Resonance Structures Resonance structures
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1 Resonance Structures Resonance structures are two or more electron-dot formulas for the same arrangement of atoms. related by a double-headed arrow ( ). written by changing the location of a double bond between the central atom and a different attached atom.
2 Writing Resonance Structures for SO2
3 Learning Check FNO 2, a rocket propellant, has two resonance structures. One is shown below. What is the other resonance structure?
4 Solution FNO 2, a rocket propellant, has two resonance structures. One is shown below. What is the other resonance structure?
5 Names of Covalent Compounds When naming a covalent compound, the first nonmetal in the formula is named by its element name, and the second nonmetal is named using the first syllable of its element name, followed by ide. Prefixes are used to indicate the number of atoms present for each element in the compound, and because two nonmetals can form two or more different compounds
6 Prefixes Used in Naming Covalent Compounds
7 Some Covalent Compounds 2013 Pearson Education, Inc. Chapter 5, Section 1 7
8 Guide to Naming Covalent Compounds with Two Nonmetals
9 Naming Covalent Compounds, SO 2 Analyze the Problem. Symbols of Elements S Name sulfur oxygen Subscripts 1 2 Prefix (none) understood di Step 1 Name the first nonmetal by its element name. In SO 2, the first nonmetal (S) is sulfur. O 2013 Pearson Education, Inc. Chapter 5, Section 1 9
10 Naming Covalent Compounds, SO 2 Step 2 Name the second nonmetal by using the first syllable of its name followed by ide. The second nonmetal (O) is named oxide. Step 3 Add prefixes to indicate the number of atoms (subscripts). Because there is one sulfur atom, no prefix is needed. The subscript two for the oxygen atoms is written as the prefix di. The name of SO 2 is sulfur dioxide Pearson Education, Inc. Chapter 5, Section 1 10
11 Learning Check Name the covalent compound P 2 O Pearson Education, Inc. Chapter 5, Section 1 11
12 Solution Name the covalent compound P 2 O 5. Analyze the Problem. Symbols of Elements P O Name phosphorus oxygen Subscripts 2 5 Prefix di penta Step 1 Name the first nonmetal by its element name. In P 2 O 5, the first nonmetal (P) is phosphorus Pearson Education, Inc. Chapter 5, Section 1 12
13 Solution Step 2 Name the second nonmetal by using the first syllable of its name followed by ide. The second nonmetal (O) is named oxide. Step 3 Add prefixes to indicate the number of atoms (subscripts). The subscript for the two P atoms is di; the subscript for the five oxygen atoms is penta. The name of P 2 O 5 is phosphorus pentoxide. When the vowels o and o, or a and o appear together (pentaoxide), the first vowel is omitted Pearson Education, Inc. Chapter 5, Section 1 13
14 Learning Check Select the correct name for each compound. 1. SiCl 4 A. silicon chloride B. tetrasilicon chloride C. silicon tetrachloride
15 #2 Name Cl 2 O 7 A. dichlorine heptoxide B. dichlorine oxide C. chlorine heptoxide
16 Writing Formulas of Covalent Compounds Write the formula for sulfur hexafluoride. Analyze the Problem. Name sulfur hexafluoride Symbols of Elements S F Subscripts 1 6 (from hexa) Step 1 Write the symbols in order of the elements in the name. S F Step 2 Write any prefixes as subscripts. Prefix hexa = 6 Formula: SF 6
17 Learning Check Write the correct formula for dinitrogen trioxide.
18 Learning Check Name each of the following compounds. 1. Ca 3 (PO 4 ) 2 2. FeBr 3 3. SCl 2 4. Cl 2 O
19 Solution Name each of the following compounds. 1. Ca 3 (PO 4 ) 2 Ca 2+, PO 3 4 calcium phosphate 2. FeBr 3 Fe 3+, Br iron(iii) bromide 3. SCl 2 1 S, 2 Cl sulfur dichloride 4. Cl 2 O 2 Cl, 1 O dichlorine oxide
20 Learning Check Write the formulas for the following compounds. 1. calcium nitrate 2. boron trifluoride 3. aluminum carbonate 4. dinitrogen tetroxide 5. copper(i) phosphate
21 Solution Write the formulas for the following compounds. 1. calcium nitrate Ca 2+, NO 3 Ca(NO 3 ) 2 2. boron trifluoride 1 B, 3 F BF 3 3. aluminum carbonate Al 3+, CO 2 3 Al 2 (CO 3 ) 3 4. dinitrogen tetroxide 2 N, 4 O N 2 O 4 5. copper(i) phosphate Cu +, PO 3 4 Cu 3 PO 4
22 Electronegativity Electronegativity is a measure of an atom s ability to attract bonding electrons. increases from left to right, going across a period on the periodic table. decreases going down a group on the periodic table. is high for the nonmetals, with fluorine as the highest. is low for the metals and transition metals.
