TIME OF COMPLETION NAME SOLUTION DEPARTMENT OF NATURAL SCIENCES. PHYS 3650, Exam 2 Section 1 Version 1 October 31, 2005 Total Weight: 100 points


 Annis Fitzgerald
 1 years ago
 Views:
Transcription
1 TIME OF COMPLETION NAME SOLUTION DEPARTMENT OF NATURAL SCIENCES PHYS 3650, Exam 2 Section 1 Version 1 October 31, 2005 Total Weight: 100 points 1. Check your examination for completeness prior to starting. There are a total of ten (10) problems on seven (7) pages. 2. Authorized references include your calculator with calculator handbook, and the Reference Data Pamphlet (provided by your instructor). 3. You will have 75 minutes to complete the examination. 4. The total weight of the examination is 100 points. 5. There are six (6) multiple choice and four (4) calculation problems. Work all problems. Show all work; partial credit will be given for correct work shown. 6. If you have any questions during the examination, see your instructor who will be located in the classroom. 7. Start: 10:30 a.m. Stop: 11:45 a.m PROBLEM POINTS CREDIT TOTAL 100 PERCENTAGE
2 CIRCLE THE SINGLE BEST ANSWER FOR ALL MULTIPLE CHOICE QUESTIONS. IN MULTIPLE CHOICE QUESTIONS WHICH REQUIRE A CALCULATION SHOW WORK FOR PARTIAL CREDIT. 1. The p state of an electronic configuration corresponds to a. n = 2. b. l = 2. c. l = 1. d. n = Bohr s quantum condition on electron orbits requires a. That the angular momentum of the electron about the hydrogen nucleus equal nh/(2 ). b. That no more than one electron occupy a given stationary state. c. That the electrons spiral into the nucleus while radiating electromagnetic waves. d. None of the above. 3. The total number of quantum states of hydrogen with quantum number n = 4 is a. 4. b. 16. c. 32. d An electron in the L shell means that
3 a. l = 1. b. n = 1. c. n = 2. d. m = The restriction that no more than one electron can occupy a given quantum state in an atom was first stated by which of the following scientists? a. Bohr. b. De Broglie. c. Heisenberg. d. Pauli. 6. If the principal quantum number for hydrogen is 5, which one of the following is not a permitted orbital magnetic quantum number for that atom? a. 6. b. 2. c. 0. d The optical spectra of atoms with two electrons in the same outer shell are similar, but they are quite different from the spectra of atoms with just one outer electron because of the interaction of the
4 two electrons. Separate the following elements into two groups such that those in each group have similar spectra: lithium (Z = 3), beryllium (Z = 4), sodium (Z = 11), magnesium (Z = 12), potassium (Z = 19), calcium (Z = 20), chromium (Z = 24), nickel (Z = 28). Please list the electronic configurations of all of these elements. Li: 1s 2 2s 1 Be: 1s 2 2s 2 Na: 1s 2 2s 2 2p 6 3s 1 Mg: 1s 2 2s 2 2p 6 3s 2 K: 1s 2 2s 2 2p 6 3s 2 3p 6 4s 1 Ca: 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 Cr: 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 4 Ni: 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 8 1 electron in the outer shell: Li, Na, K 2 electrons in the outer shell: Be, Mg, Ca, Cr, Ni 8. Calculate the wavelength of the K line of rhodium (Z = 45). K : transition from L shell to K shell E K =  (Z1) 2 E 0 /1 2 = 26,330 ev E L =  (Z1) 2 E 0 /2 2 = 6,582 ev E = E L E K = 19,748 ev = hc/ E = nm Calculate the wavelength of the L line of rhodium. L : transition from M shell to L shell
5 E M =  (Z9) 2 E 0 /3 2 = 1,958 ev E L =  (Z1) 2 E 0 /2 2 = 6,582 ev E = E M E L = 4,624 ev = hc/ E = nm 9. Spectral lines of the following wavelengths are emitted by singly ionized helium: 164 nm, nm, and 541 nm. Identify the transitions that result in these spectral lines. He: Z = 2 E n =  Z 2 E 0 /n 2 E 1 = ev E 2 = ev E 3 = ev E 4 = ev E 5 = ev E 6 = ev E 7 = ev E 8 = ev E 9 = ev E 10 = ev = hc/ E E = hc/ E 1 = hc/ (1243 evnm)/(164 nm) = 7.58 ev E 2 = hc/ (1243 evnm)/(230.6 nm) = 5.39 ev E 3 E 2 transition E 9 E 3 transition
6 E 3 = hc/ (1243 evnm)/(541 nm) = 2.30 ev E 7 E 4 transition 10. A hydrogen atom is in its tenth excited state according to the Borh model (n = 11). a. What is the radius of the Bohr orbit? r n = n 2 a 0 r 11 = (11) 2 ( nm) = 6.40 nm b. What is the angular momentum of the electron? L n = n h/(2 ) L 11 =1 h/(2 ) = 1.16 x Js c. What is the electron s kinetic energy? L = p r p = L/r = 1.78 x kgm/s KE = p 2 /(2m e ) = (1.78 x kgm/s) 2 /(2(9.11 x kg)) = 1.73 x J = ev d. What is the electron s potential energy? PE =  k e e 2 /r PE =  (8.99 x 10 9 Nm 2 /kg 2 ) (1.60 x C) 2 /(6.40 x 109 m) = ev e. What is the electron s total energy? E = KE + PE = ev + ( ev) = ev TIME OF COMPLETION NAME SOLUTION DEPARTMENT OF NATURAL SCIENCES
7 PHYS 3650, Exam 2 Section 1 Version 1 November 4, 2006 Total Weight: 100 points 1. Check your examination for completeness prior to starting. There are a total of ten (10) problems on seven (7) pages. 2. Authorized references include your calculator with calculator handbook, and the Reference Data Pamphlet (provided by your instructor). 3. You will have 50 minutes to complete the examination. 4. The total weight of the examination is 100 points. 5. There are six (6) multiple choice and four (4) calculation problems. Work five multiple choice and three (3) calculation problems. Show all work; partial credit will be given for correct work shown. 6. If you have any questions during the examination, see your instructor who will be located in the classroom. 7. Start: 11:30 a.m. Stop: 12:20 p.m PROBLEM POINTS CREDIT TOTAL 100 PERCENTAGE CIRCLE THE SINGLE BEST ANSWER FOR ALL MULTIPLE CHOICE QUESTIONS. IN MULTIPLE CHOICE QUESTIONS WHICH REQUIRE A CALCULATION SHOW WORK FOR PARTIAL CREDIT.
