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Questions and Answers
What is the main factor that causes the atomic radius to decrease along a period?
How does adding an electron shell affect the atomic radius down a group?
Which block of elements in the Periodic Table includes transition metals?
Why do elements in the same period have the same number of electron shells?
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What trend is observed in atomic radius along a period?
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In the Periodic Table, which group of elements has the same number of outer electrons?
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What effect does an increase in the number of shells have on electron shielding?
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How does the ionization energy change along a period?
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Which element among Na, Mg, and Al has the highest melting point?
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What type of bonding do sodium, magnesium, and aluminum exhibit?
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What is the trend in ionization energy down a group?
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Why does silicon have a very high melting point compared to sodium, magnesium, and aluminum?
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Study Notes
Atomic Radius Trends
- The main factor that causes the atomic radius to decrease along a period is the increase in the number of protons in the nucleus, which pulls the electrons closer.
- Adding an electron shell down a group increases the atomic radius, as the outer electrons are farther from the nucleus.
Periodic Table Structure
- The d-block of elements in the Periodic Table includes transition metals.
- Elements in the same period have the same number of electron shells because they have the same number of energy levels.
Electron Shielding
- An increase in the number of electron shells decreases electron shielding, allowing the outer electrons to be more easily removed.
Ionization Energy Trends
- Ionization energy increases along a period due to the increasing number of protons in the nucleus, which requires more energy to remove an electron.
- Ionization energy decreases down a group as the outer electrons are farther from the nucleus, making it easier to remove an electron.
Physical Properties
- The alkaline earth metals (Group 2) have the same number of outer electrons.
- Sodium, magnesium, and aluminum exhibit metallic bonding.
- Magnesium has the highest melting point among Na, Mg, and Al due to its stronger metallic bonds.
- Silicon has a very high melting point compared to sodium, magnesium, and aluminum due to its stronger covalent bonds.
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Description
Enhance your understanding of Periodicity with detailed notes from PMT Education for AQA Chemistry A-level 3.2.1. Explore the arrangement of elements in the Periodic Table based on proton number, electron shells, and outer electrons.
