GCSE AQA Chemestry unit C3 1.1-1.5 key points

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Science (chemistry) Mind Map on GCSE AQA Chemestry unit C3 1.1-1.5 key points, created by dylan.keatinge on 05/13/2014.

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GCSE AQA Chemestry unit C3 1.1-1.5 key points
1 C3 1.1
1.1 The periodic table of elements developed as chemists tried to classify the elements. It arranges them in a pattern in which similar elements are grouped together.
1.2 Newlands table put the elements in order of atomic mass but failed to take account of elements that were unknown at that time.
1.3 Mendeleev's periodic table left gaps for the unknown elements, and so provided the basis for modern periodic table.
2 C3 1.2
2.1 The atomic (proton) number of an element determines its place in the periodic table
2.2 the number of electrons in the outer shell (highest energy level) of an atom determines its chemical properties
2.3 the group number in the periodic table equals the number of electrons in the outermost shell
2.4 we can explain trends in reactivity as we go down a group in terms of
2.4.1 The distance between the outermost electrons and the nucleus
2.4.2 the number of occupied inner shells (energy levels) in the atoms
3 C3 1.3
3.1 the elements in group 1 of the periodic table are called the alkali metals
3.2 Their melting points and boiling points decrease going down the group
3.3 the metals all react with water to produce hydrogen and the alkaline metal solution containing the metal hydroxide
3.4 They form 1+ ions in reactions to make ionic compounds. these are generally white and dissolve in water, giving colourless solutions
3.5 The reactivity of alkali metals increase going down the group
4 C3 1.4
4.1 Compared with the alkali metals, transition metals have much higher melting points and densities. They are also stronger and harder but are much less reactive.
4.2 The transition metals do not react vigorously with oxygen or water.
4.3 a transition element can from ions with different charges, in compounds that are often coloured.
4.4 Transition elements and their compounds are important industrial catalysts.
5 C3 1.5
5.1 The halogens all form ions with a single negative charge in their ionic compound with metals.
5.2 The halogens form covalent compounds by sharing electrons with other non-metals
5.3 a more reactive halogen can displace a less reactive halogen from ma solution of one of its salts.
5.4 The reactivity of halogens decreases as you go down the group
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