This page contains the AQA AS Chemistry Periodicity Questions and their Kerboodle answers for revision and understanding Periodicity.This page also contains the link to the notes and video for the revision of this topic.
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8.1 The Periodic Table AQA AS Chemistry C8 Periodicity Kerboodle Answer: Page No.142
1.Ans-- i)K,Br (ii) Br,Cl (iii) Br,Cl
- i) Fe (ii) K
- Xe
- Ti
- Sr
- Xe
- Ti
- Left,middle
- Right
8.2 Trend The Properties Of Elements AQA AS Chemistry C8 Periodicity Kerboodle Answer: Page No.145
4.Ans-- Group 18
- Group 14
Practice Questions-
1.Ans-- Silicon has a giant covalent structure.
- Both sulfur and phosphorus are simple molecules with covalent bonding though sulfur molecules are larger.The melting point of sulfur is higher than that of phosphorus because the van der waals forces are stronger in case of sulfur so more energy is required.
- Aluminium is malleable, and ductile due to its polycrystalline structure and when force is applied to it the atoms roll over each other they just move from one lattice site to another.
- The melting point of aluminium is higher than that of sodium because the metallic bonding is stronger in case of aluminium in comparison to sodium due to greater nuclear charge and smaller size.
- Lithium has the largest atomic radius
- i) The ionization energy increases on moving from left to right in a period i.e from going to lithium it increases.
- ii) Boron deviates from the general trend.This is because its valence electron (2p1) of Boron is shielded by the 2s electrons, less energy is required to remove the the 2p electron(s) from a boron atom than is requried to remove the 2s electron from a beryllium atom.
- Carbon
- Melting point of carbon is high as it has very strong covalent bonds holding the atoms together in a long chain or giant structures.
- i)
- ii) 1s2,2s2,2p6,3s1
- iv) Second ionization energy of silicon is lower than the second ionization energy of aluminium because the second electron of silicon is a 3p1 electron while that of aluminium is 3s2 electron and 3p has a lower binding energy than that of 3s electron.
- Sodium because after losing one electron it attains noble gas configuration and is highly stable.
- Silicon
- The ionization energy of every element is endothermic because electron is to be removed from the atom against the nuclear force of attraction hence energy is absorbed by the atom.
- From carbon to fluorine carbon has largest atomic size because it has least nuclear charge.
- Generally ionization energy of elements increases across the period from left to right.
- Oxygen deviates from this trend.It has a ionisation energy lower than that of oxygen has nitrogen has a half filled electronic configuration 1s2,2s2,3p3which is more stale than an incomplete p-orbital if oxygen.
- Second ionisation energy of carbon is higher than the first ionisation energy of carbon because after removal of the first electron the number of protons increases in comparison to number of electrons hence a greater electrostatic pull is experienced by the electrons.
- Lithium has highest second ionisation energy since after the removal of one electron it attains a noble gas configuration.