2014 Chemistry 1 st Semester Exam Review Packet
|
|
- Naomi Bailey
- 6 years ago
- Views:
Transcription
1 Name: Date: Hour: 2014 Chemistry 1 st Semester Exam Review Packet 1. What percentage of the water on Earth is salt water? (1 point) A. 97.2% B % C. 2.11% D. 2.8 % 2. One similarity between all mixtures and compounds is that both. (1 point) A. are heterogeneous B. are homogeneous C. combine in a definite ratio D. consist of two or more substances 3. An atom of carbon-12 and an atom of carbon-14 differ in. (1 point) A. atomic number B. mass number C. nuclear charge D. number of electrons 4. How many times more acidic is a solution of ph 8 than a solution of ph 5? (1 point) A. 3X B. 30X C. 300X D. 1,000X E. 100X 5. Which of the following elements is most chemically similar to magnesium? (1 point) C4.9A A. calcium B. manganese C. sodium D. aluminum 6.. The density of tin is 7.3 g/ml. The density of lead is g/ml. The density of silicon is 2.33 g/ml. Therefore, the density of germanium must be. (1 point) C4.9c A. 1.5 g/ml B. 5.3 g/ml C g/ml D g/ml 7. Since an atom is electrically neutral, the number of protons is equal to the number of. (1 point) C4.10A A. neutrons B. electrons C. neutrons + electrons D. neutrons electrons 8. Fact 1: Zinc releases hydrogen gas when exposed to hydrochloric acid. Fact 2: Zinc s density is 7.14 g/ml. The 1 st fact describes a, and the 2 nd fact describes a. (1 point) C5.2B A. physical change, physical property D. chemical change, chemical property B. physical property, chemical change E. physical property, physical property C. chemical change, physical property F. chemical property; physical change 9. Which list of elements consists of nonmetals only? (1 point) C4.9b A. boron, gallium, germanium B. oxygen, sulfur, selenium C. aluminum, boron, silicon D. boron, silicon, germanium 10. Which of the following atoms represent the same element? (1 point) C4.10B Atoms Protons Neutrons Electrons A B C D A. Element A & Element B B. Element C & Element D C. Element B & Element C D. Element B & Element D E. Element A & Element C F. Element A & Element D 11. In an atom of argon-40, the number of protons. (1 point) A. equals the number of electrons B. equals the number of neutrons C. is less than the number of electrons D. is greater than the number of electrons 1
2 12. Which statement describes a chemical property of bromine? (1 point) A. bromine is soluble in water B. bromine has a reddish-brown color C. bromine combines with aluminum to produce AlBr 3 D. bromine changes from a liquid to a gas at 23 0 C 13. A sample of an element is malleable and can conduct electricity. This element could be. (1 point) A. H B. He C. S D. Sn 14. Given the balanced particle diagram below: + Which statement describes the type of change and the chemical properties of the product and reactants? (1 point) A. the equation represents a physical change, with the product and reactants having different chemical properties B. The equation represents a physical change, with the produce and reactants having identical chemical properties C. The equation represents a chemical change, with the product and reactants having different chemical properties D. The equation represents a chemical change, with the product and reactants having identical chemical properties 15. An element that is malleable and a good conductor of heat and electricity could have an atomic number of. (1 point) A. 16 B. 29 C. 18 D. 35 E On the modern Periodic Table, the elements are arranged in order of increasing. (1 point) A. atomic mass B. mass number C. charge D. atomic number 17. What can be determined if only the atomic number of an ion is known? (1 point) A. the total number of neutrons only B. the total number of protons only C. the total number of protons and neutrons D. the total number of protons and electrons 18. Chlorine-37 can be represented as. (1 point) A. Cl B. Cl C. Cl D. Cl Sodium and potassium have similar chemical properties because an atom of each element has the same. (1 point) A. oxidation number B. # of neutrons C. # of protons D. # of electrons Which quantity identifies an element? (1 point) A. atomic number B. mass number C. number of neutrons D. total number of electrons 22. What is the total charge of the nucleus of a nitrogen atom? (1 point) A. +5 B. +14 C. 0 D. +2 E Which of the following isotopes will be in greatest abundance in nature? (1 point) C4.10b A. P-30 B. P-31 C. P-15 D. P
3 24. Which of the following drawings represents krypton at room temperature? (1 point) A. B. C. 25. Which of the following is the products side of the chemical equation of solid calcium in aqueous copper (II) nitrate is shown below. (1 point) C5.6b Ca (s) + Cu(NO 3) 2 (aq) A. Cu (s) + Ca(NO 3) 2(aq) B. Ca (aq) + Cu (aq) + 3 N 2 (g) + 9 O 2 (g) C. Cu 3Al 2 (s) + 2 NO 3 (aq) D. Ca (s) + Cu (s) + N 2O 6 (aq) E. Cu (s) + CaNO 3 (aq) 26. What element on the periodic table will have very similar properties to copper, Cu? (1 point) (C4.9A) A. iron B. silver C. nickel D. zinc E. aluminum 27. What trend in metallic reactivity is apparent as you move from left to right across a horizontal row (period) of the periodic table? (1 point) A. Reactivity decreases B. Reactivity increases C. Reactivity stays the same D. Impossible to predict 28. Which of the following metals would be the most difficult to extract from their ores? (1 point) A.) aluminum B.) silver C.) gold D.) iron 29. In which part of the periodic table are the most reactive-metals found? (1 point) A. Bottom left B. Top right C. Middle D. Top left E. Bottom right Identify each of the following as being a physical (A) or chemical (B) change. (1 point each) 30. a cut apple left out in the air turns brown 31. dry cleaning removes oils from clothing 32. an opened carbonated beverage fizzes 33. as shoes wear out, holes appear in the soles What is happening to the average kinetic energy of the molecules in the sample during section 2? (1 point) A. increasing B. decreasing C. staying the same D. impossible to tell 3
