MANY ELECTRON ATOMS Chapter 15
|
|
- Gabriella Henderson
- 5 years ago
- Views:
Transcription
1 MANY ELECTRON ATOMS Chapter 15 Electron-Electron Repulsions ( ) The hydrogen atom Schrödinger equation is exactly solvable yielding the wavefunctions and orbitals of chemistry. Howev er, the Schrödinger equation cannot be analytically solved when there is more than one electron. Why? Consider the general Schrödinger equation for N electrons: 2 = 2 x y z 2 Were it not for the last term the above Hamiltonian would just be a sum of hydrogen atom hamiltonians for each electron. This last term represents electron-electron repulsion. It may be better understood if we examine the simplest multi-electron Hamiltonian, that for helium coulombic attraction between nucleus and electron kinetic energy of electron coulombic repulsion between electrons Since we have two or more electrons,the Schrödingeröequation cannot be solved exactly (a fundamental challenge for quantum chemistry))because of the last electron repulsion term - the motion of the electrons are correlated. If they did not interact the energy would just be a sum of each electrons's energy and the wavefunction a simple product. The Hartree-Fock Self-Consistent Field Method (15.8) How do we approach this problem?? Well,,try first keeping the simple product form for the wavefunction and use this in the Schrödinger equation: An N-electron wavefunction is approximated by a product of N one-electron wavefunctions (orbitals)) called a Hartree product. This does not mean that the electrons do not sense each other. This approach is called the Hartree Approximation or the Orbital Approximation. The Hartree-Fock self-consistent field method combined with the variational method is used to approximate eigenfunctions and eigenvalues of total energy for the many-electron atom. The variational theorem states that the energy of any approximation is always greater than or equal to the true energy of the system ((what you would obtain if you could solve the Schrödinger equation) for the N-electron atom.
2 -2- Basics of the approach The wavefunctions contain all the information possible. Where do we get intuition from them? First look at the hydrogen atom wavefunctions 1s R 10 (r) = 2 Z a 0 2s R 20(r) = 1 8 2p R 21(r) = s R 30(r) = 3p R 31(r) = 3d R 32(r) = e Zr/a 0 Z a 0 2 Zr Z Zr a 0 a 0 a 0 e Zr/2a 0 e Zr/2a 0 2 Z 18Zr Z 2 r a 0 a 0 4 Z 81 6 a 0 6Zr a 0 Z 2 r 2 a Z Z a 0 2 r 2 a 2 0 e Zr/3a 0 a 2 0 e Zr/3a 0 e Zr/3a 0 Notice how there are some general characteristics:: a factor of Z/a 00 and a decreasing exponential with the same factor, so try this form. ζ where zeta, ζ, is the effective nuclear charge. a 0 e ζr/a 0
3 -3- "...I have tried to base a system on the magnitudes of the atomic weights of the elements. My first attempt in this respect was the following: I chose the smallest atomic weights and arranged them according to the sizes of their atomic weights. This showed that there existed a periodicity in the properties of these simple substances and that even according to their atomicity [valence] the elements followed one another in the arithmetical sequence of their atomic weights." Dimitri Ivanovich Mcndeleyev (Mendeleev), 1869 "The periodicity in the properties of the elements is connected with the continuing build up and completion of the various electron groups that takes place with increasing atomic number." Niels Henrik David Bohr, 1923 (Nobel Prize in Physics in 1922 "for his services in the investigation of the structure of atoms and of the radiation emanating from them".) Multi-Electron Atoms electron spin Dirac spin quantum number, m s magnetic properties diamagnetic paramagnetic unpaired e - ferromagnetic aufbau (filling up) principle Pauli exclusion principle Hund's Rule 1A Atomic Electron Configurations 1 2 H He 1s 1 2A 3A 4A 5A 6A 7A Li 2s 1 Be exceptions to normal filling order B C N O F Ne Na Mg Al Si P S Cl Ar 3s 1 3B 4B 5B 6B 7B B B 2B K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr 4s 1 3d 5 4s 1 3d 10 4s Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te I Xe 5s 1 4d 4 5s 1 4d 5 5s 1 4d 7 5s 1 4d 8 5s 1 4d 10 4d 10 5s Cs Ba La Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn 6s 1 5d 9 6s 1 5d 10 6s Fr Ra Ac Rf Db Sg Bh Hs Mt Ds Rg Cn Fl Fv 7s 1 6d 10 7s Lanthanides Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu 4f 1 d 1 s 2 4f 7 d 1 s 2 4f 14 d 1 s Actinides Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr 6 d 2 7s 2 5f 2 d 1 s 2 5f 3 d 1 s 2 5f 4 d 1 s 2 5f 7 d 1 s 2 5f 14 d 1 s 2 8A
4 - 4 - Aufbau (Building Up) Principle (15.8) EX. 1 For the element Pb a) Give the full electron configuration of its ground state. Hund b) Give the electron configuration of its ground state using the noble gas core. c) Give the orbital diagram of its valence electrons. Pauli d) Predict the more stable ions for Pb. octet in previous level Li Effective Nuclear Charge Shielding and Effective Nuclear Charge, ζ Li: 1s 2 2s charge that the 2s electron experiences when it is closer or further from the nucleus.
