Intro to Bonding

1. Intro to Bonding Valence Electrons, Lewis Dot Structures, and Electronegativity

2. Standards 2. Biological, chemical, and physical properties of matter result from the ability of atoms to form bonds from electrostatic forces between electrons and protons and between atoms and molecules. As a basis for understanding this concept: a. Students know atoms combine to form molecules by sharing electrons to form covalent or metallic bonds or by exchanging electrons to form ionic bonds. 2. b. Students know chemical bonds between atoms in molecules such as H2, CH4, NH3, H2CCH2, N2, Cl2, and many large biological molecules are covalent. 2. c. Students know salt crystals, such as NaCl, are repeating patterns of positive and negative ions held together by electrostatic attraction. 2. d. Students know the atoms and molecules in liquids move in a random pattern relative to one another because the intermolecular forces are too weak to hold the atoms or molecules in a solid form. 2. e. Students know how to draw Lewis dot structures. 2. f.* Students know how to predict the shape of simple molecules and their polarity from Lewis dot structures. 2. g.* Students know how electronegativity and ionization energy relate to bond formation. 2. h.* Students know how to identify solids and liquids held together by van derWaals forces or hydrogen bonding and relate these forces to volatility and boiling/melting point temperatures.

6. The Hippie

7. The Hippie Sure man, it’s only money. I’ll probably be happier if I give it away anyhow.

8. The Accountant

9. The Accountant No Way am I giving you my Money! You’re Irresponsible. In fact give me your money so I can invest it for you!

10. Electronegativity • electronegativity – how much an atom wants to keep hold of its electrons. • ionization energy – the energy required to remove an electron from an atom.

12. Greater electronegativity Lower electronegativity

13. Which has the greater electronegativity? • Sodium or Oxygen? Oxygen • Fluorine or Nitrogen? Fluorine • Potassium or Iron? Iron

15. Greater ionization energy Lower ionization energy

16. E.N. and I.E. increasing

17. Which has the greater ionization energy? • Lithium or Beryllium? Beryllium • Zinc or Calcium? Zinc • Argon or Sulfur? Argon

18. Electronegativity vs. Ionization energy • The greater the electronegativity, the moreenergy is needed to remove an electron. • The lower the electronegativity, the lessenergy is needed to remove an electron.

19. Atomic Radii • When atoms have greater electronegativity, they hold their electrons closer. • Atoms with a lower electronegativity, have a greater atomic radius.

20. Atomic Radii

21. A.R. increasing

22. Reactivity • The closer atoms are to the noble gases, the more they want to react so they can become like them.

23. More Reactive More Reactive

24. More Reactive More Reactive E.N. and I.E. increasing A.R. increasing

26. Ionic Radii

27. Compounds • Sometimes two (or more) different elements encounter each other and the conditions are right to form a bond (or bonds) between them. • This usually occurs because their electrons are more stable when they reorganize to form a bond. • Often their electrons are organized more like a noble gases’ electrons after forming a compound. • The group of two (or more) different elements are now called a compound.

28. Compounds • bonds form between two different elements. • Their electrons become more stable (often arranged more like a noble gases’ electrons). • They are now called a compound.

29. Metals

30. Nonmetals

31. Three General Bonding Types • Metal with Nonmetal • Metal with Metal • Nonmetal with Nonmetal

32. Semi-metals or metalloids Nonmetals Metals

33. Metal with Nonmetal Bonding • Ionic compounds – the metal gives all of its valence electrons to the nonmetal. • Known as – Salts, ions

34. Metal with Metal Bonding • Metallic compounds – the both metals freely share their valence electrons with each other. • Known as – alloys

35. Nonmetal with Nonmetal Bonding • Covalent compounds – both nonmetals try to keep hold of their valence electrons as well as each other’s valence electrons. It ends up being a constant tug of war (although technically sharing). • Known as – molecules

36. Three General Bonding Types • Metal with Nonmetal - form ionic compounds • Metal with Metal - form metallic compounds • Nonmetal with Nonmetal - form covalent compounds

37. Three General Bonding Types • Metal with Nonmetal - form ionic compounds (one gives, the other takes) • Metal with Metal - form metallic compounds (both freely share valence electrons - ) • Nonmetal with Nonmetal - form covalent compounds (both try to hold on at the same time)

38. Semi-metals or metalloids Nonmetals Metals

39. Which kind of compound will these elements form? • Iron and Nickel: Metallic compound • Sulfur and Calcium: Ionic compound • Carbon and Oxygen: Covalent compound M + M  metallic N + N  covalent M + N  ionic

40. Which kind of compound will these elements form? • Hydrogen and Nitrogen: Covalent compound • Magnesium and Oxygen: Ionic compound • Gold and Zinc: Metallic compound M + M  metallic N + N  covalent M + N  ionic

41. Semi-metals or metalloids Nonmetals Metals M + M  metallic N + N  covalent M + N  ionic

42. K H Na Li Mg Ca Be He O S Cl Ar F P N Br Kr C Si Al Ne B I Xe

43. 4 e– in valence shell