AP WORKSHEET 00a: Significant Figures
|
|
|
- Jeremy Cooper
- 7 years ago
- Views:
Transcription
1 AP WORKSHEET 00a: Significant Figures 1. Determine the number of significant figures in each of the following. (6) (a) (b) (c) (d) (e) 1.09 x 10 4 (f) Use a calculator to find the results of the following and then round the answer to the correct number of significant figures. (6) (a) (b) (c) (d) (e) (f) State the significant figure rule that is associated with captive zeros. (1) 4. State the significant figure rule that is associated with leading zeros. (1) 5. State the significant figure rule that is associated with trailing zeros. (1) 6. State the significant figure rule that is associated with addition and subtraction operations. (1) 7. State the significant figure rule that is associated with multiplication and division operations. (1) 1
2 8. Use a calculator to find the results of the following calculations and then round the answer to the correct number of significant figures. (6) (a) 12 x (b) (1.23 x 10 3 ) x (6.4 x 10 2 ) (c) x (d) 34 / 22 (e) (1.8 x 10 5 ) / 14 (f) / Round each of the following to three significant figures. (6) (a) (b) (c) (d) (e) (f) How many significant figures in each of the following? (6) (a) nm (b) 6.02 x particles (c) g (d) 13 neutrons (e) mg (f) g 2
3 AP WORKSHEET 00b: Unit Conversions This worksheet utilizes the conversions given at this web site 1. Perform the following conversions. In each case show the full, dimensional analysis. Source any conversion factors from the web site above. An example is given below. (6) Question: 3.00 cm to mm. Answer: 3.00 cm 10 mm 1 cm = 30 mm (a) 120 J to MJ (b) 3 m to cm (c) 400 miles to km (d) 25 hectares to acres (e) 34 inches to ft (f) 289 s to hrs 2. Perform the following conversions. In each case you do NOT need to show the full, dimensional analysis. Source any conversion factors from the web site above. (6) (a) J to kj (b) 13 kg to lbs (c) 83.2 K to o C (d) 48 mins to ms (e) 34 o F to o C (f) 13.2 kg to lbs 1
4 3. Perform the following sequences of conversions. In each case show the full, dimensional analysis. Source any conversion factors from the web site above. An example is given below. (6) Question: 3.00 cm to m VIA mm. Answer: 3.00 cm 10 mm m = 0.03 m 1 cm 1 mm (a) 679 nm to cm VIA m (b) 23 miles to m VIA km (c) 567 feet to m VIA yd (d) 12 L to UK gal VIA ml (e) 8 MJ to J VIA kj (f) 418 s to hrs VIA min 2
5 AP WORKSHEET 00c: Atomic Structure & Ions Use the periodic table here; to help you answer this worksheet. 1. What is the charge on a sodium atom? (1) 2. What is the charge on a sodium nucleus? (1) 3. What is the atomic number of potassium? (1) 4. How many protons are there in the nucleus of a potassium atom? (1) 5. How many electrons in the potassium nucleus? (1) 6. What is the most likely charge (the most common charge) on an ion of sulfur? (1) 7. If a chloride ion and a strontium ion were to form a compound, what would its formula be? (1) 8. What do all the ions of the transition metals have in common with one another? (1) 1
6 AP WORKSHEET 00d: Elements & Symbols Although you will always have access to a periodic table in tests and exams, the periodic table will NOT have element names on it. In that light it will be extremely helpful to you if you can begin to recognize as many of the element names and symbols as possible. 1. Assign the 50 elements below to one of the four lists based upon their symbols. (50) List A: Elements that have symbols that are only the first letter of the element's name List B: Elements that have symbols that are the first two letters of the element's name List C: Elements that have symbols that are the first letter and another letter of the element s name List D: Elements that have symbols that are rooted in another language or other source ELEMENT NAME ELEMENT SYMBOL LIST A, B, C or D? aluminum antimony argon arsenic barium beryllium bismuth boron bromine cadmium calcium carbon cerium cesium chlorine chromium cobalt copper fluorine gallium gold helium hydrogen iodine iron 1
