Chemistry 40S Atomic Structure (This unit has been adapted from
|
|
- Ethelbert Gardner
- 5 years ago
- Views:
Transcription
1 Chemistry 40S Atomic Structure (This unit has been adapted from Name: 1
2 Lesson 1: The Nature of Light Goals: Describe light in terms of electromagnetic energy. Describe the electromagnetic spectrum. Describe the relationship between frequency, wavelength and energy of light. Identify an element based on its flame test. Describe line and continuous spectra. Wavelength Frequency 2
3 What relationship do you notice between wavelength and frequency? Frequency, Wavelength, Energy, and Electromagnetic Spectrum Max Planck If we shine sunlight through a prism we get a rainbow of colours, known as a spectrum. Each colour in the rainbow represents light of a different frequency or wavelength. 3
4 The visible spectrum is actually a very small portion of the entire electromagnetic spectrum. Line Spectra 4
5 Element Colour Practice: The Nature of Light 1. Put the following in order of increasing energy: green light, x-rays, radio, red light, ultraviolet, microwaves, blue light, gamma rays. 2. Describe the relationship between frequency, wavelength and energy. 5
6 3. Why is light called electromagnetic radiation? 4. Compare and contrast line and continuous spectra. 5. Give the colour for the flame test of each of the following: a) Copper b) Strontium c) Lithium d) Potassium e) Barium f) Calcium g) Sodium 6
7 Lesson 2: The Quantum Mechanical Model of the Atom Goals: Explain the development of the Quantum Mechanical Model of the atom. Explain the formation of line spectra. The Model of the Atom John Dalton: Joseph John Thompson: 7
8 Earnest Rutherford Explanation of Line Spectra Neil Bohr 8
9 Quantum Theory Albert Einstein Louis de Broglie 9
10 The Quantum Mechanical Model of the Atom Werner Heisenberg Erwin Schrödinger 10
11 Orbitals s-orbitals p-orbitals 11
12 d-orbitals 12
13 Practice: The Quantum Mechanical Model of the Atom 1. Identify the contribution made by each of the following to atomic theory. a) Rutherford b) Heisenberg c) Planck d) Bohr e) de Broglie f) Schrödinger 2. Describe s, p and d-orbitals. What do they represent? How are they different from each other? 13
14 Lesson 3: Electron Configurations Goals: Write the electron configuration of atoms and ions. Write the valence electron configuration of and atom or ion. The Orbitals Principle Quantum Number: Main Energy Level (n) Number of Orbitals (n 2 ) Type of Orbitals The Pauli Exclusion Principle Wolfgang Pauli 14
15 Principle Quantum Number: Main Energy Level (n) Number of Orbitals (n 2 ) Type of Orbitals Number of Electrons (2n 2 ) The Electron Configuration 15
16 Aufbau Principle 16
17 Hund s Rule Friedich Hund Element Filling of Orbitals Electron Configuration 1s 2s 2px 2py 2pz 17
18 Zig-Zag Rule 7s 7p 6s 6p 6d 5s 5p 5d 5f 4s 4p 4d 4f 3s 3p 3d 2s 2p 1s Example 1: Write the complete electron configuration for magnesium. Use the Zig-Zag Rule to assist you. Example 2: Write the complete electron configuration for germanium. Use the Zig-Zag Rule to assist you. 18
19 Exceptions to the Rules 19
20 Electron Configurations of Ions Example 3: Write the complete electron configuration for the chloride ion, Cl -. Example 4: Write the complete electron configuration for the calcium ion, Ca
21 Example 5: Write the complete electron configuration for the iron (II) ion, Fe 2+. Example 6: Write the complete electron configuration for the iron (III) ion, Fe
22 Valance Configurations Example 7: Write the valence electron configuration for fluorine. Example 8: Write the valence electron configuration for germanium. 22
23 Practice: Electron Configurations 1. How many electrons in an atom can have the designation? a) 1s b) 2p c) 3px d) 6f e) 3dxy f) n = 2 g) 4p h) n = 5 2. Write complete electronic configurations for the following atoms and ions: a) P b) Ca c) Cu d) Rh e) Sb 3+ f) Ni 2+ g) Fe 2+ h) Ni 4+ i) Zn 2+ j) Br k) Sn 2+ l) Co 3+ 23
24 3. How many unpaired electrons are there in each of the following: a) Mn b) As c) Sr d) Tl + e) Cu 2+ f) V 3+ g) Sn h) Lu 4. Write the electronic configurations for the valence electrons of each of the following: a) Mg b) P c) Se d) Pb 2+ e) Br f) S 2- g) Ni h) Ag + i) N 3- j) Fe 3+ 24
