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Quiz Review

Quiz Review. Ionic Bonding Periodic Trends Formula Writing and Naming. All atoms on the periodic table desire to become like the noble gases. Why?. a.Noble gases have a full outermost energy level. b.Noble gases bond easily with other elements. c.Noble gases make really neat explosions.

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Quiz Review

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  1. Quiz Review Ionic Bonding Periodic Trends Formula Writing and Naming

  2. All atoms on the periodic table desire to become like the noble gases. Why? a.Noblegases have a full outermost energy level. b.Noblegases bond easily with other elements. c.Noblegases make really neat explosions. d.Noblegases have 7 valence electrons.

  3. Noble gases have a full outermost energy level.

  4. Which statement about the alkali metals is correct? a.They are located in the left-most column on the periodic table. b.They are extremely nonreactive. c.They are usually gases. d.They form negative ions with a -1 charge.

  5. They are located in the left-most column on the periodic table

  6. Most halogens form compounds by a.gaining an electron to form a negative ion. b.losing an electron to form a positive ion. c.losing protons. d.losing neutrons.

  7. gaining an electron to form a negative ion

  8. Which element is more reactive, potassium or sodium? a.Potassium - It gains electrons easily because of its atomic radius. b.Potassium - It loses electrons easily because of its atomic radius. c.Sodium - It gains electrons easily because of its atomic radius. d.Sodium - It loses electrons easily because of its atomic radius.

  9. Potassium - It loses electrons easily because of its atomic radius

  10. Which element is more reactive, fluorine or iodine? a.Fluorine - It loses electrons easily because of its mass. b.Fluorine - It gains electrons easily because of its mass. c.Iodine - It loses electrons easily because of its mass. d.Iodine - It gains electrons easily because of its mass.

  11. Fluorine - It gains electrons easily because of its atomic mass

  12. In a chemical formula, the number of atoms in the compound is shown by the a.oxidation number b.coefficient c.superscript d.subscript

  13. subscript

  14. In a chemical formula, the number of molecules in the compound is shown by the a.oxidation number b.coefficient c.superscript d.subscript

  15. coefficient

  16. How many electrons are needed in the outer energy levels of most atoms for the atom to be chemically stable? a.2 b.6 c.4 d.8

  17. 8

  18. What kind of chemical bond is formed when electrons are transferred from one atom to another? a.ionic b.metallic c.covalent d.hydrogen

  19. ionic

  20. What is the total number of atoms in the compound Ca(ClO3)2? a.2 b.6 c.3 d.9

  21. 9

  22. How many total hydrogen atoms are present in one molecule of ammonium acetate NH4C2H3O2? a.3 b.7 c.4 d.11

  23. 7 ammonium acetate NH4C2H3O2

  24. An atom that has an electrical charge is called a/an a.element b.isotope c.ion d.molecule

  25. ion

  26. When an atom loses electrons, the atom gains a ________charge. a.positive b.negative

  27. positive

  28. When an atom gains an electron, the atom gains a _________ charge. a.positive b.negative

  29. negative

  30. A molecule that shares electrons unevenly between the atoms is called a.nonpolar b.ionic c.polar d.neutral

  31. polar

  32. The order of atoms on the periodic table is based on a.the number of protons in the nucleus b.the number of neutrons in the nucleus c.the electric charge of the nucleus d.atomic mass

  33. the number of protons in the nucleus

  34. Atoms of elements in the same group have the same number of a.protons b.valence electrons c.neutrons d.protons and neutrons

  35. valence electrons

  36. Alkali metals are extremely reactive because they a.have very small atomic masses b.are not solids at room temperature c.have one valence electron that is easily lost to form a positive ion. d.have two valence electrons that form compounds with calcium and magnesium

  37. have one valence electron that is easily lost to form a positive ion.

  38. The electrons in a nonpolar covalent bond are a. gained b. shared equally c. lost d. shared unequally

  39. shared equally

  40. The formula for magnesium nitrate is a. MgNO3 b. Mg(NO3)2 c. Mg2NO3 d. Mg2(NO3)3

  41. Mg(NO3)2

  42. How many electrons are gained/lost by magnesium and what is the charge of the ion that it forms? • Loses 2 electrons to form a magnesium ion with a -2 charge. • Gains 2 electrons to from a magnesium ion with a -2 charge. • Loses 2 electrons to form a magnesium ion with a +2 charge. • Gains 2 electrons to form a magnesium ion with a +2 charge.

  43. Loses 2 electrons to form a magnesium ion with a +2 charge

  44. What ions make up the compound FeCl3? a.1Fe 3+ ion and 1Cl- ion b.1Fe3+ ion and 3 Cl- ions c.1Fe2+ ionic and 3Cl- ions d.3Fe3+ ions and 1Cl- ion

  45. 1Fe 3+ ion and 1Cl- ion

  46. Which element has the largest atomic radius? a.Aluminum b.Sulfur c.Silicon d.Chlorine e.Phosphorus

  47. Aluminum

  48. Water is considered a polar molecule because • the molecule has a net positive charge b. the molecule has a net negative charge c. the molecule has a net zero charge d. the ends of the molecule have partial negative and positive charges

  49. The ends of the molecule have partial negative and positive charges

  50. Write the formula for the following ionic bonding pairs and name them! • Ca + Br • K + I • Na + O • B + S • Al + F • Al + SO4 • NH4 + Cl • Fe (III) + NO3

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