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

Size: px
Start display at page:

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

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 = - (Z-1) 2 E 0 /1 2 = -26,330 ev E L = - (Z-1) 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 = - (Z-9) 2 E 0 /3 2 = -1,958 ev E L = - (Z-1) 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 J-s c. What is the electron s kinetic energy? L = p r p = L/r = 1.78 x kg-m/s KE = p 2 /(2m e ) = (1.78 x kg-m/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 N-m 2 /kg 2 ) (1.60 x C) 2 /(6.40 x 10-9 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 = - (Z-1) 2 E 0 /1 2 = -22,862 ev E M = - (Z-9) 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 10-7 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 10-7 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 10-7 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 10-7 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 1-1 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 1-1 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 2-2 ½ )

12 ( ½ ) l = 2 m l = -1 m s = +- 1/2 (3 2-1 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 2-2 ½ ) l = 2 m l = -1 m s = +- 1/2 (3 2-1 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 = - (Z-1) 2 E 0 /1 2 = - (19) 2 (13.6 ev)/1 2 = - 4,910 ev E L = - (Z-1) 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 = - (Z-1) 2 E 0 /1 2 = - (47) 2 (13.6 ev)/1 2 = - 30,042 ev E L = - (Z-1) 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 = - (Z-1) 2 E 0 /1 2 = - (28-1) 2 (13.6 ev)/1 2 = - 9,914 ev E L = - (Z-1) 2 E 0 /2 2 = - (28-1) 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 = - (Z-1) 2 E 0 /1 2 = - (28-1) 2 (13.6 ev)/1 2 = - 9,914 ev E M = - (Z-9) 2 E 0 /3 2 = - (28-9) 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 head-on 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

### Photons. 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

### Atomic 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

### Chapter 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.

### 13- 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 10-17 J b) 2.18 x 10-19 J c) 1.55 x 10-19 J d) -2.56 x 10-19

### How To Understand Light And Color

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 second-order

### Arrangement of Electrons in Atoms

CHAPTER 4 PRE-TEST 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

### The 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

### Name Date Class ELECTRONS IN ATOMS. Standard Curriculum Core content Extension topics

13 ELECTRONS IN ATOMS Conceptual Curriculum Concrete concepts More abstract concepts or math/problem-solving Standard Curriculum Core content Extension topics Honors Curriculum Core honors content Options

### Sample 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

### Wave 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

### Question: 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

### Chem 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?

### The 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

### Multi-electron atoms

Multi-electron 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.

### SAMPLE 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

### CHEM 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

### Atoms 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

### Name 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

### Electron 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

### Electrons in Atoms & Periodic Table Chapter 13 & 14 Assignment & Problem Set

Electrons in Atoms & Periodic Table Name Warm-Ups (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

### MODERN 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

### Chemistry 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

### Chapter 7. Electron Structure of the Atom. Chapter 7 Topics

Chapter 7 Electron Structure of the Atom Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. 1 Chapter 7 Topics 1. Electromagnetic radiation 2. The Bohr model of

### Homework #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

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,):

### CHEMSITRY 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.

### CHAPTER 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

### MULTIPLE 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

### Unit 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)

### Unit 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.

### Review 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

### DO 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.

### Experiment #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,

### Light 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

### 9/13/2013. However, Dalton thought that an atom was just a tiny sphere with no internal parts. This is sometimes referred to as the cannonball model.

John Dalton was an English scientist who lived in the early 1800s. Dalton s atomic theory served as a model for how matter worked. The principles of Dalton s atomic theory are: 1. Elements are made of

### Flame 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

### Chapters 21-29. Magnetic Force. for a moving charge. F=BQvsinΘ. F=BIlsinΘ. for a current

Chapters 21-29 Chapter 21:45,63 Chapter 22:25,49 Chapter 23:35,38,53,55,58,59 Chapter 24:17,18,20,42,43,44,50,52,53.59,63 Chapter 26:27,33,34,39,54 Chapter 27:17,18,34,43,50,51,53,56 Chapter 28: 10,11,28,47,52

### 5. The Nature of Light. Does Light Travel Infinitely Fast? EMR Travels At Finite Speed. EMR: Electric & Magnetic Waves