8 1. According to the Bohr model of the atom, the angular momentum of an electron around the nucleus a. Could equal any positive value. b. Must equal an integral multiple of h. c. Must equal an integral multiple of h/2π. d. Decreases with time, eventually becoming zero. 2. The reason the position of a particle cannot be specified with infinite precision is the a. Exclusion principle. b. Uncertainty principle. c. Photoelectric effect. d. Principle of relativity. 3. The principal quantum number can have any integer value ranging from a.  to +. b. 0 to. c. 1 to. d. 1 to The spin quantum number can have values of a. 1/2, 1, 0, +1, +1/2.
9 b. 1/2, 1, +1, +1/2. c. 1/2, 0, +1/2. d. 1/2, +1/2. 5. In the ground state, the quantum numbers (n, l, m l, m s ) for hydrogen are, respectively, a. 1, 1, 1, 1. b. 1, 0, 0, 0. c. 1, 0, 0, ±1/2. d. 1, 1, 1, ±1/2. 6. In terms of an atom's electron configuration, the letters K, L, M, and N refer to a. Different shells with n equal to 1, 2, 3, or 4 respectively. b. Different sub shells with l equal to 1, 2, 3, or 4 respectively. c. The four possible levels for the magnetic quantum number. d. The four possible quantum numbers. 7. What is the full electron configuration in the ground state for elements with Z equal to (a) 10, 1s 2 2s 2 2p 6
10 (b) 16, 1s 2 2s 2 2p 6 3s 2 3p 4 (c) 28? 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 8 8. Use the Bohr theory to estimate the wavelength for an n 3 to n 1 transition in molybdenum ( Z 42). The measured value is nm. Why do we not expect perfect agreement? E K =  (Z1) 2 E 0 /1 2 = 22,862 ev E M =  (Z9) 2 E 0 /3 2 = 1,64 ev E = E M E K = 21,216 ev = hc/ E = nm 9. (a) Find the photon energy and wavelength for the series limit (shortest wavelength) in the Paschen series (n f = 3). 1/ = R(1/n 2 f 1/n 2 i ) = (1.10 x 10 7 m 1 )(1/3 2 1/inf 2 ) = x 10 7 m 1 = 8.18 x 107 m = 818 nm (b) Calculate the wavelengths for the three longest wavelengths in this series. 1/ = R(1/n f 2 1/n i 2 ) = (1.10 x 10 7 m 1 )(1/3 2 1/4 2 ) = x 10 7 m 1 = x 107 m = 1870 nm 1/ = R(1/n f 2 1/n i 2 ) = (1.10 x 10 7 m 1 )(1/3 2 1/5 2 ) = x 10 7 m 1
11 = x 107 m = 1406 nm 1/ = R(1/n f 2 1/n i 2 ) = (1.10 x 10 7 m 1 )(1/3 2 1/6 2 ) = x 10 7 m 1 = x 107 m = 1200 nm 10. Make a table of all of the allowed four quantum numbers for the first three shells of the hydrogen atom. How many electrons can each shell accommodate? K (2 electrons): n = 1 l = 0 m l = 0 m s = + 1/2 (1 0 0 ½ ) ( ½ ) 2 1s electrons L (8 electrons): n = 2 l = 0 m l = 0 m s = + 1/2 (2 0 0 ½ ) ( ½ ) 2 2s electrons ( ½ ) l = 1 m l = 1 m s = + 1/2 (2 11 ½ ) l = 1 m l = 0 m s = + 1/2 (2 1 0 ½ ) ( ½ ) 6 2p electrons 1 1 ½ ) l = 1 m l = 1 m s = + 1/2 (2 1 1 ½ ) (2 M (18 electrons): n = 3 l = 0 m l = 0 m s = + 1/2 (3 0 0 ½ ) ( ½ ) 2 3s electrons ( ½ ) l = 1 m l = 1 m s = + 1/2 (3 11 ½ ) l = 1 m l = 0 m s = + 1/2 (3 1 0 ½ ) ( ½ ) 6 3p electrons ( ½ ) ( ½ ) l = 1 m l = 1 m s = + 1/2 (3 1 1 ½ ) l = 2 m l = 2 m s = + 1/2 (3 22 ½ )
12 ( ½ ) l = 2 m l = 1 m s = + 1/2 (3 21 ½ ) l = 2 m l = 0 m s = + 1/2 (3 2 0 ½ ) ( ½ ) 10 3d electrons ( ½ ) ( ½ ) l = 2 m l = 1 m s = + 1/2 (3 2 1 ½ ) l = 2 m l = 2 m s = + 1/2 (3 2 2 ½ ) TIME OF COMPLETION NAME SOLUTION DEPARTMENT OF NATURAL SCIENCES PHYS 3650, Exam 2 Section 1 Version 1 October 31, 2008 Total Weight: 100 points 1. Check your examination for completeness prior to starting. There are a total of nine (9) problems on six (6) pages. 2. Authorized references include your calculator with calculator handbook, and the Reference Data Pamphlet (provided by your instructor). 3. You will have 50 minutes to complete the examination. 4. The total weight of the examination is 100 points. 5. There are six (6) multiple choice and three (3) calculation problems. Work five multiple choice and three (3) calculation problems. Show all work; partial credit will be given for correct work shown. 6. If you have any questions during the examination, see your instructor who will be located in the classroom. 7. Start: 10:00 a.m. Stop: 10:50 a.m PROBLEM POINTS CREDIT
13 TOTAL 100 PERCENTAGE CIRCLE THE SINGLE BEST ANSWER FOR ALL MULTIPLE CHOICE QUESTIONS. IN MULTIPLE CHOICE QUESTIONS WHICH REQUIRE A CALCULATION SHOW WORK FOR PARTIAL CREDIT. 1. Hydrogen atoms can emit lines with visible colors from red to violet. These four visible lines emitted by hydrogen atom are produced by electrons a. That start in the n = 2 level. b. That end up the n = 2 level. c. That end up in the n = 3 level. d. That start in the ground level. 2. According to the Pauli s exclusion principle, how many electrons in an atom may have a particular set of quantum numbers? a. 1. b. 2. c. 6. d The orbital angular momentum quantum number can take which of the following values for any given value of the principal quantum number, n?
14 a. l = 0, 1, 2,.. b. l = 0, 1, 2,., n. c. l = 0, 1, 2,., n 1. d. l = 0, 1, 2,., n Which of the following values are associated with the electron spin quantum number, m s? a. ± 1/2. b. 0. c. ± 1. d. ± Which ones of the atomic transition on the sodium energy level diagram below are NOT allowed by the selection rules? a. a and c. b. b and f. c. c and d. d. d and g.
