#Sheppardsoftware ion bonding update#
#Sheppardsoftware ion bonding manual#

I have recently been using a lot of materials for IGCSE revision which I would like to share with you. There are many experiments that you can browse to check the equipment needed or the associated theory. Īnother site which may help you understand experiments better is. Topics include acids and alkalis, chemical reactions and tests, compounds, mixtures and the Periodic Table. Try a quiz and be a star centre forward at the same time. If you want football fun, Canary Zoo is the site for you. It's suitable for all students studying science or chemistry from Year 9-11: Read through the file and see if you can do something constructive to improve your revision technique.Īre you going to reach your target.pdf (239,7 kB) WebsitesĪ good starter for Year 9 might be the Sheppard sofware site with its fun Periodic Table games:Ĭhalkbored is another favourite in the UK and is worth you spending a little time to find out about all its interesting contents. My revision focus sheet asks students whether they are optimising their chances of being successful in the June examinations. The qualitative analysis sheets below are vital for your studies too. They describe tests for cations, anions and gases. They are used especially for Paper 6 at IGCSE or Paper 3 at A Level. I have only done up to 2010 since no-one has informed me whether they are sensational.Ĥ.

#Sheppardsoftware ion bonding manual#

Note that the Year 11 Chemistry Manual also contains this information (page 163) in addition to the following link:ģ.

#Sheppardsoftware ion bonding update#

If you wish me to update this file, please see me. Specific topics (chapters from Chemistry for You) on Papers 3 and 6 can be checked against each exam during the years 2010 -2006. The link opens a chapter in the revision guide about bonding: If you wish to find out more about this first, really excellent guide, read on (with a click on the link). They are waiting for you to come and use at any time. You can take the books home to review. See the pictures below to remind you of the publishers' names. If you really aren't keen on using the Internet to help you in your revision, you could always try some of my revision guides. Ionic compounds are named by placing the cation name before the anion name, like lithium fluoride and sodium chloride.1. Likewise, sulf ate refers to SO 4 2- while sulf ide refers to S 2. For example, nitr ate refers to NO 3 – while nitr ide refers to N 3. Polyatomic anions containing oxygen end with -ate. For example, nitrogen forms nitr ide, oxygen forms ox ide, and fluorine forms fluoride. Monatomic anions formed from non-metallic elements are named by replacing the ending syllable of the element name with -ide. If a transition metal can form different cations with different charges, the positive charge is indicated by a Roman numeral in brackets that come after the name of the metal.

Here is a list of common polyatomic ions and their names: Chargeīesides hydroxide, polyatomic anions containing oxygen end with the suffix -ate.Ĭations formed from metallic elements have the same name as the metal, like sodium ion, calcium ion, and aluminium ion. There are also polyatomic ions: charged particles formed from multiple atoms covalently bonded to each other. There is an overall positive charge, as the central nitrogen is short of one electron, making it isoelectronic as carbon. Metallic and non-metallic ions are monatomic ions: charged particles formed from just one atom each.ĭot-and-cross diagram of ammonium, a polyatomic cation. The number of electrons gained is the difference between an octet and the number of valence electrons.Ĩ. Non-metallic elements gain electrons to complete their octet, hence forming negatively charged ions. Metallic elements lose their valence electrons (as bolded in the table) to achieve the noble gas configuration, hence forming positively charged ions. They do not include the transition metals between group II and III. Main-group elements are those in groups I to VII, and group 0 (noble gases). Given that metallic ions lose electrons while non-metallic ions gain electrons to achieve the noble gas electronic configuration, we can use this as a rule of thumb to predict the charges of main-group elements. Amongst them, metallic ones are in blue, while non-metallic ones are in red. Predicting the charges of common ions in an ionic compound Main-group elements in the first four periods are those highlighted.