Flashcards · 0620 · Topic 8

The Periodic Table flashcards

20 cards on Topic 8, subtopics 8.1 to 8.5. Pick a subtopic or study them all.

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How is the Periodic Table arranged?: In order of increasing proton number. Columns are groups; rows are periods.
How does character change across a period?: From metallic on the left to non-metallic on the right.
Why do elements in the same group have similar chemical properties?: They have the same number of outer-shell electrons.

Physical properties of lithium, sodium and potassium: Relatively soft metals with low density and low melting points.
Group I: trends down the group: Reactivity increases. Melting point decreases. Density generally increases.
Group I metal + water →: metal hydroxide + hydrogen e.g. 2Na + 2H₂O → 2NaOH + H₂

Colour and state of chlorine, bromine and iodine at room temperature: Chlorine: pale yellow-green gas. Bromine: red-brown liquid. Iodine: grey-black solid.
Group VII: trends down the group: Reactivity decreases. Colour gets darker. Density and melting point increase.
Chlorine water is added to potassium bromide solution. What happens?: Chlorine is more reactive, so it displaces bromine: chlorine + potassium bromide → potassium chloride + bromine. The solution turns orange.
Halogen molecules: Diatomic: Cl₂, Br₂, I₂.

Properties of transition elements: High densities and high melting points. They form coloured compounds, and they and their compounds often act as catalysts.
Variable oxidation numbers: 0620’s named exampleExtended: Iron: Fe²⁺ (iron(II)) and Fe³⁺ (iron(III)).
Transition elements compared with Group I metals: density, melting point and reactivity: Transition elements: high density, high melting point, low reactivity. Group I metals: low density, low melting point, very high reactivity.
Compounds of Group I metals and of transition elements: colour: Group I compounds are white or colourless. Transition element compounds are coloured.
Ion charges: Group I metals compared with transition elementsExtended: Group I metals always form 1+ ions. Transition elements form ions with variable charges, e.g. Fe²⁺ and Fe³⁺.

Noble gases (Group VIII): physical form: Unreactive, monatomic gases.
Why are the noble gases unreactive?: They have a full outer shell of electrons, so they do not need to lose, gain or share electrons.
Electronic configurations of neon and argon, and what they explain: Neon is 2,8 and argon is 2,8,8. Each has a full outer shell, so its atoms have no tendency to lose, gain or share electrons: the gases are unreactive.
Monatomic: Existing as single, separate atoms rather than as molecules. The noble gases are monatomic, unlike the diatomic halogens.
A use of helium, of neon and of argon: Helium: balloons (low density, non-flammable). Neon: lighting. Argon: lamps and welding (an inert atmosphere).