15 6. Given the energy diagram above, estimate the wavelength of a photon emitted by a sodium atom as the electron goes through the transition d. a. 800 nm. b. 620 nm. c. 450 nm. d. 75 nm. 7. Titanium (Z = 22) is in its ground state. 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 2 a. What is its electronic configuration? state. b. List all the possible combinations of quantum numbers (n, l, m l, and m s ) an electron can have while in the subshell which is only partially filled in the ground 3d subshell: n = 3, l = 2 ( ½ ) ( ½ ) ( ½ ) ( ½ ) ( ½ ) l = 2 m l = 2 m s = + 1/2 (3 22 ½ ) l = 2 m l = 1 m s = + 1/2 (3 21 ½ ) l = 2 m l = 0 m s = + 1/2 (3 2 0 ½ ) l = 2 m l = 1 m s = + 1/2 (3 2 1 ½ ) l = 2 m l = 2 m s = + 1/2 (3 2 2 ½ ) 8. Using Bohr s model, estimate the wavelength of the K line for
16 a. calcium (Z = 20), and E K =  (Z1) 2 E 0 /1 2 =  (19) 2 (13.6 ev)/1 2 =  4,910 ev E L =  (Z1) 2 E 0 /1 2 =  (19) 2 (13.6 ev)/2 2 = ev E = E L E K = 3,683 ev = hc/ E = nm b. cadmium (Z = 48) E K =  (Z1) 2 E 0 /1 2 =  (47) 2 (13.6 ev)/1 2 =  30,042 ev E L =  (Z1) 2 E 0 /1 2 =  (47) 2 (13.6 ev)/2 2 =  7,510 ev E = E L E K = 22,532 ev = hc/ E = nm 10. Find the energy of the electron in the ground state of singly ionized helium (Z = 2). E 1 =  (Z) 2 E 0 /1 2 =  (2) 2 (13.6 ev)/1 2 = ev What is the shortest possible wavelength which is emitted as a result of electron returning to the ground state? Shortest wavelength corresponds to the transition from n = : E = E E 1 = 54.4 ev = hc/ E = 22.8 nm What is the longest possible wavelength which is emitted as a result of electron returning to the ground state? Lonest wavelength corresponds to the transision from n = 2:
17 E 2 =  (Z) 2 E 0 /2 2 =  (2) 2 (13.6 ev)/2 2 = ev E = E 2 E 1 = 40.8 ev = hc/ E = 30.4 nm TIME OF COMPLETION NAME SOLUTION DEPARTMENT OF NATURAL SCIENCES PHYS 3650, Exam 2 Section 1 Version 1 November 13, 2009 Total Weight: 100 points 1. Check your examination for completeness prior to starting. There are a total of nine (9) problems on six (6) pages. 2. Authorized references include your calculator with calculator handbook, and the Reference Data Pamphlet (provided by your instructor). 3. You will have 50 minutes to complete the examination. 4. The total weight of the examination is 100 points. 5. There are six (6) multiple choice and three (3) calculation problems. Work five multiple choice and three (3) calculation problems. Show all work; partial credit will be given for correct work shown. 6. If you have any questions during the examination, see your instructor who will be located in the classroom. 7. Start: 10:00 a.m. Stop: 10:50 a.m PROBLEM POINTS CREDIT
18 9 25 TOTAL 100 PERCENTAGE CIRCLE THE SINGLE BEST ANSWER FOR ALL MULTIPLE CHOICE QUESTIONS. IN MULTIPLE CHOICE QUESTIONS WHICH REQUIRE A CALCULATION SHOW WORK FOR PARTIAL CREDIT. 1. The Pauli exclusion principle: a. Implies that in an atom no two electrons can have the same set of quantum numbers. b. Says that no two electrons in an atom can have the same orbit. c. Excludes electrons from atomic nuclei. d. Excludes protons from atomic orbits. 2. Which one of these statements is true? a. The principal quantum number of the electron in a hydrogen atom does not affect its energy. b. The principal quantum number of an electron in its ground state is zero. c. The orbital quantum number of an electron state is always less than the principal quantum number of that state. d. The electron spin quantum number can take on any one of the four different values. 3. The orbital angular momentum quantum number can take which of the following values for any given value of the principal quantum number, n? a. l = 0, 1, 2,..
19 b. l = 0, 1, 2,., n. c. l = 0, 1, 2,., n 1. d. l = 0, 1, 2,., n How many of oxygen s eight electrons are found in the p state? a. 0. b. 2. c. 4. d The total number of states of hydrogen with principal quantum number n = 4 is: a. 4. b. 16. c. 32. d Given the sodium energy diagram above, estimate the wavelength of a photon emitted by a PHYS 3650 Exam 2, Version 1 Fall
20 sodium atom as the electron goes through the transition d. a. 800 nm. b. 620 nm. c. 450 nm. d. 75 nm. 9. Nickel (Z = 28) is in its ground state. a. What is its electronic configuration? 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 8 b. List all the possible combinations of quantum numbers (n, l, m l, and m s ) an electron can have while in the subshell which is only partially filled in the ground state. n = 3; l = 2; m l = 2, 1, 0, 1, 2; m s = ±1/2 (3, 2, 2, ±1/2) (3, 2, 1, ±1/2) (3, 2, 0, ±1/2) (3, 2, 1, ±1/2) (3, 2, 2, ±1/2) 10. Using Bohr s model, estimate the wavelength of the K line for a nickel target (Z = 28). E K =  (Z1) 2 E 0 /1 2 =  (281) 2 (13.6 ev)/1 2 =  9,914 ev E L =  (Z1) 2 E 0 /2 2 =  (281) 2 (13.6 ev)/2 2 = ev E = E L E K = 7,435 ev = hc/ E = nm What is the wavelength of the K line? PHYS 3650 Exam 2, Version 1 Fall
21 E K =  (Z1) 2 E 0 /1 2 =  (281) 2 (13.6 ev)/1 2 =  9,914 ev E M =  (Z9) 2 E 0 /3 2 =  (289) 2 (13.6 ev)/3 2 = ev E = E M E K = 9,368 ev = hc/ E = nm 11. Find the energy of the electron in the ground state of doubly ionized lithium (Z = 3). E 1 =  (Z) 2 E 0 /1 2 =  (3) 2 (13.6 ev)/1 2 = ev What is the shortest possible wavelength which is emitted as a result of electron returning to the ground state? E = 0 E 1 = 122 ev = hc/ E = 10.1 nm What is the longest possible wavelength which is emitted as a result of electron returning to the ground state? E 2 =  (Z) 2 E 0 /2 2 =  (3) 2 (13.6 ev)/2 2 = ev E = E 2 E 1 = 91.8 ev = hc/ E = 13.5 nm TIME OF COMPLETION NAME SOLUTION DEPARTMENT OF NATURAL SCIENCES PHYS 3650, Exam 2 Section 1 PHYS 3650 Exam 2, Version 1 Fall
