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(a)
Interpretation:
The reason as to why ionization energy should increase as
Concept introduction:
The ionization energy is the measurement of energy, which is required to remove an electron from a neutral atom. An atom acquires a positive charge when it removes an electron from its valence shell. The valence shell electron is loosely bind, which is easily removed.
(b)
Interpretation:
The features of electron configurations with the locations of the breaks in Periods
Concept introduction:
Many of the chemical properties of an atom or ion depend on its electron configuration, the ground state distribution of electrons among the orbitals of the species. In the electron configuration the highest occupied energy level indicates the period and the numbers of valence electrons indicate to the groups.
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Chapter 11 Solutions
EBK INTRODUCTORY CHEMISTRY: AN ACTIVE L
- Does the information on alkali metals in Table 2-8 of the text confirm the general periodic trends in ionization energy and atomic radius? Explain.arrow_forwardWhat is the electron configuration of the Ba3+ ion? Suggest a reason why this ion is not normally found in nature.arrow_forwardConsider 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.arrow_forward
- Use electron configurations to explain the following observations:(a) The first ionization energy of phosphorus is greaterthan that of sulfur. (b) The electron affinity of nitrogen islower (less negative) than those of both carbon and oxygen.(c) The second ionization energy of oxygen is greater thanthe first ionization energy of fluorine. (d) The third ionizationenergy of manganese is greater than those of both chromiumand iron.arrow_forwardConsider these ground-state ionization energies of one-electron species:H=1.31X10³kJ/mol ,He⁺=5.24X10³kJ/mol Li²⁺=1.41X10⁴kJ/mol (a) Write a general expression for the ionization energy of anyone-electron species. (b) Use your expression to calculate theionization energy of B⁴⁺. (c) What is the minimum wavelengthrequired to remove the electron from the n=3 level of He⁺?(d) What is the minimum wavelength required to remove the electron from the n=2 level of Be³⁺?arrow_forward(a) Identify the following neutral elements by their condensed electron configurations. (Enter the chemical symbol or name of the element.) (i) [Ar] 4s2 3d3 (ii) [Kr] 5s2 4d10 5p3 (iii) [Ar] 4s2 3d10 4p4arrow_forward
- Identify by name the following electron configuration of a specific element. (i) How many valence electrons does this element have? 1s22s22p63s23p63d104s24p5 (ii) Write the electron configuration of the 2+ ion of the element.arrow_forwardWhich of the following chemical equations is connected tothe definitions of (a) the first ionization energy of oxygen,(b) the second ionization energy of oxygen, and (c) the electronaffinity of oxygen?(i) O(g) + e------>O-(g) (ii) O(g)---->O+(g) + e-(iii) O(g) + 2 e------->O2-(g) (iv) O(g)----->O2+(g) + 2 e-(v) O+(g)----->O2+(g) + e-arrow_forward(a) Use orbital diagrams to illustrate what happens when anoxygen atom gains two electrons. (b) Why does O3 - not exist?arrow_forward
- (a) Why do successive IEs of a given element always increase? (b) When the difference between successive IEs of a given element is exceptionally large (for example, between IE1 and IE2 of K), what do we learn about its electron configuration? (c) The bars represent the relative magnitudes of the first five ionization energies of an atom: Identify the element and write its complete electron config uration, assuming it comes from (a) Period 2; (b) Period 3; (c) Period 4.arrow_forwardQ1. This question is about atomic structure. (a) Write the full electron configuration for each of the following species. CH Fe2+ (b) Write an equation, including state symbols, to represent the process that occurs when the third ionisation energy of manganese is measured. (c) State which of the elements magnesium and aluminium has the lower first ionisation energy Explain your answer. (d) A sample of nickel was analysed in a time of flight (TOF) mass spectrometer. The sample was ionised by electron impact ionisation. The spectrum produced showed three peaks with abundances as set out in the table. m/z Abundance /% 58 61.0 60 29.1 61 9.9 Give the symbol, including mass number, of the ion that would reach the detector first in the sample. Calculate the relative atomic mass of the nickel in the sample. Give your answer to one decimal place. Page 2 of 12 Symbol of ion Relative atomic massarrow_forwardExplain how the following equation can be manipulated and used to approximate the ionization energy of a given element. 1. (Zeff Joules Е, 3D -2.178х 10-18 n²arrow_forward
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