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Name______________________ #_____ Period___ Honors Chemistry Ms. K Pages 96-131 Task Checklist: Look at Online Textbook Materials Look at Section 1 Visual Concepts Look at Section 2 Visual Concepts Look at Section 3 Visual Concepts Take Section 1 Self-Check Quiz Take Section 2 Self-Check Quiz Take Section 3 Self-Check Quiz Do the Protons and Neutrons Concept Map Other Tasks Read Section 1 Read Section 2 Read Section 3 Review Chapter Packet Examine Class Website Review PowerPoint Ms. K Chemistry Name_____________________________ #_____ Date______________________ Period_________ c = λν Worksheet E = hν c: speed of light λ: wavelength ν: frequency E: energy h: Planck’s constant 1. If you suspected something as being ?Wavelike?, how could you prove it? 2. What are two characteristics that differentiate types of electromagnetic radiation? 3. Name one characteristic that all electromagnetic radiation have in common? 4. What is the speed of yellow light? 5. What is the frequency of a radio wave with a wavelength of 10.0 m? 6. What is the energy of an X-ray with a frequency of 1.0 x 1017 Hz? 7. If the wavelength of yellow light is 570. nm, what is the frequency of yellow light in Hertz? 8. What is the energy of blue light with a wavelength of 500.nm? 9. I sometimes listen to classical music on 89.3FM. What is the wavelength of the radio ermine the frequency. See your notes.) waves for this station? (The ?Call? numbers and the ?Band? help det Ms. K Chemistry Name_____________________________ #_____ Date______________________ Period_________ 1s22s22p63s23p64s23d104p65s24d105p66s24f145d106p67s25f146d107p6 Write the ground state electron configuration for each of the following: 1. calcium 1. ______________________________________________________________ 2. lithium 2. ______________________________________________________________ 3. iron 3. ______________________________________________________________ 4. sodium 4. ______________________________________________________________ 5. oxygen 5. ______________________________________________________________ 6. iodine 6. ______________________________________________________________ 7. osmium 7. ______________________________________________________________ 8. radium 8. ______________________________________________________________ 9. fermium 9. ______________________________________________________________ 10. argon 10. _____________________________________________________________ 11. sulfide ion 11. _____________________________________________________________ 12. calcium ion 12. _____________________________________________________________ 13. chloride ion 13. _____________________________________________________________ 14. hydrogen ion 14. _____________________________________________________________ Do you notice something strange about 10-13? We call these ?isoelectronic??remember this term? If you don’t, can you figure out what it means by looking at 10-13? Name the neutral atom that corresponds to the following electron configurations: 15. 1s22s22p63s23p64s23d104p2 __________ 16. 1s22s22p63s23p64s23d104p65s24d105p66s24f145d106p2 __________ 17. 1s22s22p63s23p5 __________ 18. 1s22s22p5 __________ Ms. K Chemistry Name_____________________________ #_____ Date______________________ Period_________ 1. Write the electron configurations for three things that are isoelectronic and provide their symbols: 2. Write the most stable electron configurations for the following: a. Nb a. ______________________________________________________________ b. Mo b. ______________________________________________________________ c. Cd c. ______________________________________________________________ d. Ag d. ______________________________________________________________ e. Sc+3 e. ______________________________________________________________ +2 f. Mn f. ______________________________________________________________ 3. Write the noble-gas notation (short-hand) for the following: a. Ca a. ______________________________________________________________ b. Cu b. ______________________________________________________________ c. Cs c. ______________________________________________________________ d. Cl d. ______________________________________________________________ 4. valence electrons ? the electrons available to be lost, gained, or shared in the formation of chemical compounds These are also the electrons in the highest energy level. Example: Na: 1s22s22p63s1 Notice, the 3rd energy level is the highest occupied level, and it