22 Version 1 March 28, 2011 Total Weight: 100 points 1. Check your examination for completeness prior to starting. There are a total of nine (9) problems on six (6) pages. 2. Authorized references include your calculator with calculator handbook, and the Reference Data Pamphlet (provided by your instructor). 3. You will have 50 minutes to complete the examination. 4. The total weight of the examination is 100 points. 5. There are six (6) multiple choice and three (3) calculation problems. Work all calculation problems and 5 (five) multiple choice. Show all work; partial credit will be given for correct work shown. 6. If you have any questions during the examination, see your instructor who will be located in the classroom. 7. Start: 3:00 p.m. Stop: 3:50 p.m. PROBLEM POINTS CREDIT TOTAL 100 PERCENTAGE CIRCLE THE SINGLE BEST ANSWER FOR ALL MULTIPLE CHOICE QUESTIONS. IN MULTIPLE CHOICE QUESTIONS WHICH REQUIRE A CALCULATION SHOW WORK FOR PARTIAL CREDIT. PHYS 3650 Exam 2, Version 1 Fall
23 1. In a Compton scattering experiment, a photon of energy E is scattered from an electron at rest. After the scattering event occurs, which of the following statements is true? (A) The frequency of the photon is greater than E/h. (B) The energy of the photon is less than E. (C) The wavelength of the photon is less than hc/e. (D) (E) The momentum of the photon increases. None of those statements is true. 2. Which of the following phenomena most clearly demonstrates the wave nature of electrons? (A) The photoelectric effect. (B) The blackbody radiation. (C) The Compton effect. (D) Diffraction of electrons by crystals. (E) None of these answers. 3. A proton, an electron, and a helium nucleus all move at speed v. Rank their de Broglie wavelengths from largest to smallest. (A) (B) (C) (D) (E) electron, proton, helium nucleus. proton, helium nucleus, electron. proton, electron, helium nucleus. helium nucleus, electron, proton. helium nucleus, proton, electron PHYS 3650 Exam 2, Version 1 Fall
24 4.What is the longest wavelength in the Lyman Series? (A) (B) (C) (D) (E) nm nm nm nm nm. 5. To which of the following values of n does the longest wavelength in the Balmer series correspond? (A) 1. (B) 3. (C) 5. (D) 7. (E). 6. Which one of the following is the correct expression for the energy of a photon? (A) E = h/f. (B) E = h /c. (C) E = h. (D) E = hc/. (F) None of these. 7. The work function for aluminum is 4.08 ev. (a) Find the cutoff wavelength for aluminum. PHYS 3650 Exam 2, Version 1 Fall
25 hc 1240 ev nm 4.08 ev nm (b) What is the lowest frequency of light incident on aluminum that releases photoelectrons from its surface? 8 c m / s f nm Hz (c) If photons of energy 5.81 ev are incident on aluminum, what is the maximum kinetic energy of the ejected photoelectrons? KE hf 5.81 ev 4.08 ev ev 8. In the Compton effect, a nm photon strikes a free electron in a headon collision and knocks it into the forward direction. The rebounding photon recoils directly backward. Find a. The wavelength of the scattered photon. h m c e o ( 1 cos ) ( nm)(1 cos(180 )) nm nm nm nm b. The energy of the scattered photon. hc 1240 ev nm E 11, nm ev c. The kinetic energy of the recoiling electron. (Hint: subtract the final energy of the photon from its initial energy to find the kinetic energy of the electron.) hc 1240 ev nm E0 12, nm 0 ev PHYS 3650 Exam 2, Version 1 Fall
26 KE E0 E kev 9. (a) Find the photon energy and wavelength for the series limit (shortest wavelength) in the Paschen series (n = 3). 1 R H 1 ( ) 2 R 9 H 818 nm hc 1240 ev nm E nm ev (b) Calculate the wavelengths for the three longest wavelengths in this series. 1 R H 1 ( ) nm 1 R H 1 ( ) nm 1 R H 1 ( ) nm PHYS 3650 Exam 2, Version 1 Fall
27 PHYS 3650 Exam 2, Version 1 Fall
28 PHYS 3650 Exam 2, Version 1 Fall
Quantum Mechanics I Physics 325. Importance of Hydrogen Atom
Quantum Mechanics I Physics 35 Atomic spectra and Atom Models Importance of Hydrogen Atom Hydrogen is the simplest atom The quantum numbers used to characterize the allowed states of hydrogen can also
More informationPhotons. ConcepTest 27.1. 1) red light 2) yellow light 3) green light 4) blue light 5) all have the same energy. Which has more energy, a photon of:
ConcepTest 27.1 Photons Which has more energy, a photon of: 1) red light 2) yellow light 3) green light 4) blue light 5) all have the same energy 400 nm 500 nm 600 nm 700 nm ConcepTest 27.1 Photons Which
More informationAtomic Structure: Chapter Problems
Atomic Structure: Chapter Problems Bohr Model Class Work 1. Describe the nuclear model of the atom. 2. Explain the problems with the nuclear model of the atom. 3. According to Niels Bohr, what does n stand
More informationPractice questions for Ch. 7
Name: Class: Date: ID: A Practice questions for Ch. 7 Multiple Choice Identify the choice that best completes the statement or answers the question. 1. When ignited, a uranium compound burns with a green
More information13 What is the maximum number of electrons that can occupy the subshell 3d? a) 1 b) 3 c) 5 d) 2
Assignment 06 A 1 What is the energy in joules of an electron undergoing a transition from n = 3 to n = 5 in a Bohr hydrogen atom? a) 3.48 x 1017 J b) 2.18 x 1019 J c) 1.55 x 1019 J d) 2.56 x 1019
More informationChapter 18: The Structure of the Atom
Chapter 18: The Structure of the Atom 1. For most elements, an atom has A. no neutrons in the nucleus. B. more protons than electrons. C. less neutrons than electrons. D. just as many electrons as protons.
More informationChapter 38C  Atomic Physics. A PowerPoint Presentation by Paul E. Tippens, Professor of Physics Southern Polytechnic State University
Chapter 38C  Atomic Physics A PowerPoint Presentation by Paul E. Tippens, Professor of Physics Southern Polytechnic State University 007 Objectives: After completing this module, you should be able to:
More informationCOLLEGE PHYSICS. Chapter 29 INTRODUCTION TO QUANTUM PHYSICS
COLLEGE PHYSICS Chapter 29 INTRODUCTION TO QUANTUM PHYSICS Quantization: Planck s Hypothesis An ideal blackbody absorbs all incoming radiation and reemits it in a spectrum that depends only on temperature.
