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CHAPTER 5

CHAPTER 5. Electrons in Atoms. National Standards for Chapter 5. UCP.1 Systems, order, and organization UCP.2 Evidence, models, and explanation A.1 Abilities necessary to do scientific inquiry A.2 Understandings about scientific inquiry B.1 Structure of atoms

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CHAPTER 5

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  1. CHAPTER 5 Electrons in Atoms

  2. National Standards for Chapter 5 • UCP.1 Systems, order, and organization • UCP.2 Evidence, models, and explanation • A.1 Abilities necessary to do scientific inquiry • A.2 Understandings about scientific inquiry • B.1 Structure of atoms • B.6 Interactions of energy and matter • E.2 Understandings about science and technology • F.6 Science and technology in local national, and global challenges • G.1 Science as a human endeavor • G.2 Nature of scientific knowledge • G.3 Historical perspectives

  3. Vocabulary/Study Guide • Define each term using the Glossary • Either write on the handout, or use your own paper • This is due on Test Day (tentatively Wednesday, October 30)

  4. Section 1: Light and Quantized Energy • National Standards: • UCP.1 Systems, order, and organization • UCP.2 Evidence, models, and explanation • A.1 Abilities necessary to do scientific inquiry • A.2 Understandings about scientific inquiry • B.1 Structure of atoms • B.6 Interactions of energy and matter • G.1 Science as a human endeavor • G.2 Nature of scientific knowledge • G.3 Historical perspectives

  5. Objectives – Section 1 • Compare the wave and particle natures of light. • Define a quantum of energy, and explain how it is related to an energy change of matter. • Contrast continuous electromagnetic spectra and atomic emission spectra. REVIEW VOCABULARY: radiation: the rays and particles —alpha particles, beta particles, and gamma rays—that are emitted by radioactive material

  6. New Vocabulary electromagnetic radiationquantum WavelengthPlanck’s constant Frequencyphotoelectric effect Amplitudephoton electromagnetic spectrumatomic emissionspectrum Light, a form of electronic radiation, has characteristics of both a wave and a particle.

  7. The Atom and Unanswered Questions • Recall that in Rutherford's model, the atom’s mass is concentrated in the nucleus and electrons move around it. • The model doesn’t explain how the electrons were arranged around the nucleus. • The model doesn’t explain why negatively charged electrons aren’t pulled into the positively charged nucleus.

  8. The Atom and Unanswered Questions • In the early 1900s, scientists observed certain elements emitted visible light when heated in a flame. • Analysis of the emitted light revealed that an element’s chemical behavior is related to the arrangement of the electrons in its atoms.

  9. The Wave Nature of Light • Visible light is a type of electromagnetic radiation, a form of energy that exhibits wave-like behavior as it travels through space. • All waves can be described by several characteristics.

  10. The Wave Nature of Light • The wavelength(λ) is the shortest distance between equivalent points on a continuous wave. • The frequency(ν) is the number of waves that pass a given point per second. • The amplitude is the wave’s height from the origin to a crest.

  11. The Wave Nature of Light

  12. The Wave Nature of Light • The speed of light (3.00  108 m/s) is the product of it’s wavelength and frequency c = λν.

  13. The Wave Nature of Light • Sunlight contains a continuous range of wavelengths and frequencies. • A prism separates sunlight into a continuous spectrum of colors. • The electromagnetic spectrum includes all forms of electromagnetic radiation.

  14. The Wave Nature of Light

  15. The Particle Nature of Light • The wave model of light cannot explain all of light’s characteristics. • Ex. Why heated objects emit only certain frequencies of light at a given temperature. • In 1900, German physicist Max Planck (1858-1947) began searching for an explanation of this phenomenon as he studied the light emitted by heated objects.

  16. The Particle Nature of Light • Planck’s study led him to a startling conclusion: • Matter can gain or lose energy only in small, specific amounts called quanta. • A quantum is the minimum amount of energy that can be gained or lost by an atom. • Planck’s constanthas a value of 6.626  10–34 J ● s.

  17. The Particle Nature of Light • The photoelectric effect is when electrons are emitted from a metal’s surface when light of a certain frequency shines on it.

  18. The Particle Nature of Light • Albert Einstein proposed in 1905 that light has a dual nature. • A beam of light has wavelike and particle like properties. • A photon is a particle of electromagnetic radiation with no mass that carries a quantum of energy.

  19. Atomic Emission Spectra • Light in a neon sign is produced when electricity is passed through a tube filled with neon gas and excites the neon atoms. • The excited atoms return to their stable state by emitting light to release energy.

  20. Atomic Emission Spectra

  21. Atomic Emission Spectra • The atomic emission spectrumof an element is the set of frequencies of the electromagnetic waves emitted by the atoms of the element. • Each element’s atomic emission spectrum is unique.

