Organic Chemistry: Principles and Mechanisms (Second Edition)
2nd Edition
ISBN: 9780393663556
Author: Joel Karty
Publisher: W. W. Norton & Company
expand_more
expand_more
format_list_bulleted
Concept explainers
Question
Chapter 1, Problem 1.1YT
Interpretation Introduction
Interpretation:
Orbitals designation and electron number in the second shell are to be determined.
Concept introduction:
Electronic configuration is the arrangement of electrons in an atomic orbital. This electronic configuration mainly depends on three principles. In Pauli’s exclusion principle, two electrons must have an opposite spin, and it does not contain the same set of quantum numbers. Aufbau’s principle tells that electrons must be filled first in the lower energy orbital. According to Hund’s rule, all electrons at the same energy must contain single electron in it, or it will be half filled.
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solutionStudents have asked these similar questions
Here are the atomic radii (in pm) for the third row of
the periodic table:
Na Mg Al Si P S CI Ar
186 160 143 118 110 103 100 98
Another property of atoms is called the ionization
energy. It is the energy required to remove an electron
from an atom in the gas phase.
Here is a table of the first ionization energies (energy
required to remove the outermost electron) for the
third row of the periodic table (in kJ/mol):
Na Mg Al Si P S CI Ar
496 738 577 788 1060
1000
1258
1520
Directions: On a separate sheet of paper. Answer the following problems.
1. Give the electron configuration of Be. Draw the orbital diagram.
2. Give the electron configuration of B. Draw the orbital diagram.
What is Hund’s rule?Choice one from below.
1)The lowest energy is obtained if the number of electrons with different spins is maximized.
2)The lowest energy is obtained if the number of electrons with the same spin is maximized.
3)The highest energy is obtained if electrons are only placed in s orbitals.
4)The number of electrons in p orbitals must be half the atomic number Z.
Chapter 1 Solutions
Organic Chemistry: Principles and Mechanisms (Second Edition)
Ch. 1 - Prob. 1.1PCh. 1 - Prob. 1.2PCh. 1 - Prob. 1.3PCh. 1 - Prob. 1.4PCh. 1 - Prob. 1.5PCh. 1 - Prob. 1.6PCh. 1 - Prob. 1.7PCh. 1 - Prob. 1.8PCh. 1 - Prob. 1.9PCh. 1 - Prob. 1.10P
Ch. 1 - Prob. 1.11PCh. 1 - Prob. 1.12PCh. 1 - Prob. 1.13PCh. 1 - Prob. 1.14PCh. 1 - Prob. 1.15PCh. 1 - Prob. 1.16PCh. 1 - Prob. 1.17PCh. 1 - Prob. 1.18PCh. 1 - Prob. 1.19PCh. 1 - Prob. 1.20PCh. 1 - Prob. 1.21PCh. 1 - Prob. 1.22PCh. 1 - Prob. 1.23PCh. 1 - Prob. 1.24PCh. 1 - Prob. 1.25PCh. 1 - Prob. 1.26PCh. 1 - Prob. 1.27PCh. 1 - Prob. 1.28PCh. 1 - Prob. 1.29PCh. 1 - Prob. 1.30PCh. 1 - Prob. 1.31PCh. 1 - Prob. 1.32PCh. 1 - Prob. 1.33PCh. 1 - Prob. 1.34PCh. 1 - Prob. 1.35PCh. 1 - Prob. 1.36PCh. 1 - Prob. 1.37PCh. 1 - Prob. 1.38PCh. 1 - Prob. 1.39PCh. 1 - Prob. 1.40PCh. 1 - Prob. 1.41PCh. 1 - Prob. 1.42PCh. 1 - Prob. 1.43PCh. 1 - Prob. 1.44PCh. 1 - Prob. 1.45PCh. 1 - Prob. 1.46PCh. 1 - Prob. 1.47PCh. 1 - Prob. 1.48PCh. 1 - Prob. 1.49PCh. 1 - Prob. 1.50PCh. 1 - Prob. 1.51PCh. 1 - Prob. 1.52PCh. 1 - Prob. 1.53PCh. 1 - Prob. 1.54PCh. 1 - Prob. 1.55PCh. 1 - Prob. 1.56PCh. 1 - Prob. 1.57PCh. 1 - Prob. 1.58PCh. 1 - Prob. 1.59PCh. 1 - Prob. 1.60PCh. 1 - Prob. 1.61PCh. 1 - Prob. 1.62PCh. 1 - Prob. 1.63PCh. 1 - Prob. 1.64PCh. 1 - Prob. 1.65PCh. 1 - Prob. 1.66PCh. 1 - Prob. 1.67PCh. 1 - Prob. 1.68PCh. 1 - Prob. 1.69PCh. 1 - Prob. 1.70PCh. 1 - Prob. 1.71PCh. 1 - Prob. 1.72PCh. 1 - Prob. 1.73PCh. 1 - Prob. 1.74PCh. 1 - Prob. 1.75PCh. 1 - Prob. 1.76PCh. 1 - Prob. 1.77PCh. 1 - Prob. 1.78PCh. 1 - Prob. 1.79PCh. 1 - Prob. 1.80PCh. 1 - Prob. 1.81PCh. 1 - Prob. 1.82PCh. 1 - Prob. 1.1YTCh. 1 - Prob. 1.2YTCh. 1 - Prob. 1.3YTCh. 1 - Prob. 1.4YTCh. 1 - Prob. 1.5YTCh. 1 - Prob. 1.6YTCh. 1 - Prob. 1.7YTCh. 1 - Prob. 1.8YTCh. 1 - Prob. 1.9YTCh. 1 - Prob. 1.10YTCh. 1 - Prob. 1.11YTCh. 1 - Prob. 1.12YTCh. 1 - Prob. 1.13YTCh. 1 - Prob. 1.14YTCh. 1 - Prob. 1.15YTCh. 1 - Prob. 1.16YTCh. 1 - Prob. 1.17YT
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Similar questions
