Homework Help is Here – Start Your Trial Now!
Science
Chemistry
1s 2s 2p 1s 2s 2p @ 000 1s 2s 2p (11 1s 2s 2p

1s 2s 2p 1s 2s 2p @ 000 1s 2s 2p (11 1s 2s 2p

Chemistry
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...
See similar textbooks
icon
Related questions
Question
100%
The image displays four options representing electronic configurations using the Aufbau principle, showcasing the distribution of electrons in atomic orbitals. Each option consists of labeled sections for 1s, 2s, and 2p orbitals, with electrons represented by arrows. ### Options: 1. **First Option:** - **1s Orbital:** Two arrows pointing in opposite directions (up and down), indicating an electron pair. - **2s Orbital:** Two arrows pointing in opposite directions (up and down), indicating an electron pair. - **2p Orbitals:** Two arrows pointing in opposite directions (up and down) in the first circle, and two empty circles. 2. **Second Option:** - **1s Orbital:** Two arrows pointing in opposite directions (up and down). - **2s Orbital:** Two arrows pointing in opposite directions (up and down). - **2p Orbitals:** Three arrows pointing upwards, each in separate circles. 3. **Third Option:** - **1s Orbital:** Two arrows pointing in opposite directions (up and down). - **2s Orbital:** Two arrows pointing in opposite directions (up and down). - **2p Orbitals:** Four arrows, with three pointing upwards in separate circles and one paired with a downward arrow in a circle. 4. **Fourth Option:** - **1s Orbital:** Two arrows pointing in opposite directions (up and down). - **2s Orbital:** Two arrows pointing in opposite directions (up and down). - **2p Orbitals:** Each circle has one arrow pointing up. These diagrams illustrate how electrons fill the 1s, 2s, and 2p orbitals according to the rules of electron configuration, such as the Pauli exclusion principle and Hund's rule.
Transcribed Image Text:The image displays four options representing electronic configurations using the Aufbau principle, showcasing the distribution of electrons in atomic orbitals. Each option consists of labeled sections for 1s, 2s, and 2p orbitals, with electrons represented by arrows. ### Options: 1. **First Option:** - **1s Orbital:** Two arrows pointing in opposite directions (up and down), indicating an electron pair. - **2s Orbital:** Two arrows pointing in opposite directions (up and down), indicating an electron pair. - **2p Orbitals:** Two arrows pointing in opposite directions (up and down) in the first circle, and two empty circles. 2. **Second Option:** - **1s Orbital:** Two arrows pointing in opposite directions (up and down). - **2s Orbital:** Two arrows pointing in opposite directions (up and down). - **2p Orbitals:** Three arrows pointing upwards, each in separate circles. 3. **Third Option:** - **1s Orbital:** Two arrows pointing in opposite directions (up and down). - **2s Orbital:** Two arrows pointing in opposite directions (up and down). - **2p Orbitals:** Four arrows, with three pointing upwards in separate circles and one paired with a downward arrow in a circle. 4. **Fourth Option:** - **1s Orbital:** Two arrows pointing in opposite directions (up and down). - **2s Orbital:** Two arrows pointing in opposite directions (up and down). - **2p Orbitals:** Each circle has one arrow pointing up. These diagrams illustrate how electrons fill the 1s, 2s, and 2p orbitals according to the rules of electron configuration, such as the Pauli exclusion principle and Hund's rule.
**Task: Orbital Diagrams and the Pauli Exclusion Principle** **Instruction:** Select each of the orbital diagrams that are allowed according to the Pauli Exclusion Principle. **Listen Button:** (There is a button available to listen to the text.) **Explanation:** The Pauli Exclusion Principle states that no two electrons in the same atom can have identical quantum numbers. This means in any given orbital, the two electrons must have opposite spins. When reviewing orbital diagrams, ensure that no more than two electrons occupy any single orbital and that they have opposite spins. For further explanation or examples of allowed diagrams, refer to additional resources or interactive diagrams provided on the website.
Transcribed Image Text:**Task: Orbital Diagrams and the Pauli Exclusion Principle** **Instruction:** Select each of the orbital diagrams that are allowed according to the Pauli Exclusion Principle. **Listen Button:** (There is a button available to listen to the text.) **Explanation:** The Pauli Exclusion Principle states that no two electrons in the same atom can have identical quantum numbers. This means in any given orbital, the two electrons must have opposite spins. When reviewing orbital diagrams, ensure that no more than two electrons occupy any single orbital and that they have opposite spins. For further explanation or examples of allowed diagrams, refer to additional resources or interactive diagrams provided on the website.
Expert Solution
trending now

Trending now

This is a popular solution!

steps

Step by step

Solved in 3 steps

SEE SOLUTIONCheck out a sample Q&A here
Blurred answer
Knowledge Booster
Measurement
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
  • SEE MORE QUESTIONS
Recommended textbooks for you
Chemistry
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Organic Chemistry
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Elementary Principles of Chemical Processes, Bind…
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY
SEE MORE TEXTBOOKS