contains one electron, thus, sodium has 1 valence electron. Example: Se: 1s22s22p63s23p64s23d104p4 The 4th energy level is the highest occupied level, and it contains 2 electrons in the 4s and 4 electrons in the 4p, thus Se has 6 valence electrons. How many valence electrons are in the following atoms or ions? a. b. c. d. Li _____ C _____ Kr _____ I _____ e. f. g. h. Mg _____ Al _____ As _____ S _____ i. F- _____ j. Na+_____ Ms. K Chemistry Name_____________________________ #_____ Date______________________ Period_________ 1. Write the electron configurations for three things that are isoelectronic and provide their symbols: 2. Write the most stable electron configurations for the following: a. Nb a. ______________________________________________________________ b. Mo b. ______________________________________________________________ c. Cd c. ______________________________________________________________ d. Ag d. ______________________________________________________________ e. Sc+3 e. ______________________________________________________________ +2 f. Mn f. ______________________________________________________________ 3. Write the noble-gas notation (short-hand) for the following: a. Ca a. ______________________________________________________________ b. Cu b. ______________________________________________________________ c. Cs c. ______________________________________________________________ d. Cl d. ______________________________________________________________ 4. valence electrons ? the electrons available to be lost, gained, or shared in the formation of chemical compounds These are also the electrons in the highest energy level. Example: Na: 1s22s22p63s1 Notice, the 3rd energy level is the highest occupied level, and it contains one electron, thus, sodium has 1 valence electron. Example: Se: 1s22s22p63s23p64s23d104p4 The 4th energy level is the highest occupied level, and it contains 2 electrons in the 4s and 4 electrons in the 4p, thus Se has 6 valence electrons. How many valence electrons are in the following atoms or ions? a. b. c. d. Li _____ C _____ Kr _____ I _____ e. f. g. h. Mg _____ Al _____ As _____ S _____ i. F- _____ j. Na+_____ Ms. K Chemistry Name_____________________________ #_____ Date______________________ Period_________ Niels Bohr Worksheet Light and Energy Levels of the Atom The quantum level occupied by an electron in an atom depends on the energy of the electron. Changes in quantum level are related to absorption or emission of energy. The figure below represents the four lowest energy levels of an atom. (n = 1 to 4). The six lettered arrows represent changes in the energy level of an electron. 4 3 2 C D E F 1 A B "And anyone who thinks they can talk about quantum theory without feeling dizzy hasn't yet understood the first thing about it." – Niels Bohr 1. Why do these energy levels mean that the atom will show an emission spectrum of discrete lines rather than a continuous spectrum of emitted light? ________________________________________ __________________________________________________________________________________ __________________________________________________________________________________ __________________________________________________________________________________ 2. Which three of the lettered energy changes involve absorption of energy by the atom? __________ 3. Which three of the lettered energy changes involve emission of light energy by the atom? _______ 4. Of the three energy changes that involve emission , one results in the emission of blue light, one results in yellow light, and one results in ultraviolet light. a. Which lettered change involves the emission of blue light? _____ b. Which lettered change involves the emission of yellow light? _____ c. Which lettered change involves the emission of ultraviolet light? _____ Name Date Class CHAPTER 4 REVIEW Arrangement of Electrons in Atoms SECTION 1 SHORT ANSWER Answer the following questions in the space provided. 1. In what way does the photoelectric effect support the particle theory of light? 2. What is the difference between the ground state and the excited state of an atom? 3. Under what circumstances can an atom emit a photon? 