✨Module 2: Electrons and bonding Flashcards
Electron shells are also known as …
Electron shells are made up of …
Energy levels.
Sub-shells and orbitals.
Each shell is given a principal …
Quantum number - shell number ‘n’.
Electrons have fixed …
Energies and move around in shells.
Shells further form the nucleus have …
Higher energy, larger prin quantum number, and hold more electrons.
What are sub-shells?
Divisions within electron shells, each having a different energy.
Subshells include …
S, p, d, f, which have different number of orbitals, so a shell is a group of atomic orbitals.
Define atomic orbital.
Region around the nucleus that can hold up to 2 electrons with opposite spins.
Maximum number of electrons in a shell?
2n^2. So 1st = 2, 2nd = 8, 3rd = 18, 4th = 32.
Noble gases can be used in …
Shorthand electron configurations, but only when asked.
Ions with greater charge will have …
Greater attraction to other ions so stronger ionic bonding.
Larger ions with a greater ionic radius …
Will have weaker attraction as the attractive forces act over a greater distance.
Higher charge increases boiling point but …
Decreases solubility as water molecules can’t overcome electrostatic forces.
Define covalent bond.
Shared pair of electrons between 2 atoms and attracted to the nuclei of both atoms.
What is ‘expand the octet’?
When the atom is able to have more than 8 valence electrons. Like sulfur hexafluoride has 12 electrons in its outer shell, PCL5.
Double and triple covalent bonds are shorter than single covalent bonds as …
There’s more attraction between atoms and more electrons, so stronger bonds.
What is average bond enthalpy?
Energy required to break a bond. It is used to measure covalent bond strength.
The stronger the bond …
The greater the average bond enthalpy as more energy is required to break it.
What is a dative covalent bond?
When both electrons in the shared pair are supplied from one atom.
For a dative covalent bond to form the …
Acceptor atom must be electron deficient.
