Chemistry
Types of Chemical Bonds
Chemical bonds are the forces that hold atoms together in a compound. There are three main types of chemical bonds: ionic, covalent, and metallic. Ionic bonds form between a metal and a nonmetal, where electrons are transferred. Covalent bonds occur when atoms share electrons, and metallic bonds are found in metals where electrons are delocalized and free to move.
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12 Key excerpts on "Types of Chemical Bonds"
- Robert J. Naumann(Author)
- 2008(Publication Date)
- CRC Press(Publisher)
3 Chemical Bonding The ability of atoms and molecules to form chemical bonds is the de fi ning feature of the structure and properties of solids. The types of bonds that are formed determine if the material will be a metal, a ceramic, or a polymer, and whether the material will conduct electricity, transmit light, or be magnetic. 3.1 What Holds Stuff Together? All matter that we deal with on an everyday basis is held together by electrical forces that form chemical bonds. These forces are manifested in different ways, depending upon which elements are involved. There are three type of primary bonds: (1) the metallic bond in which electrons become detached from atoms when they come together so the ion cores become mutually attracted to the sea of electrons surrounding them; (2) the covalent bond in which atoms become mutually attracted by sharing electrons in order to form closed electron shells; and (3) the ionic bond in which a mutual attraction occurs when one or more electrons leaves a metal atom to complete an atomic shell of a nonmetallic atom forming an oppositely charged ion pair. Much weaker bonds, such as the hydrogen bond, which arise from dipolar attractions between molecules when a hydrogen atom becomes covalently bonded to an O, N, or F atom, or to the van der Waals bond, which arises from induced dipole – dipole interactions, play a secondary role in the structure of materials. Understanding these basic forces that hold materials together is crucial to understanding the structure and properties of materials. We shall start with the ionic bond since conceptu-ally it is the easiest to visualize and it lends itself to a simple analytical model. 3.2 Ionic Bonding The ionic bond is the strongest chemical bond, ranging from 10.5 eV for LiF to 5.8 eV for CsI, but it can only act between two (or more) dissimilar atoms.
- Frederick Bettelheim, William Brown, Mary Campbell, Shawn Farrell(Authors)
- 2019(Publication Date)
- Cengage Learning EMEA(Publisher)
All Rights Reserved. May not be copied, scanned, or duplicated, in whole or in part. Due to electronic rights, some third party content may be suppressed from the eBook and/or eChapter(s). Editorial review has deemed that any suppressed content does not materially affect the overall learning experience. Cengage Learning reserves the right to remove additional content at any time if subsequent rights restrictions require it. 3.3 The Two Major Types of Chemical Bonds A. Ionic and Covalent Bonds According to the Lewis model of chemical bonding, atoms bond together in such a way that each atom participating in a bond acquires a valence-shell electron configuration the same as that of the noble gas nearest to it in atomic number. Atoms acquire completed valence shells in two ways: 1. An atom may lose or gain enough electrons to acquire a filled valence shell, becoming an ion as it does so (Section 3.1). An ionic bond results from the force of electrostatic attraction between a cation and an anion. 2. An atom may share electrons with one or more other atoms to acquire a filled valence shell. A covalent bond results from the force of attraction between two atoms that share one or more pairs of electrons. A molecule or polyatomic ion is formed. Whether two atoms in a compound are bonded by an ionic bond or a co-valent bond is determined by their relative positions in the Periodic Table. Ionic bonds usually form between a metal and a nonmetal. An example of an ionic bond is that formed between the metal sodium and the nonmetal chlorine in the compound sodium chloride, Na 1 Cl 2 . When two nonmetals or a metalloid and a nonmetal combine, the bond between them is usually covalent. Examples of compounds containing covalent bonds between non-metals include Cl 2 , H 2 O, CH 4 , and NH 3 . Examples of compounds contain-ing covalent bonds between a metalloid and a nonmetal include BF 3 , SiCl 4 , and AsH 3 .
