1. Physical Science Chapter 6 Chemical Bonds

2. Bonding Chapter 6 is about different types of atomic bonding Forces of attraction is the key to this bonding The physical properties of elements is key to the different types of bonds

3. Bonding

4. Draw the electron configuration of the elements neon and sodium

5. What do you notice about the Valence electrons and the energy level of each element?

6. Stable Electron Configurations When the highest occupied energy level of an atom is filled with electrons, the atom is stable and not likely to react

7. Ionic Bonds Elements without complete sets of valence electrons tend to react They react to try to achieve the stability of a full energy level…like the noble gases

8. Transfer of Electrons Look at the electron dot diagrams for sodium and chlorine What do you think these elements will want to do?

9. Atomic Chemical Reaction When sodium and chlorine react: An electron is transferred from each sodium atom to a chlorine atom. Now each atom is more stable

10. When an atom gains or loses an electron, the protons and electrons are no longer equal and the atom is not neutral. An atom with a positive or negative charge is an ion

11. Notice the positive and negative charge on the new sodium and chlorine atoms

12. Charge An ion with a negative charge is an anion. Chlorine in NaCl is an anion…Cl - It is negative because it has one more electron than protons, thus a charge of 1- Anions are written using a part of the elemental name and the suffix ide. – chloride

13. Our new sodium ion, because it lost an electron now has more protons than electrons, making it positive or 1+ – Na + Cations are named just using the elemental name, sodium

14. Chemical Bonds A chemical bond is what holds atoms or ions together Ionic bonds are what holds cations and anions together – Ionic bond forms when electrons are transferred from one atom to another

15. Chemical Bonds http://www.youtube.com/watch?v=QXT4OVM 4vXI http://www.youtube.com/watch?v=QXT4OVM 4vXI

16. Ionization Energy The amount of energy used to remove an electron from an atom is ionization energy It varies form element to element The lower the ionization energy, the easier it is to remove an electron

18. Which element would it be easier to take an electron from, Magnesium or Calcium?

19. Ionic Compounds Compounds that contain ionic bonds are ionic compounds These can be represented by a chemical formula: – Notation that shows what elements a compound contains and the ratio of the atoms or ions of these elements in the compound: NaCl

20. Practice We want to make a compound with magnesium and chloride What group is magnesium in? What group is chlorine in?

21. How will we combine these elements? + =

22. + = MgCl 2

23. MgCl 2 = The subscript 2 shows how many atoms of that element are present If there is not a subscript, that implies that there is only one atom

24. Ratios are Easier It is easier to see the number of atoms when you break a formula down into ratios For example, H 2 O has a hydrogen to oxygen ratio of 2:1 Find the ratios of the following formulas: Sodium Chloride, NaCl= Magnesium Chloride, MgCl 2 = Sodium Oxide, Na 2 O=

25. Crystal Lattices How are the ions in a grain of salt arranged?(162) Attractions between opposing charges keeps the ions in a fixed, repeating position Solids whose particles are arranged in lattice structure are called crystals

26. The shape of an ionic crystal depends on the arrangement of ions in its lattice The arrangement of the ions depends on the ratio of ions (like the exercise you just did) and their relative sizes

27. Compare Compare figure 5a and 5b (pg 162) Answer the following questions: 1. How are the sodium ions represented? 2. How are the Chloride ions represented? 3. What do you notice about the locations of the positive and negative ions? 4. What is the similarity between the diagram of NaCl and the photograph of NaCl?

28. Properties of Ionic Compounds The properties of NaCl are typical of other ionic compounds: High melting point (801 degrees Celsius) As a solid they are poor electric conductors As a liquid they are good electric conductors They shatter when struck with a hammer

29. All of these properties of ionic compounds are explained by the strong attractions within a crystal lattice

30. For electric current to flow, charged particles must be able to flow from one location to another Ions in a crystal lattice have a fixed position When they melt, the lattice breaks apart and ions are free to flow Melted sodium chloride is an excellent elctric conductor

31. Complete the section 1 assessment in your book and the questions in your workbook for this section

32. Covalent bonds http://www.youtube.com/watch?v=yjge1WdC FPs http://www.youtube.com/watch?v=yjge1WdC FPs

33. Covalent Bonds Someone read Covalent Bonds, pg 165 Covalent Bond: a chemical bond in which two atoms share a pair of valence electrons

34. Example: Hydrogen has one valence electron If it had one more it could reach the stability of a full orbital for its energy level So it wants to share an electron with another atom that also only has one valence electron… Hydrogen

