Name Date Period Answer Key change font to white CHAPTER 4/5 THE PERIODIC TABLE/ELECTRON CONFIGURATIONS: WARM-UP

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1 Name Date Period Answer Key change font to white CHAPTER 4/5 THE PERIODIC TABLE/ELECTRON CONFIGURATIONS: WARM-UP 1. What is the periodic law? (These questions are from Chapter 5 The Periodic Table) When elements are arranged in order of increasing atomic #, their physical and chemical properties show a periodic pattern. 2. What is a group, or family of the periodic table? The vertical columns are called groups of the periodic table 3. What is a period of the periodic table? The horizontal rows are called periods 4. Give the names of at least four families, or groups of the periodic table. Alkali metals, alkaline earth metals, halogens, and the Noble Gases. 5. There are three types of elements on the periodic table, fill in the table below for each Name Properties Location on the periodic table a. Metals Shiny, good conductors, typically room temp, left of the staircase line malleable & ductile b. Non-metals not shiny, most are poor conductors, not malleable or Right of the staircase ductile, many are gases. c. Semi-metals or metalloids Have some properties of metals and some properties of non-metals or properties in between. Touching The Staircase 6. Where are the transition metals on the Periodic Table? Middle section (the d-block) 7. Where are the post-transition metals on the Periodic Table? Under the stair case 8. There are three states that the elements can exist in, list all three. State How can you tell what state they are in on the periodic table? a. Solid They are black on the periodic table b. Liquid They are blue on the periodic table c. Gas They are red on the periodic table. 9. Describe the general differences between elements on the left side of the periodic table and those on the right. The right side contains non-metals, while the left side contains metals. 10. In the rest of this chapter, 3 periodic trends will be discussed. They are listed below. Define them and explain how they will be seen on the periodic table. Property Definition How the Trend is seen a. Atomic radius c. d. Ionization Energy (IE) Electronegativity (EN) distance from the center of the nucleus to the outermost electron energy needed to remove one of the electrons. an atoms ability to attract electrons in a chemical bond 11. Why do elements within a group have similar properties? They have the same # of valence electrons. As you go down, the atoms get bigger, as you go left to right the atoms get smaller. As you go down I.E. decreases, increases as you move left to right. Increases as you move from the bottom to the top, and increases as you move left to right. 12. What are valence electrons? Electrons in the outermost energy level 13. What is the trend in valence electrons across the Periodic Table? 1,2,3,4,5,6,7,8 Last Updated: 10/12/11 Page 1/12

2 14. The technical definition of the octet rule is atoms tend to gain/lose or share electrons in order to acquire a full set of valence electrons. a. What does oct- mean? eight b. What are valence electrons? the electrons in the outermost energy level c. What does a full set of valence electrons mean for most atoms? 8 electrons in the outermost enery level d. Write a definition of the octet rule in your own words. elements try to get 8 outermost electrons by gaining, losing, or sharing electrons e. Would it be OK to call it the noble gas rule instead of the octet rule. EXPLAIN. Yes, everyones electrons end up looking like a noble gas. 15. What does it mean when an atom has become an ion? It has gained or lost electrons 16. Explain the difference between Na which explodes when put in water and Na + which we eat everyday. Na is a sodium atom which has not given away it s electrons yet. Na + has already given away it s electrons and is therefore much more stable and less dangerous. 17. Explain the trend across the Periodic Table in the typical charges of the ions. 1,2 3,4,5,6,7,8 18. Define atomic radius. Atomic radius is the distance from the center of atom s nucleus to its outermost electron. 19. Why do atoms get smaller as you move across a period of the periodic table? The increasing positive charge on the nucleus exerts a stronger pull on the electrons, shrinking their orbitals and making the atom smaller. Contrast ionization energy and electronegativity. In general, what can you say about these values for metals and 20. nonmetals? In general what can you say about the types of ions they form? Ionization energy is the energy needed to remove an electron from an atom. Electronegativity is an atoms ability to attract electrons in a chemical bond. In general, metals have both lower ionization energies and electronegativities than nonmetals. Therefore, metals tend to form positive ions while nonmetals tend to form negative ions. 21. Explain why noble gases are inert (do not react) and do not form ions. Noble gases have a full set of valence electrons and do not need to gain or lose electrons to acquire and octet 22. Define the term electronegativity. What is the periodic trend for electronegativity? Electronegativity is a measure of an atom s ability to attract electrons in a chemical bond. Electronegativity increases as you move from left to right across a period and decreases as you move down a group. 23. What information is presented in each square of the periodic table? The elements name and symbol. The atomic #. The atomic mass. Whether the element is a liquid or a solid. 24. A chemistry experiment calls for a compound that supplies ions of bromine, but unfortunately this compound is not available. Pacey substitutes a compound that supplies ions of chlorine. Dawson uses a compound that contains selenium. From what you know about the periodic table, predict whether Dawson or Pacey will run a more successful experiment. Pacey s experiment will be more successful because bromine and chlorine are in the same family (Halogens). Selenium, although next to bromine probably does not have properties that are as similar as chlorine. Last Updated: 10/12/11 Page 2/12

