Name____________________________________________________________period_____AP chemistry Unit 2 worksheet Concepts to know: Read Chapters 6, 7, 2.6, 8.3 The wave nature of light Quantized energy and photons Bohr’s model of the atom The quantum model of the atom (this is the accepted model and PES is the proof) Effective nuclear charge Electron configuration Sizes of atoms Ionization energy Electronegativity Ions and ionic compounds Practice problems 1. What are the SI units for a. Wavelength of light b. frequency of light c. speed of light -1 Meter hertz (s ) m s-1 (m/s) 2. T/F (correct the statement if it is false) a. Visible light is a form of electromagnetic radiation. True b. The frequency of radiation increases as the wavelength increases. False, the frequency decreases as wavelength increases c. Ultraviolet light has a shorter wavelength than visible light. True d. Electromagnetic radiation and sound waves travel at the same speed. False, electromagnetic radiation travels at the speed of light 3. What is the wavelength of radiation that has a frequency for 5.11 x 1011 s-1? Would this be visible to the human eye? 5.87 x 10-4 m; no 4. Exited mercury atoms emit light at 489 nm. What is the frequency of this radiation? Predict the color associated with it. 6.12 x 1014 s-1; blue 5. Calculate the smallest increment of energy that can be emitted or absorbed at a wavelength of 812 nm. 2.45 x 10-19 J 6. The most prominent line in the spectrum of neon is found at 865.438 nm. Other lines are found at 837.761 nm, 878.062 nm, 878.438 nm, and 1885.387 nm. Which of these lines represents the most energetic light? at 865.438 nm 7. Is energy emitted or absorbed when the following electronic transitions occur in hydrogen? a. From n=4 to n=2 Emitted b. From an orbit of radius 2.12 A� to one of radius 8.48 A� . Absorbed 8. In the Bohr model of the hydrogen atom, when the electron is in its ground state, it orbits the nucleus at a specific radius of 0.53A� . In the quantum mechanical description of the hydrogen atom, the most probable distance of the electron from the nucleus is 0.53 A� . Why are these statements different? The Bohr (shell model) states with 100% certainty that the electron in hydrogen can be found at 0.53 A from the nucleus. The quantum model is a statistical model that states the probability of finding the electron in certain regions around the nucleus. While 0.53 A is the radius with the highest probability, that probability is less than 100%. 9. What are the similarities and differences between the hydrogen 1s and 2s orbitals? Same spherical shape, but 2s has a larger radial extension than the 1s 10. List in order of increasing energy: 4f, 6s, 3d,1s,2p 1s, 2p, 6s, 4f 11. Explain why the effective nuclear charge experienced by a 2s electron in boron is greater than that for the 2p electron. The 2p electron in boron is shielded from the full charge of the nucleus by the 2s electrons, so the 2p electron experiences a smaller effective nuclear charge 12. Explain why the effective nuclear charge experienced by a 2s electron in aluminum is greater than that for the 2s electron experienced by boron. Aluminum has more protons than boron so the 2s electron will experience a greater effective nuclear charge 13. Which should experience the greater nuclear charge, a 2p electron in oxygen or a 2p electron in neon? A 2p electron in neon experiences a greater effective nuclear charge 14. How many f orbitals have n=3? 0 15. Two electrons in an atom both occupy the 1s orbital. What quantity must be different for the two electrons? They must have opposite spins 16. How many unpaired electrons are there in an atom of tin in its ground state? 