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T12 IB Chemistry Atomic structure

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Robert Hughes

Here is my presentation on Atomic structure, HL content. Please note that I have tried to acknowledge any sources used, in particular the Pearson textbook which I find excellent.

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12.1- Electrons in atoms
Lesson outline Lesson 1- Topic 2 review. Lesson 2- What does ionization energy (I.E.) tell us about the structure of an atom? Lesson 3- Topic 2/12 review questions.
Lesson 1- Topic 2 review . Level 4: Recall that an isotope is a variant of an element due to more or less neutrons. Level 7: Explain how emission & absorption spectra were used to come up with the idea of atomic orbitals (s,p,d etc.) Level 5/6: determine the % abundance of an isotope from given data.
Topic 2 review See worksheet and answers. You can also try this quizlet: https://quizlet.com/167940560/ib-chemistry- atomic-structure-flash-cards/
Lesson 2- What does ionization energy (I.E.) tell us about the structure of an atom? Level 4: State what the definition is for first ionization energy. Level 7: Explain how trends in successive I.E. show evidence for energy levels and sub levels. Level 5/6: Justify the general trend in first I.E. for periods 1, 2 & 3.
starter *Task: Redraw this energy level diagram of a H atom and then include an arrow to show ionization of this atom.
Ionization energy (I.E.) The first ionization energy is the energy needed to remove one mole of electrons from the ground state of one mole of the gaseous atom. In short: H(g) H+ (g) + e- KJ.mol-1 https://www.youtube.com/watch?v=0EnK4EXLDUc (short video clip 1.20min)
An important diagram to have in your head. The principle energy levels are numbered 1,2,3 etc. Then you have a certain number of different orbital types at each of these energy levels s,p,d (and f may be referred to briefly) With these orbtials you then have a certain number of sub-orbitals/sub-levels e.g. a p orbital has 3 sub orbitals.
Successive I.E. & principle energy levels. (e.g. Aluminium) *8min to justify using e configs. Q. Why is there a jump between the 3rd & 4th and the 11th&12th I.E.? Q. Why is there a need for a log scale on the y axis?
Successive I.E. & sub- levels. (e.g. Aluminium) (a) Explain, using e-configs, why there is a large increase between the ninth and tenth I.E. (b) Explain why the increase between the sixth and seventh values is greater than the increase between the fifth and sixth values.
T12 IB Chemistry Atomic structure
Trends in first I.E. across a period 1. What is the general trend in I.E. across a period/row? 2. What is the general trend in I.E. down the periodic table? 3. What is the reason for the anomaly/discontinuity between Be and B and between N and O? (which is also repeated in row 3)
Pearson questions 12.1
T12 IB Chemistry Atomic structure
Topic 2/12 review See practice questions.. (from inthinking & Pearson)

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T12 IB Chemistry Atomic structure

  • 2. Lesson outline Lesson 1- Topic 2 review. Lesson 2- What does ionization energy (I.E.) tell us about the structure of an atom? Lesson 3- Topic 2/12 review questions.
  • 3. Lesson 1- Topic 2 review . Level 4: Recall that an isotope is a variant of an element due to more or less neutrons. Level 7: Explain how emission & absorption spectra were used to come up with the idea of atomic orbitals (s,p,d etc.) Level 5/6: determine the % abundance of an isotope from given data.
  • 4. Topic 2 review See worksheet and answers. You can also try this quizlet: https://quizlet.com/167940560/ib-chemistry- atomic-structure-flash-cards/
  • 5. Lesson 2- What does ionization energy (I.E.) tell us about the structure of an atom? Level 4: State what the definition is for first ionization energy. Level 7: Explain how trends in successive I.E. show evidence for energy levels and sub levels. Level 5/6: Justify the general trend in first I.E. for periods 1, 2 & 3.
  • 6. starter *Task: Redraw this energy level diagram of a H atom and then include an arrow to show ionization of this atom.
  • 7. Ionization energy (I.E.) The first ionization energy is the energy needed to remove one mole of electrons from the ground state of one mole of the gaseous atom. In short: H(g) H+ (g) + e- KJ.mol-1 https://www.youtube.com/watch?v=0EnK4EXLDUc (short video clip 1.20min)
  • 8. An important diagram to have in your head. The principle energy levels are numbered 1,2,3 etc. Then you have a certain number of different orbital types at each of these energy levels s,p,d (and f may be referred to briefly) With these orbtials you then have a certain number of sub-orbitals/sub-levels e.g. a p orbital has 3 sub orbitals.
  • 9. Successive I.E. & principle energy levels. (e.g. Aluminium) *8min to justify using e configs. Q. Why is there a jump between the 3rd & 4th and the 11th&12th I.E.? Q. Why is there a need for a log scale on the y axis?
  • 10. Successive I.E. & sub- levels. (e.g. Aluminium) (a) Explain, using e-configs, why there is a large increase between the ninth and tenth I.E. (b) Explain why the increase between the sixth and seventh values is greater than the increase between the fifth and sixth values.
  • 12. Trends in first I.E. across a period 1. What is the general trend in I.E. across a period/row? 2. What is the general trend in I.E. down the periodic table? 3. What is the reason for the anomaly/discontinuity between Be and B and between N and O? (which is also repeated in row 3)
  • 15. Topic 2/12 review See practice questions.. (from inthinking & Pearson)