NOMENCLATURE a systematic way of naming chemical compounds

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1 NOMENCLATURE a systematic way of naming chemical compounds So far, we have looked at two types of compounds and. Ionic compounds are formed when oppositely ions stick together. There are two reasons why this happens: 1. Atoms lose or gain electrons to fill their. 2. Oppositely charged ions are attracted to each other and form an compound. The simplest ionic compounds result when a group 1 element bonds with a group element. ex. Sodium chloride OR a group 2 element bonds with a group element. ex. Magnesium oxide More complex ionic compounds can be formed when the charges of the cation and are not equal such as aluminum oxide. Molecular compounds are different because the atoms their valence instead of becoming ions. The properties of ionic compounds are vastly different then molecular compounds (salt vs. Lauric acid). Another difference between ionic compounds and molecular compounds is that ionic compounds occur in fixed ratios for any two elements. CaCl 2, NaCl, Al 2 O 3 However, a varied of ratios can exist for molecular compounds. CH 4 & C 2 H 6 or CO & CO 2 As a result, chemists have created their own naming system (nomenclature) to help distinguish between the various types of compounds. 1

2 NAMING IONIC COMPOUNDS Ionic compounds are formed when a metal is attracted to an oppositely charged. There are 3 categories for ionic compounds because of the various types of ionic compounds. Category #1 SIMPLE IONIC COMPOUNDS This type of compound is referred to as "simple" because we know the charges of certain ions (Groups 1, 2, 16, 17). Ex. NAME write the metal first (it's always first in the compound anyway) and then write the non metal, but change the ending to "ide". CHEMICAL FORMULA determine the charge of the ions and then determine the ratio (how many of each are required to form a neutral compound). Examples 1. K 2 O 2. Sodium chloride 3. AlCl 3 4. Magnesium phosphide a. Magnesium oxide b. Aluminum nitride c. Potassium sulfide d. Calcium bromide e. Aluminum sulfide f. Beryllium oxide g. Strontium phosphide h. Sodium fluoride i. Lithium selenide j. Barium oxide a. Li 2 O b. AlCl 3 c. MgS d. CaF 2 e. Al 2 O 3 f. BeF 2 g. K 3 P h. Mg 3 P 2 i. CaO j. Ag 2 S 2

3 IONIC COMPOUNDS CONTINUED Category #2 POLYATOMIC IONS If the prefix poly means, the suffix atomic means different, and the word ion means, then the term polyatomic ions refers to a group of atoms which form a single ion. These ions must be common enough to be given a common name so that chemists can easily identify them. NH 4 + OH HCO 3 CO 3 2 NO 3 PO 4 3 SO 4 2 ammonium hydroxide hydrogen carbonate carbonate nitrate phosphate sulfate The hardest part about naming polyatomic ions is RECOGNIZING the polyatomic ion. Once you recognize it, naming it is quite simple! NAME write the metal first and then write the polyatomic ion. This time, you DON'T change the ending to "ide"; leave it as is (usually "ate", but not always). CHEMICAL FORMULA determine the charge of the ions and then determine the ratio (how many of each are required to form a neutral compound). A bracket might have to be used around the polyatomic ion. Examples 1. Li 2 CO 3 3. Sodium hydroxide 2. Al 2 (SO 4 ) 3 4. Magnesium phosphate a. Magnesium carbonate b. Aluminum nitrate c. Potassium sulfate d. Aluminum sulfate e. Sodium carbonate a. Li 2 SO 4 b. MgSO 4 c. K 2 CO 3 d. Na 2 SO 4 e. K 3 PO 4 3

4 Category #3 TRANSITION METALS Of the ionic compounds we have looked at so far, the charge of both ions is fixed and so only one possible ratio can exist when the compound is formed. Chemists found that some elements formed ionic compounds in different ratios. And so, they had to come up with a different system when naming these ionic compounds. The key to the naming of these ionic compounds is the inclusion of the charge for the element that is found with multiple charges. The Transition Metals have multiple charges (they are all positive charges because they are METALS). Example: iron (II) oxide & iron (III) oxide The charge of the iron in iron (II) oxide would be. The charge of the iron in iron (III) oxide would be. Look on your periodic table and list other elements that can have multiple charges. When given the formula, the charge of the unknown ion is to be deduced from the formula. This is likely the most difficult of all nomenclature scenarios. Example: FeO and Fe 2 O 3 Try the following questions for homework. a. tin (II) fluoride b. lead (IV) nitride c. iron (III) chloride d. copper (I) oxide a. PbS b. SnO 2 c. NiO d. CuI 2 SUMMARY Ionic Compounds start with a, can be divided into 3 categories: 1. Simple Ionic Compounds: the charges are known and it is easy to determine the correct ratio. ex. 2. Polyatomic Ionic Compounds: you must recognize a small list of known groups of atoms which form a single ion. ex. 3. Transition Metals: the ions formed can vary and therefore the name must indicate the specific ion in the compound. ex. Molecular compounds have completely different properties from ionic compounds and they can exist in different ratios. Therefore, a completely different naming system was established. 4

5 MOLECULAR COMPOUNDS Molecular Compounds are formed with non or elements found on the hand side of the periodic table. Prefixes are used to indicate the specific ratio for that compound. Rules 1. The more positive atom is written first (the atom which is the furthest to the left and to the bottom of the periodic table). 2. The more negative second atom has an " ide" ending. 3. Each prefix indicates the number of each atom present in the compound. 4. If there is only one atom of the first element, we don't use any prefix. Prefixes Number of Atoms Prefix Number of Atoms Prefix 1 mono 6 hexa 2 di 7 hepta 3 tri 8 octa 4 tetra 9 nona 5 penta 10 deca Examples 1. tetraphosphorus decasulfide 2. dicarbon hexahydride 3. CH 4 4. CO Complete the following naming molecular compounds for homework. a. carbon dioxide b. silicon dioxide c. dinitrogen monoxide d. diphosphorus trisulphide e. dichlorine monoxide f. carbon disulphide g. bromine gas h. sulphur trioxide a. CF 4 b. NF 3 c. NH 3 d. P 2 S 5 e. PBr 3 f. PF 5 g. ICl h. CS 2 5

6 SNC 2D Name: PUTTING IT ALL TOGETHER: Names and Formulas Instruction: for all compounds indicate whether they are Molecular (M), Simple Ionic (I), Ionic with a Transition Metal (T), Ionic with a Polyatomic ion (P), Ionic with both a transition metal and a polyatomic ion (PT) Write the formulas for the following compounds. calcium fluoride potassium sulphate carbon disulfide barium nitride nitrogen triodide aluminum hydroxide sodium phosphide fluorine gas dichlorine monoxide silicon dioxide iron (III) carbonate calcium hydroxide phosphorus pentachloride carbon tetrachloride diphosphorus pentasulphide gold (I) nitrate tin (IV) chloride sulphur trioxide magnesium sulfate potassium hydroxide Write the names for the following compounds. CCl 4 NaNO 3 Mg(NO 3 ) 2 PBr 3 H 2 gas PCl 5 BiF 5 H 2 CO 3 PbS 2 FeCl 2 Al 2 (CO 3 ) 3 N 2 O Na 2 SO 4 Na 2 O CuCO 3 Li 3 PO 4 Al 2 (SO 4 ) 3 SnO H 2 SO 4 SeCl 2 6

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