More informationCHAPTER 4 Structure of the Atom
CHAPTER 4 Structure of the Atom 4.1 The Atomic Models of Thomson and Rutherford 4.2 Rutherford Scattering 4.3 The Classic Atomic Model 4.4 The Bohr Model of the Hydrogen Atom 4.5 Successes and Failures
More informationArrangement of Electrons in Atoms
CHAPTER 4 PRETEST Arrangement of Electrons in Atoms In the space provided, write the letter of the term that best completes each sentence or best answers each question. 1. Which of the following orbital
More informationChapter 7: Electrons in Atoms. Electromagnetic Radiation
Chapter 7: Electrons in Atoms Dr. Chris Kozak Memorial University of Newfoundland, Canada 1 Electromagnetic Radiation Electric and magnetic fields propagate as waves through empty space or through a medium.
More informationPRACTICE EXAM IV P202 SPRING 2004
PRACTICE EXAM IV P202 SPRING 2004 1. In two separate double slit experiments, an interference pattern is observed on a screen. In the first experiment, violet light (λ = 754 nm) is used and a secondorder
More informationAP CHEMISTRY CHAPTER REVIEW CHAPTER 6: ELECTRONIC STRUCTURE AND THE PERIODIC TABLE
AP CHEMISTRY CHAPTER REVIEW CHAPTER 6: ELECTRONIC STRUCTURE AND THE PERIODIC TABLE You should be familiar with the wavelike properties of light: frequency ( ), wavelength ( ), and energy (E) as well as
More informationProblem Set 1 Solutions
Chemistry 36 Dr. Jean M. Standard Problem Set Solutions. The first 4 lines in the visible region of atomic line spectrum of hydrogen atom occur at wavelengths of 656., 486., 434.0, and 40. nm (this is
More information3 Modern Atomic Theory
CHAPTER 4 3 Modern Atomic Theory SECTION Atoms KEY IDEAS As you read this section, keep these questions in mind: How are electrons organized in an atom? Can the exact location of an electron be determined?
More informationChapter 6 Electronic Structure of Atoms
Chapter 6 Electronic Structure of Atoms 1. Electromagnetic radiation travels through vacuum at a speed of m/s. (a). 6.626 x 26 (b). 4186 (c). 3.00 x 8 (d). It depends on wavelength Explanation: The speed
More informationPractice Problems (Set #1) Properties of Electromagnetic Radiation. 1. Why don't we notice the wave nature of matter in our everyday experience?
Practice Problems (Set #1) Properties of Electromagnetic Radiation 1. Why don't we notice the wave nature of matter in our everyday experience? Since matter has huge mass, the wavelength will be very large
More informationAtomic structure The product of frequency and wavelength for all forms of electromagnetic radiation (light) is a constant, the speed of light c.
Chapter 5: Electrons in Atoms Light (Electromagnetic Radiation) Light has the properties of both waves and particles. Light waves carry energy through space. wavelength (λ) meters frequency (ν) Hz (s 1
More informationAnswer: b. Answer: a. Answer: d
Practice Test IV Name 1) In a single slit diffraction experiment, the width of the slit is 3.1 105 m and the distance from the slit to the screen is 2.2 m. If the beam of light of wavelength 600 nm passes
More informationBOHR S THEORY AND PHYSICS OF ATOM CHAPTER 43
1. a BOHR S THEORY AND PHYSICS OF ATOM CHAPTER 3 1 h A T (ML T ) M L T 3 L me L MLT M(AT) M L T a has dimensions of length.. We know, 1/ 1.1 1 (1/n 1 1/n ) a) n 1, n 3 or, 1/ 1.1 1 (1/ 1/9) 36 or, 6.5
More informationThe Advanced Placement Examination in Chemistry. Part I Multiple Choice Questions Part II Free Response Questions Selected Questions from1970 to 2010
The Advanced Placement Examination in Chemistry Part I Multiple Choice Questions Part II Free Response Questions Selected Questions from1970 to 2010 Atomic Theory and Periodicity Part I 1984 1. Which of
More informationMULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.
Exam Name MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) A photo cathode whose work function is 2.4 ev, is illuminated with white light that has
More informationWAVES AND PARTICLES. (v) i.e (vi) The potential difference required to bring an electron of wavelength to rest
WAVES AND PARTICLES 1. De Broglie wavelength associated with the charges particles (i) The energy of a charged particle accelerated through potential difference q = charge on the particel (ii) Momentum
More information5.111 Principles of Chemical Science
MIT OpenCourseWare http://ocw.mit.edu 5.111 Principles of Chemical Science Fall 2008 For information about citing these materials or our Terms of Use, visit: http://ocw.mit.edu/terms. 5.111 Lecture Summary
More informationElectromagnetic radiation (Maxwell, 1864) (nature of light) Composed of perpendicular electric field and magnetic field
7 Atomic Structure and Periodicity Electromagnetic radiation (Maxwell, 1864) (nature of light) Composed of perpendicular electric field and magnetic field Electric field (E) (wavelength) t Magnetic field
More informationCHAPTER 6: ANSWERS TO ASSIGNED PROBLEMS Hauser General Chemistry I revised 8/03/08
CHAPTER 6: ANSWERS TO ASSIGNED PROBLEMS Hauser General Chemistry I revised 8/03/08 6.9 What are the basic SI units for? (a) the wavelength of light meters, although colors are usually reported in 3 digit
More informationWave Function, ψ. Chapter 28 Atomic Physics. The Heisenberg Uncertainty Principle. Line Spectrum
Wave Function, ψ Chapter 28 Atomic Physics The Hydrogen Atom The Bohr Model Electron Waves in the Atom The value of Ψ 2 for a particular object at a certain place and time is proportional to the probability
More informationSample Exercise 6.1 Concepts of Wavelength and Frequency
Sample Exercise 6.1 Concepts of Wavelength and Frequency Two electromagnetic waves are represented in the margin. (a) Which wave has the higher frequency? (b) If one wave represents visible light and the
More informationELECTRONIC CONFIGURATIONS
ELECTRONIC CONFIGURATIONS ELECTRONIC CONFIGURATIONS CONTENTS The Bohr Atom Levels and sublevels Rules and principles Orbitals Rules for filling orbitals. The Aufbau principle Electronic configurations
More informationName Date Class ELECTRONS IN ATOMS. Standard Curriculum Core content Extension topics
13 ELECTRONS IN ATOMS Conceptual Curriculum Concrete concepts More abstract concepts or math/problemsolving Standard Curriculum Core content Extension topics Honors Curriculum Core honors content Options
More informationAS Revision questions Quantum Phenomena and Electricity