5 - 5 - shielding core electrons shield outer electrons from full effect of nuclear charge effective nuclear charge nuclear charge actually experienced by outer electrons due to shielding, decreases with increasing shielding penetration probability of electron being closer to nucleus in spite of shielding; order is s < p < d FIGURE 15.7 Periodic Trends (15.9) Size of Atoms and Ions In H10 homework the average value of r for a hydrogenic atom was given as n 2 a 0 3 Z l(l + 1) 2 2n 2 so its ~ n 2 a 0 /Z. In terms of the effective nuclear charge we have r ~ n 2 a 0 /ζ First Ionization Energies (IE) of the Elements: X(g) > X + (g) + e - IE energy of orbital from which e - came 1st IE removes highest energy e - (least bound); successive IEs higher in energy distinction between core and valence electrons seen in higher IE reveals FIGURE 15.7 shell, subshell structure linearity in IE across a period noble gas configuration noble gases very stable - octet good metals Group I least stable - give up e - to form octet effect of e - repulsions repulsive e - pairing energy
6 - 6 - Electron Affinities (EA) of the Elements X(g) + e - > X - (g) negative values when reaction is exothermic and anion is a more stable species than neutral atom no atom has negative EA for adding a second e - noble gases and most alkaline earths have positive EAs reveals shell, subshell structure noble gas configuration effect of e - repulsions FIGURE 15.7 Electronegativities (EN) of the Elements ability of an atom in a molecule to attract shared electrons to itself combines IE and EA into one property (one way to define) same trend as ionization energy - increases going up a group and left to right across a period EX 2. Arrange the following in order and explain your reasoning: a) Mg 2+, Ar, Br -, Ca 2+ in order of increasing radius b) Na, Na +, O, Ne in order of increasing ionization energy c) H, F, Al, O in order of increasing electronegativity EX 3. The first ionization energy for He is the highest for any element. Which element would have the highest second ionization energy? Explain. EX 4. Why is the electon affinity of Cl more negative than the electron affinity of S?
The Periodic Table. Periodic Properties. Can you explain this graph? Valence Electrons. Valence Electrons. Paramagnetism
Periodic Properties Atomic & Ionic Radius Energy Electron Affinity We want to understand the variations in these properties in terms of electron configurations. The Periodic Table Elements in a column
More informationMade the FIRST periodic table
Made the FIRST periodic table 1869 Mendeleev organized the periodic table based on the similar properties and relativities of certain elements Later, Henri Moseley organized the elements by increasing
More informationנושא מס' 8: המבנה האלקטרוני של אטומים. Electronic Structure of Atoms. 1 Prof. Zvi C. Koren
נושא מס' 8: המבנה האלקטרוני של אטומים Electronic Structure of Atoms 1 Prof. Zvi C. Koren 19.07.10 The Electron Spin From further experiments, it was evident that the e had additional magnetic properties
More informationThe Periodic Table of Elements
The Periodic Table of Elements 8 Uuo Uus Uuh (9) Uup (88) Uuq (89) Uut (8) Uub (8) Rg () 0 Ds (9) 09 Mt (8) 08 Hs (9) 0 h () 0 Sg () 0 Db () 0 Rf () 0 Lr () 88 Ra () 8 Fr () 8 Rn () 8 At (0) 8 Po (09)
More informationPeriodicity & Many-Electron Atoms
Chap. 8 ELECTRON CONFIGURAT N & CEMICAL PERIODICITY 8.1-8.2 Periodicity & Many-Electron Atoms Understand the correlation of electron configuration and the periodic character of atomic properties such as
More informationModified from: Larry Scheffler Lincoln High School IB Chemistry 1-2.1
Modified from: Larry Scheffler Lincoln High School IB Chemistry 1-2.1 The development of the periodic table brought a system of order to what was otherwise an collection of thousands of pieces of information.
More informationWhy all the repeating Why all the repeating Why all the repeating Why all the repeating
Why all the repeating Why all the repeating Why all the repeating Why all the repeating Patterns What Patterns have you observed in your life? Where to Get Help If you don t understand concepts in chapter
More informationThe Periodic Table of the Elements
The Periodic Table of the Elements All matter is composed of elements. All of the elements are composed of atoms. An atom is the smallest part of an element which still retains the properties of that element.
