OCR A-Level Chemistry Chapter 7 – Periodicity Questions and Answers

OCR A-Level Chemistry Chapter 7 – Periodicity Questions and Answers 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 ions 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 Solubility Not a property of metals Giant Covalent Lattice Formed when non-metals covenantally bond (boron, carbon & silicon) High Temperatures Required to provide energy to overcome strong covalent bonds in giant covalent structures Solubility Not a property of giant covalent structures Conduction of Electricity Not a property of giant covalent structures Graphite/Graphene Giant Covalent structure that can conduct electricity