1 100 Practice Questions for hem 1 Midterm 1 - Joseph 1. Which of the following statements is incorrect? A) Ionic bonding results from the transfer of electrons from one atom to another. B) Dipole moments result from the unequal distribution of electrons in a molecule. ) The electrons in a polar bond are found nearer to the more electronegative element. D) A molecule with very polar bonds can be nonpolar. E) Linear molecules cannot have a net dipole moment. 2. Which of the following shows these molecules in order from most polar to least polar? A) 4 > F 2l 2 > F 2 2 > l 4 > l 2 2 B) 4 > F 2 2 > F 2l 2 > l 4 > l 2 2 ) F 2l 2 > F 2 2 > l 2 2 > 4 = l 4 D) F 2 2 > l 2 2 > F 2l 2 > 4 = l 4 E) F 2l 2 > F 2 2 > l 4 > l 2 2 > 4 3. Which of the following is polar? A) SiF 4 B) XeF 2 ) Bl 3 D) NBr 3 E) SBr 6 4. Which statement is correct? A) 2 is linear. B) The molecule l 2 cannot be accurately described by a Lewis structure consistent with the octet rule. ) The diatomic molecule l 2 is an example of a polar molecule. D) The bonds in LiF have a more covalent character than those in F 2. Use the following to answer question 5: onsider the following molecules. I. BF 3 II. Br 3 ( is the central atom.) III. Br 2 IV. Xel 2 V. VI. SF 4 Select the molecule(s) that fit the given statement. 5. These molecules have a zero net dipole moment. A) III, V B) I, III, IV ) III, IV, V D) I, III, IV, VI E) none of them 6. Select the best Lewis structure for acetone, 3 3. A) B)
2 ) D) E) 7. The Lewis structure for 3B 3 is A) B B) B ) B D) B E) B 8. Which of the following is not a valid resonance structure for N 3? A) B) ) N N N - N N N - N N N N N N - D) E) All are valid. -
3 Use the following to answer question 9: Draw the Lewis structures of the molecules below, and use them to answer the following questions. I. B 3 II. N 2 III. SF 6 IV. 3 V. Pl 5 9. Which of these molecules show resonance? A) I, II B) II, IV ) II, V D) III, IV E) III, V 10. Which of the following has an incomplete octet in its Lewis structure? A) S 2 B) Il ) SF 2 D) F 2 E) N 11. The molecule Xl 5 has a square pyramidal shape. Which of the following atoms could be X? A) B) P ) Xe D) S E) At least two of these atoms could be X. 12. The l Kr l bond angle in Krl 4 is closest to A) 90. B) 109. ) 120. D) 150. E) f the following, which molecule has the largest bond angle? A) S 3 B) SF 2 ) N D) 2S E) PF Select the correct molecular structure for SF 4. A) linear B) bent ) pyramidal D) tetrahedral 15. Select the correct molecular structure for I 3. A) linear B) bent ) pyramidal D) tetrahedral
4 16. ow many of the following molecules and ions are linear? Nl 3 N 4 + SN - 2 N 2 - A) 0 B) 1 ) 2 D) 3 E) What type of structure does the XeF 2 molecule have? A) pyramidal B) tetrahedral ) T-shaped D) trigonal planar E) octahedral 18. Which ion is planar? A) + PF 4 B) 2 3 ) 2 S 3 D) l 4 E) - Sl Select the correct molecular structure for P 3 3. A) pyramidal B) tetrahedral ) square planar D) octahedral 20. Which of the following molecules contains a nitrogen atom that is sp 2 hybridized? A) N 3 B) - N 3 ) N 2 D) N E) 2N onsider the structure of glycine, the simplest amino acid: 2 N What is the total number of bonds in the molecule? A) 0 B) 1/2 ) 1 D) 2 E) More information is needed. 22. What is the hybridization of I in the molecule Il 3? A) sp B) sp 2 ) sp 3 D) dsp 3 E) d 2 sp 3
5 23. What is the hybridization of S in the molecule 2S? A) sp B) sp 2 ) sp 3 D) dsp 3 E) d 2 sp What is the hybridization of in the ion N -? A) sp B) sp 2 ) sp 3 D) dsp 3 E) d 2 sp Atoms that are sp 3 hybridized form pi bond(s). A) 0 B) 1 ) 2 D) 3 E) What is the hybridization of the central atom in SF 6? A) sp B) sp 2 ) sp 3 D) dsp 3 E) d 2 sp What is the hybridization of the central atom in IF 5? A) sp B) sp 2 ) sp 3 D) dsp 3 E) d 2 sp What is the hybridization of the central atom in SF 4? A) sp B) sp 2 ) sp 3 D) dsp 3 E) d 2 sp onsider the following molecule. (Lone pairs are not drawn in.) 2 2 N Specify the hybridization of each carbon atom (in numeric order: -1-2 A) sp 2 sp 2 sp 2 sp 3 sp B) sp 2 sp 2 sp 2 sp 3 sp 3 ) sp 2 sp 2 sp 3 sp 3 sp D) sp 2 ssp 2 sp 3 sp 3 sp 3 E) sp sp sp sp 2 sp ).
