Name (printed): Signature:
|
|
- Madeline Cooper
- 5 years ago
- Views:
Transcription
1 CHEM Lab Section Number: Name (printed): Signature: This exam consists of 36 questions all of equal value for a total of 225 points. Make sure that your test has all of the pages. Please read each problem carefully. There are no intentionally misleading questions; each problem should be taken at its face value. Please mark your answers on the Scantron sheet provided to you and on the actual exam. You will be given a periodic table and an exam information sheet to use during the exam. You may remove it from the exam make it more accessible. You may also use the designated Casio fx-300ms-plus calculator or equivalent non-programmable non-graphing scientific calculator during the exam. Use the back pages of the test as scratch paper. You are not allowed to use any devices capable of accessing the internet, textbooks, notes, or homemade reference sheets during the exam. You may leave if you finish the exam early. Give the exam and the information sheet to your TA and leave quietly without disturbing other students. Before leaving, check that all your answers have been properly entered on the Scantron sheet and the exam and that your name is written on every page of the exam and on the Scantron sheet. All cell phones and electronic devices must be turned off and put away. Please remove all hats and caps. Place your books and all papers out of sight under your seat. If the TA believes that you might be looking at your neighbor s paper, you will be asked to move to a new location. Exam scores will be posted on Blackboard as soon as the grading is complete. Your test will be returned to you in the first lab meeting of next week. If you have any questions regarding the grading of your exam, please notify your TA. The time available for the exam is 120 minutes. Good luck! 1 of 9
2 Name: Lab Section #: Please mark your answers on the scantron sheet using a #2 pencil and also mark your answers on the exam itself. Mark Test From B on your scantron. 1. Which one of the following properties is least characteristic of substances composed of small, covalently-bonded molecules? (a) brittle (b) low boiling point (c) poor electrical conductor when solid (d) poor electrical conductor when molten (e) high melting point 2. In which of these substances are the atoms held together by polar covalent bonding? (a) S8 (b) SrCl2 (c) CsCl (d) CaF2 (e) ClF 3. Select the correct formula for a compound formed from barium and nitrogen. (a) Ba3N2 (b) Ba2N (c) Ba2N3 (d) BaN (e) BaN2 4. Select the element with the lowest electronegativity. (a) Li (b) Al (c) Cl (d) Cs (e) Ca 5. Select the compound with the highest lattice energy. (a) BaO (b) NaI (c) LiBr (d) MgO (e) CaS 2 of 9
3 6. Select the most polar bond amongst the following. (a) C O (b) Si F (c) Cl F (d) C F (e) C I 7. Select the element whose Lewis dot structure is correct. (a) (b) (c) (d) (e) 8. Which of the following contains ionic bonding? (a) SrF2 (b) CO2 (c) H2O (d) HF (e) Al 9. In which one of the following species is the central atom (the first atom in the formula) an exception to the octet rule? (a) SF6 (b) NH3 (c) NH4 + (d) I2 (e) BH4 10. Select the correct Lewis structure for ClCN. (a) (b) (c) (d) (e) 3 of 9
4 11. In which of the molecules below does the central atom have an sp 3 d 2 orbital hybridization? (a) XeF2 (b) H2O (c) CH4 (d) XeF4 (e) SO Oxygen difluoride is a powerful oxidizing and fluorinating agent. Select its Lewis structure. (a) (b) (c) (d) (e) None of the above are correct. 13. The electronic structure of the CO3 2- molecule is best represented as a resonance hybrid of equivalent structures and what is the formal change of C? (a) 2, +1 (b) 3, +2 (c) 4, +2 (d) 3, 0 (e) This molecule does not exhibit resonance, In which of the following is the best Lewis structure a resonance structure? (a) SO3 (b) BF3 (c) I3 (d) SCO (C is the central atom) (e) SO The formal charge on Cl in the structure shown for the perchlorate ion is (a) -2 (b) +1 (c) 0 (d) -1 (e) +2 4 of 9
5 16. Considering all the bonds in a molecule with trigonal bipyramidal geometry, what are the bond angles present? (a) 120 º only (b) 90 º only (c) 90 º, 120 º, and 180 º (d) 60 º and 90 º only (e) 180 º only 17. Estimate the heat of reaction at 298 K for the reaction shown, given the average bond energies below: 2H2(g) + O2(g) 2H2O(g) H-H O=O H-O Bond Energy (kj/mol) (a) 1371 kj (b) -481 kj (c) 935 kj (d) -926 kj (e) kj 18. What is the molecular shape of BCl3 as predicted by VSEPR theory? (a) linear (b) tetrahedral (c) trigonal planar (d) trigonal pyramidal (e) none of the above 19. What is the molecular shape of NO2 as predicted by the VSEPR theory? (a) bent (b) tetrahedral (c) T-shaped (d) trigonal pyramidal (e) linear 20. What is the molecular shape of XeO2F2 as predicted by the VSEPR theory? (a) square planar (b) see-saw (c) tetrahedral (d) square pyramidal (e) octahedral 5 of 9