7 ELEMENT NAME ELEMENT SYMBOL LIST A, B, C or D? lead lithium magnesium manganese mercury neon nickel oxygen phosphorus platinum potassium radium selenium silicon silver sodium strontium sulfur tin titanium tungsten uranium vanadium xenon zinc 2. Using the periodic table, find one more (i.e. not those listed in question #1.) element for each list. (4) A. B. C. D. 2
8 AP WORKSHEET 00e: Inorganic Nomenclature I 1. The following compounds are all binary compounds. Give the name of each one. (6) (a) SrO (b) K 2 O (c) Na 2 S (d) Cs 3 P (e) AlCl 3 (f) Mg 3 N 2 2. Some of the following name and formula combinations are incorrect. Identify the correct combinations. For the others, suggest corrected combinations. (13) (a) barium hydroxide, BaOH 2 (b) sodium oxide, SoO 2 (c) barium chloride, BCl 3 (d) strontium oxide SrO 2 (e) boron trifluoride, BoFl 6 (f) vanadium (III) chloride, VCl 3 (g) magnesium oxide, MgO 4 3. Write the name of the following compounds. Use Roman numerals in the names. (7) (a) FeI 3 (b) MnCl 2 (c) HgO (d) Cu 2 S (e) CuS (f) SnI 4 (g) MnBr 2 1
9 4. Write the name of each of the following. To help get the correct name, use the periodic table to determine which elements are metals, which are non-metals and which compounds should include Roman numerals in their names. (16) (a) N 2 Br 5 (b) P 2 S 5 (c) Ge 2 O 3 (d) N 2 O 5 (e) SiO 2 (f) AlH 3 (g) FeO (h) CuCl 2 (i) OCl 2 (j) XeF 6 (k) RaCl 2 (l) SeCl 2 (m) PCl 5 (n) Na 3 P (o) CuF (p) V 2 O 5 2
10 AP WORKSHEET 00f: Inorganic Nomenclature II Add either a name or a formula to complete each table. (100) 1. Potassium dichromate 2. Lithium sulfide 3. Potassium bromide 4. Cesium iodide 5. Calcium phosphide 6. Sodium fluoride 7. Strontium oxide 8. Beryllium sulfide 9. Magnesium bromide 10. Lithium oxide 11. Strontium chloride 12. Barium bromide 13. Magnesium sulfide 14. Magnesium iodide 15. Hydrogen fluoride (Hydrogen monofluoride) 16. Barium phosphide 17. Sodium hydrogen phosphate 18. Potassium chloride 19. Lithium nitride 20. Calcium sulfide 21. Rubidium oxide 22. Strontium nitride 23. Cesium phosphide 24. Magnesium carbonate 25. Beryllium sulfate 1
11 26. Dinitrogen Tetraoxide 27. Carbon dioxide 28. Mercury(I) chloride 29. Hydroiodic acid 30. Iodic acid 31. Perbromic acid 32. Hypobromous acid 33. Phosphorus pentachloride 34. Iodine monochloride 35. Antimony(III) fluoride 36. Bromine monofluoride 37. Bromine dioxide 38. Dinitrogen pentoxide 39. Carbon monosulfide 40. Tellurium dioxide 41. Phosphorus tribromide 42. Carbon tetraiodide 43. Vanadium(V) chromate 44. Zinc carbonate 45. Silver hydroxide 46. Vanadium(III) chromate 47. Mercury(II) iodide 48. Uranium(V) nitrate 49. Nickel (III) nitride 50. Sulfuric acid 2
12 51. ScCl HCl 53. PtO Sb(ClO 3 ) GeS ZnO 57. VSO CuCl TiO NiN 61. Ni 3 (PO 4 ) CoF Au 2 O Zn 3 P Cr(NO 3 ) NaIO NaIO NaI 69. H 2 SO H 2 CO AlN 72. AlH Li 3 AsO NaCN 75. Na 2 O 2 3
13 76. Li 3 PO KHCO HF 79. AuI KMnO Na 2 Cr 2 O Ag 2 CrO AgCl 84. NaCH 3 COO 85. RaF KSCN 87. FeS 88. Fe 2 (SO 3 ) FeSO MgS 91. Na 2 S 2 O RbCl 93. Cu(OH) Mg 3 N Cu 3 N 96. LiH 97. K 2 O 98. K 2 O Li 3 N 100. DsCl 3 4
14 AP WORKSHEET 00s: Preamble Summary 1. Classify the following as either chemical or physical changes. (3) (a) Ice melting (b) Gasoline burning (c) Evaporation of perfume from an open bottle 2. Mercury is a liquid metal that has a density of g/ml. Calculate the volume of mercury that must be poured out in order to obtain g of Mercury. (2) 3. Classify the following as either quantitative or qualitative observations. (4) (a) My eyes are brown (b) My neck size is 17 inches (c) My average grade last year was 79% (d) Physics is a difficult subject 4. Give an example of a natural law (other than the law of conservation of mass). (1) 5. Convert these numbers to scientific notation. (2) (a) (b)
