Electronic Structure

Electronic Structure

1. Electron shell ///maximum number of electrons 1 / 2 2 / 8 3 /18 4 /32 5/ 50

2. Half arrows are used to represnt each electron in the orbitals. drawn facing up and down as they have different orbital spins

3. electons within each shell wont have the same amount of energy

   • so the cells are broken down into subshells called orbitals. these are s, p, f and f orbitals

4. Electrons have two possible states. spin up and spin down. in orbital, each electron will be in a different spin state

5. when an atom of an element loses one or more electron and donates it to an atom of a different element. this is called ionic bonding

   • the atom that loses electrons becomes positivly charged
   • the atom that gains electrons becomes negitavly charged because of the imbalance of protons and electrons

6. covalent bonding usually occurs between atoms of two non metals

   • a covalent bond forms when an electron is shared between the atoms.