Unit 2: Section 1 - Periodicity
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How are elements in the periodic table arranged?
Elements are arranged according to their proton number
What are the 4 blocks of the periodic table?
• s-block • p-block • d-block • f-block
What elements are in each block of the periodic table?
• s-block - groups 1 and 2 • p-block - groups 3 to 0 • d-block - transition metals • f-block - radioactive elements
What is periodicity?
The study of trends within the periodic table - often linked to elements’ electronic configurations
What is the trend in atomic radius along a period?
Along a period, atomic radius decreases
Why does atomic radius decrease along a period?
• Atomic radius decreases due to an increased nuclear charge for the same number of electron shells • This means that the outer electrons are pulled in closer to the nucleus because the charge produces a greater attraction
What is the trend in atomic radius going down a group?
Going down a group, atomic radius increases
Why does atomic radius increases going down a group?
• With each increment down a group, an electron shell is added • This increases the distance between the outer electrons and the nucleus, reducing the power of attraction • More shells also increases electron shielding, so the attractive forces are reduced
What is the trend in ionisation energy along a period?
Along a period, ionisation energy increases
Why does ionisation energy increases along a period?
• It increases because atomic radius decreases, hence nuclear charge increases • This means that the outer electrons are held more strongly so more energy is required to remove the outer electron and ionise the atom
What is the trend in ionisation energy going down a group?
Going down a group, ionisation energy decreases
Why does ionisation energy decrease going down a group?
• The nuclear attraction between the nucleus and outer electrons reduces and shielding also increases • Both of these factors mean less energy is required to remove the outer electron
What does the melting point of period 3 elements depend on?
• The structure of the element • The bond strength
What happens to melting points across period 3 between sodium and aluminium?
• Sodium, magnesium and aluminium are all metals with metallic bonding - their melting points increase due to the greater positive charge of their ions • This means more electrons are released in the form of free electrons • This increases the attractive electrostatic forces from Na to Al, therefore more energy is needed to break them
Why does the melting point increase dramatically for silicone in period 3?
• Silicon has a very strong giantncovalent structure • So more energy is required to break the strong covalent bonds - giving it a very high melting point
Why does the melting point decrease in period 3 between phosphorus and chloring?
• Phosphorus, sulphur and chlorine are all simple covalent molecules held with weak van der waals forces • Less energy is needed to overcome these weak intermolecular forces, so these molecules have relatively low melting points
Why does argon have an even lower melting point than chlorine?
• Argon is a noble gas that exists as individual atoms with a full outer shell of electrons • This makes the atom very stable and the van der waals forces between them very weak • Less energy is needed to overcome these weak van der waals forces and so argon exists as a gas at room temperature