chemistry c1

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  • Created by: sadiyah:)
  • Created on: 09-03-20 17:28
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  • atomic structure C1
    • isotope same number of neutrons. ion atom where number of protons is not equal to electrons
    • atomic number is the number of protons
    • mass number is number neutrons+protons
    • conservation of mass in a chemical reaction the total mass of reactants = total mass of products
    • mixture two or more chemicals not chemically bonded
    • neutron charge of 0. mass of 1. found inside the nucleus
    • protons charge of +1. mass of 1. found inside the nucleus
    • nucleus the centre of the atom. contains neutrons and protons
    • compound is two or more different elements chemically bonded
    • an element is only one type or atom present. can be single atom or molecule
    • a molecule is two or more atoms chemically bonded
    • atom is smallest part of an element that can exist
    • paper 1 chemistry:)
      • The periodic table C2
        • Mendeleev scientist who placed elements in order to atomic weight but left gaps for undiscovered elements
        • metals have delocalised electrons that can move. atoms lose electrons and become positive ions
        • non-metals  have electrons that cannot move. nearly always gain electrons and become negative ions
        • group 0 unreactive full outer shell. boiling point increases as you go down the group
        • group 1 very reactive: only one electron  in their outer shell
          • react with water to give metal hydroxide and hydrogen eg MgOH
          • react with oxygen to give metal oxides eg MgO
          • reactivity increases as you go down the group
          • react with chlorine to give metal chloride eg MgCl
        • group 7 halogens melting and boiling point increase as you go down group
          • reactivity decreases as you go down group
          • a more reactive halogen will displace a less reactive one
      • structure and bonding C3
        • chemical bonds hold atoms together in a molecule after a reaction
        • ionic bonding is metal + non metal
          • metal loses electrons and become a positive ion. non metal gains the electrons and becomes a negative ion
        • giant ionic structures has high melting and boiling points and conduct electricity when melted or dissolved in water
        • metallic bonding metal+ metal
          • giant structures with free electrons moving throughout
        • conductors metals conduct electricity  because they have free electrons
        • graphite non-metal that conducts electricity
        • alloys a mixture of different metals. which are then harder
        • states of matters solid,liquid and gas
        • covalent bonding non-metal +mon - metal
          • atoms share elecrtons
        • giant covalent structures solids. very high melting points
        • small molecules usually gases or liquids. do not conduct electricity
        • polymers long chain molecules linked by strong covalent bonds
        • state symbols: (s) solid (l) liquids (g) gas (aq) aqueous soloution
      • chemical calculations c4
        • relative atomic mass the mass number of an atom
        • relative formula mass the mass of all the atoms of a molecule added together
        • solute solid that has been dissolved
        • isotope same number of protons different number of neutrons
        • number in reaction equations big numbers in front of a chemical tell us how many molecules / atoms of the chemical there are
        • balancing equations the number of atoms in the reactants must equal the number of atoms in the products
        • conservation of mass in a chemical reaction the total mass of reactants = total mass of products
        • if mass seems to be lost / gained conservation of mass always applies but sometimes the mass of a gas being used / made is missed
        • concentrations the mass of solute in given volume of solution
        • solution liquid containing dissolved solute
      • chemical changes C5
        • oxidation losing electrons
        • reduction gaining electrons
        • OIL RIG oxidation is loss of electrons reduction is gain of electrons
        • reactivity series list of metals with  most reactivity at top and least reactive metals at bottom the most reactive metals are most likely to lose electrons
        • displacement reaction a ore reactive metal will displace a less reactive metal from a chemical compound
        • ion atom where number of protons is not equal to electrons
        • PH scale 1 strong acid 7 neutral 14 strong alkali
        • universal indicator turns red in strong acid, turns green in neutral, turns purple in strong alkali
        • base usually contains OH ions.opposite of an opposite
        • acids contains  H ions opposite of a base
        • alkali a base that has been dissolved in water
        • test for hydrogen... hydrogen makes a squeaky pop when lit with a splint
        • test for carbon dioxide if you bubble carbon dioxide through limewater it will turn milky cloudy white
      • electrolysis C6
        • electrolysis breaking down a substance using electricity
        • the ionic compound that is broken down in electroloysis
          • must be ionic compound in liquid form
        • electrode connected  to the power supply
        • anode the positive electrode
        • cathode the negative electrode
        • ion atom where number of protons is not equal to electrons
        • positive ions metals and hydrogen collect at the cathode
        • negative ions non metals except hydrogen collect at anode
        • aluminium obtained by molten bauxite ore
        • cryolite used to extract aluminium
        • ore rock containing enough metal to be worth extacting
        • brine salt water
          • can be separated using electrolysis to produce chlorine, hydrogen and sodium hydroxide
        • test for oxygen relight a glowing splint
      • energy changes C7
        • exothermic reaction one that transfers energy to the surroundings so the temperature of the surroundings increases
          • used in hard warmers and self heating cans e.g combustions respiration oxidation netralisation
        • endothermic reaction one that absorbs energy from the surroundings so the temp
          • used in cold packs for injuries e.g photosynthesis citric acid and sodium hydrogen
        • reactant used in a reaction
        • product made in a reaction
        • conservation of energy. energy is never created or destroyed it is just transferred from one form to another
        • activation energy is the energy required to start a reaction
        • catalyst chemical which speeds up a reaction without being used itself
          • reduces the activation energy required to start a reaction
        • breaking and making bonds this is what happens during a chemical reaction
          • require energy in to break bonds energy is released when bonds are made
          • bonds between different atoms need different amounts of energy
    • electrons charge of -1 mass of almost 0. found orbiting around the nucleus
    • electron energy levels in the first shell there is 2 electrons then second shell there is 8 then the third is 8 again
  • group 1 very reactive: only one electron  in their outer shell
    • react with water to give metal hydroxide and hydrogen eg MgOH
    • react with oxygen to give metal oxides eg MgO
    • reactivity increases as you go down the group
    • react with chlorine to give metal chloride eg MgCl

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