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Ions, Ionic Bonds and Metals

Ions, Ionic Bonds and Metals. Chapter 7. Valence Electrons- Electrons in the outermost energy level of an atom VE number = the Group Number of A elements. Ions and Ion Formation. Electron Dot Structures (Diagrams) show the valence electrons ONLY drawn around the symbol of the element.

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Ions, Ionic Bonds and Metals

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  1. Ions, Ionic Bonds and Metals Chapter 7

  2. Valence Electrons- Electrons in the outermost energy level of an atom • VE number = the Group Number of A elements Ions and Ion Formation

  3. Electron Dot Structures (Diagrams) show the valence electrons ONLY drawn around the symbol of the element. • Electrons only pair after there is an electron on each side of the symbol Lewis Structures

  4. Remember- Metals give away and Nonmetals take VE • All elements want 8 VE • Bonds occur because of the giving/taking of electrons which result in charges • Opposite Charges attract Bonding

  5. Octet Rule- all elements want to have 8 valence electrons and will bond to achieve this • Noble Gases- Group 8A= 8 VE • Don’t bond because they have already achieve the Octet Rule Octet- Rule of 8

  6. Metals- lose VE and gain a positive charge based on number of VE lost • Cations • Nonmetals/Metalloids- Gain VE and gain a negative charge based on number of VE gained • Anions Meeting the Octet Rule

  7. Cations: • Name: Metal Name “Ion” • Lithium Ion • Anions: • Name: Root Name, end in –ide • Chlorine (Cl-) becomes “Chloride” • “Halide”- halogen ions Naming Ions

  8. Electrical Charges of Ionic Compounds is ALWAYS “0” or neutral. • Cations (+) and Anions (-) have opposite forces • Opposites attract and are held together • The electrostatic forces that hold ions together in ionic compounds are called ionic bonds Ionic Compounds

  9. Chemical Formula- shows the numbers of atoms of each element in the smallest representative unit of a substance. • Formula Units- the lowest whole-number ratio of ions in an ionic compound. Chemical Formula & Formula Units

  10. 1.) Crystalline Solid at room temperature • Very Stable Structure due to large attractive forces • 2.) High Melting Points- lots of energy to change state of matter • 3.)Conduct Electricity when dissolved in water Properties of Ionic Compounds

  11. When Melted or in Dissolved in Water: • Ions dissociate and exist in a solution • + and – charges floating that conduct electricity Conducting Electricity

  12. Valence Electrons are mobile and drift freely from one part of the metal to another • Metallic bonds are the forces of attraction between the free-floating valence electrons and the positively charged metal ions. Metallic Bonding

  13. Ductile- can be drawn into wires • Malleable- can be hammered into thin sheets without breaking • High Melting Point- requires a lot of energy to break the bonds Metal Properties

  14. Crystalline Structure- compact, orderly, repeating pattern • Metals form crystals in 3 forms: • Every atom except those on the surface have: • Body Centered- 8 neighbors • Face Centered- 12 neighbors • Hexagonal Close-Packed- 12 neighbors (hexagonal shape) Metallic Structures

  15. Mixtures of 2 or more elements; at least 1 is a metal • Ex. Brass • Properties are superior to the elements that make it- STRONGER • Stainless Steel Alloys

  16. Page 214; # 27-51 • Write the electron dot structures for: • Li, Mg, Al, N, O, F, Cl, Ne • Identify all possible IONIC bonds Assignment

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