6 21. Which one of the following molecules and ions will have a square planar geometry as predicted by the VSEPR theory? (a) PCl3 (b) BF4 (c) XeF4 (d) BrF5 (e) H3O What is the hybridization of the central atom in a molecule of NH3? (a) sp (b) sp 2 (c) sp 3 (d) sp 3 d (e) sp 3 d What is the molecular structure and electron pair geometry of H2S? (a) Trigonal bipyramidal and Linear (b) Linear and Tetrahedral (c) Bent and Tetrahedral (d) Tetrahedral and Bent (e) Linear and Linear (f) 24. According to the valence bond theory, which is the best definition of a pi (π) bond? (a) A removal and transfer of electrons from one atom to another. (b) A side-by-side overlap of two p orbitals. (c) The out-of-phase overlap of atomic orbitals, resulting in a node along the internuclear axis. (d) The presence of two orbitals with the same energy near their respective nuclei. (e) A covalent bond formed by the overlap of atomic orbitals along the internuclear axis. 25. The perchloric acid (HClO4) molecule contains? (a) 13 lone pairs, 1 pi bond, and 4 sigma bonds. (b) 9 lone pairs, no pi bonds, and 6 sigma bonds. (c) 8 lone pairs, 2 pi bonds, and 7 sigma bonds (d) 8 lone pairs, 3 pi bonds, and 5 sigma bonds. (e) 11 lone pairs, no pi bonds, and 5 sigma bonds. 26. Antibonding molecular orbitals are produced by (a) constructive interaction of atomic orbitals. (b) destructive interaction of atomic orbitals. (c) the overlap of the atomic orbitals of two negative ions (d) all of these 6 of 9
7 (e) none of these 27. Which of the following molecules is non-polar? (a) H2O (b) XeF4 (c) BrCl3 (d) CH3CH2OH (e) CH3Cl To the right is a molecule of Ibuprofen. The lone pairs of electrons have been omitted for clarity. Every atoms in the structure follows the octet rule. Use the structure in answering the following 4 questions. 28. How many lone pairs of electrons are there on a molecule of Ibuprofen? (a) 4 (b) 5 (c) 6 (d) 8 (e) How many of the carbon atoms in a Ibuprofen molecule have sp 2 hybridization? (a) 3 (b) 4 (c) 5 (d) 6 (e) How many pi (π) bonds are there on the molecule of Ibuprofen? (a) 2 (b) 4 (c) 6 (d) 8 (e) How many carbon atoms in the Ibuprofen structure adopts the sp 3 hybridization? (a) 2 (b) 3 (c) 4 (d) 5 (e) 6 7 of 9
8 Use the molecular orbital diagrams below to answer the following 4 questions. 32. Which of the molecules listed below does not have a bond order of 2? (a) O2 (b) F2 2+ (c) ONe (d) C2 (e) CN For the molecular N2 +. The number of electrons in the σ 2p molecular orbital is (a) 0 (b) 1 (c) 2 (d) 3 (e) What is the bond order for a molecule of O2 +? (a) 0.5 (b) 1 (c) 1.5 (d) 2 (e) For the molecule B2, the number of unpaired electrons is (a) 0 (b) 1 (c) 2 (d) 3 (e) 4 8 of 9
9 36. When a double bond is formed between two carbon atoms in the ethylene (C2H4) molecule, one of the bond is a sigma bond and the other is a pi bond, the sigma bond is formed by overlap of? (a) P orbitals (b) S orbitals (c) sp hybrid orbitals (d) sp 2 hybrid orbitals (e) sp 3 hybrid orbitals 9 of 9
Name (printed): Signature:
CHEM Lab Section Number: Name (printed): Signature: This exam consists of 36 questions all of equal value for a total of 225 points. Make sure that your test has all of the pages. Please read each problem
More informationName (printed): Signature:
CHEM Lab Section Number: Name (printed): Signature: This exam consists of 36 questions all of equal value for a total of 225 points. Make sure that your test has all of the pages. Please read each problem
More informationName (printed): Signature:
CHEM Lab Section Number: Name (printed): Signature: This exam consists of 36 questions all of equal value for a total of 225 points. Make sure that your test has all of the pages. Please read each problem
More informationName (printed): Signature:
CHEM Lab Section Number: Name (printed): Signature: This exam consists of 36 questions all of equal value for a total of 225 points. Make sure that your test has all of the pages. Please read each problem
More informationName (printed): Signature:
CHEM Lab Section Number: Name (printed): Signature: This exam consists of 36 questions all of equal value for a total of 225 points. Make sure that your test has all of the pages. Please read each problem
More informationName (printed): Signature:
CHEM Lab Section Number: Name (printed): Signature: This exam consists of 36 questions all of equal value for a total of 225 points. Make sure that your test has all of the pages. Please read each problem
More informationName (printed): Signature:
CHEM Lab Section Number: Name (printed): Signature: This exam consists of 36 questions all of equal value for a total of 225 points. Make sure that your test has all of the pages. Please read each problem
More informationCHEM 200/202 Exam 3-A November 15, Name (printed): Signature:
HEM 200/202 Exam 3-A November 15, 2014 HEM Lab Section Number: Name (printed): (Last) (irst) Signature: This exam consists of 32 questions at 5 points each for a total of 160 points. Make sure that your
More informationForm J. Test #4 Last Name First Name Zumdahl, Chapters 8 and 9 November 23, 2004
Form J Chemistry 1441-023 Name (please print) Test #4 Last Name First Name Zumdahl, Chapters 8 and 9 November 23, 2004 Instructions: 1. This exam consists of 27 questions. 2. No scratch paper is allowed.
