Chapter 5 ELECTRONS & BONDING

• What are the 4 electron subshells?

  S-orbital

  p-orbital

  d-orbital

  f-orbital
• How many electrons can there be in the s-orbital?

  2
• How many electrons can there be in the p-orbital?

  6
• How many electrons can there be in the d-orbital?

  10
• How many electrons can there be in the f-orbital?

  14
• What is spin-pairing?

  2 electrons in the same orbital spinning in opposite directions
• How does shell number link to energy?

  The higher the shell number, the further away it is from the nucleus and the higher energy it has
• In what order do electrons fill in and fill out subshells?

  The lowest energy level fills IN first and the highest energy level fills OUT first
• Why does 4s fill before 3d?

  It has a lower energy level than 3d
• Which subshell configurations can only exist as ions and why?

  3d4 and 3d9

  This is because exactly half filled or exactly filled subshells are more stable than unevenly filled subshells.
• What bonding do ionic compounds have?

  Ionic bonds held together by electrostatic attractions between oppositely charged ions
• What structure is NaCl?

  Giant Ionic Lattice
• Why are ionic compounds soluble in water?

  Water is polar so it is able to attract the positive and negative ions breaking them apart.
• Do ionic compounds conduct electricity?

  Yes, when molten or dissolved because the ions are free to move around
• Why do ionic compounds have high melting points?

  The electrostatic forces of attraction are very strong and require lots of energy to overcome
• What is covalent bonding?

  Sharing of electrons between atoms which are held together by the strong electrostatic attraction between positive nucleus and negative electrons
• What is dative covalent bonding?

  Dative covalent bonding is where one atom donates 2 electrons to another atom with no electrons to form a bond

  e.g. NH4+