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quiz3key - difference in ionization energies generally...

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CHEMISTRY 131 Quiz #3 Friday, February 10, 2006 Name: __________Key___________________________ 1. Explain the difference between metallic and ionic bonding. Why wouldn't you expect to observe metallic bonding in a solid with more than one type of atom? Why would an element such as carbon not form a metallic solid? (6 points) In metallic bonding, electrons are free to travel throughout the solid because the atoms have low ionization energies, and so they lose electrons easily. The solid consists of positively charged atoms surrounded by an electron "cloud". In contrast, ionic bonding consists of a strong electrostatic interaction between positively and negatively charged ions, which are created when an atom with a low ionization energy loses an electron to an atom with a high ionization energy. Metallic bonding is usually not observed in solids containing more than one solid because the
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Unformatted text preview: difference in ionization energies generally means that electrons will be "pinned" at the atoms with the higher ionization energies, resulting in the creation of ions. An element such as carbon would not be expected to form a metallic solid because it does not have a low enough ionization energy; instead, it tends to form molecular solids or extended solids with covalent bonding. 2. Draw a valid unit cell on each of the patterns below. (4 points) Bonus: Fill in the missing 30 elements. 21 – 30 = +1 11 – 20 = +0.5 1 – 10 = +0 1 18 H 2 13 14 15 16 17 He Li Be B C N O F Ne Na Mg 3 4 5 6 7 8 9 10 11 12 Al Si P S Cl Ar K Ca Sc Ti 23 V 24 Cr 25 Mn 26 Fe 27 Co 28 Ni 29 Cu 30 Zn Ga Ge As Se Br Kr Rb Sr Y Zr Nb Mo Tc Re Rh Pd Ag Cd In Sn Sb Te I Xe Cs Ba La Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn Fr...
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