6 Use the following to answer questions 30-31: onsider the following molecule. (Lone pairs are not drawn in.) l N 30. What is the hybridization of the carbon atom that is double-bonded to oxygen? A) sp B) sp 2 ) sp 3 D) dsp 3 E) d 2 sp What is the hybridization of the carbon atom that is bonded to chlorine? A) sp B) sp 2 ) sp 3 D) dsp 3 E) d 2 sp Which of the following has two bonds? A) 2 6 B) 2 4 ) 2 2 D) at least two of these 33. onsider the following Lewis structure. (Lone pairs are not drawn in.) Which statement about the molecule is false? A) There are 10 sigma and 2 pi bonds. B) -2 is sp 2 hybridized with bond angles of 120. ) xygen is sp 3 hybridized. D) This molecule contains 28 valence electrons. E) There are some bond angles of about 109 in the molecule.
7 Use the following to answer questions 34-36: Tetracyanoethylene has the skeleton shown here: From its Lewis structure, determine the following. 34. ow many sigma bonds and how many pi bonds are in the molecule? A) 5 sigma and 9 pi B) 6 sigma and 8 pi ) 9 sigma and 7 pi D) 9 sigma and 9 pi E) 5 sigma and 8 pi 35. ow many of the atoms are sp 2 hybridized? A) 2 B) 4 ) 6 D) 8 E) ow many of the atoms are sp hybridized? A) 2 B) 4 ) 6 D) 8 E) Which of the following has the shortest N- bond? A) N 3 B) N + ) N 2 D) N omplete the Lewis structure for the following molecule. 3 3 N This molecule has sigma bonds and pi bonds. A) 4, 5 B) 6, 3 ) 11, 5 D) 13, 2 E) 13, 3
8 39. Which of the following statements is correct? A) A triple bond is composed of two bonds and one bond. B) bonds result from the head-to-head overlap of atomic orbitals. ) Free rotation may occur about a double bond. D) bonds have electron density on the internuclear axis. E) More than one of these statements are correct. 40. As the bond order of a bond increases, its bond energy and its bond length. A) increases, increases B) decreases, decreases ) increases, decreases D) decreases, increases 41. If four orbitals on one atom overlap four orbitals on a second atom, how many molecular orbitals will form? A) 1 B) 4 ) 8 D) For which of the following diatomic molecules would the bond order become greater if an electron were removed, that is, if the molecule were converted to the positive ion in its ground state? A) B 2 B) 2 ) P 2 D) F 2 E) Na Which of the following species has the largest dissociation energy? A) 2 B) 2 ) 2 2 D) + 2 E) Which of the following is paramagnetic? A) B 2 B) 2 ) 2 D) N 2 E) F rder the following from shortest to longest bond: 2, B 2, 2, N 2 A) 2, N 2, 2, B 2 B) N 2, 2, B 2, 2 ) 2, N 2, 2, B 2 D) 2, B 2, 2, N Which of the following statements is true? A) Electrons are never found in an antibonding M. B) All antibonding Ms are higher in energy than the atomic orbitals of which they are composed. ) Antibonding Ms have electron density mainly outside the space between the two nuclei. D) None of these statements is true. E) Two of these statements are true.
