Periodic Table preview page
Students should be able to:
(a) describe the Periodic Table as an arrangement of the elements in the order of increasing proton (atomic) number
(b) describe how the position of an element in the Periodic Table is related to proton number and electronic structure
(c) describe the relationship between group number and the ionic charge of an element
(d) explain the similarities between the elements in the same group of the Periodic Table in terms of their electronic structure
(e) describe the change from metallic to non-metallic character from left to right across a period of the Period Table
(f) describe the relationship between group number, number of valency electrons and metallic/nonmetallic character (g) predict the properties of elements in Group I and Group VII using the Periodic Table.
(a) describe lithium, sodium and potassium in Group I (the alkali metals) as a collection of relatively soft, low density metals showing a trend in melting point and in their reaction with water
(b) describe chlorine, bromine and iodine in Group VII (the halogens) as a collection of diatomic nonmetals showing a trend in colour, state and their displacement reactions with solutions of other halide ions
(c) describe the elements in Group 0 (the noble gases) as a collection of monatomic elements that are chemically unreactive and hence important in providing an inert atmosphere, e.g. argon and neon in light bulbs; helium in balloons; argon in the manufacture of steel
(d) describe the lack of reactivity of the noble gases in terms of their electronic structures.