15 6. Round the following numbers to four figures. (6) (a) x 10 5 (b) x 10 6 (c) (d) (e) (f) Perform the following conversions. (5) (a) 0.75 kg to milligrams (b) 1500 millimeters to km (c) 2390 g to kg (d) 0.52 km to meters (e) 65 kg to g 8. Complete the following table of temperatures, performing the appropriate conversions. (18) Kelvin Fahrenheit Celsius
16 9. An experiment is performed in which the molar mass of a gas is found to be g mol -1. The published (actual) value is g mol -1. Calculate the percentage error. (2) 10. Distinguish carefully between precision and accuracy. (2) 11. In the table below, match the scientist with the experiment. (2) Scientist Crookes Millikan Rutherford Experiment Oil Drop Cathode Ray Gold Foil 12. Consider the following pairs; does either pair represent a pair of isotopes? Explain. (4) (a) 11 Na 23 and 11 Na 24 (b) 11 Na 24 and 12 Mg Determine the number of protons, electrons and neutrons in each of the following isotopes. (3) (a) 79 Au 171 (b) 79 Au 182 (c) 35 Br
17 14. In the following question give the missing formula or name. (10) Formula Name CaS Pb 3 N 2 AlP HBrO 4 (NH 4 ) 2 CO 3 Calcium ethanoate Phosphorous pentachloride Strontium bromite Potassium hydrogen carbonate Chloric acid 4
47374_04_p25-32.qxd 2/9/07 7:50 AM Page 25. 4 Atoms and Elements
47374_04_p25-32.qxd 2/9/07 7:50 AM Page 25 4 Atoms and Elements 4.1 a. Cu b. Si c. K d. N e. Fe f. Ba g. Pb h. Sr 4.2 a. O b. Li c. S d. Al e. H f. Ne g. Sn h. Au 4.3 a. carbon b. chlorine c. iodine d.
Monatomic Ions. A. Monatomic Ions In order to determine the charge of monatomic ions, you can use the periodic table as a guide:
Monatomic Ions Ions are atoms that have either lost or gained electrons. While atoms are neutral, ions are charged particles. A loss of electrons results in a positive ion or cation (pronounced cat-eye-on
Naming Compounds Handout Key
Naming Compounds Handout Key p. 2 Name each of the following monatomic cations: Li + = lithium ion Ag + = silver ion Cd +2 = cadmium ion Cu +2 = copper (II) ion Al +3 = aluminum ion Mg +2 = magnesium ion
Nomenclature Packet. 1. Name the following ionic compounds: a. Al 2 O 3 Aluminum oxide. b. Cs 2 O Cesium oxide. c. Rb 3 N Rubidium nitride
Nomenclature Packet Worksheet I: Binary Ionic Compounds (representative metals) metals from groups 1A, 2A, and 3A (1, 2, and 13) have constant charges as ions and do NOT get Roman Numerals in their names
B) atomic number C) both the solid and the liquid phase D) Au C) Sn, Si, C A) metal C) O, S, Se C) In D) tin D) methane D) bismuth B) Group 2 metal
1. The elements on the Periodic Table are arranged in order of increasing A) atomic mass B) atomic number C) molar mass D) oxidation number 2. Which list of elements consists of a metal, a metalloid, and
Moles, Molecules, and Grams Worksheet Answer Key
Moles, Molecules, and Grams Worksheet Answer Key 1) How many are there in 24 grams of FeF 3? 1.28 x 10 23 2) How many are there in 450 grams of Na 2 SO 4? 1.91 x 10 24 3) How many grams are there in 2.3
Problem Solving. Mole Concept
Skills Worksheet Problem Solving Mole Concept Suppose you want to carry out a reaction that requires combining one atom of iron with one atom of sulfur. How much iron should you use? How much sulfur? When
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
neutrons are present?
AP Chem Summer Assignment Worksheet #1 Atomic Structure 1. a) For the ion 39 K +, state how many electrons, how many protons, and how many 19 neutrons are present? b) Which of these particles has the smallest
Naming Compounds. There are three steps involved in naming ionic compounds- naming the cation, naming the anion, and naming the entire compound.
