1. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Fill in the chart using the notes: Section 2 Ionic Bonding and Salts Chapter 5 IonicCovalent Types of elements involved Strength of bond 1 property Electrons shared or transferred Which naming rule? Example name Example formula

2. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Chapter 5, 6, and 8 Review Section 2 Ionic Bonding and Salts Chapter 5

3. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Ionic Bonding Because opposite charges attract, cations and anions attract one another and an ionic bond is formed. Section 2 Ionic Bonding and Salts Chapter 5

4. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Ionic Compounds Do Not Consist of Molecules The ratio of cations to anions is always such that an ionic compound has no overall charge. Ionic Compounds Water is a molecular compound, so individual water molecules are each made of two hydrogen atoms and one oxygen atom. Section 2 Ionic Bonding and Salts Chapter 5

5. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Ionic Compounds, continued Ionic Compounds Do Not Consist of Molecules, continued Metals and nonmetals tend to form ionic compounds and not molecular compounds. The formula CaO likely indicates an ionic compound because Ca is a metal and O is a nonmetal. In contrast, the formula ICl likely indicates a molecular compound because both I and Cl are nonmetals. Lab tests are used to confirm such indications. Section 2 Ionic Bonding and Salts Chapter 5

6. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Ionic Compounds, continued Ionic Compounds Have Distinctive Properties Most ionic compounds have high melting and boiling points because of the strong attraction between ions. To melt, ions cannot be in fixed locations. Because the bonds between ions are strong, a lot of energy is needed to free them. Still more energy is needed to move ions out of the liquid state and cause boiling, so ionic compounds are rarely gaseous at room temperature. Section 2 Ionic Bonding and Salts Chapter 5

7. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Ionic Compounds, continued Liquid and Dissolved Salts Conduct Electric Current To conduct an electric current, a substance must satisfy two conditions: it must contain charged particles those particles must be free to move Ionic solids, such as salts, generally are not conductors because the ions cannot move. When a salt melts or dissolves, the ions can move about and are excellent electrical conductors. Section 2 Ionic Bonding and Salts Chapter 5

8. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Ionic Compounds, continued Salts Are Hard and Brittle Like NaCl, most ionic compounds are hard and brittle. Hard means that the crystal is able to resist a large force applied to it. Brittle means that when the applied force becomes too strong to resist, the crystal develops a widespread fracture rather than a small dent. Both properties are due to the patterns in which the cations and anions are arranged in all salt crystals. Section 2 Ionic Bonding and Salts Chapter 5

9. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Naming Ionic Compounds, continued Rules for Naming Simple Ions When an element forms two or more ions, the ion names include roman numerals to indicate charge. For example, the names of the two copper ions are: Cu + copper(I) ionCu 2+ copper(II) ion The name of a simple anion is also formed from the name of the element, but it ends in -ide. For example, Cl  is the chloride ion. Section 3 Names and Formulas of Ionic Compounds Chapter 5

10. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Naming Ionic Compounds, continued The Names of Ions Are Used to Name an Ionic Compound The name of a binary ionic compound is made up of just two words: the name of the cation followed by the name of the anion. NaCl sodium chlorideCuCl 2 copper(II) chloride ZnS zinc sulfideMg 3 N 2 magnesium nitride K 2 O potassium oxideAl 2 S 3 aluminum sulfide Section 3 Names and Formulas of Ionic Compounds Chapter 5

11. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Writing Ionic Formulas, continued Compounds Must Have No Overall Charge In some ionic compounds, the charges of the cation and anion differ. For example, in magnesium nitride, the Mg 2+ ion, has two positive charges, and the N 3− ion, has three negative charges. The cations and anions must be combined in such a way that there are the same number of negative charges and positive charges. Section 3 Names and Formulas of Ionic Compounds Chapter 5

12. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Chapter 6- Covalent Compounds Section 3 Names and Formulas of Ionic Compounds Chapter 5

13. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Sharing Electrons When an ionic bond forms, electrons are rearranged and are transferred from one atom to another to form charged ions. In another kind of change involving electrons, the neutral atoms share electrons. Section 1 Covalent Bonds Chapter 6

14. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Sharing Electrons, continued Forming Molecular Orbitals A covalent bond is a bond formed when atoms share one or more pairs of electrons. The shared electrons move within a space called a molecular orbital. A molecular orbital is the region of high probability that is occupied by an individual electron as it travels around one of two or more associated nuclei. Section 1 Covalent Bonds Chapter 6

15. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Electronegativity and Bond Types Section 1 Covalent Bonds Differences in electronegativity values provide one model that can tell you which type of bond two atoms will form. Another general rule states: A covalent bond forms between two nonmetals. An ionic bond forms between a nonmetal and a metal. Chapter 6

16. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Multiple Bonds, continued Naming Covalent Compounds The first element named is usually the first one written in the formula. It is usually the less-electronegative element. The second element named has the ending -ide. Unlike the names for ionic compounds, the names for covalent compounds must often distinguish between two different molecules made of the same elements. Section 2 Drawing and Naming Molecules Chapter 6

17. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Naming Covalent Compounds, continued This system of prefixes is used to show the number of atoms of each element in the molecule. Section 2 Drawing and Naming Molecules Chapter 6

18. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Naming Covalent Compounds, continued Prefixes can be used to show the numbers of each type of atom in diphosphorus pentasulfide. Section 2 Drawing and Naming Molecules Chapter 6

19. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Chapter 8-Chemical Reactions

20. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu A chemical reaction is the process by which one or more substances change into one or more new substances. Reactants are the original substances in a chemical reaction. Products are the substances that are created in a chemical reaction. Section 1 Describing Chemical Reactions Chapter 8 Chemical Reaction

21. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Writing a Word Equation or Formula Equation methane + oxygen  carbon dioxide + water ?CH 4 + ?O 2  ?CO 2 + ?H 2 O Section 1 Describing Chemical Reactions Chapter 8

22. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Reactions Conserve Mass Mass cannot be created or destroyed by a chemical or physical change Equations must be balanced. ?Na + ?H 2 O  ?NaOH + ?H 2 Section 2 Balancing Chemical Equations Chapter 8

23. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Balancing Equations The number of atoms for each element must be the same on the reactants’ side and on the products’ side. A coefficient multiplies the number of atoms of each element in the formula that follows. H 2 O: 2 hydrogen atoms, 1 oxygen atom 2H 2 O: 4 hydrogen atoms, 2 oxygen atoms Section 2 Balancing Chemical Equations Chapter 8

24. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Balancing Equations Sample Problem C Aluminum reacts with arsenic acid, HAsO 3, to form H 2 and aluminum arsenate. Write a balanced equation for this reaction. Section 2 Balancing Chemical Equations Chapter 8

25. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Balancing Equations Sample Problem C Solution 1. Identify reactants and products. reactants products Al + HAsO 3  H 2 + Al(AsO 3 ) 3 2. Count Atoms Section 2 Balancing Chemical Equations ReactantsProductsBalanced? Unbalanced formula equationAl + HAsO 3 H 2 + Al(AsO 3 ) 3 Iron atoms 11yes Oxygen atoms 12no Hydrogen atoms 13no 3226 Chapter 8 3. Insert coefficients

26. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Section 3 Classifying Chemical Reactions Combustion Reactions A combustion reaction is a reaction of a carbon- based compound with oxygen. Combustion of propane: C 3 H 8 + 5O 2  3CO 2 + 4H 2 O Combustion of ethanol: CH 3 CH 2 OH + 3O 2  2CO 2 + 3H 2 O Chapter 8

27. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Section 3 Classifying Chemical Reactions Synthesis Reactions In a synthesis reaction a single compound forms from two or more reactants. Two elements form a binary compound C + O 2  CO 2 2C + O 2  2CO Two compounds form a ternary compound CaO(s) + H 2 O(l)  Ca(OH) 2 (s) CO 2 (g) + H 2 O(l)  H 2 CO 3 (aq) Chapter 8

28. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Section 3 Classifying Chemical Reactions Decomposition Reactions In a decomposition reaction a single compound breaks down, often with the input of energy, into two or more elements or simpler compounds. Decomposition of water electricity heat Chapter 8 CaCO 3 (s)CaO(s) + CO 2 (g) A metal carbonate decomposes to form a metal oxide and carbon dioxide. 2H 2 O(l)O 2 (g) + 2H 2 (g)

29. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Section 3 Classifying Chemical Reactions Displacement Reactions In a single-displacement reaction a single element reacts with a compound and displaces another element from the compound. 2Al(s) + 3CuCl 2 (aq)  2AlCl 3 (aq) + 3Cu(s) Aluminum displaces copper. Chapter 8

30. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Section 3 Classifying Chemical Reactions Double-Displacement Reactions In a double-displacement reaction two compounds in aqueous solution appear to exchange ions and form two new compounds. One of the products must be a solid precipitate, a gas, or a molecular compound, such as water. HCl(aq) + NaOH(aq)  HOH(l) + NaCl(aq) Chapter 8

31. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Section 3 Classifying Chemical Reactions Example from pg. 292 #7 a & b Chapter 8

32. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Section 3 Classifying Chemical Reactions Example from pg. 292 #7 a & b Chapter 8

33. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Section 3 Classifying Chemical Reactions Example from pg. 292 #9 a & b Chapter 8

34. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Section 3 Classifying Chemical Reactions Example from pg. 292 #9 a & b Chapter 8