The valence shell electron configuration for the given elements and the number of valence electrons for each element is to be determined. Concept Introduction: Valence shell is the outermost shell of an atom, only the electrons present in the valence shell participate in the chemical bonding. An element’s chemical properties can be determined by the valence electrons. The electron configuration of an atom contributes to their physical and chemical properties. It helps in the better understanding of the structure of an atom and the nature of the electrons contained within that atom. Three rules that should be followed to fill the atomic orbitals by electrons: Rule 1: The lowest energy orbitals fill first, filling pattern is 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f, 5d, 6p, 7s, 5f, 6d, 7p etc . The entire subshell of a particular orbital type filled before moving to the next subshell of higher energy. Rule 2: Pauli Exclusion Principle- Only two electrons of opposite spin are permitted per orbital. Rules 3: Hund’s Rule – The orbitals of the same energy are each filled with one electron of same spin before filling any with a second electron.
The valence shell electron configuration for the given elements and the number of valence electrons for each element is to be determined. Concept Introduction: Valence shell is the outermost shell of an atom, only the electrons present in the valence shell participate in the chemical bonding. An element’s chemical properties can be determined by the valence electrons. The electron configuration of an atom contributes to their physical and chemical properties. It helps in the better understanding of the structure of an atom and the nature of the electrons contained within that atom. Three rules that should be followed to fill the atomic orbitals by electrons: Rule 1: The lowest energy orbitals fill first, filling pattern is 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f, 5d, 6p, 7s, 5f, 6d, 7p etc . The entire subshell of a particular orbital type filled before moving to the next subshell of higher energy. Rule 2: Pauli Exclusion Principle- Only two electrons of opposite spin are permitted per orbital. Rules 3: Hund’s Rule – The orbitals of the same energy are each filled with one electron of same spin before filling any with a second electron.
Solution Summary: The author explains that the valence shell electron configuration for the given elements is to be determined.
Definition Definition Connection between particles in a compound. Chemical bonds are the forces that hold the particles of a compound together. The stability of a chemical compound greatly depends on the nature and strength of the chemical bonding present in it. As the strength of the chemical bonding increases the stability of the compound also increases.
Chapter 7, Problem 22PE
Interpretation Introduction
Interpretation:
The valence shell electron configuration for the given elements and the number of valence electrons for each element is to be determined.
Concept Introduction:
Valence shell is the outermost shell of an atom, only the electrons present in the valence shell participate in the chemical bonding.
An element’s chemical properties can be determined by the valence electrons.
The electron configuration of an atom contributes to their physical and chemical properties. It helps in the better understanding of the structure of an atom and the nature of the electrons contained within that atom.
Three rules that should be followed to fill the atomic orbitals by electrons:
Rule 1: The lowest energy orbitals fill first, filling pattern is 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f, 5d, 6p, 7s, 5f, 6d, 7p etc. The entire subshell of a particular orbital type filled before moving to the next subshell of higher energy.
Rule 2: Pauli Exclusion Principle- Only two electrons of opposite spin are permitted per orbital.
Rules 3: Hund’s Rule – The orbitals of the same energy are each filled with one electron of same spin before filling any with a second electron.
Determine the number of valence electrons and give the electronic confi guration of the valence electrons of each element: (a) nitrogen; (b) potassium.
(1) What is the valence electron configuration for the arsenic atom?
(2) What is the valence electron configuration for the fluorine atom?
Q1.
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.
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Symbol of ion
Relative atomic mass