Naming Compounds Naming compounds is an important part of chemistry. Most compounds fall in to one of three categories ionic compounds, molecular compounds, or acids. Part One: Naming Ionic Compounds Identifying
CHM 1311: General Chemistry 1, Fall 2004 Exam #1, September 8, 2004. Name (print) SSN
CHM 1311: General Chemistry 1, Fall 2004 Exam #1, September 8, 2004 Name (print) SSN Pledge: I have neither given nor received aid on this exam: Signature For ALL problems: SHOW ALL WORK TO GET FULL CREDIT
Decomposition. Composition
Decomposition 1. Solid ammonium carbonate is heated. 2. Solid calcium carbonate is heated. 3. Solid calcium sulfite is heated in a vacuum. Composition 1. Barium oxide is added to distilled water. 2. Phosphorus
CHEMICAL NAMES AND FORMULAS
9 CHEMICAL NAMES AND FORMULAS SECTION 9.1 NAMING IONS (pages 253 258) This section explains the use of the periodic table to determine the charge of an ion. It also defines polyatomic ion and gives the
Periodic Table Questions
Periodic Table Questions 1. The elements characterized as nonmetals are located in the periodic table at the (1) far left; (2) bottom; (3) center; (4) top right. 2. An element that is a liquid at STP is
Exercise 3.5 - Naming Binary Covalent Compounds:
Chapter Exercise Key 1 Chapter Exercise Key Exercise.1 Classifying Compounds: Classify each of the following substances as either a molecular compound or an ionic compound. a. formaldehyde, CH 2 O (used
Chapter 2 Atoms, Ions, and the Periodic Table
Chapter 2 Atoms, Ions, and the Periodic Table 2.1 (a) neutron; (b) law of conservation of mass; (c) proton; (d) main-group element; (e) relative atomic mass; (f) mass number; (g) isotope; (h) cation; (i)
Chemistry CP Unit 2 Atomic Structure and Electron Configuration. Learning Targets (Your exam at the end of Unit 2 will assess the following:)
Chemistry CP Unit 2 Atomic Structure and Electron Learning Targets (Your exam at the end of Unit 2 will assess the following:) 2. Atomic Structure and Electron 2-1. Give the one main contribution to the
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
CHAPTER 9. 9.1 Naming Ions. Chemical Names and Formulas. Naming Transition Metals. Ions of Transition Metals. Ions of Transition Metals
CHAPTER 9 Chemical Names and Formulas 9.1 Naming Ions Monatomic Ions: a single atom with a positive or negative charge Cation (rules): listed first Anion (rules): ide ending Transition Metals have a varying
Periodic Table, Valency and Formula
Periodic Table, Valency and Formula Origins of the Periodic Table Mendelѐѐv in 1869 proposed that a relationship existed between the chemical properties of elements and their atomic masses. He noticed
Balancing Chemical Equations Worksheet
Balancing Chemical Equations Worksheet Student Instructions 1. Identify the reactants and products and write a word equation. 2. Write the correct chemical formula for each of the reactants and the products.
Name: Block: Date: Test Review: Chapter 8 Ionic Bonding
Name: Block: Date: Test Review: Chapter 8 Ionic Bonding Part 1: Fill-in-the-blank. Choose the word from the word bank below. Each word may be used only 1 time. electron dot structure metallic electronegativity
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
Topic 4 National Chemistry Summary Notes. Formulae, Equations, Balancing Equations and The Mole
Topic 4 National Chemistry Summary Notes Formulae, Equations, Balancing Equations and The Mole LI 1 The chemical formula of a covalent molecular compound tells us the number of atoms of each element present
Nomenclature and Formulas of Ionic Compounds. Section I: Writing the Name from the Formula
Purpose: Theory: Nomenclature and Formulas of Ionic Compounds 1. To become familiar with the rules of chemical nomenclature, based on the classification of compounds. 2. To write the proper name of the
Sample Exercise 2.1 Illustrating the Size of an Atom
Sample Exercise 2.1 Illustrating the Size of an Atom The diameter of a US penny is 19 mm. The diameter of a silver atom, by comparison, is only 2.88 Å. How many silver atoms could be arranged side by side
UNIT (2) ATOMS AND ELEMENTS
UNIT (2) ATOMS AND ELEMENTS 2.1 Elements An element is a fundamental substance that cannot be broken down by chemical means into simpler substances. Each element is represented by an abbreviation called
= 11.0 g (assuming 100 washers is exact).
CHAPTER 8 1. 100 washers 0.110 g 1 washer 100. g 1 washer 0.110 g = 11.0 g (assuming 100 washers is exact). = 909 washers 2. The empirical formula is CFH from the structure given. The empirical formula
MOLES AND MOLE CALCULATIONS
35 MOLES ND MOLE CLCULTIONS INTRODUCTION The purpose of this section is to present some methods for calculating both how much of each reactant is used in a chemical reaction, and how much of each product
Study Guide For Chapter 7
Name: Class: Date: ID: A Study Guide For Chapter 7 Multiple Choice Identify the choice that best completes the statement or answers the question. 1. The number of atoms in a mole of any pure substance
Calculating Molar Mass of a Compound
Instructions for Conversion Problems For every conversion problem Write the number in the problem down with unit and a multiplication sign Decide which conversion factor you should use, Avagadro s or molar
Nomenclature of Ionic Compounds
Nomenclature of Ionic Compounds Ionic compounds are composed of ions. An ion is an atom or molecule with an electrical charge. Monatomic ions are formed from single atoms that have gained or lost electrons.
