Chemistry Unit 1: Matter Outcome Study Guide
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1 1. Define: Chemistry Unit 1: Matter Outcome Study Guide Effective nuclear charge Ionization energy Electron affinity Electronegativity Anion Cation Valence electron Isoelectronic Ion Isotope Orbital Intermolecular Forces Intramolecular Forces Atomic Structure 2. Fill out the chart for subatomic particles. Subatomic Particle Charge Mass/Size Other Info Proton Neutron Electron 3. In regards to the elements found on the periodic table: a. How do you find the number of neutrons? b. How do you find the number of electrons? c. How do you find the number of protons?
2 4. How are an ion and a neutral atom different? 5. How are two atoms that are isotopes different? How are they the same? 6. List the order that you fill the energy levels and orbitals for electron configuration. 7. Give the electron configuration and orbital diagram for the following: a. Phosphorus b. Calcium c. Tungsten d. Radium 8. Give an example of an incorrect electron configuration and orbital notation. 9. What is the relationship between wavelength and amount of energy released? List the colors of the visible spectrum in order from lowest to highest energy. 10. Calculate the frequency of a wavelength of 515nm (5.15 x 10-7 m).
3 Periodic Table & Trends 11. Color or label the following on the periodic table. a. Halogens b. Alkali Metals c. Alkaline Earth Metals d. Noble Gases e. Transition Metals f. Metals g. Nonmetals h. Metalloids 12. Label the following on the periodic table. a. Increasing atomic radius b. Increasing ionization energy c. Increasing electron affinity d. Increasing electronegativity e. Valence electrons f. Ionic charge
4 13. Fill in the following chart with the properties of metals, nonmetals and metalloids. Type of Element Appearance Conductivity Reactivity w/ acid State of Matter Malleable/Brittle Metal Nonmetal Metalloid Bond Type 14. How do you determine the amount of valence electrons for an element on the periodic table? 15. How do you determine the ionic charge for an element on the periodic table? 16. Differentiate between an ionic bond and a covalent bond. 17. How can you differentiate between an ionic compound and a covalent compound? 18. What are the naming rules for ionic compounds? For covalent compounds? 19. Rank the bond types in order from strongest to weakest: ionic, nonpolar covalent, polar covalent, metallic.
5 20. Differentiate between intermolecular forces and intramolecular forces. Why are both important? 21. Rank the 4 bond types in order of highest melting and boiling points to lowest melting and boiling points. Explain why some molecules require more energy to melt/boil than others. Practice Questions 22. Match the element to its electron configuration. a. 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 5s 2 Re b. [Ar] 4s 2 3d 3 V c. 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 5s 2 4d 10 5p 6 Sr 6s 2 4f 14 5d 10 6p 4 Po d. [Xe] 6s 2 4f 14 5d Rank the elements in order from highest to lowest ionization energy. a. Zn, Kr, Ca, Br 24. Rank the elements in order from smallest to largest radius. a. Cu, Br, Ca 25. Rank the following compounds in order from weakest bond type to strongest bond type. a. HCl, CuCl 2, Cl How many valence electrons do the following elements have? a. Carbon b. Strontium c. Iodine d. Zinc 27. Which of the following are isoelectronic? (Circle all that apply) a. Ar b. Ca 2+ c. Mg 2+ d. Kr e. Cl 1-
6 28. Which of the following are isotopes? a. Ca-40 and Ca-42 b. Ni-64 and Zn-64 c. Ag-107, Au-197 and Ar Using the properties listed, identify the element. a. High luster, 2 valence electrons, period 3 element b. Nonmetal, 3 energy levels, -1 ionic charge c. Ductile, malleable, 2 valence electrons, 6 energy levels 30. How many electrons are at each energy level for the following atoms? a. Calcium b. Tin 31. Identify each as an ionic, polar covalent or nonpolar covalent compound. a. CaCl 2 b. SO 2 c. F 2 d. H 2O e. KCl f. CO Name the following compounds. a. NH 4CLO 3 d. Ca 3(PO 4) 2 g. N 2H 4 b. MgBr 2 e. CaCO 3 h. Na 2SiO 3 c. NF 3 f. Fe(NO 3) 3 i. CuCl Give the balanced formula for the following compounds. a. Ammonium phosphate g. Calcium nitrate b. Potassium Chromate h. Manganese (IV) chloride c. Dinitrogen pentoxide i. Carbon tetrabromide d. Tetraphosphorus decasulfide j. Potassium sulfate e. Silver acetate k. Dinitrogen monoxide f. Sodium phosphide l. Silicon tetrachloride
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