OFB Chapter 3 Chemical Periodicity and the Formation of Simple Compounds
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1 OFB hapter 3 hemical Periodicity and the Formation of Simple ompounds 3-1 Groups of Elements 3-2 The Periodic Table 3-3 Ions and Ionic ompounds 3-4 ovalent Bonding and Lewis Structures 3-5 Drawing Lewis Structures 3-6 Naming ompounds in which ovalent Bonding Occurs 3-7 the Shapes of Molecules 3-8 Elements Forming More than One Ion 8/26/2004 OFP hapter 3 1
2 8/26/2004 OFP hapter 3 2
3 Modern periodic law The chemical and physical properties of the elements are periodic functions of their atomic numbers. 8/26/2004 OFP hapter 3 3
4 8/26/2004 OFP hapter 3 4
5 Elements are classified as metal, non-metals, or semi-metals, and also fall into groups based on similarities in chemical and physical properties. 8/26/2004 OFP hapter 3 5
6 8/26/2004 OFP hapter 3 6
7 8/26/2004 OFP hapter 3 7
8 8/26/2004 OFP hapter 3 8
9 8/26/2004 OFP hapter 3 9
10 8/26/2004 OFP hapter 3 10
11 8/26/2004 OFP hapter 3 11
12 The Electronegativity (the power of an atom when in chemical combination to attract electrons to itself) is a periodic property. 8/26/2004 OFP hapter 3 12
13 Lewis Structures: Ionic compounds Whenever possible, the valence electrons in a compound are distributed in such a way that each main-group element in a molecule (except hydrogen) is surrounded by eight electrons (an octet of electrons). ydrogen should have two electrons in such a structure. 8/26/2004 OFP hapter 3 13
14 Lewis Structures: Na Na + a a 2+ Sodium atom Sodium ion alcium atom alcium ion Loss of a valence electron Gain of a valence electron ombination to form the compound Nal 8/26/2004 OFP hapter 3 14
15 8/26/2004 OFP hapter 3 15
16 Lewis Structures: ovalent ompounds Whenever possible, the valence electrons in a compound are distributed in such a way that each main-group element in a molecule (except hydrogen) is surrounded by eight electrons (an octet of electrons). ydrogen should have two electrons in such a structure. 8/26/2004 OFP hapter 3 16
17 Ammonia :N 3 Water 2 O: Methane 4 Ammonia and Water have a pair of lone electrons called an lone pairs 8/26/2004 OFP hapter 3 17
18 Ammonia (N 3 ) N. Nitrogen (Group V) 5 valence + 2 in 1s = 7 electrons :N: lone pair Lewis Structures N 8/26/2004 OFP hapter 3 18
19 methane carbon monoxide O ethane acetylene ethylene 8/26/2004 OFP hapter 3 19
20 Drawing Lewis Structures 1. ount up the total number of valence electrons available (symbolized by A) by first adding the group numbers of all the atoms present. If the species is a negative ion, add the absolute value of the total charge; if it is a positive ion, subtract it. 2. alculate the total number of electrons needed (N) for each atom to have its own noble-gas set of electrons around it (two for hydrogen, eight for the elements from carbon on in the periodic table). 3. Subtract the number in step 1 from the number in step 2. This is the number of shared (or bonding) electrons present (S). 4. Assign two bonding electrons (as one shared pair) to each connection between two atoms in the molecule or ion. 8/26/2004 OFP hapter 3 20
21 Drawing Lewis Structures 5. If any of the electrons earmarked for sharing remain, assign them in pairs by making some of the bonds double or triple bonds. In some cases, there may be more than one way to do this. In general, double bonds form only between atoms of carbon, nitrogen, oxygen, and sulfur. 6. Assign the remaining electrons as lone pairs to the atoms, giving octets to all atoms except hydrogen. 7. Determine the formal charge on each atom, and write it next to that atom. heck that the formal charges add to give a correct total charge on the molecule or molecular ion. Formal charge = group number - lonepair electrons - ½ (number of electrons in bonding pairs) 8/26/2004 OFP hapter 3 21
22 Drawing Lewis Structures 1. ount up the total number of valence electrons available (symbolized by A) by first adding the group numbers of all the atoms present. If the species is a negative ion, add the absolute value of the total charge; if it is a positive ion, subtract it. 8/26/2004 OFP hapter 3 22