Q1. (a) State what happens in an atom when line spectra are produced. Electrons move from one energy level (or orbit) to a higher one (1 mark) when they absorb energy from an incoming photon or interact
More informationAtomic Theory and the Periodic Table
Atomic Theory and the Periodic Table Petrucci, Harwood and Herring: Chapters 9 and 10 Aims: To examine the Quantum Theory, to understand the electronic structure of elements, To explain the periodic table
More informationPSI AP Chemistry Unit 1 MC Homework. Laws of Multiple and Definite Proportions and Conservation of Mass
PSI AP Chemistry Unit 1 MC Homework Name Laws of Multiple and Definite Proportions and Conservation of Mass 1. Dalton's atomic theory explained the observation that the percentage by mass of the elements
More informationChapter 7. Quantum Theory and Atomic Structure
Chapter 7. Quantum Theory and Atomic Structure A problem arose in Rutherford s nuclear model. A nucleus and electron attract each other; to remain apart the electron must move. The energy of the electron
More informationElectromagnetic Radiation and Atomic Physics
Electromagnetic Radiation and Atomic Physics Properties of Electrons, Protons, and Neutrons (The Main Constituents of Ordinary Matter) Mass Electrons have a mass of 9.11 1031 kg. The mass of a proton
More informationAtomic Structure and the Periodic Table. Chapter 3.5
Atomic Structure and the Periodic Table Chapter 3.5 The Periodic Table The elements of the periodic table are arranged according to the way electrons arrange themselves around the nuclei of atoms Electron
More informationSample Exercise 6.1 Concepts of Wavelength and Frequency
Sample Exercise 6.1 Concepts of Wavelength and Frequency Two electromagnetic waves are represented below. (a) Which wave has the higher frequency? (b) If one wave represents visible light and the other
More informationChapter 11 Atoms, Energy and Electron Configurations Objectives
Objectives 1. To review Rutherford s model of the atom 2. To explore the nature of electromagnetic radiation 3. To see how atoms emit light A. Rutherford s Atom.but there is a problem here!! Using Rutherford
More information2. What is the wavelength of light that has a frequency of 4.22 x Hz? 3. What is the energy of light that has a frequency of 1.30 x Hz?
Skill Practice 10 1. Define the terms ground state and excited state. Ground state: the normal energy level that an electron occupies. Excited state: when an electron has absorbed energy to occupy a higher
More informationQuestion: Do all electrons in the same level have the same energy?
Question: Do all electrons in the same level have the same energy? From the Shells Activity, one important conclusion we reached based on the first ionization energy experimental data is that electrons
More informationA1_Lotukerfið og uppbygging atómanna
Instructor Solutions Manual for Chemistry for Engineering Students, 2 nd Edition 61 Lota_2 A1_Lotukerfið og uppbygging atómanna The Electromagnetic Spectrum 6.8 Which of the waves depicted here has the
More informationMultielectron atoms
Multielectron atoms Today: Using hydrogen as a model. The Periodic Table HWK 13 available online. Please fill out the online participation survey. Worth 10points on HWK 13. Final Exam is Monday, Dec.
More informationCHAPTER 12 ATOMS ONE MARK QUESTIONS WITH ANSWER. Ans: Electrons were discovered by J.J Thomason in the year 1897.
CHAPTER 12 ATOMS ONE MARK QUESTIONS WITH ANSWER 1. Who discovered electrons? Ans: Electrons were discovered by J.J Thomason in the year 1897. 2. What is the electric charge on an atom? Ans: At atom of
More informationThe Early History of Quantum Mechanics
Chapter 2 The Early History of Quantum Mechanics In the early years of the twentieth century, Max Planck, Albert Einstein, Louis de Broglie, Neils Bohr, Werner Heisenberg, Erwin Schrödinger, Max Born,
More informationAtomic Theory. Unit 3 Development of the Atomic Theory. H. Cannon, C. Clapper and T. Guillot Klein High School
Atomic Theory Unit 3 Development of the Atomic Theory 1. Where is the mass of the atom concentrated? In the nucleus 2. What is located in the nucleus? Neutrons and protons 3. What is the negative particle
More informationChem 1A Exam 2 Review Problems
Chem 1A Exam 2 Review Problems 1. At 0.967 atm, the height of mercury in a barometer is 0.735 m. If the mercury were replaced with water, what height of water (in meters) would be supported at this pressure?
More informationChapter 5. Mendeleev s Periodic Table
Chapter 5 Perodicity and Atomic Structure Mendeleev s Periodic Table In the 1869, Dmitri Mendeleev proposed that the properties of the chemical elements repeat at regular intervals when arranged in order
More informationAP Chemistry Chapter 6 Lecture Notes Electrons! 6.1 The Wave Nature of Light. 6.2 Quantized Energy and Photons. Chapter 6 Homework
AP Chemistry Chapter 6 Lecture Notes Electrons! Chapter 6 Homework 6.1 The Wave Nature of Light pg 253 #3, 4, 13, 15, 17, 19, 21, 25, 29 The electronic structure of an atom refers to the arrangement of
More informationExam 2 Solutions Chem 6, 9 Section, Spring 2002
1. Dartmouth s FM radio station, WDCR, broadcasts by emitting from its antenna photons of frequency 99.3 MHz (99.3 10 6 Hz). (a) What is the energy of a single WDCR photon? The photon energy is simply
More informationThe Phenomenon of Photoelectric Emission:
The Photoelectric Effect. The Wave particle duality of light Light, like any other E.M.R (electromagnetic radiation) has got a dual nature. That is there are experiments that prove that it is made up of
More informationElectrons in Atoms & Periodic Table Chapter 13 & 14 Assignment & Problem Set
Electrons in Atoms & Periodic Table Name WarmUps (Show your work for credit) Date 1. Date 2. Date 3. Date 4. Date 5. Date 6. Date 7. Date 8. Electrons in Atoms & Periodic Table 2 Study Guide: Things You
More informationCHEM 1411 Chapter 5 Homework Answers
1 CHEM 1411 Chapter 5 Homework Answers 1. Which statement regarding the gold foil experiment is false? (a) It was performed by Rutherford and his research group early in the 20 th century. (b) Most of
More informationElectromagnetic Radiation and Atomic Spectra POGIL
Name _Key AP Chemistry Electromagnetic Radiation and Atomic Spectra POGIL Electromagnetic Radiation Model 1: Characteristics of Waves The figure above represents part of a wave. The entire wave can be
More informationChapter 29: Atomic Structure. What will we learn in this chapter?
