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Use the periodic table to work out the short hand electronic structure for the following elements:

Ionisation energy of the first 20 elements. Use the periodic table to work out the short hand electronic structure for the following elements: Sodium Iron Argon Calcium. The Periodic table can be used to give you lots of information regarding electronic structure. S block. P block.

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Use the periodic table to work out the short hand electronic structure for the following elements:

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  1. Ionisation energy of the first 20 elements • Use the periodic table to work out the short hand electronic structure for the following elements: • Sodium • Iron • Argon • Calcium

  2. The Periodic table can be used to give you lots of information regarding electronic structure. S block P block D block F block

  3. It gets more complicated…soz • 2.8.8 is further divided • Each level can be sub-divided • Example: Carbon KS4 = 2.4 • KS5= • Still 6 electrons but the first level has been called ‘s’ • The second level is divided into ‘s’ and ‘p’ • 1s22s22p2

  4. Look at the periodic table and answer the following • Name 3 s block elements • Name 3 p block elements • Name 3 d block elements • Name two elements that are s block in period 4 • Name two elements that are p block in period 6 • Name two elements that are d block in period 3

  5. ‘s’ ‘d’ ‘p’ block elements

  6. The number of electrons in each level • ‘s’ always has 2 • ‘p’ always has 6 • ‘s’ + ‘p’ = 8 • ‘d’ always has 10

  7. S = sphere P = 2 lobes (x 3) Each lobe contains 2 electrons 3 x 2 = 6 electrons These are sometimes called quantum shells The shapes of the energy levels

  8. Write the electronic structures for the following using the KS5 new way… • Lithium • Nitrogen • Fluorine • Magnesium • Silicon • Chlorine • Potassium

  9. The further away from the nucleus the higher energy state. You can work out the amount of electrons in the level using the periodic table (2.8.8) Expanded 2.8.8 to 2. 2,6. 2,6. 3d, is odd…4s comes first Write 4s before 3d

  10. 3d 4s 3p 3s 2p 2s 1s CORRECT ORDER OF FILLING FOR THE FIRST THIRTY ATOMS E N E R G Y

  11. Write the structure for the transition elements • Titanium • Chromium • Iron • Copper • Zinc

  12. Electron sub-levelsFill in the table

  13. This is Boron 1s2 2s2 2p1 What are the other atoms? 1s 2s 2p 3s 3p

  14. Electronic Configurations of First Eleven Elements H 1 1s1 [CORE] VALENCE SHELL He 2 1s2 Li 3 1s22s1 [1s2]2s1 Be 4 1s22s2 [1s2]2s2 B 5 1s22s22p1 [1s2]2s22px1 C 6 1s22s22p2 [1s2]2s22px12py1 N 7 1s22s22p3 O 8 1s22s22p4 F 9 1s22s22p5 Ne 10 1s22s22p6 Na 11 1s22s22p63s1 [1s22s22p6]3s1

  15. Ionic electronic structure • Write the electronic structure for the following ions: Fe2+ Mg2+ Cl- S2- Al3+

  16. Ionisation energy • Define what is the ionisation energy of an atom? • Look at the pattern and figure out the trends.

  17. Answer • Ionisation energy (first ionisation) • The enthalpy change when 1 mole of electrons is removed from 1 moles of a gaseous element Alternatively… • Enthalpy change when 1 mole of gaseous atoms forms 1 mole of gaseous ions with a single positive charge. Second ionisation energy • Enthalpy change when 1 mole of gaseous ions forms 1 mole of gaseous ions with a double positive charge.

  18. Write a paragraph regarding the general trend as the atomic number increases • There are patterns which give us explanations for observations from KS4 • What evidence is there in the patterns for existence of quantum shells? • What other trends can you see? • Look at the group 1 elements, does this explain their chemical behaviour? • Also look at group 0/7, and link with what you know of their reactivity?

  19. Look at the graph and the table that was on the board in your text • In groups try to explain each change in the graph especially when: • It goes from one level to another (1 to 2) • It changes from one sub-level to another • Explain the difference between the first energy levels values and successive levels for elements in the same group. • Why there is a drop in ionisation energy in the ‘p’ block elements (O, S, Se)

  20. Hund’s Rule • What happens when 2 magnets with like poles are pushed together? • It is the same with electrons • 2 do not like sharing the same space • A small repulsion causes the energy required to remove it to drop • Predict the energy needed to remove the first electron from Te in group 6

  21. Predict the second ionisation energy for the following elements: • Sodium • Magnesium • Fluorine • Neon • Iron • Nitrogen

  22. Predict the reactivity of the groups 1-8 using the ionisation energy information • Which metals are the most reactive and why (give evidence) • Which non-metals are the most reactive and why? • Which don’t react and why?

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