Chemistry extrasssss:

• What do electrons occupy in an atom?

  Shells, also called energy levels
• How do electrons fill the shells in an atom?

  Electrons fill each shell up before occupying a new one, starting with the lowest energy
• How many electrons are allowed in the first shell?

  2 electrons
• How many electrons can the second shell hold?

  8 electrons
• How many electrons can the third shell hold?

  8 electrons
• Where are the lowest energy shells located in relation to the nucleus?

  They are closest to the nucleus
• How can electronic structure be represented numerically?

  As numbers, for example, 2, 8, 1
• What are metals defined as in terms of ion formation?

  Elements that can form positive ions when they react
• How do non-metals behave in terms of ion formation?

  They don't generally form positive ions
• How do metals achieve a full outer shell?

  By losing electrons
• How do non-metals achieve a full outer shell?

  By gaining or sharing electrons
• When are metals more reactive?

  When they lose electrons more easily
• When are non-metals more reactive?

  When they gain electrons more easily
• Where on the periodic table are metals more reactive?

  Towards the bottom left
• Where on the periodic table are non-metals more reactive?

  Towards the top right
• What are the general properties of metals and non-metals?

  Metals:

  • Shiny appearance
  • Strong but malleable
  • High melting and boiling points
  • Good electrical and thermal conductors

  
  

  Non-metals:

  • Dull appearance
  • Brittle
  • Low melting and boiling points
  • Poor conductors
• What are transition metals?

  Metals in the centre of the periodic table
• Name an example of a transition metal.

  Iron (Fe)
• What are three main differences of transition metals compared to other metals?

  They have multiple ions, form colourful compounds, and can be good catalysts
• What is the common name for the Group 1 metals?

  Alkali metals
• What trend occurs in reactivity as you go down Group 1?

  Reactivity increases
• What happens to melting and boiling points as you go down Group 1?

  They decrease
• What happens to relative atomic mass as you go down Group 1?

  It increases
• What are the properties of Group 1 metals compared to most other metals?

  • Much more reactive
  • Less dense
  • Lower melting points
• How do Group 1 elements form ions?

  They readily form 1+ ions by losing one outer electron
• What type of compounds do Group 1 elements form when they react with water?

  Ionic compounds
• What is the general reaction of a Group 1 metal with water?

  Metal + water → metal hydroxide + hydrogen
• What is the general reaction of a Group 1 metal with chlorine?

  Metal + chlorine → metal chloride
• What is the general reaction of a Group 1 metal with oxygen?

  Metal + oxygen → metal oxide
• How does reactivity change with water as you go down Group 1?

  The reaction becomes more vigorous and explosive
• What are ions?

  Charged particles made when electrons are transferred
• How do metals and non-metals form ions?

  Metals lose electrons to form positive ions, while non-metals gain electrons to form negative ions
• What is ionic bonding?

  The electrostatic attraction between oppositely charged ions
• What type of ions does sodium form?

  Sodium forms Na+ ions
• What type of ions does chlorine form?

  Chlorine forms Cl- ions
• What is the electronic structure of a sodium atom?

  2, 8, 1
• What is the electronic structure of a chloride ion?

  2, 8, 8
• What do dot-cross diagrams show?

  They show the transfer of electrons but not the compound structure or size and arrangement of ions
• What electronic structure do the ions formed from these groups have?

  The ions formed have the electronic structure of a noble gas.
• How do metals conduct electricity?

  They are electrical conductors, because their delocalised electrons carry electrical charge through the metal.