23 Bonding and Electronegativity The difference in the electronegativity of two atoms can be used to predict the type of bond that forms. Bonds are classified as: nonpolar covalent polar covalent ionic
24 Some Electronegativity Values 2013 Pearson Education, Inc. Chapter 5, Section 1 24
25 Nonpolar Covalent Bonds A nonpolar covalent bond occurs between nonmetals. has an equal or almost equal sharing of electrons. has almost no electronegativity difference (0.0 to 0.4). Examples: Atoms Electronegativity Type of Bond Difference
26 Polar Covalent Bonds A polar covalent bond occurs between nonmetal atoms that do not share electrons equally. has a moderate electronegativity difference (0.5 to 1.7). Examples: Atoms Electronegativity Type of Bond Difference
27 Ionic Bonds An ionic bond occurs between metal and nonmetal ions. is a result of electron transfer. has a large electronegativity difference (1.8 or more). Examples: Atoms Electronegativity Type of Bond Difference
28 Electronegativity and Bond Types 2013 Pearson Education, Inc. Chapter 5, Section 1 28
29 Predicting Bond Types
30 Learning Check Use the electronegativity difference to identify the type of bond between the following atoms as nonpolar covalent (NP), polar covalent (P), or ionic (I). A. K N 2.2 B. N O 0.5 C. Cl Cl 0.0 D. B Cl 1.0
31 Break Time!!!
32 Valence-Shell Electron-Pair Repulsion Theory (VSEPR) In the valence-shell electron-pair repulsion (VSEPR) theory, the electron groups around a central atom are arranged as far apart from each other as possible. have the least amount of electron-electron repulsion. are used to predict the molecular shape.
33 Shapes of Molecules The three-dimensional shape of a molecule can be predicted by the number of bonding groups and lone-pair electrons around the central atom VSEPR theory (valence-shell-electron-pair repulsion).
34 Two Electron Groups In a molecule of BeCl 2, there are two electron groups bonded to the central atom, Be (Be is an exception to the octet rule). to minimize repulsion, the arrangement of two electron groups is 180, or opposite each other. the shape of the molecule is linear Pearson Education, Inc. Chapter 5, Section 1 34
35 Three Electron Groups In a molecule of BF 3, three electron groups are bonded to the central atom B (B is an exception to the octet rule). repulsion is minimized with 3 electron groups at angles of 120. the shape is trigonal planar Pearson Education, Inc. Chapter 5, Section 1 35
36 Three Electron Groups with a Lone Pair In a molecule of SO 2, S has 3 electron groups; 2 electron groups bonded to O atoms and one lone pair. repulsion is minimized with the electron groups at angles of 120, a trigonal planar arrangement. the shape is determined by the two O atoms bonded to S, giving SO 2 a bent (~120 ) shape Pearson Education, Inc. Chapter 5, Section 1 36
37 Four Electron Groups In a molecule of CH 4, there are four electron groups around C. repulsion is minimized by placing four electron groups at angles of 109, which is a tetrahedral arrangement. the four bonded atoms form a tetrahedral shape Pearson Education, Inc. Chapter 5, Section 1 37
38 Four Electron Groups with a Lone Pair In a molecule of NH 3, three electron groups bond to H atoms, and the fourth one is a lone (nonbonding) pair. repulsion is minimized with 4 electron groups in a tetrahedral arrangement. the three bonded atoms form a pyramidal (~109 ) shape Pearson Education, Inc. Chapter 5, Section 1 38
39 Four Electron Groups with Two Lone Pairs In a molecule of H 2 O, two electron groups are bonded to H atoms and two are lone pairs (4 electron groups). four electron groups minimize repulsion in a tetrahedral arrangement. the shape with two bonded atoms is bent (~109 ).
40 Molecular Shapes for 2 and 3 Bonded Atoms
41 Molecular Shapes for 4 Bonded Atoms
42 Guide to Predicting Molecular Shape (VSEPR Theory)
43 Predicting the Molecular Shape of H 2 Se Step 1 Draw the electron-dot formula. In the electrondot formula for H 2 Se, there are four electron groups, including two lone pairs of electrons around Se.
44 Predicting the Molecular Shape of H 2 Se Step 2 Arrange the electron groups around the central atom to minimize repulsion. The four electron groups around Se would have a tetrahedral arrangement. Step 3 Use the atoms bonded to the central atom to determine the molecular shape. Two bonded atoms give H 2 Se a bent shape with a bond angle of ~109.
45 Learning Check What is the shape of a molecule of NF 3?
46 Solution What is the shape of a molecule of NF 3? B. trigonal pyramidal Step 1 Draw the electron-dot formula. In the electron-dot structure for NF 3, there are three electron groups and a lone pair. F N F F
47 Solution What is the shape of a molecule of NF 3? B. trigonal pyramidal Step 2 Arrange the electron groups around the central atom to minimize repulsion. The four electron groups around N would have a tetrahedral arrangement. Step 3 Use the atoms bonded to the central atom to determine the molecular shape. Three bonding groups and a lone pair give NF 3 a trigonal pyramidal shape with a bond angle of 109.
48 Next Week Clicker Quiz on Chapter 5 Chapter 6 Group Assignment Ch5/6
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