Memory Anchor:

• Super Challenge:

  Stretch:

  Challenge:

Key Questions:

1. Describe the transfer of electrons in an ionic bond
   • Electrons are donated from the metal element in order to complete the outer shell of the non-metal element
2. When a metal atom become an ion it loses electrons. How does this effect its charge?
   • It becomes a positively charged ion.
3. When a non-metal atom bonds ionically it gains electrons. How does this effect its charge?
   • It becomes a negatively charged ion.
4. What is the electronic structure of ions produced by group 1,2 metals and group 6,7 non metals?
   • They have full outside shells of electrons giving them a stable electronic configuration, the same as a noble gas.
5. How could you show the formation of an ionic compound using a dot and cross diagram?
   • Showing outer electrons only. Crosses for one element and dots for the other. Show transfer of electrons on shell. Use brackets to show the overall charge of the ions formed.
6. Draw a dot cross diagram to show the ionic bond in sodium chloride.
   • Diagram: Sodium - Electron strucuture represented in square brackets, with a 1 charge on the top right outside the bracket. . It's one outer shell electron removed. Chlorine - Electron strucuture represented in square brackets, with a -1 charge on the top right outside the bracket. One extra electron represented as either a dot or cross shown to represent the electron gained from sodium.
7. What charge do ions of elements from the following groups form 1) Group 1 2) Group 2 3) Group 6 4) Group 7
   • 1) Group 1 = +1 ion 2) Group 2 = +2 ion 3) Group 6 = -2 ion 4) Group 7 = -1 ion
8. Explain why potassium chloride is KCl but potassium oxide is K2O
   • The overall charge of an ionic compound will always be neutral. Potassium forms an ion with a 1 charge, so will bond in a 1:1 ratio chlorine as chlorine forms a -1 ion. Oxygen on the other hand forms a -2 ion, so for each Oxygen 2 potassiums would be needed to neutralise the charge.