chemistry c1
- 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
- exothermic reaction one that transfers energy to the surroundings so the temperature of the surroundings increases
- The periodic table C2
- 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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