Select the element whose valence electrons experience a greater effective nuclear charge. Be Why do the valence electrons of the selected element experience a greater effective nuclear charge? The element has more protons and more core electrons than the other element. The element has more protons, but the same number of core electrons as the other element. The element has more core electrons, but fewer protons than the other element. The element has fewer core electrons and more protons than the other element.

Select the element whose valence electrons experience a greater effective nuclear charge. Be Why do the valence electrons of the selected element experience a greater effective nuclear charge? The element has more protons and more core electrons than the other element. The element has more protons, but the same number of core electrons as the other element. The element has more core electrons, but fewer protons than the other element. The element has fewer core electrons and more protons than the other element.

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter2: Atomic Structure And Periodicity

Section: Chapter Questions

Problem 146AE: An unknown element is a nonmetal and has a valence electron configuration of ns2np4 a. How many...

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Name the element corresponding to each characteristic below. (a) the element with the electron configuration 1s22s22p63s23p3 (b) the alkaline earth element with the smallest atomic radius (c) the element with the largest ionization energy in Croup 5A (d) the element whose 2+ ion has the configuration [Kr]4d5 (e) the element with the most negative electron attachment enthalpy in Croup 7A (f) the element whose electron configuration is [Ar]3d104s2
An unknown element is a nonmetal and has a valence electron configuration of ns2np4 a. How many valence electrons does this element have? b. What are some possible identities for this element? c. What is the formula of the compound this element would form with potassium? d. Would this element have a larger or smaller radius than barium? e. Would lhis element have a greater or smaller ionization energy than fluorine?
An ion having a 4+ charge and a mass of 49.9 u has 2 electrons with principal quantum number n = 1.8 electrons with n = 2. and 10 electrons with n = 3. Supply as many of the properties for the ion as possible from the information given. (Hint: In forming ions for this species, the 4j electrons are lost before the 3d elections.) a. the atomic number b. total number of s electrons c. total number of p electrons d. total number of d electrons e. the number of neutrons in the nucleus f. the ground-state electron configuration of the neutral atom
Which of the following groups of elements is arranged correctly in order of increasing ionization energy? (a) C Si Li Ne (b) Ne Si C Li (c) Li Si C Ne (d) Ne C Si Li
On the basis of the total number of electrons present, identify the elements whose electron configurations are a. 1s22s22p2 b. 1s22s22p63s1 c. 1s22s22p63s23p5 d. 1s22s22p63s23p64s23d104p3
Draw the orbital diagram associated with each of the following electron configurations. a. 1s22s22p5 b. 1s22s22p63s1 c. 1s22s22p63s23p1 d. 1s22s22p63s23p64s23d5
Classify the element with each of the following electron configurations as a representative element, transition element, noble gas, or inner transition element. a. 1s22s22p6 b. 1s22s22p63s23p4 c. 1s22s22p63s23p64s23d1 d. 1s22s22p63s23p64s2
Name and give the symbol of the element that has the characteristic given below. (a) Its electron configuration in the excited state can be 1s22s22p63s1 3p3. (b) It is the least electronegative element in period 3. (c) Its +3 ion has the configuration [36Kr]. (d) It is the halogen with the largest atomic radius. (e) It has the largest ionization energy in Group 16.
Group the following elements into three similar groups of two each: Na, O, Ne, Li, Ar, S