1 / 22

Chapter 7 Ionic and Metallic Bonding

Chapter 7 Ionic and Metallic Bonding. Ms. Wang Lawndale High School. Section 7.1 - Ions. Valence Electrons – electrons in the highest occupied energy level of an element’s atoms. To find the valence electrons in an atom of the representative element, simply look at the group number.

nadine
Download Presentation

Chapter 7 Ionic and Metallic Bonding

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. Chapter 7Ionic and Metallic Bonding Ms. Wang Lawndale High School

  2. Section 7.1 - Ions • Valence Electrons – electrons in the highest occupied energy level of an element’s atoms • To find the valence electrons in an atom of the representative element, simply look at the group number

  3. Electron Configuration and Valence Electrons Example: How many electrons are in the valence shell of sodium? Step 1: Write the electron configuration of sodium Na = [Ne]3s1 Step 2: Count the number of electrons in the valence shell (outermost shell).

  4. Determine the Valence electrons in each of these elements • K 6. Be • P 7. Li • C 8. He • O 9. Ne • N 10. B

  5. Electron Dot Structure • Diagrams that show valence electrons as dots 3 5 PRACTICE 1. K 6. Be 2. P 7. Li 3. C 8. He 4. O 9. Ne 5. N 10. B X 2 6 1 8 4 7

  6. Octet Rule • Eight electrons in the highest occupied energy level just like the noble gases (except He) • Metal elements lose their valence electrons • Nonmetal elements gain electrons

  7. Formation of Cations 3s 2p 2s 1s Sodium atom Na Sodium ion Na+ Neon atom Ne Na Na+ + e-

  8. Formation of Anions 2p 2s 1s Fluorine atom F Fluorine ion F- Neon atom Ne F + e- F-

  9. Practice • Show how a Lithium atom becomes an cation 2. Show how a Calcium atom becomes a cation 3. Show how a Chlorine atom becomes an anion 4. Show how an Oxygen atom becomes an anion

  10. Bonding • Once an atom has a stable octet, it is happy and doesn’t want to react anymore • Atoms without stable octets, are sad and want to react with another element to achieve a stable octet • Gain or Lose Valence Electrons Complete this sentence: Noble Gases do not easily form bonds because….

  11. Why do atoms form bonds?To be more chemically stable and less reactive How do atoms become more chemically stable and less reactive? • By having completely filled s and p orbitals just like the noble gases

  12. Section 7.2 – Ionic Bonds • Ionic Compounds – metal cations and nonmetal anions that are held together by electrostatic forces • Although ionic compounds are composed of ions, they are electrically neutral

  13. Ionic Bonding • An ion is an atom that has gained or lost one or more electrons and thus have an electrical charge. • To find the charge of the ion subtract the number of electrons from the number of protons. Example: [S]=1s22s22p63s23p4 (16 p+, 16e-) [S2-] 1s22s22p63s23p6 (16p+, 18e-) 16 -18 = -2

  14. Labeling the Periodic Table These elements have the following charges: Group 1A = 1+ Group 2A = 2+ Group 3A = 3+ Group 4A = 4+ or 4- Group 5A = 3- Group 6A = 2- Group 7A = 1-

  15. SALTS When cations and anions form bonds with each other they are called SALTS • The + and - charges that cations and anions have causes an attraction between the two • They come together to form an ionic bond also known as a salt. Example: Na+ Cl- NaCl

  16. SALTS When cations and anions form bonds with each other they are called SALTS • Example: Li 1s 2p F 1s 2p Li+ LiF F-

  17. Practice Show how the following compounds bond with the use of orbital diagrams • NaF • KBr • MgO • Li2S • CaCl2 • AlN

  18. Ionic Bonds • Ionic bond is typically a bond between a METAL CATION and a NONMETAL ANION • The electrostatic forces between the two types of ions hold them together • Bonds form when metals donate electrons to nonmetals

  19. Properties of Ionic Compounds • CrystallineSolid at Room Temperature • High Melting Points • Can conduct an electric current when melted or dissolved in water

  20. Section 7.3 – Bonding in Metals • Metallic bond is a bond between metal cations. • The attraction of the free floating valence electrons for the positively charged metal ions hold them together.

  21. Crystalline Structure of Metals • Metal atoms are arranged in very compact and orderly patterns • Physical Properties of Metals • Good Conductors of electrical current • Ductile - can be drawn into wires • Malleable – can be hammered or shaped • Alloys – mixtures composed of two or more elements, at least one being a metal

  22. Homework Chapter 7 Assessment #’s 30-44, 48, 53, 55, 56, 58, 59, 60, 62, 63, 64, 65, 72, 73, 87, 88, 90, 92, 93, 94, 95

More Related