Chemical Bonding. Introduction to Chemical Bonding Section 6.1
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1 Chemical Bonding Introduction to Chemical Bonding Section 6.1
2 Objectives 1. Define chemical bond. 2. Explain why most atoms form chemical bonds. 3. Describe ionic and covalent bonding. 4. Explain why most chemical bonding is neither purely ionic nor purely covalent. 5. Classify bonding type according to electronegativity differences.
3 Main Idea Chemical Bonds Atoms form compounds by binding together either by gaining, losing, or sharing electrons
4 Key Terms Chemical Bond Polarity Dipole Ionic Bonding Polar Covalent Bond Nonpolar Covalent Bond Electronegativity Covalent Bonding
5 Electronegativity Measure of an atom s ability to attract bonding electrons Function of Ionization Energy & Electron Affinity: IE => how strongly an atom holds onto its e EA => how strongly an atom attracts other e- Trends: Increasing across periods Decreasing down groups High for non-metals Low for metals and transition metals
6 Bonding and Electronegativity Predict the type of chemical bond atoms will form from the difference in EN of the atoms Types of Bonds: 1. Nonpolar covalent 2. Polar covalent 3. Ionic
7 Some Electronegativity Values
8 Biggest Change of Electronegativity on the Periodic Table Electronegativity of Fluorine: 4.0 Electronegativity of Cesium: 0.7 Difference = 3.3 Implications?
9 Predicting Bond Character with EN Differences
10 Ionic vs. Covalent Bonding
11 Nonpolar Covalent Bonds Occur bet ween nonmetals An equal or almost equal sharing of electrons Almost no EN difference (0.0 to 0.4) Molecule Diff. in EN Type of bond
12 Polar Covalent Bonds Bet ween nonmetal atoms that do not share electrons equally Moderate EN difference (0.5 to 1.7) Molecule Diff. in EN Type of bond
13 Comparing Types of Covalent Bonds
14 Polarity Polarity is the relationship bet ween t wo physical characteristics or tendencies which are opposite in orientation Bond Polarity describes the sharing of electrons bet ween 2 atoms Bond Polarity increases as difference in EN values of bonding atoms increases
15 Bond Polarity and Dipoles Polar covalent bonds have a separation of charges called a DIPOLE Size of Dipole is measured by its Dipole Moment: μ=qxr q=charge; r=distance between centers Electrons are pulled toward more EN atom Creating equal but opposite charges in bond
16 Examples of Dipoles in Polar Covalent Bonds δ represents the par:al posi:ve and nega:ve charges in the atom due to the a=rac:on of electrons by the more EN atom Indicates pull of electrons toward more EN atom
17 Ionic Bonds
18 Ionic Bonds Occur bet ween metal and nonmetal ions Result from electron transfer Large EN difference ( 1.8 or more ) Molecule Diff. in EN Type of bond
19 Another View
20 Electronegativity and Bond Types
21 Predicting Bond Types
22 Example Use the EN difference to identify the type of bond bet ween the following atoms as nonpolar covalent, polar covalent, or ionic 1. K-N 2. N-O 3. Cl-Cl 4. B-Cl
23 Solution Use the EN difference to identify the type of bond bet ween the following atoms as nonpolar covalent, polar covalent, or ionic 1. K-N 2.2 Ionic 2. N-O 0.5 Polar Covalent 3. Cl-Cl 0.0 Nonpolar Covalent 4. B-Cl 1.0 Polar Covalent
24 Review A chemical bond is a mutual electrical attraction bet ween the nuclei and valence electrons of different atoms that binds the atoms together Covalent bonding results from the sharing of electron pairs bet ween to atoms: Polar bonds share e- unequally Non-polar bonds share e- equally Ionic bonding results from the electrical attraction of cations and anions
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