Topic 5: The Language of Chemistry

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1 Topic 5: The Language of Chemistry Chemical Formulas & Chemical Compounds (Chapter 7 in Modern Chemistry) A Chemical Formula Recall that a chemical formula indicates the relative number of atoms of each kind in a chemical compound. For a molecular compound, the chemical formula reveals the number of atoms of each element contained in a single molecule of the compound. C 8 H 18 Unlike a molecular compound, an ionic compound consists of a lattice of positive and negative ions held together by mutual attraction. The chemical formula for an ionic compound represents one formula unit the simplest ratio of the compound s positive ions (cations) and its negative ion (anion). Al 2 (SO 4 ) 3 HN Chemistry Page 1

2 Note how the parentheses are used. They surround the polyatomic anion to identify it as a unit. When there is no subscript written next to an atoms symbol, the value of the subscript is understood to be one. Monatomic Ions By gaining or losing electrons, many maingroup elements form ions with noblegas configurations (recall from Topics 3 & 4). Ions formed from a single atom are known as monatomic ions. Monatomic cations are identified simply by the element s name. Naming monatomic anions is slightly more complicated. First, the ending of the element s name is dropped. Then the ending ide is added to the root name. Examples of Cations Examples of Anions Element Cation Element Cation K K + F F Potassium Potassium ion Fluorine Fluoride ion Mg Mg 2+ N N 3 Magnesium Magnesium ion Nitrogen Nitride ion The oxidation numbers of maingroup monatomic ions can be determined by looking at their group number on the periodic table. The names of many of the ions include Roman numerals. These numerals are part of the Stock system of naming chemical ion and elements. They are used for elements that have more than one oxidation number. Task 5d 1. Label the following as a cation or an anion. a. Te b. W c. Fr 2. Name the following ions. a. Ca 2+ d. N 2+ b. Cu + e. P 3 c. Se 2 f. I HN Chemistry Page 2

3 Some Common Monatomic Ions Maingroup elements lithium Li + beryllium Be 2+ aluminum Al 3+ sodium Na + magnesium Mg 2+ potassium K + calcium Ca 2+ rubidium Rb + strontium Sr 2+ cesium Cs + barium Ba fluoride F oxide O 2 nitride N 3 chloride Cl sulfide S 2 phosphide P 3 bromide Br iodide I dblock elements and others with multiple ions copper(i) Cu + vanadium(ii) V 2+ vanadium(iii) V 3+ vanadium(iv) V 4+ silver Ag + chromium(ii) Cr 2+ chromium(iii) Cr 3+ tin(iv) Sn 4+ manganese(ii) Mn 2+ iron(iii) Fe 3+ lead(iv) Pb 4+ iron(ii) Fe 2+ cobalt(iii) Co 3+ cobalt(ii) Co 2+ nickel(ii) Ni 2+ copper(ii) Cu 2+ zinc Zn 2+ cadmium Cd 2+ tin(ii) Sn 2+ lead(ii) Pb 2+ HN Chemistry Page 3

4 Binary Ionic Compounds Binary compounds are made of two elements, a metal and a nonmetal. In a binary ionic compound, the total numbers of positive charges and negative charges must be equal. In order to write the formula of an ionic compound, you need to write the cation and the anion, then balance the charges so that the sum of the charges equal zero. For example: Mg and Cl: Mg 2+, Cl There must be 2 Cl s in order for the negative charge to equal and 2 equal zero. The correct formula for Mg and Cl is MgCl 2. Al and O: Al 3+, O 2 These numbers will not go into each other so I find a number that both of them will go into, 6. I will need 2 Al s to have a charge of 6 + (2 x 3 + = 6 + ). I will need 3 O s to have a charge of 6 (3 x 2 = 6 ). The correct formula for Al and O is Al 2 O 3. Naming Binary Ionic Compounds The nomenclature, or naming system, of binary ionic compounds involves combining the names of the compound s positive and negative ions. To name binary compounds, follow the rules below. 1. Name the cation. (First ion, metal) 2. Name the anion. (Second ion, nonmetal) Remember to change the ending of the last ion to ide. For example: KBr is potassium bromide MgCl 2 is magnesium chloride K 2 O is potassium oxide Task 5e 1. Write the formulas for the binary compounds formed between the following elements; a. potassium and iodine d. aluminum and sulfur b. sodium and sulfur e. aluminum and nitrogen c. lithium and phosphorus f. barium and oxygen 2. Name the binary compounds indicated by the following formulas: a. AgCl d. SrF 2 b. ZnO e. CaO c. CaBr 2 f. Ba 2 P 3 HN Chemistry Page 4

