For a quick and enjoyable introduction to Covalent vs Ionic Bonding watch this video:

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1 Covalent Bonding Covalent Bonding is the result of sharing of electron pairs between 2 nonmetal atoms Caution: sharing can be complicated Recall the Octet Rule: Atoms tend to gain, lose or share valence electrons Electron sharing occurs so that each atom attains the electron configuration of a noble gas. Each atom has a complete outer energy level using the shared electron pair(s) For a quick and enjoyable introduction to Covalent vs Ionic Bonding watch this video: Intro video: Helpful ideas and illustrations to help you take notes Covalent bonding Two non-metal atoms share a pair or pairs of electrons to achieve a complete outer energy level. What is the electrostatic force that holds covalent bonds together? The attractive force between the protons of one atom for the valence electrons of the second There are different types of covalent bonds. The type is determined by the elements involved. A) Single, Double or Triple Difference in number of shared pairs of electrons Two nonmetal atoms Share 1 pair of electrons Two nonmetal atoms Share 2 pairs of electrons Two nonmetal atoms Share 3 pairs of electrons

2 B) Polar or Non-polar Bond Difference determined by asking is the sharing of electrons equal Sharing is complicated. We evaluate sharing by calculating differences in electronegativity If the sharing is equal, we call the bond non-polar. If the sharing is unequal we call the bond polar. The more electronegative element is the negative end. To complete the calculations, you must look up or be given Electronegativity Values The formula Difference in EN = Large - Small value Final value is + The range used to classify the bond:

3 Process of Covalent Bond Formation Two atoms of H come in contact Same electronegativity values therefore share electrons to achieve a complete outer energy level Show sharing with Lewis Dot diagrams Each dash = 1 shared pair of electrons What is the electrostatic force of attraction? Force of attraction between protons of one atom for valence electrons of the second

4 Covalent bonds produce Molecules A Molecule is a neutral group of atoms that are held together by covalent bonds. A Molecule may be: 2 or more atoms of the same element Such as O 2 or O 3 2 or more atoms of different elements Such as H 2 O or C 12 H 22 O 11 Other large organic structures A Molecular Compound is a chemical compound whose units are molecules. A Molecular Formula Gives the composition of the compound It shows the types and numbers of atoms like a blueprint. Notice this is very different from the formula unit for an ionic compound. For Example: Dihydrogen monoxide H 2 O Carbon dioxide CO 2

5 The Name Game Notice any differences between ionic and molecular compound naming? Use prefixes to indicate the number of atoms Use the following examples to determine the rules for naming all Binary Molecular Compounds. Molecular Formula Name H 2 O dihydrogen monoxide CO carbon monoxide CH 4 carbon tetrahydride N 2 O 3 dinitrogen trioxide P 2 O 5 diphosphorous pentoxide

6 What do you think the rules are? How to name the element on the left How to name the element on the right

7 Diatomic Molecule This applies to 7 nonmetal elements When they are called for by name they come in a pair N 2 O 2 F 2 Cl 2 Br 2 I 2 and don t forget H 2 You must know these 7 Example of called for by name Hydrogen reacts with oxygen to produce dihydrogen monoxide H 2 + O 2 H 2 O

8 In Class More Practice Each dash represents one shared pair of electrons To check your work count around each atom to be sure each has a complete outer energy level (For most that is 8e s) To start a Lewis Structure for molecular compounds with more than 2 elements put the element that needs the most in the center. Need is determined by how many valence e s the element has.

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11 Unequal Sharing of e s Pairs Produces Polar Covalent Bonds Equal Sharing of e s Pairs Produces Non-polar Covalent Bonds Unequal is determined by a calculation Equal is determined by a calculation Big number small number = Difference Electronegativity If the difference in electronegativity Falls in the range of the bond is polar. In Big number small number = Difference In If the difference in electronegativity Falls in the range of the bond is non-polar Electronegativity For example: Bonds between S and H 1. Look up electronegativity In your text page 151 S H Do the math = 0.4 Because the electronegativity difference is 0.4 the bond is classified as polar.

12 3. Place the poles ( + and - ) The more electronegative element gets greater share of the e s and carries a negative charge ( - )

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14 Let s summarize where we are Characteristic Ionic Metallic Covalent Bonding Bonding Bonding Atoms of metals and Atoms of metals Atoms of nonmetal nonmetals with very elements Generally different electronegativities and ionization energies Formed Between that form cations and anions by transfer of electrons Polyatomic ions Electrostatic attraction Sea of e s Two non metal atoms between Delocalized electrons sharing pairs of electrons Bond Formed by oppositely charged ions around cations of the metal atoms based on electronegativity equally (non-polar) or unequally (polar) Properties of Bond Types (think compounds)

15 Example Substances

16 Name Characteristic Ionic Metallic Covalent Bonding Bonding Bonding What type of elements are in these bonds? How is the bond formed? What force(s) hold these bonds together? List properties of the substances formed.

17 Think Compounds Example Substances How are the compounds named? Think about the name game

18 Name Let s summarize where we are Characteristic Ionic Metallic Covalent Bonding Bonding Bonding Atoms of metals Atoms of nonmetal elements Generally Formed Between Sea of e s Delocalized electrons Bond Formed by around atoms Good conductors of heat and electricity in all states Properties of High m.p. Bond Type Lustrous Ductile Malleable Most solids at room

19 T Example Substances Let s summarize where we are (continued) You know all about the Periodic Table For Ionic Compounds Told what the constituents are you can write the name and formula unit. Given the formula unit you can write the name. Given the name you can write the formula unit. Metals You recognize by name and position on the periodic table

20 You know that many d block metals have variable oxidation numbers. Covalent Compounds Given a molecular formula you can write the molecular compound s name Given a molecular compound s name you can write the molecular formula Given a molecular formula you can draw the Lewis Structure Covalent Compounds to come: You can determine if the bonds are polar or non-polar using differences in electronegativity You can determine the shape of the molecule using VSEPR You can determine if the molecule is polar or non-polar

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