Complete the following table by either identifying the electron configuration, the symbol of the neutral (no charge) a number of valence electrons, and/or the normal valence (common number of bonds) in the spaces provided. Form electron configuration answers like this: 1s22s22p4, for example (i.e. no spaces and no superscript notations). A able is provided below: Electron Configuration 1s22s22p63s23p3 D 1s²2s²2p² Neutral Atom Symbol N Si No. of Valence Electrons 5 Normal Valer number of ba

What is the electronic configuration of I, which has an atomic number of 53? O [kr]5s²4d¹04p5 O [kr]4s24d104p5 O [kr]5s25d105p5 [kr]5s24d105p5

Indicate which of the given electronic configurations are true ground state configurations for the respective atoms and which are false. (Take care! There are some exceptions to the simple rules.) O Ca 1s2s22p63s²3p64s? true false 1s22s²2p5 O Hg [Xe]4f145d106s2 true false O Si 1s22s22p63s²3p2 false 1s²2s²2p63s²3d³

Answer correctly

cloudy esc It takes 157. kJ/mol to break a nitrogen-oxygen single bond. Calculate the maximum wavelength of light for which a nitrogen-oxygen single bond could be broken by absorbing a single photon... Round your answer to 3 significant digits. nm Continue * $ G 1 X f5 % Q 5 A- 4+ & Ⓒ2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessibility 90 * 8 19 144 110 DII

c)- 3002 x 10-6 d) - 3.002 x 104 = 11. Which of the following а) те2- b) Ba2+ c) (st dj Br топь is not iso electronic with the noble gas Xenon!

Write the configuration shell of the first periodic table elements

Q25. Identify the following atoms or ions from their electron configurations:   (a) W: 1s 2 2s 2 2p6 3s 2 3p6 4s 2 3d10 4p6,5s1  (b) X-: 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6   (c) Y++: 1s2 2s2 2p6 3s 2 3p6 4s 2 3d10 4p6 5s2 4d10 5p6  (d) Z: 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f 11

Online teaching and + -owl.cengagenow.com/ilrn/takeAssignment/takeCovalentActivity.do?locator-assignment-take Consider the bright line spectrum of hydrogen shown in the figure below. 410 nm 434 nm 486 nm 656 nm [References] Hydrogen Line Spectrum. When excited hydrogen atoms return to lower energy states, they emit photons of certain energies, and thus certain colors. Shown here are the colors and wavelengths (in nanometers) of the photons in the visible region that are emitted by excited hydrogen atoms. a. Which line in the spectrum represents photons with the highest energy? 434 nm O486 nm O410 nm O 656 nm b. Which line in the spectrum represents photons with the lowest energy? O 434 nm O 486 nm O 410 nm O 656 nm. Submit Answer Try Another Version 2 item attempts remaining MacBook Pro

Write the full ground-state electron configuration for the following. (Type your answer using the format 1s2 2s2 2p6 for 1s2s2p°.) (а) Со (b) As (c) Br Submit Answer