eBook - PDFThe Sciences
An Integrated Approach
- James Trefil, Robert M. Hazen(Authors)
- 2022(Publication Date)
- Wiley(Publisher)
This situation may require that they exchange or share electrons. Usually, that process involves rearrangements with a total of 2, 10, 18, or 36 electrons. Chemical bonds result from any redistribution of electrons that leads to a more stable configuration between two or more atoms—especially configurations with a filled elec- tron shell. • Most atoms adopt one of three simple strategies to achieve a filled shell: they give away electrons, accept electrons, or share electrons. If the bond formation takes place spontaneously, without outside intervention, energy will be released in the reaction. The burning of wood or paper (once their temperature has been raised high enough) is a good example of this sort of process, and the heat you feel when you put your hands toward a fire derives ultimately from the chemical potential energy that is given off as electrons and atoms are reshuffled. Alternatively, atoms may be pushed into new configurations by adding energy to systems. Much of industrial chemis- try, from the smelting of iron to the synthesis of plastics, operates on this principle. 10.3 Types of Chemical Bonds Atoms link together by three principal kinds of chemical bonds—ionic, metallic, and covalent—all of which involve redistributing electrons between atoms. In addition, polar- ization, hydrogen bonding, and van der Waals forces result from shifts of electrons within their atoms or groups of atoms. Each type of bonding corresponds to a different way of rearranging electrons, and each produces distinctive properties in the materials it forms. 1 H 1.00794 3 Li 6.941 4 Be 9.01218 11 Na 22.98977 12 Mg 24.3050 2 He 4.00260 5 B 10.811 6 C 12.011 7 N 14.00674 8 O 15.9994 9 F 18.99840 10 Ne 20.1797 13 Al 26.98154 14 Si 28.0855 15 P 30.97376 16 S 32.066 17 Cl 35.4527 18 Ar 39.948 FIGURE 10.1 The first three rows of the periodic table, containing elements 1 and 2, 3 through 10, and 11 through 18, respectively, hold the key to understanding chemical bonding.
eBook - PDFChemistry
An Atoms First Approach
- Steven Zumdahl, Susan Zumdahl, Donald J. DeCoste, , Steven Zumdahl, Steven Zumdahl, Susan Zumdahl, Donald J. DeCoste(Authors)
- 2020(Publication Date)
- Cengage Learning EMEA(Publisher)
Bonding: General Concepts CHAPTER 3 3.1 Types of Chemical Bonds 3.2 Electronegativity 3.3 Ions: Electron Configurations and Sizes Predicting Formulas of Ionic Compounds Sizes of Ions 3.4 Partial Ionic Character of Covalent Bonds 3.5 The Covalent Chemical Bond: A Model Models: An Overview 3.6 The Localized Electron Bonding Model 3.7 Lewis Structures 3.8 Exceptions to the Octet Rule Odd-Electron Molecules 3.9 Resonance Formal Charge 3.10 Naming Simple Compounds Binary Ionic Compounds (Type I) Formulas from Names Binary Ionic Compounds (Type II) Ionic Compounds with Polyatomic Ions Binary Covalent Compounds (Type III) Acids The nudibranch uses a particular molecule (called an allomone) to defend itself against predators. (Manex Catalapiedra/Getty Images) 98 Copyright 2021 Cengage Learning. All Rights Reserved. May not be copied, scanned, or duplicated, in whole or in part. Due to electronic rights, some third party content may be suppressed from the eBook and/or eChapter(s). Editorial review has deemed that any suppressed content does not materially affect the overall learning experience. Cengage Learning reserves the right to remove additional content at any time if subsequent rights restrictions require it. A s we examine the world around us, we find it to be composed almost entirely of compounds and mixtures of compounds: Rocks, coal, soil, petroleum, trees, and human bodies are all complex mixtures of chemical compounds in which different kinds of atoms are bound together. Substances composed of unbound atoms do exist in nature, but they are very rare. Examples are the argon in the atmosphere and the helium mixed with natural gas reserves. The manner in which atoms are bound together has a profound effect on chemical and physical properties. For example, graphite is a soft, slippery material used as a lubricant in locks, and diamond is one of the hardest materials known, valuable both as a gemstone and in industrial cutting tools.
