First Semester Final Exam Study Guide
|
|
- Dustin Turner
- 5 years ago
- Views:
Transcription
1 First Semester Final Exam Study Guide Name: Chemistry multiple choice questions Chapter 4 1. Explain the law of conservation of mass. 2. What mass of product is produced in the following reaction? 2 grams H2 + 3 grams Cl2 3. Complete the chart. Subatomic Particle Charge Size Location in Atom 4. Which subatomic particle makes up most of an atom s mass? 5. Most of an atoms volume is really what? 6. Define isotope and give an example. 7. Why is the atomic mass of a given element usually NOT listed on the periodic table as a whole number? 8. What particle does the atomic number listed on the periodic table represent, and where does this particle reside? Page 1
2 9. Write the equation that relates the mass # to the number of protons and neutrons in the nucleus of an atom. 10. Calculate the number of protons, neutrons and electrons in a atom of Potassium, K? 11. What is the atomic mass and the atomic number of lead, Pb? 12. Which atom has a great atomic mass: Silver or Arsenic? 13. Which element on the periodic table has the atomic number of 17? 14. Which of the following are isotopes of each other? (CIRCLE ALL THAT APPLY) Ca-40 Cr-50 Cr-53 Cu-63 Fe What is the atomic mass of an atom that has 30 neutrons and 25 protons? Chapter Fill in the orbital diagram below for Tungsten and then write the full electron configuration below. W: Page 2
3 17. Which of the following is an incorrect orbital diagram? Why? 18. Write the unabbreviated electron configuration for the following atoms: a) Helium b) Oxygen c) Aluminum d) Neon 19. Write the abbreviated electron configuration for the following atoms: a) Silver b) Copper c) Tungsten d) Titanium 20. Define ground state. 21. Define excited state. Page 3
4 22. How do atoms jump from ground state to excited state and back? 23. Which atomic particle changes energy states? 24. Label the number total number of electrons at each energy level for each elements below: MAGNESIUM ARGON ZINC -which of the above is also an alkaline earth metal? -which of the above is unreactive? Chapter Define period. 26. Define group. What is another name for group? 27. Define electronegativity. How is it used to determine bonds? 28. Define atomic radius. 29. Define ionization energy. Page 4
5 30. Label the following on the attached periodic table (at the end of SG): 1) Atomic radius trend 2) Electronegativity trend 3) Ionization energy trend 4) Alkali metals 5) Alkaline earth metals 6) Halogens 7) Noble gases 8) Actinides 9) Lanthanides 10) Metals 11) Nonmetals 12) Metalloids Chapter 7 & How is an ion different from an atom? 32. Define cation and give an example. 33. Define anion and give an example. 34. Compare and contrast ionic and covalent bonds. 35. How many electrons are shared in a covalent bond? 36. Define octet rule. Which family on the period table has a complete octet and thus does not react to form compounds? 37. Define valence electron. 38. How many valence electrons do the following atoms have: a) Magnesium b) Bromine c) Calcium d) Phosphorous Page 5
6 39. The electron configuration of oxygen is 1s 2 2s 2 2p 4. How many more electrons does oxygen need to satisfy the octet rule? Chapter Name the following ionic compounds. a) Al(SO4)2 b) PbF4 c) KBr2 d) Ca(OH)2 e) Mg(NO2)2 41. Write the formula for the following ionic compounds. a) Magnesium chlorate b) Potassium cyanide c) Tin (IV) chloride d) Zinc nitrate e) Calcium chlorite 42. Name the following covalent (in other words molecular) compounds. a) As3P5 b) IF7 c) NO2 d) CO e) SiCl4 Page 6
7 43. Write the formula for the following covalent (molecular) compounds. a) dinitrogen pentoxide b) carbon monoxide c) trisulfur difluoride d) triarsenic pentanitride e) dihydrogen monoxide Chapter Circle the subscripts in the following chemical formula. K 2 SO What information does a subscript reveal and how would changing a subscript in a chemical formula change the chemical it represents? 46. Define molar mass. 47. Calculate the molar mass of the following: a) Au = b) H2O = c) Mg(MnO4)2 = d) CH3CH2COOH = Page 7
