We study bonding since it plays a central role in the understanding of chemical reactions and understanding the chemical & physical properties.
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1 AP Chapter 8 Notes Bonding We study bonding since it plays a central role in the understanding of chemical reactions and understanding the chemical & physical properties. Chemical Bond: holding atoms together forcing them to act as a. Bond Energy: the required to a bond Why do bonds occur? To achieve the. Ionic bonding: attractions of. charged ions. Bond Length: the distance between atoms where energy is. Coulomb s Law calculates the energy of the attraction between a pair of ions: E = where Q 1 & Q 2 are relative ion charges r is the distance between ion centers a negative result indicates an attractive force total energy of the system is: net of potential energy (due to and the kinetic energy due to the Covalent bonding: occurs when electrons are the nuclei of two atoms simultaneously of electrons) of the electrons between Polar Covalent Bonding: occurs when electrons are not completely but an unequal exists this creates partial charges or. Electronegativity: is the tendency of an atom to. to itself in a compound. The greater the differences in electronegativity, the more in nature the bond is. EX 8.1 (pg355) Order the following bonds according to polarity: H H, O H, Cl H, S H, and F H
2 Dipole: another name for a Dipole moment: when a molecule has a center of and another center of Explain how a molecule can have polar bonds with no dipole moment. O C O EX 8.2 (pg 357) For each of the following molecules, show the direction of the bond polarities and indicate which ones have a dipole moment: HCl, Cl 2, SO 3 (a planar molecule with the oxygen atoms spaced evenly around the central sulfur atom), CH 4 (tetrahedral with the carbon atom at the center, and H 2 S (V-shaped with the sulfur atom at the point) Electron configurations & sizes of atoms atoms in stable compounds have configurations electron We can predict whether a compound will be more ionic or covalent in nature. Large differences in indicate the compound will be more ionic. Predict: CaO Al 2 O 3 Ion size plays important role in: determining structure & the properties of ions in their the biologic effects of the ions of ionic solids state what influences the size of ions? 1. cations are than their parent atom 2. anions are than their parent atom 3. ion size increases going on the periodic table 2
3 Compare these isoelectric ions: Mg 2+ Na + Al 3+ O 2- F -...as the positive charge increases, the ions become smaller. List in order of smallest to largest. < < < < EX 8.3 (pg 362) Arrange the ions Se 2-, Br -, Rb +, and Sr 2+ in order of decreasing size. EX 8.4 (pg 362) Choose the largest ion in each of the following groups. a. Li +, Na +, K +, Rb +, Cs + b. Ba 2+, Cs +, I -, Te 2- Binary Ionic Compounds are mutually attractive ions which form a energy than the individual elements Lattice Energy: indicates the strength of M + (g) + X - (g) MX (s) The reaction is usually together to form an ionic solid. with lower between ions. as gaseous ions pack Li (s) + ½ F 2 (g) LiF (s) 1. Sublimation of the solid ΔH=161kJ/mol 2. Ionization of gas I.E.=520kJ/mol 3. Dissociation energy B.E.=1/2(154)kJ/mol 4. Electron affinity E.A.=-320kJ/mol 5. Lattice energy L.E.=-1040kJ/mol total overall energy for the reaction -617 kj/mol Lattice energy calculations are similar to those using Coulomb s Law: Lattice energy =. 3
4 Partial Ionic Character of Covalent Bonds Molecules with the same element like O 2...same electronegativity...covalent Molecules with different elements of different electronegativities... have a polar covalent bond Ionic bonds form when electronegativities are very different % ionic character= measured dipole moment between X-Y Calculated dipole moment between X-Y In general, we use the difference of point between ionic & covalent bond characteristics. for the turning Model for Covalent Bonding Since the molecule, CH 4, takes 1652 kj to break into it s substituents, we assume it will release 1652 kj in forming the C-H bonds. So 1 C-H bond would have an energy of:. For CH 3 Cl, calculate the C-Cl energy if it requires 1578 kj/mole to break all bonds. Bonding is just a we use to explain molecular stability. It provides a way for us to systematize chemical behavior. Covalent Bond Energies and Chemical Reactions The bond strength we use is actually an average of the bond strength in different molecules. But we find that as bonding pairs of electrons increases the bond length. Bond Energy & Enthalpy Bond energy can be used to calculate approximate energy for reactions. (See page 373) H 2 (s) + F 2 (g) 2HF (g) we must break: 1 H-H bond = 1 F-F bond = we must form: 2 H-F bonds= ΔH = ΣBE bonds broken Σ bonds formed 4