9 47. Which of the following is paramagnetic? A) 2 B) + 2 ) 2 D) N 2 E) At least two of these are paramagnetic. 48. ow many electrons are involved in pi bonding in benzene, 6 6? A) 12 B) 30 ) 3 D) 6 E) Which of the following statements about the 3 ion is false? A) The orbitals on the carbon atom are sp 2 hybridized. B) The ion is expected to be diamagnetic. ) ne bond is shorter than the others. D) The ion has a total of 24 electrons. E) It has a planar molecular geometry. 50. Which of the following should have the highest boiling point? A) Na 2 B) F ) N 3 D) N 2 E) Identify the major attractive force in F. A) London dispersion forces B) dipole-dipole interactions ) hydrogen bonding D) ionic bonding 52. Identify the major attractive force in 2S. A) London dispersion forces B) dipole-dipole interactions ) hydrogen bonding D) ionic bonding 53. Identify the major attractive force in af 2. A) London dispersion forces B) dipole-dipole interactions ) hydrogen bonding D) ionic bonding 54. Identify the major attractive force in Ne. A) London dispersion forces B) dipole-dipole interactions ) hydrogen bonding D) ionic bonding
10 55. Which of the following compounds has the lowest boiling point? A) 4 B) 2 6 ) 3 8 D) 4 10 E) Which of the following compounds has the highest boiling point? A) 2 6 B) ) 2 D) N 2 E) Ne 57. Which of the following compounds has the highest boiling point? A) 4 B) 2 ) NF 3 D) 2 E) e 58. Which substance involves no intermolecular forces except London dispersion forces? A) K B) 2S ) NaF D) 2 E) l 59. The elements of Group 5A, the nitrogen family, form compounds with hydrogen that have the boiling points listed below. Sb 3 17, As 3 55, P 3 87, N 3 33 The first three elements illustrate a trend where the boiling point decreases as the mass decreases; however, ammonia (N 3) does not follow the trend because of A) dipole-dipole attraction. B) metallic bonding. ) hydrogen bonding. D) London dispersion forces. E) ionic bonding. 60. The resistance of a liquid to an increase in its surface area is called A) capillary action. B) surface tension. ) vapor pressure D) viscosity. 61. n the basis of your knowledge of bonding in liquids and solids, which of the following substances has the highest melting temperature? A) NaBr B) Br 2 ) N 2 D) F 4 E) 2
11 62. Which of the following is the correct order of boiling points for NaN 3, 3, 2 6, and Ne? A) Ne < 3 < 2 6 < NaN 3 B) NaN 3 < 3 < 2 6 < Ne ) Ne < 2 6 < NaN 3 < 3 D) Ne < 2 6 < 3 < NaN 3 E) 2 6 < Ne < 3 < NaN In cubic closest-packed solids, what percentage of space is occupied by the spheres? A) 43.8% B) 52.4% ) 68.0% D) 74.0% 64. Which of the following is the smallest hole in a closest-packed lattice of spheres? A) trigonal B) tetrahedral ) cubic D) octahedral 65. Which substance can be described as cations bonded together by mobile electrons? A) Ag(s) B) S 8(s) ) Kr(l) D) Kl(s) E) l(l) 66. What is the net number of face-centered atoms contained in a face-centered cubic unit cell? A) 1 B) 3 ) 4 D) 6 Use the following to answer questions 67-69: The molar volume of a certain form of solid lead is 18 cm 3 /mol. Assuming cubic closest-packed structure, determine the following. 67. The number of Pb atoms per unit cell A) 3 B) 4 ) 10 D) 12 E) The volume of a single cell A) pm 3 B) pm 3 ) pm 3 D) pm 3
12 69. The radius of a Pb atom A) 1.74 pm B) 17.4 pm ) 174 pm D) 1740 pm 70. Which one of the following statements about solid u (face-centered cubic unit cell) is incorrect? A) It will conduct electricity. B) There are two atoms per unit cell. ) The number of atoms surrounding each u atom is 12. D) The solid has a cubic closest-packed structure. E) The length of a face diagonal is four times the u radius. 