More informationAtoms and the Periodic Table
Atoms and the Periodic Table Parts of the Atom Proton Found in the nucleus Number of protons defines the element Charge +1, mass 1 Parts of the Atom Neutron Found in the nucleus Stabilizes the nucleus
More informationSpeed of light c = m/s. x n e a x d x = 1. 2 n+1 a n π a. He Li Ne Na Ar K Ni 58.
Physical Chemistry II Test Name: KEY CHEM 464 Spring 18 Chapters 7-11 Average = 1. / 16 6 questions worth a total of 16 points Planck's constant h = 6.63 1-34 J s Speed of light c = 3. 1 8 m/s ħ = h π
More information9/20/2017. Elements are Pure Substances that cannot be broken down into simpler substances by chemical change (contain Only One Type of Atom)
CAPTER 6: TE PERIODIC TABLE Elements are Pure Substances that cannot be broken down into simpler substances by chemical change (contain Only One Type of Atom) The Periodic Table (Mendeleev) In 1872, Dmitri
More informationChapter 12 The Atom & Periodic Table- part 2
Chapter 12 The Atom & Periodic Table- part 2 Electrons found outside the nucleus; negatively charged Protons found in the nucleus; positive charge equal in magnitude to the electron s negative charge Neutrons
More informationPERIODIC PROPERTIES Chapter 8
PERIODIC PROPERTIES Chapter 8 "...I have tried to base a system on the magnitudes of the atomic weights of the elements. My first attempt in this respect was the following: I chose the smallest atomic
More informationTopic 3: Periodicity OBJECTIVES FOR TODAY: Fall in love with the Periodic Table, Interpret trends in atomic radii, ionic radii, ionization energies &
Topic 3: Periodicity OBJECTIVES FOR TODAY: Fall in love with the Periodic Table, Interpret trends in atomic radii, ionic radii, ionization energies & electronegativity The Periodic Table What is the periodic
More informationDO NOW: Retrieve your projects. We will be reviewing them again today. Textbook pg 23, answer questions 1-3. Use the section 1.2 to help you.
DO NOW: Retrieve your projects. We will be reviewing them again today. Textbook pg, answer questions. Use the section. to help you. Chapter test is FRIDAY. The Periodic Table of Elements 8 Uuo Uus Uuh
More informationCHEM 130 Exp. 8: Molecular Models
CHEM 130 Exp. 8: Molecular Models In this lab, we will learn and practice predicting molecular structures from molecular formulas. The Periodic Table of the Elements IA 1 H IIA IIIA IVA VA VIA VIIA 3 5
More informationORBITAL DIAGRAM - A graphical representation of the quantum number "map" of electrons around an atom.
160 ORBITAL DIAGRAM - A graphical representation of the quantum number "map" of electrons around an atom. 4p 3d 4s 3p 3s 2p 2s 1s Each blank represents an ORBITAL, and can hold two electrons. The 4s subshell
More informationCHEM 10113, Quiz 5 October 26, 2011
CHEM 10113, Quiz 5 October 26, 2011 Name (please print) All equations must be balanced and show phases for full credit. Significant figures count, show charges as appropriate, and please box your answers!
More informationAdvanced Chemistry. Mrs. Klingaman. Chapter 5: Name:
Advanced Chemistry Mrs. Klingaman Chapter 5: The Periodic Law Name: _ Mods: Chapter 5: The Periodic Law Reading Guide 5.1 History of the Periodic Table (pgs. 125-129) 1) What did Dimitri Mendeleev notice
More informationLast 4 Digits of USC ID:
Chemistry 05 B Practice Exam Dr. Jessica Parr First Letter of last Name PLEASE PRINT YOUR NAME IN BLOCK LETTERS Name: Last 4 Digits of USC ID: Lab TA s Name: Question Points Score Grader 8 2 4 3 9 4 0
More informationSolutions and Ions. Pure Substances
Class #4 Solutions and Ions CHEM 107 L.S. Brown Texas A&M University Pure Substances Pure substance: described completely by a single chemical formula Fixed composition 1 Mixtures Combination of 2 or more
More informationUsing the Periodic Table
MATH SKILLS TRANSPARENCY WORKSHEET Using the Periodic Table 6 Use with Chapter 6, Section 6.2 1. Identify the number of valence electrons in each of the following elements. a. Ne e. O b. K f. Cl c. B g.
More informationORBITAL DIAGRAM - A graphical representation of the quantum number "map" of electrons around an atom.
178 (MAGNETIC) SPIN QUANTUM NUMBER: "spin down" or "spin up" - An ORBITAL (region with fixed "n", "l" and "ml" values) can hold TWO electrons. ORBITAL DIAGRAM - A graphical representation of the quantum
More informationPERIODIC TABLE OF THE ELEMENTS
Useful Constants and equations: K = o C + 273 Avogadro's number = 6.022 x 10 23 d = density = mass/volume R H = 2.178 x 10-18 J c = E = h = hc/ h = 6.626 x 10-34 J s c = 2.998 x 10 8 m/s E n = -R H Z 2
More informationA little history. When and How? Sir William Ramsey. ü 12/5/13. ü 1. Who put together the first useable Periodic Table?
