Electron configuration based on position in TPT
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Construction of equations to explain the pH changes for reactions - oxides reacting with waterIonic: basic Na2O + H2O --> 2NaOH MgO + H2O --> Mg(OH)2 Covalent: acidic P4O10 + H2O --> 4H3PO4 SO3 + H2O --> H2SO4 More acidic across period (except group 18)PeriodicityIn Chemistry it refers to the phenomenon that, if the elements are arranged in order of increasing atomic number then a range of both chemical and physical properties show a repeated pattern.Blocks# of orbitals per energy level S 1 D 3 P 5 Lanthanoids + 7 ActinoidsAtomic radiiDecrease across the periods. Increase down a group. Ionic size increase down a group.First ionisation energyis the energy required to remove an electron from a gaseous atom. It increases from left to right across a period and decrease down a group. e- closest to positively charges nuclei is the hardest to remove. M (g) → M+ (g) + e- Difference between first ionisation energy of element in a period: Nuclear charge, energy level (or distance from the nucleus), and repulsion by other electrons (shielding).ElectronegativityAttraction between atom to its electrons in a covalent bond. Decrease down a group, because radii increase.