1 Chemistry: An Introduction 2 Measurements And Calculations 3 Matter 4 Chemical Foundations: Elements, Atoms, And Ions 5 Nomenclature 6 Chemical Reactions: An Introduction 7 Reactions In Aqueous Solutions 8 Chemical Composition 9 Chemical Quantities 10 Energy 11 Modern Atomic Theory 12 Chemical Bonding 13 Gases 14 Liquids And Solids 15 Solutions 16 Acids And Bases 17 Equilibrium 18 Oxidation–reduction Reactions And Electrochemistry 19 Radioactivity And Nuclear Energy 20 Organic Chemistry 21 Biochemistry Chapter12: Chemical Bonding
12.1 Types Of Chemical Bonds 12.2 Electronegativitly 12.3 Bond Polarity And Dipole Moments 12.4 Stable Electron Configurations And Charges On Ions 12.5 Ionic Bonding And Structures Of Ionic Compounds 12.6 Lewis Structures 12.7 Lewis Structures Of Molecules With Multiple Bonds 12.8 Molecular Structure 12.9 Molecular Structure: The Vsepr Model 12.10 Molecular Structure: Molecules With Double Bonds Chapter Questions Section: Chapter Questions
Problem 1ALQ: sing only the periodic table, predict the most stable ion for Na,Mg,Al,s,Cl,K,Ca,andGa. Arrange... Problem 2ALQ: rite the proper charges so that an alkali metal, a noble gas, and a halogen have the same electron... Problem 3ALQ: hat is meant by a chemical bond? Problem 4ALQ: hy do atoms form bonds with one another? What can make a molecule favored compared with the lone... Problem 5ALQ: ow does a bond between Naand Cldiffer from a bond between Cand O? What about a bond between Nand N? Problem 6ALQ: n your own words, what is meant by the term electronegativity? What are the trends across and down... Problem 7ALQ: xplain the difference between ionic bonding and covalent bonding. How can we use the periodic table... Problem 8ALQ: rue or false? In general, a larger atom has a smaller electronegativity. Explain. Problem 9ALQ: hy is there an octet rule (and what does actet mean) in writing Lewis structures? Problem 10ALQ: Does a Lewis structure tell which electrons came from which atoms? Explain. Problem 11ALQ: If lithium and fluorine react, which has more attraction for an electron? Why? Problem 12ALQ: In a bond between fluorine and iodine, which has more attraction for an electron? Why? Problem 13ALQ: We use differences in electronegative to account for certain properties of bonds. What if all atoms... Problem 14ALQ Problem 15ALQ: Why do we only the consider the valence electrons in drawing Lewis structures? Problem 16ALQ: How do we determine the total number of valence electrons for an ion? Provide an example of an anion... Problem 17ALQ: What is the main idea in the valence shell electron pair repulsion (VSEPR) theory? Problem 18ALQ: The molecules NH3andBF3have the same general formula (AB3)but different shapes. Find the shape of... Problem 19ALQ: How do we deal with multiple bonds in VSEPR theory? Problem 20ALQ: In Section 12.10 of your text, the term “effective pairs" is used. What does this mean? Problem 21ALQ Problem 22ALQ Problem 1QAP Problem 2QAP Problem 3QAP: hat sorts of elements react to form ionic compounds? Problem 4QAP: n general terms, what is a covalent bond? Problem 5QAP: escribe the type of bonding that exists in the Cl2(g)molecule. How does this type of bonding differ... Problem 6QAP Problem 7QAP: he relative ability of an atom in a molecule to attract electrons to itself is called the atom’s . Problem 8QAP: hat does it mean to say that a bond is polar? Give two examples of molecules with polar bonds.... Problem 9QAP Problem 10QAP: What factor determines the relative level of polarity of a polar covalent bond? Problem 11QAP: In each of the following groups, which element is the most electronegative? Which is the least... Problem 12QAP: In each of the following groups. which element is the most electronegative? Which is the least... Problem 13QAP: On the basis. of the electronegativity values given in Fig. 12.3, indicate whether each of the... Problem 14QAP: On the basis of the electronegativity values given in Fig. 12.3, indicate whether each of the... Problem 15QAP: Which of the following molecules contain polar covalent hands?... Problem 16QAP: Which of the following molecules contain polar covalent bonds?... Problem 17QAP: On the basis of the electronegativity values given in Fig. 12.3, indicate which is the more polar... Problem 18QAP: On the basis of the electronegativity values given in Fig. 12.3. indicate which is the more polar... Problem 19QAP: Which brand in each of the following pairs has the greater ionic character?... Problem 20QAP: Which hand in each of the following pairs has less ionic character?... Problem 21QAP: What is a dipole moment? Give four examples of molecules that possess dipole moments, and draw the... Problem 22QAP: Why is the presence of a dipole moment in the water molecule so important? What are some properties... Problem 23QAP: In each of the following diatomic molecules, which end of the molecule is negative relative to the... Problem 24QAP: In each of the following diatomic molecules. which end of the molecule is positive relative to the... Problem 25QAP: For each of the following bonds, draw a figure indicating the direction of the bond dipole,... Problem 26QAP: For each of the following bonds, draw a figure indicating the direction of the bond dipole,... Problem 27QAP: For each of the following bonds, draw a figure indicating the direction of the bond dipole,... Problem 28QAP: For each of the following bonds, draw a figure indicating the direction of the bond dipole.... Problem 29QAP: What does