Outline Covalent Bonds. Covalent Bonds

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1 Outline 5.1 Covalent Bonds 5.2 Covalent Bonds and the Periodic Table 5.3 Multiple Covalent Bonds 5.4 Coordinate Covalent Bonds 5.10 Naming Binary Molecular Compounds 5.11 Characteristics of Molecular Compounds 5. 1 Covalent Bonds The bond formed when atoms share electrons is called a covalent bond. (Unlike ionic bonds, which involve the complete transfer of electrons). A group of atoms held together by covalent bonds is called a molecule. Main group elements can obtain completed outer subshells with eight valence electrons (or two for hydrogen), so that they have a noble gas electron configuration, by sharing an appropriate number of electrons in covalent bonds. Prentice Hall 2007 Chapter Five 1 Prentice Hall 2007 Chapter Five 2 Covalent bonds form Covalent Bonds when atoms share electrons to complete octets. A single molecule of water contains two hydrogen atoms and one oxygen atom covalently bonded to one another. We might visualize a water molecule using a space-filling model as shown here: between two nonmetal atoms. between nonmetal atoms from Groups 4A(14), 5A(15), 6A(16), and 7A(17). 3 Prentice Hall 2007 Chapter Five 4 When two atoms come together, electrical interactions occur. Some of these interactions are repulsive the two positively charged nuclei repel each other and the negatively charged electrons repel each other. Other interactions, however, are attractive each nucleus attracts the electrons and each electron attracts both nuclei. When the attractive forces are stronger than the repulsive forces, a covalent bond is formed and the atoms stay together. When the nucleus electron attractions (blue arrows) are greater than the nucleus nucleus and electron electron repulsions (red arrows), the result is a net attractive force that holds the atoms together to form a molecule. Prentice Hall 2007 Chapter Five 5 Prentice Hall 2007 Chapter Five 6 1

2 Covalent bond formation in H 2 can be visualized by imagining that the two spherical 1s atomic orbitals blend together and overlap to give an egg-shaped molecular orbital. Both atoms share the two valence electrons and the stability of the closed shell electron configuration. The shared pair of electrons in a covalent bond can be represented as a line between atoms. If atoms are too far apart, attractions are weak and no bonding occurs. If atoms are too close, strong repulsions occur. When atoms are optimally separated, the energy is at a minimum. The distance between nuclei at this minimum energy point is called the bond length. Prentice Hall 2007 Chapter Five 7 Prentice Hall 2007 Chapter Five 8 A graph of potential energy versus internuclear distance for the H 2 molecule. An individual Cl atom has 7 valence electrons. 6 of these are paired and the 7 th is unpaired. When two Cl atoms approach each other, the unpaired 3p electrons are shared by both atoms in a covalent bond. Each Cl atom in the molecule now owns six outershell electrons and shares two more, giving each a valence shell octet like that of the noble gas Ar. Prentice Hall 2007 Chapter Five 9 Prentice Hall 2007 Chapter Five 10 Forming Octets in Molecules Carbon forms 4 covalent bonds In a fluorine, F 2,, molecule, each F atom (diatonic) shares one electron. attains an octet. In a CH 4, methane, molecule a C atom shares 4 electrons to attain an octet. each H shares 1 electron to become stable like helium

3 In nitrogen molecule, N 2, Multiple Bonds each N atom shares 3 electrons. each N attains an octet. the bond is a multiple bond called a triple bond. the name is the same as the element. Bond formation in Cl 2 can also be pictured as the overlap of the two 3p atomic orbitals containing the single unpaired electrons. The molecular orbital formed creates a region of high electron density between the two nuclei. 13 Prentice Hall 2007 Chapter Five 14 In addition to H 2 and Cl 2, five other elements always exist as diatomic (two-atom) molecules. N 2 and O 2 are colorless, odorless, nontoxic gases. F 2 is a pale yellow, highly reactive gas; Br 2 is a dark red, toxic liquid; and I 2 is a violet, crystalline solid. 5.2 Covalent Bonds and the Periodic Table Covalent bonds can form between unlike atoms making possible a vast number of molecular compounds: compounds that consist of molecules rather than ions. Water molecules consist of two hydrogen atoms joined by covalent bonds to an oxygen atom, ammonia molecules consist of three hydrogen atoms covalently bonded to a nitrogen atom, and methane molecules consist of four hydrogen atoms covalently bonded to a carbon atom. Prentice Hall 2007 Chapter Five 15 Prentice Hall 2007 Chapter Five 16 Note that in all these examples, each atom shares enough electrons to achieve a noble gas configuration: two electrons for hydrogen, and octets for oxygen, nitrogen, and carbon. Number of bonds formed to achieve octet. Numbers in parentheses indicate possible numbers of bonds that result in exceptions to the octet rule. Prentice Hall 2007 Chapter Five 17 Prentice Hall 2007 Chapter Five 18 3

