Chapter 7

• Atomic Number


  Factor by which elements are arranged from left to right along periodic table
• Group

  Vertical column containing elements with the same number of outer shell electrons and similar properties
• Period

  Horizontal row by which it's number is the number of the highest energy shell of elements within that row
• Mendeleev


  Father of the modern periodic table
• Periodicity


  Repeating trends in properties of elements across a period
• Properties

  Determined by electron configuration of an element, particularly in the outer shell
• Blocks


  Areas of periodic table defined by their element's highest energy sub-shell
• s-Block

  Leftmost two groups
• p-Block

  Rightmost 6 groups
• d-block

  Middle 10 groups
• f-Block

  Two periods below main table
• Halogens


  Name of group seven elements
• Alkali Metals


  Name of group one element
• Transition Elements/Metals

  Name of group 3-12 elements
• Ionisation Energy

  Measure of how easily atoms lose electrons to form positive ions
• First Ionisation Energy

  Energy required to remove one electron from each atom in one mole of gaseous atoms of an element to form one mole of gaseous 1+ ions
• Highest/Outermost Energy Level

  Energy level of first ionised electron
• Least Attraction From Nucleus

  Reason for outmost electrons being first ionised
• Atomic Radius


  Distance between nucleus and outermost electrons
• Nuclear Charge


  Charge of atomic nucleus due to protons
• Electron Shielding

  Repulsion of outer-shell electrons by inner-shell electrons reducing attraction to nucleus
• Successive Ionisation Energies


  Energy required to remove successive electrons from the outermost shell of an atom, increasing with succession
• Successive Ionisation Energies


  Provides important evidence for different electron energy levels in an atom
• Number of electrons in outer shell, group of element in periodic table, identity of element


  Predictions from successive ionisation energies
• General Increase/Increase

  Trend in ionisation energy across each period
• Decrease

  Trend in ionisation energy down each group
• Decreases in Ionisation Energy Across Period


  Effect of changes in orbitals being filled and pairing
• Electron Repulsion

  Reason for lower ionisation of paired electrons
• Metals to Non-Metals

  Change which takes place at diagonal line across periodic table
• Metalloids/Semi Metals

  Name for elements with properties between metals and non-metals
• Non-Metal to Metal


  Trend going down groups 3-6
• Metallic Bonding

  Bonding taking place between metals
• Conduction of Electricity

  Constant property of all metals
• Sea of Delocalised Electrons

  Formed when metal atoms donate electrons and become cations during metallic bonding
• Cation/Positive Ion

  Type of ion formed in metallic bonding
• Metallic Bonding

  Strong electrostatic forces of attraction between cations and delocalised electrons
• Cations


  Fixed in position maintaining structure and shape of metal
• Delocalised electrons


  Mobile charge carriers free to move around structure
• Giant Metallic Lattice


  Term for metal structure
• High Temperatures


  Required to provide energy to overcome strong electrostatic forces of attraction in metallic bonds