Chem 171 Review - Exam 1

Size: px
Start display at page:

Download "Chem 171 Review - Exam 1"

Transcription

1 Chem 171 Review - Exam 1 The following is a list of concepts and terms with which you should be well-acquainted. This is not a substitute for your notes. This list of review topics is not meant to be exhaustive, it is only meant to help you identify the major areas we have discussed. You are responsible for all material covered in lecture and in the text book. Chapter 1: Chemistry and Measurement Chemistry and the scientific process SI units base units: mass, length, time, temperature, amount, current, luminous intensity vs. derived units: derived from the base units; ex: density (mass / vol), vol (length width height), velocity (length / time) metric prefixes and multiples; use in unit conversions: mega-, kilo-, deci-, centi-, milli-, micro-, nano-, picoex: 1 pm = m; 1 mg = 10 3 g conversion factors and dimensional analysis you should be comfortable with intrasystem conversions (metric to metric, English to English), intersystem conversions (metric to English and vice versa), and combined unit conversions Remember: when you raise a unit to some power, you must raise the entire conversion factor to that power ex: (1 cm) 3 = (10 2 m) 3 therefore, 1 cm 3 = 10 6 m 3 uncertainty in measurements indicated by the number of recorded significant figures significant figures: all certain digits plus the 1 st uncertain digit given a number, determine how many significant figures it has understand when zeros are and are not significant determination of the number of significant figures to record when making a measurement with an instrument rules for significant figures in the answer to calculations based on measured values; rule for addition and subtraction is not the same as the rule for multiplication and division chemical vs. physical properties and changes intensive vs. extensive properties classification of matter: elements, compounds (fixed composition), and mixtures (variable composition) elements - you should know the name (properly spelled) and symbol for elements 1 56, W, Pt, Au, Hg, Pb, and Bi Chapter 2: Atoms, Molecules, and Ions atoms and atomic structure early experiments and scientists that established our modern understanding of the atom and its structure protons, electrons, neutrons - know the characteristics of these particles including relative masses and electrical charge atomic structure - where do the various subatomic particles reside? relative size and density of the atom and the nucleus atomic # vs. mass # - what are they, and what information do they provide? isotopes the periodic table arrangement periods vs. groups (families) recognize main group elements, alkali metals, alkaline earth metals, transition metals, halogens, noble (or inert) gases metal / nonmetal / metalloid (or semimetal) distinctions

2 atomic mass atomic mass unit scale for mass of single atom vs. gram unit scale calculation of the average atomic mass of an element based on that element's isotopes and percent abundances molecular compounds vs. ionic compounds molecules vs. ions cations vs. anions; ion formation; monatomic vs. polyatomic ions; p, n, and e count for a monatomic ion NOMENCLATURE: I cannot stress this enough - you should know this stuff cold! Refer to the nomenclature handout. you should be able to provide chemical formulas or IUPAC names for binary molecular compounds, ionic compounds and acids writing and balancing chemical equations; what do the stoichiometric coefficients represent? Chapter 3: Calculations with Chemical Formulas and Equations the mole and molar mass What does a mole represent? Avogadro's number, N A = x mol 1 molar mass of elements or compounds: mass (in g) per mole of an element or compound; units g/mol. molar mass of compound = molar mass of its elements interpretation of chemical formula in terms of mol of atoms, or ions per mol of compound; compound stoichiometry mass percent composition chemical formula determination from mass % data and combustion analysis data empirical formula vs. molecular formula; how are these related? chemical reaction stoichiometry: interpretation of stoichiometric coefficients to determine the mole ratios between reactants and products using mole ratios from chemical equations as conversion factors reaction yield (actual yield) vs. theortetical yield vs. percentage yield - what are they, how do you calculate them? limiting reactants and reaction tables completion of reaction table; mol reactant & product before reaction, change during reaction, remaining after reaction determination of limiting reactants within a reaction calculation of theoretical yield based on limiting reactant identification of the excess reactant and how much excess remains after reaction Chapter 4: Chemical Reactions the nature of solutions speciation and stoichiometry associated with the dissolution of ionic vs. molecular compounds in water strong vs. weak vs. nonelectrolytes: what ware the distinctions? what types of compounds fall in each category? solution compostion: molarity (M) or molar concentration = mol solute/l sol'n calculations of molarity of solutions, molarity of ions in a solution molarity as a conversion factor relating mol of solute and volume of solution calculations that involve molar concentration of solutions: dilution calculations, M i V i = M f V f, or you can think of it in terms of M conc V conc = M dil V dil solution stoichiometry in chemical reactions; ex. volume of sol n required for reaction with a given amount of reactant, or to form a given amount of product DO NOT USE M 1 V 1 = M 2 V 2 FOR REACTION STOICHIOMETRY CALCULATIONS!! You must demonstrate to me that you understand that a chemical reaction is occurring, and that you understand the mole ratios of reactants and products in that reaction.

3 The following are some of the more important conversion factors that we have discussed: density offers you a relationship between mass and volume: density = mass / volume Avogadro's number offers you a relationship between the number of particles and mol N A = x mol 1 (things per mole where things can be atoms, molecules, ions, formula units, etc.) molar mass (of elements or compounds) offers you a relationship between mass of substance and mole quantity molar mass = g (of an element or a compound) / mole Note: you determine the mass of an individual atom, molecule, or formula unit by combining Avogadro s number and molar mass as conversion factors. Follow the conversion string: atom (molecule, ion, formula unit) mol mass in g mole ratios from a BALANCED CHEMICAL EQUATION gives you a relationship between amounts of reactants being consumed and amounts of products being formed in a given chemical reaction. This allows you to convert from moles of reactant A to moles of reactant B, or moles of reactant A to moles of product C, etc. molar concentration, or molarity offers a relationship between the number of moles of solute dissolved per L of solution Review Problems: These review problems are only representative of the kinds of problems with which you should feel comfortable. This is not meant to be representative of the exam questions - in other words, DO NOT EXPECT THAT THE EXAM WILL LOOK LIKE THIS! 1. The density of a substance is 8.4 g/cm 3. Express this density in SI units. 2. Calculate the volume (in cm 3 ) occupied by 25.0 g of aluminum. For aluminum, d = 2.70 g/cm Give the symbol and name for: a. the alkali metal in the same period as chlorine b. a halogen in the same period as magnesium c. the heaviest alkaline earth metal d. a noble gas in the same period as carbon 4. How many significant figures are in each of the following numbers? a b c. 5.7 d x 10 7 e. 5 x 10 3 f g h Perform the indicated calculations and express the answer to the correct number of significant figures. Use scientific notation where appropriate. a x = b. (1.4 x 1.11) / = c x = d = e = f / ( ) = g = h x 10 3 / 1.51 x 10 4 = 6. Perform the following unit conversions. Use scientific notation where appropriate. a cm = m = mm = nm b cm 3 = dm 3 = ml = L = m 3 c. 282 oz = lb = g = mg = µg 7. Write the symbol (with mass and atomic number) for an atom with: a. 6 protons and 6 neutrons b. 13 protons and 14 neutrons c. 19 protons and 20 neutrons