ü // A little history Johahann Dobereiner (80-89) o Triads John Newlands (8-898) o Law of Octaves Who put together the first useable ic Table? Mendeleev you remember him right? When and How? You know it
More informationNucleus. Electron Cloud
Atomic Structure I. Picture of an Atom Nucleus Electron Cloud II. Subatomic particles Particle Symbol Charge Relative Mass (amu) protons p + +1 1.0073 neutrons n 0 1.0087 electrons e - -1 0.00054858 Compare
More informationBROOKLYN COLLEGE Department of Chemistry. Chemistry 1 Second Lecture Exam Nov. 27, Name Page 1 of 5
BROOKLYN COLLEGE Department of Chemistry Chemistry 1 Second Lecture Exam Nov. 27, 2002 Name Page 1 of 5 Circle the name of your lab instructor Kobrak, Zhou, Girotto, Hussey, Du Before you begin the exam,
More informationRadiometric Dating (tap anywhere)
Radiometric Dating (tap anywhere) Protons Neutrons Electrons Elements on the periodic table are STABLE Elements can have radioactive versions of itself called ISOTOPES!! Page 1 in your ESRT has your list!
More informationGuide to the Extended Step-Pyramid Periodic Table
Guide to the Extended Step-Pyramid Periodic Table William B. Jensen Department of Chemistry University of Cincinnati Cincinnati, OH 452201-0172 The extended step-pyramid table recognizes that elements
More informationCHEM 172 EXAMINATION 1. January 15, 2009
CHEM 17 EXAMINATION 1 January 15, 009 Dr. Kimberly M. Broekemeier NAME: Circle lecture time: 9:00 11:00 Constants: c = 3.00 X 10 8 m/s h = 6.63 X 10-34 J x s J = kg x m /s Rydberg Constant = 1.096776 x
More informationAtomic Structure & Interatomic Bonding
Atomic Structure & Interatomic Bonding Chapter Outline Review of Atomic Structure Atomic Bonding Atomic Structure Atoms are the smallest structural units of all solids, liquids & gases. Atom: The smallest
More informationlectures accompanying the book: Solid State Physics: An Introduction, by Philip ofmann (2nd edition 2015, ISBN-10: 3527412824, ISBN-13: 978-3527412822, Wiley-VC Berlin. www.philiphofmann.net 1 Bonds between
More informationLab Day and Time: Instructions. 1. Do not open the exam until you are told to start.
Name: Lab Day and Time: Instructions 1. Do not open the exam until you are told to start. 2. This exam is closed note and closed book. You are not allowed to use any outside material while taking this
More information8. Relax and do well.
CHEM 1314 3;30 pm Theory Exam III John III. Gelder November 13, 2002 Name TA's Name Lab Section INSTRUCTIONS: 1. This examination consists of a total of 8 different pages. The last page include a periodic
More information-"l" also contributes ENERGY. Higher values for "l" mean the electron has higher energy.
170 - Giving the four parameters will uniquely identify an electron around an atom. No two electrons in the same atom can share all four. These parameters are called QUANTUM NUMBERS. PRINCIPAL QUANTUM
More informationCh. 9 NOTES ~ Chemical Bonding NOTE: Vocabulary terms are in boldface and underlined. Supporting details are in italics.
Ch. 9 NOTES ~ Chemical Bonding NOTE: Vocabulary terms are in boldface and underlined. Supporting details are in italics. I. Review: Comparison of ionic and molecular compounds Molecular compounds Ionic
More informationAtomic Emission Spectra. and. Flame Tests. Burlingame High School Chemistry
Atomic Structure Atomic Emission Spectra and Flame Tests Flame Tests Sodium potassium lithium When electrons are excited they bump up to a higher energy level. As they bounce back down they release energy
More information5 questions, 3 points each, 15 points total possible. 26 Fe Cu Ni Co Pd Ag Ru 101.
Physical Chemistry II Lab CHEM 4644 spring 2017 final exam KEY 5 questions, 3 points each, 15 points total possible h = 6.626 10-34 J s c = 3.00 10 8 m/s 1 GHz = 10 9 s -1. B= h 8π 2 I ν= 1 2 π k μ 6 P
More information-"l" also contributes ENERGY. Higher values for "l" mean the electron has higher energy.
