Use spdf and noble gas notations to give the electron configurations of these two elements. (Express your answer as a series of orbitals. For example, the electron configuration of Li would be entered in complete form as 1s 2 2s ¹ or in condensed form as [He]2s ¹.) spdf notation configuration for the element 113: Noble gas notation configuration for the element 113: spdf notation configuration for the element 115: Noble gas notation configuration for the element 115: For each of these elements, name another element in the same periodic group. Another element for the element 113 is Another element for the element 115 is Element 113 was made by firing the nucleus of a light atom at a heavy americium atom. The two nuclei combine to give a nucleus with 113 protons. What light atom was used as a projectile?

Use spdf and noble gas notations to give the electron configurations of these two elements. (Express your answer as a series of orbitals. For example, the electron configuration of Li would be entered in complete form as 1s 2 2s ¹ or in condensed form as [He]2s ¹.) spdf notation configuration for the element 113: Noble gas notation configuration for the element 113: spdf notation configuration for the element 115: Noble gas notation configuration for the element 115: For each of these elements, name another element in the same periodic group. Another element for the element 113 is Another element for the element 115 is Element 113 was made by firing the nucleus of a light atom at a heavy americium atom. The two nuclei combine to give a nucleus with 113 protons. What light atom was used as a projectile?

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...

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Directions Complete the table below by giving the atomic number, orbital diagram and the electron configuration of the following given elements.
As we move across period 4 of the periodic table, the electron affinities of Ge, As,and Se,jumpfrom -115 kJ/mol to -7 kJ/mol to -195 kJ/mol, showing a deviation from the expected trend. Explain thesevalues in terms of the electron configurations of the atoms.
Fix any errors in these proposed electron configurations. number of electrons in atom 16 14 11 proposed electron configuration 2 4 6 1s 2s 2p 3s 2 2 8 2 1s 2s 2p 3s 2 2 2 5 1s 2s 3s 2p 5
Scientists are synthesizing new elements all the time. In theory, elements with atomic numbers well beyond those of the current periodic table are possible. We can apply the principles of quantum mechanics to predict the electron configurations of yet to be synthesized elements. Assuming perfect Aufbau filling, how many electrons would be present in the highest energy subshell of theoretical element 125? Number of electrons in highest energy subshell:
Identify the element based on the electron configuration 1s22s22p63s23p64s¹. Mg Na K Ca
Identify the element symbol of the following element. a. An excited state of this element has the electron configuration 1s²2s²2p¹3s¹. b. The ground-state electron configuration is [Ne]3s²3p¹. c. An excited state of this element has the electron configuration [Kr]5s²4d³6s¹. d. The ground-state electron configuration contains three unpaired 5p electrons.
There are four different abbreviated ways to write out the electron configuration using the symbolic form for the elements in group 18 (8A). Write out the one using the heaviest group 18 (8A) element.
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Only typed explanation of all three subparts otherwise leave it
My [Review Topics] [References] Using noble gas notation, write electron configurations for atoms of the following elements. (Express your answer using the noble gas notation. For example, the electron configuration of Li would be entered as [He]2s¹.) a. Scandium, Sc. A silvery-white metallic transition metal, it has historically been sometimes classified as a rare earth element, together with yttrium and the lanthanoids. Electron configuration: b. Zirconium, Zr. The metal is exceptionally resistant to corrosion and so has important industrial applications. Moon rocks show a surprisingly high zirconium content compared with rocks on Earth. Electron configuration: c. Rhodium, Rh. This metal is used in jewelry and in catalysts in industry. Electron configuration: d. Tin, Sn. The metal was used in the ancient world. Alloys of tin (solder, bronze, and pewter) are important. Electron configuration: Show Hint Previous Next
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?
Fill Table 1 with full electron configuration and number of unpaired electrons with the configurations. To get number of unpaired electrons, draw orbital diagram of the outermost shell, and fill the orbitals with electrons following Aufbau Rule, Hund's Rule, and Pauli Exclusion Principle, then count how many electrons are left unpaired. Table 1: Electron Configurations of Atoms and lons Element Atomic Unpaired Full Electron Configuration Symbol Number Electrons S 1s° 2s° 2p° 3s° 3p* 16 CI Na Li F Fe Fe2+ Fe+ K* P3- O2- Mg**