H2 Chemistry 12 - Periodic Table

across period, no. of e^- in same quantum shell ↑, no. of quantum shells constant

down group, no. of quantum shells ↑, no. of valence e^- constant

radii ↓ >

↑ in no. of protons while shielding effect remains relatively constant due to same no. of inner shell e^- >

nuclear attraction on valence e^- ↑

radii ↑ >

↑ in no. of principle quantum shells, valence e- further from nucleus >

↑ in shielding effect outweighs ↑ in nuclear charge >

nuclear attraction on valence e^- ↓

1st IE ↑ >

↑ in nuclear charge, shielding effect relatively constant due to same no. of inner shell e^- >

nuclear attraction valence e^- ↑ >

> energy req remove 1 e^-

1st IE ↓ >

↑ in no. of principal quantum shells, valence e^- further from nucleus >

shielding effect ↑ by more inner shell e^- outweighs ↑ in nuclear charge >

< energy req remove 1 e^-

↑; nuclear charge ↑, shielding effect relatively constant >

nuclear attraction on valence e^- ↑, electronegativity ↑

↓; ↑ in no. of principal quantum shells, valence e- further from nucleus >

↑ in shielding effect outweighs ↑ in nuclear charge >

↓ nuclear attraction on valence e^-, electronegativity ↓

Na<Mg<Al; mp ↑>

↑ amount of energy req overcome ↑ strength of metallic bonds b/w respective metal cations, mobile delocalised e- as no. of delocalised e- ↑, charge density ↑ as atomic radii ↓

Si highest >

giant covalent structure, large amount energy req overcome strong covalent bonds b/w Si atoms

S₈<P₄<Cl₂<Ar >

Cl₂,P₄,S₈; simple molecular structure, Ar; simple monoatomic structure >

↓ amount of energy req overcome ↓ strength of id-id attractions b/w molecules as no. of e^- per molecule to be polarised ↓ in same order

Na<Mg<Al; ↑>

metallic bonding, delocalised valence e- act as mobile charge carriers >

no. of such e- ↑ from Na to Al

P4<Al<Si >

Si metalloid; semi-conductor w/ low conductivity

S₈, P₄, Cl₂, Ar poor conductors, mobile charge carriers absent

down group, no. of e- to be polarised per molecule ↑ >

due to ↑ in quantum shells of inner e- >

↑ strength of id-id attractions b/w molecules, > heat energy required >

< volatile

Cl most electronegative among P3 elements, O > electronegative than P3 elements >

P3 elements always +ve OS as lose e^- >

max OS ↑ across period as > valence e^- used for bonding in oxide >

P forms PCl3/PCl5 as can expand octet config using low-lying vacant 3d orbitals

Na₂O, MgO, Al₂O₃ giant ionic lattice;

SiO₂ giant covalent structure;

P₄O₁₀, SO₃ simple molecular structure >

bonding △ from ionic to covalent across period as electronegativity difference b/w P3 elements & O ↓

NaCl, MgCl₂ giant ionic lattice;

AlCl₃ ionic w/ covalent character;

SiCl₄, PCl₅ simple molecular structure >

bonding △ from ionic to covalent across period as electronegativity difference b/w P3 elements & Cl ↓ >

however AlCl3 is ionic w/ covalent character, high charge density of AlCl₃, Al³⁺ distorts e- cloud such that there is orbital overlap b/w Al, Cl form covalent bonds

Na₂O(s) + H₂O(l) → 2NaOH(aq)

MgO(s) + H₂O(l) ⇌ Mg(OH)₂(s)

Mg(OH)₂(s) + aq ⇌ Mg²⁺(aq) + 2OH^-(aq)

Al₂O₃(s) insoluble in water

SiO₂(s) insoluble in water

P₆O₁₀(s) + H₂O(l) → 4H₃PO₄(aq)

SO₃(l) + H₂O(l) → H₂SO₄(aq)

Na₂O; react vigorously form strong alkaline pH 13-14

MgO; react small extent form Mg(OH)₂(s) sparingly soluble, form weak alkaline pH 9

Al₂O₃; insoluble, high magnitude of lattice energy - energy evolved forming ion-dipole interactions insufficient overcome strong ionic bonds b/w oppositely charged ions