175 - Giving the four parameters will uniquely identify an electron around an atom. No two electrons in the same atom can share all four. These parameters are called QUANTUM NUMBERS. PRINCIPAL QUANTUM
More information(C) Pavel Sedach and Prep101 1
(C) Pavel Sedach and Prep101 1 (C) Pavel Sedach and Prep101 1 (C) Pavel Sedach and Prep101 2 (C) Pavel Sedach and Prep101 2 (C) Pavel Sedach and Prep101 3 (C) Pavel Sedach and Prep101 3 (C) Pavel Sedach
More information1 Genesis 1:1. Chapter 10 Matter. Lesson. Genesis 1:1 In the beginning God created the heavens and the earth. (NKJV)
1 Genesis 1:1 Genesis 1:1 In the beginning God created the heavens and the earth. (NKJV) 1 Vocabulary Saturated having all the solute that can be dissolved at that temperature Neutron a particle with no
More informationUnit 1 Part 2 Atomic Structure and The Periodic Table Introduction to the Periodic Table UNIT 1 ATOMIC STRUCTURE AND THE PERIODIC TABLE
UNIT 1 ATOMIC STRUCTURE AND THE PERIODIC TABLE PART 2 INTRODUCTION TO THE PERIODIC TABLE Contents 1. The Structure of the Periodic Table 2. Trends in the Periodic Table Key words: group, period, block,
More information(please print) (1) (18) H IIA IIIA IVA VA VIA VIIA He (2) (13) (14) (15) (16) (17)
CHEM 10113, Quiz 3 September 28, 2011 Name (please print) All equations must be balanced and show phases for full credit. Significant figures count, show charges as appropriate, and please box your answers!
More informationK. 27 Co. 28 Ni. 29 Cu Rb. 46 Pd. 45 Rh. 47 Ag Cs Ir. 78 Pt.
1 IA 1 H Hydrogen 1.01 Atomic number Element symbol Element name Atomic mass VIIIA 1 H 1.01 IIA IIIA IVA VA VIA VIIA 2 He 4.00 Metalloids 3 Li 6.94 4 Be 9.01 5 B 10.81 6 C 12.01 7 N 14.01 8 O 16.00 9 F
More informationIf anything confuses you or is not clear, raise your hand and ask!
CHM 1045 Dr. Light s Section December 10, 2002 FINAL EXAM Name (please print) Recitation Section Meeting Time This exam consists of six pages. Make sure you have one of each. Print your name at the top
More informationSCIENCE 1206 UNIT 2 CHEMISTRY. September 2017 November 2017
SCIENCE 1206 UNIT 2 CHEMISTRY September 2017 November 2017 UNIT OUTLINE 1. Review of Grade 9 Terms & the Periodic Table Bohr diagrams Evidence for chemical reactions Chemical Tests 2. Naming & writing
More informationEssential Chemistry for Biology
1 Chapter 2 Essential Chemistry for Biology Biology and Society: More Precious than Gold A drought is a period of abnormally dry weather that changes the environment and one of the most devastating disasters.
More information02/05/09 Last 4 Digits of USC ID: Dr. Jessica Parr
Chemistry 05 B First Letter of PLEASE PRINT YOUR NAME IN BLOCK LETTERS Exam last Name Name: 02/05/09 Last 4 Digits of USC ID: Dr. Jessica Parr Lab TA s Name: Question Points Score Grader 2 2 9 3 9 4 2
More informationWhat is the periodic table?
The periodic table of the elements represents one of the greatest discoveries in the history of science that certain elements, the basic chemical substances from which all matter is made, resemble each
More informationChemistry 431 Practice Final Exam Fall Hours
Chemistry 431 Practice Final Exam Fall 2018 3 Hours R =8.3144 J mol 1 K 1 R=.0821 L atm mol 1 K 1 R=.08314 L bar mol 1 K 1 k=1.381 10 23 J molecule 1 K 1 h=6.626 10 34 Js N A = 6.022 10 23 molecules mol
More informationSecondary Support Pack. be introduced to some of the different elements within the periodic table;
Secondary Support Pack INTRODUCTION The periodic table of the elements is central to chemistry as we know it today and the study of it is a key part of every student s chemical education. By playing the
More informationChemistry 2 Exam Roane State Academic Festival. Name (print neatly) School
Name (print neatly) School There are fifteen question on this exam. Each question is weighted equally. n the answer sheet, write your name in the space provided and your answers in the blanks provided.
More informationElectron Configuration and Chemical Periodicity. Chapter Eight. AP Chemistry
Electron Configuration and Chemical Periodicity Chapter Eight AP Chemistry General Review Information about the Periodic Table Organization of the Elements 1869: Dmitri Mendeleev - Published an organizational
More informationCHEMISTRY. Chapter 8 The Quantum Mechanical Atom. The Molecular Nature of Matter. Jespersen Brady Hyslop SIXTH EDITION
CHEMISTRY The Molecular Nature of Matter SIXTH EDITION Jespersen Brady Hyslop Chapter 8 The Quantum Mechanical Atom Copyright 2012 by John Wiley & Sons, Inc. The nature of Light Electromagnetic Radiation
More informationLab Day and Time: Instructions. 1. Do not open the exam until you are told to start.