5 The Stock System of Nomenclature Some elements, such as iron, form two or more cations with different charges. To distinguish the ions formed by such elements, scientists use the Stock system of nomenclature. This system uses a Roman numeral to indicate an ion s charge. The numeral is enclosed in parentheses and placed immediately after the metal name. Fe 2+ Fe 3+ iron(ii) iron(iii) Names of metals that commonly form only one cation do not include a Roman numeral. Na + Ba 2+ Al 3+ sodium barium aluminum There is no element that commonly forms more than one monatomic anion. Naming a binary ionic compound according to the Stock system is illustrated below: CuCl 2 copper(ii) chloride If you are writing the name you must figure the charge to put with the cation. It is best to start at the back of the compound with the anion, to determine what the oxidation number of the cation will be. Task 5f 1. Write the formula and give the name for the compounds formed between the following ions: a. Cu 2+ and Br d. Hg 2+ and S 2 b. Fe 2+ and O 2 e. Sn 2+ and F c. Pb 2+ and Cl f. Fe 3+ and O 2 HN Chemistry Page 5

6 2. Give the names for the following compounds: a. CuO c. SnI 4 b. CoF 3 d. FeS Compounds Containing Polyatomic Ions First, you must learn your polyatomic ions. Do Not memorize. You will need these all year. Some Common Polyatomic Ions 1 + *ammonium NH * acetate *bromate BrO 3 *chlorate ClO 3 * chlorite ClO 2 CH 3 COO (C 2 H 3 O 2 ) *carbonate 2 CO 3 *chromate CrO 4 2 * dichromate Cr 2 O 7 2 *sulfate SO 4 2 *cyanide CN *sulfite SO 3 2 *hydroxide OH *iodate IO 3 *nitrate NO 3 * nitrite NO 2 *permanganate MnO 4 *phosphate PO 4 3 Notice that most of the polyatomic ions are negatively charged and most are oxyanions polyatomic ions that contain oxygen. Some elements can combine with oxygen to form more than one type of oxyanion. Learn all the oxyanions that end in ate and you ll be able to figure the other oxyanions of that element. For example: HN Chemistry Page 6

7 ClO 4 perchlorate 1 oxygen more than the ate ion ClO 3 chlorate the ate ion ClO 2 chlorite 1 oxygen less than the ate ion ClO hypochlorite 2 oxygens less than the ate ion Ternary compounds are made up of more an element and a polyatomic ion. To name ternary compounds, you must know your polyatomic ions and follow the rules below. 1. Name the cation. 2. Name the anion. If the anion is an element from the periodic table, change the ending to ide. If the anion is a polyatomic ion, do not change the ending. For example: NH 4 Cl is ammonium chloride CaCO 3 is calcium carbonate K 2 SO 4 is potassium sulfate Writing formulas of ternary compounds Just as in binary ionic compounds, the sum of the positive and negative ions must equal zero. When multiples of a polyatomic ion are present in a compound, the formula for the polyatomic ion is enclosed in parentheses as in aluminum sulfate, Al 2 (SO 4 ) 3. Task 5g 1. Write the formula for the following ternary compounds. a. Lithium nitrate b. Copper(II) sulfate c. Sodium carbonate d. Calcium nitrite e. Potassium perchlorate 2. Give the names for the following compounds. a. Ca(OH) 2 b. KClO 3 HN Chemistry Page 7

8 c. NH 4 OH d. Fe 2 (CrO 4 ) 3 e. KClO Molecular Compounds Molecular binary compounds are made of two nonmetals. Unlike ionic compound, molecular compounds are composed of individual covalently bonded units, or molecules. Chemists use two nomenclature systems to name binary molecules. Naming Molecular Compounds with Prefixes The old system of naming molecular compounds is based on the use of prefixes. For example, the molecular compound CCl 4 is named carbon tetrachloride. The prefix tetra indicates that four chloride atoms are present in a single Numerical Prefixes molecule of the compound. Number The rules for the prefix system of nomenclature of binary molecular compounds are as follows. 1. The element that has the smaller group number is usually given first. If both elements are in the same group, the element whose period number is greater is given first. This element is given a prefix only if it contributes more than one atom to a molecule of the compound. 2. The second element is named by combining (a) a prefix indicating the number of atoms contributed by the element, (b) the root of the name of the element, and (c) the ending ide. 10 deca 3. The o or a at the end of a prefix is usually dropped when the word following the prefix begins with another vowel. P 4 O 10 Prefix 1 mono 2 di 3 tri 4 tetra 5 penta 6 hexa 7 hepta 8 octa 9 nona Tetraphosphorus decoxide HN Chemistry Page 8

