* Your assessment is very important for improving the workof artificial intelligence, which forms the content of this project
Download Chp 5 Guided Reading Notes and Vocabulary
Bremsstrahlung wikipedia , lookup
History of quantum field theory wikipedia , lookup
Particle in a box wikipedia , lookup
Chemical bond wikipedia , lookup
EPR paradox wikipedia , lookup
Molecular orbital wikipedia , lookup
Hidden variable theory wikipedia , lookup
X-ray photoelectron spectroscopy wikipedia , lookup
Double-slit experiment wikipedia , lookup
Auger electron spectroscopy wikipedia , lookup
Quantum electrodynamics wikipedia , lookup
Astronomical spectroscopy wikipedia , lookup
Matter wave wikipedia , lookup
X-ray fluorescence wikipedia , lookup
Hydrogen atom wikipedia , lookup
Theoretical and experimental justification for the Schrödinger equation wikipedia , lookup
Tight binding wikipedia , lookup
Wave–particle duality wikipedia , lookup
Atomic orbital wikipedia , lookup
CP Chem: 1 Atomic Structure, Periodic Properties and Nuclear Chemistry Chp 5 Electrons in Atoms Sec 1 (2nd half) Guided Reading Notes Chp 5 Electrons in Atoms Sec 2-3 Guided Reading Notes Vocabulary 5.1 Models of the Atom This section explains the significance of quantized energies as they relate to the quantum mechanical model of the atom. The Quantum Mechanical Model 1. What is the difference between the previous models of the atom and the modern quantum mechanical model? _______________________________________________________________________ _______________________________________________________________________ 2. Is the following sentience true or false? The quantum mechanical model of the atom estimates the probability of finding an electron in a certain position. ___________ Atomic Orbitals 3. A(n) ____________________ is often thought of as a region of space in which there is a high probability of finding an electron. 4. What is the term that is used to label the energy levels of electrons? _______________________________________________________________________ 5. The letter __________ is used to denote a spherical orbital. 6. How many orientations does the p orbital have? _____________________________ 7. How are the p orbitals similar? ___________________________________________ 8. How are the p orbitals different? _________________________________________ 9. Circle the letter of the formula for the maximum number of electrons that can occupy a principle energy level? Use n for the principle quantum number. a. 2n2 b. n2 c. 2n d. n 5.2 Electron Arrangement in Atoms This section shows you how to apply the aufbau principle, the Pauli exclusion principle, and Hund’s rule to help you write the electron configurations of elements. It also explains why the electron configurations for some elements are exceptions to the aufbau principle. Electron Configurations 1. The ways in which electrons are arranged into orbitals around the nuclei of atoms are called ____________________. 2. Look at the aufbau diagram, Figure 5.7 on page 133. Which atomic orbital is of higher energy, a 4f or a 5p orbital? __________ 3. Fill in the electron configurations for the elements given in the table. Use the orbital filling diagram to complete the table. Electron Configurations for Some Selected Elements Orbital filling Element 1s 2s 2px 2py 2pz 3s Electron Configuration 1s1 He 1s22s1 C 1s22s22p3 O 1s22s22p5 Ne 1s22s22p63s1 4. In an electron configuration, what does a superscript stand for? _______________________________________________________________________ 5. In an electron configuration, what does the sum of the superscripts equal? _______________________________________________________________________ Exceptional Electron Configurations 6. Is the following sentence true or false? Every element in the periodic table follows the aufbau principle. __________ 7. Filled energy sublevels are more __________ than partially filled sublevels. 8. Half-filled levels are not as stable as __________ levels, but are more stable than other configurations. 5.3 Physics and the Quantum Mechanical Model This section describes the variables used to describe light. It also explains how atomic emission spectra are produced, and compares the dual wave-particle nature of light and electrons. Light 1. The units of frequency are usually cycles per second. The SI unit of cycles per second is called a(n) __________. 2. The product of wavelength and frequency always equals a (n) __________, the speed of light. 3. Is the following sentences true or false? The wavelength and frequency of light are inversely proportional to each other. __________ 4. Light consists of electromagnetic waves. What kind of visible and invisible radiation are included in the electromagnetic spectrum? _______________________________________________________________________ _______________________________________________________________________ 5. When sunlight passes through a prism, the different wavelengths separate into a(n) __________ of colors. 6. What is the color of visible light with the highest frequency? __________ 7. What is the color of visible light with the lowest frequency? __________ 8. Look at Figure 5.10 on page 139. The electromagnetic spectrum consists of radiation over a broad band of wavelengths. What type of radiation has the lowest frequency? The highest frequency? _______________________________________________________________________ Atomic Spectra 9. What happens when an electric current is passed through the gas or vapor of an element? _______________________________________________________________ 10. Passing the light emitted by an element through a prism gives the ____________________ of the element. 11. Is the following sentence true or false? The emission spectrum of an element can be the same as the emission spectrum of another element. __________ An Explanation of Atomic Spectra 12. What is the lowest possible energy of an electron called? __________ 13. Only electrons moving from __________ to __________ energy levels lose energy and emit light. Quantum Mechanics 14. What did Albert Einstein call the quanta of light energy? __________ 15. What does de Broglie’s equation predict about the behavior of particles? _______________________________________________________________________ 16. Is the following sentence true or false? Quantum mechanics describes the motions of subatomic particles and atoms as waves. __________ 17. According to the Heisenberg uncertainty principle, it is impossible to know exactly both the __________ and the __________ of a particle at the same time. 18. Does the Heisenberg uncertainty principle apply to cars and airplanes? Why? _______________________________________________________________________ Vocabulary Define the following words and concepts quantum quantum mechanical model atomic orbital Schrödinger principle energy level electron configuration Aufbau principle Pauli exclusion principle Hund’s rule amplitude wavelength frequency hertz electromagnetic radiation spectrum atomic emission spectrum ground state photons Heisenberg uncertainty principle Einstein de Broglie Heisenberg