Naming and Writing Formulas for Ionic Compounds Using IUPAC Rules
Naming and Writing Formulas for Ionic Compounds Using IUPAC Rules There are three categories of ionic compounds that we will deal with. 1.Binary ionic o simple ions (only single charges) o multivalent
CHAPTER 5: MOLECULES AND COMPOUNDS
CHAPTER 5: MOLECULES AND COMPOUNDS Problems: 1-6, 9-13, 16, 20, 31-40, 43-64, 65 (a,b,c,e), 66(a-d,f), 69(a-d,f), 70(a-e), 71-78, 81-82, 87-96 A compound will display the same properties (e.g. melting
APPENDIX B: EXERCISES
BUILDING CHEMISTRY LABORATORY SESSIONS APPENDIX B: EXERCISES Molecular mass, the mole, and mass percent Relative atomic and molecular mass Relative atomic mass (A r ) is a constant that expresses the ratio
Molar Mass Worksheet Answer Key
Molar Mass Worksheet Answer Key Calculate the molar masses of the following chemicals: 1) Cl 2 71 g/mol 2) KOH 56.1 g/mol 3) BeCl 2 80 g/mol 4) FeCl 3 162.3 g/mol 5) BF 3 67.8 g/mol 6) CCl 2 F 2 121 g/mol
CHAPTER 2 ATOMS AND THE ATOMIC THEORY
1A 1B 2A 2B A CHAPTER 2 ATOMS AND THE ATOMIC THEORY PRACTICE EXAMPLES The total mass must be the same before and after reaction. mass before reaction = 0.82 g magnesium + 2.652 g nitrogen =.04 g mass after
2. John Dalton did his research work in which of the following countries? a. France b. Greece c. Russia d. England
CHAPTER 3 1. Which combination of individual and contribution is not correct? a. Antoine Lavoisier - clarified confusion over cause of burning b. John Dalton - proposed atomic theory c. Marie Curie - discovered
Solution. Practice Exercise. Concept Exercise
Example Exercise 8.1 Evidence for a Reaction Which of the following is experimental evidence for a chemical reaction? (a) Pouring vinegar on baking soda gives foamy bubbles. (b) Mixing two solutions produces
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
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
Chemistry Post-Enrolment Worksheet
Name: Chemistry Post-Enrolment Worksheet The purpose of this worksheet is to get you to recap some of the fundamental concepts that you studied at GCSE and introduce some of the concepts that will be part
Naming Ionic Compounds Answer Key
Naming Ionic Compounds Answer Key Give the name of the following ionic compounds: Name 1) Na 2 CO 3 sodium carbonate 2) NaOH sodium hydroxide 3) MgBr 2 magnesium bromide 4) KCl potassium chloride 5) FeCl
Atomic Structure. Name Mass Charge Location Protons 1 +1 Nucleus Neutrons 1 0 Nucleus Electrons 1/1837-1 Orbit nucleus in outer shells
Atomic Structure called nucleons Name Mass Charge Location Protons 1 +1 Nucleus Neutrons 1 0 Nucleus Electrons 1/1837-1 Orbit nucleus in outer shells The number of protons equals the atomic number This
Electrons in Atoms & Periodic Table Chapter 13 & 14 Assignment & Problem Set
Electrons in Atoms & Periodic Table Name Warm-Ups (Show your work for credit) Date 1. Date 2. Date 3. Date 4. Date 5. Date 6. Date 7. Date 8. Electrons in Atoms & Periodic Table 2 Study Guide: Things You
Find a pair of elements in the periodic table with atomic numbers less than 20 that are an exception to the original periodic law.
Example Exercise 6.1 Periodic Law Find the two elements in the fifth row of the periodic table that violate the original periodic law proposed by Mendeleev. Mendeleev proposed that elements be arranged
Multiple Choice Identify the letter of the choice that best completes the statement or answers the question.
Introduction to Chemistry Exam 2 Practice Problems 1 Multiple Choice Identify the letter of the choice that best completes the statement or answers the question. 1.Atoms consist principally of what three
Untitled Document. 1. Which of the following best describes an atom? 4. Which statement best describes the density of an atom s nucleus?