8 48. Define molecular formula. 49. Define empirical formula. 50. What is the empirical formula for C6H12? 51. What is the empirical formula for C11H22O11? 52. Calculate the percent composition of each element in the following compounds: a) potassium cyanide, KCN b) butane, C4H10 c) sulfuric acid, H2SO4 53. Find the empirical formula of a compound that is % iron and % sulfur. 54. Calculate the empirical formula of a compound containing 1.0 g K, 0.70 g Cr, and 0.82 g of O. Page 8
9 55. A white powder is analyzed and found to have an empirical formula of P2O5. The compound has a molar mass of g/mol. What is the compound s molecular formula? 56. A compound with the empirical formula CH4O was found to have a molar mass of approximately 192 g/mol. What is the molecular formula of the compound? 57. How many atoms are there in a mole of gold? 58. Convert 3.5 moles of nickel into atoms. 59. How many moles are in 1.20 x atoms of Zinc? 60. What is the mass of 5 moles of C6H12O6, glucose? 61. How many grams are in 3 moles of HCl, hydrochloric acid? 62. How many moles are in 1 gram sample of gold? Page 9
10 63. A scientist has a sample of magnesium that has a mass of 5 grams. How many atoms of magnesium does the scientist have? Chapter 11 & Define product. 65. Define reactant. 66. Label the products and reactants in the following chemical reactions: H2 (g) + O2 (g) H2O (l) Copper sulfate (aq) + iron (s) iron sulfate (aq) + copper (s) H2O + CO2 + light C6H12O6 + O2 67. What is changed when balancing a chemical equation? 68. Identify the type of reaction and balance: a) Al + NaOH Na3AlO3 + H2 b) C12H22O11 + O2 CO2 + H2O c) Ca + H2SO4 CaSO4 + H2 d) CaCl2 + NaCO3 NaCl + CaCO3 Page 10
11 69. Predict the products and balance these chemical reactions: a) Cu(NO3)2 + K b) SiF4 + NaOH c) MnO2 + K d) K + Cl2 e) C2H8 + O2 70. Define limiting reactant. 71. Define excess reactant. 72. Mg(OH)2 + 2 HCl MgCl2 + 2 H2O If the reaction begins with 25.44g of Mg(OH)2, what mass of H2O is produced from the reaction? Page 11
12 73. 6 Li + Ca3(PO4)2 2 Li3PO4 + 3 Ca If the reaction above produced 84.3 grams of calcium, what mass of lithium was used to start the reaction? 74. Ba3(PO4)2 + 6 KCl 3 BaCl2 + 2 K3PO4 The above reaction begins with 3.71 g of Ba3(PO4)2 and 3.71 g of KCl. What is the limiting reactant? What is the excess reactant? N2H4 + N2O4 3 N2 + 4 H2O The above reaction begins with g of N2H4 and g of N2O4, what is the limiting reactant? If the reaction actually produces 190.4g of N2, what is the percent yield? Na + Cl2 2 NaCl If 17 grams of Na and 17 grams of Cl2 reaction, what mass of NaCl will be made? Page 12
13 Page 13
First Semester Final Exam Study Guide
First Semester Final Exam Study Guide Name: Chemistry 1 2 3 4 5 6 7 60 multiple choice questions Chapter 1 1. Define matter and list five examples. Chapter 2 2. Define pure substance. 3. Define element.
More informationGeneral Chemistry First Semester Final Exam Study Guide 60 multiple choice questions
General Chemistry First Semester Final Exam Study Guide 60 multiple choice questions 1. Define product. 2. Define reactant. 3. Label the products and reactants in the following chemical reactions: H 2
More informationFinal Exam Study Guide Honors Chemistry Semester Multiple Choice Questions
Final Exam Study Guide Honors Chemistry Semester 1 2017 60 Multiple Choice Questions Name: Students should be able to: Convert between metric units Convert between scientific notation and expanded (decimal)
More informationChemistry 1-2E Semester I Study Guide
Chemistry 1-2E Semester I Study Guide Name Hour Chapter 1 1. Define the following terms. Matter Mass Law of Conservation of Mass 2. Define and give 2 examples of the following: Pure substance Element Compound
More informationUnit 1 Study Guide Chemistry. Subatomic particle Charge Relative size
VOCABULARY define the following terms: Unit 1 Study Guide Chemistry 1) Atomic mass- 2) Atomic number- 3) Proton- 4) Neutron- 5) Electron- 6) Electron configuration- 7) Isotope 8) Ion 9) Anion 10) Cation
More information1. Dimensional Analysis: convert the following values a. 47,340 cm to m Unit 1: Chemistry Matters b. 40.64 km to m c. 58,700 ml to L 2. Calculate the number of significant figures a. 0.0210 b. 3.6056 c.
