Study Guide for Content Mastery - Covenant Science Stuff

1 Copyright Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Guide for Content MasteryChemistry: Matter and Change Chapter 1161 The MoleThe MoleSection MatterIn your textbook, read about counting Column B, rank the quantities from Column A from smallest to AColumn 000 000 your textbook, read about converting moles to particles and particles to the boxes provided, write the conversion factor that correctly completes each mol Cu 1023Cu 1022molecules CH4 10 1mol 1026atoms Xe 102mol mol F2 1024molecules F2 Study Guide FOR Content MASTERYCHAPTER11 Copyright Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, : Matter and Change Chapter 11 Study Guide for Content MasterySection and the MoleIn your textbook, read about the mass of a each statement below, write trueor isotope hydrogen-1 is the standard used for the relative scale ofatomic mass of an atom of helium-4 is 4 mass of a mole of hydrogen atoms is mass in grams of one mole of any pure substance is called its atomic masses recorded on the periodic table are weighted averagesof the masses of all the naturally occurring isotopes of each molar mass of any element is numerically equal to its atomic mass in molar mass unit is the measured mass of an element is numerically equal to its molar mass,then you have indirectly counted 1023atoms of the element in themeasurement.

2 In your textbook, read about using molar each problem listed in Column A, select from Column B the letter of the conversionfactor that is needed to solve the problem. You may need to use more than one conver-sion factor to solve the AColumn the number of moles in g of the mass of 1020zinc the mass of moles of the number of atoms in g of zinc. the number of moles that contain the number of atoms in moles of Guide FOR Content mol Zn 1023atoms 1023atoms Zn 1 mol Zn1 mol Zn g g Zn 1 mol ZnCopyright Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Guide for Content MasteryChemistry: Matter and Change Chapter 1163 Section of CompoundsIn your textbook, read about chemical formulas and the mole, the molar mass of com-pounds, and conversions among mass, moles, and number of the table and the diagram of a methane molecule and a trichloromethane molecule.

3 Then answer the following elements and how many atoms of each does a molecule of methane contain? elements and how many atoms of each does a molecule of trichloromethane contain? many moles of each element are in a mole of methane? many moles of each element are in a mole of trichloromethane? of the following values represents the number of carbon atoms in one mole ofmethane? 1023; 1023; 1023; of the following values represents the number of chlorine atoms in one mole oftrichloromethane? 1023; 1024; 1024; of the following values represents the molar mass of methane? g/mol; g/mol; g/mol; (CH3Cl) has a molar mass of g/mol. Which of the following valuesrepresents the number of molecules of CH3Cl in 101 grams of the substance? 1023; 1023; 1024; 1026 Study Guide FOR Content MASTERYCHAPTER11 ElementMolar Mass (g/mol) Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, : Matter and Change Chapter 11 Study Guide for Content MasterySection and Molecular FormulasIn your textbook, read about percent the following is the percent composition of a compound?

4 How to find the percent composition of a compound if you know the mass of asample of a compound and the mass of each element in the sample. In your textbook, read about empirical and molecular the letter of the choice that best answers the information about a compound can you use to begin to determine the empiricaland molecular formulas of the compound? of the composition of the of elements in the of the have determined that a compound is composed of moles of carbon and moles of oxygen. What must you do to determine the mole ratio of the elements inthe empirical formula of the compound? each mole value by each mole value by each mole value by each mole value by mole ratio of carbon to hydrogen to oxygen in a compound is 1 mol C : 2 mol H : 1 mol O. What is the empirical formula of the compound? calculate the mole ratio of oxygen to aluminum in a compound to be mol O : 1 mol Al.

5 What should you do to determine the mole ratio in the empirical formula of the compound? each mole value by each mole value by each mole value by each mole value by is the relationship between the molecular formula and the empirical formula of acompound?a.(molecular formula)(empirical formula) formula formula (empirical formula) formula n empirical formulaempirical formula nSTUDY Guide FOR Content MASTERYCHAPTER11 Copyright Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Guide for Content MasteryChemistry: Matter and Change Chapter know that the empirical formula of a compound has a molar mass of g/mol. Theexperimental molar mass of this compound is g/mol. What must you do to deter-mine the value of nin the relationship between the molecular formula and the empiricalformula? g/mol and g/mol by g/mol by g/mol by know that the experimental molar mass of a compound is three times the molar massof its empirical formula.

6 If the compound s empirical formula is NO2, what is its molecu-lar formula? the following problem. Show your work in the space sample of a compound contains g potassium, g carbon, and g the empirical and molecular formulas of this compound, which has a molarmass of g/mol. Study Guide FOR Content MASTERYCHAPTER11 Section continuedCopyright Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, : Matter and Change Chapter 11 Study Guide for Content MasterySection Formula for a HydrateIn your textbook, read about naming and analyzing each of the terms below just once to complete the (n) (1)is a compound that has a specific number of watermolecules bound to its atoms. Molecules of water that become part of a hydrate are calledwaters of (2). In the formula for a hydrate, the number of(3)associated with each (4)of thecompound is written following a dot. The substance remaining after a hydrate has been heated and its waters of hydrationreleased is called (5).

7 The ratio of the number of moles of(6)to one mole of the anhydrous compound indicates thecoefficient of H2O that follows the dot in the formula of the hydrate. Because the anhydrousform of the hydrate can absorb water into its (7), hydrates are usedas (8), which are drying agents. Complete the table of the following problem. Show your work in the space sample of a hydrate of iron(II) chloride produces g of anhydrous iron(II) chlo-ride (FeCl2) after heating. Determine the empirical formula and the name of the hydrate. Study Guide FOR Content MASTERYCHAPTER11anhydrouscrystal structuredesiccantsformula unithydratehydrationwater moleculeswater of hydrationChemical FormulaNameCdSO4 Cadmium sulfate, anhydrousCdSO4 sulfate tetrahydrat