- Finish the electron configuration with arrows instead of the written version.arrow_forward' For a cobalt (Co) atom in its ground electronic state: How many electrons are there in the 4s orbital? . Number (Enter an integer.) (Enter an integer.) How many electrons are there in the 3d orbitals? - Number (Enter an integer.) How many electrons are there in the 4p orbitals? Number How many unpaired electrons are there? Number (Enter an integer.) To what block does this atom belong? (Enter s, p, d, or f.)arrow_forwardDirection: Complete the table by filling up the correct quantum number and corresponding atomic orbital.arrow_forward
- Ni Express your answer in condensed form in the order of orbital filling as a string without blank space between orbitals.arrow_forwardShown below are three valence-shell electron diagrams showing electron configurations and spin directions represented by arrows. Only the valence shell of the atom is intended to be depicted by these diagrams. Figure out which of these three diagrams (top, middle, or bottom diagram) is correct for the valence shell of Se and how many unpaired electrons an atom of Se has. a) Se has the valence shell depicted in the bottom diagram with 0 unpaired electrons. b) Se has the valence shell depicted in the top diagram with 2 unpaired electrons. c) Se has the valence shell depicted in the bottom diagram with 4 unpaired electrons. d) Se has the valence shell depicted in the middle diagram with 2 unpaired electrons. e) Se has the valence shell depicted in the middle diagram with 0 unpaired electrons.arrow_forwardExamine the radial factor, R(r), and 95% probability surface below for a particular orbital of the hydrogen atom. What is the correct orbital designation for this orbital? R(r) y r Enter the appropriate n value: Select the appropriate subshell and orientation: [ ] Px [ ] Ру [ ] Pz [ ] dxy [ ] dxz [ ] dyz [ ] dy2-y2 [ ] dz2 [ ]arrow_forward
- Suppose you have an h-orbital. How many ml values would be possible?arrow_forwardUsing Fig. 2-30, list the elements (ignore the lanthanides and actinides) that have ground-state electron configurations that differ from those we would expect from their positions in the periodic table.arrow_forwardHow many nodal planes exist for a 5d orbital? (a) 0 (b) 1 (c) 2 (d) 3arrow_forward
- Identification. Directions: Supply the correct term described in each number. 1. It is the quantum number that represents the energy level the electron is in. 2. It is a representation of the wave function of a hydrogen-like atom. 3. It is a quantum number that represents the shape of orbitals. 4. It is the particle that can be described by four quantum numbers 5. It represents the quantum number that describes the orientation of an orbital. 6. It is being represented by n. 7. It is the shape of the s orbital. 8. Each orbital is represented by a square (or circle), and the electrons as arrows pointing up or down (indicating the electron spin). 9. The distribution of electrons among the orbitals of an atom. 10. The electrons are filled in according to a scheme known as "building-up".arrow_forward(Q1). Out of these atoms (S,N,Mn, Ni) determine which one has the most unpaired electrons in its ground state electron configuration.arrow_forwardWhich of the following atoms and ions has the correct condensed electron configuration? (Note: The ordering with which the orbitals are written is not important) Check ALL the apply. There are penalties for incorrect answers. C2-: [He] 2s2 2p4 Sb: [Kr] 5s2 4d10 5p3 Na: [Ne] 2s1 Na2+: [He] 2s2 2p5arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
- Chemistry & Chemical ReactivityChemistryISBN:9781133949640Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage LearningChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage Learning
- World of Chemistry, 3rd editionChemistryISBN:9781133109655Author:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCostePublisher:Brooks / Cole / Cengage LearningLiving By Chemistry: First Edition TextbookChemistryISBN:9781559539418Author:Angelica StacyPublisher:MAC HIGHER
Chemistry & Chemical Reactivity
Chemistry
ISBN:9781133949640
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:Cengage Learning
Chemistry
Chemistry
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Chemistry: An Atoms First Approach
Chemistry
ISBN:9781305079243
Author:Steven S. Zumdahl, Susan A. Zumdahl
Publisher:Cengage Learning
World of Chemistry, 3rd edition
Chemistry
ISBN:9781133109655
Author:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste
Publisher:Brooks / Cole / Cengage Learning
Living By Chemistry: First Edition Textbook
Chemistry
ISBN:9781559539418
Author:Angelica Stacy
Publisher:MAC HIGHER