Alternatively, atoms may be pushed into new configurations by adding energy to systems. Much of industrial chemis- try, from the smelting of iron to the synthesis of plastics, operates on this principle. 1 H 1.00794 3 Li 6.941 4 Be 9.01218 11 Na 22.98977 12 Mg 24.3050 2 He 4.00260 5 B 10.811 6 C 12.011 7 N 14.00674 8 O 15.9994 9 F 18.99840 10 Ne 20.1797 13 Al 26.98154 14 Si 28.0855 15 P 30.97376 16 S 32.066 17 Cl 35.4527 18 Ar 39.948 Figure 10-1 • The first three rows of the periodic table, containing elements 1 and 2, 3 through 10, and 11 through 18, respectively, hold the key to understanding chemical bonding. Types of Chemical Bonds Atoms link together by three principal kinds of chemical bonds—ionic, metallic, and covalent—all of which involve redistributing electrons between atoms. In addition, polar- ization, hydrogen bonding, and van der Waals forces result from shifts of electrons within their atoms or groups of atoms. Each type of bonding corresponds to a different way of rearranging electrons, and each produces distinctive properties in the materials it forms. Types of Chemical Bonds | 209 IONIC BONDS We’ve seen that atoms with “magic numbers” of 2, 10, 18, or 36 electrons are particu- larly stable. By the same token, atoms that differ from these magic numbers by only one electron in their outer orbits are particularly reactive—in effect, they are “anxious” to fill or empty their outer orbits. Such atoms tend to form ionic bonds, chemical bonds in which the electrical force between two oppositely charged ions holds the atoms together. Ionic bonds often form as one atom gives up an electron while another receives it. Sodium (a soft, silvery white metal), for example, has 11 electrons in an electrically neutral atom—2 in the lowest orbit, 8 in the next, and a single electron with lots of chemical potential energy in its outer shell. Sodium’s best bonding strategy, therefore, is to lose one electron.
eBook - PDF- 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
eBook - PDF- Amos Turk(Author)
- 2013(Publication Date)
- Academic Press(Publisher)
7 • Types of Chemical Bonds 7.1 • INTRODUCTION Most molecules that are stable under terrestrial conditions are de-stroyed at temperatures above about 10 3 or 10 4 O C, and other species of matter become predominant. Typical among these are N, 0, CaH, AICI, (LiF) 3 , Na 2 CI + , and NaCI 2 . At still higher temperatures, more extensive ionization occurs until matter consists largely of individual nuclei which move about independently of their electrons. This condition is called the state. At high pressures, 10 5 -10 6 atm, most sub-stances become metallic (Ch. 23); wood and chalk (CaC0 3 ), for ex-ample, become metallic conductors under pressures of about 10 5 atm. These remarks emphasize that our study of chemical bonding is largely directed to phenomena that occur under conditions that are familiar to us on earth. 7.2 • WHAT TYPE OF ATTRACTIVE FORCES HOLD ATOMS TOGETHER IN CHEMICAL BONDS? We know of three types of attractive forces among macroscopic bodies —gravitational, magnetic, and electrostatic. Of these, only electrostatic forces are strong enough to account for observed bond energies. The simplest notion we might entertain, then, is that chemical bonds are the result of Coulombic forces of attraction between individual positive and negative ions. Such an idea was the basis for the of Jons Jakob Berzelius, Humphry Davy, and others in the nineteenth century. Thus, sodium atoms were thought to be positively charged, or at least to acquire such a charge near other atoms. Oxygen atoms, on the other hand, were believed to be negative. A positive charge was considered to characterize a basic substance, a negative charge an acidic substance. The resulting attraction accounted for the forma-110 I l l • 7.3 L E W I S S Y M B O L S tion of the compound Na 2 0. But the positive charge on 2Na was thought to be greater than the negative charge on 0, with the result that Na 2 0 was considered to have some residual positive charge, accounting for its basic character.
