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1 Goals 1. What is an ion, what is an ionic bond, and what are the general characteristics of ionic compounds? Be able to describe ions and ionic bonds, and give the general properties of compounds that contain ionic bonds. 2. What is the octet rule, and how does it apply to ions? Be able to state the octet rule and use it to predict the electron configurations of ions of main group elements. 3. What is the relationship between an element s position in the periodic table and the formation of its ion? Be able to predict what ions are likely to be formed by atoms of a given element.
2 Goals, Continued 4. What determines the chemical formula of an ionic compound? Be able to write formulas for ionic compounds, given the identities of the ions. 5. How are ionic compounds named? Be able to name an ionic compound from its formula or give the formula of a compound from its name. 6. What are acids and bases? Be able to recognize common acids and bases.
3 3.1 Ions Metals tend to form compounds with nonmetals. Alkali metals (group IA) react with halogens (group 7A) to make a variety of compounds with similar properties. The two elements are always found in a 1:1 ratio. The compounds have melting points over 500 C. Each is a stable, white, crystalline solid. Each is soluble in water. The water solution of each compound conducts electricity.
4 3.1 Ions The symbol for a cation is written by adding the positive charge as a superscript to the symbol for the element. An anion symbol is written by adding the negative charge as a superscript. If the charge is greater than 1, the number is used.
5 3.3 Ionic Bonds Ion-transfer reactions of metals and nonmetals form products unlike either element. Because opposite electrical charges attract each other, the positive ion and negative ion are said to be held together by an ionic bond. There are many ions attracted by ionic bonds to their nearest neighbors. These crystals are ionic solids. Compounds of this type are referred to as ionic compounds.
6 3.4 Some Properties of Ionic Compounds Ions in each compound settle into a pattern that efficiently fills space and maximizes ionic bonding. Ions in an ionic solid are held rigidly in place by attraction to their neighbors. Once an ionic solid is dissolved in water, the ions can move freely, which accounts for the electrical conductivity of these compounds in solution.
7 3.5 Ions and the Octet Rule Alkali metals have a single valence electron and an electron configuration ns 1. Halogens have seven valence electrons and an electron configuration ns 2 np 5. When halogens and alkali metals react, an electron is transferred, giving both ns 2 np 6 configurations with eight valence electrons. This is a noble gas electron configuration. Octet rule: Main group elements tend to undergo reactions that leave them with eight valence electrons.
8 3.6 Ions of Some Common Elements
9 3.6 Ions of Some Common Elements Group 1A: M M + + e Group 2A: M M e Group 3A: Al Al e ; no other common ions. Group 4A, 5A: no common ions. Group 6A: X + 2e X 2 Group 7A: X + e X Transition metals form cations, but can lose one or more d electrons in addition to losing valence s electrons. The octet rule is not followed.
10 3.6 Ions of Some Common Elements Important Points about Ion Formation and the Periodic Table Metals form cations by losing one or more electrons. Group 1A and 2A metals form +1 and +2 ions, respectively, to achieve a noble gas configuration. Transition metals can form cations of more than one charge by losing a combination of valence-shell s electrons and inner-shell d electrons. Reactive nonmetals form anions by gaining one or more electrons to achieve a noble gas configuration. Group 6A nonmetals oxygen and sulfur form the anions O 2 and S 2. Group 7A elements (the halogens) form 1 ions. Group 8A elements (the noble gases) are unreactive. Ionic charges of main group elements can be predicted using the group number and the octet rule. For 1A and 2A metals, cation charge = group number. For nonmetals in groups 5A, 6A, and 7A, anion charge = 8 (group number).
11 3.7 Naming Ions Main group metal cations in groups 1A, 2A, and 3A are named by identifying the metal, followed by the word ion. Transition metals can form more than one type of cation. Two naming systems are used. Old System: The ion with the smaller charge is given the ending -ous and the ion with the larger charge is given the ending -ic. New System: The charge on the ion is given as a Roman numeral in parentheses right after the metal name.
12 3.7 Naming Ions Main group metal cations are named by identifying the metal, followed by the word ion. Transition metals can form more than one type of cation. Two naming systems are used. Old: The ion with the smaller charge is given the ending -ous and the ion with the larger charge is given the ending -ic. New: The charge on the ion is given as a Roman numeral in parentheses right after the metal name. Anions are named by replacing the ending of the element name with -ide, followed by the word ion.
13 3.8 Polyatomic Ions Polyatomic ion An ion that is composed of more than one atom. The atoms in a polyatomic ion are held together by covalent bonds. A polyatomic ion is charged because it contains a total number of electrons that is different from the total number of protons in the combined atoms. These ions are encountered so frequently that it is essential to memorize their names and formulas.
14 3.8 Polyatomic Ions
15 3.9 Formulas of Ionic Compounds All chemical compounds are neutral. Once the ions are identified, decide how many ions of each type give a total charge of zero. The chemical formula of an ionic compound tells the ratio of anions and cations.
