3.1.1
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What is the arrangement of elements in the periodic table?
Elements are arranged in increasing atomic number
What is a period in the periodic table?
A horizontal row
What is a group in the periodic table?
A vertical column
What does periodicity mean?
The repeating trends in chemical and physical properties
What change occurs across each period?
Elements change from metals to non-metals
How can electron configuration be written in shorthand?
Use the noble gas before the element as a reference
What is first ionisation energy?
The energy required to remove one mole of electrons from one mole of gaseous atoms to form one mole of gaseous 1+ ions
Write the equation for the first ionisation energy of magnesium.
Mg(g) → Mg⁺(g) + e⁻
What factors affect ionisation energy?
Atomic radius, nuclear charge, electron shielding
Explain the trend in first ionisation energy across period 3.
It increases due to increased nuclear charge, decreased atomic radius, and constant electron shielding
Why is there a dip in ionisation energy between groups 2 and 3?
In group 3, the outer electron is in a higher energy p-orbital, making it easier to remove
Why is there a dip in ionisation energy between groups 5 and 6?
In group 6, the outer electron is paired in a p-orbital, causing electron-electron repulsion and making it easier to remove
Does first ionisation energy increase or decrease between the end of one period and the start of the next?
It decreases due to increased atomic radius and electron shielding
Does first ionisation energy increase or decrease down a group?
It decreases because of increased electron shielding and atomic radius
What are the properties of giant metallic lattices?
High melting and boiling points, good electrical conductors, malleable, ductile
What is a ductile metal?
A metal that can be stretched into wires
What is a malleable metal?
A metal that can be hammered or rolled into sheets
Describe the structure, forces, and bonding in elements across period 2.
Li & Be: Giant metallic; strong attraction between positive ions and delocalised electrons; metallic bonding. B & C: Giant covalent; strong forces between atoms; covalent bonding. N₂, O₂, F₂, Ne: Simple molecular; weak intermolecular forces; covalent bonding within molecules.
Describe the structure, forces, and bonding in elements across period 3.
Na, Mg, Al: Giant metallic; strong attraction between positive ions and delocalised electrons; metallic bonding. Si: Giant covalent; strong forces between atoms; covalent bonding. P₄, S₈, Cl₂, Ar: Simple molecular; weak intermolecular forces; covalent bonding within molecules.