  22. Homework, Section 1 • SECTION 1 REVIEW, Page 145 • Questions #8,9,11-14 • Answer with complete sentences • Due tomorrow

  23. Section 2: Quantum Theory and the Atom • National Standards: • UCP.1 Systems, order, and organization • UCP.2 Evidence, models, and explanation • A.2 Understandings about scientific inquiry • B.1 Structure of atoms • B.6 Interactions of energy and matter • G.2 Nature of scientific knowledge • G.3 Historical perspectives

  24. Objectives – Section 2 • Compare the Bohr and quantum mechanical models of the atom. • Explain the impact of de Broglie's wave article duality and the Heisenberg uncertainty principle on the current view of electrons in atoms. • Identify the relationships among a hydrogen atom's energy levels, sublevels, and atomic orbitals. Review Vocabulary: atom: the smallest particle of an element that retains all the properties of that element, is composed of electrons, protons, and neutrons.

  25. New Vocabulary ground stateatomic orbital quantum numberprincipal quantum number de Broglie equationenergy sublevel Heisenberg uncertaintyprincipal energy level principle quantum mechanical model of the atom Wavelike properties of electrons help relate atomic emission spectra, energy states of atoms, and atomic orbitals.

  26. Bohr’s Model of the Atom • Einstein’s theory of light’s dual nature accounted for several unexplainable phenomena but not why atomic emission spectra of elements were discontinuous rather continuous. • In 1913, Niels Bohr, a Danish physicist working in Rutherford’s laboratory, proposed a quantum model for the hydrogen atom that seemed to answer this question.

  27. Bohr’s Model of the Atom • Bohr correctly predicted the frequency lines in hydrogen’s atomic emission spectrum. • The lowest allowable energy state of an atom is called its ground state. • When an atom gains energy, it is in an excited state.

  28. Bohr’s Model of the Atom • Bohr suggested that an electron moves around the nucleus only in certain allowed circular orbits.

  29. Bohr’s Model of the Atom • Each orbit was given a number, called the quantum number.

  30. Bohr’s Model of the Atom • Hydrogen’s single electron is in the n = 1 orbit in the ground state. • When energy is added, the electron moves to the n = 2 orbit.

  31. Bohr’s Model of the Atom

  32. Bohr’s Model of the Atom

  33. Bohr’s Model of the Atom • Bohr’s model explained the hydrogen’s spectral lines, but failed to explain any other element’s lines. • The behavior of electrons is still not fully understood, but it is known they do not move around the nucleus in circular orbits.

  34. The Quantum Mechanical Model of the Atom • Louis de Broglie (1892–1987) hypothesized that particles, including electrons, could also have wavelike behaviors.

  35. The Quantum Mechanical Model of the Atom • The figure illustrates that electrons orbit the nucleus only in whole-number wavelengths.

  36. The Quantum Mechanical Model of the Atom • The de Broglie equationpredicts that all moving particles have wave characteristics.

  37. The Quantum Mechanical Model of the Atom • Heisenberg showed it is impossible to take any measurement of an object without disturbing it. • The Heisenberg uncertainty principlestates that it is fundamentally impossible to know precisely both the velocity and position of a particle at the same time. • The only quantity that can be known is the probability for an electron to occupy a certain region around the nucleus.

  38. The Quantum Mechanical Model of the Atom

  39. The Quantum Mechanical Model of the Atom • Schrödinger treated electrons as waves in a model called the quantum mechanical model of the atom. • Schrödinger’s equation applied equally well to elements other than hydrogen.

  40. The Quantum Mechanical Model of the Atom • The wave function predicts a three-dimensional region around the nucleus called the atomic orbital.

  41. Hydrogen’s Atomic Orbitals • Principal quantum number (n) indicates the relative size and energy of atomic orbitals. • n specifies the atom’s major energy levels, called the principal energy levels.

  42. Hydrogen’s Atomic Orbitals • Energy sublevels are contained within the principal energy levels.

  43. Hydrogen’s Atomic Orbitals • Each energy sublevel relates to orbitals of different shape.

  44. Hydrogen’s Atomic Orbitals

  45. Homework, Section 2 • SECTION 2 REVIEW, Page 155 • Questions #15,17-20 • Answer with complete sentences • Due tomorrow

  46. Section 3: Electron Configuration • National Standards: • UCP.1 Systems, order, and organization • UCP.2 Evidence, models, and explanation • A.1 Abilities necessary to do scientific inquiry • A.2 Understandings about scientific inquiry • B.1 Structure of atoms • B.6 Interactions of energy and matter • E.2 Understandings about science and technology • F.6 Science and technology in local national, and global challenges • G.2 Nature of scientific knowledge • G.3 Historical perspectives

  47. Objectives – Section 3 • Apply the Pauli exclusion principle, the aufbau principle, and Hund's rule to write electron configurations using orbital diagrams and electron configuration notation. • Define valence electrons, and draw electron-dot structures representing an atom's valence electrons. Review Vocabulary: electron: a negatively charged, fast-moving particle with an extremely small mass that is found in all forms of matter and moves through the empty space surrounding an atom's nucleus

  48. New Vocabulary electron configuration aufbau principle Pauli exclusion principle Hund's rule valence electrons electron-dot structure A set of three rules determines the arrangement in an atom.

  49. Ground-State Electron Configuration • The arrangement of electrons in the atom is called the electron configuration. • The aufbau principle states that each electron occupies the lowest energy orbital available.

  50. Ground-State Electron Configuration

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