More informationAP Chemistry- Practice Bonding Questions for Exam
AP Chemistry- Practice Bonding Questions for Exam Multiple Choice Identify the choice that best completes the statement or answers the question. 1. Which of the following is a correct Lewis structure for
More informationName (printed): Signature:
CHEM Lab Section Number: Name (printed): Signature: This exam consists of 36 questions all of equal value for a total of 225 points. Make sure that your test has all of the pages. Please read each problem
More informationChemical Bonding II: Molecular Geometry and Hybridization of Atomic Orbitals
Chemical Bonding II: Molecular Geometry and Hybridization of Atomic Orbitals 1 Chemical Bonding II Molecular Geometry (10.1) Dipole Moments (10.2) Valence Bond Theory (10.3) Hybridization of Atomic Orbitals
More informationUNIVERSITY OF VICTORIA. CHEMISTRY 101 Mid-Term Test 2, November
NAME Student No. SECTIN (circle one): A01 (Codding) A02 (Sirk) A03 (Briggs) Version A UNIVERSITY F VICTRIA CEMISTRY 101 Mid-Term Test 2, November 19 2010 Version A This test has two parts and 8 pages,
More informationDownloaded from
Points to Remember Class: XI Chapter Name: Chemical Bonding and Molecular Structure Top Concepts 1. The attractive force which holds together the constituent particles (atoms, ions or molecules) in chemical
More informationLewis Structure. Lewis Structures & VSEPR. Octet & Duet Rules. Steps for drawing Lewis Structures
Lewis Structure Lewis Structures & VSEPR Lewis Structures shows how the are arranged among the atoms of a molecule There are rules for Lewis Structures that are based on the formation of a Atoms want to
More information2011, Robert Ayton. All rights reserved.
Chemical Bonding Outline 1. Lewis Dot Structures 2. Bonds 3. Formal Charges 4. VSEPR (Molecular Geometry and Hybridzation) 5. Common Resonance Structures and Dimerization Review 1. Lewis Dot Structures
More informationCovalent bonding does not involve electrostatic attraction between oppositely charged particles.
