2008 Brooks/Cole 2. Frequency (Hz)
|
|
- Eleanore Williamson
- 5 years ago
- Views:
Transcription
1 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 like the ripples on a pond All types ( colors ) have the same velocity (through a vacuum). c = speed of light = x 10 8 ms -1 (exact) 2008 Brooks/Cole Brooks/Cole 2 Electromagnetic Radiation and Matter + λ Electromagnetic Radiation and Matter E increases from radio waves (low ν, long λ) to gamma rays (high ν, short λ) Amplitude 0 distance Frequency (Hz) γ-rays X-rays UV IR Microwave Radiowave FM AM Long radio waves Wavelength (m) Atom Virus Bacterial Animal Thickness Width Dog cell cell of a CD of a CD Wavelength (nm) Visible light is a very small portion of the entire spectrum 2008 Brooks/Cole Brooks/Cole 4 Planck s Quantum Theory Heated solid objects emit visible light Intensity and color distribution depend on T Planck s Quantum Theory As T, the wavelength of maximum intensity shifts toward the blue Increasing filament T 2008 Brooks/Cole Brooks/Cole 6 1
2 Planck s Quantum Theory Classical theory: no restriction on the E emitted by hot atoms. didn t fit experimental data. The Photoelectric Effect Light can cause ejection of e - from a metal surface. Metal cathode (-) An anode (+) attracts e -. Current is measured. vacuum window Anode (+) 2008 Brooks/Cole Brooks/Cole 8 The Photoelectric Effect If λ > threshold (E too low), no e - emission. Higher intensity does NOT cause e - emission if E < threshold! Thresholds: metal λ (nm) color Cs 579 yellow K 539 green Na 451 blue Li 428 violet current (# of ejected e - ) increasing E threshold High I low I The Photoelectric Effect Imagine photons (balls) hitting e - embedded in glue: If the E of the ball: is low, it can t eject an e -. exceeds the strength of the glue, an e - is released Higher intensity = more photons (balls). If E > threshold, more balls eject more e Brooks/Cole Brooks/Cole 10 The Photoelectric Effect Light waves waves match waves cancel + = + = The Bohr Model of the Hydrogen Atom Heated solid objects emit continuous spectra. Excited atomic gases emit line spectra. Each element has a unique pattern. Hydrogen, H wavelength (nm) Mercury, Hg wavelength (nm) 2008 Brooks/Cole Brooks/Cole 12 2
3 The Bohr Model of the Hydrogen Atom Neils Bohr (1913): Energy The Bohr Model of the Hydrogen Atom visible emission ir emission n 3 absorption 2 absorption: ΔE > 0, n emission: ΔE < 0, n Bohr s model exactly predicts the H-atom spectrum. E = x J 1 n = 1, 2, 3,... n 2 ultraviolet emission wavelength (nm) 2008 Brooks/Cole Brooks/Cole 14 The Bohr Model of the Hydrogen Atom H-atom transitions: ΔE = x J n f 2 n i 2 The Bohr Model of the Hydrogen Atom Calculate the E and wavelength (in nm) for an H-atom n = 4 n = 2 transition. ΔE = x [(½) 2 (¼) 2 ] J = x J = x J (negative sign omitted. Losing energy = emission) ν = ΔE/h = x J /6.626 x Js = x s -1 = x Hz λ = c/ν = x 10 8 ms -1 /6.166 x s -1 λ = x 10-7 m = nm 2008 Brooks/Cole Brooks/Cole 16 Bohr s model predicts the H-atom: λ = h mv λ = wavelength (m) h = Planck s constant (J s) m = mass (kg) v = velocity (m s -1 ) Davidson and Germer (1927) observed e - diffraction by metal foils. Wave-like behavior! 2008 Brooks/Cole Brooks/Cole 18 3