4 8. How many protons, electrons and neutrons are in each of the following ions? a. 23 Na + b. 81 Br - c. 39 K + d. 40 Ca 2+ e. 115 In 3+ f. 127 Te 2-9. An element has two isotopes with masses of amu and amu % of the atoms are the heavier isotope. Calculate the atomic mass of this element and give its name and symbol. 10. Naturally occurring rubidium is 72.17% 85 Rb (atomic mass = amu). The remaining atoms are 87 Rb (atomic mass = amu). Calculate the average atomic mass of rubidium. 11. Determine the molar mass of the following compounds: a. phosphorus trichloride b. potassium carbonate c. nickel (II) phosphate d. sodium thiosulfate Na 2 S 2 O a. A g sample of coal contains g of carbon. Calculate the mass percentage of carbon in the coal. b. A fertilizer is advertised to contain 15.8% nitrogen by mass. Calculate the mass (in g) of N in 4.15 kg of fertilizer. 13. a. Calculate the quantity (in mol) of HCl in g HCl. b. Calculate mol Na 2 SO 4 in 284 g of the compound. 14. Calculate the mass (in g) of each of the following: a mol of CO 2 b mol of K 2 SO 4 c mol of NH Calculate the mass (in g) of a single atom, molecule, ion, or formula unit of each of the following: a. Br b. BrF 3 c. BrO 4 d. KBrO Calculate the number of atoms, molecules, or formula units in each of the following samples: a g of magnesium b g of aluminum oxide c g of xenon hexafluoride 17. Consider a ml sample of ethanol (CH 3 CH 2 OH, d= g/ml). a. Calculate the mass (in g) of this sample. b. Calculate the mol of ethanol in this sample. c. Calculate the number of ethanol molecules in this sample. 18. Name the following elements and list their group and period numbers. Classify each as a metal or non-metal. a. P b. Sb c. Ag d. Zn e. Ba 19. Pewter is an alloy (metal mixture) with the following composition by mass: 6.00% antimony, 1.50% copper, 92.5% tin. Calculate the mass (in g) of each element in a 47.7 g pewter figurine. 20. Provide the missing name or chemical formula for each of the following: barium bromide aluminum oxide copper (II) nitrate Cl 2 O N 2 O 4 NF 3 SnBr 2 sulfurous acid tetraphosphorus hexaoxide sodium hypoiodite HClO 2 (aq) potassium permanganate SrSO 3 CuCN iron (III) hydroxide 21. The bitter tasting compound quinine is a component of tonic water and is used as a protection against malaria. Quinine contains only C, H, O, and N. When a sample of mass g was burned, g carbon dioxide, g of water, and g of N 2 were produced. The molar mass of quinine is 324 g/mol. Determine the empirical and molecular formulas of quinine. 22. A compound containing only Na, Al, and F is 32.79% Na, % Al, and 54.19% F by mass. Determine the empirical formula of this compound. 23. One mole of N 2 contains how many N 2 molecules? N atoms? 24. Consider one mole of iron (III) sulfate, Fe 2 (SO 4 ) 3. Calculate the mol SO 4 2 in this sample. Calculate the number of O atoms in this sample.

5 25. Balance the following chemical equations: a. Na (s) + H 2 O (l) NaOH (aq) + H 2 (g) b. C 2 H 4 (g) + O 2 (g) CO 2 (g) + H 2 O (l) c. Al (s) + HCl (aq) AlCl 3 (aq) + H 2 (g) d. Mg 3 N 2 (s) + HCl (aq) MgCl 2 (aq) + NH 4 Cl (aq) e. Fe(OH) 3 (s) + H 2 SO 4 (aq) Fe 2 (SO 4 ) 3 (aq) + H 2 O (l) 26. Iron in the form of fine wire burns in oxygen to form iron (III) oxide. How many mol of O 2 are required to produce 5.21 mol of iron (III) oxide? 27. Butane, C 4 H 10 burns with the oxygen in air to give carbon dioxide and water: 2 C 4 H 10 (g) + 13 O 2 (g) 8 CO 2 (g) + 10 H 2 O (g) What type of reaction is this? What mass of CO 2 can be produced from the reaction of 0.15 mol C 4 H 10 with excess O 2? 28. Ethanol, C 2 H 5 OH burns in air to give carbon dioxide and water. This combustion reaction is describe by the following equation: C 2 H 5 OH (l) + 3 O 2 (g) 2 CO 2 (g) + 3 H 2 O (l) a. Consider a 88.8 ml sample of ethanol (d = g/ml). Calculate the mol C in this sample. Calculate the number of oxygen atoms in this sample. b. What is the amount of water (in mol) produced from the complete reaction of 0.25 mol ethanol? c. What is the mass of water (in grams) produced from the complete combustion of g of ethanol? 29. Hematite, Fe 2 O 3, is an important ore of iron. Iron metal is obtained by reacting hematite with carbon monoxide (CO) in a blast furnace. The balanced chemical equation for this reaction is: Fe 2 O 3 (s) + 3 CO (g) 2 Fe (s) + 3 CO 2 (g) Calculate the mass (in g) of iron that can be produced from the complete reaction of 1.00 kg of Fe 2 O Chlorine can be produced in the laboratory by heating hydrochloric acid with manganese (IV) oxide. How many grams of HCl are required to react with 5.00 g of MnO 2 according to this equation? 4 HCl (aq) + MnO 2 (s) 2 H 2 O (l) + MnCl 2 (aq) + Cl 2 (g) 31. Zinc sulfide ore is an important source of zinc metal. The first step in the processing of the ore consists of heating the sulfide with oxygen to give zinc oxide, ZnO and sulfur dioxide, SO 2. Calculate the mass (in kg) of O 2 (g) required to react completely with 5.00 x 10 3 g of ZnS. 32. Nitric acid, HNO 3, is manufactured by the Ostwald process, in which nitrogen dioxide, NO 2 reacts with water: 3 NO 2 (g) + H 2 O (l) 2 HNO 3 (aq) + NO (g) How many grams of nitrogen dioxide (with excess water) would be required to produce 5.00 g of nitric acid? 33. Methanol, CH 3 OH, is prepared industrially from the gas-phase catalytic reaction: CO (g) + 2 H 2 (g) CH 3 OH (g) In a laboratory test, a reaction vessel was filled with 35.4 g CO and 10.2 g H 2. Calculate the mass (in g) of methanol that can be produced in this reaction. Which reactant remains unconsumed at the end of this reaction? What mass (in g) of it remain? 34. Carbon disulfide (CS 2 ) burns in oxygen. Complete combustion gives the reaction: CS 2 (g) + 3 O 2 (g) CO 2 (g) + 2 SO 2 (g) Calculate the grams of sulfur dioxide produced when a mixture of 15.0 g of carbon disulfide and 35.0 g of oxygen reacts. Which reactant remains unconsumed at the end of the combustion? How many grams remain? 35. Calculate the molarity of the following solutions: a mol of Na 2 SO 4 dissolved in enough water to form ml of solution b g of NaCl dissolved in enough water to form ml of solution 36. Calculate the mass (in g) of solute present in each of the following solutions: a x 10 2 ml of M Na 2 SO 4 b x 10 2 ml of M KBrO 3