Name: Lab Day and Time: Instructions 1. Do not open the exam until you are told to start. 2. This exam is closed note and closed book. You are not allowed to use any outside material while taking this
More information25 Mn Ni Co Rh Fe Ru Os Uns (262) Une (266) 195.
1 Chem 64 Solutions to Problem Set #1, REVIEW 1. AO n l m 1s 1 0 0 2s 2 0 0 2p 2 1 1,0,1 3d 3 2 2, 1,0,1,2 4d 4 2 2, 1,0,1,2 4f 4 3 3, 2, 1,0,1,2,3 2. Penetration relates to the radial probability distribution
More informationCHEM Come to the PASS workshop with your mock exam complete. During the workshop you can work with other students to review your work.
It is most beneficial to you to write this mock midterm UNDER EXAM CONDITIONS. This means: Complete the midterm in 1.5 hours. Work on your own. Keep your notes and textbook closed. Attempt every question.
More information7. Relax and do well.
CHEM 1215 Exam II John II. Gelder October 7, 1998 Name TA's Name Lab Section INSTRUCTIONS: 1. This examination consists of a total of 5 different pages. The last page includes a periodic table and a solubility
More information8. Relax and do well.
CHEM 1014 Exam I John I. Gelder September 16, 1999 Name TA's Name Lab Section Please sign your name below to give permission to post your course scores on homework, laboratories and exams. If you do not
More informationCLASS TEST GRADE 11. PHYSICAL SCIENCES: CHEMISTRY Test 4: Matter and materials 1
CLASS TEST GRADE PHYSICAL SCIENCES: CHEMISTRY Test 4: Matter and materials MARKS: 45 TIME: hour INSTRUCTIONS AND INFORMATION. Answer ALL the questions. 2. You may use non-programmable calculators. 3. You
More informationHANDOUT SET GENERAL CHEMISTRY II
HANDOUT SET GENERAL CHEMISTRY II Periodic Table of the Elements 1 2 3 4 5 6 7 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 IA VIIIA 1 2 H He 1.00794 IIA IIIA IVA VA VIA VIIA 4.00262 3 Li 6.941 11 Na 22.9898
More informationChem 6 Sample exam 2 (150 points total) NAME:
hem 6 Sample exam 2 (150 points total) @ This is a closed book exam to which the onor Principle applies. @ The last page contains equations and physical constants; you can detach it for easy reference.
More information- Atomic line spectra are UNIQUE to each element. They're like atomic "fingerprints".
- Atomic line spectra are UNIQUE to each element. They're like atomic "fingerprints". - Problem was that the current model of the atom completely failed to explain why atoms emitted these lines. An orbit
More informationK. 27 Co. 28 Ni. 29 Cu Rb. 46 Pd. 45 Rh. 47 Ag Cs Ir. 78 Pt.
1 IA 1 ydrogen 1.01 Atomic number Element symbol Element name Atomic mass VIIIA 1 1.01 IIA IIIA IVA VA VIA VIIA 2 e 4.00 Metalloids 3 Li 6.94 4 Be 9.01 5 B 10.81 6 C 12.01 7 N 14.01 8 O 16.00 9 F 19.00
More informationElement Cube Project (x2)
Element Cube Project (x2) Background: As a class, we will construct a three dimensional periodic table by each student selecting two elements in which you will need to create an element cube. Helpful Links
More informationMarks for each question are as indicated in [] brackets.
Name Student Number CHEMISTRY 140 FINAL EXAM December 10, 2002 Numerical answers must be given with appropriate units and significant figures. Please place all answers in the space provided for the question.
More informationAdvanced Placement. Chemistry. Integrated Rates
Advanced Placement Chemistry Integrated Rates 204 47.90 9.22 78.49 (26) 50.94 92.9 80.95 (262) 52.00 93.94 83.85 (263) 54.938 (98) 86.2 (262) 55.85 0. 90.2 (265) 58.93 02.9 92.2 (266) H Li Na K Rb Cs Fr
More information8. Relax and do well.
CHEM 1215 Exam III John III. Gelder November 11, 1998 Name TA's Name Lab Section INSTRUCTIONS: 1. This examination consists of a total of 7 different pages. The last page includes a periodic table and
More informationPOLYTECHNIC OF NAMIBIA
POLYTECHNIC OF NAMIBIA DEPARTMENT OF HEALTH SCIENCES BACHELOR OF ENVIRONMENTAL HEALTH SCIENCES HEALTH SCIENCE CHEMISTRY (HSC 511S) NQF level 5 SECOND OPPORTUNITY EXAMINATION November 2014 TIME: MARKS:
More informationINSTRUCTIONS: Exam III. November 10, 1999 Lab Section
CHEM 1215 Exam III John III. Gelder November 10, 1999 Name TA's Name Lab Section INSTRUCTIONS: 1. This examination consists of a total of 7 different pages. The last page includes a periodic table and
More information7. Relax and do well.