3 DETERMINING HOW THE TRENDS FOLLOW THE PERIODIC TABLE (TAKE NOTES) 25. Atomic Radius (size of the atom) The 1 st criterion is: Up Down The 2 nd criterion is: Left Right st Ionization Energy (IE) The 1 st criterion is: Up Down The 2 nd criterion is: Left Right 27. Electronegativity (EN) fluorine is the most electronegative element on the periodic table. The 1 st criterion is: Up Down The 2 nd criterion is: Left Right 28. For all 3 trends above (size, IE, EN), what causes a more significant change, going across a period or down a group? WHY? Up Down because change by entire energy level of e-, not just be 1 e- Last Updated: 10/12/11 Page 3/12

4 SECTION 5-3 PROBLEMS Complete the table. Column 1 and 2 tell the number or protons and electrons in the atom/ion. Column 3 write the elements state (sol, liq, or gas). Column 4 write the type of element (metal, semi-, or non-metal). Column 5 write number of electron shells each atom has. Column 6, 7, & 8 rank each group as LO for smallest/lowest, HI for biggest/largest, & MID for in between. Column 9 write the symbol of most common ion Element Protons Electrons State Type # of e- Shells Atomic Radius Ionization Energy EN # of valence e- Common Ion Chlorine Gas Non 3 LO HI HI 7 Cl - (-1) Selenium Solid Non 4 HI LO LO 6 Se -2 (-2) Bromine Liquid Non 4 MID MID MID 7 Br - (-1) Phosphorus Solid Non 3 MID MID MID 5 P -3 (-3) Sulfur Solid Non 3 LO HI HI 6 S -2 (-2) Selenium Solid Non 4 HI LO LO 6 Se -2 (-2) Scandium Solid Metal 4 LO HI HI 2 Sc +2 (+2) Yttrium Solid Metal 5 MID MID MID 2 Y +2 (+2) Lutetium Solid Metal 6 HI LO LO 2 Lu +2 (+2) Vanadium Solid Metal 4 MID MID MID 2 V +2 (+2) Chromium Solid Metal 4 LO HI HI 2 Cr +2 (+2) Tungsten Solid Metal 6 HI LO LO 2 W +2 (+2) Nitrogen 7 7 Gas Non 2 LO HI HI 5 N -3 (-3) Phosphorus Solid Non 3 MID MID MID 5 P -3 (-3) Arsenic Solid Semi 4 HI LO LO 5 As -3 (-3) K Solid Metal 4 1 K+1 K Rb Solid Metal 5 1 Rb+1 Cl Gas Non 3 7 Cl-1 Cl Br Liquid Non 4 7 Br-1 Li 3 3 Solid Metal 2 1 Li+1 Li Na Solid Metal 3 1 Na+1 Te I Xe Gas Non 5 8 Aluminum Solid Metal 3 LO LO 3 Al +3 (+3) Silicon Solid Semi 3 MID MID 4 Si +4 (+4) Phosphorus Solid Non 3 HIGH HI 5 P -3 (-3) Last Updated: 10/12/11 Page 4/12

5 Which atom in each pair has the larger atomic radius? 39. Li or K 40. O or C 41. Si or S K C Si 42. Ca or Ni 43. Cl or Br 44. Fe or Au Ca Br Au 45. Ga or B 46. Be or Ba Ga Ba Which atom in each pair has the larger ionization energy? 47. Na or O 48. Cu or Ra 49. Ca or Fr O Cu Ca 50. Be or Ba 51. I or Ne 52. W or Se Be Ne Se 53. Ar or F 54. K or V Ar V Which atom in each pair has the smaller electronegativity? 55. Na or O 56. Cu or Ra 57. Ca or Fr Na Ra Fr 58. B or Be 59. Fe or Rh 60. C or Ge Be Rh Ge 61. N or S 62. Ca or Na S Ca Write the charge that each of the following atoms will acquire when it has a complete set of valence electrons. 63. O 64. F 65. Ca O -2 (-2) F - (-1) Ca +2 (+2) 66. Na 67. N 68. Ar Na + (+1) N -3 (-3) No Charge Last Updated: 10/12/11 Page 5/12