5. The Nature of Light Light travels in vacuum at 3.0. 10 8 m/s Light is one form of electromagnetic radiation Continuous radiation: Based on temperature Wien s Law & the Stefan-Boltzmann Law Light has

### 2. John Dalton did his research work in which of the following countries? a. France b. Greece c. Russia d. England

CHAPTER 3 1. Which combination of individual and contribution is not correct? a. Antoine Lavoisier - clarified confusion over cause of burning b. John Dalton - proposed atomic theory c. Marie Curie - discovered

### Calculating 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

### AP* Atomic Structure & Periodicity Free Response Questions KEY page 1

AP* Atomic Structure & Periodicity ree Response Questions KEY page 1 1980 a) points 1s s p 6 3s 3p 6 4s 3d 10 4p 3 b) points for the two electrons in the 4s: 4, 0, 0, +1/ and 4, 0, 0, - 1/ for the three

### Bohr's Theory of the Hydrogen Atom

OpenStax-CNX module: m42596 1 Bohr's Theory of the Hydrogen Atom OpenStax College This work is produced by OpenStax-CNX and licensed under the Creative Commons Attribution License 4.0 Abstract Describe

### Part 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

### Level 3 Achievement Scale

Unit 1: Atoms Level 3 Achievement Scale Can state the key results of the experiments associated with Dalton, Rutherford, Thomson, Chadwick, and Bohr and what this lead each to conclude. Can explain that

### PHOTOELECTRIC EFFECT AND DUAL NATURE OF MATTER AND RADIATIONS

PHOTOELECTRIC EFFECT AND DUAL NATURE OF MATTER AND RADIATIONS 1. Photons 2. Photoelectric Effect 3. Experimental Set-up to study Photoelectric Effect 4. Effect of Intensity, Frequency, Potential on P.E.

### IONISATION ENERGY CONTENTS

IONISATION ENERGY IONISATION ENERGY CONTENTS What is Ionisation Energy? Definition of t Ionisation Energy What affects Ionisation Energy? General variation across periods Variation down groups Variation

### 3) Of the following, radiation has the shortest wavelength. A) X-ray B) radio C) microwave D) ultraviolet E) infrared Answer: A

1) Which one of the following is correct? A) ν + λ = c B) ν λ = c C) ν = cλ D) λ = c ν E) νλ = c Answer: E 2) The wavelength of light emitted from a traffic light having a frequency of 5.75 1014 Hz is.

### Untitled Document. 1. Which of the following best describes an atom? 4. Which statement best describes the density of an atom s nucleus?

Name: Date: 1. Which of the following best describes an atom? A. protons and electrons grouped together in a random pattern B. protons and electrons grouped together in an alternating pattern C. a core

### Basic Nuclear Concepts

Section 7: In this section, we present a basic description of atomic nuclei, the stored energy contained within them, their occurrence and stability Basic Nuclear Concepts EARLY DISCOVERIES [see also Section

### Chapter 28 Atomic Physics

614 Chapter 28 Atomic Physics GOALS After you have mastered the contents of this chapter, you will be able to achieve the following goals: Definitions Define each of the following terms and use it in an

### Chemistry 102 Summary June 24 th. Properties of Light

Chemistry 102 Summary June 24 th Properties of Light - Energy travels through space in the form of electromagnetic radiation (EMR). - Examples of types of EMR: radio waves, x-rays, microwaves, visible

### 3. What would you predict for the intensity and binding energy for the 3p orbital for that of sulfur?

PSI AP Chemistry Periodic Trends MC Review Name Periodic Law and the Quantum Model Use the PES spectrum of Phosphorus below to answer questions 1-3. 1. Which peak corresponds to the 1s orbital? (A) 1.06

### Electron Orbits. Binding Energy. centrifugal force: electrostatic force: stability criterion: kinetic energy of the electron on its orbit:

Electron Orbits In an atom model in which negatively charged electrons move around a small positively charged nucleus stable orbits are possible. Consider the simple example of an atom with a nucleus of

### ATOMIC SPECTRA. Apparatus: Optical spectrometer, spectral tubes, power supply, incandescent lamp, bottles of dyed water, elevating jack or block.