Name: Date: 1. Which of the following best describes an atom? A. protons and electrons grouped together in a random pattern B. protons and electrons grouped together in an alternating pattern C. a core
Name period AP chemistry Unit 2 worksheet Practice problems
Name period AP chemistry Unit 2 worksheet Practice problems 1. What are the SI units for a. Wavelength of light b. frequency of light c. speed of light Meter hertz (s -1 ) m s -1 (m/s) 2. T/F (correct
Chemical Composition Review Mole Calculations Percent Composition. Copyright Cengage Learning. All rights reserved. 8 1
Chemical Composition Review Mole Calculations Percent Composition Copyright Cengage Learning. All rights reserved. 8 1 QUESTION Suppose you work in a hardware store and a customer wants to purchase 500
The Mole. Chapter 2. Solutions for Practice Problems
Chapter 2 The Mole Note to teacher: You will notice that there are two different formats for the Sample Problems in the student textbook. Where appropriate, the Sample Problem contains the full set of
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
Problem Solving. Percentage Composition
Skills Worksheet Problem Solving Percentage Composition Suppose you are working in an industrial laboratory. Your supervisor gives you a bottle containing a white crystalline compound and asks you to determine
ATOMS A T O M S, I S O T O P E S, A N D I O N S. The Academic Support Center @ Daytona State College (Science 120, Page 1 of 39)
ATOMS A T O M S, I S O T O P E S, A N D I O N S The Academic Support Center @ Daytona State College (Science 120, Page 1 of 39) THE ATOM All elements listed on the periodic table are made up of atoms.
PERIODIC TABLE OF THE ELEMENTS
PERIODIC TABLE OF THE ELEMENTS Periodic Table: an arrangement of elements in horizontal rows (Periods) and vertical columns (Groups) exhibits periodic repetition of properties First Periodic Table: discovered
Monday 25 June 2012 Afternoon
THIS IS A NEW SPECIFICATION H Monday 25 June 2012 Afternoon GCSE TWENTY FIRST CENTURY SCIENCE CHEMISTRY A A172/02 Modules C4 C5 C6 (Higher Tier) *A135370612* Candidates answer on the Question Paper. A
Tuesday 22 January 2013 Morning
THIS IS A NEW SPECIFICATION H Tuesday 22 January 2013 Morning GCSE TWENTY FIRST CENTURY SCIENCE CHEMISTRY A A172/02 Modules C4 C5 C6 (Higher Tier) *A135780113* Candidates answer on the Question Paper.
Unit 9 Stoichiometry Notes (The Mole Continues)
Unit 9 Stoichiometry Notes (The Mole Continues) 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
Stoichiometry Review
Stoichiometry Review There are 20 problems in this review set. Answers, including problem set-up, can be found in the second half of this document. 1. N 2 (g) + 3H 2 (g) --------> 2NH 3 (g) a. nitrogen
Description of the Mole Concept:
Description of the Mole Concept: Suppose you were sent into the store to buy 36 eggs. When you picked them up you would get 3 boxes, each containing 12 eggs. You just used a mathematical device, called
Naming Ionic Compounds
Naming Ionic Compounds I. Naming Ions A. Cations (+ions) 1. Element name followed by "ion" (when in Group IA, IIA, Al 3+, Ga 3+, Zn 2+, Cd 2+, Ag +, Ni 2+ ). Na + sodium ion, K + potassium ion, Al 3+ aluminum
NAMING QUIZ 3 - Part A Name: 1. Zinc (II) Nitrate. 5. Silver (I) carbonate. 6. Aluminum acetate. 8. Iron (III) hydroxide
NAMING QUIZ 3 - Part A Name: Write the formulas for the following compounds: 1. Zinc (II) Nitrate 2. Manganese (IV) sulfide 3. Barium permanganate 4. Sulfuric acid 5. Silver (I) carbonate 6. Aluminum acetate
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
XIX. Chemistry, High School
XIX. Chemistry, High School High School Chemistry Test The spring 05 high school Chemistry test was based on learning standards in the Chemistry content strand of the Massachusetts Science and Technology/Engineering
David A. Katz Chemist, Educator, Science Communicator, and Consultant Department of Chemistry, Pima Community College
WRITING CHEMICAL EQUATIONS 2004, 2002, 1989 by David A. Katz. All rights reserved. Permission for classroom used provided original copyright is included. David A. Katz Chemist, Educator, Science Communicator,
Solution. Practice Exercise. Concept Exercise
Example Exercise 9.1 Atomic Mass and Avogadro s Number Refer to the atomic masses in the periodic table inside the front cover of this textbook. State the mass of Avogadro s number of atoms for each of
7) How many electrons are in the second energy level for an atom of N? A) 5 B) 6 C) 4 D) 8