6 CHAPTER 4 LIGHT & ELECTRON CONFIGURATIONS 69. Quickly sketch the electromagnetic spectrum and label the general areas. Below the spectrum indicate whether the energy is increasing or decreasing left to right. (These Questions are now from Chapter 4 Electron Configurations) Gamma Rays X-rays UV Visible Infrared Microwaves TV Radio ENERGY IS DECREASING What is the photoelectric effect? Einstein took different colored lights and shone them on two charged plates that were about to spark, he found that red light would not make them spark, but blue light would. (Do the phosphorescent screen.) 71. What did Einstein call these particles that make up light? Photons 72. What is a (bright) line spectrum? When certain elements are excited and the light the emit is passed through a prism, only certain frequencies of light(colors) are visible. 73. How can you get a (bright) line spectrum? By exciting gas samples of pure elements. 74. Sketch a quick model of the atom. 75. Draw a sketch of an atom showing what happens when an electron gets excited. 76. What must have happened for the electron in the sketch above to have gotten excited? Energy in, either heat or electricity 77. Draw a sketch of an atom showing what happens when an electron returns from an excited state to a lower energy state. 78. What happens when that electron falls to the lower energy state in the sketch above? light emitted 79. If the electron falls further in energy, what will be different? bluer light 80. What is the difference between the ground state and the excited state? Last Updated: 10/12/11 Electron Configurations: Page 6/12

7 The ground state is when all the electrons in an atom are in the lowest possible orbital, the excited state is when one or more of the electrons have jumped to a higher energy level. 81. In your own words describe Heisenberg s Uncertainty Principle. You can t know where an electron is and where it is headed at the same time. Knowing one changes the other. 82. Bohr s model is the 4 th model of the atom, what is the name of the currently accepted model? Quantum mechanical model (electron cloud model) 83. What are the letters associated with the 4 different shapes? s, p, d, f 84. Quickly sketch the general shape of an s, p and a d orbital. 85. Every principal energy level (n) can be divided into how many sublevels? The 1 st principal energy level (n=1) can be divided into one sublevel (s). The 2 nd (n=2) can be divided into 2(s, p). The 3 rd can be divided into 3(s, p, d). The 4 th can be divided into 4(s, p, d, f) Fill in the following chart Quantum Numbers and Number of Electrons Electron Shells, Sublevels, & Orbitals Electron Shell or Principal Quantum Number (n) Number of Sublevels (shapes) Name of Sublevels Max Number of electrons in each sublevel Maximum # Electrons possible in the n th shell 1 1 1s 2 2 2s p 6 3s p 6 3d 10 4s 2 4p 6 4d 10 4f Last Updated: 10/12/11 Electron Configurations: Page 7/12

8 SPECTROSCOPIC IDENTIFICATION Decreasing energy You work in a factory and your boss is mad that some chemicals have been mixed together. Being the bright chemistry student (and employee) that you are, you remember hearing that every element gives of its own unique bright line specta, which is almost like a fingerprint on a human, no two elements have the same one. So you take your Stevie Wonder glasses, then take the mixture and vaporize it in a flame. Above is the bright line spectrum that you see. So you grab a chemical reference and look up a bunch of spectra (shown on the back). Can you tell me what elements have been mixed The chemicals are argon and sodium Decreasing energy Decreasing energy Last Updated: 10/12/11 Electron Configurations: Page 8/12

