Bonding and Naming Review

1. Bonding and Naming Review By Mrs. Billings

2. Overview • What is a bond? • 4 Types of bonds • Naming type I, II, & III

3. What is a bond? • A bond is an electrostatic force that holds atoms together. • Atoms will bond using their electrons.

4. Types of Bonds • Ionic bonding • Electrons are transferred from one atom to the other. (give/take) • Happens between metals & nonmetals (cations & anions). • The atom that loses the electron becomes positive (cation) and the atom that gains the electron becomes negative (anion). . .ions, get it, ionic bond. • Why does this happen? The electrogegativity difference between the atoms is > 1.7 so one atom is able to rip the electron away. • Form a crystal lattice structure.

5. Types of Bonding • Covalent Bonding • Electrons are shared between atoms. • Happens between nonmetals only. • There are 2 types of covalent bonding based on the amount of sharing of electrons. • Polar covalent is uneven sharing, thus creating a pole. • Bond electronegativity difference <1.7 • Structure asymmetrical. • Nonpolar covalent is even sharing, thus no pole. • Bond electronegativity difference <0.4 • Structure symmetrical.

6. Types of Bonding • Metallic bonding • Delocalized electrons float around the electron sea. • Happens between metals only. • Characteristics: • Malleable • Ductile • Luster • Conductor

7. Identify the type of bond • A for ionic, B for covalent, and C for metallic • Li2S • AuAg • PbNO3 • NO • C6H12O6 • SnN

8. Identify the type of bond • A for ionic, B for polar covalent, C for nonpolar covalent • K2O • NS3 • N2 • AuI • NaF • C6H12

9. Nomenclature (Naming) • Type I • Use for ionic bonds when the cation has only one charge (groups1A-3A). • The first element keeps its name and the second element changes the end of its name to –ide (unless it already has a fancy name). • Criss-cross charges if uneven. • Ex. NaBr is sodium bromide • Ex. CaCl2 is calcium chloride • Ex. Be(ClO3)2 is beryllium chlorate

10. Nomenclature • Type II • Use for ionic bonds when the cation has more than one charge (transition metals). • The first element keeps its name and the second element changes the end of its name to –ide (unless it already has a fancy name). • Use a roman numeral to show the charge of the first ion. • Criss-cross charges if uneven. • Ex. AuI is gold (I) iodide • Ex. Mn2O3 is manganese (III) oxide • Ex. W3(PO4)2 is tungsten (II) phosphate

11. Nomenclature • Type III • Use for covalent bonds. • Use prefixes to denote the number of atoms and change the ending of the second element to -ide. • Ex. S2O3 is disulfur trioxide • Ex.N3P4 is trinitrogentetraphosphide • Ex. BrH5 is bromine pentahydride

12. Naming Organizer

13. Name the compound • Li2S • AuI3 • PbNO3 • C5H10 • NO • SnN

14. Write the formula • Barium fluoride • Zinc (II) nitride • Carbonheptaiodide • Ammonium sulfate • Aluminum hypochlorite • Pentaphosporusnonanitride • Tungsten (IV) permanganate

15. Review Game • whiteboards

16. #1 • What part of the atom is involved in a chemical bond? • electrons

17. #2 • What type of bond is SrS? • ionic

18. #3 • Name Ni2S3. • Nickel (III) sulfide

19. #4 • What happens to the electrons in a metallic bond? • Delocalized electrons float in electron sea.

20. #5 • What structure does an ionic bond make? • Crystal lattice

21. #7 • What type of bond is H2O? (Be specific!!) • Polar covalent

22. #8 • Write the formula for Cobalt (III) oxide. • Co2O3

23. #9 • What happens to the electrons in a nonpolar covalent bond? • Shared equally

24. #10 • Write the name for C4H10. • Tetracarbondecahydride

25. #11 • What happens to the electrons in an ionic bond? • Transferred • Give/take

26. #12 • What are 2 characteristics of metals? • Malleable • Ductile • Luster • Conductor • Solid