EBK CHEMISTRY
4th Edition
ISBN: 8220102797864
Author: Burdge
Publisher: YUZU
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Chapter 6.10, Problem 1PPC
Practice Problem
CONCEPTUALIZE
Consider again the alternate universe and its allowed values of ml from Practice Problem 6.9C. At whit
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51) Which of the following sets of quantum numbers could
represent the "last" electron added to complete the electron
configuration for the ground state atom of Br according to the
Aufbau Principle. (last electron meaning adding an electron to
form Br -1).
mi
ms
--1/2
(a)
4
-- 1/2
(b)
1
1
-- 1/2
(c)
3
1
1
+ 1/2
(d)
4
1
2
-- 1/2
(e)
2
1
ment
Paired Exercise 10.11
FULL SCREEN
PR
For each of the orbital diagrams given, write out the corresponding electron configurations (full).
Put superscripts in parentheses. (For example: correct answer for He is 1s(2), for Li - 1s(2)2s(1)). Do not leave spaces between the levels/sublevels.
11四11]
(a)
Ca
(b)
[田11111 [11111
Ar
(c)
|11 11|1|
Br
(d)
11[111111」1!1111 四1 NMM 1N
Fe
(e)
[T1[11111111[四 1111[1
t1 11t
4
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Tutored Practice Problem 7.3.1 COUNTS TOWARDS GRADE
Apply the Pauli exclusion principle.
(a) Indicate which orbitals in the following list fill before the 4s orbital.
3s yes 3p yes ✓ 3d no 4p no v
(b) What is the maximum number of electrons in the 6d subshell?
(c) An electron in an orbital has the following quantum numbers: n = 4, l=3, me = 0, and m, = +12.
Identify the type orbital.
What is the direction of the electron spin?
Check & Submit Answer
C
H
Show Approach 5 attempts remaining
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Chapter 6 Solutions
EBK CHEMISTRY
Ch. 6.1 - Practice ProblemATTEMPT What is the frequency (in...Ch. 6.1 - Prob. 1PPBCh. 6.1 - Practice Problem CONCEPTUALIZE
Which of the...Ch. 6.1 - Prob. 1CPCh. 6.1 - Calculate the frequency of light with wavelength...Ch. 6.1 - Prob. 3CPCh. 6.1 - Prob. 4CPCh. 6.2 - Practice Problem ATTEMPT
Calculate the difference...Ch. 6.2 - Prob. 1PPBCh. 6.2 - Prob. 1PPC
Ch. 6.2 - Prob. 1CPCh. 6.2 - Prob. 2CPCh. 6.2 - Prob. 3CPCh. 6.2 - Prob. 4CPCh. 6.3 - Prob. 1PPACh. 6.3 - Practice Problem BUILD
(a) Calculate the...Ch. 6.3 - Prob. 1PPCCh. 6.3 - Prob. 1CPCh. 6.3 - Prob. 2CPCh. 6.3 - Prob. 3CPCh. 6.3 - Prob. 4CPCh. 6.4 - Prob. 1PPACh. 6.4 - Prob. 1PPBCh. 6.4 - Prob. 1PPCCh. 6.4 - Prob. 1CPCh. 6.4 - Prob. 2CPCh. 6.5 - Practice ProblemATTEMPT Calculate the de Broglie...Ch. 6.5 - Prob. 1PPBCh. 6.5 - Prob. 1PPCCh. 6.5 - What is the minimum uncertainty in the position of...Ch. 6.5 - Prob. 2CPCh. 6.6 - Prob. 1PPACh. 6.6 - Prob. 1PPBCh. 6.6 - Prob. 1PPCCh. 6.6 - Prob. 1CPCh. 6.6 - Prob. 2CPCh. 6.6 - Prob. 3CPCh. 6.6 - Prob. 4CPCh. 6.7 - Practice Problem ATTEMPT
(a) What are the possible...Ch. 6.7 - Practice ProblemBUILD (a) What is the lowest...Ch. 6.7 - Practice Problem CONCEPTUALIZE
Imagine a cobbler's...Ch. 6.7 - Prob. 1CPCh. 6.7 - Prob. 2CPCh. 6.7 - Prob. 3CPCh. 6.7 - Prob. 4CPCh. 6.8 - Prob. 1PPACh. 6.8 - Prob. 1PPBCh. 6.8 - Prob. 1PPCCh. 6.8 - Prob. 1CPCh. 6.8 - What element is represented by the following...Ch. 6.8 - Which orbital diagram is correct for the...Ch. 6.9 - Practice Problem ATTEMPT