eBook - PDF- Edward J. Neth, Paul Flowers, Klaus Theopold, Richard Langley, William R. Robinson(Authors)
- 2019(Publication Date)
- Openstax(Publisher)
For example, two hydrogen atoms bond covalently to form an H 2 molecule; each hydrogen atom in the H 2 molecule has two electrons stabilizing it, giving each atom the same number of valence electrons as the noble gas He. Compounds that contain covalent bonds exhibit different physical properties than ionic compounds. Because the attraction between molecules, which are electrically neutral, is weaker than that between electrically charged ions, covalent compounds generally have much lower melting and boiling points than ionic compounds. In fact, many covalent compounds are liquids or gases at room temperature, and, in their solid states, they are typically much softer than ionic solids. Furthermore, whereas ionic compounds are good conductors of electricity when dissolved in water, most covalent compounds are insoluble in water; since they are electrically neutral, they are poor conductors of electricity in any state. Formation of Covalent Bonds Nonmetal atoms frequently form covalent bonds with other nonmetal atoms. For example, the hydrogen molecule, H 2 , contains a covalent bond between its two hydrogen atoms. Figure 4.4 illustrates why this bond is formed. Starting on the far right, we have two separate hydrogen atoms with a particular potential energy, indicated by the red line. Along the x-axis is the distance between the two atoms. As the two atoms approach each other (moving left along the x-axis), their valence orbitals (1s) begin to overlap. The single electrons on each hydrogen atom then interact with both atomic nuclei, occupying the space around both atoms. The strong attraction of each shared electron to both nuclei stabilizes the system, and the potential energy decreases as the bond distance decreases. If the atoms continue to approach each other, the positive charges in the two nuclei begin to repel each other, and the potential energy increases. The bond length is determined by the distance at which the lowest potential energy is achieved.
eBook - PDF- Bernard Moody(Author)
- 2013(Publication Date)
- Arnold(Publisher)
5 Bonding and the structures displayed by elements and their compounds The general physical properties of compounds related to bond type The nature of the bonding in a compound and of the geometrical pattern adopted by the ions or molecules in a solid, will largely determine the physical properties ofthat substance. While distinc-tive properties associated with ionic and covalent bonding may be discerned, there is a gradual merging of characteristics when the compounds of a large number of elements are compared. This gradual transition is not altogether unexpected. When fused or dissolved in water, an ionic com-pound will conduct electricity. The current is carried through the liquid by the ions which gain their mobility when the compound is melted or dispersed in a solvent. Unless a reaction occurs with the solvent, covalent substances yield non-conducting liquids. In the crystal lattice of an ionic compound, each ion is surrounded by oppositely charged ions, the number depending on the particular pattern adopted in the crystal. Strong electrical forces hold the ions in position although each atom oscillates by virtue of its thermal energy. Considerable energy is required to overcome the forces of attraction and ionic compounds usually melt at high temperatures and are non-volatile. On the other hand, covalent molecules, each electrically neutral, are held by much weaker intermolecular forces. Therefore, fusion, boiling and sublimation are relatively easy to accomplish. To illustrate this point, the melting-points of the fluorides formed by the elements of Period 3, sodium-sulphur, are shown in Table 5.1.
