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Clicker Questions

Review. Clicker Questions . As atoms bond with each other, they. increase their potential energy, thus creating less-stable arrangements of matter. decrease their potential energy, thus creating less-stable arrangements of matter.

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Clicker Questions

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  1. Review Clicker Questions

  2. As atoms bond with each other, they • increase their potential energy, thus creating less-stable arrangements of matter. • decrease their potential energy, thus creating less-stable arrangements of matter. • increase their potential energy, thus creating more-stable arrangements of matter. • decrease their potential energy, thus creating more-stable arrangements of matter.

  3. A compound that conducts electricity and is a solid at room temperature is usually: • Ionic • Covalent

  4. As light strikes the surface of a metal, the electrons in the electron sea • a. allow the light to pass through. • b. become attached to particular positive ions. • c. fall to lower energy levels. • d. absorb and re-emit the light.

  5. Most chemical bonds are • purely ionic. • purely covalent. • partly ionic and partly covalent. • metallic.

  6. Dinitrogen pentoxide contains how many oxygens? • 5 • 0.0

  7. In the compound Fe2O3, the charge of iron is • 3 • 0.0

  8. If you were to bond Tin (IV) with oxygen (-2 charge), what is the subscript behind oxygen? (Sn_O) • 2 • 0.0

  9. An ionic bond is between: • Two or more metals • A metal and a non-metal • Two or more non-metals • All of the above

  10. A covalent bond is between: • Two or more metals • A metal and a non-metal • Two or more non-metals • All of the above

  11. Chemical Bonding II. Molecular Compounds

  12. A. Energy of Bond Formation • Potential Energy • based on position of an object • low PE = high stability

  13. no interaction increased attraction A. Energy of Bond Formation • Potential Energy Diagram attraction vs. repulsion

  14. increased repulsion balanced attraction & repulsion A. Energy of Bond Formation • Potential Energy Diagram attraction vs. repulsion

  15. Bond Energy Bond Length A. Energy of Bond Formation • Bond Energy • Energy required to break a bond

  16. A. Energy of Bond Formation • Bond Energy • Short bond = high bond energy

  17. X 2s 2p B. Lewis Structures • Electron Dot Diagrams • show valence e- as dots • distribute dots like arrows in an orbital diagram • 4 sides = 1 s-orbital, 3 p-orbitals • EX: oxygen O

  18. Ne B. Lewis Structures • Octet Rule • Most atoms form bonds in order to obtain 8 valence e- • Full energy level stability ~ Noble Gases

  19. - + + B. Lewis Structures • Nonpolar Covalent - no charges • Polar Covalent - partial charges

  20. C. Molecular Nomenclature – Review! • Prefix System (binary compounds) 1. Less e-neg atom comes first. 2. Add prefixes to indicate # of atoms. Omit mono- prefix on first element. 3. Change the ending of the second element to -ide.

  21. PREFIX mono- di- tri- tetra- penta- hexa- hepta- octa- nona- deca- NUMBER 1 2 3 4 5 6 7 8 9 10 C. Molecular Nomenclature

  22. C. Molecular Nomenclature • CCl4 • N2O • SF6 • carbon tetrachloride • dinitrogen monoxide • sulfur hexafluoride

  23. C. Molecular Nomenclature • arsenic trichloride • dinitrogen pentoxide • tetraphosphorus decoxide • AsCl3 • N2O5 • P4O10

  24. C. Molecular Nomenclature • The Seven Diatomic Elements Br2 I2 N2 Cl2 H2 O2 F2 H N O F Cl Br I

  25. Chemical Bonding III. Ionic Compounds

  26. A. Energy of Bond Formation • Lattice Energy • Energy released when one mole of an ionic crystalline compound is formed from gaseous ions

  27. B. Lewis Structures • Covalent – show sharing of e- • Ionic – show transfer of e-

  28. B. Lewis Structures • Covalent – show sharing of e- • Ionic – show transfer of e-

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