Lessons 16/17 Periodic table review Poster project Booklet – paper lab

Lesson objectives (review of Y8) Relate the Bohr-Rutherford atomic model to properties of elements and their positions in the periodic table Give examples of how patterns in reactions can be predicted with reference to the periodic table Understand that the periodic table is a method of classifying elements and predicting their properties Describe the properties of group I, group II, group VII, group VIII and the transition elements

Atomic structure (Bohr-Rutherford)

Periodic Table- organization

Simpler version

Groups and Periods

Trends

Bonds (3 types) Ionic Between reactive metals and non-metals Covalent Between non-metals and non-metals Metallic Metal and metal

Properties of Group I and II Group 1- Alkali Metals Group 2- Alkali Earth Metals Very reactive Only found in compounds in natural world Silvery appearance Soft – can be cut with knife Have lowest density of all metals

Properties of Group VI and VII Group VI- oxygen family Oxygen is a gas O2 Sulfur smells like rotten eggs used to make H2SO4– most used chemical in industry Group VII- halogens Very reactive Bond with themselves Cl2, F2, Br2 or with group I, II or III

Properties of Group VIII Noble Gases (Inert) Non reactive Create colors when electricity is passed through them

Transition metals Shiny Good conductors High melting points High densities Malleable and ductile Hard, strong and tough Used for Coins jewellery Electric and heat Building materials

Predicting reactions Metals- Reactivity series More reactive metals will change places with less reactive metals Group I and II react easily with Group VI and VII Group VI and VII bond with themselves Group VIII do not react with other elements

Task- lessons 16/17- Periodic Table Poster 20 marks- 4 for each element, 4 for presentation A4 piece of paper into 4 Pick one element from Group I, II, VII and VIII Atomic number less than 20 Draw and label a Bohr-Rutherford diagram for each element State three things that you know about this element from its position in the periodic table i.e. Na, Group I, solid, highly reactive, one valence electron, always found as a compound in natural world

Tasks lesson 17- paper labs Finish poster New Chemistry Booklet Page 8, periodic table Page 9-10, looking for patterns (graph and answer questions) Page 11-12, which metal reacts better?