Write the electron...Ch. 6.9 - Prob. 1PPBCh. 6.9 - Prob. 1PPCCh. 6.9 - Prob. 1CPCh. 6.9 - Prob. 2CPCh. 6.9 - 6.9.3 Which of the following is a d-block element?...Ch. 6.9 - Prob. 4CPCh. 6.10 - Practice ProblemATTEMPT Without referring to...Ch. 6.10 - Practice ProblemBUILD Without referring to Figure...Ch. 6.10 - Practice ProblemCONCEPTUALIZE Consider again the...Ch. 6 - Key Skills Problems What is the noble gas core for...Ch. 6 - Which of the following electron configurations...Ch. 6 - What element is represented by the electron...Ch. 6 - What is the electron configuration of the Lu atom?...Ch. 6 - What is a wave? Using a diagram, define the...Ch. 6 - 6.2 What are the units for wavelength and...Ch. 6 - List the types of electromagnetic radiation having...Ch. 6 - 6.4 Give the high and low wavelength values that...Ch. 6 - (a) What is the wavelength (in nm) of light having...Ch. 6 - 6.6 (a) What is the frequency of light having a...Ch. 6 - 6.7 The SI unit of time is the second, which is...Ch. 6 - 6.8 How many minutes would it take a radio wave to...Ch. 6 - The average distance between Mars and Earth is...Ch. 6 - 6.10 Four waves represent light in four different...Ch. 6 - Briefly explain Planck’s quantum theory and...Ch. 6 - Prob. 12QPCh. 6 - 6.13 Explain what is meant by the photoelectric...Ch. 6 - 6.14 What are photons? What role did Einstein’s...Ch. 6 - A photon has a wavelength of 705 nm. Calculate the...Ch. 6 - The blue color of the sky results from the...Ch. 6 - 6.17 A photon has a frequency of . (a) Convert...Ch. 6 - What is the wavelength (in nm) of radiation that...Ch. 6 - When copper is bombarded with high energy...Ch. 6 - 6.20 A particular form of electromagnetic...Ch. 6 - The retina of a human eye can detect light when...Ch. 6 - The radioactive 60 Co isotope is used in nuclear...Ch. 6 - Photosynthesis makes use of visible light or bring...Ch. 6 - A red light was shined onto a metal sample and the...Ch. 6 - A photoelectric experiment was performed by...Ch. 6 - What are emission spectra? How do line spectra...Ch. 6 - What is an energy level? Explain the difference...Ch. 6 - Briefly describe Bohr's theory of the hydrogen...Ch. 6 - The first line of the Balmer series occurs at a...Ch. 6 - 6.30 Calculate the wavelength (in nm) of a photon...Ch. 6 - Calculate the frequency (Hz) and wavelength (nm)...Ch. 6 - Careful spectral analysis shows that the familiar...Ch. 6 - 6.33 An electron in the hydrogen atom makes a...Ch. 6 - 6.34 Consider the following energy levels of a...Ch. 6 - Some copper compounds emit green light when they...Ch. 6 - Is it possible for a fluorescent material to emit...Ch. 6 - Explain how astronomers are able to tell which...Ch. 6 - How does do Broglie's hypothesis account for the...Ch. 6 - 6.39 Why is Equation 6.9 meaningful only for...Ch. 6 - Does a baseball in flight possess wave properties?...Ch. 6 - 6.41 Thermal neutrons are neutrons that move