Match the principle/rule with the correct statement.No two electrons in thesame atom can have alltheir quantum numbers thesame.1. The Aufbau PrincipleElectrons are placed intoorbitals from the lowestenergy to the highest2. Hund's Ruleenergy.3. The Pauli Exclusion PrincipleAll orbitals of the samesubshell must have oneelectron before any.electrons are paired.

Aufbau, Hund's and Pauli exclusion principles are related to the atomic orbitals they define the…

Match the principle/rule with the correct statement. No two electrons in the same atom can have all their quantum numbers the same. 1. The Aufbau Principle Electrons are placed into orbitals from the lowest 2. Hund's Rule energy to the highest energy. 3. The Pauli Exclusion Principle All orbitals of the same subshell must have one electron before any. electrons are paired.

Match the principle/rule with the correct statement. No two electrons in the same atom can have all their quantum numbers the same. 1. The Aufbau Principle Electrons are placed into orbitals from the lowest 2. Hund's Rule energy to the highest energy. 3. The Pauli Exclusion Principle All orbitals of the same subshell must have one electron before any. electrons are paired.

Living By Chemistry: First Edition Textbook

1st Edition

ISBN:9781559539418

Author:Angelica Stacy

Publisher:Angelica Stacy

ChapterU1: Alchemy: Matter, Atomic Structure, And Bonding

SectionU1.24: Shell Game: Electron Configurations

Problem 9E

See similar textbooks

Similar questions

Suppose that the spin quantum number could have the values 12,0 and 12 . Assuming that the rules governing the values of the other quantum numbers and the order of filling sublevels were unchanged, (a) what would be the electron capacity of an s sublevel? a p sublevel? a d sublevel? (b) how many electrons could fit in the n=3 level? (c) what would be the electron configuration of the element with atomic number 8? 17?
Consider the representations of the p and d atomic orbitals in Figs. 2-15 and 2- 17. What do the + and signs indicate?
Answer the following questions, assuming that ms, could have three values rather than two and that the rules for n, l, and ml are the normal ones. a. How many electrons would an orbital be able to hold? b. How many elements would the first and second periods in the periodic table contain? c. How many elements would be contained in the first transition metal series? d. How many electrons would the set of 4f orbitals be able to bold?
Construct an energy level diagram showing all orbitals for the hydrogen atom up to n=5, labeling each orbital with its appropriate quantum numbers. How many different orbitals are in each shell?
Consider the following representation of a set of p orbitals for an atom: mg src=Images/HTML_99425-11-30QAP_image001.jpg alt="" align="top"/> ich of the following statements is(are) true? The areas represented by the p orbitals are positively charged clouds with negatively charged electrons embedded within these clouds. The nucleus is located at the center point of each axis. The electrons move along the elliptical paths as indicated by the p orbitals above. The atom could not be hydrogen because its electron is found in the 1s orbital.
The outermost electron in an alkali-metal atom is sometimes described as resembling an electron in the corresponding state of a one-electron atom. Compare the first ionization energy of lithium with the binding energy of a 2s electron in a one-electron atom that has nuclear charge Zeff , and determine the value of Zeff that is necessary for the two energies to agree. Repeat the calculation for the 3s electron of sodium and the 4s electron of potassium.
Which atom would be expected to have a half-filled 4s subshell?