5 EX 8.5 (pg 375) Using the bond energies in Table 8.4, calculate ΔH for the reaction of methane with chlorine and fluorine to give freon-12 (CF 2 Cl 2 ). CH 4(g) + 2Cl 2(g) + 2F 2(g) CF 2 Cl 2(g) + 2HF (g) + 2HCl (g) Localized Electron Bonding Model...is one model describing energy and location of electrons (those bonding as well as those which are not involved). We will cover other models in future chapters! Average bond energies (kj/mol) H-H 432 N-H 391 S-H 347 C=C 614 H-F 565 N-N 160 S-F 327 C C 839 H-Cl 427 N-F 272 S-Cl 253 O=O 495 H-Br 363 N-Cl 200 S-Br 218 C=O* 745 H-I 295 N-Br 243 S-S 266 C O N-O 201 N=O 607 C-H 413 O-H 467 Si-Si 340 N=N 418 C-C 347 O-O 146 Si-H 393 N N 941 C-N 305 O-F 190 Si-C 360 C N 891 C-O 358 O-Cl 203 Si-O 452 C=N 516 C-F 485 O-I 234 C-Cl 339 F-F 154 C-Br 276 I-I 149 F-Cl 253 C-I 240 I-Cl 208 F-Br 237 C-S 259 I-Br 175 Cl-Cl 239 Cl-Br 218 Br-Br 193 C=O (CO 2) = 799 This model assumes: assumes a molecule is composed of bound together by of electrons this bond uses the of the atoms pairs of electrons are assumed to be on an atom (we call these ) or they are in the spaced in between 2 atoms (we call these ) Localized Electron model uses to show the arrangement of electrons to predict the geometry to hold shared or lone e- pairs Lewis Structure: sum the valence electrons use a pair to form bond between atoms arrange other e- to satisfy octet rule PF 3 EX 8.6 (pg 379) Give the Lewis structure for each of the following. a. HF b. N 2 c. NH 3 d. CH 4 e. CF 4 f. NO + some exceptions to the octet rule: 5
6 Be & B & Al can be what we call. 3 rd period elements such as obey and can sometimes the octet rule...they are called electron. 2 nd period elements never exceed the octet rule EX 8.7 (pg 382) Write the Lewis structure for PCl 5. EX 8.8 (pg 383) Write the Lewis structure for each molecule or ion. a. ClF 3 b. XeO 3 c. RnCl 2 d. BeCl 2 e. ICl 4 - Resonance Structures occur when a double or triple bond could occur on any of several bond in a compound...experimentation shows that instead of a single and a double bond, for example, the bond strength appears to be an of the bonds. EX 8.9 (pg 385) Describe the electron arrangement in the nitrite anion (NO 2 - ) using the localized electron model. Formal Charge 6
7 Because electrons are really delocalized or move around the entire molecule, we have to have a different method for assigning charges especially when normal oxidation states do not apply....it is the difference between the number of valence electrons on a free atom and the number of valence electrons assigned to the atom in the molecule. Valence electrons assigned: sum of lone pairs and one from each bond Or 2- SO 4 S = S = O = 2O = 2O = Assumptions about formal charges: atoms in molecules try to achieve formal charge as close to as possible formal charges should be on the more electronegative atom O O S O O EX 8.10 (pg 389) Give possible Lewis structures for XeO 3, an explosive compound of xenon. Which Lewis structure or structures are most appropriate according to the formal charges? VSEPR is a model which helps us predict molecular shape & structure V. S. E. P. R. EX 8.11 (pg 394) 7
8 Describe the molecular structure of the water molecule. EX 8.12 (pg 396) When phosphorus reacts with excess chlorine gas, the compound phosphorous pentachloride (PCl 5 ) is formed. In the gaseous and liquid states, this substance consists of PCl 5 molecules, but in the solid state it consists of a 1:1 mixture of PCl 4 + and PCl 6 - ions. Predict the geometric structures of PCl 5, PCl 4 +, and PCl 6 -. EX 8.13 (pg 397) Because the noble gases have filled s and p valence orbitals, they were not expected to be chemically reactive. In fact, for many years these elements were called inert gases because of this supposed inability to form any compounds. However, in the early 1960's several compounds of krypton, xenon, and radon were synthesized. For example, a team at the Argonne National Laboratory produced the stable colorless compound xenon tetrafluoride (XeF 2 ). Predict its structure and whether it has a dipole moment. EX 8.14 (pg 400) Predict the molecular structure of the sulfur dioxide molecule. Is this molecule expected to have a dipole moment? 8
9 Assignment Chapter 8: # 13, 16, 17, 20, 22, 26, 28, 32, 34, 36, 40, 42, 43, 46, 48, 50, 56, 58, 60, 64a, 65, 72, 74, 77a-e, 86, 90, 92, 94, 96 9
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