Title Chemistry (Secondary) Summary - Y3 2023, New Syllabus.pdf ✅

YEAR 3 SUMMARY BOOKLET UNITS 1 to 11| 2023 EDITION If found, please return this booklet to _____________.
3 Particulate Nature Kinetic Particle Theory | Elements, Compounds & Mixtures 4 Atomic Structure & Bonding 4 Chemical Bonding 5 Acids and Bases includes Ammonia & the Haber Process 7 Qualitative Analysis Contents 8 Mole Concept 9 Reduction & Oxidation 10 Periodic Table 1 Formulae & Equations 11 Metals 2 Experimental Techniques 6 Salts
FORMULAE & EQUATIONS © 2 0 2 3 A F T E R S K O O L L E A R N I N G C E N T R E Elements Compounds Metallic Elements - represented using atomic symbols Diatomic Elements – only seven examples Other Non-Metals - represented using atomic symbols, except two Hydrides Oxides Organic Acids Na sodium Al aluminium H2 hydrogen F2 fluorine C graphite C diamond H2O water CO carbon monoxide CO2 carbon dioxide C6H12O6 glucose HCl hydrochloric acid Mg magnesium Ca calcium N2 nitrogen Cl2 chlorine Si silicon Ar argon NH3 ammonia NO nitrogen monoxide NO2 nitrogen dioxide C2H5OH ethanol HNO3 nitric acid Cu copper Fe iron O2 oxygen Br2 bromine He helium P or P4 phosphorus CH4 methane SO2 sulfur dioxide SO3 sulfur trioxide CH3COOH ethanoic acid H2SO4 sulfuric acid Pb lead Zn zinc I2 iodine Ne neon S or S8 sulfur HCl hydrogen chloride HBr hydrogen bromide HI hydrogen iodide H3PO4 phosphoric acid Cations Anions Group 1 1+ charge Group 2 2+ charge Groups 3 to 12 (see roman numerals) Group 13 3+ charge Special - memorize! Group 15 3– charge Group 16 2– charge Group 17 1– charge Special - memorize! Li+ lithium Be2+ beryllium Cu2+ copper(II) Cu+ copper(I) Al 3+ aluminium NH4 + ammonium N3– nitride O2– oxide F – fluoride OH– hydroxide CO3 2– carbonate Na+ sodium Mg2+ magnesium Fe2+ iron(II) Fe3+ iron(III) Ga3+ gallium Ag+ silver P 3– phosphide S 2– sulfide Cl – chloride NO3 – nitrate SO4 2– sulfate K+ potassium Ca2+ calcium Ni2+ nickel(II) Cr3+ chromium(III) Zn2+ zinc Br– bromide NO2 – nitrite SO3 2– sulfite Li+ lithium Be2+ beryllium Pb2+ lead(II) Pb4+ lead(IV) H+ hydrogen I – iodide PO4 3– phosphate Step 1: Identify reactants and products, i.e. write a word equation. Step 2: Replace names with respective formulae. (If state symbols are needed, add (s), (l), (g) or (aq) after each formula.) Step 3: Balance equation by adding coefficients only. hydrogen + oxygen → water H2 (g) + O2 (g) → H2O (l) 2 H2 (g) + O2 (g) →2 H2O (l) Step 1: Split aqueous ionic compounds into their respective ions. Step 2: Cancel spectator ions, i.e. ions with same formula on both sides. 2 FeCl2 (aq)+Cl2 (g) → 2 FeCl3 (aq) 2 FeCl2 (aq)+Cl2 (g) → 2 FeCl3 (aq) 2 Fe2+ (aq) +Cl2 (g) → 2 Fe3+(aq) + 2 Cl – (aq) ⎯⎯⎯⎯⎯ 2Fe2+ + 4Cl – ⎯⎯⎯⎯⎯ 2Fe3+ + 6Cl – ⎯⎯⎯⎯⎯ 2Fe2+ + 4Cl – ⎯⎯⎯⎯⎯ 2Fe3+ + 6Cl / – 2 Constructing Chemical Equations Constructing Ionic Equations 1
EXPERIMENTAL TECHNIQUES © 2 0 2 3 A F T E R S K O O L L E A R N I N G C E N T R E 2