it mean when we say that in forming bonds, atoms try to achieve an electron configuration... Problem 30QAP Problem 31QAP: Nonmetals form negative ions by (losing/gaining) enough electrons to achieve the electron... Problem 32QAP: Explain how the atoms in covalent molecules achieve electron configurations similar to those of the... Problem 33QAP: Which simple ion would each of the following elements he expected to form? What noble gas has an... Problem 34QAP: Which simple ion would each of the following elements be expected to form? Which noble gas has an... Problem 35QAP: For each of the following numbers of electrons, give the formula of a positive ion that would have... Problem 36QAP: What is the expected ground—state electron configuration for Te2-? Problem 37QAP: On the basis of their electron configurations, predict the formula of the simple binary ionic... Problem 38QAP: On the basis of their electron configurations, predict the formula of the simple binary ionic... Problem 39QAP: Name the noble gas atom that has the same electron configuration as each of the ions in the... Problem 40QAP: Atoms form ions so as to achieve electron configurations similar to those of the noble gases. For... Problem 41QAP Problem 42QAP: Describe in general terms the structure of ionic solids such as NaCl. How are the ions packed in the... Problem 43QAP: Why are cations always smaller than the atoms from which they are formed? Problem 44QAP: Why are anions always larger than the atoms from which they are formed? Problem 45QAP: For each of the following pairs, indicate which species is smaller. Explain your reasoning in terms... Problem 46QAP Problem 47QAP Problem 48QAP: For each of the following pairs, indicate which is larger. msp;a.IorFb.ForFc.Na+orF Problem 49QAP: Why are the valence electrons of an atom the only electrons likely to be involved in bonding to... Problem 50QAP: Explain what the “duet" and “octet” rules are and how they are used to describe the arrangement of... Problem 51QAP: What type of structure must each atom in a compound usually exhibit for the compound to be stable? Problem 52QAP: When elements in the second and third periods occur in compounds, what number of electrons in the... Problem 53QAP: How many electrons are involved when two atoms in a molecule are connected by a “double bond”? Write... Problem 54QAP Problem 55QAP: Write the simple Lewis structure for each of the following atoms.... Problem 56QAP: Write the simple Lewis structure for each of the following atoms.... Problem 57QAP: Give the total number of valence electrons in each of the following molecules.... Problem 58QAP: Give the total number of valence electrons in each of the following molecules.... Problem 59QAP: Write a Lewis structure for each of the following simple molecules. Show all bonding valence... Problem 60QAP: Write a Lewis structure for each of the following simple molecules. Show all bonding valence... Problem 61QAP: Write a Lewis structure for each of the following simple molecules. Show all bonding valence... Problem 62QAP: Which of the following species exhibits resonance? msp;CH4,OCl2,NO2,HCN(C is the central atom) Problem 63QAP: The “Chemistry in Focus“ segment Broccoli—Miracle Food? discusses the health benefits of eating... Problem 64QAP: The “Chemistry in Focus" segment Hiding Carbon Dioxide- discusses attempts at sequestering (storing)... Problem 65QAP: Write a Lewis structure for each of the following polyatomic ions. Show all bonding valence electron... Problem 66QAP: Write a Lewis structure for each of the following polyatomic ions. Show all bonding valence electron... Problem 67QAP: Write a Lewis structure for each of the following polyatomic ions. Show all bonding valence electron... Problem 68QAP: Write a Lewis structure for each of the following polyatomic ions. Show all bonding valence electron... Problem 69QAP: What is the geometric structure of the water molecule? How many pairs of valence electrons are there... Problem 70QAP: What is the geometric sanctum of the ammonia molecule? How many pairs of electrons surround the... Problem 71QAP: What is the geometric structure of the boron trifluoride moleCule, BF3? How many pairs of valence... Problem 72QAP: What is the geometric structure of the SiF4molecule? How many pairs of valence electrons are present... Problem 73QAP: Why is the geometric structure of a molecule important, especially for biological molecules? Problem 74QAP Problem 75QAP: How is the structure around a given atom related to repulsion between valence electron pairs on the... Problem 76QAP: Why are all diatomic molecules linear, regardless of the number of valence electron pairs on the... Problem 77QAP: Although the valence electron pairs in ammonia have a tetrahedral arrangement me overall geometric... Problem 78QAP: Although both the BF3and NF3molecules contain the same number of atoms, the BF3molecule is flat,... Problem 79QAP: For the indicated atom in each of the following molecules or ions. give the number and arrangement... Problem 80QAP Problem 81QAP: Using the VSEPR theory, predict the molecular structure of each of the following molecules.... Problem 82QAP Problem 83QAP: Using the VSEPR theory, predict the molecular structure of each of the following polyatomic ions.... Problem 84QAP: Using the VSEPR theory, predict the molecular structure of each of the following polyatomic ions.... Problem 85QAP: For each of the following molecules or ions, indicate the bond angle expected between the