HOMEWORK CHEM 107 Chapter 3 Compounds Putting Particles Together 3.1 Multiple-Choice 1) How many electrons are in the highest energy level of sulfur? A) 2 B) 4 C) 6 D) 8 2) An atom of phosphorous has how
Chapter 8 Atomic Electronic Configurations and Periodicity
Chapter 8 Electron Configurations Page 1 Chapter 8 Atomic Electronic Configurations and Periodicity 8-1. Substances that are weakly attracted to a magnetic field but lose their magnetism when removed from
7.4. Using the Bohr Theory KNOW? Using the Bohr Theory to Describe Atoms and Ions
7.4 Using the Bohr Theory LEARNING TIP Models such as Figures 1 to 4, on pages 218 and 219, help you visualize scientific explanations. As you examine Figures 1 to 4, look back and forth between the diagrams
Chem 1100 Chapter Three Study Guide Answers Outline I. Molar Mass and Moles A. Calculations of Molar Masses
Chem 1100 Chapter Three Study Guide Answers Outline I. Molar Mass and Moles A. Calculations of Molar Masses B. Calculations of moles C. Calculations of number of atoms from moles/molar masses 1. Avagadro
CHEM 1411 General Chemistry I Practice Problems, Chapters 1 3
CHEM 1411 General Chemistry I Practice Problems, Chapters 1 3 Chapter 1 Chemistry: The Study of Change 1. Element, compound, homogeneous mixture (solution), or heterogeneous mixture: a) orange juice b)
19.2 Chemical Formulas
In the previous section, you learned how and why atoms form chemical bonds with one another. You also know that atoms combine in certain ratios with other atoms. These ratios determine the chemical formula
WRITING CHEMICAL FORMULA
WRITING CHEMICAL FORMULA For ionic compounds, the chemical formula must be worked out. You will no longer have the list of ions in the exam (like at GCSE). Instead you must learn some and work out others.
Writing and Balancing Chemical Equations
Name Writing and Balancing Chemical Equations Period When a substance undergoes a chemical reaction, chemical bonds are broken and new bonds are formed. This results in one or more new substances, often
Chemistry: Chemical Equations
Chemistry: Chemical Equations Write a balanced chemical equation for each word equation. Include the phase of each substance in the equation. Classify the reaction as synthesis, decomposition, single replacement,
1332 CHAPTER 18 Sample Questions
1332 CHAPTER 18 Sample Questions Couple E 0 Couple E 0 Br 2 (l) + 2e 2Br (aq) +1.06 V AuCl 4 + 3e Au + 4Cl +1.00 V Ag + + e Ag +0.80 V Hg 2+ 2 + 2e 2 Hg +0.79 V Fe 3+ (aq) + e Fe 2+ (aq) +0.77 V Cu 2+
Polyatomic Ions Worksheet. 2. Name or write the formula for the following Type I polyatomic ionic compounds
Polyatomic Ions Worksheet Polyatomic Practice 1. Name or write the formula for the following polyatomic ions sulfate - CO nitrite MnO perphosphate - SO hypoiodite BrO chlorite - CO phosphite - PO percarbonate
Oxidation States of Nitrogen
Oxidation States of Nitrogen HNO 3 NH 3 HNO 2 NO N 2 O N 2 HN 3 N 2 H 5 + +3 +2 +1 0-1/3-2 Oxidation +5-3 Reduction Oxidation States of Chlorine HClO 4 HClO 3 ClO 2 HClO 2 HClO Cl 2 HCl +5 +4 +3 +1 0 Oxidation
Chapter 6 Notes Science 10 Name:
6.1 Types of Chemical Reactions a) Synthesis (A + B AB) Synthesis reactions are also known as reactions. When this occurs two or more reactants (usually elements) join to form a. A + B AB, where A and
Chapter 11. Electrochemistry Oxidation and Reduction Reactions. Oxidation-Reduction Reactions. Oxidation-Reduction Reactions
Oxidation-Reduction Reactions Chapter 11 Electrochemistry Oxidation and Reduction Reactions An oxidation and reduction reaction occurs in both aqueous solutions and in reactions where substances are burned
Polyatomic ions can form ionic compounds just as monatomic ions.
1 POLYATOMIC IONS We have seen that atoms can lose or gain electrons to become ions. Groups of atoms can also become ions. These groups of atoms are called polyatomic ions. Examples: O hydroxide ion NO
Success criteria You should be able to write the correct formula for any ionic compound
Chemical Formulas and Names of Ionic Compounds WHY? Going back to pre-historic times, humans have experimented with chemical processes that helped them to make better tools, pottery and weapons. In the
Monday 25 June 2012 Afternoon
THIS IS A NEW SPECIFICATION F Monday 25 June 2012 Afternoon GCSE TWENTY FIRST CENTURY SCIENCE CHEMISTRY A A172/01 Modules C4 C5 C6 (Foundation Tier) *A135360612* Candidates answer on the Question Paper.
