The Aufbau Principle describes the order of subshells in an atom in terms of energy. Higher numbered shells have higher energy. It is complicated by occasiona overlapping. The specific order of subshells using the Aufbau Principle can be found using the diagonal arrow diagram found in Chapter 8, and this is the same order found on the periodic table. What is the order of subshells in period 7? (there are 4) 7s a. 1s b. 2s С. 3s d. 4s е. 5s f. 6s g. 7s h. 1p i. 2p j. Зр k. 4p I. 5p m. 6p n. 7p o. 1d р. 2d q. 3d r. 4d s. 5d t. 6d u. 7d v. 1f w. 2f y. 3f z. 4f aa. 5f bb. 6f сс. 7f

The Aufbau Principle describes the order of subshells in an atom in terms of energy. Higher numbered shells have higher energy. It is complicated by occasiona overlapping. The specific order of subshells using the Aufbau Principle can be found using the diagonal arrow diagram found in Chapter 8, and this is the same order found on the periodic table. What is the order of subshells in period 7? (there are 4) 7s a. 1s b. 2s С. 3s d. 4s е. 5s f. 6s g. 7s h. 1p i. 2p j. Зр k. 4p I. 5p m. 6p n. 7p o. 1d р. 2d q. 3d r. 4d s. 5d t. 6d u. 7d v. 1f w. 2f y. 3f z. 4f aa. 5f bb. 6f сс. 7f

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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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
D. Give the quantum numbers for the last electron of each element given in Part II following the table below. Element 1 subshell N - 7 1s22s22p3 70 Ga,17⁰ Ar 1840 Sb,1122 112 AU79197 n main energy level 2 s=0 p=1 d=2 f=3 1 m₁ orbital -1 to 0 to +1 -1, 0, +1 +1 m₂ magnetic spin (+1/2, -1/2) +1/2
5. Down a group in the periodic table: Do you think the ionization energy of Lithium (Li) is larger or smaller than that of Sodium (Na)?A. Larger B. Smaller C. Same D. Don’t KnowWhat did you base your answer on?6. Across a row in the periodic table: Do you think the ionization energy of Lithium (Li) is larger or smaller than that of Neon (Ne)?A. Larger B. Smaller C. Same D. Don’t KnowWhat did you base your answer on?
How many electrons are possible in the n = 3 energy level? -- 2 8 18 32 36
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
Answer number 1 to 5
Only question 8
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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