6. There are three rules electrons normally follow when occupying orbitals in an atom. (i) Name each of these rules and then (ii) explain how each rule has an effect on the electron filling order. To illustrate these rules, (iii) draw a diagram of the electron filling pattern for oxygen. Note: Do not just write out the electron configuration; you must draw some form of diagram that explains the order electrons

6. There are three rules electrons normally follow when occupying orbitals in an atom. (i) Name each of these rules and then (ii) explain how each rule has an effect on the electron filling order. To illustrate these rules, (iii) draw a diagram of the electron filling pattern for oxygen. Note: Do not just write out the electron configuration; you must draw some form of diagram that explains the order electrons

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

Similar questions

7 please
What is the maximum number of electrons that the set of atomic orbitals shown in the image can hold? Which of the atoms cannot be represented by this set of atomic orbitals? O C N Z X
4. Explain why and what makes the spectrum of hydrogen different from the spectrum of helium.
6 please
please explain both parts 3b and 3c
Part 6: 6a. What trend in atomic radius occurs as you go up a group on the periodic table? Explain why this occurs. 6b. Write the complete electron configuration for Sr*. 6c. What element is the electron configuration for Sr+ isoelectric with? 6d. Write the abbreviated electron configuration for Bi. 6e. Write four quantum numbers to describe the highest energy electron in the Sr atom. The answer must include the four symbols and four correct numbers.
8 please
Write the ground state electron configuration and corresponding orbital diagram for each ion or neutral atom below. Do not use noble gas abbreviations for period 1, 2 or 3 elements. (HINT: Cations are formed by removing electrons from a neutral atom. Electrons are removed from more accessible orbitals first.
7- Identify the following atoms or ions from their electron configurations. a) atom: 1s 2s 2p 3s 3p 4s² 3d
Compare the configurations below with two electrons located in p orbitals. Which would be the most stable (have the lowest energy)? Which would be the least stable? Explain your answers.</o:p> </v:imagedata> </v:shape></o:p>
When more than one electron exists in an atom, the energy levels (n) split into sub-levels (s, p, d, f orbitals have different energies—even at the same n level). How electrons exist in these orbitals changes the properties of atoms. Electron configurations are either written in electron configuration notation or as an orbital diagram (boxes corresponding to orbitals of increasing energy). Write the ground state electron configuration and corresponding orbital diagram for each ion or neutral atom below. Do not use noble gas abbreviations for period 1, 2 or 3 elements.
What are the key differences in (a) energy and (b) location of electron density between a 2s orbital and a 2px orbital. Maybe a diagram to help?