4 Schrödinger equation (1926): Treats e - as standing waves (not particles). Developed by analogy to classical equations for the motion of a guitar string. Called wave mechanics or quantum mechanics Explains the structure of all atoms and molecules. Complicated math; important results Brooks/Cole Brooks/Cole 20 ψ 2 = probability of finding an e - at a point in space. Each ψ describes a different energy level. An electron density (probability) map plots ψ 2 for each point in space. Bigger value = darker shade. The H-atom ground-state orbital 2008 Brooks/Cole Brooks/Cole 22 Quantum Numbers Quantum Numbers Most important in determining the orbital energy. Defines the orbital size. Orbitals with equal n are in the same shell. l Code s p d f g h Brooks/Cole Brooks/Cole 24 4
5 Quantum Numbers l = 0, or 1, or 2 if n = 3 and l = 2 (3d), m l is -2, -1, 0, 1 or 2. if n = 3 and l = 1 (3p), m l is -1, 0, or 1. if n = 3 and l = 0 (3s), m l must be 0. Every (n, l, m l ) set has a different shape and/or orientation. Quantum Numbers Number of Number of Maximum Electron Subshell Orbitals Electrons Electrons Shell type Available Possible for n th Shell (n) (=2l + 1) in Subshell (=2n 2 ) 1 s s 1 2 p s 1 2 p 3 6 d s 1 2 p 3 6 d 5 10 f s 1 2 p 3 6 d 5 10 f 7 14 g* Brooks/Cole Brooks/Cole 26 Electron Spin Experiments showed a 4 th quantum no. was needed +½ or ½ only. s Orbitals l = 0 orbital: Every shell (n level) has one s orbital. Spherical. Larger n value = larger sphere View an e - as a spinning sphere. Spinning charges act as magnets. 1s 2s 3s Probability of finding e - at distance r from nucleus Distance from nucleus, r (pm) 2008 Brooks/Cole Brooks/Cole 28 p Orbitals d Orbitals Three p orbitals (l = 1): Related to m l = -1, 0, +1. p x, p y and p z Five d orbitals (l = 2): 3d xz 3d xy 3d yz 3d x 2 - y 2 3d z Brooks/Cole Brooks/Cole 30 5
6 Hydrogen Atom Energies E = x n 2 (in J/atom). Many-Electron Atoms All other atoms are more complex. Subshells do not have equal E. Energy 4s 3s 2s 4p 3p 2p 3d Note: E 3s E 3p E 3d. But, E 3px = E 3py = E 3pz 1s Also: 3d is above 4s (but E 4s E 3d ) 2008 Brooks/Cole Brooks/Cole 32 Atom Electron Configurations Add e - to orbitals in increasing E order Paired spins: +½ and -½ ; Unpaired spins: all +½ or -½ ; or H He Li Be B C N O F Ne Atom Electron Configurations 1s 2s 2p Electron configurations Expanded Condensed 1s 1 1s 1 1s 2 1s 2 1s 2 2s 1 1s 2 2s 1 1s 2 2s 2 1s 2 2s 2 1s 2 2s 2 2p 1 1s 2 2s 2 2p 1 1s 2 2s 2 2p 1 2p 1 1s 2 2s 2 2p 2 1s 2 2s 2 2p 1 2p 1 2p 1 1s 2 2s 2 2p 3 1s 2 2s 2 2p 2 2p 1 2p 1 1s 2 2s 2 2p 4 1s 2 2s 2 2p 2 2p 2 2p 1 1s 2 2s 2 2p 5 1s 2 2s 2 2p 2 2p 2 2p 2 1s 2 2s 2 2p 6 Energy 3s 2s 1s 3p 2p 2008 Brooks/Cole Brooks/Cole 34 Atom Electron Configurations Increasing (n + l), then increasing n n value l value s 7s 6s 5s 4s 3s 2s 1s 7p 6p 6d 5p 5d 5f n + l = 8 4p 4d 4f n + l = 6 n + l = 7 3p 3d n + l = 4 n + l = 5 2p n + l = 2 n + l = 3 n + l = 1 Atom Electron Configurations 1s 2 s 3 s 4 s 3d 5 s 4d 6 s 5d 7 s 6d Main group s block 4 f 5 f Lanthanides and actinides f block 3d 4d 5d 6d Transition elements d block Block identities show where successive e - add. Note: d steps down, f steps down again. 2p 3p 4p 5p 6p 7p 1s Main group p block 2008 Brooks/Cole Brooks/Cole 36 6