6 37. A sample of mol of iron (III) chloride was dissolved in water to give 25.0 ml of solution. Calculate the molarity of this solution. What is the molarity of chloride ions in this solution? 38. An experiment calls for g of potassium hydroxide, KOH. What volume (in ml) of M KOH is required? 39. You wish to prepare 0.12 M HNO 3 from a stock solution of nitric acid that is 15.8 M. What volume (in ml) of the stock solution is required to prepare 1.00 L of the 0.12 M HNO 3? 40. Calculate the volume of M HNO 3 that will react completely with 42.4 ml of M Na 2 CO 3 according to the following reaction: 2 HNO 3 (aq) + Na 2 CO 3 (aq) 2 NaNO 3 (aq) + H 2 O (l) + CO 2 (g) 41. A 3.33 g sample of iron ore is treated resulting in a solution of iron (II) sulfate. The resulting solution is then reacted with M K 2 Cr 2 O 7 (see balanced equation given below) ml of the potassium dichromate solution are required for complete reaction. Calculate the mass percent iron in the ore sample. 6 FeSO 4 (aq) + K 2 Cr 2 O 7 (aq) + 7 H 2 SO 4 (aq) 3 Fe 2 (SO 4 ) 3 (aq) + Cr 2 (SO 4 ) 3 (aq) + 7 H 2 O (l) + K 2 SO 4 (aq) 42. Bone is dissolved in hydrochloric acid resulting in 50.0 ml of a solution containing calcium chloride, CaCl 2. To precipitate the calcium ion from this solution, an excess of potassium oxalate is added g of calcium oxalate is collected. Calculate the molar concentration of the CaCl 2 solution. Chem 171: Review - Exam 1 Answers x 10 3 kg/m cm 3 3. a. Na b. Cl c. Ra d. Ne 4. a. 5 b. 2 c. 2 d. 3 e. 1 f. 5 g. 6 h a. 216 b..037 c..224 d..5 e f..39 g h a m, 30.1 mm, 3.01 x 10 7 nm 7. a. b dm 3, 50.0 ml,.0500 L, 5.00 x 10 5 m 3 c lb, 7.98 x 10 3 g, 7.98 x 10 6 mg, 7.98 x 10 9 µg 12 6 C 27 Al b. 13 c. 39 K a. 11 p, 10 e, 12 n b. 35 p, 36 e, 46 n c. 19 p, 18 e, 20 n d. 20 p, 18 e, 20 n e. 49 p, 46 e, 66 n f. 52 p, 54 e, 75 n 9. Cu, atomic number 29, amu amu 11. a g/mol b g/mol c g/mol d g/mol 12. a % b. 656 g N 13. a mol HCl b mol Na 2 SO a. 18 g CO 2 b. 35 g K 2 SO 4 c g NH a x g b x g c x g d x g 16. a x atoms b x formula units c x molecules 17. a g b..258 moles c x molecules

7 18. a. phosphorus, group 5A (or group 15), period 3, non-metal b. antimony, group 5A (or group 15), period 5, metal (or metalloid) c. silver, group 11, period 5, metal d. zinc, group 12, period 4, metal e. barium, group 2A (or group 2), period 6, metal g Sb, g Cu, 44.1 g Sn 20. BaBr 2 Al 2 O 3 Cu(NO 3 ) 2 dichlorine oxide dinitrogen tetraoxide nitrogen trifluoride tin (II) bromide H 2 SO 3 (aq) P 4 O 6 NaIO chlorous acid KMnO 4 strontium sulfite copper (I) cyanide Fe(OH) C 10 H 12 NO, C 20 H 24 N 2 O Na 3 AlF x N 2 molecules, 1.20 x N atoms mol SO 2 4 ions, x O atoms 25. a. 2 Na (s) + 2 H 2 O (l) 2 NaOH (aq) + H 2 (g) b. C 2 H 4 (g) + 3 O 2 (g) 2 CO 2 (g) + 2 H 2 O (l) c. 2 Al (s) + 6 HCl (aq) 2 AlCl 3 (aq) + 3 H 2 (g) d. Mg 3 N 2 (s) + 8 HCl (aq) 3 MgCl 2 (aq) + 2 NH 4 Cl (aq) e. 2 Fe(OH) 3 (s) + 3 H 2 SO 4 (aq) Fe 2 (SO 4 ) 3 (aq) + 6 H 2 O (l) mol O g CO a mol C, 9.16 x O atoms b mol H 2 O c g H 2 O g Fe g HCl kg O g NO g CH 3 OH, H 2, 5.12 g H g SO 2, O 2, 16 g O a..128 M b M 36. a g b g M FeCl 3 (aq), 4.09 M Cl (aq) ml ml ml % M

General Chemistry (Chem110) Dr. Rima Alharthy

General Chemistry (Chem110) Dr. Rima Alharthy General Chemistry (Chem110) Dr. Rima Alharthy Assistant professor in Medicinal and organic synthesis University of Nottingham, UK iaaalharte@kau.edu.sa Building 4 room 204 Office hours (Mondays and Wednesdays

More information

You must check out a Chemistry book from the textbook room for this summer assignment. You may check out books May from the textbook room.

You must check out a Chemistry book from the textbook room for this summer assignment. You may check out books May from the textbook room. Name You must check out a Chemistry book from the textbook room for this summer assignment. You may check out books May 24 27 from the textbook room. There will be 2 summer study sessions for Chemistry

More information

Equations & Quantitative Relationships. + O 2(g)» H 2» 2 H 2

Equations & Quantitative Relationships. + O 2(g)» H 2» 2 H 2 Woods Chem-1 Lec-05 09-2 Stoichiometry (std)+ Page 1 States of matter: (s) (l) (g) (aq) Balancing Equations: Equations & Quantitative Relationships H 2 (g) + O 2(g)» H 2 Can t change H 2 O to H 2 O 2 2

More information

Chemistry 1 Review. 1. Round the following to the correct number of significant figures:

Chemistry 1 Review. 1. Round the following to the correct number of significant figures: Chemistry 1 Review 1. Round the following to the correct number of significant figures: a) 0.00342892 (3 sig. fig.) b) 3423 (2 sig. fig.) c) 144.98 (1 sig. fig.) 2. Make sure the answers to the following

More information

1) Convert the following

1) Convert the following 1) Convert the following 1) 125 g to Kg 6) 26.9 dm 3 to cm 3 11) 1.8µL to cm 3 16) 4.8 lb to Kg 21) 23C to K 1.25 x 10-1 Kg 2) 21.3 Km to cm 2.13 x 10 6 cm 2.69 x 10 3 cm 3 7) 18.2 ml to cm 3 1.82 x 10

More information

Chapter 6 Chemical reactions Classification And Mass Relationships. Chapter 6 1

Chapter 6 Chemical reactions Classification And Mass Relationships. Chapter 6 1 Chapter 6 Chemical reactions Classification And Mass Relationships Chapter 6 1 Chemical reactions and Chemical Equations Balancing Chemical Equations Mole, Avogadro s Number Stoichiometric Problems Percent