SCH3U7 - Topic 4: Bonding Review SL Which of these bonding types would not be classified as strong? Metallic Covalent Ionic Dipole dipole The bond dissociation energy of NaCl is 411 kj mol -1, while that
More informationName: Class: Date: 3. How many lone pairs of electrons are assigned to the carbon atom in carbon monoxide? a. 0 b. 1 c. 2 d. 3
Class: Date: Midterm 3, Fall 2009 Record your name on the top of this exam and on the scantron form. Record the test ID letter in the top right box of the scantron form. Record all of your answers on the
More informationI. Multiple Choice Questions (Type-I)
I. Multiple Choice Questions (Type-I) 1. Isostructural species are those which have the same shape and hybridisation. Among the given species identify the isostructural pairs. (i) [NF 3 and BF 3 ] [BF
More informationMolecular Geometry and Chemical Bonding Theory
Molecular Geometry and Chemical Bonding Theory The Valence -Shell Electron -Pair Repulsion (VSEPR) Model predicts the shapes of the molecules and ions by assuming that the valence shell electron pairs
More informationSUPeR Chemistry CH 222 Practice Exam
SUPeR Chemistry CH 222 Practice Exam This exam has been designed to help you practice working multiple choice problems over the material that will be covered on the first CH 222 midterm. The actual exams
More informationMolecular Geometry and intermolecular forces. Unit 4 Chapter 9 and 11.2
1 Molecular Geometry and intermolecular forces Unit 4 Chapter 9 and 11.2 2 Unit 4.1 Chapter 9.1-9.3 3 Review of bonding Ionic compound (metal/nonmetal) creates a lattice Formula doesn t tell the exact
More informationMOLECULAR ORBITAL DIAGRAM KEY
365 MOLECULAR ORBITAL DIAGRAM KEY Draw molecular orbital diagrams for each of the following molecules or ions. Determine the bond order of each and use this to predict the stability of the bond. Determine
More informationChapter 9 practice questions
Class: Date: Chapter 9 practice questions Multiple Choice Identify the choice that best completes the statement or answers the question. 1. All of the following statements concerning valence bond (VB)
More informationClass XI: Chemistry Chapter 4: Chemical Bonding and Molecular Structure Top Concepts
1 Class XI: Chemistry Chapter 4: Chemical Bonding and Molecular Structure Top Concepts 1. The attractive force which holds together the constituent particles (atoms, ions or molecules) in chemical species
More informationChemical Bonding II: Molecular Geometry and Hybridization of Atomic Orbitals Chapter 10
Chemical Bonding II: Molecular Geometry and Hybridization of Atomic Orbitals Chapter 10 Linear Trigonal 180 o planar 120 o Tetrahedral 109.5 o Trigonal Bipyramidal 120 and 90 o Octahedral 90 o linear Linear
More informationChapter 6 PRETEST: Chemical Bonding
Chapter 6 PRETEST: Chemical In the space provided, write the letter of the term or phrase that best completes each statement or best answers each question. 1.The charge on an ion is a. always positive.
More informationChemical Bonding AP Chemistry Ms. Grobsky
Chemical Bonding AP Chemistry Ms. Grobsky What Determines the Type of Bonding in Any Substance? Why do Atoms Bond? The key to answering the first question are found in the electronic structure of the atoms
More informationCHEMISTRY 15 EXAM IV-Version A (White)
CHEMISTRY 15 EXAM IV-Version A (White) Dr. M. Richards-Babb June 26, 2001 An optical scoring machine will grade this examination. The machine is not programmed to accept the correct one of two sensed answers
More informationEXAM II Material. Part I Chemical Bonding I Lewis Theory Chapter 9 pages A. Drawing electron dot structures HOW TO:
CHEMISTRY 112 LECTURE EXAM II Material Part I Chemical Bonding I Lewis Theory Chapter 9 pages 376-386 A. Drawing electron dot structures HOW TO: 1. Write e- dot structure for the individual atoms. 2. a)
More informationGeneral and Inorganic Chemistry I.
General and Inorganic Chemistry I. Lecture 1 István Szalai Eötvös University István Szalai (Eötvös University) Lecture 1 1 / 29 Outline István Szalai (Eötvös University) Lecture 1 2 / 29 Lewis Formulas
More informationName ID# Section # CH 1010 EXAM 2 Fall Form A
Name ID# Section # CH 1010 EXAM 2 Fall 2016 - Form A Fill in your name, ID#, and section on this test booklet. Fill in and bubble in your name, ID# (for the letter C bubble zero), and section on the scantron
More informationWhat Do Molecules Look Like?
What Do Molecules Look Like? The Lewis Dot Structure approach provides some insight into molecular structure in terms of bonding, but what about 3D geometry? Recall that we have two types of electron pairs:
More informationEx. 1) F F bond in F = 0 < % covalent, no transfer of electrons
#60 Notes Unit 8: 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
More informationSL Score. HL Score ! /30 ! /48. Practice Exam: Paper 1 Topic 4: Bonding. Name
Name Practice Exam: Paper 1 Topic 4: Bonding SL SL Score! /30 HL Score! /48 1. What is the correct Lewis structure for hypochlorous acid, a compound containing chlorine, hydrogen and oxygen? A. B. C. D.