7 Atom Electron Configurations Valence Electrons The first 20 elements have only s and p e - : 2008 Brooks/Cole Brooks/Cole 38 Valence Electrons atom configuration core valence N 1s 2 2s 2 2p 3 [He] 2s 2 2p 3 Si 1s 2 2s 2 2p 6 3s 2 3p 2 [Ne] 3s 2 3p 2 Se 1s 2 2s 2 2p 6 3s 2 3p 6 3d 10 4s 2 4p 4 [Ar] 3d 10 4s 2 4p 4 Mn 1s 2 2s 2 2p 6 3s 2 3p 6 3d 5 4s 2 [Ar] 3d 5 4s 2 Note: # of valence e - = A group # Valence Electrons Lewis dot symbols: Dots represent valence e -. Usually only used for s- and p-block elements. N 2008 Brooks/Cole Brooks/Cole 40 Valence Electrons Electron Configurations of Transition Metals 1A 2A 3A 4A 5A 6A 7A 8A ns 1 ns 2 ns 2 np 1 ns 2 np 2 ns 2 np 3 ns 2 np 4 ns 2 np 5 ns 2 np 6 Li Be B C N O F Ne Na Mg Al Si P S Cl Ar Sn (5 th period, group 4A). Noble-gas core: [Kr] Complete 5s and 4d. 2 e - into 5p: [Kr] 4d 10 5s 2 5p Brooks/Cole Brooks/Cole 42 7
8 Electron Configurations of Transition Metals Electron Configurations of Transition Metals [Kr] 4d 5 5s 2 Sc 3d 1 4s 2 Ti 3d 2 4s 2 V 3d 3 4s 2 Fe 3d 6 4s 2 Co 3d 7 4s 2 Ni 3d 8 4s 2 Y 4d 1 5s 2 Zr 4d 2 5s 2 Nb 4d 4 5s 1 Ru Rh 4d 7 5s 1 4d 8 5s 1 Ni (4 th ; 8B; 8 e - into 3d) [Ar] 3d 8 4s 2 La 5d 1 6s 2 Hf 5d 2 6s 2 Ta 5d 3 6s 2 W 5d 4 6s 2 Os 5d 6 6s 2 Ir 5d 7 6s 2 Pt 5d 9 6s 1 Cu (4 th ; 1B; 9 e - into 3d) [Ar] 3d 9 4s 2 Cu has lower E with filled d-block and half-filled s-block [Ar] 3d 10 4s Brooks/Cole Brooks/Cole 44 Ion Electron Configurations Same approach. Positive ion: remove one e - for each + Negative ion: add one e - for each - Ion Electron Configurations A-group ions usually adopt the nearest noble-gas configuration many ions are isoelectronic Brooks/Cole Brooks/Cole 46 Transition Metal Ions Paramagnetism & Unpaired Electrons Spinning e - = tiny magnet. If all e - are paired: Fe [Ar] 3d 6 4s 2 Fe 2+ [Ar] 3d 6 Fe 3+ [Ar] 3d 5 Mn [Ar] 3d 5 4s 2 Mn 2+ [Ar] 3d 5 Mn 4+ [Ar] 3d 3 Mn 7+ [Ar] 2008 Brooks/Cole Brooks/Cole 48 8
9 Paramagnetism & Unpaired Electrons Paramagnet Ferromagnet Periodic Trends: Atomic Radii Estimate of atomic size ½(homonuclear bond length) Cl = 100 pm (Cl 2 bond = 200 pm) H = 37 pm (H 2 bond =74 pm) Cl 200 pm Cl Radii are additive. HCl has a ( ) = 137 pm bond 100 pm 2008 Brooks/Cole Brooks/Cole 50 Periodic Trends: Atomic Radii Periodic Trends: Atomic Radii Increasing Size p + add to the nucleus. Larger charge pulls all e - in, shrinking the atom. Increasing Size 2008 Brooks/Cole Brooks/Cole 52 Periodic Trends: Ionic Radii Group 1A Group 2A Group 3A Li Li + Be Be 2+ B B Na Na + Mg Mg 2+ Al Al K K + Ca Ca 2+ Ga Ga Rb Rb + Sr Sr 2+ In In Periodic Trends: Ionic Radii Group 6A Group 7A O O 2- F F S S 2- Cl Cl Se Se 2- Br Br Te Te 2- I I Main block: outer shell completely removed. e - /e - repulsion reduced (fewer e - ). More e - /e - repulsion (more e - ). The shell swells Brooks/Cole Brooks/Cole 54 9