More information

Chemistry 1411 Practice Exam 1, Chapters 1-4 Chang

Chemistry 1411 Practice Exam 1, Chapters 1-4 Chang Chemistry 1411 Practice Exam 1, Chapters 1-4 Chang Show your calculations clearly on show work problems. A periodic table is also attached to the end of the exam. Good luck! 1. Give the number of significant

More information

HOMEWORK 4A. Definitions. Oxidation-Reduction Reactions. Questions

HOMEWORK 4A. Definitions. Oxidation-Reduction Reactions. Questions HOMEWORK 4A Oxidation-Reduction Reactions 1. Indicate whether a reaction will occur or not in each of following. Wtiring a balcnced equation is not necessary. (a) Magnesium metal is added to hydrochloric

More information

Chemistry 112 Sample Exam (1st Hour) Harwood KEY

Chemistry 112 Sample Exam (1st Hour) Harwood KEY 1. Phenylalanine is one of the compounds found in low calorie sweeteners. It contains C, H, N, and O. Analysis of a 1.255 g sample of phenylalanine gives 0.8213 g C, 0.1063 g N, and 0.2431 g O. Calculate

More information

Stoichiometry Homework Packet

Stoichiometry Homework Packet Name: Period: Stoichiometry Homework Packet Chapter 16: 16.1 and 16.2 Chapter 11: 11.1 and 11.2 Chapter 12: All sections Upon completion of the Stoichiometry Unit, you should be able to: Explain how a

More information

Gen Chem I Exam 1 Review (Chapters 1 & 2)

Gen Chem I Exam 1 Review (Chapters 1 & 2) Gen Chem I Exam 1 Review (Chapters 1 & 2) 1 Multiple Choice Identify the choice that best completes the statement or answers the question. 1. All of the following are properties of antimony. Which one

More information

IB Chemistry. DP Chemistry Review

IB Chemistry. DP Chemistry Review DP Chemistry Review Topic 1: Quantitative chemistry 1.1 The mole concept and Avogadro s constant Assessment statement Apply the mole concept to substances. Determine the number of particles and the amount

More information

Chemistry 142 Multiple Choice. Fill in your name, section, and student number on Side 1 of the Answer Sheet.

Chemistry 142 Multiple Choice. Fill in your name, section, and student number on Side 1 of the Answer Sheet. Chemistry 142 Multiple Choice (a) Before starting, please check to see that your exam has 6 pages, which includes the periodic table. (b) (c) Fill in your name, section, and student number on Side 1 of

More information

Moles and Stoichiometry

Moles and Stoichiometry Moles and Stoichiometry I. Moles A. Definition. 1. A mole (mol) = 6.022 x 10 23 units. 6.022 x 10 23 = Avogadro's constant, with a dimension of particles mol 1 or mol 1 b. A mass in grams equal to the

More information

1. Hydrobromic acid reacts with aqueous lithium sulfide Molecular Equation

1. Hydrobromic acid reacts with aqueous lithium sulfide Molecular Equation NAME Hr Chapter 4 Aqueous Reactions and Solution Chemistry Practice B (Part 1 = Obj. 1-3) (Part 2 = Obj. 4-6) Objective 1: Electrolytes, Acids, and Bases a. Indicate whether each of the following is strong,

More information

Chapter 3 Mass Relationships in Chemical Reactions

Chapter 3 Mass Relationships in Chemical Reactions Chapter 3 Mass Relationships in Chemical Reactions Student: 1. An atom of bromine has a mass about four times greater than that of an atom of neon. Which choice makes the correct comparison of the relative

More information

AP Chemistry Prep - Summer Assignment 2013

AP Chemistry Prep - Summer Assignment 2013 AP Chemistry Prep - Summer Assignment 2013 Multiple Choice Identify the choice that best completes the statement or answers the question. 1. Which value has only 4 significant digits? a. 6.930 c. 8450

More information

SESSION 14. REVISION TUTORIAL ANSWERS

SESSION 14. REVISION TUTORIAL ANSWERS SESSION 14. REVISION TUTORIAL ANSWERS QUESTION 1. SYMBOLS AND FORMULAS. 1 mark for each answer (a) Give the symbol for the following elements: (i) sodium Na (ii) calcium Ca (iii) strontium Sr (iv) boron

More information

Chemistry Final Exam Review

Chemistry Final Exam Review Name: Date: Block: Chemistry Final Exam Review 2012-2013 Unit 1: Measurement, Numbers, Scientific Notation, Conversions, Dimensional Analysis 1. Write 0.000008732 in scientific notation 8.732x10-6 2. Write

More information

CHAPTER 3 STOICHIOMETRY OF FORMULAS AND EQUATIONS

CHAPTER 3 STOICHIOMETRY OF FORMULAS AND EQUATIONS CHAPTER 3 STOICHIOMETRY OF FORMULAS AND EQUATIONS FOLLOW UP PROBLEMS 3.1A Plan: The mass of carbon must be changed from mg to g. The molar mass of carbon can then be used to determine the number of moles.

More information

Chemistry 65 Chapter 5 COMPOUNDS. Compounds are formed from elements by combining in a definite, fixed composition.

Chemistry 65 Chapter 5 COMPOUNDS. Compounds are formed from elements by combining in a definite, fixed composition. COMPOUNDS Compounds are pure substances that contain 2 or more elements combined in a definite proportion by mass. Compounds have unique properties compared to their component elements. For example, although

More information

Chapter 3 Stoichiometry: Ratios of Combination

Chapter 3 Stoichiometry: Ratios of Combination Chapter 3 Stoichiometry: Ratios of Combination 1 3.1 Molecular and Formula Masses 3.2 Percent Composition of Compounds 3.3 Chemical Equations 3.4 The Mole and Molar Mass 3.5 Combustion Analysis 3.6 Calculations

More information

Summer Assignment Coversheet

Summer Assignment Coversheet Summer Assignment Coversheet Course: A.P. Chemistry Teachers Names: Mary Engels Assignment Title: Summer Assignment A Review Assignment Summary/Purpose: To review the Rules for Solubility, Oxidation Numbers,

More information

4. Aluminum chloride is 20.2% aluminum by mass. Calculate the mass of aluminum in a 35.0 gram sample of aluminum chloride.

4. Aluminum chloride is 20.2% aluminum by mass. Calculate the mass of aluminum in a 35.0 gram sample of aluminum chloride. 1. Calculate the molecular mass of table sugar sucrose (C 12 H 22 O 11 ). A. 342.30 amu C. 320.05 amu B. 160.03 amu D. 171.15 amu 2. How many oxygen atoms are in 34.5 g of NaNO 3? A. 2.34 10 23 atoms C.