at...Ch. 6 - Protons can be accelerated to speeds near that of...Ch. 6 - 6.43 What is the de Broglie wavelength (in cm) of...Ch. 6 - 6.44 What is the de Broglie wavelength (in nm)...Ch. 6 - Prob. 45QPCh. 6 - Prob. 46QPCh. 6 - Prob. 47QPCh. 6 - How is the concept of electron density used to...Ch. 6 - 6.49 What is an atomic orbital? How does an atomic...Ch. 6 - 6.50 Alveoli are tiny sacs of air in the lungs....Ch. 6 - 6.51 The speed of a thermal neutron (see Problem...Ch. 6 - 6.52 In the beginning of the twentieth century,...Ch. 6 - Prob. 53QPCh. 6 - Prob. 54QPCh. 6 - Which quantum number defines a shell? Which...Ch. 6 - Prob. 56QPCh. 6 - Prob. 57QPCh. 6 - Prob. 58QPCh. 6 - Prob. 59QPCh. 6 - Prob. 60QPCh. 6 - Prob. 61QPCh. 6 - 6.62 List the hydrogen orbitals in increasing...Ch. 6 - Prob. 63QPCh. 6 - Prob. 64QPCh. 6 - Prob. 65QPCh. 6 - Give the values of the four quantum numbers of an...Ch. 6 - Prob. 67QPCh. 6 - Prob. 68QPCh. 6 - Why do the 3s, 3p, and 3d orbitals have the same...Ch. 6 - Prob. 70QPCh. 6 - Prob. 71QPCh. 6 - Prob. 72QPCh. 6 - Prob. 73QPCh. 6 - Prob. 74QPCh. 6 - Prob. 75QPCh. 6 - Prob. 76QPCh. 6 - Prob. 77QPCh. 6 - Prob. 78QPCh. 6 - Prob. 79QPCh. 6 - Prob. 80QPCh. 6 - Prob. 81QPCh. 6 - Prob. 82QPCh. 6 - Indicate the number of unpaired electrons present...Ch. 6 - Prob. 84QPCh. 6 - Prob. 85QPCh. 6 - Prob. 86QPCh. 6 - Describe the characteristics of transition metals.Ch. 6 - What is the noble gas core? How does it simplify...Ch. 6 - Prob. 89QPCh. 6 - Prob. 90QPCh. 6 - 6.91 Explain why the ground-state electron...Ch. 6 - 6.92 Write the electron configuration of a xenon...Ch. 6 - Prob. 93QPCh. 6 - Prob. 94QPCh. 6 - Prob. 95QPCh. 6 - Prob. 96QPCh. 6 - 6.97 Write the ground-state electron...Ch. 6 - Prob. 98APCh. 6 - Discuss the current view of the correctness of the...Ch. 6 - Distinguish carefully between the following terms:...Ch. 6 - Prob. 101APCh. 6 - Identify the following individuals and their...Ch. 6 - Prob. 103APCh. 6 - Prob. 104APCh. 6 - Prob. 105APCh. 6 - Prob. 106APCh. 6 - Prob. 107APCh. 6 - 6.108 Ionization energy is the minimum energy...Ch. 6 - Prob. 109APCh. 6 - Prob. 110APCh. 6 - Prob. 111APCh. 6 - All molecules undergo vibrational motions. Quantum...Ch. 6 - When an electron makes a transition between energy...Ch. 6 - Prob. 114APCh. 6 - Prob. 115APCh. 6 - Prob. 116APCh. 6 - 6.11 The wave function for the is orbital in the...Ch. 6 - Prob. 118APCh. 6 - Prob. 119APCh. 6 - Prob. 120APCh. 6 - 6.121 Calculate the wavelength and frequency of an...Ch. 6 - Prob. 122APCh. 6 - 6.123 In a photoelectric experiment a student uses...Ch. 6 - Prob. 124APCh. 6 - Prob. 125APCh. 6 - Prob. 126APCh. 6 - Prob. 127APCh. 6 - Prob. 128APCh. 6 - Prob. 129APCh. 6 - Prob. 130APCh. 6 - Prob. 131APCh. 6 - Prob. 132APCh. 6 - 6.133 Blackbody radiation is the term used to...Ch. 6 - Prob. 134APCh. 6 - Prob. 135APCh. 6 - How many photons at 586 nm must be absorbed to...Ch. 6 - Prob. 137APCh. 6 - Prob. 1SEPPCh. 6 - Prob. 2SEPPCh. 6 - What is the energy of a photon with wavelength λ...Ch. 6 - The visible region of the electromagnetic spectrum...