More informationChemistry Unit 1: Matter Outcome Study Guide
1. Define: Chemistry Unit 1: Matter Outcome Study Guide Effective nuclear charge Ionization energy Electron affinity Electronegativity Anion Cation Valence electron Isoelectronic Ion Isotope Orbital Intermolecular
More informationCP Chemistry Final Exam Review
I. Matter and Measurement 1) Chemical or physical property? CP Chemistry Final Exam Review Diamond is a very hard substance. The density of aluminum is 2.7 g/cm 3. Zinc reacts with acid. Copper melts at
More informationCP Chemistry Final Exam Review
I. Matter and Measurement 1) Chemical or physical property? CP Chemistry Final Exam Review Diamond is a very hard substance. The density of aluminum is 2.7 g/cm 3. Zinc reacts with acid. Copper melts at
More informationA. ATOMS Name Period Date 1. Complete the following table. Element Symbol Number of Protons. Number of electrons Ac 227
A. ATOMS Name Period Date 1. Complete the following table. Element Symbol Number of Protons Number of electrons Number of neutrons Atomic Number 25 53 11 12 35 45 Mass Number 39 89 33 75 Ac 227 2. Fill
More informationVOCABULARY define the following terms:
VOCABULARY define the following terms: Unit 1 Study Guide Honors Chem 1) Electron configuration- 2) Effective nuclear charge 3) Isotope 4) Ion 5) Anion 6) Cation - 7) Isoelectronic - 8) Halogens 9) Electronegativity
More informationVOCABULARY define the following terms:
VOCABULARY define the following terms: Unit 1 Study Guide Honors Chem 1) Electron configuration- 2) Effective nuclear charge 3) Isotope 4) Ion 5) Anion 6) Cation - 7) Isoelectronic - 8) Halogens 9) Electronegativity
More informationSophomore AP Chem Practice Problems
Due on 8/17/18 Sophomore AP Chem Practice Problems Scientific notation and significant figures Determine the number of Significant Figures in the following numbers: 00034 2431. 8900 0.0094 Convert the
More informationWP Unit 2 Practice: The Atom
WP Unit 2 Practice: The Atom Name 1. Name, and identify them clearly in your answer, one halogen, one noble gas, one alkali metal, one alkali earth metal, one metalloid, one transition metal and finally
More informationACP Chemistry (821) - Mid-Year Review
ACP Chemistry (821) - Mid-Year Review *Be sure you understand the concepts involved in each question. Do not simply memorize facts!* 1. What is chemistry? Chapter 1: Chemistry 2. What is the difference
More informationAn Incomplete Study Guide For The First Semester Exam
An Incomplete Study Guide For The First Semester Exam Dr Mandes 1. 2. Which term refers to the number of protons in an atom? a. atomic mass b. atomic number c. isotopic mass d. proton number A cation is
More informationAP CHEMISTRY THINGS TO KNOW
AP CHEMISTRY THINGS TO KNOW Diatomic Molecules H2-hydrogen gas (do not write H) N2-nitrogen gas (do no write N) O2-oxygen gas (do not write O) F2-fluorine gas (do not write F) Cl2-chlorine gas (do not
More informationFinal Exam Review Questions You will be given a Periodic Table, Activity Series, and a Common Ions Chart CP CHEMISTRY
Final Exam Review Questions You will be given a Periodic Table, Activity Series, and a Common Ions Chart CP CHEMISTRY Part A True-False State whether each statement is true or false. If false, correct
More informationCa K C Ne Sb Rb Te Be Si Cl
Station 1. Ionic Charge Review Using your periodic table complete the questions below. Part 1: Determine the # of valence electrons for each element. Phosphorus Bromine Xenon Nitrogen Halogens Alkali metals
More informationRegents Chemistry Unit 3- Bonding, Moles & Stoichiometry Study Guide & Pre-Test KEY
Name: Regents Chemistry Unit 3- Bonding, Moles & Stoichiometry Study Guide & Pre-Test KEY Focus Questions for the Unit: How are compounds different... from elements?... from mixtures? What role do valence
More informationReview Multiple Choice Questions
Chapter 2 Matter and Changes Review Multiple Choice Questions 1. The random molecular motion of a substance is greatest when the substance is a. condensed b. a liquid c. frozen d. a gas 2. After elements
More informationCounting by mass: The Mole. Unit 8: Quantification of Chemical Reactions. Calculating molar mass. Particles. moles and mass. moles and particles
Unit 8: Quantification of Chemical Reactions Chapter 10: The mole Chapter 12: Stoichiometry Counting by mass: The Mole Chemists can t count individual atoms Use moles to determine amounts instead mole
More informationb. Na. d. So. 1 A basketball has more mass than a golf ball because:
Chem I Semester Review All of the following are general characteristics of a substance in the liquid state except a. definite volume. c. not easily compressed. b. able to flow. d. definite shape. In the
More informationChem 101 Review. Fall 2012
Chem 101 Review Fall 2012 Elements, Atoms, Ions Elements in nature symbols Constant composition chemical formula Dalton s atomic theory Atomic structure what makes up the atom ions isotopes Periodic table
More informationSCI-CH Chem Test II fall 2018 Exam not valid for Paper Pencil Test Sessions
SCI-CH Chem Test II fall 2018 Exam not valid for Paper Pencil Test Sessions [Exam ID:25FPCV 1 When a strontium atom loses its valence electrons, it has the same electron configuration as which element?