9 SECTION 4-5 TABLE #1 Fill in the following table: Element Electron Configuration Noble Gas Configuration Last e - Configuration 86. Potassium 1s 2 2s 2 2p 6 3s 2 3p 6 4s 1 [Ar]4s 1 4s Cobalt 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 7 [Ar]4s 2 3d 7 3d Nitrogen 1s 2 2s 2 2p 3 [He]2s 2 2p 3 2p Silicon 1s 2 2s 2 2p 6 3s 2 3p 2 [Ne]3s 2 3p 2 3p Lithium 1s 2 2s 1 [He]2s 1 2s Phosphorus 1s 2 2s 2 2p 6 3s 2 3p 3 [Ne]3s 2 3p 3 3p Iridium 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 5s 2 4d 10 5p 6 6s 2 4f 14 5d 7 [Xe]6s 2 4f 14 5d 7 5d Selenium 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 4 [Ar]4s 2 3d 10 4p 4 4p Scandium 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 1 [Ar]4s 2 3d 1 3d Bismuth 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 5s 2 4d 10 5p 6 6s 2 4f 14 5d 10 6p 3 [Xe]6s 2 4f 14 5d 10 6p 3 6p Vanadium 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 3 [Ar]4s 2 3d 3 3d Cadmium 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 5s 2 4d 10 [Kr]5s 2 4d 10 4d Sulfur 1s 2 2s 2 2p 6 3s 2 3p 4 [Ne]3s 2 3p 4 3p Mercury 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 5s 2 4d 10 5p 6 6s 2 4f 14 5d 10 [Xe]6s 2 4f 14 5d 10 5d Osmium 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 5s 2 4d 10 5p 6 6s 2 4f 14 5d 6 [Xe]6s 2 4f 14 5d 6 5d 6 2 # of Valence Electrons Last Updated: 10/12/11 Electron Configurations: Page 9/12

10 Element Noble gas notation # Valence electrons Most common ion Group Name 101. N [He]2s 2 2p 3 5 N S [Ne]3s 2 3p 4 6 S Ti [Ar] 4s 2 3d 2 2 Ti Na + [He] 2s 2 2p Sr [Kr] 5s 2 2 Sr Tc [Kr] 5s 2 4d 5 2 Tc Fr + [Rn] W [Xe] 6s 2 4f 14 5d 4 2 W K + [Ne]3s 2 3p Co [Ar] 4s 2 3d 7 2 Co Ge [Ar] 4s 2 3d 10 4p or Cl - [Ne]3s 2 3p Br [Ar] 4s 2 3d 10 4p 5 7 Br In [Kr] 5s 2 4d 10 5p 1 3 In Pb [Xe] 6s 2 4f 14 5d 10 6p or Xe [Kr] 5s 2 4d 10 5p 6 8 Xe or No Ion formed Last Updated: 10/12/11 Electron Configurations: Page 10/12

11 117. TABLE #2 Fill in the following table Element Noble Gas Configuration Last e - # Valence e - N -3 (Nitride) [He]2s 2 2p K + [Ar] or [Ne]3s 2 3p 6 3p S -2 (Sulfide) [Ne] 3s 2 3p 2 3p Co +2 [Ar]3d 7 3d Ti [Ar]4s 2 3d 2 3d Ge [Ar]4s 2 3d 10 4p 2 4p Na + [Ne] or [He]2s 2 2p 6 2p Cl - (Chloride) [Ar] or [Ne]3s 2 3p 6 3p Sr [Kr]5s 2 5s Se -2 (Selenide) [Ar]4s 2 3d 10 4p 2 4p Tc [Kr]5s 2 4d 5 4d In [Kr]5s 2 4d 10 5p 1 5p Fr +1 [Rn] 7s Pb [Xe]6s 2 4f 14 5d 10 6p 2 6p W +4 [Xe]4f 14 5d 2 5d 4 2 Last Updated: 10/12/11 Electron Configurations: Page 11/12

12 Ch 4 Electron Configurations Radiant Energy Waves (Amplitude, Frequency, Wavelength, Speed of Light) Visible Sectrum Quantum Theory (Quantum, Planck s constant, photoelectrics effect, photons) Line Spectra, energy level numbers (1st quantum number), ground versus excited states, Uncertainty Principle Quantum Mechanical Model, electron density, orbitals, principle energy level, sublevels Electron Configurations Orbital Diagrams Ch 5 The Periodic Table Periodic Law Groups/Families, Periods Alkali metals, Alkaline Earth Metals, Halogens, Noble Gases Metals, Non-Metals, Semi-Metals Transition Metals & Post-Transition Metals Valence electrons Octet Rule (not in book until Chap 7) Abbreviated electron configurations Noble gas inner core electron configurations Periodic Trends Atomic Radius Ionic Radius Ionization Energy ElectronAffinity Electronegativity Valence e- Ion Charges Last Updated: 10/12/11 Electron Configurations: Page 12/12