Unit 1 - Periodic Table 0.0 / 5 ? Applied SciencePeriodic Table BTEC NationalAQA Created by: Hannah Marie WilliamsonCreated on: 23-05-19 19:58 Why are Group 0 elements not reactive? They have a full outer shell. 1 of 17 Explain what happens to the reactivity of Group 1 elements as you go down the group? Increase in reactivity. The outer electron is more easily lost as it gets further from the nucleus. 2 of 17 Explain what happens to the reactivity of Group 7 elements as you go down the group? A decrease in reactivity, because it is harder to gain an extra electron as the outer shell is further from the nucleus. 3 of 17 S Block Elements - Radii Increases down group. 4 of 17 S Block Elements - Ionisation Energy Decreases down Group 2 5 of 17 S Block Elements - Electronegativity Decreases down = more shielding. 6 of 17 D Block Elements - Radii Decreases with increasing atomic number. 7 of 17 D Block Elements - Ionisation Energy Increases 8 of 17 D Block Elements - Electronegativity Decreases down. 9 of 17 Group 0 and 7 Elements - Radii Increases as number of shells increase due to increase shielding. 10 of 17 Group 0 and 7 Elements - Ionisation Energy Decreases down the groups. 11 of 17 Group 0 and 7 Elements - Electronegativity 0 - None 7 - Decreases as you go down. 12 of 17 How are the elements in the periodic table listed? Increasing order of proton number. 13 of 17 What does each row tell you? How many shells there are. 14 of 17 What does the group number tell you? How many electrons are on the outer shell. 15 of 17 What does each row begin with and end with? Begins with a alkali metal. Ends with a noble gas. 16 of 17 Across a row the properties of elements go from? Metallic to Non Metallic. 17 of 17
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