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IB Chemistry Topic 3 Periodicity 3.2 Periodic Trends
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IB Chemistry Topic 3 Periodicity 3.2 Periodic Trends
The key to doing well in topic 3 is being aware to use the key words and make key word rich concise explanations of the periodic trends in the periodic table. The main ones to remember are effective nuclear charge, valance shell electrons, valance shell/principle energy level, mutual repulsion, electron shielding, electron repulsion, attraction of valance shell electrons to positive protons. Second to that in importance is knowing the definitions (word for word so you don't miss key points) and their symbolic definitions in chemical equation form.
0:04 Atomic radii
2:10 Ionic radii
2:37 First ionisation energy
4:45 Demonstration of effective nuclear charge, electron affinity and ionisation energy
5:50 Electron affinity/Electronegativity
7:25 Displacement reactions with halogen
8:52 Demonstration of electronegativity
9:41 Halogen properties
11:04 Metal and non-metal oxide reactions and pH
3.2 Periodic trends SL
• Vertical and horizontal trends in the periodic table exist for atomic radius, ionic radius, ionization energy, electron affinity and electronegativity.
• Trends in metallic and non-metallic behaviour are due to the trends above.
• Oxides change from basic through amphoteric to acidic across a period.
• Prediction and explanation of the metallic and non-metallic behaviour of an element based on its position in the periodic table.
• Discussion of the similarities and differences in the properties of elements in the same group, with reference to alkali metals (group 1) and halogens (group 17).
• Construction of equations to explain the pH changes for reactions of Na2O, MgO, P4O10, and the oxides of nitrogen and sulfur with water.
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The key to doing well in topic 3 is being aware to use the key words and make key word rich concise explanations of the periodic trends in the periodic table. The main ones to remember are effective nuclear charge, valance shell electrons, valance shell/principle energy level, mutual repulsion, electron shielding, electron repulsion, attraction of valance shell electrons to positive protons. Second to that in importance is knowing the definitions (word for word so you don't miss key points) and their symbolic definitions in chemical equation form.
0:04 Atomic radii
2:10 Ionic radii
2:37 First ionisation energy
4:45 Demonstration of effective nuclear charge, electron affinity and ionisation energy
5:50 Electron affinity/Electronegativity
7:25 Displacement reactions with halogen
8:52 Demonstration of electronegativity
9:41 Halogen properties
11:04 Metal and non-metal oxide reactions and pH
3.2 Periodic trends SL
• Vertical and horizontal trends in the periodic table exist for atomic radius, ionic radius, ionization energy, electron affinity and electronegativity.
• Trends in metallic and non-metallic behaviour are due to the trends above.
• Oxides change from basic through amphoteric to acidic across a period.
• Prediction and explanation of the metallic and non-metallic behaviour of an element based on its position in the periodic table.
• Discussion of the similarities and differences in the properties of elements in the same group, with reference to alkali metals (group 1) and halogens (group 17).
• Construction of equations to explain the pH changes for reactions of Na2O, MgO, P4O10, and the oxides of nitrogen and sulfur with water.
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