25 Lesson 4: Electronegativity Goals: Use electronegativity values to predict the type of bond between two atoms. Describe a bond in terms of polar covalent, non-polar covalent and ionic. Electronegativity 25
26 Polar, Non-Polar, and Ionic Bonds Electronegativity Difference Character of Bond Percent Ionic Character Example 1: What type of bond forms between sodium and chlorine in NaCl? Example 2: What type of bond forms between sulphur and oxygen in SO3? 26
27 Example 3: What type of bond forms between aluminum and chlorine in AlCl3? Practice: Electronegativity Answer the following questions. Refer to the Electronegativity Table when needed. 1. Describe the trend of electronegativity on the periodic table. 2. Describe each of the following in terms of electronegativity. a) non-polar covalent bond b) polar covalent bond c) ionic bond 27
28 3. Describe the following as non-polar covalent, polar covalent, or ionic. a) N and H b) F and F c) Ca and O d) Al and Br e) H and I f) K and Cl 4. List the following in increasing ionic character. a) Mg-F, Ca-I, Ca-Cl, Mg-Cl b) Al-Cl, H-Cl, K-Cl, Cu-Cl c) C-O, C-H, C-F, C-Br d) S-Cl, H-C, H-F, H-H, H-Cl, H-O 28
29 Lesson 5: Lewis Dot Structure Goals: Draw dot diagrams for covalent compounds. Dot Structures for Atoms and Octet Rule Gilbert Lewis 29
30 Drawing Lewis Dot Structure Example 1: Draw the Lewis Dot structure for HF. 30
31 Example 2: Draw the Lewis structure for CO2. Example 3: Draw the Lewis structure for the sulphate ion, SO
32 Practice: Lewis Dot Structure 1. Draw the Lewis structure for each of the following. a) NH3 b) SO3 c) BrF d) O2 e) PO4 3 f) CH4 g) HCN h) N2 i) Cl2O j) ClO3 - k) CO3 2- l) SiF4 32
33 Lesson 6: Ionization Energy and Periodic Trends Goals: Describe the factors that affect the force on an electron. Explain the trends in atomic radius, ionic radius and ionization energy. A Force on an Electron Atomic Radii 33
34 Atomic Radii (pm) of Group 1 Atom Ionic Radii 34
35 Periodic Trends and Ionization Energy 35
36 36
37 Practice: Ionization Energy and Periodic Trends 1. Briefly explain why barium has a lower first ionization energy than calcium. 2. Given the following elements and their electron configuration. Which element will have the lowest first ionization energy? Why? Element A 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 Element B 1s 2 2s 2 2p 6 3s 2 3p 5 Element C 1s 2 2s 2 2p 6 3s 2 3p 6 4s 1 Element D 1s 2 2s 2 2p 6 3s 2 3p 6 37
38 3. The first four ionization energies (IE) for the element aluminum are as follows: IE1 = 577 kj/mol IE2 = kj/mol IE3 = kj/mol IE4 = kj/mol How many valence electrons does aluminum have? 4. An atom has the following successive ionization energy levels. IE1 = 737 kj/mol IE2 = kj/mol IE3 = kj/mol IE4 = kj/mol IE5 = kj/mol How many valence electrons does this element have? Explain. 5. Which of these elements would have the highest value for the second ionization energy? Why? K Si Ar Br 38
39 6. Which of the following has the largest atomic radius and which has the smallest? Explain. Nitrogen Antimony Arsenic 7. For each of the following properties: atomic radius first ionization energy ionic radius Indicate which has the larger value fluorine or bromine. 8. Arrange the following from largest to smallest. Explain the order. Ne, Mg 2+, F -, Na +, O 2-39
40 40
Chemistry 40S Atomic Structure (This unit has been adapted from https://bblearn.merlin.mb.ca)
Chemistry 40S Atomic Structure (This unit has been adapted from https://bblearn.merlin.mb.ca) Name: 1 2 Lesson 1: The Nature of Light Goals: Describe light in terms of electromagnetic energy. Describe
More informationChemistry 40S Atomic Structure (This unit has been adapted from
Chemistry 40S Atomic Structure (This unit has been adapted from https://bblearn.merlin.mb.ca) Name: 1 2 Lesson 1: The Nature of Light Goals: Describe light in terms of electromagnetic energy. Describe
More informationDiscovered the electron
Aubrey High School AP Chemistry 8 Atomic Theory Name Period Date / / 8.0 Prep Problems History of the Atom 1. Describe the contributions of the following scientists and their research to the theory of
More informationClassify each of these statements as always true, AT; sometimes true, ST; or never true, NT.
