https://padlet.com/hol_cjones/gzeo175yekw7 Made with a bold sensibility en-us 2019-01-30 12:12:16 UTC 2026-01-16 21:22:40 UTC hello@padlet.com https://padlet-assets.s3.amazonaws.com/icons/Soccerball.png 317683 https://padlet.com/hol_cjones/gzeo175yekw7/wish/325795592 1. Work out formulae of the species before & after change; balance if required
2. Work out oxidation state before & after change
3. Add electrons to 1 side of the equation so that oxidation states balance
4. The charges on species(ions & electrons) on either side of the equation don’t balance, add H⁺ ions to one side to balance
5. If equation doesn’t balance chemically, add sufficient H₂O molecules ]]> 2019-01-30 12:12:40 UTC https://padlet.com/hol_cjones/gzeo175yekw7/wish/325795592 317683 https://padlet.com/hol_cjones/gzeo175yekw7/wish/325795594 Split an ionic equation into two, which separately describes what happens to each substance present. One half-equation represents oxidation & the other reduction.
1. Write out 2 half-equations 
2. Multiply equation(s) to give equal number of electrons in both
3. Add equations & cancel electrons on both sides
4. If necessary, cancel out species’ that occur on both sides ]]> 2019-01-30 12:12:40 UTC https://padlet.com/hol_cjones/gzeo175yekw7/wish/325795594