71. Which of the following statements is(are) false? I. The hexagonal closest-packed structure is ABAB... II. A body-centered cubic unit cell has four atoms per unit cell. III. For unit cells having the same edge length, a simple cubic structure would have a smaller density than a body-centered cube. IV. Atoms in a solid consisting of only one element would have six nearest neighbors if the crystal structure was a simple cubic array. A) I only B) II only ) II, III only D) I, IV E) II, III, IV 72. Aluminum metal crystallizes in a face-centered cubic structure. What is the relationship between the radius of an Al atom (r) and the length of an edge of the unit cell (E)? A) r = E/2 B) r E/ 8 ) r ( 3 / 4) E D) r = 2E E) r = 4E 73. A metal crystallizes in a body-centered unit cell with an edge length of pm. Assume the atoms in the cell touch along the cube diagonal. What will be the percentage of empty volume in the unit cell? A) 0.00% B) 26.0% ) 32.0% D) 68.0% E) 75.5% 74. A metal crystallizes with a face-centered cubic lattice. The edge of the unit cell is 434 pm. What is the diameter of the metal atom? A) 376 pm B) 217 pm ) 307 pm D) 434 pm E) 614 pm
13 75. hromium metal crystallizes as a body-centered cubic lattice. If the atomic radius of r is 1.25 angstroms, what is the density of r metal in grams per cubic centimeter? A) 5.52 g/cm 3 B) 7.18 g/cm 3 ) 7.81 g/cm 3 D) 2.76 g/cm 3 E) 3.59 g/cm You are given a small bar of an unknown metal, X. You find the density of the metal to be 10.5 g/cm 3. An X- ray diffraction experiment measures the edge of the unit cell as 409 pm. Assuming that the metal crystallizes in a face-centered cubic lattice, what is X most likely to be? A) Ag B) Rh ) Pt D) Pb 77. A certain solid substance that is very hard, has a high melting point, and is nonconducting unless melted is most likely to be A) I 2 B) Kl ) N 2 D) 2 E) r 78. The unit cell in a certain lattice consists of a cube formed by an anion at each corner, an anion in the center, and a cation at the center of each face. The unit cell contains a net A) 5 anions and 6 cations. B) 5 anions and 3 cations. ) 2 anions and 3 cations. D) 3 anions and 4 cations. E) 2 anions and 2 cations. 79. A certain metal fluoride crystallizes in such a way that the fluoride ions occupy simple cubic lattice sites, while the metal atoms occupy the body centers of half the cubes. What is the formula for the metal fluoride? A) MF 2 B) M 2F ) MF D) MF Sodium oxide (Na 2) crystallizes in a structure in which the 2 ions are in a face-centered cubic lattice and the Na + ions are in tetrahedral holes. What is the number of Na + ions in the unit cell? A) 2 B) 4 ) 6 D) In the unit cell of sphalerite, Zn 2+ ions occupy half the tetrahedral holes in a face-centered cubic lattice of S 2 ions. What is the number of formula units of ZnS in the unit cell? A) 5 B) 4 ) 3 D) 2 E) 1
14 82. A p-type semiconductor A) is made by doping host atoms with atoms having more valence electrons than the host. B) is made by doping host atoms with atoms having fewer valence electrons than the host. ) has electrons that lie close in energy to the conduction bands. D) two of these 83. Which of the compounds below is an example of a network solid? A) S 8(s) B) Si 2(s) ) Mg(s) D) Nal(s) E) 25 52(s) 84. Which of the following statements is true about p-type silicon? A) It is produced by doping Si with P or As. B) Electrons are the mobile charge carriers. ) It does not conduct electricity as well as pure Si. D) All are true. E) None is true. 85. Doping Se with As would produce a(n) semiconductor with conductivity compared to pure Se. A) n-type, increased B) n-type, decreased ) p-type, increased D) p-type, decreased E) intrinsic, identical 86. What is the vapor pressure of water at 100.0? A) 85 torr B) 760 torr ) 175 torr D) 1 torr E) More information is needed. 87. Which of the following processes must exist in equilibrium with the condensation process when a measurement of vapor pressure is made? A) fusion B) evaporation ) sublimation D) boiling 88. Given below are the temperatures at which two different liquid compounds with the same empirical formula have a vapor pressure of 400 torr. ompound T ( ) dimethyl ether, ethanol, Which of the following statements is false? A) Increasing the temperature will increase the vapor pressure of both liquids. B) Intermolecular attractive forces are stronger in (liquid) ethanol than in (liquid) dimethyl ether. ) The normal boiling point of dimethyl ether will be higher than the normal boiling point of ethanol. D) The reason why the temperature at which the vapor pressure is 400 torr is higher for ethanol (than for dimethyl ether) is that there is strong hydrogen bonding in ethanol. E) None of these statements is false.
