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]ns² md¹⁰ np³ [G]ns² np³ [G]ns² mf location of elements (check all that apply) blocks OS OP Od Of Os Op Od Of Os Op Od Of metals or nonmetals? Ometals O nonmetals Ometalloids metals Ononmetals O metalloids O metals Ononmetals O metalloids X

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]ns² md¹⁰ np³ [G]ns² np³ [G]ns² mf location of elements (check all that apply) blocks OS OP Od Of Os Op Od Of Os Op Od Of metals or nonmetals? Ometals O nonmetals Ometalloids metals Ononmetals O metalloids O metals Ononmetals O metalloids X

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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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)
● What are valence electrons? Noble gases are sometimes called "inert gases." How do their electron configurations explain why noble gases do not participate in many chemical reactions? If fluorine gains 1 electron, which element will it be similar to?_ If sodium loses 1 electron, which element will it be similar to?_ What group of elements are the "other elements" striving to be similar to?
The Pauli Exclusion Principle tells us that no two electrons in an atom can have the same four quantum numbers. For an electron in the 3p 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 3p orbitals. m₁ = mg = Submit Answer Retry Entire Group 9 more group attempts remaining
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
Give the number of s, p, d, and f electrons in each of the following atoms. (Please remember that Cu and Cr have irregular electron configurations. Also, the total number of electrons should add up to the atomic number of the neutral atom.) d atom Cd (Z=48) Fr (Z=87) Cu (Z=29) Р
Electron affinity, EA, is the energy required to add an electron to a neutral gaseous atom and is related to an element's position on the periodic table. Electron affinities can be positive, negative, or zero, as shown in the table. Element Electron affinity(kJ/mol) N (nitrogen) >0 Br (bromine) −325 Sr (strontium) −5 Rank the following elements by electron affinity, from most positive to most negative EA value. Rank from most positive to most negative. If any elements are equivalent, please note that. Iodine Rubidium Krypton Bismuth Oxygen
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 2 [G]ns²mfs 5 3 [G]ns² md¹np³ [G]ns²md¹np 6 blocks 00 00 S e S S location of elements (check all that apply) a U 0 00 р f р f р f metals or nonmetals? 00 000 0 0 0 X metals nonmetals metalloids metals nonmetals metalloids metals nonmetals metalloids Ś
Arrange atoms C, K, Ge, Cs in order of:decreasing atomic size: biggest size – ___ > ___ > ___ > ___ – smallest size
Give the indicated full or noble gas electron configuration Note: you can't do superscripts in questions answers, so format your answer without superscripts but with one space between each orbital. E.g. Li would be 1s2 2s1 instead of 1s22s The number in parentheses after the symbol is the element's atomic number. Full configuration: N (7) Full configuration: Si (14) Full configuration: Ti (22) Noble gas configuration: Ba (56) ( Noble gas configuration: Te (52) (99+ hp
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.
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