Chem notes for help it will, Cheat Sheet of Chemistry

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Formulas • RF = 𝐝𝐝𝐝𝐝𝐝𝐝𝐝𝐝𝐝𝐝𝐝𝐝𝐝𝐝𝐝𝐝 𝐝𝐝𝐭𝐭𝐝𝐝𝐭𝐭𝐝𝐝𝐭𝐭𝐭𝐭𝐝𝐝𝐝𝐝 𝐛𝐛𝐛𝐛 𝐝𝐝𝐭𝐭𝐝𝐝 𝐝𝐝𝐜𝐜𝐜𝐜𝐜𝐜𝐜𝐜𝐝𝐝𝐝𝐝𝐝𝐝𝐝𝐝 𝐝𝐝𝐝𝐝𝐝𝐝𝐝𝐝𝐝𝐝𝐝𝐝𝐝𝐝𝐝𝐝 𝐝𝐝𝐭𝐭𝐝𝐝𝐭𝐭𝐝𝐝𝐭𝐭𝐝𝐝𝐝𝐝 𝐛𝐛𝐛𝐛 𝐝𝐝𝐭𝐭𝐝𝐝 𝐝𝐝𝐜𝐜𝐭𝐭𝐭𝐭𝐝𝐝𝐝𝐝𝐝𝐝 • Relative atomic mass (Ar) = (𝐜𝐜𝐝𝐝𝐝𝐝𝐝𝐝 𝐜𝐜𝐨𝐨 𝐝𝐝𝐝𝐝𝐜𝐜𝐝𝐝𝐜𝐜𝐜𝐜𝐝𝐝 𝟏𝟏 × % 𝐜𝐜𝐨𝐨 𝐝𝐝𝐝𝐝𝐜𝐜𝐝𝐝𝐜𝐜𝐜𝐜𝐝𝐝 𝟏𝟏) + (𝐜𝐜𝐝𝐝𝐝𝐝𝐝𝐝 𝐜𝐜𝐨𝐨 𝐝𝐝𝐝𝐝𝐜𝐜𝐝𝐝𝐜𝐜𝐜𝐜𝐝𝐝) 𝟐𝟐 × % 𝐜𝐜𝐨𝐨 𝐝𝐝𝐝𝐝𝐜𝐜𝐝𝐝𝐜𝐜𝐜𝐜𝐝𝐝 𝟐𝟐) 𝟏𝟏𝟏𝟏𝟏𝟏 • Mass = moles×Mr • Percentage Yield = 𝐀𝐀𝐝𝐝𝐝𝐝𝐀𝐀𝐝𝐝𝐭𝐭 𝐛𝐛𝐝𝐝𝐝𝐝𝐭𝐭𝐝𝐝 𝐓𝐓𝐭𝐭𝐝𝐝𝐜𝐜𝐭𝐭𝐝𝐝𝐝𝐝𝐝𝐝𝐝𝐝𝐝𝐝𝐭𝐭 𝐛𝐛𝐝𝐝𝐝𝐝𝐭𝐭𝐝𝐝 ×100% • Moles=Concentration×volume • q = m × c × △T o q is the heat transferred, j o m is the mass of water, g o c is the specific heat capacity, jg-1K-1 o T is the temperature, K • molar enthalpy change = heat change for the reaction ÷ number of moles, ΔH = q ÷ n • General formula : o Alkane – CnH(2n+2) o Alkene – CnH2n o Alcohol - CnH2n+1OH o Carboxylic acid - CnH2n+1COOH Avogadro constant= 6.02×1023 RTP of gas=24dm3 or 24000cm3 ACRONYMS • OILRIG - (O)xidation (I)s (L)oss of electron, (R)eduction (I)s (G)ain of electrons • PANC - (P)ositive (A)node, (N)egative (C)athode • Reactivity series: potassium please Sodium send Lithium ion Calcium Cat Magnesium Monkey Aluminum and Carbon cute Zinc zebra Iron in Hydrogen hot Copper countries Silver Signed Gold Gordon HALOGENS • Fluorine - Yellow gas • Chlorine - Green gas • Bromine - Red-Brown liquid • Iodine - Grey solid, purple vapor % OF GASES • Nitrogen 78% • Oxygen 21% • Argon 0.9% • Carbon Dioxide 0.04% • Others 0.06% Soluble Salts • All sodium • All potassium • All ammonium • All nitrates • All chloride except - silver, lead • All sulfates except - lead, barium, calcium Insoluble Salts • All carbonates except - sodium, potassium, ammonium, • All hydroxides except - sodium, potassium, (calcium) INDICATORS Indicators Colour in acid Colour in alkaline Methyl Orange red yellow Phenolphthalein colourless pink litmus red blue • universal indicator  red = strongly acidic (pH 0-3)  Orange = weakly acidic (pH 4-6)  Green = neutral (pH 7)  Blue = weakly alkaline (pH 8-10)  Purple = strongly alkaline (pH 11-14) USES AND PROPERTIES • Aluminum  aero planes (low-density)  Electricity cables (good conductor, ductile)  Saucepans (good conductors, malleable) • Low-Carbon steel  Contains 0.25% carbon  hard, strong, malleable, ductile  uses: car bodies, bridges, shipbuilding  disadvantages: high density(heavy), rust easily • High-Carbon steel  contains 0.6 - 1.2% carbon  harder and more resistant to wearing the low-carbon  brittle  uses: cutting tools e.g. knives, sword • Stainless steel  Contains iron, chromium & nickel  Oxide layer prevents corrosion  Uses: sinks, saucepans, cutlery, gardening tools SEPARATION OF MIXTURES • Crystallisation (used to separate self-produced soluble salt from the solution) - React - Filter to remove excess reactant - Heat to evaporate the solvent - Test if the solution is saturated by dipping glass rod, crystal would form on the glass (if saturated) - Cool & filter the solid crystal that form - Wash the crystal with cold distilled water - allow them to dry in a warm place • Simple distillation (used to separate a liquid and soluble solid from a solution) - heat the solution in a boiling flask which connect to a condenser - pure liquid evaporates - vapours cool down in the condenser - Collect pure liquid from the condenser in a beaker - After all the liquid has evaporated only solid solute is left behind • Fractional distillation (used to separate a mixture of two or more liquids with different temperatures) - (Liquid A – Lowest boiling point, Liquid B – Second lowest boiling point) - Heat up to the boiling point of the liquid A - Liquid A will evaporate first - pass the vapours in a condenser to cool & condense - Pure liquid A will form in the condenser - Collect pure liquid A in a beaker - Stop heating immediately when the temperature starts reaching the boiling point of liquid B • Filtration (used to separate undissolved solids in a liquid) - Place filter funnel with filter paper on it above a beaker - Pour the mixture into the filter funnel - Collect liquid in the beaker - Undissolved solids should be left behind in the filter funnel • Fractional distillation(used to separate crude oil) - Crude oil is heated so vapours rise - Vapours of hydrocarbons with very high boiling points will immediately condense into liquid at the higher temperatures lower down and are tapped off at the bottom of the column - Vapours of hydrocarbons with low boiling points will rise up the column and condense at the top to be tapped off - The different fractions condense at different heights according to their boiling points and are tapped off as liquids - The fractions containing smaller hydrocarbons are collected at the top of the fractionating column as gases - The fractions containing bigger hydrocarbons are collected at the lower sections of the fractionating column • Paper Chromatography (used to separate substances that have different solubilities in a given solvent) - Draw a pencil line on chromatography paper - Place spots of the sample - Lower the paper into a solvent container of hot water - Make sure the pencil line sits above the level of solvent - Solvent travels up the paper taking along some substance with it - Different substance with different solubilities travels at different rates - Which shows the different components the sample contains MAKING SALTS Soluble (I). Crystallisation- - React (except NH4+, K+, Na+) : acid + Metal oxide/hydroxide/carbonate - Filter to remove excess reactant - heat to evaporate water - Cool & collect crystals that form - allow them to dry in a warm place (II). Titration: - React (NH4+, K+, Na+) - Acid (in a burette) + Metal hydroxide/carbonate (in a conical flask) - Acid (in a burette) + ammonia solution (in a conical flask) - add an indicator to know when the alkali is neutralized - add acid from the burette until the indicator changes colour and record acid volume - Repeat with the same volume of alkali and acid without any indicator - heat to Evaporate - Cool and collect crystals that form - allow them to dry in a warm place Insoluble (I). Precipitation - React : Soluble salt1 + Soluble salt2 → Insoluble salt + Soluble salt3 - Cool the solution - Filter the Insoluble salt from soluble salt3 solution - Wash the insoluble salt - allow them to dry in a warm place Appearance • Magnesium Oxide – White powder • Magnesium ribbon – Shiny/Silvery • Silver chloride – White • Copper Oxide – Black • Copper(II)Carbonate – Green • Bromine – Red-brown liquid Naming Organic Compound First Part of the name Second part of the name Name Number of carbon atoms Name Functional Group Family Meth… 1 …Ane None Alkane Eth… 2 …Ene C=C Alkene Prop… 3 …Anol R-OH Alcohol But… 4 …Anoic Acid R-C=I-OH Carboxylic Acid Pent… 5 …Amine R-NH2 Amine Hex… 6 …Yl…Anoate R-C=O-O-R Esters