Consider the molecule NH3. Part A Review Constants I What is the electron configuration of an isolated N atom? Express your answer in condensed form in order of increasing orbital energy as a string without blank space between orbitals. For example, [He]2822p2 should be entered as [He]2s^22p^2. 1s^22s^22p^3 2 Submit Previous Answers Request Answer X Incorrect; Try Again; 4 attempts remaining What is the electron configuration of an isolated H atom? Express your answer in condensed form in order of increasing orbital energy as a string without blank space between orbitals. For example, [He]2s22p2 should be entered as [He]2s^22p^2. Part B 1s^1 @ 3 Previous Answers જ a MacBook Pro $ % 4 5 6 9> & 87 7 E R T 3M > = * ∞ 8 + < ( ) 9 0

Consider the molecule NH3. Part A Review Constants I What is the electron configuration of an isolated N atom? Express your answer in condensed form in order of increasing orbital energy as a string without blank space between orbitals. For example, [He]2822p2 should be entered as [He]2s^22p^2. 1s^22s^22p^3 2 Submit Previous Answers Request Answer X Incorrect; Try Again; 4 attempts remaining What is the electron configuration of an isolated H atom? Express your answer in condensed form in order of increasing orbital energy as a string without blank space between orbitals. For example, [He]2s22p2 should be entered as [He]2s^22p^2. Part B 1s^1 @ 3 Previous Answers જ a MacBook Pro $ % 4 5 6 9> & 87 7 E R T 3M > = * ∞ 8 + < ( ) 9 0

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter4: Introduction To Quantum Mechanics

Section: Chapter Questions

Problem 39P: Chapter 3 introduced the concept of a double bond between carbon atoms, represented by C=C , with a...

See similar textbooks

Similar questions

Using a simple particle-in-a-box model for the multiple bonding in 1,2-butadiene (see Example 4.7) and the n=2 wave function for the weakest bound electron, calculate the probability of finding the electron in an 0.1 interval centered midway between the two inner carbon atoms (that is, the center is at x=2.11 , so this interval is from x1=2.06 to x2=2.16 ). Then calculate the probability of finding the electron in an 0.1 interval centered midway between an end carbon atom and the carbon atom that is double-bonded to it in the Lewis dot structure. (You may calculate the appropriate integrals or estimate the relevant areas under the curve graphically.) Then recalculate the probabilities by approximating the integral as |( x 0)|2x , where x0 is evaluated in the middle of the range from x1 to x2 . Finally, explain why you can’t approximate the integral needed for Problem 37(a) in this way.
Schrodinger and de Broglie suggested a ‘Wave—particle duality" for small particles—that is, if electromagnetic radiation showed some particle-like properties, then perhaps small punicles might exhibit same wave-like properties. Explain. How does the wave mechanical picture of the atom fundamentally differ from the Bohr model? How do wave mechanical arbitals differ from Bohr’s orbits? What does it mean to say that an orbital represents a probability map for an electron?
Chapter 3 introduced the concept of a double bond between carbon atoms, represented by C=C , with a length near 1.34 Å. The motion of an electron in such a bond can be treated crudely as motion in a one-dimensional box. Calculate the energy of an electron in each of its three lowest allowed states if it is confined to move in a one-dimensional box of length 1.34 Å. Calculate the wavelength of light necessary to excite the electron from its ground state to the first excited state.
Do atoms in excited states emit radiation randomly, at any wavelength? Why? What does it mean to say that the hydrogen atom has only certain discrete energy levels available? How do we know this? Why was the quantization of energy levels surprising to scientists when it was first discovered?
For each of the statements below, indicate whether it is true or false and explain your reasoning. (1 sentence ) 1/ It takes more energy to ionize an electron from the 2s orbital than an electron from the 2p orbital in the Li2+ ion. 2/ The electron affinity of the Ne atom is larger than the electron affinity of the F atom. 3/ K* has a larger radius than Ar. 4/ For a diatomic molecule, in which the internuclear axis is the z-axis, the 3dz? orbital cannot mix with the 2px orbital. 5/ The internuclear distance of O2 increases as it takes an additional electron to become O2".
and lea X G The element in period 5 that has X takeCovalentActivity.do?locator-assignment-take C Solved The following Lewis diagr. X Solution of the Schrödinger wave equation for the hydrogen atom results in a set of functions (orbitals) that describe the behavior of the electron. Each function is characterized by three quantum numbers: n, I, and my. If the value of n = 2 The quantum number / can have values from to The total number of orbitals possible at the n = 2 energy level is Submit Answer Use the References to access important values if needed for this question. If the value of 1 = 2 to The quantum number m, can have values from The total number of orbitals possible at the / = 2 sublevel is BUTY + Retry Entire Group 9 more group attempts remaining Previous Email Instructor A ENG Save and Exit 11:58 AM 11/28/2022 *
MINI-PTASK IN GENERAL CHEMISTRY 1 (Lesson 4 and 5) Answer the following and do as drected in 1 whole sheet of bond paper and should be handwritenidrawn. Submt a copy of your work in the given template. 1. Draw the shape of the orbital with the quantum numbers nes, t0 2. Draw the shape of the subshell with the quantum numbers na4, 2. me2 3. Draw the orientation in space of the orbital if1 for the shell n2 and with mt values ort andt 4. Draw the shape of the atomic orbital ne3, 2, me= 0, ms= % 5. Write the long configuration and noble gas configuration of the given elements and draw the orbital diagram of the folowing elements at s ground state a chiorine a Potassium B. Manganese C Aluminum 6. ldentity the magnetic property of the elements given in number 5. . angon
In what column of the Periodic Table would you expect to find the atom with each of the following configurations: (a) 1s²2s²2p°; (b) 1s²2s²2p°3s²;_ (c) 1s²2s²2p°3s²3p°; (d) 1s²2s²2p°3s²3p°4s!? 6.
Prove that the potential energy of the electron is Etotal -e?/ (8πεoΥ)
Q8, What is electron affinity? How it varies in groups and periods of the Periodic Table. Note please solve within 30 minutes. Asap. Avoid plagiarism.
1. II. II. IV. V. Which of the orbitals above would represent one of the possible 5p atomic orbitals? No work needs to be shown for this problem. || IV O v V O II
Which is a correct ground-state electron configuration for Cs? O 1s²2s²2p63s²3p63d104s²4p64d105s²5p65d106s1 O 1s²2s²2p63s²3p64s²3d104p65s²4d105p6s! 1s²2s²2p°3s²3p°4s²3d104p65s²4d105p©6s² 1s²2s²2p63s²3p63d1045²4p©5s²4d105p6s! 1s²1p61d102s²2p62d103s²3p©3d10