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Test Review

Test Review . 6.1 Intro to Chemical Bonding 6.2 – 6.4 Ionic Bonding and Compounds 6.5 Covalent Compounds and Their Names. ANSWER KEY. 1. Which of the following properties of a compound depends on the type of bonding between the atoms . Melting point Brittleness

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Test Review

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  1. Test Review 6.1 Intro to Chemical Bonding 6.2 – 6.4 Ionic Bonding and Compounds 6.5 Covalent Compounds and Their Names

  2. ANSWER KEY

  3. 1. Which of the following properties of a compound depends on the type of bonding between the atoms • Melting point • Brittleness • Boiling point • Conductivity • All of the above

  4. 2. Which compound is a poor conductor of heat and electricity and has a high melting point? • CO2 • MgO • N2O • H2O • OF2

  5. 3. The P-Cl bond in phosphorus trichloride is: • ionic • polar covalent • Non-polar covalent

  6. 4. The electronegativity (EN) value of an element is a measure of the atom’s: • Degree of stability • Number of valence electrons • Ability to attract electrons • Degree of conductivity • Ability to attract protons

  7. 5. Which formula represents an ionic compound? • KCl • NO2 • HCl • CH4 • XeF2

  8. 6. To form an ion, a sodium atom • gains one electron • gains two electrons • loses seven electrons • loses one electron • loses two electrons

  9. 7. The octet rule indicates that • all of the noble gases have 8 total electrons • all of the shells in an atom hold a maximum of 8 electrons • all of the Group A elements have 8 valence electrons • atoms lose, gain, or share valence electrons to have 8 valence electrons • the noble gases react with other compounds to get 8 valence electrons

  10. 8. What is the symbol for an ion with 19 protons and 18 electrons? • F+ • F- • Ar+ • K- • K+

  11. 9. An ionic compound • has a net positive charge • has a net negative charge • contains only cations • contains only anions • has a net charge of zero

  12. 10. In a molecule with covalent bonding • oppositely charged ions are held together by strong electrical attractions • atoms of metals form bonds to atoms of nonmetals • atoms of different metals form bonds • atoms are held together by sharing electrons • atoms of noble gases are held together by attractions between oppositely charged ions

  13. 11. A group of covalently bonded atoms that has an overall electrical charge is called a(n) ___. • ionic compound • anion • polyatomic ion • cation • molecule

  14. 12. In a covalently bonded molecule, the number of electrons that an atom chares with others is usually equal to the number of electrons ___. • in the atom • in its nucleus • in all the atoms • in its ion • needed to have noble gas arrangement

  15. 13. How many valence electrons does carbon have? • one • two • three • four • five

  16. 14. An atom of sulfur has ___ pairs and ___ unpaired valence electrons. • 1, 2 • 2, 2 • 2, 1 • 3, 2 • 2, 3

  17. 15. An ionic bond is the result of ___. • a large difference in EN between the bonded atoms • a small difference in EN between the bonded atoms • no difference in EN between the bonded atoms • two nonmetals bonding • two metals bonding

  18. 16. Which of the following substances would most likely have the highest melting point? • CO • SO3 • H2 • Na2O • NO2

  19. 17. Which of the following substances has a molecules as its smallest unit? • NaCl • CH4 • Mg(OH)2 • CuO • All of the above.

  20. 18. Which of the following elements can be an exception to the octet rule? • germanium • oxygen • boron • carbon • chlorine

  21. 19. Unequal sharing of electrons results in: • nonpolar covalent bonds • ionic bonds • polar covalent bonds • no bonds being formed • compounds with VERY high boiling points

  22. 20. If the following generic atom were to ionize, what would be the most likely product? • + 6 • - 6 • + 2 • - 2 • probably would NOT ionize!

  23. 21. If compound “A” has a higher melting point than compound “B”, which compound is most likely the ionic compound? • A • B • neither

  24. 22. Which of the following best describes covalent compound? • they conduct electricity in their gas or liquid phase • they are ordered into crystal lattice structures in their solid states • they have very low melting points • they bond to make formula units • they are held together by electrostatic attraction

  25. 23. Because one atom usually attracts the electrons more strongly than the other atom: • nonpolar covalent bonds are rare • Polar covalent bonds are rare • ionic bonds are rare • most substances are nonpolar covalent • very few substances are ionic

  26. 24. The % ionic characteristic of a bond is very large when the difference in EN is: • small • large • negligible • zero • EN plays no part in the % ionic character of a bond

  27. 25. The least whole number ratio of cations to anions refers to the chemical formula for ___ compounds. • molecular • ionic • covalent • polar covalent • nonpolar covalent

  28. 26. In the diagrams below, represents an atom of sulfur and represents an atom of oxygen. Which diagram best represents the compound sulfur (IV) oxide? • A • B • C • D • none of these

  29. 27. Which of the following is a binary compound? • NaOH • H2O • H2 • Na • sodium iodite

  30. 28. Which element forms more than one binary compound with chlorine? • Zn • Fe • Li • Ca • Mg

  31. 29. Which kind of compound generally results when nonmetal atoms chemically combine with metal atoms? • molecular • covalent • nonpolar covalent • polar covalent • ionic

  32. 30. Which EN value is closest to that of an alkali metal? • 0 • 1.0 • 2.0 • 3.0 • 4.0

  33. 31. The greatest degree of ionic character would be found between sulfur and ___. • oxygen • phosphorus • chlorine • another sulfur • bromine

  34. 32. Which of the following elements will most likely form an ion with a -1 charge? • Mg • Na • Cl • S • Ne

  35. 33. Which of the following contains an ionic bond? • PO43- • SF3 • MgCl2 • Cl2 • none of the above

  36. 34. How many chloride ions are needed to balance the positive charge of a barium ion? • 1 • 2 • 3 • 4 • cannot tell without knowing more about the compound

  37. 35. How many covalent bonds would the following atom usually form? • 1 • 2 • 3 • 4 • would be unlikely to form covalent bonds!

  38. 36. How many nonbonding pairs of electrons are in the following molecule? H – H • 6 pairs • 8 pairs • 1 pair • 0 pairs • none of the above

  39. 37. The bonding in NH3 is most similar to the bonding in • KF • H2O • NaCl • MgO • none of the above

  40. 38. Which compound contains both covalent bonds and ionic bonds? • N2O5 (g) • HCl (g) • NaCl (s) • NaNO3(s) • none of the above

  41. 39. What type of bond is present one unit of water? • polar covalent • nonpolar covalent • ionic

  42. 40. A substance that has a melting point of 1,074 K conducts electricity when dissolved in water, but does not conduct electricity in the solid phase. The substance is most likely • molecular • covalent • ionic • nonpolar covalent

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