Paper 1

    Cards (85)

    • Isotope
      An atom with the same number of protons and electrons but different numbers of neutrons
    • Ionic bonding
      1. Metal atoms become positive ions
      2. Non-metal atoms become negative ions
    • An ionic bond can only be formed between a metal and a non metal
    • Element
      Only one type of atom
    • Compound
      Made from two or more types of atoms chemically bonded together
    • Mixture
      Made from two or more types of atoms not chemically bonded together (easy to separate)
    • Subatomic particles in an atom
      • Protons
      • Neutrons
      • Electrons
    • Nucleus
      In the middle of an atom and is made up of protons and neutrons
    • On an atom there are the same number of protons and electrons
    • Protons and neutrons cannot be transferred, only electrons
    • Maximum number of electrons on atom shells
      • First outer shell: 2
      • Other shells: 8
    • Group 1 - alkali metals

      • Put them in water and they will catch on fire
      • Put them in acid they will catch on fire but a bigger reaction
      • The further you go down the bigger the reaction
    • Group 7 - halogens
      • Dangerous
      • Toxic to humans
      • React similarly because they all have the same number of electrons on their outer shell
    • Group 8 - noble gases
      • Completely unreactive because they have a full outer shell of electrons
    • Neutralization
      Reaction between an acid and a base
    • Combination
      Two or more substances combine to form a single new substance
    • Combustion
      Fuel combines with oxygen
    • Electrolysis
      Using electricity to break down electrolytes to form elements
    • Covalent Bonding
      A bond formed between two non metals atoms where the atoms share pairs of electrons
    • Metallic Bonding
      A bond formed between two or more metal atoms, where the atoms share delocalised electrons
    • Polymers
      • Long chains of molecules joined together by strong covalent bonds
      • They have strong intermolecular forces meaning they have high melting and boiling points
    • Metals consist of giant structures of atoms arranged in regular patterns
    • Alloy
      A mixture of two or more elements with one being a metal
    • Most alloys are mixtures of two or more metals
    • Alloys
      • They are harder than pure metals as the atoms are arranged in irregular patterns making it more difficult for layers of atoms to slide over each other
    • Diamond
      Forms giant covalent structures with no delocalised electrons and each carbon atom is joined to four other carbon atoms
    • Graphite
      • Forms giant covalent structures with delocalised electrons and each carbon atom is joined to three other carbon atoms
      • The carbon atoms form layers and the layers have no covalent bonds between them
    • Diamond and graphite are both different forms of the element carbon. Both of their structures are hold together by covalent bonds. Since their structures are different their properties are also different.
    • PH range
      • 1-6 = acids
      • 7 = water/neutral
      • 8-14 = alkali
    • The closer to 1
      The more acidic
    • The closer to 14
      The more alkaline
    • Acid
      Has H+ ions (positive hydrogen ions)
    • Alkali
      Has OH- (hydrogen peroxide ions)
    • Universal indicator in an acid
      1. If weak acid, turns more yellow and orange
      2. If strong acid, turns more orange and red
    • Universal indicator in an alkali
      1. If weak alkali, turns blue
      2. If strong alkali, turns more purple/violet
    • Universal indicator in water/neutral
      Turns green
    • Alkali metal flames
      • Lithium - Crimson red
      • Sodium - Golden yellow
      • Potassium - Pale violet
    • Melting point
      The temperature at which a solid substance changes to a liquid state
    • Substances have high melting point

      It takes a lot of energy to break the bonds between
    • Pure substance
      A single substance