15 89. Knowing that vap for water is 40.7 kj/mol, calculate P vap of water at 37. A) 6.90 torr B) 12.4 torr ) 18.7 torr D) 25.4 torr E) 52.6 torr 90. Which of the following statements is true about the vapor pressures of methane ( 4) and ammonia (N 3)? A) The vapor pressure of ammonia is greater than the vapor pressure of methane because ammonia is polar and methane is nonpolar. B) The vapor pressure of ammonia is less than the vapor pressure of methane because ammonia is nonpolar and methane is polar. ) The vapor pressure of methane is greater than the vapor pressure of methane because methane has more hydrogen bonding than ammonia. D) The vapor pressure of ammonia is equal to the vapor pressure of methane. E) None of these statements is true. 91. You are given the following boiling-point data: water, methanol, ethanol, diethyl ether, ethylene glycol, Which one of these liquids would you expect to have the highest vapor pressure at room temperature? A) water, 2 B) methanol, 3 ) ethanol, 3 2 D) diethyl ether, E) ethylene glycol, Given the graph below, what is the boiling point of carbon tetrachloride at standard pressure? A) 60 B) 34 ) 98 D) 77 E) The graph does not give this information.
16 93. Shown below is a phase diagram for compound X. At 25 and 1 atm, in what state will X exist? A) solid. B) liquid. ) gas. D) gas/liquid at equilibrium. E) gas/solid at equilibrium. 94. A sample consisting of 2(g) and 2(s) at equilibrium at 78 and 1 atm pressure is heated to 30, and the pressure is increased to 8 atm. Based on the phase diagram below, what will happen? A) At equilibrium, only 2(g) will be present. B) All the 2 will be converted to 2(l). ) At equilibrium, 2(g) and 2(l) will be present. D) The melting point of the 2(s) will decrease. 95. Shown below is a phase diagram for compound X. ow will the melting point of X change with increased pressure? A) It will increase. B) It will decrease. ) It will remain the same. D) There is not enough information given. E) It will increase and then decrease.
17 96. Based on the phase diagram shown below, which of the following statements are correct? I. Sublimation occurs at a point in the transformation that falls along a straight line from point A to point F. II. and E represent points where the gas and liquid phases are in equilibrium. III. vap can be measured at point B. IV. Molecules at point D have a greater average kinetic energy than those at point F. V. The temperature at point E is called the critical temperature of the compound. A) II, V B) I, III, IV ) I, II, III D) II, IV, V E) I, II, IV 97. hoose the correct statement about the diagram below. A) The diagram is qualitatively correct for water. B) The diagram shows that the melting point of the solid increases with increasing pressure. ) The diagram shows the triple point above 1 atm pressure. D) The diagram could represent the phase diagram of 2. E) None of these statements is correct. 98. A certain substance, X, has a triple-point temperature of 20 at a pressure of 2.0 atm. Which one of the following statements cannot possibly be true? A) X can exist as a liquid above 20. B) X can exist as a solid above 20. ) Liquid X can exist as a stable phase at 25, 1 atm. D) Both liquid and solid X have the same vapor pressure at 20. E) All of these statements could be true.