10 Periodic Trends: Ionic Radii Periodic Trends: Ionization Energies Isoelectronic Ions O 2- F - Na + Mg 2+ Ionic radius (pm) Number of protons Number of electrons Increasing nuclear charge decreasing size Mg(g) Mg + (g) + e - ΔE = Ionization Energy Also called IE Brooks/Cole Brooks/Cole 56 Periodic Trends: Ionization Energies Periodic Trends: Ionization Energies Mg(g) Mg + (g) + e - ΔE = IE 1 Mg + (g) Mg 2+ (g) + e - ΔE = IE 2 Down a group: IE. Larger atom = less tightly held e - Across a period: IE. Smaller atom = more tightly held e - IE 2 > IE 1 Mg + holds the 2 nd e - more tightly. Huge increase if e - removal breaks a complete shell (the core) Brooks/Cole Brooks/Cole 58 Periodic Trends: Ionization Energies Table 7.8 Ionization Energies Required to Remove Successive Electrons Ionization Energy Li Be B C N O F Ne (MJ/mol) 1s 2 2s 1 1s 2 2s 2 1s 2 2s 2 2p 1 1s 2 2s 2 2p 2 1s 2 2s 2 2p 3 1s 2 2s 2 2p 4 1s 2 2s 2 2p 5 1s 2 2s 2 2p 6 IE IE IE IE IE IE IE IE 8 Core electrons IE IE Periodic Trends: Electron Affinities F(g) + e - F - (g) ΔE = Electron Affinity Usually exothermic (EA is negative) EA increases from left to right. Metals have low EA; nonmetals have high EA. Some tables list positive numbers. a sign-convention choice Brooks/Cole Brooks/Cole 60 10
11 Periodic Trends: Electron Affinities Table 7.9 Electron Affinities (kj/mol) 1A 2A 3A 4A 5A 6A 7A 8A (1) (2) (13) (14) (15) (16) (17) (18) H -73 Li -60 Na -53 K -48 Rb -47 Be Mg Ca -2 Sr -5 B -27 Al -43 Ga -30 In -30 C -122 Si -134 Ge -119 Sn -107 N P -72 As -78 Sb -103 O -141 S -200 Se -195 Te -190 F -328 Cl -349 Br -325 I -295 He Ne Ar Kr Xe Ion Formation and Ionic Compounds Ionic compound formation is very exothermic: K(s) + ½ F 2 (g) KF(s) Two, of several, steps are: ΔH f = kj K K + + e - IE = 419 kj [Ne] 4s 1 [Ne] F + e - F - EA = -328 kj [He] 2s 2 2p 5 [He] 2s 2 2p 6 = [Ne] 2008 Brooks/Cole Brooks/Cole 62 Energy in Ionic Compound Formation K(g) F(g) ΔH 1 = ΔH sub ΔH 3 = IE ΔH 4 = EA K + (g) + F - (g) Energy in Ionic Compound Formation Lattice energies are hard to measure K(g) F(g) ΔH 1 = +89 kj ΔH 3 = +419 kj ΔH 4 = -328 kj K + (g) + F - (g) ΔH 2 = ½ Bond E ΔH 5 = Lattice E ΔH 2 = +79 kj Lattice Energy K(s) + ½ F 2 (g) ΔH f KF(s) K(s) + ½ F 2 (g) ΔH f = kj KF(s) ΔH f = ΔH 1 + ΔH 2 + ΔH 3 + ΔH 4 + ΔH 5 (H is a state function) 2008 Brooks/Cole 63 Lattice Energy = ΔH f - ΔH 1 - ΔH 2 - ΔH 3 - ΔH 4 = (-328) = -826 kj 2008 Brooks/Cole 64 Energy in Ionic Compound Formation Table 7.10 Effect of Ion Size and Charge on Lattice E and Melting Point Compound Charges of Ions r + + r - Lattice Energy Melting Point (kj/mol) (K) NaCl +1, = 283 pm BaO +2, = 275 pm MgO +2, = 212 pm Brooks/Cole 65 11
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 information1) Which electron would be most likely to emit x-ray electromagnetic energy?