eBook - PDF- Brian W. Pfennig(Author)
- 2021(Publication Date)
- Wiley(Publisher)
4 An Introduction to Chemical Bonding “A bond does not really exist at all—it is a most convenient fiction.” —Charles Coulson 4.1 THE DEFINITION OF A CHEMICAL BOND Almost every chemical reaction involves the making and/or breaking of a chemical bond. Despite its central importance in the lexicon of chemistry, there continues to be a healthy debate about what a bond actually is, so much so that the British theoretician, Charles Coulson, once quipped that “a bond does not really exist at all—it is a most convenient fiction.” Suppose that I asked my students for their definition of a chemical bond. I imagine that many of them might turn to the fountain of all knowledge known as Wikipedia for a definition. Going straight to the source myself, Wikipedia defines a chemical bond as “a lasting attraction between atoms that enables the formation of a chemical compound,” a circular argument if ever there was one. The Collins English dic- tionary has only a slightly better answer, defining a bond as “a mutual attraction between two atoms resulting from a redistribution of their outer electrons.” Dissatisfied with either of these definitions, I thought I would turn to the OG himself—Gilbert Newton Lewis, who is arguably the godfather of the chemical bond.
eBook - ePubUnderstanding Basic Chemistry
The Learner's Approach
- Kim Seng Chan, Jeanne Tan(Authors)
- 2014(Publication Date)
- WSPC(Publisher)
to gain electrons across the period!In a nutshell, remember:•Elements across a period experience increasing ease to gain electrons BUT decreasing ease to lose electrons.•Elements down a group experience decreasing ease to gain electrons BUT increasing ease to lose electrons.3.1 Metallic BondingChemical bonds are electrostatic forces of attraction (positive charge attracting negative charge) that bind particles together to form matter. When different types of particles interact electrostatically, different Types of Chemical Bonds are formed. There are four different types of conventional chemical bonds, namely, metallic, ionic, covalent, and intermolecular forces.Within a metal, atoms partially lose their loosely bound valence electrons. These electrons are mobile and delocalized, not belonging to any one single atom and yet not completely lost from the lattice.A metal can thus be viewed as a rigid lattice of positive ions surrounded by a sea of delocalized electrons. What holds the lattice together is the strong metallic bonding — the electrostatic attraction between the positive ions and the delocalized valence electrons.Metallic bonds are strong and non-directional. Therefore, when a force is applied across a piece of metal, the metal atoms can slide over one another without breaking of the metallic bonds. This accounts for the malleability (can be deformed into different shapes) and ductility (can be drawn into wires) of metals.Since metallic bonding is the result of the interaction between the delocalized electrons and the positive ions, the strength of a metallic bond depends on:•The number
eBook - PDF- Morris Hein, Susan Arena, Cary Willard(Authors)
- 2016(Publication Date)
- Wiley(Publisher)
An ionic bond is the attraction between oppositely charged ions. Ionic bonds are formed whenever one or more electrons are transferred from one atom to another. Metals, which have relatively little attraction for their valence electrons, tend to form ionic bonds when they combine with nonmetals. It’s important to recognize that substances with ionic bonds do not exist as molecules. In sodium chloride, for example, the bond does not exist solely between a single sodium ion and a single chloride ion. Each sodium ion in the crystal attracts six near-neighbor negative chloride ions; in turn, each negative chloride ion attracts six near-neighbor posi- tive sodium ions (see Figure 11.5). A metal will usually have one, two, or three electrons in its outer energy level. In reacting, metal atoms characteristically lose these electrons, attain the electron structure of a noble gas, and become positive ions. A nonmetal, on the other hand, is only a few electrons short of having a noble gas electron structure in its outer energy level and thus has a tendency to gain electrons. In reacting with metals, nonmetal atoms characteristically gain one to four electrons, attain the electron structure of a noble gas, and become negative ions. The ions 226 CHAPTER 11 • Chemical Bonds: The Formation of Compounds from Atoms formed by loss of electrons are much smaller than the corresponding metal atoms; the ions formed by gaining electrons are larger than the corresponding nonmetal atoms. The dimen- sions of the atomic and ionic radii of several metals and nonmetals are given in TABLE 11.3. P R A C T I C E 1 1 . 3 What noble gas structure is formed when an atom of each of these metals loses all its valence electrons? Write the formula for the metal ion formed. (a) K (b) Mg (c) Al (d) Ba Study the following examples. Note the loss and gain of electrons between atoms; also note that the ions in each compound have a noble gas electron structure.
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