TOPIC 7. CHEMICAL CALCULATIONS I - atomic and formula weights.
TOPIC 7. CHEMICAL CALCULATIONS I - atomic and formula weights. Atomic structure revisited. In Topic 2, atoms were described as ranging from the simplest atom, H, containing a single proton and usually
Tuesday 22 January 2013 Morning
THIS IS A NEW SPECIFICATION F Tuesday 22 January 2013 Morning GCSE TWENTY FIRST CENTURY SCIENCE CHEMISTRY A A172/01 Modules C4 C5 C6 (Foundation Tier) *A135770113* Candidates answer on the Question Paper.
Unit 3 Study Guide: Electron Configuration & The Periodic Table
Name: Teacher s Name: Class: Block: Date: Unit 3 Study Guide: Electron Configuration & The Periodic Table 1. For each of the following elements, state whether the element is radioactive, synthetic or both.
MODERN ATOMIC THEORY AND THE PERIODIC TABLE
CHAPTER 10 MODERN ATOMIC THEORY AND THE PERIODIC TABLE SOLUTIONS TO REVIEW QUESTIONS 1. Wavelength is defined as the distance between consecutive peaks in a wave. It is generally symbolized by the Greek
AP Chemistry Reaction Questions
AP Chemistry Reaction Questions Directions: Give the formulas to show the reactants and the products for the following chemical reactions. Each of the reactions occurs in aqueous solution unless otherwise
Unit 3 Notepack Chapter 7 Chemical Quantities Qualifier for Test
Unit 3 Notepack Chapter 7 Chemical Quantities Qualifier for Test NAME Section 7.1 The Mole: A Measurement of Matter A. What is a mole? 1. Chemistry is a quantitative science. What does this term mean?
Chapter 1 The Atomic Nature of Matter
Chapter 1 The Atomic Nature of Matter 6. Substances that cannot be decomposed into two or more simpler substances by chemical means are called a. pure substances. b. compounds. c. molecules. d. elements.
Chemical Proportions in Compounds
Chapter 6 Chemical Proportions in Compounds Solutions for Practice Problems Student Textbook page 201 1. Problem A sample of a compound is analyzed and found to contain 0.90 g of calcium and 1.60 g of
b. N 2 H 4 c. aluminum oxalate d. acetic acid e. arsenic PART 2: MOLAR MASS 2. Determine the molar mass for each of the following. a. ZnI 2 b.
CHEMISTRY DISCOVER UNIT 5 LOTS OF PRACTICE ON USING THE MOLE!!! PART 1: ATOMIC MASS, FORMULA MASS, OR MOLECULAR MASS 1. Determine the atomic mass, formula mass, or molecular mass for each of the following
The Periodic Table: Periodic trends
Unit 1 The Periodic Table: Periodic trends There are over one hundred different chemical elements. Some of these elements are familiar to you such as hydrogen, oxygen, nitrogen and carbon. Each one has
Instructions Answer all questions in the spaces provided. Do all rough work in this book. Cross through any work you do not want to be marked.
GCSE CHEMISTRY Higher Tier Chemistry 1H H Specimen 2018 Time allowed: 1 hour 45 minutes Materials For this paper you must have: a ruler a calculator the periodic table (enclosed). Instructions Answer all
(b) Formation of calcium chloride:
Chapter 2: Chemical Compounds and Bonding Section 2.1: Ionic Compounds, pages 22 23 1. An ionic compound combines a metal and a non-metal joined together by an ionic bond. 2. An electrostatic force holds
Balancing Chemical Equations Practice
Science Objectives Students will describe what reactants and products in a chemical equation mean. Students will explain the difference between coefficients and subscripts in chemical equations. Students
Chemistry Themed. Types of Reactions
Chemistry Themed Types of Reactions 1 2 Chemistry in the Community-2015-2016 Types of Reactions Date In-Class Assignment Homework T 10/20 TEST on Reactivity of Metals and Redox None W 10/21 Late Start
Problem Solving. Mole Concept
Skills Worksheet Problem Solving Mole Concept Suppose you want to carry out a reaction that requires combining one atom of iron with one atom of sulfur. How much iron should you use? How much sulfur? When
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
Chapter 4 Compounds and Their Bonds
Chapter 4 Compounds and Their Bonds 4.1 Octet Rule and Ions Octet Rule An octet is 8 valence electrons. is associated with the stability of the noble gases. He is stable with 2 valence electrons (duet).