ELECTRONS IN ATOMS Chapter Quiz Classify each of these statements as always true, AT; sometimes true, ST; or never true, NT. 1. The orbitals of a principal energy level are lower in energy than the orbitals
More informationCDO AP Chemistry Unit 5
1. a. Calculate the wavelength of electromagnetic radiation that has a frequency of 5.56 MHz. b. Calculate the frequency of electromagnetic radiation that has a wavelength equal to 667 nm. 2. Electromagnetic
More informationCHM 1045 Test #4 December 4, 2000
CHM 1045 Test #4 December 4, 2000 1. The scientist who was first to propose that electrons in an atom could have only certain energies was a. Planck. b. Einstein. c. Bohr. d. Rydberg. 2. Select the arrangement
More informationHonors Chemistry: Chapter 4- Problem Set (with some 6)
Honors Chemistry: Chapter 4- Problem Set (with some 6) All answers and work on a separate sheet of paper! Classify the following as always true (AT), sometimes true (ST), or never true (NT) 1. Atoms of
More informationName: Electrons in Atoms Chemical Periodicity Chapters 13 and 14
Name: Electrons in Atoms Chemical Periodicity Chapters 13 and 14 1 Chapter 13 Electrons in Atoms We need to further develop our understanding of atomic structure to help us understand how atoms bond to
More information5. The outermost principal energy level electron configuration of the element bromine is: a. 4s 2 c. 4s 2 4p 5 b. 4p 5 d.
1 c E = h 1. Sodium and potassium have similar properties because they have the same a. atomic radii. c. number of valence electrons. b. ionization energy. d. electronegativity. 2. Electrons must be added
More information1. What is the phenomenon that occurs when certain metals emit electrons when illuminated by particular wavelengths of light? a.
CHEMISTRY 123-07 Midterm #3 solution key December 02, 2010 Statistics: Average: 77 p (77%); Highest: 100 p (100%); Lowest: 33 p (33%) Number of students performing at or above average: 54 (52%) Number
More informationCHEMISTRY Midterm #3 November 27, 2007
Name: The total number of points in this exam is 100. CHEMISTRY 123-01 Midterm #3 November 27, 2007 PART I: MULTIPLE CHOICE (Each multiple choice question has a 2-point value). Mass of electron = 9.11
More informationElectronic configurations, Auf-bau principle, Pauli principle, Hunds rule 1. Which of the following statements in relation to the hydrogen atom is correct? 1) 3s and 3p orbitals are of lower energy than
More informationAtoms, Electrons and Light MS. MOORE CHEMISTRY
Atoms, Electrons and Light MS. MOORE CHEMISTRY Atoms Remember Rutherford??? What did he discover with his gold foil experiment. A: Atoms contain a dense nucleus where the protons and neutrons reside. ATOMS
More informationChapter 4 The Structure of the Atom
Chapter 4 The Structure of the Atom Read pg. 86-97 4.1 Early Theories of Matter The Philosophers Democritus Artistotle - Artistotle s influence so great and the science so primitive (lacking!) his denial
More informationElectrons in Atoms. So why does potassium explode in water? Quantum Mechanics Periodic Trends Chemical Bonding
Electrons in Atoms So why does potassium explode in water? Quantum Mechanics Periodic Trends Chemical Bonding 12.1 Development of Atomic Models Dalton s Thompson s Rutherford s Bohr s carbon Quantum Model
More informationPart I: It s Just a Trend
Part I: It s Just a Trend 1. What is the trend with the atomic numbers of the elements as you move from left to right across a period on the Periodic Table? How does this sequence continue to the next
More informationHonors Unit 6 Atomic Structure
Honors Unit 6 Atomic Structure Miss Adams Honors Chemistry 1 Name: 1 Homework #1: Frequency, Wavelength and the Speed of Light Show all of your work for the problems, including the initial formula, substitution
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 information1) What type of relationship (direct or indirect) exists between wavelength, frequency, and photon energy?
Chapter 7 Study Guide Name: AP Chemistry 6 points DUE AT TEST (Mon., 11/20/17) Date: Topics/people to be covered on the test: wavelength frequency c=ëí ideas of Max Planck E=hí quanta photons relationship
More informationA. 24 B. 27 C. 30 D. 32 E. 33. A. It is impossible to tell from the information given. B. 294 mm C. 122 mm D. 10 mm E. 60 mm A. 1 H B. C. D. 19 F " E.
CHEMISTRY 110 EXAM 1 Sept. 24, 2012 FORM A 1. A microwave oven uses 2.45! 10 9 Hz electromagnetic waves to heat food. What is the wavelength of this radiation in mm? A. It is impossible to tell from the
More information#9 Modern Atomic Theory Quantitative Chemistry
Name #9 Modern Atomic Theory Quantitative Chemistry Student Learning Map Unit EQ: What is the current model of the atom? Key Learning: The current model of the atom is based on the quantum mechanical model.