18 99. Given the phase diagram shown below, which of the following statements is false? A) The solid has a higher density than the liquid. B) At some (constant) temperature, the gaseous substance can be compressed into a solid and then into a liquid in this order. ) When phase A is compressed at constant temperature at point X, no change is observed. D) When heated at 1 atm, this substance will first melt and then boil. E) None of these statements is false The density of the solid phase of a substance is 0.90 g/cm 3 and the density of the liquid phase is 1.0 g/cm 3. A large increase in pressure will A) lower the freezing point. B) raise the freezing point. ) lower the boiling point. D) raise the triple point. E) lower the triple point. Answer Key 1. E 2. D 3. D 4. B 5. B 6. B 7. D 8. A 9. B 10. E 11. D 12. A E 15. A B 19. A 20. B D A 25. A 26. E 27. E 28. D 29. A 30. B D 35. A 36. D 37. B 38. E 39. B D 43. E 44. A 45. A 46. E 47. E 48. D A B 53. D 54. A 55. A 56. A 57. B 58. D B 61. A 62. D 63. D 64. A 65. A 66. B 67. B 68. D B 71. B 72. B B 76. A 77. B A 80. D 81. B 82. B 83. B 84. E B 87. B E 90. E 91. D 92. D 93. B 94. B 95. A 96. E 97. B A 100. A
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Summer 2003 1. The molecular geometry of PF 4 + ion is: A. bent B. trigonal planar C. tetrahedral D. octahedral CHEMISTRY 113 EXAM 4(A) 2. The Cl-C-Cl bond angle in CCl 2 O molecule (C is the central atom)
College Chemistry - Problem Drill 15: Chemical Bonding No. 1 of 10 1. Alcohols are a class of organic compounds characterized by one or more hydroxyl (-OH) groups connected to a carbon atoms of a hydrocarbon
Chapter 16 Covalent Bonding Reading Assignment C16! 1. Read C16 pp. 436-469 and while reading, continue building your science vocabulary table that includes all terms in bold face type and all terms you
Molecular Structure I. Valence Bond Theory A. General 1. We will consider the covalent compounds formed by the interactions of nonmetals. 2. They interact by sharing electrons between them. 3. Two theories,
ν = = = = λ ν = = = = = = = λ λ = ν = = = λ ν λ = = = ν λ = λ 2004 SCORING GUIDELINES Question 7 Use appropriate chemical principles to account for each of the following observations. In each part, your
Class: Date: Chapter 9-10 practice test Multiple Choice Identify the choice that best completes the statement or answers the question. 1. Which one of the following is most likely to be an ionic compound?
Lewis Structures Molecular Shape VSEPR Model (Valence Shell Electron Pair Repulsion Theory) PART 1: Ionic Compounds Complete the table of Part 1 by writing: The Lewis dot structures for each metallic and
Chapter 6 Chemical Bonding 6-1 Introduction to Chemical Bonding 1. A chemical bond is a mutual between the nuclei and electrons of different atoms that binds the atoms together. 2. By bonding with each
Revised 12/2015 LEWIS STRUCTURES Chemistry 1104 L The purpose of this experiment is to gain practical experience of drawing lewis structures and to use molecular models to represent the three-dimensional
Chemical Bonds Elements form bonds to be in a lower energy state 1. Ionic Bonds transfer of electrons, between metal and nonmetal 2. Covalent Bonds sharing of electrons, between two nonmetals 3. Metallic
CEM 101 Exam 4 Form 2 (Green) November 30, 2001 Page 1 Section This exam consists of 8 pages. When the exam begins make sure you have one of each. Print your name at the top of each page now. Show your
CHAPTER NINE COVALENT BONDING: ORBITALS Questions 7. Bond energy is directly proportional to bond order. Bond length is inversely proportional to bond order. Bond energy and bond length can be measured.
