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Bonding

Bonding. 5-2. Why Bond. Bonds form when their valance electrons interact Bonds form to achieve stable electron configuration (full outer shell) Bonds act like springs, they are not rigid . Types of bonds. Ionic Metallic Covalent. Ionic bonds. Transfer of electrons

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Bonding

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  1. Bonding 5-2

  2. Why Bond • Bonds form when their valance electrons interact • Bonds form to achieve stable electron configuration (full outer shell) • Bonds act like springs, they are not rigid

  3. Types of bonds • Ionic • Metallic • Covalent

  4. Ionic bonds • Transfer of electrons • Forms between oppositely charged ions • One atom looses electrons, another gains • Causes one atom to become negative, and the other to be positive • Opposites attract and a network structure forms • Typically occurs between metals and nonmetals

  5. Strong attractions so very high melting points • They conduct electricity when melted or dissolved in water • Electricity is moving charges • Ions are free to move and carry the electric charge

  6. Metallic Bonds • Special type of ionic bonds • Attraction between one atoms nucleus and another’s electrons • Atoms in metals are tightly packed • Electrons are free to move from one atom to another • Atoms can move past one another easily

  7. Covalent bonds • Sharing of electrons • Often between non metals • Low melting points • Can be polar or non polar • Polar = uneven distribution or electrons • Non polar = even sharing of electrons • Make up molecules

  8. Polar vs non polar • polar • Non polar

  9. How to predict the bond type • Find melting point • High = ionic • Low = covalent • Are electrons shared or lost/gained • Lost/gained = ionic • Shared = covalent • Is it two non metals • Covalent • Is it two metals • metallic

  10. Polyatomic ions • Some complex compounds have both ionic and covalent bonds • These are called polyatomic ions • They are groups of covalently bonded atoms that have lost or gained electrons

  11. examples

  12. The ion can not be broken up • () show that the group are used to show that it acts as a single ion

  13. 1. What type of bond will form between Barium (group 2) and oxygen (group 16) • Metallic • Ionic • Covalent • No bond • I don’t know

  14. 2. In the bond from the last question (Barium group 2 and Oxygen group 16) what is the ratio of barium to oxygen • 2:1 • 1:2 • 1:1 • 2:16 • I don’t know

  15. 3. Carbon must form 4 bonds to be complete. Oxygen needs two bonds. What is the structural formula for carbon dioxide (CO2) • C=O=O • O-C-O • C=O=C • O=C=O • I don’t know

  16. 4. Sulfuric acid has a chemical formula H2SO4 it is made of hydrogen atoms and sulfate ions. How many of each are there? • 1 hydrogen and 1 sulfate • 2 hydrogen and 4 sulfate • 2 hydrogen 1 sulfate 4 oxygen • 2 hydrogen and 1 sulfate • I don’t know

  17. 5. Ammonium sulfate (NH4)2SO4 has two polyatomic ions, ammonium and sulfate, and has a neutral net charge. Sulfate has a 2- charge, what charge does ammonium have? • 1+ • 2+ • 1- • 2- • I don’t know

  18. 6. What type of bond is shown below • Metallic • Ionic • Covalent • No bond • I don’t know

  19. 7. How many bonds are present in this molecule • 1 • 3 • 5 • 6 • I don’t know

  20. Complete section 2 review page 158 all problems • Due tomorrow

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