Forming and Naming Binary Ionic Compounds Practice Worksheet Answer Key

-ide is a suffix for anions or anionic fragments of compounds. The suffix was taken from "oxide", which originally simply meant any compound of oxygen. Oxide was a portmonteau of oxygène and acide, and was coined by Lavoisier. In the 1800s the use was rapidly extrapolated to binary compounds of other elements.

If the compound is binary (only two element types) and contains both a metal and non-metal, then it is ionic and you must use the ionic naming system.If the compound is binary and contains only non-metals, then it is covalent and you must use the covalent naming system.Other cases depend:If it has more than two element types, then you have to start looking for known polyatomic ions. You’ll need to memorize these. For example, NH4Cl contains the ammonium ion, NH4+. As soon as you recognize that the compound contains an ion like this, you’ll be using the ionic naming system because it is an ionic compound.You also need to be familiar with what a basic organic compound looks like. If it has a bunch of carbons and hydrogens with other elements, most likely it is an organic compound. In this case, you don’t use either naming system… you’ll use the hydrocarbon (IUPAC) naming system. (-, eth-, prop-, etc prefixes)However, even this has some trickiness to it. For example, I could give you the compound NaCH3CH2COO. This contains a bunch of carbons and so you’d think it was a type of hydrocarbon. Yes, you’d be right… but it also has the metal in it, which means it probably is ionic. So, the overall molecule would be named using the ionic naming method. However, the anion would be named using the organic naming method: sodium propanoateSome metal containing compounds are not ionic. For example, the compound Fe(CO)5, iron pentacarbonyl. This is a different type of compound called a coordination compound and it is sometimes not taught in a general chemistry class.If I were teaching the general chemistry class, the first exam would contain a section on naming compounds from formula (and writing formula from names). I would expect you to know points 1, 2, and 3a. Point 3b is sometimes taught in the same chapter and sometimes taught in a later chapter. However, most of the key organic anions you need to know will be in the list of polyatomic ions you will have learned when studying for point 3a. Point 3c would usually be saved until the second semester of general chemistry or even a separate inorganic chemistry class. In any case, coordination chemistry makes more sense when you start learning about solvation… i.e. what happens at the molecular level to metal ions when they are dissolved in water or other solvents. This is usually the introduction to this topic.

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K2SPotassium sulfideIn order for the charges to cancel out, 2 potassium ions are needed to cancel out the 2- charge of the sulfur ion, -2 + 1 + 1 = 0.They aren’t really exchanging electrons as they’re not covalently bonding. They form a compound because they’re oppositely charged and opposite charges attract each other.

It forms K2S, Potassium Sulfide, but needs two atoms of Potassium (K) to one of Sulfur (S).Potassium sulfide - Wikipedia

You got two ions, (i) [math]SO_{4}^{2-}[/math], and (ii) [math]Al^{3+}[/math], which combine to form a neutral salt, i.e. a NET CHARGE of ZERO. It does not make too much algebra to take THREE of (i), and TWO of (ii), to give [math]Al_{2}(SO_{4})_{3}[/math].And please note that while we combine CHARGED ions…we do not exchange electrons…these are involved in redox transitions… What salt would we form if we have [math]Ca^{2+}[/math]?