2 17. Of the following elements, which one is most likely to form an ion through the loss of two electrons? a. strontium b. sulfur c. sodium d. chlorine e. aluminum 18. An atom has two electrons with principal quantum number (n) = 1, eight electrons with principal quantum number (n) = 2 and seven electrons with principal quantum number (n) = 3. From this data, supply the following values (if insufficient information is given, say so). (a) The mass number. __not enough info_______ (b) The atomic number. ___17______ (c) The electron configuration. _1s22s22p63s23p5______ 19. What is the maximum number of electrons that can occupy each of the following a. 3d 10 b. 4s 2 c. 2nd shell 8 e. 2p 6 f. 5f 14 g. One 2p orbital 2 d. n=3 18 h. n= 4 32 20. Write the orbital notation (can use noble gas) for each of the following a. Sc b. Si ↑↓ [Ar] 4s c. Sn ↑↓ [Kr] 5s ↑ __ __ __ __ 3d ↑↓ ↑↓ ↑↓ ↑↓ ↑↓ 4d ↑↓ [Ne] 3s d. Mn ↑ ↑ __ 5p [Ar] 21. Write the noble gas configuration for the following a. Rb b. Se 1 [Kr]5s [Ar]4s23d104p4 d. Pb e. Mn 2 10 14 2 [Xe]6s 5d 4f 6p [Ar]4s23d5 ↑_ __↑ ____ 3p ↑↓ 4s ↑_ ↑_ ↑_ ↑_ ↑_ 3d c. Zn [Ar]4s23d10 f. N [He]2s22p3 22. Write the full electronic configuration for argon 1s22s22p63s23p6 23. Identify the element from the electron configurations of atoms shown below. (3) 2 2 (a) [Ne] 3s 3p ___Si______ 2 7 (b) [Ar] 4s 3d ___Co______ 2 (c) [Xe] 6s _____Ba____ 24. H, He, Li, B, Ne, Na a. For each atom, tell how many peaks we will see in PES 1,1,2,3,3,4 b. Tell what peaks go with what orbitals. (See in class) c. Draw what a PES would look like for each atom. (See in class) 25. Which will be closer to the nucleus, the n=3 electron shell in Ar or the n=3 shell in Kr? Kr 26. Arrange the following atoms in order of increasing atomic radius: F, P, S, As and explain why. F, S, P, As (atoms get bigger when a shell is added or less protons in the same number of shells) 27. Arrange the following atoms in order of increasing atomic radius: Al, Nb, Se, F, Mn and explain why. F, Al, Se,Mn, Nb, (atoms get bigger when a shell is added or less protons in the same number of shells) 28. An element having the configuration [Xe]6s1 belongs to the group: a. alkaline earth metals b. alkali metals c. halogens d. noble gases e. none of these 29. What is the trend in the first ionization energy as one proceeds down group 1? Explain how this relates to size of the atoms. It decreases, the atoms have more shells as you go down a group so they have a larger radius and the nucleus does not hold on to them as well. 30. Arrange the following pure solid elements in order of increasing electrical conductivity: P, Ag, and Sb P, Sb, Ag 31. Explain in terms of electron configurations, why hydrogen exhibits properties similar to both lithium and fluorine It has one valence electron like lithium, but only needs one valence electron to have a full shell like fluorine 32. Which of the following statements are true a. All are false b. the first ionization energy of fluorine is greater than the first ionization energy of oxygen c. as the atomic number increases within a group of the main group elements, the tendency is for first ionization energy to increase d. it is easier to remove an electron from Na+ than from Na. e. all particles with the electron configuration [Ar]4s2 have the same ionization energy. 33. Consider the element Scandium, atomic # 21. (a) If the electronic configuration of the element were constructed "from scratch", into which orbital (and into which shell) would the final electron be placed? 3d (b) When scandium forms an ion with a charge of +1, from which orbital (and from which shell) would the electron be removed? 4s 34. Based on their position on the periodic table, predict which atom of the following pairs will have the largest first ionization energies. In each case explain with electron configuration and effective nuclear charge a. O, Ne b. Mg, Sr c. K, Cr d. Br, Sb e. Ga, Ge Ne Mg Cr Br Ge Smaller atoms have a harder time losing their electrons because the valence electrons feel a greater effective nuclear charge so it takes more energy to remove the electron. 35. For each pair, which element will have greater metallic character a. Li or Be b. Li or Na c. Sn or P 36. Predict whether each of the following oxides is ionic or molecular: SO2, MgO, Li2O, N2O, XeO3 Molecular, ionic, ionic, molecular, molecular 37. Identify two positive and two negative ions that are isoelectronic with argon. (4) + 2+____ (a) Two Positive ions _K _______ ____Ca -_____ 2-______ __S (b) Two Negative ions ___Cl 38. Compare the elements sodium and magnesium with respect to the following properties a. Electron configuration 1s22s22p63s1; 1s22s22p63s2 b. Most common ionic charge+1; +2 c. First ionization energy magnesium has a higher first ionization energy d. Atomic radius magnesium is smaller than sodium 39. Compare the elements fluorine and chlorine with respect to the following properties a. Electron configuration b. Most common ionic charge c. Atomic radius 2 2 5 2 2 6 2 5 1s 2s 2p ; 1s 2s 2p 3s 3p -1;-1 Chlorine is larger than fluorine 40. Why are monatomic cations smaller than their corresponding neutral atom? Lost one electron so the remaining electrons have less repulsion and a greater effective nuclear charge 41. Write the noble gas configuration a. Fe3+ b. Ni2+ [Ar]3d5 [Ar]3d8 42. Which neutral atom is isoelectric with each of the following a. Clb. Se2c. Mg2+ Ar Kr Ne 43. Arrange the atoms and ions in each of the following sets in order of increasing size a. Br-, Na+, Mg2+ b. Ar, Cl-, S2-, K+ 44. 