16 3.9 Formulas of Ionic Compounds If the ions have the same charge, one of each is needed. K + + F KF If the ions have different charges, unequal numbers of anions and cations must combine to have a net charge of zero. 2 K + + O 2 K 2 O Ca Cl CaCl 2
17 3.9 Formulas of Ionic Compounds When the two ions have different charges, the number of one ion is equal to the charge on the other ion.
18 3.9 Formulas of Ionic Compounds The formula of an ionic compound shows the lowest possible ratio of atoms and is known as a simplest formula. There is no such thing as a single neutral particle of an ionic compound. Formula unit The formula that identifies the smallest neutral unit of an ionic compound.
19 3.9 Formulas of Ionic Compounds Once the numbers and kinds of ions in a compound are known, the formula is written using the following rules: List the cation first and the anion second. Do not write the charges of the ions. Use parentheses around a polyatomic ion formula if it has a subscript.
20 3.10 Naming Ionic Compounds These compounds are named by citing first the cation and then the anion, with a space between words. There are two kinds of ionic compounds: Type I ionic compounds contain cations of main group elements. Type II ionic compounds contain metals that can exhibit more than one charge. These require different naming conventions.
21 3.10 Naming Ionic Compounds Type I ionic compounds contain cations of main group elements. The charges on these cations do not vary. Do not specify the charge on the cation. NaCl is sodium chloride MgCO 3 is magnesium carbonate
22 3.10 Naming Ionic Compounds Type II ionic compounds contain metals that can exhibit more than one charge. Specify the charge on the cation in these compounds with either the old (-ous, -ic) or the new (Roman numerals) system. FeCl 2 is iron(ii) chloride or ferrous chloride. FeCl 3 is iron(iii) chloride or ferric chloride.
23 3.10 Naming Ionic Compounds Do not name these compounds iron dichloride or iron trichloride. Once the charge on the metal is known, the number of anions needed to yield a neutral compound is also known. Charges do not need to be included as part of the compound name.
24 3.10 Naming Ionic Compounds
25 3.11 H + and OH Ions: An Introduction to Acids and Bases A hydroxide anion is a polyatomic ion in which an oxygen atom is covalently bonded to a hydrogen atom. The importance of the H + cation and the OH anion is that they are fundamental to the concepts of acids and bases. Acid: A substance that provides H + ions in water Base: A substance that provides OH - ions in water
26 3.11 H + and OH Ions: An Introduction to Acids and Bases
27 3.11 H + and OH Ions: An Introduction to Acids and Bases Different acids can provide different numbers of H + ions per acid molecule. Hydrochloric acid, HCl, provides one H + ion per acid molecule. Sulfuric acid, H 2 SO 4, can provide two H + ions per acid molecule. Phosphoric acid, H 3 PO 4, can provide three H + ions per acid molecule.
28 3.11 H + and OH Ions: An Introduction to Acids and Bases Sodium hydroxide (NaOH) and potassium hydroxide (KOH) are bases. When these compounds dissolve, OH anions go into solution along with the metal cation. Different bases can provide different numbers of OH ions per formula unit. Sodium hydroxide provides one OH ion per formula unit. Barium hydroxide, Ba(OH) 2 can provide two OH ions per formula unit.
29 Chapter Summary 1. What is an ion, what is an ionic bond, and what are the general characteristics of ionic compounds? Atoms are converted into cations by the loss of electrons and into anions by the gain of electrons. Ionic bonds result from the attraction between opposite electrical charges. Ionic compounds conduct electricity when dissolved, and generally are crystalline solids with high melting and boiling points.
30 Chapter Summary 2. What is the octet rule, and how does it apply to ions? A valence-shell electron configuration of eight electrons leads to stability and lack of reactivity, as typified by the noble gases. According to the octet rule, atoms of main group elements tend to form ions in which they have gained or lost the number of electrons to reach a noble gas configuration.
31 Chapter Summary 4. What determines the chemical formula of an ionic compound? Ionic compounds contain appropriate numbers of anions and cations to maintain overall neutrality This provides a means of determining their chemical formulas.
32 Chapter Summary 5. How are ionic compounds named? Cations have the same name as the metal from which they are derived. Monatomic anions have the name ending -ide. For metals that form more than one ion, a Roman numeral equal to the charge on the ion is added to the name of the cation. Alternatively, the ending -ous is added to the name of the cation with the lesser charge and the ending -ic is added to the name of the cation with the greater charge. To name an ionic compound, the cation name is given first, with the charge of the metal ion indicated if necessary. The anion name is given second.
33 Chapter Summary 6. What are acids and bases? The hydrogen ion, H +, and the hydroxide ion, OH, are among the most important ions in chemistry An acid is a substance that yields H + ions when dissolved in water. A base is a substance that yields OH ions when dissolved in water.
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