Chapter 8: The Periodic Table and Properties of Metals
Name ____________________________
______________ 1. For which of the following processes will energy be absorbed?
a) separating an electron from an electron.
b) separating an electron from a proton.
c) separating a proton from a proton.
d) removing an electron from a neutral atom.
Per _____
______________ 2. a) How much would 0.754 mol of chlorine – 35 atoms weigh?
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b) How much would 0.246 mol of chlorine – 37 atoms weigh?
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c) What is the mass of a mole of “average “ atoms in a mixture of the above samples?
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d) What is the atomic weight of the naturally occurring mixture of these two isotopes of
chlorine?
3. Why are metals malleable? (Use solid structure to explain) ___________________________
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______________ 4. In what area of the periodic table do we find the elements of highest ionization energy?
(center? lower right? upper left? etc.)
______________ 5. Which of these properties increase as we move down the periodic table?
a) atomic radius
b) ionization energy
c) metallic character
______________ 6. Which of the following elements has the largest ionization energy?
a) C
b) N
c) Si
d) P
7. If a new element were made and found to have 115 protons and 187 neutrons,
a) its atomic number would be ______________
b) its approximate molar mass would be ___________________
c) its probable electron configuration would be
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The element it would most resemble in chemical properties would be _________________
8. a) An alkali metal produces ions having the same electron configuration as atoms of the
preceding inert gas. In what ways do these ions differ from the inert gases?
b) In what ways are they similar to inert gases?
______________ 9. Which of the following is NOT a correct formula for a normal substance?
a) H2S (g)
b) CaCl2 (s)
c) He (g)
d) NaNe (s)
e) Al2O3 (s)
10. Write the molecular formulas of the hydrogen compounds of the second row elements.
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______________11. Which of the following properties does NOT apply to alkali metals?
a) high ionization energy
b) large atomic radius
c) high electrical conductivity
d) outer configuration of n s1
12. All of the isotopes of the element with atomic number 87 are radioactive. Hence, it is not
found in nature. Yet, prior to its preparation by nuclear bombardment, chemists were
confident they knew the chemical reactions this element would show. EXPLAIN. What
predictions about this element would you make?
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a) Prediction ____________________________
b) Prediction ___________________________________
13. Using the periodic table, write possible chemical formulas for
a) barium hydride __________________
b) germanium chloride ____________________
c) indium oxide ____________________
d) tin fluoride ____________________________
14. Magnesium metal burns in air, emitting light useful for flares and forming clouds of white
smoke. Write the equation for the reaction. Include phases.
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______________15. How much heat is evolved if one pound (454 g) of lime is slaked according to the following
reaction?
CaO (s) + H2O (l) → Ca(OH)2 (s) + 15.6 kcal
16. What property held in common by the alkaline earth elements accounts for the fact that the
free elements are not found in nature?
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17. What property held in common by the following compounds accounts for their presence in
natural mineral deposits? MgCO3, CaCO3, SrCO3, BaSO4, Ca3(PO4)2.
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18. Using your list of alloys as reference, list nine alloys which contain copper, underlining
those which are greater than 50% copper. (see reference worksheet)
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19. What is pewter? Give its composition and a use. Which metal dominates?
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20. What is an amalgam? Which metal dominates the alloy? Give a use for an amalgam.
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