Patterns in the Periodic Table structured questions · SEC G3 Pure Chemistry

Learning objectives

• describe the Periodic Table as an arrangement of the elements in the order of increasing proton (atomic) number
• describe how the position of an element in the Periodic Table is related to proton number and electronic configuration
• describe the relationship between number of outer (valence) electrons and the ionic charge of an ion for the first twenty elements
• explain the similarities between the elements in the same group of the Periodic Table in terms of their electronic configuration
• describe the change from metallic to non-metallic character from left to right across a period of the Periodic Table
• describe the relationship between number of outer (valence) electrons and metallic/non-metallic character
• predict the properties of elements in Group 1 and Group 17 using the Periodic Table.
• describe lithium, sodium and potassium in Group 1 (the alkali metals) as a collection of relatively soft, low density metals showing a trend in melting point and in their reaction with water
• describe chlorine, bromine and iodine in Group 17 (the halogens) as a collection of diatomic non- metals showing a trend in colour, state and their displacement reactions with solutions of other halide ions
• describe the elements in Group 18 (the noble gases) as a collection of monoatomic elements that are chemically unreactive and hence important in providing an inert environment, e.g. argon and neon in light bulbs; helium in balloons; argon in the manufacture of steel
• describe the lack of reactivity of the noble gases in terms of their electronic configurations.
• describe typical transition elements as metals having high melting point, high density, variable oxidation state and forming coloured compounds
• state that the elements and/or their compounds are often able to act as catalysts (see also 10(d)).
• place in order of reactivity calcium, copper, (hydrogen), iron, lead, magnesium, potassium, silver, sodium and zinc by reference to the reactions, if any, of the metals with water, steam and dilute hydrochloric acid
• place in order of reactivity calcium, copper, (hydrogen), iron, lead, magnesium, potassium, silver, sodium and zinc by reference to — the reduction, if any, of their oxides by carbon and/or by hydrogen
• describe the reactivity series as related to the tendency of a metal to form its positive ion, illustrated by its reaction with — the aqueous ions of the other listed metals
• describe the reactivity series as related to the tendency of a metal to form its positive ion, illustrated by its reaction with — the oxides of the other listed metals
• deduce the order of reactivity from a given set of experimental results
• describe the action of heat on the carbonates of the listed metals and relate thermal stability to the reactivity series
• describe the ease of obtaining metals from their ores by relating the elements to their positions in the reactivity series
• describe the essential conditions for the corrosion (rusting) of iron as the presence of oxygen and water; prevention of rusting can be achieved by placing a barrier around the metal, e.g. painting; greasing; plastic coating; galvanising
• describe the sacrificial protection of iron by a more reactive metal in terms of the reactivity series where the more reactive metal corrodes preferentially, e.g. underwater pipes have a piece of magnesium attached to them.