Upper Secondary Pure Chemistry 6092 notes HG

Done by MF (completed in 2024) 1 Upper Secondary Pure Chemistry – Subject Code: 6092 How to use? - This deck of notes can be used as a crash course across O Levels Pure Chemistry syllabus 6092. However, this deck of notes may not have sufficient content and examples for in depth learning. - You are highly encouraged to create your own deck of Chemistry notes that covers more content, while adding in content that you find useful in this deck of notes. - This deck of notes is highly recommended for final revision before exams and tests, as it allows students to cover all the chapters in a glance. - The below is the breakdown of this attachment: o Random overviews o Periodic Table o Qualitative Analysis Notes o List of Definitions (blanks are to be added by you if you find other definitions useful) o Physical State of substance at r.t.p. (blanks are to be added by you if you find other definitions useful) o Notes arranged by chapter Final Tips - This deck of notes should NOT replace what you learn from your teachers. This can only act as a supplementary to aid your learning. - When in doubt, ALWAYS FOLLOW what your CHEMISTRY TEACHERS say - Spread the word and share the notes J (Sharing is caring guys!) - I have other notes as well! o Pure Biology: o Social Studies: o History Elective: - Further questions/ general queries: Reach out to me (https://t.me/your101nolifer) ~ I will try to help, but I do make mistakes at times ~ - ALL THE BEST FOR YOUR STUDIES!

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Done by MF (completed in 2024) 6 QA Notes are… 1. GIVEN during PRACTICAL 2. MEMORISE during WRITTEN 6092 CHEMISTRY GCE ORDINARY LEVEL SYLLABUS 30 NOTES FOR QUALITATIVE ANALYSIS Test for anions anion test test result carbonate (CO32–) add dilute acid effervescence, carbon dioxide produced chloride (Cl –) [in solution] acidify with dilute nitric acid, then add aqueous silver nitrate white ppt. iodide (I–) [in solution] acidify with dilute nitric acid, then add aqueous silver nitrate yellow ppt. nitrate (NO3–) [in solution] add aqueous sodium hydroxide, then aluminium foil; warm carefully ammonia produced sulfate (SO42–) [in solution] acidify with dilute nitric acid, then add aqueous barium nitrate white ppt. Test for aqueous cations cation effect of aqueous sodium hydroxide effect of aqueous ammonia aluminium (Al 3+) white ppt., soluble in excess giving a colourless solution white ppt., insoluble in excess ammonium (NH4+) ammonia produced on warming – calcium (Ca2+) white ppt., insoluble in excess no ppt. copper(II) (Cu2+) light blue ppt., insoluble in excess li ght blue ppt., soluble in excess giving a dark blue solution iron(II) (Fe2+) green ppt., insoluble in excess green ppt., insoluble in excess iron(III) (Fe3+) red-brown ppt., insoluble in excess red-brown ppt., insoluble in excess zinc (Zn2+) white ppt., soluble in excess giving a colourless solution white ppt., soluble in excess giving a colourless solution Test for gases gas test and test result ammonia (NH3) turns damp red litmus paper blue carbon dioxide (CO2) gives white ppt. with limewater (ppt. dissolves with excess CO2) chlorine (Cl2) bleaches damp litmus paper hydrogen (H2) ‘pops’ with a lighted splint oxygen (O2) relights a glowing splint sulfur dioxide (SO2) turns aqueous acidified potassium manganate(VII) from purple to colourless

