Show all work (A) Find Pi, Pa, and Pats (B) Determine whether each element is supplying orabsorbing power. (C) Determine lo24 V6A+8VI6V +33A87+63A44Ix=2A+210 V56VW1A16 V

Answered: (A) Find Pi, Pa, and Pats (B) Determine…

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter5: Electron Configurations And The Periodic Table

Section: Chapter Questions

Problem 142QRT

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Write condensed electron configurations for the following atoms and ions, using appropriate noble-gas core abbreviations. Put superscripted electron count numbers in parentheses. Examples: Fe = [Ar]4s(2)3d(6), Sn²+ = [Kr]4d(10)5s(2), S²- = [Ar]. (a) v3+ (b) T₁²+ (c) 0²- = (e) Si = = = (d) Te²2- =
The electron in the hydrogen atom (in its ground state) orbits the nucleus at a distance of 0.5292 Å. (a) Calculate the gravitational force and (b) the electrostatic force of attraction between the two. (c) Comment on the magnitude and the importance of these two forces. [G, gravitational constant = 6.672 x 10-11 N m2 kg-2; 4+Єo = 1.113 x 10-10 C2 m-1 J-1]
1. An element has the following electronic configuration: [Kr]4d105s25p4(a) What period does it belong to?(b) What is its group number? (Use group numbers from 1 to 18)(c) What kind of element is it? (Main group metal, transition metal, metalloid, nonmetal?)(d) How many unpaired electrons are there in an atom of this element? 3. (a) Which of the following atoms or ions is diamagnetic?Li+ Ni2+ Al Fe2+ Mn3+(b) Which of the following atoms or ions is paramagnetic?C4- S4+ V4+ Se2- Ge4+
Which element would you expect to be more metallic?(a) Ca or Rb(b) Mg or Ra(c) Br or I
Boron, atomic number 5, occurs naturally as two isotopes, 10B and 11B, with natural abundances of 19.9% and 80.1%, respectively. (a) In what ways do the two isotopes differ from each other? Does the electronic configuration of 10B differ from that of 11B? (b) Draw the orbital diagram for an atom of 11B. Which electrons are the valence electrons? (c) Indicate three ways in which the 1s electrons in boron differ from its 2s electrons. (d) Elemental boron reacts with fluorine to form BF3, a gas. Write a balanced chemical equation for the reaction of solid boron with fluorine gas. (e) ΔHf° for BF3(g) is -1135.6 kj/mol. Calculate the standard enthalpy change in the reaction of boron with fluorine. (f) Will the mass percentage of F be the same in 10BF3 and 11BF3? If not, why is that the case?
An element has the following electronic configuration: [Kr]4d105s25p2(a) What period does it belong to?(b) What is its group number? (Use group numbers from 1 to 18)(c) What kind of element is it? (Main group metal, transition metal, metalloid, nonmetal?)(d) How many unpaired electrons are there in an atom of this element?
Write condensed electron configurations for the following atoms and ions, using appropriate noble-gas core abbreviations. Put superscripted electron count numbers in parentheses. Examples: Fe = [Ar]4s(2)3d(6), Sn²+ = [Kr]4d(10)5s(2), s2- = [Ar]. (a) Te2- (b) I = (c) Fe3+ (d) v3+ (e) Ba2+ =
(1) What is the name of the element with a valence electron configuration of 3s-3p*? (2) What is the name of the element with a valence electron configuration of 4s²4p?
(1) What is the valence electron configuration for the helium atom? (2) What is the valence electron configuration for the gallium atom? (1) What is the name of the element with a valence electron configuration of 3s23p2?(2) What is the name of the element with a valence electron configuration of 4s1?
choose three . What are the characteristerses of a metal like element? (a) they try to get additional electrons (b) they are melleable. (c) they are lightly to give away or share electrons. (d) they are good conductors of electricity
Question 20 Answer the following questions: (a) Without using quantum numbers, describe the differences between the shells, subshells, and orbitals of an atom. (b) How do the quantum numbers of the shells, subshells, and orbitals of an atom differ? Question 21 Identify the subshell in which electrons with the following quantum numbers are found: (a) n = 2, l = 1 (b) n = 4, l = 2 (c) n = 6, l = 0
(ii) Draw the Born-Haber cycle and use the data below for the formation of calcium chloride, to calculate the electron affinity of chlorine: Ca(s) → Ca(g) AHat = +190 kJ/mol Ca(g) > Caz*(g) + 2e¨ AH¡ɛ = +1730 kJ/mol Cl2{g) 2C1(g) AHat = +121 kJ/mol Caz (g) + 2Cl(g) > CaCl2(s) AHLE = -2184 kJ/mol Ca(s) + Cl2(g) –> CaCl2(s) AH; = -795 kJ/mol

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(A) Find Pi, Pa, and Pats (B) Determine whether each element is supplying or absorbing power. (C) Determine lo 24 V 6A +8V I 6V + 3 3A 87+ 6 3A 44 Ix=2A + 2 10 V 5 6V W1A 16 V