More information1st Semester Review Worth 10% of Exam Score
1st Semester Review 2014-2015 Worth 10% of Exam Score Name: P: 1. Which of the following is the correct electron configuration for a neutral atom of oxygen in the ground state? A) 1s 2 2p 4 B) 1s 2 2s
More informationChemistry Final Exam Sample Items
Chemistry Final Exam Sample Items 1. Which best describes the current atomic theory? a. Atoms consist of electrons circling in definite orbits around a positive nucleus. b. Atoms are composed of electrons
More informationREVIEW OF BASIC CHEMISTRY ANSWER KEY
REVIEW OF BASIC CHEMISTRY ANSWER KEY 1. Name the following elements. Spelling counts: 2. Write the symbols for the following elements. H hydrogen sodium Na S sulphur phosphorus P Cl chlorine fluorine F
More informationSCH4U Chemistry Review: Fundamentals
SCH4U Chemistry Review: Fundamentals Particle Theory of Matter Matter is anything that has mass and takes up space. Anything around us and in the entire universe can be classified as either matter or energy.
More informationChemistry Review. a) all of the b) a&b c) a,b&c d) a,b&d above
Chemistry Review 1. The elements whose symbols are P, C, and N are (a) potassium, cadmium, and nickel. (b) potassium, carbon, and nitrogen. (c) phosphorus, calcium, and neon. (d) phosphorus, carbon, and
More informationUNIT 1: Matter & Lab Safety
Directions: Complete all of the following questions. Turn this in on the day of your final and you can earn up to 10 bonus points on your final. You must correctly answer every questions in order to receive
More informationCHM 1045 Qualifying Exam
CHM 1045 Qualifying Exam 1. Which of the following is the basic unit of volume in the metric system? A) liter B) kilogram C) meter D) centimeter E) gram 2. Which of the following is the largest unit? A)
More informationReview for Chemistry Final Exam [Chapters 1-9 & 12]
Name: Block: Date: Chapter 1 Matter and Change Review for Chemistry Final Exam [Chapters 1-9 & 12] 1-1. Define the terms matter and atom. 1-2. Define the terms element and compound and list some examples
More informationUnit Five- Chemical Quantities Chapter 9: Mole ratios, conversions between chemicals in a balanced reaction (mole, mass), limiting reactant, % yield
Chemistry Midterm Review Exam date: Wednesday, 2/15 during class The midterm exam must be completed before February vacation if you are absent The midterm exam is worth 6% of your year grade and it contains
More informationName: Period: CHEMISTRY I HONORS SEMESTER 1 EXAM REVIEW
Name: Period: CHEMISTRY I HONORS SEMESTER 1 EXAM REVIEW Unit 1: Nature of Science What rules must be obeyed to safely conduct an experiment? What are the components of a good scientific experiment? What
More informationSemester 1 Review Chemistry
Name Period Date Semester 1 Review Chemistry Units & Unit Conversions Ch. 3 (p. 73-94) PART A SI UNITS What type of measurement is indicated by each of the following units? Choices are in the last column.