More information14. Use reactions 1 and 2 to determine the value of H (in kj) for reaction 3.
11. A 2.85 g sample of a food substance was burned in a calorimeter that had a heat capacity of 9.84 kj/ C. The temperature of the calorimeter increased from 22.51 C to 35.66 C. Calculate the amount of
More information1. The elements on the Periodic Table are arranged in order of increasing A atomic mass C molar mass
1. The elements on the Periodic Table are arranged in order of increasing A atomic mass C molar mass A Br, Ga, Hg C O, S, Se B atomic number D oxidation number 2. Which list includes elements with the
More informationDuncan. Electrons, Energy, & the Electromagnetic Spectrum Notes Simplified, 2-D Bohr Model: Figure 1. Figure 2. Figure 3
Electrons, Energy, & the Electromagnetic Spectrum Notes Simplified, 2-D Bohr Model: Figure 1 Figure 2 Figure 3 Light Calculation Notes Here s how the type/form of EM radiation can be determined The amount
More information5) Which statement correctly describes the relationship of wavelength and frequency in a wave?
Exam 2 Name: Multiple Choice (2 pts each) 1) Which of the following bonds is the most polar? a) C O b) N O c) O O d) Si O 2) The maximum electron capacity of an f sublevel is a) 7 c) 14 b) 6 d) 10 3) Which
More information1. Electronic Structure 2. Electron Configuration 3. Core Notation 4. EC Relationship to Periodic Table 5. Electron Configuration of Ions
Pre-AP Chemistry 11 Atomic Theory II Name: Date: Block: 1. Electronic Structure 2. Electron Configuration 3. Core Notation 4. EC Relationship to Periodic Table 5. Electron Configuration of Ions Electronic
More informationWorksheet 5 - Chemical Bonding
Worksheet 5 - Chemical Bonding The concept of electron configurations allowed chemists to explain why chemical molecules are formed from the elements. In 1916 the American chemist Gilbert Lewis proposed
More informationAE Chemistry Midterm Study Guide
Name Date Define Chemistry AE Chemistry Midterm Study Guide Since chemistry studies matter what is the definition of matter. What is the Law of Conservation of Matter? What is energy, what are the two
More informationChemistry 1411 Practice Exam 2, Chapters 5-8 Brown
Chemistry 1411 Practice Exam 2, Chapters 5-8 Brown Some constants and equations: E = q + w q = C p T Heat = m T Cs h = 6.626 X 10 34 J. s c = 2.998 X 10 8 m/s R H = 2.18 X 10 18 J E = (2.18 X 10 18 J)(1/n
More informationKey Equations. Determining the smallest change in an atom's energy.
ATOMIC STRUCTURE AND PERIODICITY Matter and Energy Key Equations λν = c ΔE = hν Relating speed of a wave to its wavelength and frequency. Determining the smallest change in an atom's energy. H( λ =R n
More informationCHEMISTRY 110 EXAM 1 SEPTEMBER 20, 2010 FORM A
CHEMISTRY 110 EXAM 1 SEPTEMBER 20, 2010 FORM A 1. What are the correct numbers of protons, neutrons and electrons in a 39 K + ion? p n e A. 20 19 18 B. 20 19 19 C. 19 20 18 D. 19 20 19 E. 20 19 20 2. Which
More informationName Date Period Unit 3 Review: Electrons and the periodic table
Name Date Period Unit 3 Review: Electrons and the periodic table G Chem; Coleman SHOW YOUR WORK ON ANY AND ALL CALCULATIONS. SIG FIGS MATTER. UNITS MATTER. General Questions: 1. Use the following terms
More informationSCH4U1 Atomic & Molecular Structure Test Review
SCH4U1 Atomic & Molecular Structure Test Review 1. Which object(s) would you use to describe the shape of the 2p orbital? a. a dumb-bell b. a circle c. a sphere d. two perpendicular dumb-bells e. a doughnut
More information1. The elements on the Periodic Table are arranged in order of increasing A atomic mass C molar mass
1. The elements on the Periodic Table are arranged in order of increasing A atomic mass C molar mass A Br, Ga, Hg C O, S, Se B atomic number D oxidation number 2. Which list includes elements with the
More informationThe orbitals in an atom are arranged in shells and subshells. orbital 3s 3p 3d. Shell: all orbitals with the same value of n.
