QF4Which electron is, on average, closer to the nucleus: an electron in a 2s orbital or an electron in a 3s orbital?Match the words in the left column to the appropriate blanks in the sentences on the right.SubmitProvide Feedback%5TG9F5Bmi2s38increases6decreases1nRequest AnswerYcMacBook AirF6H&7NThe size of the orbital is determined by thethe nucleus than is an electron in a<F7* 00J8이UMas this value increases. Therefore, an electron in aDIIF8K(9F9VOş)OLorbital.quantum number, so the size of the orbitalorbital is closer toF10PAF11لال{?+ 11Reset Help=Show All»)F12Next >}d

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Which electron is, on average, closer to the nucleus: an electron in a 2s orbital or an electron in a 3s orbital? Match the words in the left column to the appropriate blanks in the sentences on the right. Submit Provide Feedback mi 28 38 increases decreases 1 n Request Answer The size of the orbital is determined by the as this value increases. Therefore, an electron in a the nucleus than is an electron in a orbital. Reset Help quantum number, so the size of the orbital orbital is closer to Next

Which electron is, on average, closer to the nucleus: an electron in a 2s orbital or an electron in a 3s orbital? Match the words in the left column to the appropriate blanks in the sentences on the right. Submit Provide Feedback mi 28 38 increases decreases 1 n Request Answer The size of the orbital is determined by the as this value increases. Therefore, an electron in a the nucleus than is an electron in a orbital. Reset Help quantum number, so the size of the orbital orbital is closer to Next

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Which transition emits the highest energy photons? -- Multiple choice A → B A → C B → C B → A C → A C → B
t ot pt pt pt 1 pt 1 pt 1 pt 1 pt at 1 pt 3 1 pt 1 pt 1 pt What is the maximum number of orbitals that can be identified by the following set of quantum numbers? Note that in cases where the set of quantum numbers is not "allowed," the answer will be zero. a. n = 2, l = 2, me = 0 orbital(s) 1 pt gnment b. n = 4 Submit Answer orbital(s) Try Another Version [References] 10 item attempts remaining Cengage Learning Cengage Technical Support the new Terms and Conditions. MacBook Pro Previous Next Save and Exit
What is the smallest possible value of the principal quantum number n for a p electron? TOCAMLAGI Jobinel 11 = Continue 0 1-95 S/US-1 S/... Closed road X 3 Q Search S 2023 McGraw Hill LLC
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Part A Cs Express your answer in condensed form in the order of orbital filling as a string without blank space between orbitals. For example, He 2s 2p should be entered as [He]2s^22p^2. [Xe]6s^1 Previous Answers V Correct Our first step is to write the noble-gas core We do this by locating cesium, element 55, in the periodic table. We then move backward to the nearest noble gas, which is Xe, element 54 Thus, the noble-gas core is Xe. Next, we trace the path in order of incre Moving from Xe to Cs, element 55, we find ourselves in period six of the s block. Knowing the block and the period identifies the subshell in which we begin placing outer electrons, 6s. As we move through the s block, we add one electron, giving us Xe 6s Рart B Ni Express your answer in condensed form in the order of orbital filling as a string without blank space between orbitals. For example, Hel2s 2p should be entered as [He]2s^22p 2. Submit Request Answer Part C Se Express your answer in condensed form in the…
esc Page 1: 1 4 ! 7 10 13 16 2 19 5 ✓ 8 9 11 12 HAB 14 15 17 18 11 20 21 S 22 23 24 25 26 27 D F1 3 6 ! F2 Answer the following question by matching the numbers with the descriptions. Numbers may be used more than once. Not all the numbers will be used. 1. 1 2. 2 3. 3 4. 4 5. 5 6. 6 The number of orbitals in a 4d subshell or sublevel 7. 7 The number of electrons in a full 5p orbital. 8. 8 The number of electrons in 9. 9 a full 3d subshell or sublevel 10. 10 80 F3 F4 F5 MacBook Air F6 AA F7 DII F8 A F9 F10 F11
When writing the ground-state electron configuration of a many-electron atom, three main rules must be followed: . The aufbau principle: Electrons are added to the lowest energy orbitals available. . The Pauli exclusion principle: No two electrons in an atom can have the same set of four quantum numbers (n. l. me, and m₂). • Hund's rule: For degenerate orbitals, the lowest energy state is attained when the number of electrons with the same spin is maximized. So for a degenerate set of orbitals, one electron goes into each orbital until all the orbitals of the subshell are half-filled. Once all the orbitals of the subshell are half-filled the pairing of electrons can take place. Note that aufbau is the German word for "building up." ▾ Part A Classify each orbital diagram for ground-state electron configurations by the rule or principle it violates. Drag the appropriate items to their respective bins. View Available Hint(s) Aufbau violation 3p 111 3p 111 3p 11 3s 11 45 1 Hund violation…
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Complete the table describing orbitals in the n=4 energy level: l Possible ml values Orbital name(s) 0 0 4s (1 orbital) 1 -1, 0, +1 ____ (3 orbitals) 2 ____ (__ orbitals) 3 ____ (__ orbitals) Total number of orbitals = ________ Maximum number of electrons in the n = 4 energy level = __________