23 Drawing Lewis Structures 2. alculate the total number of electrons needed (N) for each atom to have its own noble-gas set of electrons around it (two for hydrogen, eight for the elements from carbon on in the periodic table). 8/26/2004 OFP hapter 3 23
24 Drawing Lewis Structures 3. Subtract the number in step 1 from the number in step 2. This is the number of shared (or bonding) electrons present (S). 8/26/2004 OFP hapter 3 24
25 Drawing Lewis Structures 4. Assign two bonding electrons (as one shared pair) to each connection between two atoms in the molecule or ion. 8/26/2004 OFP hapter 3 25
26 Drawing Lewis Structures 1. ount up the total number of valence electrons available (symbolized by A) by first adding the group numbers of all the atoms present. If the species is a negative ion, add the absolute value of the total charge; if it is a positive ion, subtract it. 8/26/2004 OFP hapter 3 26
27 Drawing Lewis Structures 2. alculate the total number of electrons needed (N) for each atom to have its own noble-gas set of electrons around it (two for hydrogen, eight for the elements from carbon on in the periodic table). 8/26/2004 OFP hapter 3 27
28 Drawing Lewis Structures 3. Subtract the number in step 1 from the number in step 2. This is the number of shared (or bonding) electrons present (S). 8/26/2004 OFP hapter 3 28
29 Drawing Lewis Structures 4. Assign two bonding electrons (as one shared pair) to each connection between two atoms in the molecule or ion. 8/26/2004 OFP hapter 3 29
30 Drawing Lewis Structures 5. If any of the electrons earmarked for sharing remain, assign them in pairs by making some of the bonds double or triple bonds. In some cases, there may be more than one way to do this. In general, double bonds form only between atoms of carbon, nitrogen, oxygen, and sulfur. 8/26/2004 OFP hapter 3 30
31 Drawing Lewis Structures 1. ount up the total number of valence electrons available (symbolized by A) by first adding the group numbers of all the atoms present. If the species is a negative ion, add the absolute value of the total charge; if it is a positive ion, subtract it. O 8/26/2004 OFP hapter 3 31
32 Drawing Lewis Structures 2. alculate the total number of electrons needed (N) for each atom to have its own noble-gas set of electrons around it (two for hydrogen, eight for the elements from carbon on in the periodic table). O 8/26/2004 OFP hapter 3 32
33 Drawing Lewis Structures 3. Subtract the number in step 1 from the number in step 2. This is the number of shared (or bonding) electrons present (S). O 8/26/2004 OFP hapter 3 33
34 Drawing Lewis Structures 4. Assign two bonding electrons (as one shared pair) to each connection between two atoms in the molecule or ion. O 8/26/2004 OFP hapter 3 34
35 Drawing Lewis Structures 5. If any of the electrons earmarked for sharing remain, assign them in pairs by making some of the bonds double or triple bonds. In some cases, there may be more than one way to do this. In general, double bonds form only between atoms of carbon, nitrogen, oxygen, and sulfur. O 8/26/2004 OFP hapter 3 35
36 Drawing Lewis Structures 6. Assign the remaining electrons as lone pairs to the atoms, giving octets to all atoms except hydrogen. O 8/26/2004 OFP hapter 3 36
37 Drawing Lewis Structures Steps Determine the formal charge on each atom, and write it next to that atom. heck that the formal charges add to give a correct total charge on the molecule or molecular ion. Methane 4 Formal charge = group number - lone-pair electrons - ½ (number of electrons in bonding pairs) 8/26/2004 OFP hapter 3 37
38 Drawing Lewis Structures 7. Determine the formal charge on each atom, and write it next to that atom. heck that the formal charges add to give a correct total charge on the molecule or molecular ion. 8/26/2004 OFP hapter 3 38
