1. C HAPTER 6 – C HEMICAL B ONDS Jennie L. Borders

2. S TANDARDS SPS1. Students will investigate our current understanding of the atom b. Compare and contrast ionic and covalent bonds in terms of electron movement. SPS2. Students will explore the nature of matter, its classification and its system for naming types of matter B. Predict formulas for stable binary ionic compounds based on balance of charges C. Use IUPAC nomenclature for transition between chemical names and chemical formulas of Binary ionic compounds (containing representative elements) Binary covalent compounds (ie. carbon dioxide, carbon tetrachloride

3. S TANDARDS SPS4. Students will investigate the arrangement of the periodic table. a. Determine the trends of the following Number of valence electrons Types of ions formed by representative elements Locations of metals, nonmetals and metalloids Phases at room temperature

4. S ECTION 6.1 – I ONIC B ONDS When the highest occupied energy level of an atom is filled with electrons, the atom is stable and not likely to react. The noble gases have stable electron configurations with eight valence electrons (or two in the case of helium).

5. S TABLE E LECTRON C ONFIGURATIONS The chemical properties of an element depend on the number of valence electrons. An electron dot diagram is a model of an atom in which each dot represents a valence electron.

6. I ONIC B ONDS Some elements achieve stable electron configurations through the transfer of electrons between atoms. An atom that has a net positive or negative charge is called an ion.

7. I ONS An ion with a negative charge is an anion. Anions like the Cl - ion are named by adding the suffix –ide to the element name. (Ex. Cl - = chloride) An ion with a positive charge is a cation. The name of a cation is the same as the element name. (Ex. Na + = sodium)

8. I ON C HARGES The charges that an ion has are based on the number of valence electrons that an element has. All of the elements in the same group have the same charge.

9. I ON C HARGES Is it easier for lithium to gain 7 more electrons or lose 1 electron? What charge would lithium have? lose 1 electron +1

10. I ON C HARGES Is it easier for beryllium to gain 6 more electrons or lose 2 electrons? What charge would beryllium have? lose 2 electrons +2

11. I ON C HARGES Is it easier for boron to gain 5 more electrons or lose 3 electrons? What charge would boron have? lose 3 electrons +3

12. I ON C HARGES Is it easier for carbon to gain 4 more electrons or lose 4 electrons? What charge would carbon have? lose or gain 4 electrons +4 or -4

13. I ON C HARGES Is it easier for nitrogen to gain 3 more electrons or lose 5 electrons? What charge would nitrogen have? gain 3 electrons -3

14. I ON C HARGES Is it easier for oxygen to gain 2 more electrons or lose 6 electrons? What charge would oxygen have? gain 2 electrons -2

15. I ON C HARGES Is it easier for fluorine to gain 1 more electron or lose 7 electrons? What charge would fluorine have? gain 1 electron

16. I ON C HARGES Would neon want to gain or lose electrons? What charge would neon have? No, it has a full energy level 0

17. I ON C HARGES Since elements in the same group have the same number of valence electrons, they all have the same charge.

18. F ORMATION OF I ONIC B ONDS A chemical bond is the force that holds atoms or ions together as a unit. An ionic bond is the force that holds cations and anions together. An ionic bond forms when electrons are transferred from one atom to another.

19. F ORMATION OF I ONIC B ONDS When an ionic bond is formed, electrons are transferred until each atom has a full outer energy level.

20. I ONIC C OMPOUNDS Compounds that contain ionic bonds are ionic compounds, which can be represented by chemical formulas. A chemical formula is a notation that shows what elements a compound contains and the ratio of the atoms or ions of these elements in the compound.

21. C RYSTAL L ATTICES A chemical formula for an ionic compound tells you the ratio of the ions in the compound. Solids whose particles are arranged in a lattice structure are called crystals.

22. P ROPERTIES OF I ONIC C OMPOUNDS Ionic compounds tend to have high melting points (above 300 o C). Ionic compounds are poor conductors in the solid state, but they can conduct heat or electricity when they are melted. Ionic compounds are brittle, so they shatter when struck by a hammer. The properties of ionic compounds can be explained by the strong attractions among ions within a crystal lattice.

23. I ONIC C OMPOUNDS AND E LECTRICITY

24. S ECTION 6.1 A SSESSMENT 1. When is an atom least likely to react? 2. Describe one way an element can achieve a stable electron configuration. 3. What characteristic of ionic bonds can be used to explain the properties of ionic compounds? 4. What will the ratio of ions be in any compound formed from a Group 1 metal and a Group 7 nonmetal?

25. S ECTION 6.1 A SSESSMENT 5. Why do ionic compounds include at least one metal? 6. Based on their chemical formulas, which of these compounds is not likely to be an ionic compounds: KBr, SO 2, or FeCl 3 ?

26. S ECTION 6.2 – C OVALENT B ONDING A covalent bond is a chemical bond in which two atoms share a pair of valence electrons. When two atoms share one pair of electrons, the bond is called a single bond.

