Naming Ionic Compounds Cl Cl - sodium sodium chlorine chloride sodium chloride Photo by Ra’ike

When metals lose electrons they become ions. Remember… When metals lose electrons they become ions. When nonmetals gain electrons they become ions. Let’s learn how to name ions…

chlor- + -ide = chloride Rules for Naming Ions 1. The names of metals do not change. 2. The names of nonmetals do change: root of element name + -ide = name of ion Examples of nonmetals: The name of chlorine’s ion: chlor- + -ide = chloride The name of nitrogen’s ion: nitr- + -ide = nitride

Examples of naming ions: The name of calcium’s ion: calcium (The names of metals don’t change!) The name of oxygen’s ion: ox- + -ide = oxide The name of aluminum’s ion: aluminum (The names of metals don’t change!)

Write the name of each of the ions on your notes. sulfide lithium nitride bromide potassium chloride oxide hydrogen (+), hydride (-)

It is also important that you can identify the names of polyatomic ions. Polyatomic ions are covalently bonded elements that have a charge!

Write the name of each of the polyatomic ions on your notes using your reference sheet as a guide. sulfate carbonate permanganate sulfite hydroxide nitrate

Steps for Naming Ionic Compounds YOU ARE DONE! It is that easy. CaBr2 calcium bromide Step 1: Write the name of the metal ion. Step 2: Write the name of the nonmetal ion. YOU ARE DONE! It is that easy.

1. NaF 2. MgO sodium fluoride magnesium oxide 3. SrCl2 4. Li2S strontium chloride lithium sulfide 5. CaO 6. KI calcium oxide potassium iodide

When polyatomic ions are used, simply use the name of the polyatomic ion in the compound. 1. NH4F 2. CaSO4 ammonium fluoride calcium sulfate 3. Mg(NO3)2 4. NaOH magnesium nitrate sodium hydroxide

Mg I +2 - MgI2 magnesium iodide You can also determine the formula of an ionic compound from its name. To do this, you will need to use what you already know about the Periodic Table. magnesium iodide Mg I +2 - MgI2 Step 1: Write the symbol and charge of the metal ion using the Periodic Table. Step 2: Write the symbol and charge of the nonmetal ion using the Periodic Table. Step 3: Determine the formula from the ions.

Sr NO3 +2 - Sr(NO3)2 strontium nitrate This is just as easy to do with polyatomic ions. You just need to use the table of polyatomic ions found on the naming compounds reference sheet. strontium nitrate Sr NO3 +2 - Sr(NO3)2 Step 1: Write the symbol and charge of the metal ion. Step 2: Write the formula and charge of the polyatomic ion using your STAAR Reference Sheet. Step 4: Determine the formula from the ions.

N-3 NO3- S-2 SO3-2 P-3 PO4-3 nitrate nitride sulfide sulfite phosphate Be very careful that you do not mix up the names of ions. This is very common for beginners to naming. Decide which name goes with each ion. nitrate N-3 NO3- nitride sulfide S-2 SO3-2 sulfite phosphate P-3 PO4-3 phosphide

SO4-2 S-2 SO3-2 N-3 NO2- NO3- Helpful Hint: If the ion ends in –ide, it is probably from the periodic table. If the ion ends in –ate or –ite, it is a polyatomic ion. If you’re not sure, just check the list to see if it is there! Examples: sulfate sulfide sulfite SO4-2 S-2 SO3-2 nitride nitrite nitrate N-3 NO2- NO3-

We know they are positive because metals are always positive. Remember that the names of transition metals includes their charge because their charges are less predictable. What are the charges of the transition metals below: Iron (II) _______ Iron (III) _______ Copper (II) _______ Copper (I) _______ Tin (IV) _______ Tin (II) _______ Lead (II) _______ Lead (IV) _______ +2 +3 +2 +1 +4 +2 +2 +4 We know they are positive because metals are always positive.

