CHEM 6A Study Guide - Final Guide: Molar Mass, Empirical Formula, Molecular Mass

Chemical Formulas 1- First decide whethereach of the following formulas represents an ionic or molecular substance. If molecular, then decide if the formula is molecular-empirical and/or the actual or true molecular formula. g) 2 2- Determine the molar mass (the mass of one mole in grams) for each of the following elements or compounds to the indicated number of significant figures (5SF) c) Na,sO, (5 SF) d) FeCl, 6H,O (5 SF) a) CiH22, (5 SF) b) B e) Mg,(PO,2 (6 SF) Moles to Mass 3- Calculate the mass in grams of the following a) 0.150 mol Na b) 48.1 mol K,CrO c) 2.787 mol CH,C Mass to Moles 4- a) 3.43gC b) 0.467 gP 37.5 g H,O d) 153 g A(SO.)2 e) 14.8 g NO 3 않

Study Guide for Exam 2 Chapter 3: Molecules, Compounds, and Chemical Equations Sections: 3.2- 3.11 Important Questions and Concepts: . What are ionic and covalent bonds? . How do we represent compounds? What is the difference between a molecular formula and an empirical formula? What is a structural formula? How do we show the 3D structure of a molecule? What is the difference between an element, molecular element, ionic compound, and molecular compound? .How do we write the chemical formula for ionic compounds? What is the naming scheme for ionic compounds? . What is the naming scheme for molecular compounds including acids? What is the formula mass of a compound? How is it related to the molar mass of a compound? How do we calculate the mass percent of elements in a compound? quan- tities are needed and in what units? . How is the empirical formula related to the molecular formula? . How are chemical equations written? Why must a chemical equation be balanced?