SiO₂; insoluble, large amt energy req break many strong Si-O bonds

P₆O₁₀; react form acidic soln pH 2

SO₃; react form strongly acidic soln pH 1

Na₂O(s) + 2H⁺ → 2Na⁺(aq) + H₂O(l)

MgO(s) + 2H⁺ → Mg²⁺(aq) + H₂O(l)

Al₂O₃ reacts w/ both acids, alkalis

Al₂O₃(s) + 6H⁺(aq) → 2Al³⁺(aq) + 3H₂O(l)

Al₂O₃(s) + 2OH^-(aq) + 3H₂O(l) → 2[Al(OH)₄]^-(l)

SiO₂ reacts ONLY w/ hot conc alkali due to GCS

SiO₂(s) + 2OH^-(aq) → SiO₃^2-(aq) + H₂O(l)

P₆O₁₀(s) + 12OH^-(aq) → 4PO₄^3-(aq) + 6H₂O(l)

SO₃(g) + 2OH^-(aq) → SO₄^2-(aq) + H₂O(l)

across P3, nature △ from basic>amphoteric>acidic >

bonding △ from ionic>covalent, electronegativity diff b/w P3 elements, O ↓ >

metallic oxides/hydroxides ionic, ionic oxides/hydroxides basic >

non-metallic oxides covalent, covalent oxides acidic >

ionic w/ covalent character amphoteric

NaOH(s) + H⁺(aq) → Na⁺(aq) + H₂O(l)

Mg(OH)₂(s) + 2H⁺(aq) → Mg²⁺(aq) + 2H₂O(aq)

Al(OH)₃(s) + 3H⁺(aq) → Al³⁺(aq) + 3H₂O(l)

Al(OH)₃(s) + OH^-(aq) → [Al(OH)₄]^-(aq)

NaCl(s) + aq → Na⁺(aq) + Cl^-(aq)

MgCl₂(s) + 6H₂O(l) → [Mg(H₂O)₆]²⁺(aq) + 2Cl^-(aq)

[Mg(H₂O)₆]²⁺(aq) ⇌ [Mg(H₂O)₅OH]⁺(aq) + H⁺(aq)

AlCl₃(s) + 6H₂O(l) → [Al(H₂O)₆]³⁺(aq) + 3Cl^-(aq)

[Al(H₂O)₆]³⁺(aq) ⇌ [Al(H₂O)₅OH]²⁺(aq) + H⁺(aq)

SiCl₄(l) + 2H₂O(l) → SiO₂(s) + 4HCl(aq)

hot excess water

PCl₅(s) + 4H₂O(l) → H₃PO₄(aq) + 5HCl(aq)

cold excess water

PCl₅(s) + H₂O(l) → POCl₃(l) + 2HCl(aq)

NaCl; dissolve give neutral soln(low charge density, no hydrolysis) pH 7

MgCl₂; dissolve give [Mg(H₂O)₆]²⁺, hydrolyses slightly(higher charge density) give slightly acidic soln pH 6.5

AlCl₃; dissolve give [Al(H₂O)₆]³⁺, hydrolyses(high charge density) give acidic soln pH 3

SiCl₄, PCl₅; covalent chlorides hydrolyse completely give strongly acidic soln as HCl formed, pH 1-2 >

central atom has low-lying vacant 3d orbitals form dative bond w/ water by accepting lp of e^- on O to form unstable transition state, break down form HCl

down group, E^⦵ value ↑ly -ve >

> readily oxidised >

reducing power ↑

down group, E^⦵ value ↓ly +ve >

< readily reduced >

oxidising power ↓

polarising power of M²⁺; larger charge density, greater ability polarise C-O bond of CO₃^2-, bond weakened to larger extent

polarisability of anion; polarisability measures how easily e- cloud distorted by M²⁺, larger size of anion, greater its polarisability

down group, thermal stability ↑ >

ionic radius of M²⁺ ↑, charge density of M²⁺ ↓ >

ability of M²⁺ polarise large anion ↓, C-O bond weakened to smaller extent >

> heat energy req overcome stronger (bonds) idk what bonds

down group, thermal stability ↓ >

atomic radius ↑ from Cl to I >

bond length of H-X ↑ >

strength of H-X bond ↓ >

< heat energy req overcome weaker H-X bonds