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Study Guide for Chemistry Exam 3

by: Makayla Richardson

Study Guide for Chemistry Exam 3 CHEM 111 - 02

Makayla Richardson

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About this Document

This study guide covers sections 3.1-3.9 in the textbook and asks a wide variety of open-ended, multiple choice, and and fill-in the blank questions. The answers are also attached.
General Chemistry I
Dr. Antonio Lara
Study Guide
General Chemistry
50 ?




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This 4 page Study Guide was uploaded by Makayla Richardson on Saturday October 15, 2016. The Study Guide belongs to CHEM 111 - 02 at New Mexico State University taught by Dr. Antonio Lara in Fall 2016. Since its upload, it has received 17 views. For similar materials see General Chemistry I in Chemistry and Biochemistry at New Mexico State University.

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Date Created: 10/15/16
Study Guide Chemistry 111 Exam 3 1) List the waves of light from shortest wavelength to longest wavelength. 2) List the waves of light from lowest energy to highest energy. 3) What is a frequency? 4) A wavelength consists of oscillating what? (Two properties) 5) Describe the atomic emissions spectra. 6) Describe the atomic absorption spectra. 7) Photons are given off in _______ increments. 8) Which of the following is quantized? a. Amount of water in the Pacific Ocean. b. The time it takes you to get ready in the morning. c. Amount of eggs in a carton. d. Inches of a zip line. 9) Give the Bohr Model. 10)What is the ground state of an electron? 11)What is the excited state of an electron? 12)Who calculated electron wavelength? 13)What is a node? 14)Describe the Heisenberg Uncertainty Principle? Express it mathematically as well. 15)What is quantum/wave mechanics? 16)What is Schrödinger’s Wave Equation? 17)The principle quantum number is represented as _____ and describes the ____ and  _______ of an orbital, or represents the ________ of orbitals. 18)What does the angular momentum quantum number (l) define. 19)List the value of l to its letter identifier: 0,1,2,3,4  20)What are the allowed values of the magnetic quantum numberm l for 2p? 21)What are the m l for 3d? 22)Spin can be either ____ or _____ but never the same because they ______ each other. 23)How many subshells in n=4? 24)How many orbitals in n=5? 25)How many electrons in n=3? 26)An atom in ground state has 4 n=3 electrons, how many electrons does the atom have? 27)What is the Pauli Exclusion Principle? 28)What is Hund’s Rule? 29)The s orbital has how many subshells? 30)The p orbital has how many subshells?  31)The d orbital has how many subshells? 32)The f orbital has how many subshells? 33)Define core electrons. 34)Define valence electrons. 35)Where is the s block located on the periodic table? 36)Where is the p block located on the periodic table? 37)Where is the d block on the periodic table? 38) Where is the f block located in the periodic table? 39)How many electrons can be found in the s block? 40)How many electrons can be found in the p block? 41)How many electrons can be found in the d block? 42)How many electrons can be found in the f block? 43)Which element is 1s 2s 2p 3s ? 6 1 2 1 44)Which element is [Kr] 5s 4d ? 45)Give the complete electron configuration for Cu. 46)Give the complete electron configuration for Te. 47)Give the condensed electron configuration for Es. 48)Give the condensed electron configuration for Mo.  49)What element is   2s 2p 50)What element is      3s     3p           3d      4s Answers 1. Gamma Rays, X­Rays, Ultraviolet, Visible Light, Infrared, Microwave, Radio  Waves. Violet, Blue, Green, Yellow, Orange, Red. 2. Radio Waves, Microwaves, Infrared, Visible, Ultraviolet, X­Rays, and Gamma  Rays. 3. Frequency: the number of crest a wave gives off in a certain amount of time.  Measured from crest to crest. 4. Electric Field and Magnetic Field. 5. Atomic Emission Spectra: Individual lines given off from an element where it is  lacking in properties of wavelength. 6. Atomic Absorption Spectra: a wide range of color with small black line given off  by an element. 7. Quantized 8. C­ amount of eggs in a carton ­18 1 1 9. ∆ E=−¿ 2.178x10 J( n 2  ­  n 2 ) final❑ initial❑ 10. Ground State: where the electron and element are the most stable and have the  lowest energy. 11. Excited State: where the electron is moving between energy levels. 12. Louis De Broglie  13. The point in a wavelength where it is experiencing no displacement.  14. Heisenberg Uncertainty Principle: you cannot know the energy and location of an  electron at the same time, only one or the other.   ∆ x∙m∆u≥ h 4π 15. Quantum/Wave Mechanics: the description of wavelike behavior in electrons.  16. How the electron matter varies in the wave regarding location and time is  expressed as  ψ∨ψ 2 . 17.  n, size, energy, group 18. Values from 0 to n­1,and determines the shape of an orbital. 19. 0=s     1=p     2=d    3=f     4=g 20. 2p= ­1,0,+1 21. 3d= ­2,­1,0,+1,+2 22. Up, down, repel  23. 4 24. 5 =25 2 25. 3 = 9x2= 18 electrons 26. 1 = 1x2= 2 2 = 4x2=8 8+2+4= 14 electrons 27. Pauli Exclusion Principle: no two electrons can have the same set of four quantum numbers. AKA the electron cannot be paired until there is at least one in every  orbital. 28. Hund’s Rule: the lowest energy electron configuration has maximum number of  unpaired electrons with the same spin and are degenerate. AKA orbitals must all  have the same spin until they are paired.  29. 1 30. 3 31. 5 32. 7 33. Core electrons: electrons closest to the nucleus. 34. Valence electrons: Electrons furthest from the nucleus.  35. The first two groups on the left hand side and Helium. 36. The 3a through 8a groups on the right hand side. 37. All of the transition metals. 38. The lanthanide and actinide series.  39. 2 40. 6 41. 10 42. 14 43. Na, Sodium 44. Y, Yttrium 2 2 6 2 6 1 10 45. 1s 2s 2p 3s 3p 4s 3d 46. 1s 2s 2p 3s 3p 4s 3d 4p 5s 4d 5p 2 10 4 47. [Rn] 7s 5f 11 1 5 48. [Kr] 5s 4d 49. N, Nitrogen  50. Ti, Titanium 


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