Shells and Subshells The orbitals in an atom are arranged in shells and subshells. n=3 orbital 3s 3p 3d Shell: all orbitals with the same value of n n=3 3s 3p 3d Subshell: all orbitals with the same value
More informationReview Package #3 Atomic Models and Subatomic Particles The Periodic Table Chemical Bonding
Chemistry 11 Review Package #3 Atomic Models and Subatomic Particles The Periodic Table Chemical Bonding 1. Atomic Models and Subatomic Particles: A. Subatomic Particles and Average Atomic Mass: - Subatomic
More informationAtomic Structure and Periodicity
Atomic Structure and Periodicity Atoms and isotopes: Isotopes-#p + same for all but mass number is different b/c of # n o Average atomic mass is weighted average of all the isotopes for an element Average
More informationRegan & Johnston Chemistry Unit 3 Exam: The Periodic Table Class Period
Regan & Johnston Name Chemistry Unit 3 Exam: The Periodic Table Class Period 1. An atom of which element has the largest atomic radius? (1) Si (2) Fe (3) Zn (4) Mg 2. Which characteristics both generally
More informationHonors Chemistry - Unit 4 Bonding Part I
Honors Chemistry - Unit 4 Bonding Part I Unit 4 Packet - Page 1 of 8 Vocab Due: Quiz Date(s): Test Date: UT Quest Due: Bonding Vocabulary: see separate handout assignment OBJECTIVES: Chapters 4-8 Be able
More informationUnit Five Practice Test (Part I) PT C U5 P1
Unit Five Practice Test (Part I) PT C U5 P1 Name Period LPS Standard(s): --- State Standard(s): 12.3.1 Short Answers. Answer the following questions. (5 points each) 1. Write the electron configuration
More informationHSVD Ms. Chang Page 1
Name: Chemistry, PERIODIC TABLE 1. A solid element that is malleable, a good conductor of electricity, and reacts with oxygen is classified as a (1) noble gas (2) metalloid (3) metal (4) nonmetal 2. Which
More informationPeriod: Chemistry Semester 1 Final Exam Review Packet. 1. What is the difference between a hypothesis and a theory?
Chemistry Name: Period: Chemistry Semester 1 Final Exam Review Packet 1. What is the difference between a hypothesis and a theory? 2. Distinguish between quantitative and qualitative observations. States
More informationName Chemistry-PAP Period. Notes: Electrons. Light travels through space as a wave. Waves have three primary characteristics:
Name Chemistry-PAP Period The Wave Nature of Light Notes: Electrons Light travels through space as a wave. Waves have three primary characteristics: Wavelength (λ): the distance between 2 consecutive crests
More informationTest Topics: Periodic Table, Atomic Theory, Physical/Chemical Properties, Atom, Isotopes, Average Atomic Mass
Elemental Properties Review Worksheet Test Topics: Periodic Table, Atomic Theory, Physical/Chemical Properties, Atom, Isotopes, Average Atomic Mass Periodic Table 1. List the element symbols for the following
More informationTrends in the Periodic Table
Trends in the Periodic Table Effective nuclear charge: < effective nuclear charge is the attraction felt by the valence electrons from the nucleus < increases across a period : increases across because
More informationEM SPECTRUM, WAVELENGTH, FREQUENCY, AND ENERGY WORKSHEET
EM SPECTRUM, WAVELENGTH, FREQUENCY, AND ENERGY WORKSHEET 1.) Look at the EM spectrum below to answer this question. As you move across the visible light spectrum from red to violet (A) Does the wavelength
More informationUnit 1 Atomic Theory
Unit 1 Atomic Theory 1.0 You are expected to be already familiar with. Ionic nomenclature (binary, polyatomic, multivalency) Covalent nomenclature Writing chemical formulas for ionic and covalent compounds
More informationChapter 9: Electrons and the Periodic Table
C h e m i s t r y 1 2 C h 9 : E l e c t r o n s a n d P e r i o d i c T a b l e P a g e 1 Chapter 9: Electrons and the Periodic Table Work on MasteringChemistry assignments What we have learned: Dalton
More informationCHEMISTRY 113 EXAM 3(A)
Summer 2003 CHEMISTRY 113 EXAM 3(A) 1. Specify radiation with the greatest energy from the following list: A. ultraviolet B. gamma C. infrared D. radio waves 2. The photoelectric effect is: A. reflection
More informationATOMIC THEORY, PERIODICITY, and NUCLEAR CHEMISTRY
ATOMIC THEORY, PERIODICITY, and NUCLEAR CHEMISTRY Note: For all questions referring to solutions, assume that the solvent is water unless otherwise stated. 1. The nuclide is radioactive and decays by the
More informationUnit 3: The Periodic Table and Atomic Theory
Name: Period: Unit 3: The Periodic Table and Atomic Theory Day Page # Description IC/HW 1 2-3 Periodic Table and Quantum Model Notes IC 1 4-5 Orbital Diagrams Notes IC 1 14 3-A: Orbital Diagrams Worksheet
More informationWhat is the energy of a photon with wavelength 232 nm?