AP Chemistry Test (Chapter 7) Multiple Choice (40%) 1) Which electron would be most likely to emit x-ray electromagnetic energy? A) n = 1 n = 6 B) n = 2 n = 3 C) n = 6 n = 1 D) n = 3 n = 2 2) Which statement
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 101 Chapter 9 CHEMICAL BONDING. Chemical bonds are strong attractive force that exists between the atoms of a substance
CHEMICAL BONDING Chemical bonds are strong attractive force that exists between the atoms of a substance Chemical Bonds are commonly classified into 3 types: 1. IONIC BONDING Ionic bonds usually form between
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 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 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 informationElectrons. Unit H Chapter 6
Electrons Unit H Chapter 6 1 Electrons were discovered by 1. Dalton 2. Lavoisier 3. Proust 4. Mendeleev 6. Rutherford 7. Bohr 8. Schrodinger 9. Dirac 5. Thomson 2 Electrons were discovered by 1. Dalton
More informationC H E M 1 CHEM 101-GENERAL CHEMISTRY CHAPTER 6 THE PERIODIC TABLE & ATOMIC STRUCTURE INSTR : FİLİZ ALSHANABLEH
C H E M 1 CHEM 101-GENERAL CHEMISTRY CHAPTER 6 THE PERIODIC TABLE & ATOMIC STRUCTURE 0 1 INSTR : FİLİZ ALSHANABLEH CHAPTER 6 THE PERIODIC TABLE & ATOMIC STRUCTURE The Electromagnetic Spectrum The Wave
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 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 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 informationAP Chapter 6 Study Questions
Class: Date: AP Chapter 6 Study Questions True/False Indicate whether the statement is true or false. 1. The wavelength of radio waves can be longer than a football field. 2. Black body radiation is the
More informationMANY ELECTRON ATOMS Chapter 15
MANY ELECTRON ATOMS Chapter 15 Electron-Electron Repulsions (15.5-15.9) The hydrogen atom Schrödinger equation is exactly solvable yielding the wavefunctions and orbitals of chemistry. Howev er, the Schrödinger
More informationHow many grams of sodium metal is required to completely react with 2545 grams of chlorine gas?
EXAMPLE PROBLEM: How many grams of sodium metal is required to completely react with 2545 grams of chlorine gas? 1 - Convert 2545 grams of chlorine to moles chlorine using formula weight 2 - Convert moles
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 informationWhy Patterns for Charges of Common Cations and Anions? Electrons in Atoms
Electrons in Atoms From Light to Energy of Electrons in Atom Quantum mechanical description of Atom 1. Principal quantum number: Shell 2. Orientation (shape) of : Subshell 3. Orbitals hold electrons with
More informationLight. Light (con t.) 2/28/11. Examples
Light We can use different terms to describe light: Color Wavelength Frequency Light is composed of electromagnetic waves that travel through some medium. The properties of the medium determine how light
More informationCh. 7 The Quantum Mechanical Atom. Brady & Senese, 5th Ed.
Ch. 7 The Quantum Mechanical Atom Brady & Senese, 5th Ed. Index 7.1. Electromagnetic radiation provides the clue to the electronic structures of atoms 7.2. Atomic line spectra are evidence that electrons
More informations or Hz J atom J mol or -274 kj mol CHAPTER 4. Practice Exercises ΔE atom = ΔE mol =
CHAPTER 4 Practice Exercises 4.1 10 1 2.1410 s or Hz 4.3 ΔE atom = ΔE mol = 4.5610 J atom 19 1 2.7410 J mol or -274 kj mol 5 1-1 4.5 excitation energy = 471 kj mol 1 + 275 kj mol 1 = 746 kj mol 1 Hg 4.7
More informationBecause light behaves like a wave, we can describe it in one of two ways by its wavelength or by its frequency.
Light We can use different terms to describe light: Color Wavelength Frequency Light is composed of electromagnetic waves that travel through some medium. The properties of the medium determine how light
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 informationSummation of Periodic Trends
Summation of Periodic Trends Factors Affecting Atomic Orbital Energies The Effect of Nuclear Charge (Z effective ) Higher nuclear charge lowers orbital energy (stabilizes the system) by increasing nucleus-electron
More information- Why are phase labels required? Because phase changes either absorb or release energy. ... what does this mean?
157 SINCE the enthalpy change does NOT depend on path, this means that we can use standard values for enthalpy to predict the heat change in reactions that we have not tested in a calorimeter. THERMOCHEMICAL
More informationSummation of Periodic Trends Factors Affecting Atomic Orbital Energies
Summation of Periodic Trends Factors Affecting Atomic Orbital Energies The Effect of Nuclear Charge (Z effective ) Higher nuclear charge lowers orbital energy (stabilizes the system) by increasing nucleus-electron
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 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 informationChapter 6. Electronic Structure of Atoms. The number & arrangement of e - in an atom is responsible for its chemical behavior.