1 ATOMIC SPECTRA Objective: To measure the wavelengths of visible light emitted by atomic hydrogen and verify the measured wavelengths against those predicted by quantum theory. To identify an unknown

### Quantum Mechanics and Atomic Structure 1

Quantum Mechanics and Atomic Structure 1 INTRODUCTION The word atom is derived from the Greek word, atomos, which means uncut or indivisible. It was Dalton (1808) who established that elementary constituents

### IONISATION ENERGY CONTENTS

IONISATION ENERGY IONISATION ENERGY CONTENTS What is Ionisation Energy? Definition of t Ionisation Energy What affects Ionisation Energy? General variation across periods Variation down groups Variation

### Electron Arrangements

Section 3.4 Electron Arrangements Objectives Express the arrangement of electrons in atoms using electron configurations and Lewis valence electron dot structures New Vocabulary Heisenberg uncertainty

### Student Exploration: Electron Configuration

Name: Date: Student Exploration: Electron Configuration Vocabulary: atomic number, atomic radius, Aufbau principle, chemical family, diagonal rule, electron configuration, Hund s rule, orbital, Pauli exclusion

### Electrons In Atoms Mr. O Brien (SFHS) Chapter 5 Standard 1D

Electrons In Atoms Mr. O Brien (SFHS) Chapter 5 Standard 1D Electrons in Atoms (std.1d) What are Bohr Models? planetary model in which the negatively-charged electrons orbit a small, positively-charged

### Chapter 8 Atomic Electronic Configurations and Periodicity

Chapter 8 Electron Configurations Page 1 Chapter 8 Atomic Electronic Configurations and Periodicity 8-1. Substances that are weakly attracted to a magnetic field but lose their magnetism when removed from

### 7.4. Using the Bohr Theory KNOW? Using the Bohr Theory to Describe Atoms and Ions

7.4 Using the Bohr Theory LEARNING TIP Models such as Figures 1 to 4, on pages 218 and 219, help you visualize scientific explanations. As you examine Figures 1 to 4, look back and forth between the diagrams

### CHAPTER 11: MODERN ATOMIC THEORY

CHAPTER 11: MODERN ATOMIC THEORY Active Learning Questions: 1-2, 8-10, 14-18; End-of-Chapter Problems: 3-9, 11-13, 16, 18, 20-36, 45-54, 56-64, 66b, 67, 69-91, 98, 101-102, 108, 110, 113, 116, 11.2 ELECTROMAGNETIC

### 6.5 Periodic Variations in Element Properties

324 Chapter 6 Electronic Structure and Periodic Properties of Elements 6.5 Periodic Variations in Element Properties By the end of this section, you will be able to: Describe and explain the observed trends

### Bohr s Model of the Atom

Bohr Models Bohr s Model of the Atom Focuses on electrons and their arrangement. Bohr stated that electrons move with constant speed in fixed orbits around the nucleus, like planets around a sun. Bohr

### Atomic Structure Ron Robertson

Atomic Structure Ron Robertson r2 n:\files\courses\1110-20\2010 possible slides for web\atomicstructuretrans.doc I. What is Light? Debate in 1600's: Since waves or particles can transfer energy, what is

### Main properties of atoms and nucleus

Main properties of atoms and nucleus. Atom Structure.... Structure of Nuclei... 3. Definition of Isotopes... 4. Energy Characteristics of Nuclei... 5. Laws of Radioactive Nuclei Transformation... 3. Atom

### PHY4604 Introduction to Quantum Mechanics Fall 2004 Practice Test 3 November 22, 2004

PHY464 Introduction to Quantum Mechanics Fall 4 Practice Test 3 November, 4 These problems are similar but not identical to the actual test. One or two parts will actually show up.. Short answer. (a) Recall

### Nanoelectronics. Chapter 2 Classical Particles, Classical Waves, and Quantum Particles. Q.Li@Physics.WHU@2015.3

Nanoelectronics Chapter 2 Classical Particles, Classical Waves, and Quantum Particles Q.Li@Physics.WHU@2015.3 1 Electron Double-Slit Experiment Q.Li@Physics.WHU@2015.3 2 2.1 Comparison of Classical and

### Student Exploration: Electron Configuration

www.explorelearning.com Name: Date: Student Exploration: Electron Configuration Vocabulary: atomic number, atomic radius, Aufbau principle, chemical family, diagonal rule, electron configuration, Hund