More informationSolid Gas Liquid Plasma
Unit 1: MATTER 1. Define CHEMISTRY: 2. Define MATTER: Use one of the states of matter to complete each statement. (Words will be used more than once.) Solid Gas Liquid Plasma 3. A has definite volume and
More informationChemistry Study Guide
Chemistry Study Guide Marking Period 3 Exam Week of 3/21/17 Study Guide due - When studying for this test, use your do nows, notes, homework, class handouts, and your textbook. Vocabulary Chapter 7 Anion
More informationScience 9 Midterm Study Guide
Science 9 Midterm Study Guide Name 1. What are the atomic mass units for protons, neutrons, and electrons? 2. What is the atomic number? 3. What is the mass number? 4. What particles are in equal numbers
More informationCP Chemistry Semester 1 Final Test Review
Mass in grams 10 20 30 40 50 CP Chemistry Semester 1 Final Test Review 1. Know the symbol and the power of 10 for the following metric prefixes: A. Mega M 10 6 D. deka da 10 1 G. milli m 10 6 B. kilo k
More informationName: 1. Show all work on Math Problems!!! Significant Figures and Calculations (*all math problems will require the use of sig figs)
Name: 1 AP Chemistry Summer Assignment The goal of this assignment is to make sure that everyone has the fundamentals that they will need to be successful in Chemistry II & AP Chemistry. You should have
More informationHONORS Chemistry Midterm Review
2015-2016 HONORS Chemistry Midterm Review This review sheet is a list of topics and sample practice problems only. The practice problems are good representation of what to expect on the midterm, but it
More informationPeriod: Chemistry Semester 1 Final Exam Review Packet. 1. What is the difference between a hypothesis and a theory?
Chemistry Name: Period: Chemistry Semester 1 Final Exam Review Packet 1. What is the difference between a hypothesis and a theory? 2. Distinguish between quantitative and qualitative observations. States
More informationUnit 1 Physical Science: Chemical Reactions
Unit 1 Physical Science: Chemical Reactions The physical sciences are concerned with the study of inanimate natural objects. Chemistry is the study of matter, its properties, how and why substances combine
More informationHonors Chemistry Review for Semester One Final Exam
Honors Chemistry Review for Semester One Final Exam Chapter 1 What is chemistry? Branches of chemistry Scientific method 1. What is chemistry? 2. Which measurement depends on gravitational force mass or
More informationUnit 5. Chemical Composition
Unit 5 Chemical Composition Counting by Mass Individually mass a few Calculate the average mass of one Can count large numbers of by mass Atomic Mass Unit (amu) 1 amu = 1.66 x 10-24 g Subatomic particles
More informationQuantitative chemistry Atomic structure Periodicity
IB chemistry Units 1-3 review Quantitative chemistry Significant figures The mole- be able to convert to number of particles and mass Finding empirical and molecular formulas from mass percentage States
More informationPractice Packet Unit 6: Moles & Stoichiometry
Regents Chemistry: Mr. Palermo Practice Packet Unit 6: Moles & Stoichiometry 1 LESSON 1: Moles and Molar Mass 1. Put an M if the substance is molecular/covalent, an I if ionic under the formula listed.
More informationPrinciples of Chemistry: A Molecular Approach (Tro) Chapter 2 Atoms and Elements
Principles of Chemistry: A Molecular Approach (Tro) Chapter 2 Atoms and Elements 1) Which of the following is an example of the law of multiple proportions? A) A sample of chlorine is found to contain
More informationChapter 4 Compounds and Their Bonds. Octet Rule. Metals Form Positive Ions. Ionic and Covalent Bonds. Formation of a Sodium Ion, Na +
Chapter 4 Compounds and Their Bonds Octet Rule 4.1 Octet Rule and Ions An octet Is 8 valence electrons. Is associated with the stability of the noble gases. Helium (He) is stable with 2 valence electrons
More informationUnit 1 Atomic Structure
Unit 1 Atomic Structure Unit 1 Text Questions 1.1 Atoms/Ions/Isotopes Problems Ch 5 Prob: 9,23,24,38 1.2 Average Atomic Mass Problems Ch 5 Prob: 15,17 1.3 Atomic Theory Development Problems Ch 5 Prob:
More information1) What is the volume of a tank that can hold Kg of methanol whose density is 0.788g/cm 3?
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) 23 F to K 2) 21.3 Km to cm 7) 18.2 ml to cm 3 12) 2.45 L to µm 3 17) 1.2 m to inches 22) 180 ºC to K
More informationQuestions Booklet. UNIT 1: Principles & Applications of Science I CHEMISTRY SECTION. Level 3 Applied Science. Name:.. Teacher:..