39 Drawing Lewis Structures 7. Determine the formal charge on each atom, and write it next to that atom. heck that the formal charges add to give a correct total charge on the molecule or molecular ion. Ethylene 2 4 Formal charge = group number - lone-pair electrons - ½ (number of electrons in bonding pairs) 8/26/2004 OFP hapter 3 39
40 Drawing Lewis Structures 7. Determine the formal charge on each atom, and write it next to that atom. heck that the formal charges add to give a correct total charge on the molecule or molecular ion. 8/26/2004 OFP hapter 3 40
41 Drawing Lewis Structures 7. Determine the formal charge on each atom, and write it next to that atom. heck that the formal charges add to give a correct total charge on the molecule or molecular ion. arbon monoxide Formal charge = group number - lone-pair electrons - ½ (number of electrons in bonding pairs) O 8/26/2004 OFP hapter 3 41
42 3-7 the Shapes of Molecules The VESPR theory The Valence Shell Electron-Pair Repulsion Theory Steric Number SN = (number of atoms bonded to a central atom) + ( number of lone pairs on central atom) 8/26/2004 OFP hapter 3 42
43 3-7 The Shapes of Molecules The VESPR theory Text Error OFB 4 th Edition Page 123 Exercise 3-12 SeOF 4 The steric number for the Se atom is 5, not 4 See website for other corrections in the text and solutions manual. 8/26/2004 OFP hapter 3 43
44 The VSEPR Theory The Valence Shell Electron-Pair Repulsion Theory Electron pairs in the valence shell of an atom repel each other on a spherical surface formed by the underlying core of the atom. The geometry which applies to a particular arrangement is determined by the steric number (SN) of the central atom. Steric means having to do with space. The steric number of an atom in a molecule can be determined by drawing the Lewis structure of the molecule and adding the number of atoms that are bonded to it and the number of lone pairs that it has. 8/26/2004 OFP hapter 3 44
45 Geometry and Steric Number SN = 2 Linear 180 SN = 3 Trigonal planar 120 SN = 4 Tetrahedral SN = 5 Trigonal bipyramidal 90 (equatorial - axial or 120 (equatorial equatorial) SN = 6 Octahedral 90 SN for Double and triple bonds count the same as single bonded atoms SN = 5 Lone pairs occupy equatorial positions in preference to axial positions. When lone pairs are present, the situation is more complicated due to repulsive forces Lone pr. vs lone pair > Lone pr vs. bonding pair > Bonding pr. Vs. bonding pair 8/26/2004 OFP hapter 3 45
46 Examples with no Lone Pairs on the central Atom 8/26/2004 OFP hapter 3 46
47 The VSEPR Theory 8/26/2004 OFP hapter 3 47
48 The VSEPR Theory 8/26/2004 OFP hapter 3 48
49 The VSEPR Theory 8/26/2004 OFP hapter 3 49
50 The VSEPR Theory 8/26/2004 OFP hapter 3 50
51 The VSEPR Theory 8/26/2004 OFP hapter 3 51
52 The VSEPR Theory 8/26/2004 OFP hapter 3 52
53 8/26/2004 OFP hapter 3 53
54 8/26/2004 OFP hapter 3 54
55 8/26/2004 OFP hapter 3 55
56 8/26/2004 OFP hapter 3 56
57 8/26/2004 OFP hapter 3 57
58 8/26/2004 OFP hapter 3 58
59 Dipole Moments Bonded atoms share electrons unequally, whenever they differ in Electronegativity E.g., l. The l atom carries a slightly negative electric charge and the atom a slightly positive charge of equal magnitude. Aligns itself in an electric field Dipolar or polar molecules posses a dipole moment, µ To find µ, first draw the VESPR molecular geometry. Next assign a dipole moment to each bond, then vectorially add the dipole moments for each bond 8/26/2004 OFP hapter 3 59
60 8/26/2004 OFP hapter 3 60
61 3-8 Elements Forming more than One Ion Oxidation State (Oxidation Number) Ionic vs ovalent bonding Not formal electric charges, rather what the charge would be if the compound were ionic Range from -3 to +7 Examples 1. ro 3 2. Tll 3 3. Mn 3 N 2 4. Vl 4 5. Mn 2 O 7 8/26/2004 OFP hapter 3 61
62 hapter 3 hemical Periodicity and the Formation of Simple ompounds Examples / exercises All (3-1 to 3-16) W Problems 4, 8, 16, 24, 30, 62 (on WebT) Be familiar with Lewis structures and shapes (e.g. 33, 34, 39, 57) 8/26/2004 OFP hapter 3 62
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