More information

Unit 2. Molar Mass Worksheet

Unit 2. Molar Mass Worksheet Unit 2 Molar Mass Worksheet Calculate the molar masses of the following chemicals: 1) Cl 2 8) UF 6 2) KOH 9) SO 2 3) BeCl 2 10) H 3 PO 4 4) FeCl 3 11) (NH 4 ) 2 SO 4 5) BF 3 12) CH 3 COOH 6) CCl 2 F 2

More information

Exam 1, Ch 1-4 September 21, Points

Exam 1, Ch 1-4 September 21, Points Chem 130 Name Exam 1, Ch 1-4 September 21, 2016 100 Points Please follow the instructions for each section of the exam. Show your work on all mathematical problems. Provide answers with the correct units

More information

Review/Chapter 1. A) 1 only B) 2 only C) 3 only D) 1 and 2 E) 1, 2, and 3 ANS: C

Review/Chapter 1. A) 1 only B) 2 only C) 3 only D) 1 and 2 E) 1, 2, and 3 ANS: C Review/Chapter 1 1. What is a scientific theory? A) It is a collection of experimental data. B) It is an assertion of scientific fact. C) It is a guess or conjecture about natural phenomena. D) It is a

More information

B. Elements: We cannot determine how many electrons are lost for the elements b/c their in their valence electrons can change.

B. Elements: We cannot determine how many electrons are lost for the elements b/c their in their valence electrons can change. Unit 6 Notepack: Chapters 9 &10 Chemical Quantities 9.1 Naming Ions NAME Period: A. ions: Ions made of single. B. Elements: There is a pattern in predicting how many electrons are lost and gained for the

More information

Summer Assignment Part 2

Summer Assignment Part 2 Summer Assignment Part 2 Name: 1. Metric Conversions. Remember 1 cm 3 = 1 ml 1 L = 1 dm 3 ITEM GIVEN METRIC UNIT DESIRED METRIC UNIT A 8.43 cm mm B 2.41 x 10 2 cm m C 294.5 nm cm D 1.445 x 10 4 m km E

More information

PART I: MULTIPLE CHOICE (30 multiple choice questions. Each multiple choice question is worth 2 points)

PART I: MULTIPLE CHOICE (30 multiple choice questions. Each multiple choice question is worth 2 points) CHEMISTRY 123-07 Midterm #1 Answer key October 14, 2010 Statistics: Average: 74 p (74%); Highest: 97 p (95%); Lowest: 33 p (33%) Number of students performing at or above average: 67 (57%) Number of students

More information

1. [7 points] Which one of the following choices has the element symbol and name correctly matched?

1. [7 points] Which one of the following choices has the element symbol and name correctly matched? Avogadro s Number, N A = 6.022 10 23 1. [7 points] Which one of the following choices has the element symbol and name correctly matched? (a) P, potassium (b) C, copper (c) Mg, manganese (d) Ag, silver

More information

Chapter 4 Solution Chemistry

Chapter 4 Solution Chemistry Chapter 4 Solution Chemistry Solution Stoichiometry Many reactions (biochemical, marine, etc.) take place in solution. We need to be able to express the number of moles of particles in a certain volume

More information

Year 9 Extra Credit Assignment

Year 9 Extra Credit Assignment Complete the following problem by the Strategy: A. Balance the chemical equation for the reaction (see study guide. B. Use the given densities to convert from volume to mass. Then use each molar mass to

More information

DAWSON COLLEGE DEPARTMENT OF CHEMISTRY & CHEMICAL TECHNOLOGY SOLUTIONS TO PRACTICE FINAL EXAMINATION INTRODUCTION TO COLLEGE CHEMISTRY

DAWSON COLLEGE DEPARTMENT OF CHEMISTRY & CHEMICAL TECHNOLOGY SOLUTIONS TO PRACTICE FINAL EXAMINATION INTRODUCTION TO COLLEGE CHEMISTRY DAWSON COLLEGE DEPARTMENT OF CHEMISTRY & CHEMICAL TECHNOLOGY SOLUTIONS TO PRACTICE FINAL EXAMINATION INTRODUCTION TO COLLEGE CHEMISTRY Solutions Print your Name: Student Number: INSTRUCTORS: Please circle

More information

6/27/2014. Periodic Table of the ELEMENTS. Chemical REACTIONS you should know. Brief Review for 1311 Honors Exam 2

6/27/2014. Periodic Table of the ELEMENTS. Chemical REACTIONS you should know. Brief Review for 1311 Honors Exam 2 Brief Review for 3 Honors Exam 2 Chapter 2: Periodic Table I. Metals. Representative Metals Alkali Metals Group Alkaline Earth Metals. Group 2 2. Transition Metals II. Metalloids Chapter 3: All Chapter

More information

Welcome to AP Chemistry

Welcome to AP Chemistry Dear AP Chemistry Student: Welcome to AP Chemistry 20152016 We hope you are ready for a fun, yet challenging year. AP Chemistry involves really understanding chemistry concepts and being able to apply

More information

Atoms, Molecules, and Ions (Chapter 2) Old Quiz and Test Questions Answer Key

Atoms, Molecules, and Ions (Chapter 2) Old Quiz and Test Questions Answer Key Atoms, Molecules, and Ions (Chapter 2) Old Quiz and Test Questions Answer Key 1. a. Give the name and symbol for one alkaline earth metal. Choose from any element in Group 2: Be, Mg, Ca, Sr, Ba, Ra b.

More information

Oxidation and Reduction Questions

Oxidation and Reduction Questions Oxidation and Reduction Questions 1 2CO + O 2 = 2CO 2 In the above reaction the oxidation number of carbon changes from (1) +2 to +1 (2) +2 to +4 (3) +4 to +1 (4) +4 to +2 2 Which metal will react spontaneously

More information

2. Draw the Bohr-Rutherford diagrams for the following Ions: S 2-, Al +3, Li +1, P -3

2. Draw the Bohr-Rutherford diagrams for the following Ions: S 2-, Al +3, Li +1, P -3 1. Complete the following table: ATOMIC STRUCTURE Name Symbol # protons # neutrons # electrons Net charge Sodium ion Na +1 +1 Oxygen atom Gold ion +3 C Cl -1 Cesium ion +1 12 +2 16-2 18 +1 10 0 Ba +2 Helium

More information

2. [7 points] What is the empirical formula of the ionic compound that forms between calcium and iodine?

2. [7 points] What is the empirical formula of the ionic compound that forms between calcium and iodine? Avogadro s Number, N A = 6.022 10 23 1. [7 points] Which of the following statements is true? (a) Air is an element (b) Air is a compound (c) Air is a heterogeneous mixture (d) Air is a homogeneous mixture

More information

Chapter 3. Stoichiometry: Ratios of Combination. Insert picture from First page of chapter. Copyright McGraw-Hill 2009 1

Chapter 3. Stoichiometry: Ratios of Combination. Insert picture from First page of chapter. Copyright McGraw-Hill 2009 1 Chapter 3 Insert picture from First page of chapter Stoichiometry: Ratios of Combination Copyright McGraw-Hill 2009 1 3.1 Molecular and Formula Masses Molecular mass - (molecular weight) The mass in amu

More information

MOLE. Chapter #3 : Stoichiometry. Mole - Mass Relationships of Elements

MOLE. Chapter #3 : Stoichiometry. Mole - Mass Relationships of Elements Chapter #3 : Stoichiometry MOLE The Mole is based upon the definition: The amount of substance that contains as many elementary parts (atoms, molecules, or other?) as there are atoms in exactly 12 grams