### Physics 30 Worksheet # 14: Michelson Experiment

Physics 30 Worksheet # 14: Michelson Experiment 1. The speed of light found by a Michelson experiment was found to be 2.90 x 10 8 m/s. If the two hills were 20.0 km apart, what was the frequency of the

### PROTONS AND ELECTRONS

reflect Imagine that you have a bowl of oranges, bananas, pineapples, berries, pears, and watermelon. How do you identify each piece of fruit? Most likely, you are familiar with the characteristics of

### MASS DEFECT AND BINDING ENERGY

MASS DEFECT AND BINDING ENERGY The separate laws of Conservation of Mass and Conservation of Energy are not applied strictly on the nuclear level. It is possible to convert between mass and energy. Instead

### Chemistry CP Unit 2 Atomic Structure and Electron Configuration. Learning Targets (Your exam at the end of Unit 2 will assess the following:)

Chemistry CP Unit 2 Atomic Structure and Electron Learning Targets (Your exam at the end of Unit 2 will assess the following:) 2. Atomic Structure and Electron 2-1. Give the one main contribution to the

### SCPS Chemistry Worksheet Periodicity A. Periodic table 1. Which are metals? Circle your answers: C, Na, F, Cs, Ba, Ni

SCPS Chemistry Worksheet Periodicity A. Periodic table 1. Which are metals? Circle your answers: C, Na, F, Cs, Ba, Ni Which metal in the list above has the most metallic character? Explain. Cesium as the

### From lowest energy to highest energy, which of the following correctly orders the different categories of electromagnetic radiation?

From lowest energy to highest energy, which of the following correctly orders the different categories of electromagnetic radiation? From lowest energy to highest energy, which of the following correctly

### 47374_04_p25-32.qxd 2/9/07 7:50 AM Page 25. 4 Atoms and Elements

47374_04_p25-32.qxd 2/9/07 7:50 AM Page 25 4 Atoms and Elements 4.1 a. Cu b. Si c. K d. N e. Fe f. Ba g. Pb h. Sr 4.2 a. O b. Li c. S d. Al e. H f. Ne g. Sn h. Au 4.3 a. carbon b. chlorine c. iodine d.

### Matter Waves. Home Work Solutions

Chapter 5 Matter Waves. Home Work s 5.1 Problem 5.10 (In the text book) An electron has a de Broglie wavelength equal to the diameter of the hydrogen atom. What is the kinetic energy of the electron? How

### 5.4 Trends in the Periodic Table

5.4 Trends in the Periodic Table Think about all the things that change over time or in a predictable way. For example, the size of the computer has continually decreased over time. You may become more

### Name: Worksheet: Electron Configurations. I Heart Chemistry!

1. Which electron configuration represents an atom in an excited state? 1s 2 2s 2 2p 6 3p 1 1s 2 2s 2 2p 6 3s 2 3p 2 1s 2 2s 2 2p 6 3s 2 3p 1 1s 2 2s 2 2p 6 3s 2 Worksheet: Electron Configurations Name:

### A-level PHYSICS (7408/1)

SPECIMEN MATERIAL A-level PHYSICS (7408/1) Paper 1 Specimen 2014 Morning Time allowed: 2 hours Materials For this paper you must have: a pencil a ruler a calculator a data and formulae booklet. Instructions

### Instructors Guide: Atoms and Their Isotopes

Instructors Guide: Atoms and Their Isotopes Standards Connections Connections to NSTA Standards for Science Teacher Preparation C.3.a.1 Fundamental structures of atoms and molecules. C.3.b.27 Applications

### Models of the Atom and periodic Trends Exam Study Guide

Name 1. What is the term for the weighted average mass of all the naturally occurring isotopes of an element? ans: atomic mass 2. Which is exactly equal to 1/12 the mass of a carbon -12 atom? ans: atomic

### CHAPTER 9 ATOMIC STRUCTURE AND THE PERIODIC LAW

CHAPTER 9 ATOMIC STRUCTURE AND THE PERIODIC LAW Quantum mechanics can account for the periodic structure of the elements, by any measure a major conceptual accomplishment for any theory. Although accurate

