1. Identify what is being referred by the following: Main energy level of an orbital. A.Principal Quantum Number B.Spin quantum number C.Magnetic Quantum Number D.Azimuthal Quantum Number 2. These are the four sets of numbers wherein each is unique to an element: A.Electron Orbital B.Valence Configuration C.Quantum Numbers D.Aufbau Principle

1. Identify what is being referred by the following: Main energy level of an orbital. A.Principal Quantum Number B.Spin quantum number C.Magnetic Quantum Number D.Azimuthal Quantum Number 2. These are the four sets of numbers wherein each is unique to an element: A.Electron Orbital B.Valence Configuration C.Quantum Numbers D.Aufbau Principle

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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Using complete subshell notation, match the predicted electron configuration of each of the following atoms. (match one from the top (letter) to one at the bottom (number). a. Sb b. P c. Sm d. V e. C 1. 1s22s22p63s23p3 2. 1s22s22p63s23p63d104s24p64d105s25p3 3. 1s22s22p2 4. 1s22s22p63s23p63d104s24p64d105s25p66s24f6 5. 1s22s22p63s23p64s23d3
О Which of the statements most accurately describes the following electron configuration? 1 ↓ 1 a. It is a valid configuration for a ground state atom. b. It violates the aufbau principle. c. It is invalid and violates multiple rules/principles. d. It violates the Pauli exclusion principle. e. It violates Hund's rule.
For an electronic transition from n = 5 to n = 3 in the Bohr hydrogen atom, answer the following questions:a. Calculate the energy (in J) required for such transition b. Calculate the wavelength (in nm) associated with this transition. c. Does this transition correspond to absorption or emission of light? d. What region of the electromagnetic spectrum does this occur in?
1. How many unpaired electrons are in the carbon atom? A. Paramagnetic B. Diamagnetic This atom is 2. How many unpaired electrons are in the cobalt atom? A. Paramagnetic B. Diamagnetic This atom is
9
11. What is the most likely electron configuration for a sodium ion in its ground state? a. 1S² 2S² 2P5 b. 1S² 2S² 2P6 c. 1S22S2 2P 3S1 d. 1S2 2S2 2P5 3S² e. 1S22S2 2P6 3S² 12. Which of the following atoms is in an excited state? a. 1s² 2s² 2p¹ b. 1s² 2s² 2p4 c. 1s2 2s² 2p5 3s¹ d. 1s² 2s² 2p 3s² e. 1s2 2s² 2p 3s² 3p²
Give the number of valence electrons in each element. Write out the electronic confi guration for the valence electrons. a. neon b. rubidium c. aluminum d. manganese
The lowest energy level in an atom is a. the absolute zero temperature. b. the ground state. c. the ionization level. d. responsible for Doppler shifts. e. the energy level from which the Paschen series of hydrogen originates.
How many nodal surfaces are associated with the following orbitals? a. 4s orbital nodal surface(s) b. 2s orbital nodal surface(s) c. 2p orbital nodal surface(s)
16. The n = 1 shell contains p sub-orbitals. All the other shells contains p sub- orbitals. A.3,6 B. 0,3 C: 6,2 D. 3,3 17. How many orbitals are their in the second shell? OF A.1 B. 2 C 4 D. 8 18. Which of the orbitals below do not exist due to the constraints upon the angular quantum number? A.3f B. 2p C. 2s D. 2d 19. Which of the orbitals below do not exist due to the constraints upon the angular quantum number? A.3d B. 3p C. 3s D. 3f 20. Which one of the following is an incorrect orbital notation? A.4f B.2d C. 3s D.2p
Which rule states that the electrons go in singularly until you half fill the orbital set then begin pairing of electrons? A. Hunds Rule B. Paul Exclusion principle C. Bohrs Rule D. Aufbau Principle
4 n-electrons are moving in a square-box of length 2.15 Å. Assuming the validity of the particle-in-a box model, calculate the wavelength (nm) of the photon needed to excite the electrons from the HOMO to the LUMO. a. 76 b. 110 c. 89 d. 100 e. 51