Done by MF (completed in 2024) 7 Definitions (this list is NON-EXHAUSTIVE) Chapter Term Definition 2 Diffusion Diffusion is the net movement of particles from a region of higher concentration to a region of lower concentration 3 Isotopes Isotopes are atoms of the same element that have the same proton number but different nucleon number. This means they have different number of neutrons. 5 Allotropes Different forms of the same element with different structural arrangement of atoms Alloys A mixture of a metal with one or more other elements *(other elements can be non-metal) 8 Acid An acid is a substance that produces hydrogen ions, H+, in aqueous solutions. Strong Acid A strong acid is an acid that is completely ionized in an aqueous solution Weak Acid A weak acid is an acid that is only partially ionized in an aqueous solution Base A base is any metal oxide or hydroxide. They contain either the oxide ion (O2-) or the hydroxide ion (OH-) Alkali Alkalis are bases that are soluble in water that produces hydroxide ions, OH-, in aqueous solutions. Strong Alkali A strong alkali is an alkali that is completely ionised in an aqueous solution Weak Alkali A weak alkali is an alkali that is only partially ionised in an aqueous solution 14 Noble gases are UNREACTIVE Noble gases have a fully filled valence electron shell and therefore has attained stable electronic configuration. They do not have the tendency to lose, gain or share electrons hence unreactive. 19 Hydrocarbons Hydrocarbons are organic compounds that contain only carbon and hydrogen atoms Saturated Hydrocarbons Saturated hydrocarbons are hydrocarbons that contain only carbon-carbon single bonds between carbon atoms

Done by MF (completed in 2024) 8 Unsaturated Hydrocarbons Unsaturated hydrocarbons are hydrocarbons that contain at least one carbon-carbon double bond between carbon atoms Isomers Isomers are compounds that have the same molecular formula but different structural formula 21 Polymer A large, long-chain molecule made from many units of monomers Physical States of common elements/compounds at room temperature and pressure (r.t.p) Group number Element Physical State at r.t.p. 1 Solid 17 Fluorine / Chlorine Gas Bromine Liquid Iodine / Astatine Solid 3 – 12 (transition metals) Mostly except… Solid Mercury Liquid 18 (Noble gases) Gas Ionic Compound Solid Simple Covalent Compound Gas Giant Covalent Compound Solid Metal / Alloys Solid

Done by MF (completed in 2024) 9 Chapter 1: Experimental Chemistry Apparatus Pipette Measures accurate fixed volumes (e.g. 10.0cm3 or 25.0cm3) – 1 d.p. Volumetric Flask Measures accurate fixed volumes that are larger (e.g. 100 cm3 or 250 cm3) Measuring Cylinder Measures a range of volumes to the nearest 0.5 cm3 (e.g. 31.5 cm3 or 23.0 cm3) Burette Measures a range of volumes to the nearest 0.05 cm3 (e.g. 31.55 cm3 or 23.00 cm3) – most accurate (when 2 d.p. value, usually burette) Collection Method Water Displacement Gas must be insoluble/slightly soluble in water (e.g. Hydrogen, Oxygen, Carbon Dioxide) Downward Delivery Gas must be denser than air – Mr/Ar > 28 (e.g. chlorine, hydrogen chloride, sulfur dioxide) Upward Delivery Gas must be less dense than air – Mr/Ar < 28 (e.g. Ammonia, helium, hydrogen) Drying Agent Concentrated Sulfuric Acid Most gases except basic gas (e.g. ammonia) Quicklime (Calcium Oxide) Gases (ammonia can be dried here) except acidic gases (e.g. Sulfur Dioxide, Carbon Dioxide, Nitrogen Dioxide, Chlorine, Hydrogen Chlorine) Fused Calcium Chloride Gases except those who react with Calcium Chloride (e.g. Ammonia) à must be freshly heated before use

Done by MF (completed in 2024) 10 Separation of Mixtures Magnetic Attraction A magnet can be used to separate magnetic solids from non-magnetic solids (Solid – Solid) Sieving A sieve can be used to separate solids of different particle sizes (Solid – Solid) Suitable Solvents A suitable solvent can be used to separate solid-solid mixtures in which only one of the solids is soluble in the solvent (Solid – Solid) Sublimation Sublimation can be used to separate a substance that changes from the solid to gaseous state directly (Solid – Solid) (e.g. pure iodine, dry ice…) Filtration Filtration can be used to separate insoluble solids from liquids (Solid – Liquid) Evaporation to Dryness Evaporation to dryness is used to separate a dissolved solid from its solvent b