Gas Tests Oxygen (O 2 ) – glowing splint test Carbon Dioxide (CO 2 ) – limewater test Hydrogen (H 2 ) - pop test Gas Tests Oxygen (O 2 ) – glowing splint test Carbon Dioxide (CO 2 ) – limewater test Hydrogen (H 2 ) - pop test Only has elements on it Metals on the left Non-metals on the right Only has elements on it Metals on the left Non-metals on the right 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 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 Protons, Neutrons, Electrons, Isotopes, Mass Number, Atomic Number Neutral atom: #protons = # electrons Electron arrangement (2,8,8,8) Drawing atoms 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 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 Acids Contains H + Ions Neutralises Bases Tastes Sour Low pH Bases Contains OH - Neutralises Acids Tastes Bitter & Feels Soapy Has high pH Acids Contains H + Ions Neutralises Bases Tastes Sour Low pH Bases Contains OH - Neutralises Acids Tastes Bitter & Feels Soapy Has high pH Indicators pH: 0-7 = Acid, 7= Neutral, 7-14 = Base Red=AcidBlue=Base Litmus: Red=Acid, Blue=Base Universal Indicator (UI, UTP): Red / Orange= Acid, Green = Neutral, Purple / Blue = Base Indicators pH: 0-7 = Acid, 7= Neutral, 7-14 = Base Red=AcidBlue=Base Litmus: Red=Acid, Blue=Base Universal Indicator (UI, UTP): Red / Orange= Acid, Green = Neutral, Purple / Blue = Base Acid + Base  Salt + Water Metal + Acid  Metal Salt + Hydrogen Metal Carbonate + Acid  Salt + CO 2 + Water Acid + Base  Salt + Water Metal + Acid  Metal Salt + Hydrogen Metal Carbonate + Acid  Salt + CO 2 + 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) 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 equation below 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 Write out the word equation below 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 Acids & the Salt formed HCl = Hydrochloric Acid forms Chlorides H 2 SO 4 = Sulfuric Acid forms Sulfates HNO 3 = Nitric Acid forms Nitrates Common Bases NaOH = Sodium Hydroxide KOH = Potassium Hydroxide Ca(OH) 2 = Calcium Hydroxide (limewater) Acids & the Salt formed HCl = Hydrochloric Acid forms Chlorides H 2 SO 4 = Sulfuric Acid forms Sulfates HNO 3 = Nitric Acid forms Nitrates Common Bases NaOH = Sodium Hydroxide KOH = Potassium Hydroxide Ca(OH) 2 = Calcium Hydroxide (limewater) 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 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 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 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 AS Science 1.5 Chemistry Exam The Atom Acids & Bases Rate of Reaction Formula & Equations Periodic Table Ionic bonding strong electrostatic attraction between postive (+) & negative ( -) Ions Ionic bonding strong electrostatic attraction between postive (+) & negative ( -) Ions