CHEM 1014 Exam III John III. Gelder November 18, 1999 Name TA's Name Lab Section INSTRUCTIONS: 1. This examination consists of a total of 7 different pages. The last page includes a periodic table and
More informationPart 2. Multiple choice (use answer card). 90 pts. total. 3 pts. each.
1 Exam I CHEM 1303.001 Name (print legibly) Seat no. On my honor, I have neither given nor received unauthorized aid on this exam. Signed Date Part 1. Nomenclature. 10 pts. total. 2 pts. each. Fill in
More informationCHEM 107 (Spring-2005) Exam 3 (100 pts)
CHEM 107 (Spring-2005) Exam 3 (100 pts) Name: ------------------------------------------------------------------------, Clid # ------------------------------ LAST NAME, First (Circle the alphabet segment
More information8. Relax and do well.
CHEM 1314.03 Exam I John I. Gelder September 25, 1997 Name TA's Name Lab Section Please sign your name below to give permission to post, by the last 4 digits of your student I.D. number, your course scores
More information- Light has properties of WAVES such as DIFFRACTION (it bends around small obstructions).
170 LIGHT wavelength Diffraction frequency = wavelengths / time = - Light has properties of WAVES such as DIFFRACTION (it bends around small obstructions). - Einstein noted that viewing light as a particle
More information6.3 Classifying Elements with the Periodic Table
6.3 Classifying Elements with the Periodic Table The Periodic Table was developed by scientists to organize elements in such a way as to make sense of the growing information about their properties. The
More information8. Relax and do well.
CHEM 1225 Exam I John I. Gelder February 4, 1999 Name KEY TA's Name Lab Section Please sign your name below to give permission to post your course scores on homework, laboratories and exams. If you do
More informationCHM 101 PRACTICE TEST 1 Page 1 of 4
CHM 101 PRACTICE TEST 1 Page 1 of 4 Please show calculations (stuffed equations) on all mathematical problems!! On the actual test, "naked answers, with no work shown, will receive no credit even if correct.
More informationChemistry 1 Second Lecture Exam Fall Abbasi Khajo Kruft Levine Mathias Mathias/Ortiz Metlitsky Rahi Sanchez-Delgado Vasserman
Page 1 of 9 Chemistry 1 Second Lecture Exam Fall 2011 Name Circle the name of your recitation/lab instructor(s) Abbasi Khajo Kruft Levine Mathias Mathias/Ortiz Metlitsky Rahi Sanchez-Delgado Vasserman
More informationM10/4/CHEMI/SPM/ENG/TZ2/XX+ CHEMISTRY. Wednesday 12 May 2010 (afternoon) 45 minutes INSTRUCTIONS TO CANDIDATES
M10/4/CHEMI/SPM/ENG/TZ/XX+ 106116 CHEMISTRY standard level Paper 1 Wednesday 1 May 010 (afternoon) 45 minutes INSTRUCTIONS TO CANDIDATES Do not open this examination paper until instructed to do so. Answer
More information(FIRST) IONIZATION ENERGY
181 (FIRST) IONIZATION ENERGY - The amount of energy required to remove a single electron from the outer shell of an atom. - Relates to reactivity for metals. The easier it is to remove an electron, the
More informationInstructions. 1. Do not open the exam until you are told to start.
Name: Lab Day and Time: Instructions 1. Do not open the exam until you are told to start. 2. This exam is closed note and closed book. You are not allowed to use any outside material while taking this
More informationChem Exam 1. September 26, Dr. Susan E. Bates. Name 9:00 OR 10:00
Chem 1711 Exam 1 September 26, 2013 Dr. Susan E. Bates Name 9:00 OR 10:00 N A = 6.022 x 10 23 mol 1 I A II A III B IV B V B VI B VII B VIII I B II B III A IV A V A VI A VII A inert gases 1 H 1.008 3 Li
More informationCHEMICAL COMPOUNDS MOLECULAR COMPOUNDS
48 CHEMICAL COMPOUNDS - Dalton's theory does not mention this, but there is more than one way for atoms to come together to make chemical compounds! - There are TWO common kinds of chemical compound, classified
More informationName Unit 4: Periodic Table Period. Unit 4 Vocabulary.Due Test Day
Name Unit 4: Periodic Table Period 1. History and Language of the Periodic Table 2. Identifying PROPERTIES OF METALS, METALLOIDS, & NONMETALS 3. Identifying GROUP PROPERTIES 4. Classifying elements 5.
