Trends in Ionic Charge

4 Key excerpts on "Trends in Ionic Charge"

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  eBook - PDF

  Foundations of College Chemistry

  • Morris Hein, Susan Arena, Cary Willard(Authors)
  • 2021(Publication Date)
  • Wiley

    (Publisher)

  229 Dr. Norbert Lange/Shutterstock CHAPTER OUTLINE 11.1 Periodic Trends in Atomic Properties 11.2 The Ionic Bond: Transfer of Electrons from One Atom to Another 11.3 Predicting Formulas of Ionic Compounds 11.4 The Covalent Bond: Sharing Electrons 11.5 Electronegativity 11.6 Lewis Structures of Compounds 11.7 Complex Lewis Structures 11.8 Compounds Containing Polyatomic Ions 11.9 Molecular Shape For centuries we’ve been aware that certain metals cling to a magnet. High-speed levitation trains are heralded to be the wave of the future. How do they function? In each case, forces of attraction and repulsion are at work. Human interactions also suggest that “opposites attract” and “likes repel.” Attractions draw us into friendships and significant relationships, whereas repulsive forces may produce debate and antagonism. We form and break apart interpersonal bonds throughout our lives. In chemistry, we also see this phenomenon. Substances form chemi- cal bonds as a result of electrical attractions. These bonds provide the tremendous diversity of compounds found in nature. The photograph above shows a crystal formed by molecules of tartaric acid, a molecule found in baking powder and other food additives. The atoms in tartaric acid bond together in a very specific orientation to form the shape of the molecule and produce this beautiful pattern. This chapter is one of the most significant and useful chapters in the book—chemical bond- ing between atoms. This is what chemistry is really all about. Study it carefully. Chemical Bonds: The Formation of Compounds from Atoms CHAPTER 11

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  The Study of Ions and salts in chemistry

  • Rose Marie O. Mendoza(Author)
  • 2023(Publication Date)
  • Arcler Press

    (Publisher)

  INTRODUCTION TO IONS AND IONIC COMPOUNDS 1 CONTENTS 1.1. Introduction ........................................................................................ 2 1.2. Ions and the Periodic Table ................................................................. 5 1.3. Ionic Bonding ................................................................................... 10 1.4. Practice Writing Correct Ionic Formulas ............................................ 13 1.5. Naming Ions and Ionic Compounds.................................................. 15 1.6. Polyatomic Ions ................................................................................ 17 1.7. Properties and Formation of Ionic Compounds ................................. 23 1.8. Arrhenius Acids and Bases and Their Role in Salt Formation ............. 24 1.9. Ions, Neurons, and Neuron Impulses ................................................ 25 1.10. Chapter Summary ........................................................................... 34 References ............................................................................................... 37 CHAPTER The Study of Ions and Salts in Chemistry 2 1.1. INTRODUCTION By definition, an atom is considered neutral because the total number of electrons (charged negatively) is the same as the total number of protons (positively charged particle). Since the number of negatively charged particles is equivalent to the number of the positively charged patricles, the total charge on the atom is zero (0). However, this one-to-one charge ratio is not the most frequent condition for a large number of elements. Disorders, therefore, in ratio result in the formation of charged particles termed ions (Koppenol, 2002; Poulsen, 2010; Ball et al., 2011). Across nature, high- energy objects flow to lesser-energy positions.. These lesser energy variables are exemplified as noble gas components in terms of atoms.

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  eBook - ePub

  Introduction to Geochemistry

  Principles and Applications

  • Kula C. Misra(Author)
  • 2012(Publication Date)
  • Wiley-Blackwell

    (Publisher)

  Fig. 2.8 ).

  2.4 Chemical behavior of elements

  The chemical behavior of an element is governed by its electronic configuration because the energy level of the atom is determined by the spatial distribution of its electron cloud. It is only the most loosely bound electrons in the outermost orbitals that take part in chemical interaction with other atoms. For example, the alkali elements (group IA of the Periodic Table), all of which have one electron in the outermost orbital, exhibit similar chemical properties; so do the alkaline earth metals (group IIA of the Periodic Table), all of which have two electrons in the outermost orbital.

  2.4.1 Ionization potential and electron affinity

  Two concepts are useful in predicting the chemical behavior of elements: ionization potential (or ionization energy) ; and electron affinity . Ions are produced by the removal of electron(s) from or the addition of electron(s) to a neutral atom. The energy that must be supplied to a neutral atom (M) in the gas phase to remove an electron to an infinite distance is called the ionization potential (I) . In other words, the ionization potential is the difference in potential between the initial state, in which the electron is bound, and the final state, in which it is at rest at infinity; the lower the ionization potential, the easier it is to convert the atom into a cation. This is the reason why the ionization potential generally increases from left to right in a given period and from top to bottom within a given group of the Periodic Table (Fig. 2.9 ). The first ionization potential (I 1 ) refers to the energy required to remove the first (the least tightly bound) electron, the second ionization potential (I 2

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  Introduction to Modern Inorganic Chemistry, 6th edition

  • R.A. Mackay, W. Henderson(Authors)
  • 2017(Publication Date)
  • CRC Press

    (Publisher)

  Table. 2.14 that these increase towards the right of the Periods and decrease down the Groups. In addition, they reflect the other, smaller, variations which have been remarked; for example, the changes in the Main Groups are more pronounced than in the Transition Groups, and the discontinuity in properties of the elements from gallium to bromine when compared with the rest of their respective Groups is reflected in their electronegativity values.

  8.5 Chemical behaviour and periodic position

  The detailed chemistry of the elements is discussed in the succeeding chapters. In this section, the skeleton of the periodic properties is outlined to provide a framework for the more detailed account which follows.

  Those elements where the outermost electrons are in a new quantum level, after a rare gas configuration, normally react by losing these loosely bound electrons and forming cations. This mode of behaviour is typical of the elements of the lithium, beryllium and scandium Groups together with the lanthanide elements, which have the respective valency shell configurations, s1 , s2 and d1 s2 . All these elements, with the exception of beryllium itself, lose these outer electrons completely with the formation of cations; M+ in the lithium Group, M2+ in the beryllium Group, and M3+ for scandium, yttrium and the lanthanides.

  The elements of the boron, carbon, nitrogen, oxygen, and fluorine Groups, where the outermost electrons are in p orbitals, show more complicated behaviour.

  (a) Elements with electron configurations close to the rare gases can acquire electrons to form anions with complete rare gas shells. Thus the elements of the halogen Group all form X– ions, and we also find stable compounds containing O2− , S2− and N3−

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