Level 3 Applied Science UNIT 1: Principles & Applications of Science I CHEMISTRY SECTION Questions Booklet Name:.. Teacher:.. Level 3 Applied Science 2017-2018 Unit 1 (Chemistry) 1 1. State the relative
More informationPrinciples of Chemistry: A Molecular Approach 2e (Tro) Chapter 2 Atoms and Elements
Principles of Chemistry: A Molecular Approach 2e (Tro) Chapter 2 Atoms and Elements 1) Which of the following is an example of the law of multiple proportions? A) A sample of chlorine is found to contain
More informationChemistry I: Midterm Review 2014
Chemistry I: Midterm Review 2014 General Stuff 1. Density and formula: density is mass per unit volume The units usually are g/cm 3 or g/l or g/ml m D = V 2. Define Accuracy and precision: Accuracy refers
More informationThis exam will be given over 2 days. Part 1: Objectives 1-13 Part 2: Objectives 14-24
Name Hour January Exam Practice A This exam will be given over 2 days. Part 1: Objectives 1-13 Part 2: Objectives 14-24 This practice exam will be graded in the exam portion of the grade book. Objectives
More informationHonors Chemistry Semester 2 Final Exam MC Practice
Honors Chemistry Semester 2 Final Exam MC Practice Name MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1. What do the alkali metals all have in common?
More informationComplete this study guide to receive 5 bonus points on your test. Only study guides that are complete will receive the bonus.
CHEMISTRY AND PERIODIC TABLE STUDY GUIDE Assigned: Thursday, 09 10 14 Due: Thursday, 09 18 14 Test Day: Friday, 09 19 14 Complete this study guide to receive 5 bonus points on your test. Only study guides
More informationMemorize: Understand: Know how to:
NAME: CLASS PERIOD: REVIEW FOR HONORS CHEMISTRY SEMESTER 1 EXAM Memorize: Understand: Know how to: 1 SI units for different measurements (length, volume, number, mass, temperature, density) Definition
More informationelemental state. There are two different possibilities: DESCRIPTION 1. One cation (+ ion) replaces another. 2. One anion (- ion) replaces another.
CHEMICAL TYPES HANDOUT In these reactions, a free element reacts with a compound to form another compound and release one of the elements of the original compound in the elemental state. There are two
More informationLaw of Definite Proportion** (Proust): A given compound always contains exactly the same proportion of elements by mass.
# 10 Notes Unit 2: Laws, Properties & Mols Ch. Atoms, Molecules, Ions 5 Chemical Laws: I. Law of Conservation of Mass** (Lavoisier): Mass cannot be created or destroyed. II. III. IV. Law of Definite Proportion**
More informationChemistry: A Molecular Approach, 2e (Tro) Chapter 2 Atoms and Elements. Multiple Choice Questions
Chemistry: A Molecular Approach, 2e (Tro) Chapter 2 Atoms and Elements Multiple Choice Questions 1) In a chemical reaction, matter is neither created or destroyed. Which law does this refer to? A) Law
More informationHONORS Chemistry Midterm Review
2014-2015 HONORS Chemistry Midterm Review This review sheet is a list of topics and sample practice problems only. The practice problems are good representation of what to expect on the midterm, but it
More informationWorksheet 1: REPRESENTATIVE PARTICLES
Worksheet 1: REPRESENTATIVE PARTICLES Directions: For each substance below, state the representative particle. If the RP is a molecule, state the number of atoms that make up the molecule. If the RP is
More information5. What is the name of the compound PbO? 6. What is the name of HCl(aq)?