4 The octet rule is a useful guideline, but it has numerous exceptions. Boron has only 3 valence electrons it can share and thus forms compounds in which it has only 3 covalent bonds. Elements in the third row and below have vacant d orbitals that can be used to make more than 4 bonds. 5.3 Multiple Covalent Bonds The bonding in some molecules cannot be explained by the sharing of only two electrons between atoms. The only way the atoms in CO 2 and N 2 can have octets is by sharing more than two electrons. Prentice Hall 2007 Chapter Five 19 Prentice Hall 2007 Chapter Five 20 Single bond: A covalent bond formed by sharing one electron pair. Double bond: A covalent bond formed by sharing two electron pairs. Triple bond: A covalent bond formed by sharing three electron pairs. Just as a single bond is represented by a single line between atoms, a double bond is represented by two lines between atoms and a triple bond by three lines. Carbon, nitrogen, and oxygen are the elements most often present in multiple bonds. Prentice Hall 2007 Chapter Five 21 Prentice Hall 2007 Chapter Five 22 Ethylene, a simple compound used commercially to induce ripening in fruit, has the formula C 2 H 4. The only way for the 2 carbon atoms to have octets is for them to share 4 electrons in a double bond: Acetylene, the gas used in welding, has the formula C 2 H 2. To achieve octets, two carbons share six electrons in a triple bond. In compounds with multiple bonds like ethylene and acetylene, each carbon atom still forms a total of four covalent bonds. Prentice Hall 2007 Chapter Five 23 Prentice Hall 2007 Chapter Five 24 4

5 5.4 Coordinate Covalent Bonds Coordinate covalent bond: The covalent bond that forms when both electrons are donated by the same atom. The ammonium ion, is an example of a species with a coordinate covalent bond. Coordination compounds are an entire class of substances based on the ability of transition metals to form coordinate covalent bonds with nonmetals. Essential metal ions are held in enzyme molecules by coordinate covalent bonds. Prentice Hall 2007 Chapter Five 25 Prentice Hall 2007 Chapter Five Naming Binary Molecular Compounds The prefix mono- is omitted for the first element. The formulas of binary molecular compounds are written with the less electronegative element first. Name the first element in the formula, using a prefix to indicate the number of atoms. Name the second element in the formula, using the ending -ide as for anions along with a prefix if needed. Prentice Hall 2007 Chapter Five 27 Prentice Hall 2007 Chapter Five 28 The structures and names of several binary molecular compounds are shown below. Naming Covalent Compounds What is the name of SO 3? 1. The first nonmetal is S sulfur. 2. The second nonmetal is O named oxide. 3. The subscript 3 of O is shown as the prefix tri. SO 3 sulfur trioxide The subscript 1 (for S) or mono is understood. Prentice Hall 2007 Chapter Five

6 Naming Covalent Compounds Name P 4 S The first nonmetal P is phosphorus. 2. The second nonmetal S is sulfide. 3. The subscript 4 of P is shown as tetra. The subscript 3 of O is shown as tri. P 4 S 3 tetraphosphorus trisulfide Learning Check Select the correct name for each compound. A. SiCl 4 1) silicon chloride 2) tetrasilicon chloride 3) silicon tetrachloride B. P 2 O 5 1) phosphorus oxide 2) phosphorus pentoxide 3) diphosphorus pentoxide C. Cl 2 O 7 1) dichlorine heptoxide 2) dichlorine oxide 3) chlorine heptoxide Solution Select the correct name for each compound Characteristics of Molecular Compounds A. SiCl 4 3) silicon tetrachloride B. P 2 O 5 3) diphosphorus pentoxide C. Cl 2 O 7 1) dichlorine heptoxide 33 Prentice Hall 2007 Chapter Five 34 Learning Check Identify each compound as ionic or covalent and give its correct name. A. SO 3 B. BaCl 2 C. (NH 4 ) 3 PO 4 D. Cu 2 CO 3 E. N 2 O 4 Solution Identify each compound as ionic or covalent and give its correct name. A. SO 3 covalent sulfur trioxide B. BaCl 2 ionic barium chloride C. (NH 4 ) 3 PO 3 ionic ammonium phosphite D. Cu 2 CO 3 ionic copper(i) carbonate E. N 2 O 4 covalent dinitrogen tetroxide

7 Chapter Summary A covalent bond is formed by the sharing of electrons between atoms rather than by the complete transfer of electrons from one atom to another. Two shared electrons are a single bond, four are a double bond, and six are a triple bond. The group of atoms held together by covalent bonds is called a molecule. When a lone pair of electrons on one atom overlaps a vacant orbital on another atom a coordinate covalent bond is formed. An atom shares enough electrons to reach a noble gas configuration. Prentice Hall 2007 Chapter Five 37 Chapter Summary Contd. Molecular formulas show the numbers and kinds of atoms in a molecule. Lewis structures show how atoms are connected in molecules. Covalent bonds are indicated as lines between atoms, and valence electron lone pairs are shown as dots. Molecules have shapes that can be predicted using the VSEPR model. The electronic geometry of atoms with 2 electron charge clouds is linear, with 3 it is planar triangular, and with 4 it is tetrahedral. Prentice Hall 2007 Chapter Five 38 Chapter Summary Contd. Bonds between atoms are polar if the bonding electrons are not shared equally between the atoms. The ability of an atom to attract electrons is electronegativity. It is highest on the upper right of the periodic table and lowest on the lower left. Molecular polarity is the sum of all individual bond polarities and lone pair contributions in a molecule. Molecular compounds usually have lower melting points and boiling points than ionic compounds, many are water insoluble, and they do not conduct electricity when melted or dissolved. Prentice Hall 2007 Chapter Five 39 7

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