Chapter 6 Electronic Structure of Atoms The number & arrangement of e - in an atom is responsible for its chemical behavior I) The Wave Nature of Light A) Electromagnetic Radiation Radiant Energy light,
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 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 informationCHEM 1311A. E. Kent Barefield. Course web page.
CHEM 1311A E. Kent Barefield Course web page http://web.chemistry.gatech.edu/~barefield/1311/chem1311a.html Two requests: cell phones to silent/off no lap tops in operation during class Bring your transmitter
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 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 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 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 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 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 informationI. Multiple Choice Questions (Type-I)
I. Multiple Choice Questions (Type-I) 1. Which of the following conclusions could not be derived from Rutherford s α -particle scattering experiement? (i) Most of the space in the atom is empty. (ii) The
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 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 informationHow many grams of sodium metal is required to completely react with 2545 grams of chlorine gas?
146 EXAMPLE PROBLEM: How many grams of sodium metal is required to completely react with 2545 grams of chlorine gas? 1 - Convert 2545 grams of chlorine gas to moles. Use formula weight. 2 - Convert moles
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 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 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 informationA.P. Chemistry Practice Test - Ch. 7, Atomic Structure and Periodicity
A.P. Chemistry Practice Test - Ch. 7, Atomic Structure and Periodicity 1) Ham radio operators often broadcast on the 6-meter band. The frequency of this electromagnetic radiation is MHz. A) 50 B) 20 C)
More informationProfessor K. Section 8 Electron Configuration Periodic Table
Professor K Section 8 Electron Configuration Periodic Table Schrödinger Cannot be solved for multielectron atoms We must assume the orbitals are all hydrogen-like Differences In the H atom, all subshells
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 informationThe Electronic Structures of Atoms Electromagnetic Radiation The wavelength of electromagnetic radiation has the symbol λ.
CHAPTER 7 Atomic Structure Chapter 8 Atomic Electron Configurations and Periodicity 1 The Electronic Structures of Atoms Electromagnetic Radiation The wavelength of electromagnetic radiation has the symbol
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 informationCHEMISTRY - KIRSS 2E CH.3 - ATOMIC STRUCTURE: EXPLAINING THE PROPERTIES OF ELEMENTS
!! www.clutchprep.com CONCEPT: THE NATURE OF LIGHT Visible light represents a small portion of the continuum of radiant energy known as. The visible light spectrum ranges from to. Its wave properties of
More informationUnit 7. Atomic Structure
Unit 7. Atomic Structure Upon successful completion of this unit, the students should be able to: 7.1 List the eight regions of the electromagnetic spectrum in the designated order and perform calculations
More informationCHEM Course web page. Outline for first exam period
CHEM 3 Course web page http://web.chemistry.gatech.edu/~barefield/3/chem3a.html Outline for first exam period Atomic structure and periodic properties Structures and bonding models for covalent compounds
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 informationU N I T T E S T P R A C T I C E
South Pasadena AP Chemistry Name 8 Atomic Theory Period Date U N I T T E S T P R A C T I C E Part 1 Multiple Choice You should allocate 25 minutes to finish this portion of the test. No calculator should
More informationLight. Chapter 7. Parts of a wave. Frequency = ν. Kinds of EM waves. The speed of light
Chapter 7 Atomic Structure Light Made up of electromagnetic radiation Waves of electric and magnetic fields at right angles to each other. 1 2 Parts of a wave Wavelength λ Frequency = ν Frequency = number
More informationElectromagnetic spectrum
All course materials, including lectures, class notes, quizzes, exams, handouts, presentations, and other materials provided to students for this course are protected intellectual property. As such, the
More informationChapter 5. The Electromagnetic Spectrum. What is visible light? What is visible light? Which of the following would you consider dangerous?
Which of the following would you consider dangerous? X-rays Radio waves Gamma rays UV radiation Visible light Microwaves Infrared radiation Chapter 5 Periodicity and Atomic Structure 2 The Electromagnetic
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 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 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 informationElectron Configurations and the Periodic Table
Electron Configurations and the Periodic Table The periodic table can be used as a guide for electron configurations. The period number is the value of n. Groups 1A and 2A have the s-orbital filled. Groups
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 information2011 CHEM 120: CHEMICAL REACTIVITY
2011 CHEM 120: CHEMICAL REACTIVITY INORGANIC CHEMISTRY SECTION Lecturer: Dr. M.D. Bala Textbook by Petrucci, Harwood, Herring and Madura 15 Lectures (4/10-29/10) 3 Tutorials 1 Quiz 1 Take-home test https://chemintra.ukzn.ac.za/
More informationCHEMISTRY - ZUMDAHL 8E CH.7 - ATOMIC STRUCTURE & PERIODICITY.