9 Binary Compounds of Nitrogen and Oxygen Formula N 2 O NO NO 2 N 2 O 3 N 2 O 4 N 2 O 5 Prefixsystem name dinitrogen monoxide nitrogen monoxide nitrogen dioxide dinitrogen trioxide dinitrogen tetroxide dinitrogen pentoxide Task 5h 1. Name the following binary molecular compounds using prefixes. a. CI 4 e. As 2 S 3 b. SO 3 f. NCl 3 c. PCl 3 g. SO 2 d. PCl 5 h. ClBr 2. Write the formulas for the following compounds: a. Carbon tetrachloride c. oxygen difluoride b. Dinitrogen trisulfide d. sulfur hexafluoride Naming Molecular Compounds with the Stock System In order to name molecular compounds using the stock system, or for that matter even ionic compounds using the stock system, you have to be able to assign oxidation numbers to the elements in the compound. Namely, you must be able to assign the oxidation number to the first element in the compound. These oxidation numbers, indicate the general distribution of electron among the bonded atoms in a molecular compound or a polyatomic ion. Oxidation numbers are also called oxidation states. A list of rules for assigning oxidation numbers follows. HN Chemistry Page 9

10 Rules for Assigning Oxidation Numbers As a general rule in assigning oxidation numbers, shared electrons are assumed to belong to the more electronegative atom in each bond. 1. The atoms in a pure element have an oxidation number of zero. 2. The more electronegative element in a binary molecular compound is assigned the number equal to the negative charge it would have as an anion. 3. Fluorine has an oxidation number of 1 in all of its compounds because it is the most electronegative element. 4. Oxygen has an oxidation number of 2 in almost all compounds. Exceptions include when it is in peroxides, such as H 2 O 2, in which its oxidation number is 1, and when it is in compounds with fluorine. 5. Hydrogen has an oxidation number of +1 in all compounds containing elements that are more electronegative than it; it has an oxidation number of 1 in compounds with metals. 6. The algebraic sum of the oxidation numbers of all atoms in a neutral compound is equal to zero. 7. The algebraic sum of the oxidation numbers of all atoms in a polyatomic ion is equal to the charge of the ion. Here are some examples. UF 6 Start with the most electronegative (last), F is 1 (rule 3). Multiply that oxidation number by the number of fluorine atoms. 6 x 1 = 6. Sum must equal zero (rule 6), so U must be +6 H 2 SO 4 Oxygen must have a 2 oxidation number (rule 4). Multiply 2 x 4 = 8 Hydrogen must have a +1 oxidation number (rule 5). +1 x 2 = +2 The sum must equal zero (rule 6), so S must equal +6. ClO 3 Oxygen must have a 2 oxidation number (rule 4). Multiply 2 x 3 = 6. The sum of a polyatomic ion equals its charge, in this case, 1. That means the oxidation number of chlorine is +5. HN Chemistry Page 10

11 Task 5 i 1. Assign oxidation numbers to each atom in the following compounds or ions. a. HF e. CS 2 b. CI 4 f. H 2 CO 3 c. H 2 O g. NO 2 2 d. PI 3 h. SO 4 2. Name the following binary molecular compounds using the Stock system. a. CI 4 e. As 2 S 3 b. SO 3 f. NCl 3 c. PCl 3 g. SO 2 d. PCl 5 h. ClBr 3. Write the formulas for the following compounds. a. Sulfur(II) chloride b. Nitrogen(V) oxide c. Carbon(IV) chloride Names & Formulas for Acids An acid is a distinct type of molecular compound. Most acids used in the laboratory can be classified as either binary acids or oxyacids. Binary acids are acids that consist of two elements, hydrogen and a nonmetal. Oxyacids are acids that contain hydrogen, oxygen, and a third element (usually a nonmetal). Oxyacids acids are derived from polyatomic ions. To name a binary acid, follow this guideline. Examples: Hydro STEM ic acid HCl Hydrosulfuric acid hydrochloric acid H 2 S HN Chemistry Page 11

12 To name an oxyacid, follow this guideline. ate ic, ite ous ate ions make ic acids and ite ions make ous acids Examples: H 2 SO 4 H 2 SO 3 HClO 4 sulfuric acid sulfurous acid perchloric acid Nitric acid HNO 3 Nitrous acid HNO 2 Carbonic acid H 2 CO 3 Task 5j 1. Name the following acids. a. H 3 PO 4 c. HI b. HBr d. HC 2 H 3 O 2 2. Write the formulas for the following acids. a. hypochlorous acid c. arsenic acid b. hydroiodic acid d. hydroselenic acid HN Chemistry Page 12

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