EMISTRY 110 EXAM 1 February 6, 2012 FRM A 1 ow many single covalent bonds must a sulfur atom form to have a complete octet in its valence shell? A. 3 B. 4. 1 D. 2 E. 0 2. What are the correct numbers of
More informationChapter 2 Atoms and the Periodic Table
Chapter 2 1 Chapter 2 Atoms and the Periodic Table Solutions to In-Chapter Problems 2.1 Each element is identified by a one- or two-letter symbol. Use the periodic table to find the symbol for each element.
More informationName: SCH3U Worksheet-Trends
PERIODIC TRENDS WORKSHEET 1. Choose which statement about the alkali metals lithium and cesium is correct. a) as the atomic number increases, the Electronegativity of the elements increases b) as the atomic
More informationUnit 3 Periodic Table and Quantum HW Packet Name Date. Periodic Table Concepts. 1. In what family are the most active metals located?
Directions: Answer the following questions. Periodic Table Concepts 1. In what family are the most active metals located? 2. In what family are the most active non-metals located? 3. What family on the
More information6.1.5 Define frequency and know the common units of frequency.
CHM 111 Chapter 6 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 corresponding
More informationElectron Configurations
Section 3 Electron Configurations Key Terms electron configuration Pauli exclusion principle noble gas Aufbau principle Hund s rule noble-gas configuration Main Ideas Electrons fill in the lowest-energy
More informationUnit 2 ~ Learning Guide Name:
Unit 2 ~ Learning Guide Name: Instructions: Using a pencil, complete the following notes as you work through the related lessons. Show ALL work as is explained in the lessons. You are required to have
More informationA) I and III B) I and IV C) II and IV D) II and III E) III 5. Which of the following statements concerning quantum mechanics is/are true?
PX0311-0709 1. What is the wavelength of a photon having a frequency of 4.50 10 14 Hz? (, ) A) 667 nm B) 1.50 10 3 nm C) 4.42 10 31 nm D) 0.0895 nm E) 2.98 10 10 nm 2. When a particular metal is illuminated
More informationElectronic Structure and Bonding Review
Name: Band: Date: Electronic Structure and Bonding Review 1. For electrons: a. What is the relative charge? b. What is the relative mass? c. What is the symbol? d. Where are they located in the modern
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 informationPeriodic Table Workbook
Key Ideas: The placement or location of elements on the Periodic Table gives an indication of physical and chemical properties of that element. The elements on the Periodic Table are arranged in order
More informationActivity # 2. Name. Date due. Assignment on Atomic Structure
Activity # 2 10 Name Date Date due Assignment on Atomic Structure NOTE: This assignment is based on material on the Power Point called Atomic Structure, as well as pages 167-173 in the Science Probe textbook.
More information2008 Brooks/Cole 2. Frequency (Hz)
Electromagnetic Radiation and Matter Oscillating electric and magnetic fields. Magnetic field Electric field Chapter 7: Electron Configurations and the Periodic Table Traveling wave moves through space
More informationName Date Class MODELS OF THE ATOM
5.1 MODELS OF THE ATOM Section Review Objectives Identify inadequacies in the Rutherford atomic model Identify the new assumption in the Bohr model of the atom Describe the energies and positions of electrons
More information1. Ham radio operators often broadcast on the 6 meter band. The frequency of this electromagnetic radiation is MHz. a. 500 b. 200 c. 50 d. 20 e. 2.
Name: Score: 0 / 60 points (0%) [1 open ended question not graded] Chapters 6&7 Practice Exam Multiple Choice Identify the choice that best completes the statement or answers the question. 1. Ham radio
More information! Chemical!Bond!! Lewis!Diagram!(HI!#13)! o Ionic!and!covalent!bond!(M!+!NM!or!NM!+!NM)!(Complete!transfer!of!e S!or!sharing!of!e S )!
!! Unit*2.*Atomic*Theory*! Molar!mass!calculation!using!the!abundance!of!isotopes!of!an!element!!!! Electron!configuration!(both!full!notation!and!core!notation)!(HI!#12)! o Neutral!atom,!anion,!cation!(ensure!you!know!the!rules!associated!with!ions)!