1. Which idea of John Dalton is no longer considered part of the modern view of atoms? (A) Atoms are extremely small. (B) Atoms of the same element have identical masses. (C) Atoms combine in simple whole
More informationChapter 6 Inorganic and Organic Compounds: Names and Formulas
Chapter 6 Inorganic and Organic Compounds: Names and Formulas 6.1 Octet Rule and Ions 1 Octet Rule An octet is 8 valence electrons is associated with the stability of the noble gases does not occur with
More informationFirst Semester Review Worksheet
First Semester Review Worksheet 1. Determine the number of significant figures in each of the numbers below a. 1000 b. 4.567 c. 2030 d. 0.0240 e. 0.02677 f. 200.00 g. 4.65 x 10 4 h. 100.300 2. Convert
More informationUnit 2. Chemical Foundations: Elements, Atoms, and Ions
Unit 2 Chemical Foundations: Elements, Atoms, and Ions Memorize the list of elements You will have a quiz on this list. All of the elements will be on the quiz! Elements in the Earth System (% mass in
More informationUnit Five- Chemical Quantities Chapter 9: Mole ratios, conversions between chemicals in a balanced reaction (mole, mass), limiting reactant, % yield
Chemistry Midterm Review Exam date: Wednesday, 2/15 during class The midterm exam must be completed before February vacation if you are absent The midterm exam is worth 6% of your year grade and it contains
More informationPhysical Science Study Guide
Name: Class: Date: Physical Science Study Guide Multiple Choice Identify the choice that best completes the statement or answers the question. 1. Mendeleev arranged the known chemical elements in a table
More informationChapter 6 and 7 Practice MC
Chapter 6 and 7 Practice MC MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) Ammonium fluoride is considered which of the following? 1) A) molecular
More informationIonic Bonding Ionic bonding occurs when metals and nonmetals trade one or more electrons and the resulting opposite charges attract each other. Metals
Chemical Bonding Now that we know what atoms look like A very small (less than 0.001% of the volume) and massive (more than 99.99% of the mass) nucleus with protons (+) and neutrons (neutral) and electrons
More informationFinal Review Packet. When 100% correct, you will receive a
Final Review Packet When 100% correct, you will receive a 15-point bonus sticker to place on the final exam. Deadline: Wednesday, Feb. 8. NO EXCEPTIONS!!!!!! Note! The Final Exam will be worth two tests
More informationCHM 111 Final Fall 2012
Name Part I. Multiple Choice 1. Consider the following specific heats of metals. Metal copper cobalt chromium gold silver CHM 111 Final Fall 2012 Specific Heat 0.385 J/(g C) 0.418 J/(g C) 0.447 J/(g C)
More information9. The ratio of the volume of nitrogen to that of the ammonia in the reaction N2 + 3 H2 2 NH3 is 1) 1:2; 2) 1:3; 3) 3:2; 4) 2:3.
1. In a balanced chemical equation l) coefficients are equal; 2) atoms are conserved; 3) molecules are equal; 4) energy is always produced; 5) none of these. 2. Which of the following statements about
More informationLab Chemistry - Final Exam Review 1. Express in scientific notation. A) D) B) E) C)
Lab Chemistry - Final Exam Review 1. Express 30554000 in scientific notation. A) 3 10 7 D) 30554 10 3 B) 3.0554 10 7 E) 305540 10 7 C) 306 10 7 2. What is the result of the following multiplication expressed
More informationChemical Bonding. Chemical Bonds. Metals, Ions, or Molecules. All Matter Exists as Atoms,
Chemical Bonding Valence electrons (the outer most electrons) are responsible for the interaction between atoms when forming chemical compounds. Another way to say that is that valence electrons are the
More informationStudent Instructions. 1. Ensure that you have blank paper and a Data Booket.. 2. Record all aswers on a separate piece of paper.
Student Instructions 1. Ensure that you have blank paper and a Data Booket.. 2. Record all aswers on a separate piece of paper. 3. Answer keys are provided at the beginning of each section. 4. When you
More informationIf Sally has 4.56 x atoms of oxygen in a sample of aluminum oxide, how many kilograms of aluminum does she have?
If Sally has 4.56 x 10 34 atoms of oxygen in a sample of aluminum oxide, how many kilograms of aluminum does she have? Bertha has.025 milligrams of sodium that she got from a sample of Sodium phosphate,
More informationPrinciples of Chemistry: A Molecular Approach, 3e (Tro) Chapter 2 Atoms and Elements
Principles of Chemistry: A Molecular Approach, 3e (Tro) Chapter 2 Atoms and Elements 1) Which of the following is an example of the law of multiple proportions? A) A sample of chlorine is found to contain
More informationChemistry Final Review 2017
Chemistry Final Review 2017 Atomic/Molecular Structure and Periodic Trends 1. What is the atomic number trend on the periodic table? 2. On the following periodic table label metals, nonmetals, Alkali metals,
More informationRegents Chemistry Practice Problems from Units 1-9 March 2018
1. Which is a pure substance? A) table salt B) bronze C) air D) soil 2. A tentative explanation of certain facts that provides the basis for further experimentation is a(n) A) observation B) hypothesis
More informationMULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.
Exam Name MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) A molecule of water contains hydrogen and oxygen in a 1:8 ratio by mass. This is a statement
More informationTest Review # 5. Chemistry: Form TR5-8A. Average Atomic Mass. Subatomic particles.