#52 Notes Unit 7: Bonding Ch. Bonding I. Bond Character Bonds are usually combinations of ionic and covalent character. The electronegativity difference is used to determine a bond s character. Electronegativity
7 Chapter Covalent Bonding Chemistry 4th Edition McMurry/Fay Dr. Paul Charlesworth Michigan Technological University The Covalent Bond 01 Covalent bonds are formed by sharing at least one pair of electrons.
1 Shape of Molecules and their Interactions Chapter 3 Lewis Structures 2 Predicts what molecules look like in three dimension. The 3-Dimensional structure determines the physical properties such as B.P.,
HW07 - VSEPR & VB This is a preview of the draft version of the quiz Started: Aug 8 at 4:51pm Quiz Instructions Homework 07 - VSEPR & VB Question 1 Consider the structural formula of phenol. The active
Previous Chapter Table of Contents Next Chapter Chapter 9: Molecular Geometry and Hybridization of Atomic Orbitals Section 9.1: Molecular Geometry and the VSEPR Model Molecular geometry is the three-dimensional
Molecular and VSEPR We gratefully acknowledge Portland ommunity ollege for the use of this experiment. Objectives To construct molecular models for covalently bonded atoms in molecules and polyatomic ions
Chapter 11 Review Student: 1. Helium atoms do not combine to form He 2 molecules, yet He atoms do attract one another weakly through A. dipole-dipole forces. B. ion-dipole forces. C. dispersion forces.
Name Date Class MOLECULAR COMPOUNDS Section Review Objectives Distinguish molecular compounds from ionic compounds Identify the information a molecular formula provides Vocabulary covalent bond diatomic
Solids An Introduction to Structures and Types of Solids Amorphous Solids: Considerable disorder in structure Crystalline Solids: Highly regular arrangements of their components (atoms, ions, molecules)
Chemical Bonding Introduction to Chemical Bonding Chemical Bonds A chemical bond is a mutual attraction between nuclei and valence electrons of different atoms that binds the atoms together. A chemical
A REVIEW OF GENERAL CEMISTRY: ELECTRONS, BONDS AND MOLECULAR PROPERTIES A STUDENT SOULD BE ABLE TO: 1. Draw Lewis (electron dot and line) structural formulas for simple compounds and ions from molecular
Page 1 of 9 AP Chemistry--Chapters 8,9,10: Bonding, Orbitals, and Liquids and Solids I. Bond Formation A. Bond Energy--Bonds result from the tendency of a system to seek its lowest possible energy (table
Please print: Last name: Answer Key First name: hem 1062 Exam 1 Spring 2005 Andy Aspaas, Instructor Thursday, February 3, 2005 Instructions: Time: You have 90 minutes to complete this exam. Equations and
1. Which of the following compounds is capable of hydrogen bonding? A. H 2 CO B. CH 3 COCH 3 C. CH 3 OCH 3 D. NF 3 E. CH 3 CH 2 OH 2. Which of the following correctly illustrates the relative magnitudes
CEMICAL BONDS UNIT 5: Bonding A. Definition: A chemical bond is the force holding two atoms together in a chemical compound. B. Bonds form from the attraction 1. Between the positive nucleus of one atom
Liquids and Solids General Chemistry I 2302101 Dr Rick Attrill Office MHMK 1405/5 Intermolecular Forces Properties of Liquids Crystal Structure X ray Diffraction by Crystals Types of Crystals Amorphous
3 Types of Chemical Bonds 1. Ionic Bonds: refers to the electrostatic forces between oppositely charged particles (usually a metallic and a nonmetallic element). Ex: NaCl ------ Na + and Cl - Because Na
Objectives 1. To learn about ionic and covalent bonds and explain how they are formed - what holds compounds together? 2. To learn about the polar covalent bond are all covalent bonds equal? 3. To understand
Chapter 6: Chemical Bonding I. Introduction to Chemical Bonding A. A Chemical Bond is a mutual electrical attraction between the nuclei and valence electrons of different atoms that binds the atoms together.