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Trends in the Periodic Table

Trends in the Periodic Table. Week 4. Vertical rows = groups Group 1 = alkali metals Group 2 = alkaline earths Groups 1 and 2 together = s block elements Group 7 = halogens Group 8 = inert gases Groups 3,4,5,6,7 and 8 = p lock elements. Group 1 elements:.

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Trends in the Periodic Table

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  1. Trends in the Periodic Table Week 4

  2. Vertical rows = groups • Group 1 = alkali metals • Group 2 = alkaline earths • Groups 1 and 2 together = s block elements • Group 7 = halogens • Group 8 = inert gases • Groups 3,4,5,6,7 and 8 = p lock elements

  3. Group 1 elements: • All have 1 electron in outside quantum level • All can achieve stability by losing this outside electron • Which element in group 1 will have the lowest 1st ionisation energy? • Why? • Due to shielding effect • What is this?

  4. Group 2 elements: • Achieve stability by losing 2 electrons in the outer quantum level. • Why does it require more energy to lose the second electron than the first one? • Which member of group 2 would be the easiest to ionise? • And the most difficult to ionise?

  5. Group 7 elements: • Can attain stability by gaining and electron in the outside quantum level to achieve the electron configuration of the neighbouring inert gas. • Which element is the most reactive member of group 7? • Explain why you have given this answer to the question above

  6. Horizontal rows = periods • Described as either short or long periods • Which elements form the first short period? • The second short period? • The first long period? • The long periods include the d block elements • Why are they called the d block elements? • How many d block elements are there in each long period?

  7. For a given period: • Which would be bigger: an ion for a group 1 element or the neighbouring group 2 element? • Why? • Which would be bigger: an ion for a group 1 element or an ion of the group 7 element in the same period? • Why?

  8. Group 6: • Elements in this group are less reactive than their neighbours in group 7 • Why?

  9. Groups 3,4 and 5 • Group 3: large amount of energy to ionise • Group 5: some examples of elements at top of group ionising. Lower members don’t ionise. • Group 4: covalent compounds

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