More informationCHEM 10123/10125, Exam 2
CHEM 10123/10125, Exam 2 March 7, 2012 (50 minutes) Name (please print) Please box your answers, and remember that significant figures, phases (for chemical equations), and units do count! 1. (13 points)
More information- Some properties of elements can be related to their positions on the periodic table.
179 PERIODIC TRENDS - Some properties of elements can be related to their positions on the periodic table. ATOMIC RADIUS - The distance between the nucleus of the atoms and the outermost shell of the electron
More informationLab Day and Time: Instructions. 1. Do not open the exam until you are told to start.
Name: Lab Day and Time: Instructions 1. Do not open the exam until you are told to start. 2. This exam is closed note and closed book. You are not allowed to use any outside material while taking this
More informationINSTRUCTIONS: 7. Relax and do well.
EM 1314 Name Exam III TA Name John III. Gelder November 16, 1992 Lab Section INSTRUTIONS: 1. This examination consists of a total of 7 different pages. The last page includes a periodic table and some
More informationNAME: FIRST EXAMINATION
1 Chemistry 64 Winter 1994 NAME: FIRST EXAMINATION THIS EXAMINATION IS WORTH 100 POINTS AND CONTAINS 4 (FOUR) QUESTIONS THEY ARE NOT EQUALLY WEIGHTED! YOU SHOULD ATTEMPT ALL QUESTIONS AND ALLOCATE YOUR
More informationChapter 10: Modern Atomic Theory and the Periodic Table. How does atomic structure relate to the periodic table? 10.1 Electromagnetic Radiation
Chapter 10: Modern Atomic Theory and the Periodic Table How does atomic structure relate to the periodic table? 10.1 Electromagnetic Radiation Electromagnetic (EM) radiation is a form of energy that exhibits
More informationChemistry Standard level Paper 1
Chemistry Standard level Paper 1 Thursday 12 May 2016 (morning) 45 minutes Instructions to candidates Do not open this examination paper until instructed to do so. Answer all the questions. For each question,
More information7. Relax and do well.
CHEM 1215 Exam II John II. Gelder October 7, 1998 Name TA's Name Lab Section INSTRUCTIONS: 1. This examination consists of a total of 5 different pages. The last page includes a periodic table and a solubility
More informationLab Day and Time: Instructions. 1. Do not open the exam until you are told to start.
Name: Lab Day and Time: Instructions 1. Do not open the exam until you are told to start. 2. This exam is closed note and closed book. You are not allowed to use any outside material while taking this
More information610B Final Exam Cover Page
1 st Letter of Last Name NAME: 610B Final Exam Cover Page No notes or calculators of any sort allowed. You have 3 hours to complete the exam. CHEM 610B, 50995 Final Exam Fall 2003 Instructor: Dr. Brian
More informationHANDOUT SET GENERAL CHEMISTRY I
HANDOUT SET GENERAL CHEMISTRY I Periodic Table of the Elements 1 2 3 4 5 6 7 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 IA VIIIA 1 2 H He 1.00794 IIA IIIA IVA VA VIA VIIA 4.00262 3 Li 6.941 11 Na 22.9898
More informationLab Day and Time: Instructions. 1. Do not open the exam until you are told to start.
Name: Lab Day and Time: Instructions 1. Do not open the exam until you are told to start. 2. This exam is closed note and closed book. You are not allowed to use any outside material while taking this
More informationCHEM 167 FINAL EXAM MONDAY, MAY 2 9:45 11:45 A.M GILMAN HALL
PROF. JOHN VERKADE SPRING 2005 THIS EXAM CONSISTS OF 12 QUESTIONS ON 9 PAGES CHEM 167 HOUR EXAM IV APRIL 20, 2005 SEAT NO. NAME RECIT. INSTR. RECIT. SECT. GRADING PAGE Page 2 Page 3 Page 4 Page 5 Page
More informationFall 2011 CHEM Test 4, Form A
Fall 2011 CHEM 1110.40413 Test 4, Form A Part I. Multiple Choice: Clearly circle the best answer. (60 pts) Name: 1. The common constituent in all acid solutions is A) H 2 SO 4 B) H 2 C) H + D) OH 2. Which
More informationK. 27 Co. 28 Ni. 29 Cu Rb. 46 Pd. 45 Rh. 47 Ag Cs Ir. 78 Pt.
1 IA 1 ydrogen 1.01 Atomic number Element symbol Element name Atomic mass VIIIA 1 1.01 IIA IIIA IVA VA VIA VIIA 2 e 4.00 Metalloids 3 Li 6.94 4 Be 9.01 5 B 10.81 6 C 12.01 7 N 14.01 8 O 16.00 9 F 19.00
More information