4. How can the energy levels of the atom be determined by measuring the light emitted from an atom? 5. Why does electromagnetic radiation in the ultraviolet region represent a larger energy transition than does radiation in the infrared region? MODERN CHEMISTRY Copyright © by Holt, Rinehart and Winston. All rights reserved. ARRANGEMENT OF ELECTRONS IN ATOMS 25 Name Date Class SECTION 1 continued 6. Which of the waves shown below has the higher frequency? (The scale is the same for each drawing.) Explain your answer. Wavelength Wavelength Wave A Wave B 7. How many different photons of radiation were emitted from excited helium atoms to form the spectrum shown below? Explain your answer. Spectrum for helium PROBLEMS provided. Write the answer on the line to the left. Show all your work in the space 8. What is the frequency of light that has a wavelength of 310 nm? 9. What is the wavelength of electromagnetic radiation if its frequency is 3.2 102 Hz? 26 ARRANGEMENT OF ELECTRONS IN ATOMS MODERN CHEMISTRY Copyright © by Holt, Rinehart and Winston. All rights reserved. Name Date Class CHAPTER 4 REVIEW Arrangement of Electrons in Atoms SECTION 1 SHORT ANSWER Answer the following questions in the space provided. 1. In what way does the photoelectric effect support the particle theory of light? In order for an electron to be ejected from a metal surface, the electron must be struck by a single photon with at least the minimum energy needed to knock the electron loose. 2. What is the difference between the ground state and the excited state of an atom? The ground state is the lowest energy state of the atom. When the atom absorbs energy, it can move to a higher energy state, or excited state. 3. Under what circumstances can an atom emit a photon? A photon is emitted when an atom moves from an excited state to its ground state or to a lower-energy excited state. 4. How can the energy levels of the atom be determined by measuring the light emitted from an atom? When an atom loses energy, it falls from a higher energy state to a lower energy state. The frequency of the emitted light, observed in an element’s line-emission spectrum, may be measured. The energy of each transition is calculated using the equation E hv, where v is the frequency of each of the lines in the element’s lineemission spectrum. From the analysis of these results, the energy levels of an atom atom of each element may be determined. 5. Why does electromagnetic radiation in the ultraviolet region represent a larger energy transition than does radiation in the infrared region? Energy is proportional to frequency, and ultraviolet radiation has a higher frequency than infrared radiation. To produce ultraviolet radiation, electrons must drop to lower energy levels than they do to produce infrared radiation. MODERN CHEMISTRY Copyright © by Holt, Rinehart and Winston. All rights reserved. ARRANGEMENT OF ELECTRONS IN ATOMS 25 Name Date Class SECTION 1 continued 6. Which of the waves shown below has the higher frequency? (The scale is the same for each drawing.) Explain your answer. Wavelength Wavelength Wave A Wave B Wave B has the higher frequency. Wavelength is inversely proportional to frequency, so as the wavelength decreases, its frequency increases. 7. How many different photons of radiation were emitted from excited helium atoms to form the spectrum shown below? Explain your answer. Spectrum for helium Six different photons were emitted. Each time an excited helium atom falls back from an excited state to its ground state or to a lower energy state, it emits a photon of radiation that shows up as this specific line-emission spectrum. There are six lines in this helium spectrum. PROBLEMS provided. 8. 9. 26 Write the answer on the line to the left. Show all your work in the space 9.7 1014 Hz 9.4 109 m What is the frequency of light that has a wavelength of 310 nm? What is the wavelength of electromagnetic radiation if its frequency is 3.2 102 Hz? ARRANGEMENT OF ELECTRONS IN ATOMS MODERN CHEMISTRY Copyright © by Holt, Rinehart and Winston. All rights reserved. Name Date Class CHAPTER 4 REVIEW Arrangement of Electrons in Atoms SECTION 2 SHORT ANSWER 1. Answer the following questions in the space provided. How many quantum numbers are used to describe the properties of electrons in atomic orbitals? (a) 1 (b) 2 2. (c) 3 (d) 4 A spherical electron cloud surrounding an atomic nucleus would best represent (a) an s orbital. (b) a p orbital. 3. (c) a combination of two different p orbitals. (d) a combination of an s and a p orbital. How many electrons can an energy level of n 4 hold? (a) 32 (b) 24 4. (c) 8 (d) 6 How many electrons can an energy level of n 2 hold? (a) 32 (b) 24 5. (c) 8 (d) 6 Compared with an electron for which n 2, an electron for which n 4 has more (a) spin. (b) particle nature. 