More information

CDO AP Chemistry Unit 1 Review 2

CDO AP Chemistry Unit 1 Review 2 1. Why is it that the vast majority of alpha particles that traveled through the gold foil in Rutherford s experiment experienced no deflection? 2. Describe the results of the experiment that proved electrons

More information

Chapter 5 Molecules and Compounds

Chapter 5 Molecules and Compounds Chemistry 25 Chapter 5 Molecules and Compounds Molecules and Compounds Salt Sodium Chlorine Sugar Carbon Hydrogen Oxygen 1 Law of Constant Composition All pure substances have constant composition. All

More information

MOLE CONVERSION PROBLEMS. 2. How many moles are present in 34 grams of Cu(OH) 2? [0.35 moles]

MOLE CONVERSION PROBLEMS. 2. How many moles are present in 34 grams of Cu(OH) 2? [0.35 moles] MOLE CONVERSION PROBLEMS 1. What is the molar mass of MgO? [40.31 g/mol] 2. How many moles are present in 34 grams of Cu(OH) 2? [0.35 moles] 3. How many moles are present in 2.5 x 10 23 molecules of CH

More information

Chemistry 100 Practice Final Exam. Do not begin the exam until you have been instructed to do so. You have 120 minutes to complete this exam.

Chemistry 100 Practice Final Exam. Do not begin the exam until you have been instructed to do so. You have 120 minutes to complete this exam. Chemistry 100 Practice Final Exam Instructions: Do not begin the exam until you have been instructed to do so. You have 120 minutes to complete this exam. There are 50 multiple choice questions. You must

More information

Mole - Mass Relationships in Chemical Systems

Mole - Mass Relationships in Chemical Systems Chapter 3: Stoichiometry Mole - Mass Relationships in Chemical Systems 3.1 The Mole 3.2 Determining the Formula of an Unknown Compound 3.3 Writing and Balancing Chemical Equations 3.4 Calculating the Amounts

More information

1. Balance the following equation. What is the sum of the coefficients of the reactants and products?

1. Balance the following equation. What is the sum of the coefficients of the reactants and products? 1. Balance the following equation. What is the sum of the coefficients of the reactants and products? 1 Fe 2 O 3 (s) + _3 C(s) 2 Fe(s) + _3 CO(g) a) 5 b) 6 c) 7 d) 8 e) 9 2. Which of the following equations

More information

Formulae, stoichiometry and the mole concept

Formulae, stoichiometry and the mole concept 3 Formulae, stoichiometry and the mole concept Content 3.1 Symbols, Formulae and Chemical equations 3.2 Concept of Relative Mass 3.3 Mole Concept and Stoichiometry Learning Outcomes Candidates should be

More information

Molecular Formula: Example

Molecular Formula: Example Molecular Formula: Example A compound is found to contain 85.63% C and 14.37% H by mass. In another experiment its molar mass is found to be 56.1 g/mol. What is its molecular formula? 1 CHAPTER 3 Chemical

More information

produce whole numbers but they should do (allowing for the low relative mass of the electron). This was explained when the

produce whole numbers but they should do (allowing for the low relative mass of the electron). This was explained when the Atomic Structure 28 THE STRUCTURE OF ATOMS ATOMS Atoms consist of a number of fundamental particles, the most important ones are... Mass / kg Charge / C Relative mass Relative Charge PROTON NEUTRON ELECTRON

More information

4. During respiration, glucose reacts with oxygen gas to produce carbon dioxide and water. Write a balanced equation:

4. During respiration, glucose reacts with oxygen gas to produce carbon dioxide and water. Write a balanced equation: Name: Date: Unit 7B - Stoichiometry Accelerated Chemistry I Mole Ratios 1. This balanced equation shows reaction of carbon monoxide reacts with oxygen gas: 2CO(g) + O 2 (g) 2CO 2 (g) a. What is the ratio

More information

2 Which electron configurations represent the first two elements in Group 17 (VIIA) of the Periodic Table?

2 Which electron configurations represent the first two elements in Group 17 (VIIA) of the Periodic Table? CHE-100 Review Questions 1 The total number of orbitals found in an f sublevel is A) 5 B) 3 C) 7 D) 1 2 Which electron configurations represent the first two elements in Group 17 (VIIA) of the Periodic

More information

Chemistry 101 Chapter 4 STOICHIOMETRY

Chemistry 101 Chapter 4 STOICHIOMETRY STOICHIOMETRY Stoichiometry is the quantitative relationship between the reactants and products in a balanced chemical equation. Stoichiometry allows chemists to predict how much of a reactant is necessary

More information

Atoms, Molecules and Ions

Atoms, Molecules and Ions Atoms, Molecules and Ions Chapter 2 Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. Dalton s Atomic Theory (1808) 1. Elements are composed of extremely small

More information

Unit 10A Stoichiometry Notes

Unit 10A Stoichiometry Notes Unit 10A Stoichiometry Notes Stoichiometry is a big word for a process that chemist s use to calculate amounts in reactions. It makes use of the coefficient ratio set up by balanced reaction equations

More information

Date: October 31, 2016 Objective: Name binary ionic compounds. Add ionic charges to your Periodic Table:

Date: October 31, 2016 Objective: Name binary ionic compounds. Add ionic charges to your Periodic Table: Do Now Date: October 31, 2016 Objective: Name binary ionic compounds. Add ionic charges to your Periodic Table: Quick practice Classify as ionic or covalent: CaCl 2 H 2 O KI NaCl Ca 2+ Ionic compounds

More information

IB Chemistry 1 Mole. One atom of C-12 has a mass of 12 amu. One mole of C-12 has a mass of 12 g. Grams we can use more easily.

IB Chemistry 1 Mole. One atom of C-12 has a mass of 12 amu. One mole of C-12 has a mass of 12 g. Grams we can use more easily. The Mole Atomic mass units and atoms are not convenient units to work with. The concept of the mole was invented. This was the number of atoms of carbon-12 that were needed to make 12 g of carbon. 1 mole

More information

Chemistry EOC Practice Test #1

Chemistry EOC Practice Test #1 Chemistry EOC Practice Test #1 1. Which of these would be best to measure 12.6 ml of liquid ethanol? A. 25 ml beaker B. 25 ml volumetric flask C. 25 ml Erlenmeyer flask D. 25 ml graduated cylinder 2. Potassium

More information

CH 221 Chapter Two Part 2 Concept Guide

CH 221 Chapter Two Part 2 Concept Guide CH 221 Chapter Two Part 2 Concept Guide 1. Ion Charges What charge are the following ions expected to have? (a) ionic barium (b) ionic oxygen (c) ionic potassium (a) Barium is expected to form cations.

