Write the electron configurations for neutral atoms of gallium (Ga), chlorine (Cl), phosphorus (P) , calcium (Ca), and sulfur(S).electron configuration for Ga:electron configuration for Cl:electron configuration for P:electron configuration for Ca:electron configuration for S:Arrange the atoms according to both decreasing atomic radius and increasing first ionization energy (IE).Largest radiusSmallest first IE? Smallest radiusLargest first IEAnswer BankAnswer BankСаSClPGaSClGaСаSelect the statement(s) that explain(s) the relationship between the arrangement of elements by size and firstionization energy.O Ap subshell with only one unpaired electron is extremely stable, making the fifth electron in a p subshell easyto remove.The first set of paired electrons in a p subshell experience a large amount of electron-electron repulsion, making thefourth electron in a p subshell easy to remove.The two arrangements are the same because IE of elements increases from left to right and the radii of elementsdecreases from left to right.A full s subshell is able to shield a newly filled p subshell from the nucleus, making the first electron in a p subshelleasy to remove.The third unpaired electron in ap subshell causes a lot of electron-electron repulsion among the orbitals, making thethird electron in a p subshell easy to remove.?

Given that : We have to write the electron configurations for the following atoms : (i) Gallium (Ga)…

Answered: Write the electron configurations for…

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter11: Modern Atomic Theory

Section: Chapter Questions

Problem 126CP

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Similar questions

6.84 Which graph correctly depicts the first ionization energy of three elements in groups 14 (dashed line) and 17 (solid line)? Explain the reasoning you used to make your choice.
Consider the following statement "The ionization energy for the potassium atom is negative, because when K loses an electron to become K +, it achieves a noble gas electron configuration." Indicate everything that is correct in this statement. Indicate everything that is incorrect. Correct the incorrect information and explain.
Consider the eight most abundant elements in the human body, as outlined in Exercise 156. Excluding hydrogen, which of these elements would have the smallest size? largest size? smallest first ionization energy? largest first ionization energy?
r Questions 11—13, you will need to consider ionizations beyond the first ionization energy. For example, the second ionization energy is the energy to remove a second electron from an element. Compare the first ionization energy of helium to its second ionization energy, remembering that both electrons come from the 1s orbital. l> X Y First 170 200 second 350 400 Third 1800 3500 fouth 2500 5000 entify the elements X and Y. There may be more than one answer. so explain completely.
Compare the elements B, Al, C, Si. (a) Which has the most metallic character? (b) Which has the largest atomic radius? (c) Arrange the three elements B, Al, and C in order of increasing first ionization energy.
Read the labels of several commercial products and identify monatomic ions of at least six main group elements contained in the products. Write the complete electron configurations of these cations and anions.
If sufficient energy is absorbed by an atom, an electron can be lost by the atom and a positive ion formed. The amount of energy required is called the ionization energy. In the H atom, the ionization energy is that required to change the electron from n = 1 to n = infinity. Calculate the ionization energy for the He+ ion. Is the ionization energy of the He+ more or less than that of H? (Bohrs theory applies to He+ because it, like the H atom, has a single electron. The electron energy, however, is now given by E = Z2Rhc/n2, where Z is the atomic number of helium.)
Answer the following questions about first ionization energies. (a) Generally ionization energies increase on proceeding across a period, but this is not true for magnesium (738 kJ/mol) and aluminium (578 kJ/mol). Explain this observation. (b) Explain why the ionization energy of phosphorus (1012 kJ/mol) is greater than that of sulphur (1000 kJ/mol) when the general trend in ionization energies in a period would predict the opposite.
Write the symbol of (a) all the elements in which all the 4d orbitals are half-full. (b) all the nonmetals in period 2 that have 2 or more unpaired electrons. (c) all the elements in group 2 in which the 4p sublevel is full. (d) all the metalloids that have unpaired 5p electrons.

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