S3.1 The periodic table: Classification of elementsIB Chemistry SL: Flashcards

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What does the period number tell you?

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What does the period number tell you?: The outer main energy level occupied by electrons.
What do elements in the same group share?: The same number of valence (outer) electrons.
Which sublevels define the four blocks?: s, p, d and f.
Configuration of the group 15, period 4 element?: [Ar]3d¹⁰4s²4p³ (arsenic).
Trend in atomic radius across a period, and why?: Decreases: nuclear charge rises while shielding stays similar.
Why is Cl⁻ larger than Cl?: An extra electron adds repulsion with the same nuclear charge.
Order the radii of P³⁻, S²⁻, Cl⁻.: P³⁻ > S²⁻ > Cl⁻: isoelectronic, nuclear charge increases.
Define electronegativity.: The ability of an atom to attract a shared pair of electrons in a covalent bond.
Equation for sodium and water?: 2Na + 2H₂O → 2NaOH + H₂.
Why does group 1 reactivity increase down the group?: The outer electron is further away and more shielded, so it is lost more easily.
Equation for chlorine with bromide ions?: Cl₂ + 2Br⁻ → 2Cl⁻ + Br₂.
Acid–base trend of period 3 oxides?: Basic (Na₂O, MgO) → amphoteric (Al₂O₃) → acidic (SiO₂, P₄O₁₀, SO₃).
Products of SO₂ and SO₃ with water?: H₂SO₃ and H₂SO₄.
Oxidation state of S in H₂SO₄?: +6.