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Gas Tests Oxygen (O 2 ) – glowing splint test Carbon Dioxide (CO 2 ) – limewater test

Acids Contains H + Ions Neutralises Bases Tastes Sour Low pH Bases Contains OH - Neutralises Acids Tastes Bitter & Feels Soapy Has high pH . Ions Positive (+) = lost electrons Negative (-) = Gained electrons number of protons and neutrons don't change

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Gas Tests Oxygen (O 2 ) – glowing splint test Carbon Dioxide (CO 2 ) – limewater test

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  1. Acids • Contains H+ Ions • Neutralises Bases • Tastes Sour • Low pH • Bases • Contains OH- • Neutralises Acids • Tastes Bitter & Feels Soapy • Has high pH Ions Positive (+) = lost electrons Negative (-) = Gained electrons number of protons and neutrons don't change one negative balances out one positive Solid made oup of ions has Protons, Neutrons, Electrons , Isotopes, Mass Number, Atomic Number Neutral atom: #protons = # electrons Electron arrangement (2,8,8,8) Drawing atoms • Indicators • pH: 0-7 = Acid, 7= Neutral, 7-14 = Base • Litmus:Red=Acid, Blue=Base • Universal Indicator (UI, UTP): • Red / Orange= Acid, • Green = Neutral, • Purple / Blue = Base Ionic bonding strong electrostatic attraction between postive (+) & negative ( -) Ions • Only has elements on it • Metals on the left • Non-metals on the right • Acids & the Salt formed • HCl = Hydrochloric Acid forms Chlorides • H2SO4 = Sulfuric Acid forms Sulfates • HNO3= Nitric Acid forms Nitrates • Common Bases • NaOH = Sodium Hydroxide • KOH = Potassium Hydroxide • Ca(OH)2 = Calcium Hydroxide (limewater) • Each group (column) of periodic table forms the same ion • (same # of valance electrons) • Each period (row) of periodic table • Has the same number of electron shells • Gas Tests • Oxygen (O2) – glowing splint test • Carbon Dioxide (CO2) – limewater test • Hydrogen (H2) - pop test • There are four things that we can change to make the reaction go faster • Temperature • Increase the temperature = the particles have more energy so move faster & collide with other particles more often • Surface area • If we make the pieces of the reactants smaller we increase the number of particles on the surface which can react. • Concentration • If we make one reactant more concentrated. There are more particles in the same volume to react • Using a catalyst • A catalyst is a chemical which is added to a reaction. The catalyst does not get used up in the reaction. • It gives the reaction the energy to get started • Acid + Base Salt + Water • Metal + Acid Metal Salt + Hydrogen • Metal Carbonate + Acid  Salt + CO2+ Water Naming and writing formula Look at Ion table find out charge Positive and negative cancel each other out use swap and drop to balance ion charges (polyatomic ions in brackets if more than 1) Write out the word equationbelow write formula for each substance (use ion table) Write big number in front of formula to balance atoms Should have same number of each element on each side • A chemical reaction involves a collision between particles. The particles collide and make new substances. • More collisions per second result in more effective collisions per second. Therefor reaction occurs faster so a faster rate of reaction

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