More informationCH 222 Sample Exam Exam I Name: Lab Section:
222 Sample Exam Exam I Name: Lab Section: Part I: Multiple hoice Questions (100 Points) Use a scantron sheet for Part I. There is only one best answer for each question. 1. Which of the following statements
More informationName Unit Three MC Practice March 15, 2017
Unit Three: Bonding & Molecular Geometry Name Unit Three MC Practice March 15, 2017 1. What is the hybridization of the oxygen atom in water? a) sp b) sp 2 c) sp 3 d) It is not hybridized 2. When a double
More informationGroup 1 Group 2 Group 3 Group 4 Group 5 Group 6 Group 7 Group 8. Na Mg Al Si P S Cl Ar
CHM 111 Chapters 7 and 8 Worksheet and Study Guide Purpose: This is a guide for your as you work through the chapter. The major topics are provided so that you can write notes on each topic and work the
More informationCHEM 110 Exam 2 - Practice Test 1 - Solutions
CHEM 110 Exam 2 - Practice Test 1 - Solutions 1D 1 has a triple bond. 2 has a double bond. 3 and 4 have single bonds. The stronger the bond, the shorter the length. 2A A 1:1 ratio means there must be the
More informationCHEMISTRY 112 LECTURE EXAM II Material
CHEMISTRY 112 LECTURE EXAM II Material Part I Chemical Bonding I Lewis Theory Chapter 9 pages 376-386 A. Drawing electron dot structures HOW TO: 1. Write e- dot structure for the individual atoms. 2. a)
More informationChapter 9. Lewis Theory-VSEPR Valence Bond Theory Molecular Orbital Theory
Chapter 9 Lewis Theory-VSEPR Valence Bond Theory Molecular Orbital Theory Problems with Lewis Theory Lewis theory generally predicts trends in properties, but does not give good numerical predictions.
More informationBonding. Honors Chemistry 412 Chapter 6
Bonding Honors Chemistry 412 Chapter 6 Chemical Bond Mutual attraction between the nuclei and valence electrons of different atoms that binds them together. Types of Bonds Ionic Bonds Force of attraction
More informationChapter 7. Chemical Bonding I: Basic Concepts
Chapter 7. Chemical Bonding I: Basic Concepts Chemical bond: is an attractive force that holds 2 atoms together and forms as a result of interactions between electrons found in combining atoms We rarely
More information51. Pi bonding occurs in each of the following species EXCEPT (A) CO 2 (B) C 2 H 4 (C) CN (D) C 6 H 6 (E) CH 4
Name AP Chemistry: Bonding Multiple Choice 41. Which of the following molecules has the shortest bond length? (A) N 2 (B) O 2 (C) Cl 2 (D) Br 2 (E) I 2 51. Pi bonding occurs in each of the following species
More informationHybridisation 1. Hybridisation involves 1. Inter mixing of electron s 2. Inter mixing and redistribution of atomic orbitals of only one atom 3. Inter mixing and redistribution of atomic orbitals of different
More informationChapter 10: Chemical Bonding II: Molecular Shapes; VSEPR, Valence Bond and Molecular Orbital Theories
C h e m i s t r y 1 A : C h a p t e r 1 0 P a g e 1 Chapter 10: Chemical Bonding II: Molecular Shapes; VSEPR, Valence Bond and Molecular Orbital Theories Homework: Read Chapter 10: Work out sample/practice
More informationChapters 8 and 9. Octet Rule Breakers Shapes
Chapters 8 and 9 Octet Rule Breakers Shapes Bond Energies Bond Energy (review): The energy needed to break one mole of covalent bonds in the gas phase Breaking bonds consumes energy; forming bonds releases
More informationHouston Community College System. Chemistry EXAM # 3A Sample
Houston Community College System Chemistry 1411 EXAM # A Sample 1 CHEM 1411 EXAM # (Chapters 8, 9,10,and 11) Name: Score: Directions- please answer the following multiple-choice questions next to each
More informationShapes of Molecules. Lewis structures are useful but don t allow prediction of the shape of a molecule.
Shapes of Molecules Lewis structures are useful but don t allow prediction of the shape of a molecule. H O H H O H Can use a simple theory based on electron repulsion to predict structure (for non-transition
More informationCHE 105 FINAL EXAMINATION December 13, 2010
CHE 105 FINAL EXAMINATIN December 13, 2010 University of Kentucky Department of Chemistry READ THESE DIRECTINS CAREFULLY BEFRE STARTING THE EXAMINATIN! It is extremely important that you fill in the answer
More informationLecture outline: Section 9. theory 2. Valence bond theory 3. Molecular orbital theory. S. Ensign, Chem. 1210
Lecture outline: Section 9 Molecular l geometry and bonding theories 1. Valence shell electron pair repulsion theory 2. Valence bond theory 3. Molecular orbital theory 1 Ionic bonding Covalent bonding
More informationStructures, Shapes and Polarity. of Molecules. Level 2 recap: - Polar and non polar bonds - Lewis diagrams - Lone pairs - Shapes - Polarity