27. C OVALENT VS I ONIC B OND

28. M OLECULES OF E LEMENTS A molecule is a neutral group of atoms that are joined together by one or more covalent bonds. The attractions between the shared electrons and the protons in each nucleus hold the atoms together in a covalent bond. Many nonmetal elements exist as diatomic molecules. Diatomic means two atoms. They are H 2, F 2, Cl 2, N 2, Br 2, O 2, and I 2.

29. D IATOMIC E LEMENTS

30. M ULTIPLE C OVALENT B ONDS When two atoms share two pairs of electrons, the bond is called a double bond. When two atoms share three pairs of electrons, the bond is called a triple bond.

31. S ECTION 6.2 A SSESSMENT 1. What attractions hold atoms together in a covalent bond? 2. Which of these elements does not bond to form molecules: oxygen, chlorine, neon, or sulfur? 3. Based on their electron dot diagrams, what is the formula for the covalently bonded compound of nitrogen and hydrogen?

32. S ECTION 6.3 – N AMING C OMPOUNDS AND W RITING F ORMULAS The name of an ionic compound must distinguish the compound from other ionic compounds containing the same elements. The formula of an ionic compound describes the ratio of the ions in the compound.

33. B INARY I ONIC C OMPOUNDS A compound made from only two elements is a binary compound. When naming an ionic compound the name of the metal (cation) does not change and the name of the nonmetal (anion) has the suffix –ide. Ex. MgBr 2 = magnesium bromide

34. M ETAL WITH M ULTIPLE I ONS Many transition metals form more than one type of ion. When a metal forms more than one ion, the name of the ion contains a roman numeral to indicate the charge of the ion. Ex: Fe +2 = iron (II) Fe +3 = iron (III)

35. P OLYATOMIC I ONS A covalently bonded group of atoms that has a positive or negative charge and acts as a unit is a polyatomic ion.

36. WRITING FORMULAS FOR IONIC COMPOUNDS Place the symbol of the cation first, followed by the symbol of the anion. Use subscripts to show the ratio of the ions in the compound. Because all compounds are neutral, the total charges on the cations and anions must add up to zero.

37. C ROSSING C HARGES To balance the charges in an ionic compound, you can cross the charges if they are not the same.

38. D ESCRIBING M OLECULAR C OMPOUNDS The name and formula of a molecular compound describe the type and number of atoms in a molecule of the compound. Molecular compounds only contain nonmetals.

39. N AMING M OLECULAR C OMPOUNDS The name of the first element is the same. The name of the second element ends in the suffix -ide. Prefixes tell the number of atoms of each element. A prefix is not used when the first element only has 1 atom. Ex. CO 2 = carbon dioxide

40. P REFIXES 1 = mono6 = hexa 2 = di7 = hepta 3 = tri8 = octa 4 = tetra9 = nona 5 = penta10 = deca

41. W RITING M OLECULAR F ORMULAS Write the symbols for the elements in the order the elements appear in the name. The prefixes indicate the number of atoms of each element in this molecule. Ex: diphosphorus pentoxide = P 2 O 5

42. S ECTION 6.3 A SSESSMENT 1. What does the formula of an ionic compound describe? 2. What do the name and formula of a molecular compound describe? 3. What suffix is used to indicate an anion? 4. Why are Roman numerals used in the names of compounds that contain transition metals? 5. What is a polyatomic ion?

43. S ECTION 6.3 A SSESSMENT 6. How is it possible for two different ionic compounds to contain the same elements? 7. How many potassium ions are needed to bond with a phosphate ion? 8. What are the name of these ionic compounds: LiCl, BaO, and Na 3 N? 9. Name the molecular compounds with these formulas: N 2 O 7 and CO. 10. What is the formula for the ionic compound formed from potassium and sulfur?

44. S ECTION 6.4 – T HE S TRUCTURE OF M ETALS In a metal, valence electrons are free to move among the atoms, so the cations are surrounded by a sea of electrons. A metallic bond is the attraction between a metal cation and the shared electrons that surround it.

45. M ETALLIC B ONDS The cations in a metal form a lattice that is held in place by strong metallic bonds between the cations and the surrounding valence electrons. The more valence electrons an atom can contribute to the shared pool, the stronger the metallic bond will be.

46. P ROPERTIES OF M ETALS The mobility of electrons within a metal lattice explains the fact that metals are good conductors and malleable.

47. A LLOYS An alloy is a mixture of two or more elements that have metallic properties.

48. SECTION 6.4 ASSESSMENT 1. What holds metal ions together in a metal lattice? 2. What characteristic of a metallic bond explains some of the properties of metals? 3. Explain why the metallic bonds in some metals are stronger than the bonds in other metals. 4. Why are metals good conductors of electric current? 5. Can two different elements form a metallic bond together?