6. (c) energy. (d) wave nature. According to Bohr, which is the point in the figure below where electrons cannot reside? (a) point A (b) point B (c) point C (d) point D Orbitals D Nucleus 7. A B C According to the quantum theory, point D in the above figure represents (a) (b) (c) (d) the fixed position of an electron. the farthest position from the nucleus that an electron can achieve. a position where an electron probably exists. a position where an electron cannot exist. MODERN CHEMISTRY Copyright © by Holt, Rinehart and Winston. All rights reserved. ARRANGEMENT OF ELECTRONS IN ATOMS 27 Name Date Class SECTION 2 continued 8. How did de Broglie conclude that electrons have a wave nature? 9. Identify each of the four quantum numbers and the properties to which they refer. 10. How did the Heisenberg uncertainty principle contribute to the idea that electrons occupy “clouds,” or “orbitals”? 11. Complete the following table: Principal quantum number, n Number of sublevels Types of orbitals 1 2 3 4 28 ARRANGEMENT OF ELECTRONS IN ATOMS MODERN CHEMISTRY Copyright © by Holt, Rinehart and Winston. All rights reserved. Name Date Class CHAPTER 4 REVIEW Arrangement of Electrons in Atoms SECTION 2 SHORT ANSWER 1. d Answer the following questions in the space provided. How many quantum numbers are used to describe the properties of electrons in atomic orbitals? (a) 1 (b) 2 2. a (c) 3 (d) 4 A spherical electron cloud surrounding an atomic nucleus would best represent (a) an s orbital. (b) a p orbital. 3. a (c) a combination of two different p orbitals. (d) a combination of an s and a p orbital. How many electrons can an energy level of n 4 hold? (a) 32 (b) 24 4. c (c) 8 (d) 6 How many electrons can an energy level of n 2 hold? (a) 32 (b) 24 5. c (c) 8 (d) 6 Compared with an electron for which n 2, an electron for which n 4 has more (a) spin. (b) particle nature. 6. c (c) energy. (d) wave nature. According to Bohr, which is the point in the figure below where electrons cannot reside? (a) point A (b) point B (c) point C (d) point D Orbitals D Nucleus 7. c A B C According to the quantum theory, point D in the above figure represents (a) (b) (c) (d) the fixed position of an electron. the farthest position from the nucleus that an electron can achieve. a position where an electron probably exists. a position where an electron cannot exist. MODERN CHEMISTRY Copyright © by Holt, Rinehart and Winston. All rights reserved. ARRANGEMENT OF ELECTRONS IN ATOMS 27 Name Date Class SECTION 2 continued 8. How did de Broglie conclude that electrons have a wave nature? Scientists knew that any wave confined to a space could have only certain frequencies. De Broglie suggested that electrons should be considered as waves confined to the space around an atomic nucleus; in this way, electron waves could exist only at specific frequencies. According to the relationship E h , these frequencies correspond to the specific quantized energies of the Bohr orbitals. 9. Identify each of the four quantum numbers and the properties to which they refer. The principal quantum number refers to the main energy level. The angular momentum quantum number refers to the shape of the orbital. The magnetic quantum number refers to the orientation of an orbital around the nucleus. The spin quantum number indicates the spin state of an electron in an orbital. 10. How did the Heisenberg uncertainty principle contribute to the idea that electrons occupy “clouds,” or “orbitals”? The Heisenberg uncertainty principle states that it is impossible to determine simultaneously both the position and velocity of an electron (or any other particle). Because measuring the position of an electron actually changes its position, there is always a basic uncertainty in trying to locate an electron. Thus, the exact position of the electron cannot be found. An electron cloud or orbital represents the region that is the probable location of an electron. 11. Complete the following table: 28 Principal quantum number, n Number of sublevels Types of orbitals 1 1 s 2 2 s,p 3 3 s,p,d 4 4 s,p,d,f ARRANGEMENT OF ELECTRONS IN ATOMS MODERN CHEMISTRY Copyright © by Holt, Rinehart and Winston. All rights reserved. Name Date Class CHAPTER 4 REVIEW Arrangement of Electrons in Atoms SECTION 3 SHORT ANSWER Answer the following questions in the space provided. 1. State the Pauli exclusion principle, and use it to explain why electrons in the same orbital must have opposite spin states. 