central... Problem 86QAP: For each of the following molecules or ion. indicate the bond angle expected between the central... Problem 87QAP: The “Chemistry in Focus" segment Taste—It's the Structure That Counts discusses artificial... Problem 88QAP Problem 89AP Problem 90AP: In ionic bonding, the electrons are shared between the atoms. the process of fanning an ionic bond... Problem 91AP: The geometric arrangement of electron pairs around a given atom is determined principal by the... Problem 92AP Problem 93AP Problem 94AP: Which of the following statements is false concerning bonding? Elements with extremely different... Problem 95AP Problem 96AP: For each of the following pairs of elements, identify which element would be expected to be more... Problem 97AP: On the basis of the electronegativity values given in Fig. 12.3, indicate whether each of the... Problem 98AP: Which of the following molecules contain polar covalent hands? carbon monoxide, CO chlorine, Cl2... Problem 99AP Problem 100AP Problem 101AP: or each of the following bonds, draw a figure indicating the direction of the bond dipole, including... Problem 102AP Problem 103AP Problem 104AP Problem 105AP: hich noble gas has the same electron configuration as each of the ions in the following compounds?... Problem 106AP Problem 107AP: rite the Lewis structure for each of the following atoms.... Problem 108AP Problem 109AP: rite a Lewis structure for each of the following simple molecules. Show all bonding valence electron... Problem 110AP Problem 111AP: rite a Lewis structure for each of the following simple molecules. Show all bonding valence electron... Problem 112AP Problem 113AP: hy is the molecular structure of H2Ononlinear, whereas that of BeF2is linear, even though both... Problem 114AP Problem 115AP: sing the VSEPR theory, predict the molecular structure of each of the following molecules.... Problem 116AP Problem 117AP: or each of the following molecules, indicate the bond angle expected between the central atom and... Problem 118AP Problem 119AP Problem 120AP Problem 121AP Problem 122AP: Classify the bonding in each of the following molecules as ionic, polar covalent, or nonpolar... Problem 123CP: ompare the electronegativities of each pair of atoms. State the element of each pair that has the... Problem 124CP Problem 125CP: rrange the atoms and/or ions in the following groups in order of decreasing size.... Problem 126CP Problem 127CP Problem 128CP: he formulas of several chemical substances are given in the table below. For each substance in the... Problem 1CR Problem 2CR: hat does temperature measure? Are the molecules in a beaker of warm water moving at the same speed... Problem 3CR Problem 4CR Problem 5CR Problem 6CR: hat is the enthalpy change for a process? Is enthalpy a state function? In what experimental... Problem 7CR Problem 8CR Problem 9CR Problem 10CR: What is a driving force? Name two common and important driving forces, and give an example of each.... Problem 11CR Problem 12CR: Methane, CH4, is the major component of natural gas. Methane burns in air, releasing approximately... Problem 13CR: What is electronegative radiation? Give some examples of such radiation. Explain what the wavelength... Problem 14CR Problem 15CR: Do atoms in excited states emit radiation randomly, at any wavelength? Why? What does it mean to say... Problem 16CR Problem 17CR: Schrodinger and de Broglie suggested a ‘Wave—particle duality" for small particles—that is, if... Problem 18CR: Describe the general characteristics of the first (lowest-energy) hydrogen atomic orbital. How is... Problem 19CR Problem 20CR: Describe the sublevels and orbitals that constitute the third and fourth principal energy levels of... Problem 21CR: Describe electron spin. How does electron spin affect the total number of electrons that can be... Problem 22CR Problem 23CR: List the order in which the orbitals are filled as the atoms beyond hydrogen are built up. How many... Problem 24CR Problem 25CR Problem 26CR Problem 27CR: What are the representative elements? In what region(s) of the periodic table are these elements... Problem 28CR Problem 29CR Problem 30CR Problem 31CR Problem 32CR Problem 33CR Problem 34CR Problem 35CR: Give evidence that ionic bonds are very strong. Does an ionic substance contain discrete molecules?... Problem 36CR Problem 37CR Problem 38CR: For three simple molecules of your own choice, apply the rules for writing Lewis structures. Write... Problem 39CR Problem 40CR Problem 41CR Problem 42CR Problem 43CR Problem 44CR Problem 45CR Problem 46CR Problem 47CR: Which of the following statements is correct and provides the best explanation when removing the... Problem 48CR: Hydrogen gas and oxygen gas react violently to form water. When this occurs, a very loud noise is... Problem 18QAP: On the basis of the electronegativity values given in Fig. 12.3. indicate which is the more polar...
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In detail, define the terms endothermic and exothermic in relation to chemical reactions and giving relevant examples. Explain in detail the difference between the two processes in terms of bond making and bond breaking.
Definition Definition Transformation of a chemical species into another chemical species. A chemical reaction consists of breaking existing bonds and forming new ones by changing the position of electrons. These reactions are best explained using a chemical equation.
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