!! www.clutchprep.com CONCEPT: THE NATURE OF LIGHT Visible light represents a small portion of the continuum of radiant energy known as. The visible light spectrum ranges from to. Its wave properties of
More informationElectronic structure the number of electrons in an atom as well as the distribution of electrons around the nucleus and their energies
Chemistry: The Central Science Chapter 6: Electronic Structure of Atoms Electronic structure the number of electrons in an atom as well as the distribution of electrons around the nucleus and their energies
More informationPeriodic Relationships
Periodic Relationships 1 Tabulation of Elements Mendeleev (1869) Arranged by mass Tabulation by chem.& physical properties Predicted missing elements and properties 2 Modern Periodic Table Argon vs. potassium
More informationAP Chemistry A. Allan Chapter 7 Notes - Atomic Structure and Periodicity
AP Chemistry A. Allan Chapter 7 Notes - Atomic Structure and Periodicity 7.1 Electromagnetic Radiation A. Types of EM Radiation (wavelengths in meters) 10-1 10-10 10-8 4 to 7x10-7 10-4 10-1 10 10 4 gamma
More informationI. The Periodic Law and the Periodic Table. Electronic Configuration and Periodicity. Announcements Newland Law of Octaves
Announcements EM radiation --Exam 3 Oct 3...Includes chapters 7/8/9/10 The excluded items include: 1. Classical distinction between energy and matter (p. 217) 2. Numerical problems involving the Rydberg
More informationCHEMISTRY - BROWN 13E CH.7 - PERIODIC PROPERTIES OF THE ELEMENTS
!! www.clutchprep.com CONCEPT: EFFECTIVE NUCLEAR CHARGE & SLATER S RULES When looking at any particular electron within an atom it experiences two major forces. A(n) force from the nucleus and a(n) force
More informationChemistry 111 Dr. Kevin Moore
Chemistry 111 Dr. Kevin Moore Black Body Radiation Heated objects emit radiation based on its temperature Higher temperatures produce higher frequencies PhotoElectric Effect Light on a clean metal surface
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 informationElectron Configuration and Chemical Periodicity
Electron Configuration and Chemical Periodicity The Periodic Table Periodic law (Mendeleev, Meyer, 1870) periodic reoccurrence of similar physical and chemical properties of the elements arranged by increasing
More information2. What is the wavelength, in nm, of light with an energy content of 550 kj/mol? a nm b nm c. 157 nm d. 217 nm e.
1. What is the frequency associated with radiation of 4.59 x 10-8 cm wavelength? a. 6.54 x 10 17 s -1 b. 6.54 x 10 15 s -1 c. 1.53 x 10-8 s -1 d. 13.8 s -1 e. 2.18 x 10 7 s -1 1 2. What is the wavelength,
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 informationTopic 3: Periodic Trends and Atomic Spectroscopy
Topic 3: Periodic Trends and Atomic Spectroscopy Introduction Valence Electrons are those in the outer most shell of an element and are responsible for the bonding characteristics of that element. Core
More information1. Following Dalton s Atomic Theory, 2. In 1869 Russian chemist published a method. of organizing the elements. Mendeleev showed that
20 CHEMISTRY 11 D. Organizing the Elements The Periodic Table 1. Following Dalton s Atomic Theory, By 1817, chemists had discovered 52 elements and by 1863 that number had risen to 62. 2. In 1869 Russian
More informationChapter 11: MODERN ATOMIC THEORY
Chapter 11: MODERN ATOMIC THEORY LIGHT: Electromagnetic Radiation Light is a form of electromagnetic radiation, a type of energy that travels through space at a constant speed, known as the speed of light
More information100% ionic compounds do not exist but predominantly ionic compounds are formed when metals combine with non-metals.