2. Explain the conditions under which the following orbital notation for helium is possible: ↑ ↑ 1s 2s Write the ground-state electron configuration and orbital notation for each of the following atoms: 3. Phosphorus 4. Nitrogen 5. Potassium MODERN CHEMISTRY Copyright © by Holt, Rinehart and Winston. All rights reserved. ARRANGEMENT OF ELECTRONS IN ATOMS 29 Name Date Class SECTION 3 continued 6. Aluminum 7. Argon 8. Boron 9. Which guideline, Hund’s rule or the Pauli exclusion principle, is violated in the following orbital diagrams? 3s2 a. 2p6 2s2 1s2 b. 2p4 2s2 1s2 30 ARRANGEMENT OF ELECTRONS IN ATOMS MODERN CHEMISTRY Copyright © by Holt, Rinehart and Winston. All rights reserved. Name Date Class CHAPTER 4 REVIEW Arrangement of Electrons in Atoms SECTION 3 SHORT ANSWER Answer the following questions in the space provided. 1. State the Pauli exclusion principle, and use it to explain why electrons in the same orbital must have opposite spin states. The Pauli exclusion principle states that no two electrons in an atom may have the same set of four quantum numbers. If both electrons in the same orbital had the same spin state, each electron would have the same four quantum numbers. If one electron has the opposite spin state, the fourth quantum number is different and the exclusion principle is obeyed. 2. Explain the conditions under which the following orbital notation for helium is possible: ↑ ↑ 1s 2s This orbital notation is possible if the helium atom is in an excited state. Write the ground-state electron configuration and orbital notation for each of the following atoms: 3. Phosphorus ↑↓ ↑↓ ↑↓ ↑↓ ↑↓ ↑↓ 1s 2s 2px 2py 2pz 3s ↑↓ ↑↓ ↑ 1s 2s 1s22s22p63s23p3; ↑ ↑ ↑ 3px 3py 3pz 4. Nitrogen 1s22s22p3; ↑ ↑ 2px 2py 2pz 5. Potassium 1s22s22p63s23p64s1; ↑↓ ↑↓ ↑↓ ↑↓ ↑↓ ↑↓ ↑↓ ↑↓ ↑↓ ↑ 1s 2s 2px 2py 2pz 3s 3px 3py 3pz 4s MODERN CHEMISTRY Copyright © by Holt, Rinehart and Winston. All rights reserved. ARRANGEMENT OF ELECTRONS IN ATOMS 29 Name Date Class SECTION 3 continued 6. Aluminum ↑↓ ↑↓ ↑↓ ↑↓ ↑↓ ↑↓ 1s 2s 2px 2py 2pz 3s ↑↓ ↑↓ ↑↓ ↑↓ ↑↓ ↑↓ ↑↓ ↑↓ ↑↓ 1s 2s 2px 2py 2pz 3s 3px 3py 3pz ↑↓ ↑↓ ↑ 1s 2s 1s22s22p63s23p1; ↑ 3px 3py 3pz 7. Argon 1s22s22p63s23p6; 8. Boron 1s22s22p1; 2px 2py 2pz 9. Which guideline, Hund’s rule or the Pauli exclusion principle, is violated in the following orbital diagrams? 3s2 a. Pauli exclusion principle b. Hund’s rule 2p6 2s2 1s2 2p4 2s2 1s2 30 ARRANGEMENT OF ELECTRONS IN ATOMS MODERN CHEMISTRY Copyright © by Holt, Rinehart and Winston. All rights reserved. Ms. K Honors Chemistry Name_______________________ #______ Date________________ Period_____ Chapter 4 Review Sheet REVIEW TERMS AND CONCEPTS energy work Joules, calories, and Calories Law of conservation of energy forms of energy kinetic vs. potential energy absolute zero electromagnetic radiation electromagnetic spectrum waves nodes amplitude wavelength frequency speed of light energy radio station’s frequency Planck’s constant photoelectric effect quantum photon ground state excited state bright-line emission spectrum continuous spectrum Bohr model of the atom Niels Bohr orbit emission absorption diffraction interference double-slit experiment Thomas Young Heisenberg uncertainty principle Werner Heisenberg quantum theory orbital s, p, d, f degenerate orbitals electron dot model quantum mechanical model quantum numbers principal quantum number, n energy level angular momentum quantum number, l magnetic quantum number, m spin quantum number, s orbital diagrams electron configurations Aufbau principle Pauli Exclusion principle Hund’s Rule Exceptions ? Cr, Cu, Mo, Ag ion electron configuration noble-gas configuration isoelectronic valence electrons REVIEW QUESTIONS 1. Which form of electromagnetic radiation has the higher ν, blue light or radio waves? 2. Which form of electromagnetic radiation has the higher λ, red light or orange light? 3. Which form of electromagnetic radiation has the higher E, ultraviolet light or microwaves? 4. Which form of electromagnetic radiation has the higher speed, green light or infrared waves? 5. Write the equation for the calculation for the energy of any photon of light. 6. Write the equation for the calculation for the wavelength of light. 7. What is it called when a light of high enough frequency is shined on a metal and electrons are emitted? 8. Why do you see discrete lines when a beam of emitted light from an element is shined through a prism and not a continuous spectrum? 9. Why is Ag?s electron configuration not in the ground state? 10. Write the electron configuration for element 116, both long-hand and short-hand. 11. Be able to answer the following questions from you textbook, pages 124-127: 4, 6, 8, 10, 11, 12, 13, 14, 18, 19, 22, 23, 24, 25, 26, 27, 28, 30, 31, 32, 35, 36, 37, 38, 41