Attention BMC Students,
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1 Attention BMC Students, There will be no chemistry seminars on October 23 rd (Thursday) and October 24 th (Friday). For those who miss the seminar, an optional make-up seminar will be given on Oct. 27, Monday, (Dept. Obstetrics and Gynecology, Lecture Hall))
2 Chemical bonds
3 Which of the following drawings is more likely to represent an ionic compound, and which a covalent compound? ionic covalent
4 Each of the pictures (a) (d) represents one of the following substances at 25 C: sodium, chlorine, iodine, sodium chloride. Which picture corresponds to which substance? iodine sodium NaCl chlorine
5 Which of the following alkaline earth oxides has the larger lattice energy? Explain. A B The magnitude of the lattice energy depends directly on the charge on the ions and inversely on the distance between ions (that is, on the radii of the ions). In this instance, all the ions in both drowings are doubly charged, either M 2+ or O 2-, so only the size of the ions is important. Q Q k 1 d E 2 B has the larger lattice energy as the ions in B are smaller.
6 . Blue: Green: Red: AB 2 (SrF 2 ) AB 4 (CBr 4 ) AB or AB 2 (PbS or PbS 2 )
7 VALENCE ELECTRONS Electrons in the outermost shell of the atom BONDING ELECTRONS Number of valence electrons shared with other atoms NON-BONDING ELECTRONS Valence electrons, not shared with other atoms
8 Drawing Lewis Structures Sum the valence electrons from all atoms. Add one for each negative charge and subtract one for each positive charge. Draw a skeleton structure with atoms attached by single bonds. The central atom is the least electronegative one (except H). Complete the octets of atoms bound to the central atom. Place extra electrons on the central atom. If the central atom doesn t have an octet, try forming multiple bonds.
9 Give the electron-dot structures (Lewis structures) for the following species: (a) Ammonium ion (b) HCN (c) IF 3 : (d) Phosphorus pentachloride (e) Sulfur tetrafluoride
10 Resonance Structures Resonance structures are attempts to represent a real structure that is a mix between several extreme possibilities. Some molecules are not well described by Lewis Structures. Typically, structures with multiple bonds can have similar structures with the multiple bonds between different pairs of atoms
11 Draw as many electron-dot resonance structures as possible for (a) O 3, (b) sulfur dioxide, and (c) the nitrite ion giving the octet of all atoms.
12 What if different sets of atomic linkages can be used to construct Lewis Dot Structures? Cl O Cl Cl Cl O Cl O Cl Cl Cl O Which is correct?
13 Formal charge (FC) Formal charge is the difference between the number of valence electrons in the free atom and the number assigned to that atom in the Lewis structure. Mathematically: FC = X (Y + Z/2) where X = the number of valence electrons in the free atom (Group Number) Y = the number of unshared electrons Z = the number of shared electrons The most stable structure has: the lowest formal charge on each atom, the most negative formal charge on the most electronegative atoms.
14 Formal Charge Cl O Cl Cl Cl O #of e - (Y + Z/2) #of e - in free atom (X) F. C The most stable structure has: the lowest formal charge on each atom, the most negative formal charge on the most electronegative atoms.
15 Formal charge O: 6-4 ½ - 4 = 0 N: 5-6 ½ -2 = 0 O: 6 2 ½ - 6 = -1 N: 5 8 ½ - 0 = + 1 More favorable
16 VALENCE SHELL ELECTRON PAIR REPULSION: VSEPR Pairs of electrons repel each other Shape of molecule is governed by pairs of valence electrons being as far apart as possible.
17 The VSEPR Model To apply VSEPR theory: 1. Draw the Lewis structure. 2. Determine the electron domain geometry. 3. Determine the molecular geometry. Electron domain geometry: arrangement of electron pairs around the central atom. Molecular geometry: arrangement of atoms around the central atom. This does not include lone electron pairs. The molecular shape differs from the electron shape if lone pairs are present
18
19 Five basic shapes Two charge clouds, no lone pair Three charge clouds, no lone pair
20 Four charge clouds, no lone pair Five charge clouds, no lone pair
21 Six charge clouds, no lone pair
22 Number of Bonds Number of Lone Pairs Number of Charge Clouds Geometry Example
23 Number of Bonds Number of Lone Pairs Number of Charge Clouds Geometry Example
24 Number of Bonds Number of Lone Pairs Number of Charge Clouds Geometry Example
25 Number of Bonds Number of Lone Pairs Number of Charge Clouds Geometry Example
26 Number of Bonds Number of Lone Pairs Number of Charge Clouds Geometry Example
27 (a) Trigonal planar (b) Trigonal bypiramidal (d) Octahedral (c) Linear
28 Draw the Lewis structure and predict the shape of the following molecules: (a) CO 2 linear (b) H 2 CO trigonal planar (c) CBr 4 (d) H 2 S : : H-S-H tetrahedral bent (e) PCl 3 (f) PCl 5 trigonal pyramidal trigonal bypyramidal
29 What shape and bond angle do you expect for each of the following molecules? (a) H 2 O (b) BF 3 (c) CO 2 (d) SF 6 (e) CCl 4 (a) O: 4 Charge Clouds, bent, o (b) B: 3 CC, trigonal planar, 120 o (c) C: 2 Charge Clouds,linear, 180 o (d) S: 6 CC, octahedral, 90 o (e) C: 4 CC, tetrahedral, 109 o
30 Molecular Structure and Covalent Bonding Theories
31
32
33 bonds bond
34 Hybridization The valence shell orbitals (atomic orbitals) commonly combine to change their character in order to obtain a lower energy mixed orbital set for bonding in a particular geometry Hybridization process by which atomic orbitals combine to form a set of mixed orbitals of lower energy when bonding covalently The mixed orbitals are called hybrid orbitals
35 Valence Bond(VB) Theory
36 sp 3 Hybridization
37
38
39 sp 2 Hybridization
40 sp Hybridization
41
42
43 Identify each of the following sets of hybrid orbitals:
44 What is the hybridization of the central atom in: (a) AlCl 3 sp 2 (d) [Cr(H 2 O) 6 ] 3+ (b) SiH 4 sp 3 (e) H 2 Be (c) PCl 5 sp 3 d (f) ClO 4 sp sp 3 sp 3 d 2
45
46 Molecular Geometry and Polarity The polarity can be determine once the geometry is known A polar bond is created if the atoms sharing the electron pair have different electronegativities HCl and the associated dipole moment. This molecule is polar. For diatomics, determination of polarity is easy. What if the molecule has two or more atoms? All the dipole have to be summed. If the sum equals zero, the molecule has no dipole.
47 Molecular Geometry and Polarity
48 Which of the following molecules are polar? (a) H 2 O (b) SO 2 (c) CO 2 (d) CH 4
49 Intermolecular Forces
50
51
52
53 Which substance in each of the following pairs would you expect to have the lower boiling point. Explain. a) C 6 H 6 or C 6 Cl 6 b) H 2 C=O or CH 3 OH c) He or Kr d) H 2 Se or H 2 O a) C 6 H 6 smaller mass weaker London forces c) He smaller mass b) H 2 C=O no H-bonding d) H 2 Se no H-bonding
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