More information

2. In a double displacement reaction, 3. In the chemical equation, H 2 O 2 H 2 + O 2, the H 2 O 2 is a

2. In a double displacement reaction, 3. In the chemical equation, H 2 O 2 H 2 + O 2, the H 2 O 2 is a What are the missing coefficients for the skeleton equation below? Al 2 (SO 4 ) 3 + KOH Al(OH) 3 + K 2 SO 4 2. In a double displacement reaction, A. 1,6,2,3 B. 2,12,4,6 C. 1,3,2,3 D. 4,6,2,3 E. 2,3,1,1

More information

21 st Century Chemistry Multiple Choice Question in Topic 3 Metals Unit 11

21 st Century Chemistry Multiple Choice Question in Topic 3 Metals Unit 11 21 st Century Chemistry Multiple Choice Question in Topic 3 Metals Unit 11 1. Consider the equation: 2Ca(s) + O 2 (g) 2CaO(s) Which of the following statements are correct? (1) Calcium and oxygen are reactants.

More information

Sample Exercise 4.1 Relating Relative Numbers of Anions and Cations to Chemical Formulas

Sample Exercise 4.1 Relating Relative Numbers of Anions and Cations to Chemical Formulas Sample Exercise 4.1 Relating Relative Numbers of Anions and Cations to Chemical Formulas The diagram on the right represents an aqueous solution of one of the following compounds: MgCl 2, KCl, or K 2 SO

More information

FINAL EXAM CHEM 1310 FS11 VERSION GREEN

FINAL EXAM CHEM 1310 FS11 VERSION GREEN FINAL EXAM CHEM 1310 FS11 VERSION GREEN Name: 1. How many liters of chlorine gas at 25 C and 0.950 atm can be produced by the reaction of 12.0 g of MnO 2? MnO 2 (s) + 4HCl(aq) MnCl 2 (aq) + 2H 2 O(l) +

More information

Chemical Reactions. Chemical equation

Chemical Reactions. Chemical equation Handout Kimia Dasar I 2013/2014 Chemical Reactions Chemical equation All chemical reactions take place according to a set of general principles that relate the amounts of materials consumed in a reaction

More information

More on ions (Chapters 2.1 and )

More on ions (Chapters 2.1 and ) More on ions (Chapters 2.1 and 3.5 3.7) Ion: an atom or molecule that has a net electrical charge. Examples: Na + (sodium ion), Cl - (chloride), NH 4 + (ammonium). Anion: a negative ion, formed when electrons

More information

Chapter 2 Stoichiometry describes the quantitative relationships among elements

Chapter 2 Stoichiometry describes the quantitative relationships among elements Chapter 2 Stoichiometry describes the quantitative relationships among elements 1. in compounds (composition stoichiometry) 2. in chemical changes (reaction stoichiometry) Dalton s Atomic Theory summarized

More information

W1 WORKSHOP ON STOICHIOMETRY

W1 WORKSHOP ON STOICHIOMETRY INTRODUCTION W1 WORKSHOP ON STOICHIOMETRY These notes and exercises are designed to introduce you to the basic concepts required to understand a chemical formula or equation. Relative atomic masses of

More information

Chapter 3: Stoichiometry

Chapter 3: Stoichiometry Chapter 3: Stoichiometry Goal is to understand and become proficient at working with: 1. Avogadro's Number, molar mass and converting between mass and moles (REVIEW). 2. empirical formulas from analysis.

More information

Chemistry Chapter 7. Chemical Formulas and Chemical Compounds

Chemistry Chapter 7. Chemical Formulas and Chemical Compounds Chemistry Chapter 7 Chemical Formulas and Chemical Compounds Heart cell rhythm depends on the opening and closing of a complex series of valves on the cell membrane, called ion channels. Some valves let

More information

Chapter 7. Writing Formulas and Naming Compounds. Chemistry

Chapter 7. Writing Formulas and Naming Compounds. Chemistry Chapter 7 Writing Formulas and Naming Compounds Chemistry Systematic Naming There are too many compounds to remember the names of all of the known compounds. Compounds are made of two or more elements.

More information

Chapter 6 Oxidation-Reduction Reactions. Section 6.1 2. Which one of the statements below is true concerning an oxidation-reduction reaction?

Chapter 6 Oxidation-Reduction Reactions. Section 6.1 2. Which one of the statements below is true concerning an oxidation-reduction reaction? Chapter 6 Oxidation-Reduction Reactions 1. Oxidation is defined as a. gain of a proton b. loss of a proton c. gain of an electron! d. loss of an electron e. capture of an electron by a neutron 2. Which

More information

Chemistry Bridging Task PLC

Chemistry Bridging Task PLC Name: Chemistry Bridging Task PLC Checklist questions: Can you... C R State the fundamental charges in an atom, their relative charges and masses Draw the electronic configuration of a given atom State

More information

Predicting Products Look at the following reactions and do the following:

Predicting Products Look at the following reactions and do the following: Predicting Products Look at the following reactions and do the following: 1) Identify the reaction as C, S, D, SD, DD, or AB 2) If it is a S or D, identify it as: a. hydroxide b. carbonate c. chlorate

More information

H 2 O. Chapter 9 Chemical Names and Formulas

H 2 O. Chapter 9 Chemical Names and Formulas H 2 O Chapter 9 Chemical Names and Formulas Section 9.1: Naming Ions OBJECTIVES: Identify the charges on monatomic ions by using the periodic table, and name the ions. Define a polyatomic ion and write

More information

Chapter 8. Chemical Equations and Reactions

Chapter 8. Chemical Equations and Reactions Chapter 8 Chemical Equations and Reactions Section 8 1 Describing Chemical Reactions Chemical Reaction the process by which one or more substances are changed into one more different substances. Reactants

More information

CHEM J-2 June /01(a) What is the molarity of the solution formed when 0.50 g of aluminium fluoride is dissolved in ml of water?

CHEM J-2 June /01(a) What is the molarity of the solution formed when 0.50 g of aluminium fluoride is dissolved in ml of water? CHEM1001 2014-J-2 June 2014 22/01(a) What is the molarity of the solution formed when 0.50 g of aluminium fluoride is dissolved in 800.0 ml of water? 2 The molar mass of AlF 3 is: molar mass = (26.98 (Al)

More information

SCH 3UI Unit 7 Outline Stoichiometry. Stoichiometry 1: Mole Mole Problems. Stoichiometry II: Mass Problems. Stoichiometry III: Volume of Gas Problems

SCH 3UI Unit 7 Outline Stoichiometry. Stoichiometry 1: Mole Mole Problems. Stoichiometry II: Mass Problems. Stoichiometry III: Volume of Gas Problems SCH 3UI Unit 7 Outline Stoichiometry Lesson Topics Covered Handouts to Print 1 Note: Stoichiometry definition the meaning of the coefficients in balanced chemical reactions mole mole calculations Stoichiometry

More information

TOPIC 9. CHEMICAL CALCULATIONS III - stoichiometry.

TOPIC 9. CHEMICAL CALCULATIONS III - stoichiometry. TOPIC 9. CHEMICAL CALCULATIONS III - stoichiometry. Stoichiometric calculations. By combining a knowledge of balancing equations with the concept of the mole, it is possible to easily calculate the masses

More information

Chemical Change:

Chemical Change: Section 1: Vocabulary Review Use the spaces provided below to give brief (but accurate!) definitions for each term. Besides past notes and work, your textbook is a great resource for finding definitions.