35. These two hydrogen atoms that share a valence electron form a molecule Molecule: a neutral group of atoms that are joined together by one or more covalent bonds

36. The molecule is neutral because it has two protons and two electrons The attraction between the shared electrons and the protons in the individual nuclei holds the atoms together in a covalent bond

37. The chemical formula for this covalent bond/molecule is H 2 The subscript 2 is for the 2 hydrogen atoms in the molecule

38. Diatomic molecules: Two atoms Many nonmetals make diatomic molecules…why?

39. Halogens, for example, all have 7 valence electrons If two of them share an electron they both achieve a stable electron configuration

41. Multiple covalent bonds Atoms can share more than one electron They can share pairs If they share 2 pairs, it is called a double bond If they share 3 pairs it is called a triple pair

44. Ionic and Covalent bonds http://www.youtube.com/watch?v=QqjcCvzW www http://www.youtube.com/watch?v=QqjcCvzW www

45. Polar Covalent Bonds A covalent bond in which electrons are not shared equally is a polar covalent bond In a molecule with the same element, the attraction is the same In a molecule of a compound, this may not be the case

46. Some atoms may have a greater attraction than others and thus the electrons spend more time near that atom in the bond than the other

47. Because they are sharing electrons, neither atom becomes + or – like ionic bonds. However, they can become partially + or – when the electrons are shared unequally If so, they are assigned the symbol delta – or delta +, depending on which one gains or loses the electrons most

48. Polar and Nonpolar Molecules http://www.youtube.com/watch?v=PVL24HAe snc http://www.youtube.com/watch?v=PVL24HAe snc

49. Polar and Nonpolar Molecules *Recall that a molecule is a neutral group of atoms that are joined together by one or more covalent bonds* A molecule that has only two atoms that share a covalent bond, the molecule will be polar A molecule that has more more than two atoms that share a covalent bond, the molecule may not be polar

50. The type of atom in a molecule and its shape determine whether a molecule is polar or nonpolar

51. Nonpolar example Carbon dioxide CO 2 Oxygen has a stronger attraction for electrons Therefore it is a polar molecule Because the molecule is linear, However, the equal pull cancels Out the polarity and the Molecule is nonpolar

52. Polar Example Water, H 2 O Oxygen has a stronger attraction to electrons than hydrogen, making this a polar molecule Because the shape is bent, the polar bonds do not cancel out This is a polar molecule

53. Attraction Between Molecules Attractions between Molecular compounds are not as strong as ionic or covalent bonds Attractions between polar molecules are stronger than attractions between nonpolar molecules

54. These strengths and weaknesses explain a lot about elements and their behavior Water and methane are very similar in mass, but methane boils at -161.5 C and water boils at 100 C

55. Methane is nonpolar and water is polar These attractions increase the energy required for materials to boil/break the bonds

56. Activity Create a comparison chart Compare the different bonds we have discussed – 1. ionic bonds – 2. covalent bonds – 3. polar bonds – 4. nonpolar bonds Include how the electrons behave, types of elements involved in the bond, strength of the bond, etc.

57. When you finish Complete the section 2 assessment Complete the section 2 questions in your work book Due tomorrow Quiz tomorrow

58. 6.3: Naming Compounds and Writing Formulas/Ionic Formulas Ionic formulas involve the transfer of electrons from one atom to another Many of our examples will include a metal giving away their electrons to a non metal

59. Both elements in the transaction now become atoms, specifically the element that lost electron(s) becomes a cation with a positive charge. The name of this ion remains the same The element that gained electron(s) becomes a anion with a negative charge. The name of this ion is changed to the element name with the new suffix ide

60. Binary Ionic Compounds Bi=two Binary ionic compounds include only two elements: one cation and one anion Ex: NaCl, The order is always cation,anion

61. Common Anions

62. Metal Cations Alkali metals, alkaline earth metals, and aluminum form ions with charges equal to their group number – Potassium ion= K + – Calcium ion= Ca 2+ – Aluminum ion= Al 3+

63. Transition Metals Many transition metals form more than one type of ion. Look at the Table of metal cations on pg 172 There are several elements that can form more than one type of ion. The Roman Numeral after the element name indicates the charge of the ion

64. So looking at the elements and their notation, how would you write the formula for the compound that makes red copper? copper one oxide

65. Copper one= copper (I)= Cu 1+ Oxide = O 2- Because it takes 2 of the copper with only one + charge to balance the -2 charge of the Oxide, we would write the formula: Cu 2 O