Structures, Shapes and Polarity Level 2 recap: - Polar and non polar bonds - Lewis diagrams - Lone pairs - Shapes - Polarity of Molecules Do now: Brainstorm what you know/remember about these L2 concepts
More informationChapter 10. VSEPR Model: Geometries
Chapter 10 Molecular Geometry VSEPR Model: Geometries Valence Shell Electron Pair Repulsion Theory Electron pairs repel and get as far apart as possible Example: Water Four electron pairs Farthest apart
More informationUnit Six --- Ionic and Covalent Bonds
Unit Six --- Ionic and Covalent Bonds Electron Configuration in Ionic Bonding Ionic Bonds Bonding in Metals Valence Electrons Electrons in the highest occupied energy level of an element s atoms Examples
More informationChapter 9 Molecular Geometries. and Bonding Theories
Chapter 9 Molecular Geometries and Bonding Theories Coverage of Chapter 9 9.1 All 9.2 All 9.3 All 9.4 All 9.5 Omit Hybridization Involving d Orbitals 9.6 All 9.7 and 9.8 Omit ALL MOLECULAR SHAPES The shape
More informationBonding/Lewis Dots Lecture Page 1 of 12 Date. Bonding. What is Coulomb's Law? Energy Profile: Covalent Bonds. Electronegativity and Linus Pauling
Bonding/Lewis Dots Lecture Page 1 of 12 Date Bonding What is Coulomb's Law? Energy Profile: Covalent Bonds Electronegativity and Linus Pauling 2.1 H 1.0 Li 0.9 Na 0.8 K 0.8 Rb 0.7 Cs 0.7 Fr 1.5 Be 1.2
More informationFill in the chart below to determine the valence electrons of elements 3-10
Chemistry 11 Atomic Theory IV Name: Date: Block: 1. Lewis Diagrams 2. VSEPR Lewis Diagrams Lewis diagrams show the bonding between atoms of a molecule. Only the outermost electrons of an atom (called electrons)
More informationCHEM PRACTICE EXAM IV CLASS - SPRING 2017 ANSWER KEY
CHEM 1031 - PRACTICE EXAM IV CLASS - SPRING 2017 ANSWER KEY 1. When Group 1A (except for H) and Group 17 (7A) elements react with each other, they are most likely to form: A. Covalent or ionic bonds B.
More informationInstant download Test bank for Chemistry The Central Science 10th Edition by Brown, LeMay, Bursten CLICK HERE
Chemistry, 10e (Brown) Chapter 9, Molecular Geometry and Bonding Theories Instant download Test bank for Chemistry The Central Science 10th Edition by Brown, LeMay, Bursten CLICK HERE http://testbankair.com/download/test-bank-for-chemistry-the-central-science-10th-edition-by-brown-lemay-bursten/
More informationMolecular shape is determined by the number of bonds that form around individual atoms.
Chapter 9 CH 180 Major Concepts: Molecular shape is determined by the number of bonds that form around individual atoms. Sublevels (s, p, d, & f) of separate atoms may overlap and result in hybrid orbitals
More information1. There are paired and unpaired electrons in the Lewis symbol for a phosphorus atom. a. 4, 2 b. 2, 4 c. 2, 3 d. 4, 3 e. 0, 3
Name: Score: 0 / 42 points (0%) [2 open ended questions not graded] C8&9Practice Multiple Choice Identify the choice that best completes the statement or answers the question. 1. There are paired and unpaired
More informationChapter 10 Theories of Covalent Bonding
Chapter 10 Theories of Covalent Bonding 1 Atomic Orbitals Molecules Bonding and 2 Molecular Structure Questions How are molecules held together? Why is O 2 paramagnetic? And how is this property connected
More informationMolecular Geometry. Objectives N H H. The objectives of this laboratory are to:
Objectives The objectives of this laboratory are to: Molecular Geometry Write Lewis structure representations of the bonding and valence electrons in molecules. Use the VSEPR model to predict the molecular
More informationName (printed): Signature:
CHEM Lab Section Number: Name (printed): Signature: This exam consists of 36 questions all of equal value for a total of 225 points. Make sure that your test has all of the pages. Please read each problem
More informationChapter 7 Chemical Bonding and Molecular Structure
Chapter 7 Chemical Bonding and Molecular Structure Three Types of Chemical Bonding (1) Ionic: formed by electron transfer (2) Covalent: formed by electron sharing (3) Metallic: attraction between metal
More information3) Find the Bond Order of H2, N2, and O2 respectively 1. 0, 1, , 3, , 3, , 1, 0 5. None of the Above
Form Code X NAME CHM 2045, Spring 2018, Exam 3 Review Packet (Broward Teaching Center) Final Packet Instructions: Do your best and don t be anxious. Read the question, reread the question, write down all
More informationCovalent Compounds: Bonding Theories and Molecular Structure
CHM 123 Chapter 8 Covalent Compounds: Bonding Theories and Molecular Structure 8.1 Molecular shapes and VSEPR theory VSEPR theory proposes that the geometric arrangement of terminal atoms, or groups of
More informationBonding and IMF practice test MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.
