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Essential ideas:
- The arrangement of elements in the periodic table helps to predict their electron configuration.
- Elements show trends in their physical and chemical properties across periods and down groups.
3.1 Groups and periods, metals and non-metals (introduction to the periodic table)
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Understandings:
The periodic table consists of groups (vertical columns) and periods (horizontal rows). The periodic table shows the positions of metals, non-metals and metalloids. The period number (n) is the outer energy level that is occupied by electrons. The number of the principal energy level and the number of the valence electrons in an atom can be deduced from its position on the periodic table. |
| new_syllabus_the_periodic_table.pdf |
3.1 Electron configuration and the periodic table
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Understandings:
The periodic table is arranged into four blocks associated with the four sub- levels--s, p, d, and f. Applications and skills: Deduction of the electron configuration of an atom from the element’s position on the periodic table, and vice versa. |
| electronic_configurations_and_the_periodic_table.pdf |
3.2 Electron shielding and effective nuclear charge
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This video covers the trends in electron shielding and effective nuclear charge in the periodic table.
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3.2 Trends in atomic radii
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Understandings:
Vertical and horizontal trends in the periodic table exist for atomic radius, ionic radius, ionization energy, electron affinity and electronegativity. |
3.2 Trends in ionic radii
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Understandings:
Vertical and horizontal trends in the periodic table exist for atomic radius, ionic radius, ionization energy, electron affinity and electronegativity. |
3.2 Trends in ionisation energy
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Understandings:
Vertical and horizontal trends in the periodic table exist for atomic radius, ionic radius, ionization energy, electron affinity and electronegativity. Guidance: For ionization energy the discontinuities in the increase across a period should be covered. |
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Guidance:
For ionization energy the discontinuities in the increase across a period should be covered. This video covers the exceptions to the trend in ionisation energy across a period. |
3.2 Trends in electronegativity
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Understandings:
Vertical and horizontal trends in the periodic table exist for atomic radius, ionic radius, ionization energy, electron affinity and electronegativity. |
| topic_3_trends_in_electronegativity_and_electron_affinity.pdf |
3.2 Trends in metallic character
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Understandings:
Trends in metallic and non-metallic behaviour are due to the trends above. Applications and skills: Prediction and explanation of the metallic and non-metallic behaviour of an element based on its position in the periodic table. |
3.2 Trends in electron affinity
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Understandings:
Vertical and horizontal trends in the periodic table exist for atomic radius, ionic radius, ionization energy, electron affinity and electronegativity. |
3.2 Trends in melting points
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This video covers the trend in melting point across periods 2 and 3 in the periodic table.
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| topic_3_trends_in_melting_point.pdf |
3.2 Physical and chemical properties of the group 1 alkali metals (old version)
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Applications and skills:
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). |
| topic_3_group_1_alkali_metals.pdf |
3.2 Group 1 metals (new version)
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Applications and skills:
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). A note about Francium - it is a radioactive element with a very short half-life. More information can be found here. |
3.2 Physical and chemical properties of group 17 elements - the halogens.
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Applications and skills:
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). |
| topic_3_group_17_elements.pdf |
3.2 Bonding and acid-base properties of the period 3 oxides
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Understandings:
Oxides change from basic through amphoteric to acidic across a period. Applications and skills: Construction of equations to explain the pH changes for reactions of Na2O, MgO, P4O10, and the oxides of nitrogen and sulfur with water. |
| topic_3_bonding_of_the_period_3_oxides.pdf |