Inorganic 1 Section 2 - Unit 8: Periodicity
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Write an equation, including state symbols, to show the process that occurs when the first ionisation energy of an element is measured (1 mark)
X(g) → X+(g) + e–
State and explain the trend in atomic radius from phosphorus to chlorine (3 marks)
• Decreases • Number of protons increases • Attracting outer electrons in the same shell
In terms of atomic structure, explain why the van der Waals’ forces in liquid argon are very weak (2 marks)
• Argon particles are single atoms with electrons closer to nucleus • So they cannot easily be polarised
Describe the bonding in metals (2 marks)
• Lattice of positive ions - Surrounded by delocalised electrons
Explain how metals conduct electricity (2 marks)
• Delocalised electrons - Flow in a given direction
Explain the meaning of the term periodicity as applied to the properties of rows of elements in the Periodic Table (2 marks)
• Trend in the properties of elements across a period - Repeated in the next row
Describe and explain the trend in atomic radius across a period (3 marks)
• Decreases across the row • Since the number of protons increases • So there’s more attraction for electrons in same shell
Describe and explain the trend in electronegativity across a period (4 marks)
• Increases across the row • Since the number of protons increases • Atomic radius decreases • More attraction for bonding or shared electrons
Describe and explain the trend in conductivity across a period (4 marks)
• Decreases across the row • Left hand side are metals • Right hand side are non-metals • Electrons free to move (or delocalised) in metals but aren’t able to in non-metals