Exam Name Bonding and IMF practice test MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) There are paired and unpaired electrons in the Lewis symbol
More informationHourEx4 Practice Chapt 8 & 9 Kotz
HourEx4 Practice Chapt 8 & 9 Kotz Multiple Choice 5 pts apiece Identify the letter of the choice that best completes the statement or answers the question. PUT YOUR ANSWER ON THE BUBBLE SHEET PROVIDED.You
More informationName (printed): Signature:
CHEM Lab Section Number: Name (printed): Signature: This exam consists of 36 questions all of equal value for a total of 225 points. Make sure that your test has all of the pages. Please read each problem
More information2. Write the electron configuration notation and the electron dot notation for each: (a) Ni atom (b) Ni 2+ ion (c) Ni 3+ ion
EXTRA HOMEWORK 2A 1. Predict whether each of the following types of matter will be bonded with ionic, covalent, or metallic bonds, and identify whether each will be composed of atoms, ions, or molcules
More informationCovalent Bonds: overlap of orbitals σ-bond π-bond Molecular Orbitals
Covalent Bonding What is covalent bonding? Covalent Bonds: overlap of orbitals σ-bond π-bond Molecular Orbitals Hybrid Orbital Formation Shapes of Hybrid Orbitals Hybrid orbitals and Multiple Bonds resonance
More informationContents. 1. Basic Concepts. 2. The Covalent Bond. 3. The Valence-Shell Electron-Pair Repulsion Models 4. Bond theories. 5. The Metallic Bond.
Chemical Bonding (II) Topic 4. Chemical Bonding (II) (II) 1 Contents 1. Basic Concepts. a) Molecular parameters b) Lewis Dot Symbols 2. The Covalent Bond a) Polar Covalent Bond b) Formal Charge c) Exceptions
More informationChemical Bonding II: Molecular Geometry and Hybridization of Atomic Orbitals Chapter 1
Chemical Bonding II: Molecular Geometry and Hybridization of Atomic Orbitals Chapter 1 Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. How to get the book of
More information1. Sodium nitrite is an ionic compound containing a polyatomic ion. Answer the following questions relative to nitrite.
Ch 10-11 Practice Problems - KEY The following problems are intended to provide you with additional practice in preparing for the exam. Questions come from the textbook, previous quizzes, previous exams,
More informationQ. No. 2 Bond formation is. Neither exothermic nor endothermic
Q. No. 1 Which combination will give the strongest ionic bond? K + and Cl - K + and O 2- Ca 2+ and Cl - Ca 2+ and O 2- In CaO, the polarizability of O 2- is very less therefore it has the maximum ionic
More informationValence Bond Theory - Description
Bonding and Molecular Structure - PART 2 - Valence Bond Theory and Hybridization 1. Understand and be able to describe the Valence Bond Theory description of covalent bond formation. 2. Understand and
More informationChemistry 1210, Section 1 Third Hour Exam November 21, 2011
Chemistry 1210, Section 1 Third Hour Exam November 21, 2011 Instructions: Do not begin until 8:30 AM. The exam must be turned in by 9:20 AM. Enjoy your thanksgiving break! This exam should have 25 questions.
More informationChapter 9. Chemical Bonding II: Molecular Geometry and Bonding Theories
Chapter 9 Chemical Bonding II: Molecular Geometry and Bonding Theories Topics Molecular Geometry Molecular Geometry and Polarity Valence Bond Theory Hybridization of Atomic Orbitals Hybridization in Molecules
More informationChapter 4. Molecular Structure and Orbitals
Chapter 4 Molecular Structure and Orbitals Chapter 4 Table of Contents (4.1) (4.2) (4.3) (4.4) (4.5) (4.6) (4.7) Molecular structure: The VSEPR model Bond polarity and dipole moments Hybridization and
More informationNOTES #28 Bonds & Thermochemistry AP Chemistry
NOTES #28 Bonds & Thermochemistry AP Chemistry - When studying thermochemistry, we determined ΔH or ΔH rxn of a reaction by using ΔH f values. For practice s sake, determine ΔH rxn for the formation of
More informationLESSON 10. Glossary: Molecular Geometry. a quantitative measure of the degree of charge separation in a molecule. Dipole moment
LESSON 10 Glossary: Molecular Geometry Dipole moment Electronegativity Molecular geometry Pi bond Polar covalent bond Sigma bond Valence-shell electronpair repulsion (VSEPR) model a quantitative measure
More informationDO NOT OPEN UNTIL INSTRUCTED TO DO SO. CHEM 110 Dr. McCorkle Exam #5 KEY. While you wait, please complete the following information:
DO NOT OPEN UNTIL INSTRUCTED TO DO SO CHEM 110 Dr. McCorkle Exam #5 KEY While you wait, please complete the following information: Name: Student ID: Turn off cellphones and stow them away. No headphones,
More informationCHM2045 S13: Exam # MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.
