P pt ionic formulae
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When metals react with non-metals, electrons are transferred from the metal atoms to the non-metal atoms. This results in the metal atoms becoming positively charged ions with fewer electrons than protons and the non-metal atoms becoming negatively charged ions with more electrons than protons. Examples of common monatomic ions formed include Na+, Ca2+, Al3+, Cl-, O2-, and N3-. Polyatomic ions such as NO3- and SO42- also exist. Ionic compounds are formed by combining these ions following rules based on their charges.
P pt ionic formulae
- 1. Ionic Formulae When metals combine with non-metals they do not share electrons. Electron(s) are transferred from the metal atom(s) to the non-metal atoms. This results in Metal atoms with fewer electrons than protons.These are called positive ions. Non-metal atoms with more electrons than protons. These are called negative ions.
- 2. Element E/a Ion E/a Sodium 2,8,1 Na+ 2,8 Calcium 2,8,8,2 Ca2+ 2,8,8 Aluminiu m 2,8,3 Al3+ 2,8 Chlorine 2,8,7 Cl- 2,8,8 Oxygen 2,6 O2- 2,8 Nitrogen 2,5 N3- 2,8 Some examples
- 3. Group 1 +1 Group 2 +2 Group 3 +3 Group 5 -3 Group 6 -2 Group 7 -1 Ion Charges Transition Metals - Charge is the same as the valency (Roman number) and all are positive ions. Group ions e.g. nitrate (NO3 -) - The charge is given in the table in the data book.
- 4. Writing Ionic Formulae Sodium chloride Na+ Cl- Calcium carbonate Ca2+ CO3 2- Copper(II) nitride (Cu2+ )3(N3- )2 Ammonium sulphate (NH4 + )2SO4 2-
- 5. TRY… Aluminium fluoride Al3+ (F- )3 Tin(II) sulphide Sn2+ S2- Lithium oxide (Li+ )2O2- Ammonium phosphate (NH4 + )3PO4 3- Iron(III) chromate (Fe3+ )2(CrO4 2- )3
- 6. TRY… Aluminium fluoride Al3+ (F- )3 Tin(II) sulphide Sn2+ S2- Lithium oxide (Li+ )2O2- Ammonium phosphate (NH4 + )3PO4 3- Iron(III) chromate (Fe3+ )2(CrO4 2- )3
Editor's Notes
- #3: You can practice using the examples given above