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Entry Task: Oct 22 nd Monday

Entry Task: Oct 22 nd Monday. Grab a Clicker Calculator Scratch paper Equation sheet. Agenda. Review Ch. 6-9. Clicker Questions Chapter 6. What is the frequency of a wave which has a wavelength of 0.156 nm. 5.2 x 10 -10 1.92 x 10 9 0.468 x 10 8 1.92 x 10 -9. 0 of 30.

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Entry Task: Oct 22 nd Monday

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  1. Entry Task: Oct 22nd Monday Grab a Clicker Calculator Scratch paper Equation sheet

  2. Agenda • Review Ch. 6-9

  3. Clicker QuestionsChapter 6

  4. What is the frequency of a wave which has a wavelength of 0.156 nm 5.2 x 10-10 1.92 x 109 0.468 x 108 1.92 x 10-9 0 of 30

  5. Which color of visible light has the least amount of energy per photon? Violet Blue Yellow Red 0 of 30

  6. As the principal energy level increases in an atom's orbitals, the average distance of an electron energy level from the nucleus ______________. Increases Decreases stays the same varies 0 of 30

  7. The probability map for an electron is called An orbit Electron configuration orbital Electron map 0 of 30

  8. A given set of f orbitals consists of ______________ orbital(s). 3 5 7 9 0 of 30

  9. The maximum number of electrons allowed in each of the d orbitals is 2 4 8 18 0 of 30

  10. The maximum number of electrons allowed in the p sublevel of the third principal level is 2 6 8 18 0 of 30

  11. Phosphorus has how many electrons in its outermost principal energy level? 2 3 5 15 0 of 30

  12. The electron configuration for the sulfur atom is 1s22s22p63s23p2 1s22s22p63s23p4 1s22s22p63s5 1s22s22p63s23p5 0 of 30

  13. How many electrons are in the third principal energy level (n = 3) of one atom of Fe? 2 8 14 18 0 of 30

  14. Clicker QuestionsChapter 7

  15. The first Periodic Table was created by Amadeo Avogadro. Dmitri Mendeleev. Henry Moseley. Ernest Rutherford. 0 of 30

  16. The effective nuclear charge felt by an atom’s valence electrons (X) going from left to right and (Y) going down a column on the Periodic Table. X = increases Y = increases X = increases Y = decreases X = decreases Y = increases X = decreases Y = decreases 0 of 30

  17. The correct order of increasing atomic radius (smallest  largest) is Na < Mg < K < Rb. Mg < Na < K < Rb. Rb < K < Na < Mg. Rb< K < Mg < Na. 0 of 30

  18. The statements below refer to ionic radii. Which statement is FALSE? Br1– is larger than Cl1–. Se2– is larger than Br1–. K1+ is larger than Ca2+. Na1+ is larger than K1+. 0 of 30

  19. Two ions are isoelectronic if they have the same charge. number of protons. number of electrons. number of neutrons. 0 of 30

  20. The minimum energy needed to remove an electron from an atom in its ground state is called the atom’s potential energy. activation energy. electron affinity. ionization energy. 0 of 30

  21. The energy change that occurs when an electron is added to an atom is called the atom’s potential energy. activation energy. electron affinity. ionization energy. 0 of 30

  22. The correct order of increasing first ionization energy (smallest  largest) is Na < Ca < Al < Sn. Na < Al < Ca < Sn. Na < Al < Sn < Ca. Ca < Na < Sn < Al. 0 of 30

  23. The correct order of increasing electron affinity (most negative  least negative) is O < Cl < B < C. O < Cl < C < B. Cl < O < C < B. Cl< O < B < C. 0 of 30

  24. Most metal oxides form _______ solutions when dissolved in water. acidic basic neutral amphoteric 0 of 30

  25. Most nonmetal oxides form _______ solutions when dissolved in water. acidic basic neutral amphoteric 0 of 30

  26. A soft gray solid reacts with water to form a flammable gas and a basic solution. The solid is most likely to be a noble gas. halogen. group IIA metal. transition metal. 0 of 30

  27. Ozone is an allotrope of which element? hydrogen oxygen sulfur chlorine 0 of 30

  28. Unknown solid X turns a Bunsen burner flame green and produces a purple color on reaction with NaOCl. X is BaI2. BaBr2. SrI2. d. SrBr2. 0 of 30

  29. The noble gases are monatomic. have filled s and p subshells. are generally unreactive. d. All of the above. 0 of 30

  30. Clicker QuestionsChapter 8

  31. The two types of chemical bonds commonly found in compounds are doric and covalent. ionic and electrolytic. ionic and covalent. electrolytic and compound. 0 of 30

  32. The Lewis symbol for a sulfur atom includes how many dots? 5 6 7 8 0 of 30

  33. The octet rule states that atoms tend to gain, lose, or share electrons until they have _______ valence electrons. 5 6 7 8 0 of 30

  34. Which compound below has the largest lattice energy? NaCl KBr CaO CsI 0 of 30

  35. When a transition metal atom forms a +1 ion, it loses an electron from what type of orbital? s p d f 0 of 30

  36. Which choice below correctly lists the elements in order of increasing electronegativity (least  most) ? C < N < O < F N < C < O < F N < C < F < O C < N < F < O 0 of 30

  37. Which choice below correctly lists the elements in order of increasing electronegativity (least  most) ? F < Cl < Br < I F < Cl < I < Br I < Cl < Br < F I < Br < Cl < F 0 of 30

  38. The carbon disulfide (CS2) molecule has two single bonds. two double bonds. a single bond and a double bond. a single bond and a triple bond. 0 of 30

  39. The hydrogen cyanide (HCN) molecule has two single bonds. two double bonds. a single bond and a double bond. a single bond and a triple bond. 0 of 30

  40. The formal charge on the nitrogen atom in the nitrate ion (NO31–) is +2 +1 0 –1 0 of 30

  41. The formate ion (HCO21–) is stabilized by resonance, which suggests that the oxygen atoms’ formal charges are: –1 and –1 0 and 0 –1 and 0 –1/2 and –1/2 0 of 30

  42. Which molecule below violates the octet rule? PF5 CH4 NBr3 OF2 0 of 30

  43. Which molecule below has an unpaired electron? NO NH3 BF3 PF5 0 of 30

  44. For atoms X and Y, the bond enthalpy of an X-Y bond is _______ the bond enthalpy of an X=Y bond. greater than less than equal to variable, depending on X and Y 0 of 30

  45. For atoms X and Y, the bond length of an X-Y bond is _______ the bond length of an X=Y bond. greater than less than equal to variable, depending on X and Y 0 of 30

  46. Clicker QuestionsChapter 9

  47. The overall shape of a molecule is determined by its atoms. bond angles. Symmetry. electron affinity. 0 of 30

  48. If a central atom is surrounded by six electron domains, the term used to describe its fundamental geometry is square planar. octahedral. square pyramidal. tetrahedral. 0 of 30

  49. The geometry of the methane (CH4) molecule is linear. trigonalbipyramidal. trigonal planar. tetrahedral. 0 of 30

  50. The geometry of the phosphorus trichloride (PCl3) molecule is tetrahedral. trigonal planar. pyramidal. trigonalbipyramidal. 0 of 30

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