Write the electron configurations for the following elements using spectroscopic (spdf) and orbital box notation. Identify the element as paramagnetic or diamagnetic. (a) Fe, iron Full electron configuration = (do not use noble gas notation) Orbital box notation: Зd 4s Зр 3s 2p 2s 1s Fe is (b) Se, selenium Noble gas electron configuration = Orbital box notation: 4p Se is

Write the electron configurations for the following elements using spectroscopic (spdf) and orbital box notation. Identify the element as paramagnetic or diamagnetic. (a) Fe, iron Full electron configuration = (do not use noble gas notation) Orbital box notation: Зd 4s Зр 3s 2p 2s 1s Fe is (b) Se, selenium Noble gas electron configuration = Orbital box notation: 4p Se is

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. Electron Configuration. Write the electron configurations for (a) oxygen and (b) sulfur. What do the electron configurations of these two elements have in common?
7. Transition elements come from the d block. Examples of d block elements are manganese, cobalt, iron, copper, scandium and zinc. (a) Write the electron configurations for the atoms and ions of manganese and cobalt below. Mn atom: 1s? Co2* ion: 1s? (b) When iron is added to copper (II) sulfate solution, the iron displaces the copper ions from solution. However, when copper is added to iron (II) sulfate solution, the iron ions are not displaced and they remain in solution. (i) Write the half equation for the reduction of copper (II) ions to form copper. (ii) Explain why the reaction takes place only if iron is added to copper (II) sulfate solution.
Cr forms two monatomic ions, Cr²+ and Cr³t. From which sublevels do you expect electrons are lost in forming these ions? (Hint: It is possible for electrons other than those in the s and p sublevels to be involved in forming ions.) In forming the Cr*+ ion are: electron(s) lost from the 4s orbital? electron(s) lost from the 3d orbital? To support your answer, complete the following. It is OK to use the noble gas core notation. (Express your answer as a series of orbitals. For example, the electron configuration of Li would be entered in 1 complete form as 1s 2 2s or in condensed form as [He]2s '.) Electron configuration of Cr: Electron configuration of Cr2+:
An element X has 16 protons (p+1); 16 electrons (e-1) and 16 neutrons (n0). a) Write the ground state electron configuration.
x |H|V R E S You will use the known periodic trends to compare properties for elements indicate with letters in this periodic table. Consider their relative positions for these questions. Your answers will be letters as indicated above, not the actual element symbol they would coordinate to. (Do not use a real periodic to answer this question.) ● Which alkali metal would be expected to have the lowest first ionization energy? BI H O N> T D LIQ A 0
The electronic configuration of a certain element known as element E, is 1s22s22p4. Write a balanced equation to represent the first (1st) ionization energy of element E. Use “E” as the symbol of the element. Include the physical states.
(i) Write the equation that represents the first electron affinity of Selenium (Se). (ii) Do you expect this process to be exothermic or endothermic? Explain your answer.
There are many chemical concepts to explain the behavior of electrons. Electron affinity and ionization energy are two such concepts in chemistry. 1)Determine the group of element R 2)Determine the electron configuration of element R.
An atom of an element contains 29 electrons and 35 neutrons. Deduce (i) the number of protons and (ii) the electronic configuration of the element.
4
(1) Give the electron configuration of the element belonging to: a) Group 14 and Period 2 b) Group 14 and Period 3 c) What is similar in their electron configurations? bas
Given the following information, identify the groupfrom the periodic table that contains elements that behave likemain-group element “E.”(i) The electron affinity of E is greater than zero.(ii) The ionization energy (IE) trend for element E is: firstionization energy < second ionization energy <<< thirdionization energy.(iii) Samples of E are lustrous and are good electricalconductors.