Chapter 29: Atomic Structure What will we learn in this chapter? Contents: Electrons in atoms Wave functions Electron spin Pauli exclusion principle Atomic structure Periodic table W. Pauli & N. Bohr Both
More informationThe Evolution of the Atom
The Evolution of the Atom 1808: Dalton s model of the atom was the billiard ball model. He thought the atom was a solid, indivisible sphere. Atoms of each element were identical in mass and their properties.
More informationBohr s Model and Emission Spectra of Hydrogen and Helium
PHYS01 LAB03 Bohr s Model and Emission Spectra of Hydrogen and Helium 1. Objective The objective of this experiment is to study the emission spectrum of hydrogen and to understand its origin in terms
More informationSAMPLE EXAM 2 FALL 2012 SOLUTIONS Chemistry 11, Fall 2007 Exam II November 15, 2007 7:30 PM 9:30 PM
Name: SOLUTIONS III, IV, and V Section (circle): 1 2 3 4 5 SAMPLE EXAM 2 FALL 2012 SOLUTIONS Chemistry 11, Fall 2007 Exam II November 15, 2007 7:30 PM 9:30 PM As always, full credit will not be given unless
More informationThe Bohr model for the electrons
The Bohr model for the electrons Electronic structure how the electrons are arranged inside the atom Applying the quantum principle of energy Two parameters: Energy Position Learning objectives Describe
More informationUnit 2: Chemical Bonding and Organic Chemistry
Chemistry AP Unit : Chemical Bonding and Organic Chemistry Unit : Chemical Bonding and Organic Chemistry Chapter 7: Atomic Structure and Periodicity 7.1: Electromagnetic Radiation Electromagnetic (EM)
More informationElectron Configuration Worksheet (and Lots More!!)
Electron Configuration Worksheet (and Lots More!!) Brief Instructions An electron configuration is a method of indicating the arrangement of electrons about a nucleus. A typical electron configuration
More informationCHEMSITRY NOTES Chapter 13. Electrons in Atoms
CHEMSITRY NOTES Chapter 13 Electrons in Atoms Goals : To gain an understanding of : 1. Atoms and their structure. 2. The development of the atomic theory. 3. The quantum mechanical model of the atom. 4.
More informationChapter 7: The QuantumMechanical Model of the Atom
C h e m i s t r y 1 A : C h a p t e r 7 P a g e 1 Chapter 7: The QuantumMechanical Model of the Atom Homework: Read Chapter 7. Work out sample/practice exercises Suggested Chapter 7 Problems: 37, 39,
More informationQuantum Atom: Atomic Structure, Electron Configuration, and Periodicity
Quantum Atom: Atomic Structure, Electron Configuration, and Periodicity Equations: λν = c E = hν E = hν energy of photon difference of energy levels λ = h/p p = mu (momentum and particle wavelength) debroglie
More informationName period AP chemistry Unit 2 worksheet Practice problems
Name period AP chemistry Unit 2 worksheet Practice problems 1. What are the SI units for a. Wavelength of light b. frequency of light c. speed of light Meter hertz (s 1 ) m s 1 (m/s) 2. T/F (correct
More informationWAVES AND ELECTROMAGNETIC RADIATION
WAVES AND ELECTROMAGNETIC RADIATION All waves are characterized by their wavelength, frequency and speed. Wavelength (lambda, ): the distance between any 2 successive crests or troughs. Frequency (nu,):
More informationLecture 12 Quantum Mechanics and Atomic Orbitals
Lecture 12 Quantum Mechanics and Atomic Orbitals Bohr and Einstein demonstrated the particle nature of light.e = hν. De Broglie demonstrated the wavelike properties of particles. λ = h/mv. However, these
More informationOutline. Chapter 6 Electronic Structure and the Periodic Table. Review. Arranging Electrons in Atoms. Fireworks. Atomic Spectra
Outline William L Masterton Cecile N. Hurley Edward J. Neth cengage.com/chemistry/masterton Chapter 6 Electronic Structure and the Periodic Table Light, photon energies and atomic spectra The hydrogen
More informationAtoms Absorb & Emit Light
Atoms Absorb & Emit Light Spectra The wavelength of the light that an element emits or absorbs is its fingerprint. Atoms emit and absorb light First Test is Thurs, Feb 1 st About 30 multiple choice questions
More informationAP Chemistry A. Allan Chapter 7 Notes  Atomic Structure and Periodicity
AP Chemistry A. Allan Chapter 7 Notes  Atomic Structure and Periodicity 7.1 Electromagnetic Radiation A. Types of EM Radiation (wavelengths in meters) 101 1010 108 4 to 7x107 104 101 10 10 4 gamma
More informationChapter 6 Electromagnetic Radiation and the Electronic Structure of the Atom
Chapter 6 In This Chapter Physical and chemical properties of compounds are influenced by the structure of the molecules that they consist of. Chemical structure depends, in turn, on how electrons are
More informationHistory of Atomic Theory
History of Atomic Theory Alchemy ~ Before 400 B.C. Experiment: Pseudoscience concerned with: Changing metal to gold Finding an eternal life elixir Aristotle Beliefs: All matter was made up of a combination
More informationHomework #10 (749508)
Homework #10 (749508) Current Score: 0 out of 100 Description Homework on quantum physics and radioactivity Instructions Answer all the questions as best you can. 1. Hewitt10 32.E.001. [481697] 0/5 points
More informationChapter 7. Electron Structure of the Atom. Chapter 7 Topics
Chapter 7 Electron Structure of the Atom Copyright The McGrawHill Companies, Inc. Permission required for reproduction or display. 1 Chapter 7 Topics 1. Electromagnetic radiation 2. The Bohr model of
More informationnm cm meters VISIBLE UVB UVA Near IR 200 300 400 500 600 700 800 900 nm
Unit 5 Chapter 13 Electrons in the Atom Electrons in the Atom (Chapter 13) & The Periodic Table/Trends (Chapter 14) Niels Bohr s Model Recall the Evolution of the Atom He had a question: Why don t the
More informationMODERN ATOMIC THEORY AND THE PERIODIC TABLE
CHAPTER 10 MODERN ATOMIC THEORY AND THE PERIODIC TABLE SOLUTIONS TO REVIEW QUESTIONS 1. Wavelength is defined as the distance between consecutive peaks in a wave. It is generally symbolized by the Greek
More informationCHAPTER 8 PRACTICE TEST QUESTIONS (END OF CHAPTER 7 TOO)
CHAPTER 8 PRACTICE TEST QUESTIONS (END OF CHAPTER 7 TOO) Information that most likely will be on the front cover of your exam: h i Z 2 ΔE = @ 2.18 x 10 @ 18 f Z 2 f J j @ k n f 2 n i 2 1. Which of the
More informationChemistry 2 Chapter 13: Electrons in Atoms Please do not write on the test Use an answer sheet! 1 point/problem 45 points total
Chemistry 2 Chapter 13: Electrons in Atoms Please do not write on the test Use an answer sheet! 1 point/problem 45 points total 1. Calculate the energy in joules of a photon of red light that has a frequency
More informationPeople s Physics book
The Big Idea Quantum Mechanics, discovered early in the 20th century, completely shook the way physicists think. Quantum Mechanics is the description of how the universe works on the very small scale.