45. 46. 47. 48. 49. 50. Mg, Na, Br K, Ar, Cl, S What is a covalent bond? A bond that forms when atoms share electrons What is an ionic bond? A bond that forms when atoms give and take electrons What is a metallic bond? A bond that forms when nuclei are attracted to a “sea of electrons” Why can metals conduct electricity? There are electrons moving around Using the periodic table, select the most electronegative atom in each of the following sets a. B, Be, C, Si b. Zn, Ga, Ge, As c. Na, Mg, K, Ca C As Mg Label each of the following as ionic, metallic, or covalent a. NaOH b. N2O c. KCl d. HF e. O2 f. Al foil ionic covalent ionic covalent covalent metallic Which of the following forms molecules? a. K2CO3 b. F2 c. BaCl2 d. H2O e. Fe2O3 51. How many protons, neutrons, and electrons are in the following a. 65Zn2+ b. 40Ar c. 14N3d. 23Na+ 30,35,28 18,22,18 7,7,10 11,12,10 52. Which ions are cations in the previous problem, which are anions? A,d 53. How is bonding in Cl2 different than NaCl? In Cl2, electrons are being shared, and in NaCl sodium gives an electron to chlorine 54. Which of the following species contain more electrons than neutrons? a. 2H b. 11B c. 16O2d. 19F55. How many valence electrons does each of the following atoms have? a. C b. Ca c. H d. Pb e. Ar 4 2 1 4 8 56. What is the most common charge when each become ions a. Mg b. O c. Al d. P e. K +2 -2 +3 -3 +1 57. The ionization energies for an element are listed below First second third fourth 8 eV 15eV 80eV 109eV f. Cl 7 f. Br -1 fifth 141 eV Based on the ionization energies, the element is most likely to be a. Sodium b. magnesium c. aluminum d. silicon e. phosphorus Practice MQ and FRQ 58. Which of the following contains only atoms that are diamagnetic in their ground state? a. Kr, Ca, and P b. Ne, Be, and Zn c. Ar, K, and Ba d. He, Sr, and C 59. How many protons, neutrons, and electrons are in an Protons Neutrons Electrons a. 26 30 26 b. 26 56 26 c. 56 26 26 d. 56 82 56 56 26Fe atom? 60. Which of the following is the electron configuration of an excited atom that is likely to emit a quantum of energy? 2 2 6 2 1 2 2 6 2 5 (B) 1s 2s 2p 3s 3p (A) 1s 2s 2p 3s 3p 2 2 6 2 2 2 6 1 1 (C) 1s 2s 2p 3s (D) 1s 2s 2p 3s 3p -1 61. The bond energy of fluorine in 159 kJ mol . -19 i. Determine the energy, in J, of a photon of light needed to break an F-F bond. 2.64 x 10 J -1 14 -1 3.98 x 10 s ii. Determine the frequency of this photon in s iii. Determine the wavelength of this photon in nanometers 750 nm b. Barium imparts a characteristic green color to a flame. The wavelength of this light is 551 nm. Determine the energy involved in kJ/mol 220 kJ/mol Review 62. How many significant figures are in each of the following? a.0.030100 kJ b. 6.022 x 1023 atoms c. 100 d. 1001 5 4 1 4 63. Calculate the following to the correct number of significant figures. a.1.27g/5.296cm3 b. 12.2mL + 0.38mL c. 7.355g - 2.785g d. 0.1 m x 3.21m 0.240 g/mL 12.6 mL 4.570 g 0.3 m2 3 64. The density of pure silver is 10.5 g/cm . If 5.25 g of pure silver pellets are added to a graduated cylinder containing 11.2 mL of water, to what level will the water in the cylinder rise? 11.7 mL 65. Let’s pretend you are holding two atoms of carbon that are isotopes. Describe what the two atoms have in common and what they have different. They have the same number of protons, but one would have more mass than the other one. 66. What is the mass, in grams, of 1.75 x 1020 molecules of caffeine, C8H10N4O2? 0.0563 g 67. Determine the empirical formula of the compound with the following compositions by mass 10.4 percent C, 27.8 percent S, and 61.7 percent Cl CSCl2
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