CHM2045 S13: Exam #2 2013.03.01 MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) How would replacing one of benzene's C atoms and the H atom attached
More informationPlease pass in only this completed answer sheet on the day of the test. LATE SUBMISSIONS WILL NOT BE ACCEPTED
CHM-201 General Chemistry and Laboratory I Unit #4 Take Home Test Due December 13, 2018 Please pass in only this completed answer sheet on the day of the test. LATE SUBMISSIONS WILL NOT BE ACCEPTED CHM-201
More informationTest bank for Chemistry The Central Science 10th Edition by Brown, LeMay, Bursten
Test bank for Chemistry The Central Science 10th Edition by Brown, LeMay, Bursten Chapter 9, Molecular Geometry and Bonding Theories Multiple-Choice and Bimodal 1) For a molecule with the formula A) linear
More informationChapter 13: Phenomena
Chapter 13: Phenomena Phenomena: Scientists measured the bond angles of some common molecules. In the pictures below each line represents a bond that contains 2 electrons. If multiple lines are drawn together
More informationHonors Chemistry Unit 6 ( )
Honors Chemistry Unit 6 (2017-2018) Lewis Dot Structures VSEPR Structures 1 We are learning to: 1. Represent compounds with Lewis structures. 2. Apply the VSEPR theory to determine the molecular geometry
More informationThursday, 10:45AM. December 8, PRINT your name on this page and on your computer answer sheet.
Name hemistry 151-001 (3150-151-001) EXAM III Bubble on your scan sheet the orm ode below: Instructions: RM A Thursday, 10:45AM December 8, 2005 225+ pts. 1. Each student is responsible for following instructions.
More informationCh 6 Chemical Bonding
Ch 6 Chemical Bonding What you should learn in this section (objectives): Define chemical bond Explain why most atoms form chemical bonds Describe ionic and covalent bonding Explain why most chemical bonding
More informationCHM2045 F13--Exam # MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.
CHM2045 F13--Exam #2 2013.10.18 MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) A valid Lewis structure of cannot be drawn without violating the
More informationLewis structures show the number and type of bonds between atoms in a molecule or polyatomic ion.
VSEPR & Geometry Lewis structures show the number and type of bonds between atoms in a molecule or polyatomic ion. Lewis structures are not intended to show the 3-dimensional structure (i.e. shape or geometry)
More informationCovalent Bonding and Molecular Structures
CHAPTERS 9 AND 10 Covalent Bonding and Molecular Structures Objectives You will be able to: 1. Write a description of the formation of the covalent bond between two hydrogen atoms to form a hydrogen molecule.
More informationChapter 9. Covalent Bonding: Orbitals
Chapter 9 Covalent Bonding: Orbitals Localized electron model A bond is made when a half-filled orbital of one atom overlaps with a half-filled orbital of another.! Bond: orbitals overlap straight on p
More informationFor more info visit Chemical bond is the attractive force which holds various constituents together in a molecule.
Chemical bond:- Chemical bond is the attractive force which holds various constituents together in a molecule. There are three types of chemical bonds: Ionic Bond, Covalent Bond, Coordinate Bond. Octet
More informationMolecular shape is only discussed when there are three or more atoms connected (diatomic shape is obvious).
Chapter 10 Molecular Geometry (Ch9 Jespersen, Ch10 Chang) The arrangement of the atoms of a molecule in space is the molecular geometry. This is what gives the molecules their shape. Molecular shape is
More informationChem 121 Exam 4 Practice Exam
Chem 121 Exam 4 Practice Exam 1. What is the correct electron configuration for bromine? b. 1s 2 2s 2 2p 6 3s 2 3p 6 3d 9 4s 2 4p 6 c. 1s 2 2s 2 2p 6 3s 2 3p 6 3d 10 4s 2 4p 5 d. 1s 2 2s 2 2p 6 3s 2 3p
More informationCHM1045 Exam 3 Chapters 5, 8, & 9
1. Which of the following conditions will never result in a decrease in the internal energy of a system? CHM1045 Exam 3 Chapters 5, 8, & 9 a. System loses heat and does work on the surroundings. b. System
More informationAssignment 09 A. 2- The image below depicts a seesaw structure. Which of the following has such a structure?
Assignment 09 A 1- Give the total number of electron domains, the number of bonding and nonbonding domains, and the molecular geometry, respectively, for the central atom of P 3. a) four electron domains,
More informationCHE 105 FINAL EXAMINATION May 4, 2010
CE 105 FINAL EXAMINATION May 4, 2010 University of Kentucky Department of Chemistry Read these directions carefully before starting the examination. It is extremely important that you fill in the answer
More information