gain electrons from their outermost sub levels