Chemistry: Form TR5-8A REVIEW Name Date Period Test Review # 5 Subatomic particles. Type of Particle Location Mass Relative Mass Charge Proton Center 1.67 10-27 kg 1 +1 Electron Outside 9.11 10-31 kg 0-1
More informationChapter 28: Nuclear Chemistry (pg ) On a graph of n 0 versus p + use the position of a plotted nucleus relative to the band of
Chemistry A Final Exam Review Packet Fall 2016 The topics and questions on this review are intended to help you study for the final exam. The exam will include both multiple choice and short answer questions
More informationCHEM 115 EXAM #3 Practice Exam Fall 2013
Name CHEM 115 EXAM #3 Practice Exam Fall 2013 Circle the correct answer. (numbers 1-9, 3 points each) 1. Choose the correct statement about the compound SO 2. a. the S O bonds are ionic in character b.
More informationName Pd SN Date Chemistry Review Packet- Spring 2014
Name Pd SN Date Chemistry Review Packet- Spring 2014 1.1.1 Draw pictures to illustrate the differing isotopes and ions of a given element. 1.1.1 Which atomic symbol represents an isotope of sulfur with
More informationChapter 2: Atoms, Molecules, and Ions
Chapter 2: Atoms, Molecules, and Ions 1. Which of the following pairs of compounds can be used to illustrate the law of multiple proportions? A) NH 4 and NH 4 Cl B) ZnO 2 and ZnCl 2 C) H 2 O and HCl D)
More informationAP Chemistry Summer Assignment
Name AP Chemistry Summer Assignment Welcome to AP chemistry! This summer assignment is intended to help you review the basic topics you learned in pre-ap chemistry that are crucial for your success in
More informationCP Chemistry Semester 1 Final Test Review 1. Know the symbol and the power of 10 for the following metric prefixes: A. Mega B.
Mass in grams 10 20 30 40 50 CP Chemistry Semester 1 Final Test Review 1. Know the symbol and the power of 10 for the following metric prefixes: A. Mega B. kilo D. deka E. deci G. milli H. micro C. hecto
More informationCHEMISTRY REVIEW REVIEW WORKSHEET
The student should be able to: 1. Describe the classification of matter. 2. Describe the conservation of mass. 3. Identify products and reactions in a chemical equation. 4. Describe the structure of an
More informationBalancing Equations Notes
. Unit 6 Chemical Equations and Reactions What is a Chemical Equation? A Chemical Equation is a written representation of the process that occurs in a chemical reaction. A chemical equation is written
More informationUNIT 9 - STOICHIOMETRY
General Stoichiometry Notes STOICHIOMETRY: tells relative amts of reactants & products in a chemical reaction Given an amount of a substance involved in a chemical reaction, we can figure out the amount
More informationLesson 13: Ionic Equations & Intro to the Mole with Conversions
NOTES Name: Date: Class: Lesson 13: Ionic Equations & Intro to the Mole with Conversions Box 1: Balance: 1. Mg + O2 MgO 2. KClO3 KCl + O2 3. C2H6 + O2 CO2 + H2O Write and balance the equation that represents
More informationSpring Semester Final Exam Study Guide
Honors Chemistry Name Period AlCl3 Cu2S NaCN HI PCl3 CrBr3 Naming and Formula Writing 1. Write the name or formula for each of the following: HClO2 (NH4)2SO4 I4O10 H3N NiN H3PO4 Mercury (II) bromide Phosphorous
More informationAnswer Sheet for Sample Problems for Chemistry Level 1 Final Exam 2016 Study Guide
Answer Sheet for Sample Problems for Chemistry Level 1 Final Exam 2016 Study Guide Electrons in Atoms Chapter 5 1. What is the frequency of green light, which has a wavelength of 4.90 x 10-7 m? 8 c 3.00x10
More information4. Draw a concept map showing the classifications of matter. Give an example of each.
Name Bring calculator, pencils, and this completed worksheet to the midterm exam. For problems involving an equation, carry out the following steps: 1. Write the equation. 2. Substitute numbers and units.
More informationBalancing Equations Notes
. Unit 9 Chemical Equations and Reactions What is a Chemical Equation? A Chemical Equation is a written representation of the process that occurs in a chemical reaction. A chemical equation is written
More informationParticle Relative Mass Charge
ADVANCED CHEMISTRY REVISION THE FIRST 5 WEEKS 1. Define each of the following words so that you can differentiate between them:- ELEMENT and COMPOUND, ATOM and MOLECULE An element is comprised of one type
More information4) A specific isotope of an element is known to have 15 protons and 16 neutrons. Which symbol would properly represent this isotope?
CHM1025 Exam 2 Chapter 4 & 5 MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) All of the following statements about different elements are true
More information