2.21 Ionic Bonding 100% ionic compounds do not exist but predominantly ionic compounds are formed when metals combine with non-metals. Forming ions Metal atoms lose electrons to form +ve ions. Non-metal
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 informationCHEM 1211K Test III. 4) Of the following elements, which has the largest first ionization energy? A) As B) Sb C) Ge D) Se E) S
CEM 1211K Test III MULTIPLE COICE. (3 points each) 1) The photoelectric effect is. A) a relativistic effect B) the production of current by silicon solar cells when exposed to sunlight C) the total reflection
More informationGilbert Kirss Foster. Chapter3. Atomic Structure. Explaining the Properties of Elements
Gilbert Kirss Foster Chapter3 Atomic Structure Explaining the Properties of Elements Chapter Outline 3.1 Waves of Light 3.2 Atomic Spectra 3.3 Particles of Light: Quantum Theory 3.4 The Hydrogen Spectrum
More informationThe Electronic Structure of Atoms
The Electronic Structure of Atoms Classical Hydrogen-like atoms: Atomic Scale: 10-10 m or 1 Å + - Proton mass : Electron mass 1836 : 1 Problems with classical interpretation: - Should not be stable (electron
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 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 informationSection 11: Electron Configuration and Periodic Trends
Section 11: Electron Configuration and Periodic Trends The following maps the videos in this section to the Texas Essential Knowledge and Skills for Science TAC 112.35(c). 11.01 The Bohr Model of the Atom
More informationPART 2 Electronic Structure and the Periodic Table. Reference: Chapter 7 8 in textbook
PART 2 Electronic Structure and the Periodic Table Reference: Chapter 7 8 in textbook 1 Experiment to Discover Atom Structure -particle: He 2+ mass number = 4 Nucleus and Electron Model 2 Atomic Structure
More informationChapter 2. Atomic Structure and Periodicity
Chapter 2 Atomic Structure and Periodicity Chapter 2 Table of Contents (2.1) (2.2) (2.3) (2.4) (2.5) (2.6) (2.7) (2.8) (2.9) Electromagnetic radiation The nature of matter The atomic spectrum of hydrogen
More information- Some properties of elements can be related to their positions on the periodic table.
180 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 informationSample Exercise 6.1 Concepts of Wavelength and Frequency
Sample Exercise 6.1 Concepts of Wavelength and Frequency Two electromagnetic waves are represented in the margin. (a) Which wave has the higher frequency? (b) If one wave represents visible light and the
More informationUnit 1, Lesson 01: Summary of Atomic Structure so far
Unit 1, Lesson 01: Summary of Atomic Structure so far Atoms are made of sub-atomic particles: Protons: found in the nucleus, charge of 1+, mass of 1 amu (u) Neutrons: found in nucleus, no charge, mass
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 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 informationChapter 6 Electronic Structure of Atoms
Chapter 6 Electronic Structure of Atoms What is the origin of color in matter? Demo: flame tests What does this have to do with the atom? Why are atomic properties periodic? 6.1 The Wave Nature of Light
More informationATOMIC STRUCTURE, ELECTRONS, AND PERIODICITY
ATOMIC STRUCTURE, ELECTRONS, AND PERIODICITY All matter is made of atoms. There are a limited number of types of atoms; these are the elements. (EU 1.A) Development of Atomic Theory Atoms are so small
More informationPART 2 Electronic Structure and the Periodic Table. Reference: Chapter 7 8 in textbook
PART 2 Electronic Structure and the Periodic Table Reference: Chapter 7 8 in textbook 1 Early Atomic Models 2 Thomson s 1904 Model of the Atom Plumb Pudding Model He discovered the electron, a discovery
More information2. For the following two compounds between oxygen and hydrogen: 3. Tell what discoveries were made by each of the following scientists:
EXTRA HOMEWORK 1A 1. When Dalton proposed that matter was composed of atoms, why was his Atomic Theory accepted? 2. For the following two compounds between oxygen and hydrogen: Mass of O Mass of H Compound
More informationElectromagnetic Radiation. Chapter 12: Phenomena. Chapter 12: Quantum Mechanics and Atomic Theory. Quantum Theory. Electromagnetic Radiation
Chapter 12: Phenomena Phenomena: Different wavelengths of electromagnetic radiation were directed onto two different metal sample (see picture). Scientists then recorded if any particles were ejected and
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 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 informationChemistry 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 Lesson 1: The Nature of Light Goals: Describe light in terms of electromagnetic energy. Describe the
More information