More informationThe Periodic Table & Formation of Ions
The Periodic Table & Formation of Ions Development of the Periodic Table Mendeleev: Considered to be the father of the periodic table Arranged elements by increasing atomic mass Placed elements with similar
More informationRegan & Johnston Chemistry Unit 3 Exam: The Periodic Table Class Period
Regan & Johnston Name Chemistry Unit 3 Exam: The Periodic Table Class Period 1. An atom of which element has the largest atomic radius? (1) Si (2) Fe (3) Zn (4) Mg 2. Which characteristics both generally
More informationElectrons and Periodic Table (Ch. 4 & 5) OTHS Academic Chemistry
Name Objectives: Per. Electrons and Periodic Table (Ch. 4 & 5) OTHS Academic Chemistry Express the arrangement of electrons in atoms through electron configurations Understand the electromagnetic spectrum
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 informationTest Bank for General Chemistry Atoms First 2nd Edition by John E. McMurry and Robert C. Fay
Test Bank for General Chemistry Atoms First 2nd Edition by John E. McMurry and Robert C. Fay Link download full: https://digitalcontentmarket.org/download/test-bank-for-general-chemistry-atoms-f irst-2nd-edition-by-mcmurry-and-fay/
More informationCDO CP Chemistry Unit 5
1. Of the three particles; protons, neutrons, and electrons, which one(s) are responsible for most of the mass of an atom? a) the protons only b) the electrons only c) the neutrons only d) the protons
More informationNotes: Electrons and Periodic Table (text Ch. 4 & 5)
Name Per. Notes: Electrons and Periodic Table (text Ch. 4 & 5) NOTE: This set of class notes is not complete. We will be filling in information in class. If you are absent, it is your responsibility to
More informationName: 1. The mass of a proton is approximately equal to the mass of (1) an alpha particle (2) a beta particle (3) a positron (4) a neutron
Chemistry Section Name: MID TERM STUDY GUIDE Date: A. Multiple Choice. 1. The mass of a proton is approximately equal to the mass of (1) an alpha particle (2) a beta particle (3) a positron (4) a neutron
More informationArrangement of Electrons. Chapter 4
Arrangement of Electrons Chapter 4 Properties of Light -Light s interaction with matter helps to understand how electrons behave in atoms -Light travels through space & is a form of electromagnetic radiation
More informationPractice Packet Unit: 5 Periodic Table
Regents Chemistry: Practice Packet Unit: 5 Periodic Table 1 VOCABULARY For each word, provide a short but specific definition from YOUR OWN BRAIN! No boring textbook definitions. Write something to help
More informationSlide 1 / Put the following elements in order of increasing atomic size: P, Cs, Sn, F, Sr, Tl
Slide 1 / 54 1 Put the following elements in order of increasing atomic size: P, Cs, Sn, F, Sr, Tl Slide 2 / 54 2 Put the following elements in order of increasing atomic size: Ca, Rb, K, O, Al, As Slide
More information3.1 Hydrogen Spectrum
3.1 Hydrogen Spectrum Light is electromagnetic radiation that can be produced at different energy levels. High energy light has a short wavelength (λ) and a high frequency (ƒ, ν) (gamma rays, x-rays, ultraviolet).
More informationAP Chemistry Summer Assignment
Name AP Chemistry Summer Assignment Welcome to AP chemistry! This summer assignment is intended to help you review the basic topics you learned in pre-ap chemistry that are crucial for your success in
More informationCHEMISTRY 102 Fall 2014 HOUR EXAM I Page 1
OUR EXAM I Page 1 1. Draw the Lewis structure for ICl5. ow many of the following four statements (I-IV) is/are true regarding ICl5? I. The central atom in ICl5 has one lone pair of electrons. II. Some
More information2 e. 14 e. # e # orbitals. 10 e 5. sublevel. shape of orbital. Orbital Shapes. Notes Orbital Notation; e Config; NGN.
How to build an atom: The bigger (more massive) the atom, the more protons (and neutrons) The bigger the atom, the more electrons Electrons fill lower energy levels first "Aufbau" Principle ("To build
More informationTest Review # 5. Chemistry: Form TR5-8A. Average Atomic Mass. Subatomic particles.
Chemistry: Form TR5-8A REVIEW Name Date Period Test Review # 5 Subatomic particles. Type of Particle Location Mass Relative Mass Charge Proton Center 1.67 10-27 kg 1 +1 Electron Outside 9.11 10-31 kg 0-1
More information7. How many unpaired electrons are there in an atom of tin in its ground state? 2
Name period AP chemistry Unit 2 worksheet 1. List in order of increasing energy: 4f, 6s, 3d,1s,2p 1s, 2p, 6s, 4f 2. Explain why the effective nuclear charge experienced by a 2s electron in boron is greater
More information2. Which of the following salts form coloured solutions when dissolved in water? I. Atomic radius II. Melting point III.
1. Which pair of elements reacts most readily? A. Li + Br 2 B. Li + Cl 2 C. K + Br 2 D. K + Cl 2 2. Which of the following salts form coloured solutions when dissolved in water? I. ScCl 3 II. FeCl 3 III.