### Experiment IV: Atomic Spectra and the Bohr model

P19: INTRODUCTORY PHYSICS III Experiment IV: Atomic Spectra and the Bohr model Department of Physics and Astronomy Dartmouth College 6127 Wilder Laboratory Hanover, NH 03755 USA Overview In this lab, we

### Arrangement of Electrons in Atoms

CHAPTER 4 Arrangement of Electrons in Atoms The emission of light is fundamentally related to the behavior of electrons. Neon Walkway The Development of a New Atomic Model T he Rutherford model of the

### Chapter 9: ELECTRONS IN ATOMS AND THE PERIODIC TABLE

Chapter 9: ELECTRONS IN ATOMS AND THE PERIODIC TABLE Problems: 1-3, 13-15, 19, 23-25, 31-32, 43, 45-46, 49c, 50a, 50b, 57c, 58 (b,c,d), 61-62, 69, 71-74, 77-88, 91-94 9.5 LIGHT: Electromagnetic Radiation

### Astronomy 110 Homework #04 Assigned: 02/06/2007 Due: 02/13/2007. Name:

Astronomy 110 Homework #04 Assigned: 02/06/2007 Due: 02/13/2007 Name: Directions: Listed below are twenty (20) multiple-choice questions based on the material covered by the lectures this past week. Choose

### Objectives. PAM1014 Introduction to Radiation Physics. Constituents of Atoms. Atoms. Atoms. Atoms. Basic Atomic Theory

PAM1014 Introduction to Radiation Physics Basic Atomic Theory Objectives Introduce and Molecules The periodic Table Electronic Energy Levels Atomic excitation & de-excitation Ionisation Molecules Constituents

### KEY. Honors Chemistry Assignment Sheet- Unit 3

KEY Honors Chemistry Assignment Sheet- Unit 3 Extra Learning Objectives (beyond regular chem.): 1. Related to electron configurations: a. Be able to write orbital notations for s, p, & d block elements.

### Note: Please use the actual date you accessed this material in your citation.

MIT OpenCourseWare http://ocw.mit.edu 5.111 Principles of Chemical Science, Fall 2005 Please use the following citation format: Sylvia Ceyer and Catherine Drennan, 5.111 Principles of Chemical Science,

### Trends of the Periodic Table Diary

Trends of the Periodic Table Diary Trends are patterns of behaviors that atoms on the periodic table of elements follow. Trends hold true most of the time, but there are exceptions, or blips, where the

### Periodic Table Questions

Periodic Table Questions 1. The elements characterized as nonmetals are located in the periodic table at the (1) far left; (2) bottom; (3) center; (4) top right. 2. An element that is a liquid at STP is

### Atomic and Nuclear Physics Laboratory (Physics 4780)

Gamma Ray Spectroscopy Week of September 27, 2010 Atomic and Nuclear Physics Laboratory (Physics 4780) The University of Toledo Instructor: Randy Ellingson Gamma Ray Production: Co 60 60 60 27Co28Ni *

### Physics 1104 Midterm 2 Review: Solutions

Physics 114 Midterm 2 Review: Solutions These review sheets cover only selected topics from the chemical and nuclear energy chapters and are not meant to be a comprehensive review. Topics covered in these

### 18.2 Comparing Atoms. Atomic number. Chapter 18

As you know, some substances are made up of only one kind of atom and these substances are called elements. You already know something about a number of elements you ve heard of hydrogen, helium, silver,

### Elements in the periodic table are indicated by SYMBOLS. To the left of the symbol we find the atomic mass (A) at the upper corner, and the atomic num

. ATOMIC STRUCTURE FUNDAMENTALS LEARNING OBJECTIVES To review the basics concepts of atomic structure that have direct relevance to the fundamental concepts of organic chemistry. This material is essential

### GRID AND PRISM SPECTROMETERS

FYSA230/2 GRID AND PRISM SPECTROMETERS 1. Introduction Electromagnetic radiation (e.g. visible light) experiences reflection, refraction, interference and diffraction phenomena when entering and passing

### Chapter 2. Quantum Theory

Chapter 2 Quantum Theory 2.0 Introduction 2.6 Orbital Shapes, Signs, and Sizes 2.1 The Nature of Light 2.7 Electron Configurations 2.2 Quantization 2.8 Quantum Theory and the Periodic Table 2.3 Bohr Model