Fe O +3 -2 Fe2O3 iron (III) oxide The charges of the transition metals are important when you are determining the formula of an ionic compound. iron (III) oxide Fe O +3 -2 Fe2O3 Step 1: Write the symbol and charge of the metal ion using the roman numeral given. Step 2: Write the symbol and charge of the anion. Step 4: Determine the formula from the ions.

Write the formula of each of the ionic compounds named on your notes. KI SnCl4 BaSO4 NaCl SrS CuCO3 AlBr3 Li3N

Now let’s talk about naming Covalent Compounds

So why do atoms share electrons? Atoms share electrons so that they can both be in the most stable configuration! So when are atoms the most stable? Atoms are the most stable when they have 8 valence electrons in their outer energy level. (Hydrogen and Helium only need 2 valence electrons.)

Chemical reactions occur when atoms gain, lose, or share electrons. Nonmetals Chemical reactions occur when atoms gain, lose, or share electrons. Sharing electrons creates a covalent bond Nonmetals can _______ electrons to form a covalent bond. This creates a ___________. share molecule

There are 7 elements that exist in nature as diatomic molecules. What elements exist as diatomic molecules? H2, N2, O2, F2, Cl2, Br2, I2 21

Binary Covalent Compounds There are millions of covalent compounds. These can be classified into many different types of compounds. Each type of compound has a different set of rules for naming. You will be learning about the easiest type of covalent compound to name: Binary Covalent Compounds What does binary mean? Binary means 2. Binary covalent compounds are between 2 different nonmetals.

phosphorous and chlorine Nonmetals can share electrons in many different ways. This means that two nonmetals can create multiple compounds together. carbon and oxygen phosphorous and chlorine CO CO2 PCl3 PCl5 nitrogen and oxygen N2O4 N2O3 Each of these contains a different ratio of elements. Because of this, we have to make sure that the name of the compound explains the correct ratio.

To show the correct ratio of elements, we use prefixes.

Binary Covalent Compounds Steps for Naming Binary Covalent Compounds N2O4 dinitrogen nitrogen tetroxide oxide Step 1: Write the name of the first nonmetal. Step 2: Write the name of the second nonmetal changing its ending to -ide. Step 3: Add prefixes to specify how many of each element are present.

Rules for Using Prefixes Rule 1: Prefixes are only for COVALENT compounds. Rule 2: The prefix mono- is never used on the first element of a binary covalent compound. Without a prefix it is assumed that there is only 1. Example: CO2 is carbon dioxide, not monocarbon dioxide. Rule 3: Remove the -o or -a from a prefix before adding it to oxide. Example: CO is carbon monoxide, and not carbon monooxide.

How would you write each of the prefixes in front of oxide? Remember: Remove the -o or -a from a prefix before adding it to oxide. Leave -i alone. mono- ____________ di- ____________ tri- ____________ tetra- ____________ penta- ____________ hexa- ____________ hepta- ____________ octa- ____________ nona- ____________ deca- ____________ monoxide dioxide trioxide tetroxide pentoxide hexoxide heptoxide octoxide nonoxide decoxide

Name the binary covalent compounds that are found on your notes. carbon dioxide carbon disulfide phosphorous tribromide phosphorous pentabromide diphosphorous pentasulfide dinitrogen monosulfide silicon disulfide nitrogen tribromide dinitrogen tetrachloride

dinitrogen tetrafluoride Because of the prefixes, it is very easy to go from the name of a binary covalent compound to its formula. dinitrogen tetrafluoride N2 F4 Step 1: Write the symbol of the first nonmetal and the subscript that matches the prefix. Step 2: Write the symbol of the second nonmetal and the subscript that matches the prefix.

Write the formulas of the binary covalent compounds in your notes. CCl4 IF7 PCl5 N2O4 N2O PCl3 CS CO BH3 ICl S2Br6 S4N4 SiS2 H2O PI3 ClF5 NCl3 NO2