More informationAll chemical bonding is based on the following relationships of electrostatics: 2. Each period on the periodic table
UNIT VIII ATOMS AND THE PERIODIC TABLE 25 E. Chemical Bonding 1. An ELECTROSTATIC FORCE is All chemical bonding is based on the following relationships of electrostatics: The greater the distance between
More informationAtomic Structure. Part 3: Wave-Mechanical Model of the Atom. Key Question: How does the wave mechanical model explain the location of electrons?
Name Chemistry Atomic Structure Essential Question: How was the structure of the atom determined? Vocabulary: bright-line spectrum electron configuration excited state ground state orbital wave-mechanical
More informationA1 Models of the atom. A2 Size of the atom
A1 Models of the atom 1. Describe the improvements to our understanding of the atom from each of the following scientists: 1.1. Democritus 1.2. Dalton 1.3. Thomson 1.4. Rutherford 1.5. Bohr 1.6. Chadwick
More informationNote that the protons and neutrons are each almost 2,000 times more massive than an electron; What is the approximate diameter of an atom?
Atomic Structure and the Periodic Table Evolution of Atomic Theory The ancient Greek scientist Democritus is often credited with developing the idea of the atom Democritus proposed that matter was, on
More information273 TC. Mass Length Volume 1 lb = g * 1 in = 2.54 cm 1 L = qt* 1 kg = lb * 1 m = yd * 1 ft 3 = L * 1 mi = 1.
Chem 106 Midterm Study Questions Name: Chapters 1-5,11-12 Review Mon 10/10/2016 Due 10/13/2016 (Midterm exam) This is a homework assignment. Please show your work for full credit. If you do work on separate
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 information2) The energy of a photon of light is proportional to its frequency and proportional to its wavelength.
Advanced Chemistry Chapter 13 Review Name Per Show all work Wave Properties 1) Which one of the following is correct? A) ν + λ = c B) ν λ = c C) ν = cλ D) λ = c ν E) νλ = c 2) The energy of a photon of
More informationCh 9 Electrons in Atoms & the Periodic Table Study Sheet Acc. Chemistry SCANTRON. Name /99. 3) Light is a type of matter. 3)
Ch 9 Electrons in Atoms & the Periodic Table Study Sheet Acc. Chemistry SCANTRON Name /99 TRUE/FALSE. Write 'T' if the statement is true and 'F' if the statement is false. 1) When the elements are arranged
More informationChapter 28: Nuclear Chemistry (pg ) On a graph of n 0 versus p + use the position of a plotted nucleus relative to the band of
Chemistry A Final Exam Review Packet Fall 2016 The topics and questions on this review are intended to help you study for the final exam. The exam will include both multiple choice and short answer questions
More informationADVANCED PLACEMENT CHEMISTRY CHAPTERS 7, 8 AND 9 REVIEW QUESTIONS
1. What is the minimum wavelength (in nm) of a photon of light that can excite an electron in the hydrogen atom from the n = 1 to the n = 8 energy level? 2. A carbonoxygen double bond in a certain organic
More informationChem 106 Midterm Study Questions Chapters 1-5,11-12
Chem 106 Midterm Study Questions Chapters 1-5,11-12 Name: Review Mon 10/12/15 Due 10/13/15 (Midterm exam) This is a homework assignment. Please show your work for full credit. If you do work on separate
More informationName PRACTICE Unit 3: Periodic Table
1. Compared to the atoms of nonmetals in Period 3, the atoms of metals in Period 3 have (1) fewer valence electrons (2) more valence electrons (3) fewer electron shells (4) more electron shells 2. On the
More informationHL Chemistry Topic 12 Atomic Structure
Define: ionization energy - 1 - Trends in Ionization Energy in the Periodic Table Why do these trends in ionization energy occur? Background information: Understand the concept of effective nuclear charge
More informationE J The electron s energy difference between the second and third levels is J. = J
The wavelength of light emitted is 654 nm. = c f c 3.00 10 8 m/s f c 3.00 108 m 1s 6.54 10 7 m f 4.59 4.59 10 14 z 1 s 10 14 The frequency of the light emitted is 4.59 10 14 z. E hf h 6.63 10 34 J/z E
More information8. Which of the following could be an isotope of chlorine? (A) 37 Cl 17 (B) 17 Cl 17 (C) 37 Cl 17 (D) 17 Cl 37.5 (E) 17 Cl 37
Electronic Structure Worksheet 1 Given the following list of atomic and ionic species, find the appropriate match for questions 1-4. (A) Fe 2+ (B) Cl (C) K + (D) Cs (E) Hg + 1. Has the electron configuration:
More information