CHEM EXAM 2 STUDY GUIDE
CHEM EXAM 2 STUDY GUIDE Chemistry 1030
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This 5 page Study Guide was uploaded by Emma Shoupe on Friday March 4, 2016. The Study Guide belongs to Chemistry 1030 at Auburn University taught by Dr. Livia Streit in Spring 2016. Since its upload, it has received 134 views. For similar materials see General Chemistry 1 in Chemistry at Auburn University.
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Date Created: 03/04/16
CHEMISTRY 1030 STUDY GUIDE –EXAM 2 – DR. STREIT This may be a really long study guide. Feel free to do all of it, some of it, or none of it. I went ahead and put a lot on there for extra practice and review. Happy studying! First of all…. A list of topics to study – o Ionization energy o Electron affinity o Metallic character o Isoelectric o Ionic radius o Compounds o Lewis Dot o Ionic, metallic and covalent bonding o Naming ions o Formulas (molecular, ionic, empirical) o Naming molecular compounds o Compounds with hydrogen o Organic compounds o Hydrates o Molecular Mass o Percent composition o Molar mass o Octet rule o Electronegativity Remember to memorize polyatomic ions and the names (such as – ate, -ite, etc.). Also, try to memorize the prefixes. Also, there are some topics I cannot cover on this study guide because I can’t add what we learn in Tuesday’s (March 8) class to this study guide. Second… Here are some questions as well as some problems to try in the textbook – 1. What is Ionization energy? 2. Arrange the following in order of increasing first ionization energy: F, K, P, Ca, Ne. 3. What happens to an element as a result of the removal of an electron? 4. What does Z effective mean? 5. Why does shielding occur? 6. What is the relationship of the elements and ionization energy? (how do you tell how big or small the energy will be?) 7. What is electron affinity? 8. What is the relationship between elements and electron affinity? 9. Specify which of the following elements you would expect to have the greatest electron affinity: He, K, Co, S, Cl. 10. Explain why alkali metals have a greater affinity for electrons than alkaline earth metals. (Page 137; 4.61; 4.63 is also a good one) 11. What happens to an element as a result of the accepting of an electron? 12. Name 3 characteristics of metals. 13. Name 3 characteristics of nonmetals. 14. What are metalloids and why are they important? 15. What does it mean for elements to be isoelectric? 16. What is the relationship between having a high/low ionization energy, or a high/low electron affinity? 17. Arrange the following atoms in order of increasing atomic radius: Si, Mg, Cl, P, Al. 18. What is the ionic radius and what is the relationship? 19. Consider two ions with opposite charges separated by a distance, d. What effect does each of the following changes have on the force between the ions? (Page 136; 4.41; other good ones include 4.49, 4.53, 4.55 4.57) a. Both charges are doubled. b. The positive charge is doubled and the negative charge is tripled. c. The negative charge and the distance are tripled. d. The positive charge is doubled and the distance is doubled. e. Both charges and the distance are halved. 20. What is a compound? 21. An atom of a certain element has 16 electrons. Using only the periodic table, identify the element and write its ground-state electron configuration. (Page 135; 4.15 in textbook; some other good ones to try are 4.17, 4.19, and 4.21) +¿ 2+¿ 22. Explain which cation is larger and why: Cu ¿ or ¿ . Cu 23. What is a Lewis Dot symbol? 24. Write the Lewis Dot symbols for the following atoms/ions: a. Br b. N c. I d. As e. F +¿ f. P ¿ g. +¿ ¿ Na 2+¿ h. Mg ¿ 25. What is an ionic bond? 26. Name 3 characteristics of ionic bonds/compounds. 27. What is a chemical formula? 28. How do you name a cation and anion? 29. What is a covalent bond? 30. What is an empirical formula? 31. Write the empirical formulas for the following compounds: a. C 6 6 b. C8H18 c. C2H6O 2 32. Write the names for the following covalent compounds: a. N 2 3 b. SCl 2 c. NBr 3 d. SeF 2 33. What does it mean to be a hydrate? How would you write that? What does it mean to be an anhydrous salt? 34. What is the molecular mass? Formula mass? 35. What is the formula for percent composition? 36. Find the percent composition for the following compounds: a. NaOH b. CaCO 3 c. Sn(CO )3 2 d. NH NO 4 3 37. Calculate the molar mass for the following: a. SiF4 b. KOH 38. What is the octet rule? Draw an example of it. 39. What are some of the bond length “rules?” 40. What is electronegativity? 41. What is required for a bond to be considered a polar covalent bond? 42. What is the equation for dipole moment? What is a dipole moment? 43. Rank the following bonds in order from most covalent to most ionic. a. Na-Cl b. Li-H c. H-C d. H-F e. Rb-O Remember the problems in the book are a GREAT resource for studying. The odd problems have the answers in the back of the book. Good luck! I hope this helps.
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