More informationElectron Configurations
SECTION 4.3 Electron Configurations Bohr s model of the atom described the possible energy states of the electron in a hydrogen atom. The energy states were deduced from observations of hydrogen s emissionline
More informationAtomic Emission Spectra (Teacher Demonstration)
SKILL FOCUS Analyzing and interpreting Communicating results Atomic Emission Spectra (Teacher Demonstration) When a high voltage current is passed through a glass tube that contains hydrogen gas at low
More informationNo Brain Too Small PHYSICS ATOMS: PHOTONS AND THE PHOTOELECTRIC EFFECT QUESTIONS
ATOMS: PHOTONS AND THE PHOTOELECTRIC EFFECT QUESTIONS SODIUM LAMPS (2012;2) Low pressure sodium lamps are widely used in street lighting. The lamps produce light when an electric current is passed through
More informationMULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.
Practice Questions  Chapter 7 Name MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) Which one of the following represents an impossible set of
More informationCHAPTER 10 MODERN ATOMIC THEORY AND THE PERIODIC TABLE SOLUTIONS TO REVIEW QUESTIONS
HEINS10118128v4.qxd 12/30/06 2:05 PM Page 118 CHAPTER 10 MODERN ATOMIC THEORY AND THE PERIODIC TABLE SOLUTIONS TO REVIEW QUESTIONS 1. An electron orbital is a region in space around the nucleus of an
More informationUnit 3 Study Guide: Electron Configuration & The Periodic Table
Name: Teacher s Name: Class: Block: Date: Unit 3 Study Guide: Electron Configuration & The Periodic Table 1. For each of the following elements, state whether the element is radioactive, synthetic or both.
More informationLithium Atomic number: 3 Atomic weight: 7 State of matter: solid Protons: 3 Neutrons (usually): 4 Electrons: 3 Number of electron shells:
Hydrogen Atomic number: 1 Atomic weight: 1 Protons: 1 Neutrons (usually): 0 Electrons: 1 H Helium Atomic number: 2 Atomic weight: 4 Protons: 2 Neutrons (usually): 2 Electrons: 2 He Lithium Atomic number:
More informationLecture 20: Polyelectronic Atoms
Lecture 20: Polyelectronic Atoms Reading: Zumdahl 12.1012.13 Outline: Spin (the 4 th quantum number) The Aufbau ( fillingup ) Principle Filling up orbitals and the Periodic Table Electronic Configuration
More informationExperiment #12: The Bohr Atom. Equipment: Spectroscope Hydrogen and Helium Gas Discharge Tubes, Holder, and Variac Flashlight
Experiment #12: The Bohr Atom Purpose: To observe the visible spectrum of hydrogen and helium and verify the Bohr model of the hydrogen atom. Equipment: Spectroscope Hydrogen and Helium Gas Discharge Tubes,
More informationDO PHYSICS ONLINE FROM QUANTA TO QUARKS QUANTUM (WAVE) MECHANICS
DO PHYSICS ONLINE FROM QUANTA TO QUARKS QUANTUM (WAVE) MECHANICS Quantum Mechanics or wave mechanics is the best mathematical theory used today to describe and predict the behaviour of particles and waves.
More informationThe Periodic Table: Chapter Problems Periodic Table Class Work Homework Special Groups Class Work Homework Periodic Families Class Work
The Periodic Table: Chapter Problems Periodic Table 1. As you move from left to right across the periodic table, how does atomic number change? 2. What element is located in period 3, group 13? 3. What
More informationCalculating particle properties of a wave
Calculating particle properties of a wave A light wave consists of particles (photons): The energy E of the particle is calculated from the frequency f of the wave via Planck: E = h f (1) A particle can
More informationFlame Tests & Electron Configuration
Flame Tests & Electron Configuration INTRODUCTION Many elements produce colors in the flame when heated. The origin of this phenomenon lies in the arrangement, or configuration of the electrons in the
More information2. For the following two compounds between oxygen and hydrogen: 3. Tell what discoveries were made by each of the following scientists:
EXTRA HOMEWORK 1A 1. When Dalton proposed that matter was composed of atoms, why was his Atomic Theory accepted? 2. For the following two compounds between oxygen and hydrogen: Mass of O Mass of H Compound
More informationPSI AP Chemistry Unit 1: The Atom Free Response CW/HW
PSI AP Chemistry Unit 1: The Atom Free Response CW/HW Name Laws of Multiple and Definite Proportions and Conservation of Mass Classwork: 1. Exactly twice as much oxygen is required to react with 1 gram
More informationPart I: Principal Energy Levels and Sublevels
Part I: Principal Energy Levels and Sublevels As you already know, all atoms are made of subatomic particles, including protons, neutrons, and electrons. Positive protons and neutral neutrons are found
More informationExperiment 13 ~ Diffraction, Wavelength, and Atomic Line Spectra
Experiment 13 ~ Diffraction, Wavelength, and Atomic Line Spectra Part 1 1.1. Atomic Line Spectra. In this experiment, we will look at the diffraction of light, and how wavelengths can be calculated from
More informationLight as a Wave. The Nature of Light. EM Radiation Spectrum. EM Radiation Spectrum. Electromagnetic Radiation
The Nature of Light Light and other forms of radiation carry information to us from distance astronomical objects Visible light is a subset of a huge spectrum of electromagnetic radiation Maxwell pioneered
More informationReview of the isotope effect in the hydrogen spectrum
Review of the isotope effect in the hydrogen spectrum 1 Balmer and Rydberg Formulas By the middle of the 19th century it was well established that atoms emitted light at discrete wavelengths. This is in
More informationQuantum, Atomic and Nuclear Physics
Quantum, Atomic and Nuclear Physics Regular Quantum, Atomic and Nuclear Physics Worksheets and Solutions QR1: Photons 3 QR2: Wave Functions I Particles as Waves 7 QR3: Wave Functions II Particles in Boxes
More informationemission of light from atoms discrete line spectra  energy levels, FranckHertz experiment
Introduction Until the early 20 th century physicists used to explain the phenomena in the physical world around them using theories such a mechanics, electromagnetism, thermodynamics and statistical physics
More information