Some patterns of electron configuration are listed below. In each case, [G] stands for a noble-gas core and n, m, or o stand for integer numbers like 1, 2, 3 and so on. Note: assume G is lighter than Rn. Think about the chemical elements made of atoms with an electron configuration that matches each pattern. In what block or blocks of the Periodic Table would these elements lie? Would they be metals, nonmetals, metalloids, some of each? Use your answers to these questions to complete the table. electron configuration of atoms [G]ns²mf³ [G]ns² md¹np [G]ns² blocks location of elements (check all that apply) sp Od f S S P df Р nd f metals or nonmetals? X metals nonmetals metalloids metals nonmetals metalloids metals nonmetals metalloids

Some patterns of electron configuration are listed below. In each case, [G] stands for a noble-gas core and n, m, or o stand for integer numbers like 1, 2, 3 and so on. Note: assume G is lighter than Rn. Think about the chemical elements made of atoms with an electron configuration that matches each pattern. In what block or blocks of the Periodic Table would these elements lie? Would they be metals, nonmetals, metalloids, some of each? Use your answers to these questions to complete the table. electron configuration of atoms [G]ns²mf³ [G]ns² md¹np [G]ns² blocks location of elements (check all that apply) sp Od f S S P df Р nd f metals or nonmetals? X metals nonmetals metalloids metals nonmetals metalloids metals nonmetals metalloids

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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In the Zn2+ ion (in its ground state), how many electrons are l = 2? The atomic number of Zn is 30. In the As atom (in its ground state), how many electrons are l = 1 and m = 0? The atomic number of As is 33. In the Mn2+ ion (in its ground state), how many electrons are m = 0? The atomic number of Mn is What is the effffective charge seen by a valence electron in Ti4+? The atomic number of Ti is 22. Who proposed the photon?
The Pauli Exclusion Principle tells us that no two electrons in an atom can have the same four quantum numbers. y For an electron in the 2s orbital shown above, enter a possible value for each quantum number. n = 1 = Give ONE example. Give ONE example. Though a given electron only has one value for possible mi, there are my values for electrons in 2s orbitals. m = m = Submit Answer Retry Entire Group 9 more group attempts remaining
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Write the electron configuration for the ground state of Hg2+ (mercury 2+). Use the noble gas shortcut. Since Canvas doesn't support superscripts and the like, type in the electron configuration with a space between each sublevel, and without special formatting. For example, [He]2s2p? would be typed in the answer box as "[He] 2s2 2p2".
An unidentified element is known to have an electron configuration, [X] ns^2, in its ground state. This element must be in the same family as… A) arsenic B) lead C) radon (Rn) D) rubisium (rb) E) radium (Ra)
Some patterns of electron configuration are listed below. In each case, [G] stands for a noble-gas core and n, m, or o stand for integer numbers like 1, 2, 3 and so on. Note: assume G is lighter than Rn. Think about the chemical elements made of atoms with an electron configuration that matches each pattern. In what block or blocks of the Periodic Table would these elements lie? Would they be metals, nonmetals, metalloids, some of each? Use your answers to these questions to complete the table. electron configuration of atoms 6 [G]ns²np [G]ns¹ 2 [G]ns²mf³ 3 blocks 00 P S 00 P 00 S location of elements (check all that apply) S C р р f р f metals or nonmetals? 000 000 000 metals nonmetals metalloids metals nonmetals metalloids metals nonmetals metalloids
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Imagine a universe where there are three spin states for the electron instead of two (for example, spin up, spin down, and spin cray-cray). The number of subshells per shell and number of orbitals per subshell stay the same, but an orbital now holds three electrons instead of two. The names of the elements stay the same. Draw the top three rows of what this new periodic table would look like, indicating which elements are in which groups in our new universe, and show the electron configurations of each of the elements of these three rows.
Give typed full explanation not a single word hand written otherwise leave it
The Pauli Exclusion Principle tells us that no two electrons in an atom can have the same four quantum numbers. In progress For an electron in the 3s orbital shown above, enter a possible value for each quantum number. n = 1 = = Give ONE example. Give ONE example. Though a given electron only has one value for possible mi, there are my values for electrons in 3s orbitals. m₁ = ms = Submit Answer Retry Entire Group 9 more group attempts remaining