More information

Chapter 8 Chemical Quantities

Chapter 8 Chemical Quantities Chapter 8 Chemical Quantities Introductory Info The atomic masses of the elements on the periodic table are in the units. These measurements are based on the mass of the standard isotope of the element,

More information

Crucible and Lid Evaporating Dish Stirring Rod Bunsen Burner. Beaker Graduated Cylinder Test Tube Erlenmeyer Flask

Crucible and Lid Evaporating Dish Stirring Rod Bunsen Burner. Beaker Graduated Cylinder Test Tube Erlenmeyer Flask Midterm Review: Due 15-11 111 You will use your class notes, lab materials, and class work assignments to complete the following Midterm Review. Lab Equipment Sketch the piece of lab equipment in each

More information

Stoichiometry Notes. Review of Moles. Determine the molar mass of Ca 3 (PO 4 ) 2. How many moles of H 2 O are in 9.87 grams of H 2 O?

Stoichiometry Notes. Review of Moles. Determine the molar mass of Ca 3 (PO 4 ) 2. How many moles of H 2 O are in 9.87 grams of H 2 O? Stoichiometry Notes Review of Moles Determine the molar mass of Ca 3 (PO 4 ) 2 How many moles of H 2 O are in 9.87 grams of H 2 O? How many molecules are in 87.9 grams of nitrogen dioxide? How many oxygen

More information

midterm1, 2009 Name: Class: Date:

midterm1, 2009 Name: Class: Date: Class: Date: midterm1, 2009 Record your name on the top of this exam and on the scantron form. Record the test ID letter in the top right box of the scantron form. Record all of your answers on the scantron

More information

Name: Chemistry. Introduction to Inorganic and Physical Chemistry

Name: Chemistry. Introduction to Inorganic and Physical Chemistry Name: Chemistry Introduction to Inorganic and Physical Chemistry Terminology Term atom ion molecule element compound relative atomic mass, Ar relative formula mass, Mr formula unit molar mass, Mr mole,

More information

Name : ( ) Class: 3 Date :

Name : ( ) Class: 3 Date : Name : ( ) Class: 3 Date : Topic 7.2 : The From Equation Syllabus Objectives : (a) Define relative atomic mass, A r (b) Define relative molecular mass, M r, and calculate relative molecular mass (and relative

More information

1. Identify the mass law that the following observation demonstrates. (1 pt)

1. Identify the mass law that the following observation demonstrates. (1 pt) Quiz 2 Take out 1 sheet of paper and your calculator (remove covers). Please place all books on the floor. You have 10 minutes from START. Show all work to get points. Please stop when asked to stop. 1.

More information

10/21/2013. Chemical REACTIONS you should know. Chemical Reactions. 1 st Write Reaction

10/21/2013. Chemical REACTIONS you should know. Chemical Reactions. 1 st Write Reaction Chapter 3: Chemical Stoichiometry Chemical Equations (Write, Balance, Interpret) Reactions You Should Know Formula Weights (Must know chemical formula Avogadro s number and the Mole Limiting Reactants

More information

SCH 4C1 Unit 2 Problem Set Questions taken from Frank Mustoe et all, "Chemistry 11", McGraw-Hill Ryerson, 2001

SCH 4C1 Unit 2 Problem Set Questions taken from Frank Mustoe et all, Chemistry 11, McGraw-Hill Ryerson, 2001 SCH 4C1 Unit 2 Problem Set Questions taken from Frank Mustoe et all, "Chemistry 11", McGraw-Hill Ryerson, 2001 1. A small pin contains 0.0178 mol of iron. How many atoms of iron are in the pin? 2. A sample

More information

Solve The diagram shows twice as many cations as anions, consistent with the formulation K 2 SO 4.

Solve The diagram shows twice as many cations as anions, consistent with the formulation K 2 SO 4. Sample Exercise 4.1 Relating Relative Numbers of Anions and Cations to Chemical Formulas The accompanying diagram represents an aqueous solution of either MgCl 2, KCl, or K 2 SO 4. Which solution does

More information

Chem I Final Review Worksheet Name Hour Chem 1Review

Chem I Final Review Worksheet Name Hour Chem 1Review Name Hour Chem 1Review 1. Write the number of protons for each of the metalloids in their boxes. 2. Color the metals blue. 3. Color the non-metals yellow. 4. Label the groups with their numbers. 5. Label

More information

Q1. The chart shows the processes involved in the manufacture of nitric acid from ammonia.

Q1. The chart shows the processes involved in the manufacture of nitric acid from ammonia. Chemistry C2 Foundation and Higher Questions Q1. The chart shows the processes involved in the manufacture of nitric acid from ammonia. (a) Complete the word equation for the reaction that takes place

More information

6. What is the mass of a phosphorus sample which contains moles of phosphorus atoms? a g b g c g d g e. 34.

6. What is the mass of a phosphorus sample which contains moles of phosphorus atoms? a g b g c g d g e. 34. General Chemistry 1. Fall 2006. Exam 1. October 30, 2006. 64 points total. Choose the best answer for questions 1-20. You must show your work for all questions to receive credit. Be sure to include units

More information

Big Bang Theory Experiment Hypothesis Variable

Big Bang Theory Experiment Hypothesis Variable Chemistry Semester 1 Course Review Unit 1 : Nature of Science Scientific method Significant figures Metric system Base units Big Bang Theory Experiment Hypothesis Variable Control Accuracy Precision 1.

More information

2014 Spring CHEM101 Ch1-2 Review Worksheet Modified by Dr. Cheng-Yu Lai,

2014 Spring CHEM101 Ch1-2 Review Worksheet Modified by Dr. Cheng-Yu Lai, Ch1 1) Which of the following underlined items is not an intensive property? A) A chemical reaction requires 3.00 g of oxygen. B) The density of helium at 25 C is 1.64 10-4 g/cm3. C) The melting point

More information

AP Chemistry Chemical Equations Worksheet

AP Chemistry Chemical Equations Worksheet Name: AP Chemistry Chemical Equations Worksheet Write the balanced chemical equation (excluding spectator ions) underneath each reaction description, and answer the question. (a) A solution of ammonia

More information

Stoichiometry Chapter 9 Assignment & Problem Set

Stoichiometry Chapter 9 Assignment & Problem Set Stoichiometry Name Warm-Ups (Show your work for credit) Date 1. Date 2. Date 3. Date 4. Date 5. Date 6. Date 7. Date 8. Stoichiometry 2 Study Guide: Things You Must Know Vocabulary (know the definition

More information

CHEMICAL QUANTITIES. Chapter 10

CHEMICAL QUANTITIES. Chapter 10 CHEMICAL QUANTITIES Chapter 10 What is a mole? A unit of measurement in chemistry 1 mole of a substance = 6.02 x 10 23 (Avagadro s number) representative particles of a substance Representative particle

More information

Reactions. Balancing Chemical Equations uses Law of conservation of mass: matter cannot be lost in any chemical reaction

Reactions. Balancing Chemical Equations uses Law of conservation of mass: matter cannot be lost in any chemical reaction Reactions Chapter 8 Combustion Decomposition Combination Chapter 9 Aqueous Reactions Exchange reactions (Metathesis) Formation of a precipitate Formation of a gas Formation of a week or nonelectrolyte

More information