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- State which of the following sets of quantum numbers would be possible and which impossible for an electron in an atom. a n = 2, I = 0, mi = 0, ms=+12 b n = 1, I = 1, mi = 0, ms=+12 c n = 0, I = 0, mi = 0, ms=12 d n = 2, I = 1, mi = 1, ms=+12 e n = 2, I = 1, mi = 2, ms=+13arrow_forwardWithout referring to your text, predict the trend of second ionization energies for the elements sodium through argon. Compare your answer with Table 2-5. Explain any differences.arrow_forwardWhat is the maximum number of orbitals that can be identified by each of the following sets of quantum numbers? When none is the correct answer, explain your reasoning. (a) n = 3, = 0, m = +1 (b) n = 5, = 1, (c) n = 7, = 5, (d) n = 4, = 2, m = 2arrow_forward
- Explain briefly why each of the following is not a possible set of quantum numbers for an electron in an atom. In each case, change the incorrect value (or values) to make the set valid. (a) n = 4, = 2, m = 0, ms = 0 (b) n = 3, = 1, m = 3, ms = 1/2 (c) n = 3, = 3, m = 1, ms = +1/2arrow_forwardExplain why each of the following sets of quantum numbers would not be permissible for an electron, according to the rules for quantum numbers. a n = 1, I = 0, mi = 0, ms = +1 b n = 1, I = 3, mi = +3, ms=+12 c n = 3, I = 2, mi = +3, ms=12 d n = 0, I = 1, mi = 0, ms=+12 e n = 2, I = 0, mi = 1, ms=+32arrow_forwardin order of increasing energy. Indicate which of these two configurations for an atom either because they violate the Pauli exclusion principle or because orbitals are not filled principles is violated in each example. (a) [Ne]3s²3p°3d° 6.79 The following do not represent valid ground-state electron configurations for an atom either because they violate the Pauli exclusion principle or because orbitals are not filled principles is violated in each example. (a) [Ne]3s²3p°3d (b) [Xe]6s³ (c) 1s²3s'.arrow_forward
- How many orbitals in an atom could have quantum numbers | = 2 and ml = -3? (A) 0 (B) 1 (C) 2 (D) 5arrow_forward4. Chemists can identify the composition of some unknown salts by conducting a flame test. When potassium salts are heated in a flame, a purple color is observed. This is due to the movement of electrons between energy levels. What is the electron configuration of a potassium atom at ground state? (A) 1s²2s²2p63s²3p°4d! (B) 1s²2s²2p°3s?3p°3d1 (C) 1s²2s²2d®3s²3d$4s! (D) 1s²2s²2p®3s?3p°4s' atoms of gold (Au). In a 3.7-gram sample, there are (A) 1.1 x 1022 atoms of gold (B) 3.2 x 1025 atoms of gold (C) 4.4 x 1026 atoms of gold (D) 3.1 x 10-26 atoms of gold 5. 6. Which total mass is the largest? (A) The mass of 2 electrons (B) The mass of 2 neutrons (C) The mass of 1 electron plus the mass of 1 proton (D) The mass of 1 neutron plus the mass of 1 electronarrow_forwardChemists can identify the composition of some unknown salts by conducting a flame test. Whenpotassium salts are heated in a flame, a purple color is observed. This is due to the movement ofelectrons between energy levels. What is the electron configuration of a potassium atom at groundstate?(A) 1s22s22p63s23p64d1(B) 1s22s22p63s23p63d1(C) 1s22s22d63s23d64s1(D) 1s22s22p63s23p64s1arrow_forward
- 4. Chemists can identify the composition of some unknown salts by conducting a flame test. When potassium salts are heated in a flame, a purple color is observed. This is due to the movement of electrons between energy levels. What is the electron configuration of a potassium atom at ground state? (A) 1s 2s 2p 3s23p 4d (B) 1s 25 2p 3s23p 3d (C) 1s²2s 2d63s23d64s (D) 1s²2s²2p 3s23p 4s ate EducationT, Inc.arrow_forwardUsing complete subshell notation (e.g., 1s2 2s2 2p6, and so forth, not abbreviations), predict the electron configuration of each of the following atoms. (a) Mg (b) Al (c) Sm (d) O (e) Nbarrow_forwardWhat's More (B) Activity 2.2: ldentify the orbital Directions: For the table below, write which orbital goes with the quantum numbers. If the quantum numbers are not allowed, write "not allowed." mi Orbital -1 2p (example) 0. 0. -3 -2 0. -1 0. 0. 1. 2133204arrow_forward
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