4 35. As a substance goes from step 3-4, what happens to the distance between the particles?(1 point) A. increasing B. decreasing C. staying the same D. impossible to tell 36. What is the condensing point (temperature) of this substance? (1 point) A C B C C C D C E C Identify each of the following as being an element (A), mixture (B), or compound (C). (1 point each) 37. milk 38. CO silver 40. concrete Identify each of the following compounds as being soluble (A) or insoluble (B) in water. (1 point each) 45. silver sulfate 46. potassium hydroxide 47. CuNO Na 2CO 3 Use each element s electronegativity to identify whether each of the following molecules are polar covalent (A), nonpolar covalent (B), or ionic (C). (1 point each) 49. H 2O 50. LiF 51. NH O 2 Identify each of the following statements as referring to an acid (A), base (B) or neither (C). (1 point each) 53. KOH 59. ph = HNO sour tasting 55. NaCl 61. [H+] = [OH-] 56. H 2SO slippery to touch 57. red litmus turns blue 63. ph = ph = [H+] < [OH-] 65. Where is most of Earth s fresh water located? (1 point) A. lakes & ponds B. rivers and streams C. glaciers D. ocean Match the following terms. (8 points) 66. supersaturated A. substance being dissolved (in lesser quantity) 67. saturated B. maximum amount of solute dissolved 68. unsaturated C. not able to dissolve 69. soluble D. homogeneous mixture 70. insoluble E. excess solute dissolved at higher temperature, then cooled 71. solvent AB. able to dissolve 72. solution AC. more solute is still able to be dissolved 73. solute AD. substance doing the dissolving (in greater quantity) 4
5 74. Which substance in the solubility curve above is least soluble at 10 0 C? (1 point) A. KI B. Ce 2(SO 4) 3 C. KClO 3 D. NH 3 E. KNO Ammonia, NH 3, is a gas. What happens to the solubility of gases as temperature decreases? (1 point) A. increases B. decreases C. stays the same 76. At 40 0 C, 70 g KNO 3 is dissolved in 100 g of water. Is this solution? (1 point) A. saturated B. supersaturated C. unsaturated? 77. Which substance s solubility changes the least from 0 0 C to C? A. KI B. Ce 2(SO 4) 3 C. KClO 3 D. NH 3 E. NaCl 78. Which of the following is the best method to purify water that is contaminated with insoluble solid (can t dissolve) substances such as sand? (1 point) A. distillation B. precipitation C. filtration D. decanting 1. Calculate the density of a substance that has a mass of 4.5 g and a volume of 2.4 ml. (2 points) 2. Calculate the mass of a 5.5 ml nugget of aluminum that has a density of 1.9 g/ml. (2 points) 3. In each of the following beakers, draw what the same sample of water, H 2O, would look like on a molecular scale as a solid, liquid, and gas. C2.2B (3 points) Solid Water Liquid Water Water Vapor 5
6 4. Convert the following measurements. You must show your work and use the fence method to receive full credit. (4 points) 46.3 hours = years 65 mi/hr = km/s 5. Complete the chart. (8 points) Substance S Fe Atomic number 13 Mass number Protons Neutrons Electrons Metal, Nonmetal, Metalloid Name the following ionic compounds. (6 points) CoCl 2: Mn 3(PO 4) 2: MgBr 2: NaOH: (NH 4) 2Cr 2O 7: AuP: 7. Write formulas for the following ionic compounds. (6 points) calcium iodide: tin (IV) carbonate: copper (II) nitrate: aluminum oxide: lead (IV) sulfide: barium hydroxide: 8. In beakers A and B draw two different compounds, one in each box, using the representations for atoms of element X and element Z given below. In beaker C draw a mixture of these two compounds. (3 points) Atom of element X = Atom of element Z = A B C 6
7 9. How many moles of CaCl 2 are in 150 g of CaCl 2? (2 points) 10. What is the molarity of a solution containing 70 g of CaCl 2 in 275 ml of solution? (2 points) Atom/Ion/Element A B C D E F G # electrons # protons # neutrons Table Which of the substances in Table 1 represent the same element? (1 point) 12. Write the correct isotopic symbol for substances A, C, and E listed in Table 1. Include in your symbol the element symbol, atomic number, mass number, and charge if applicable. (An example is given for reference.) (3points) 2 Ex: 1 H +1 A C E 13. Using the metal reactivity series, write the products of the reactions that will occur. Balance all reactions. If a reaction will not occur, write NR after the arrow. (3 points) C5.6b (Use the following charge for the transition metal: Pt +4 ) Al (s) + Zn(NO 3) 2 (aq) Pt (s) + Sn(NO 3) 2 (aq) Br 2 + KI 14. Assign oxidation numbers for all elements in each compound. (5 points) NaClO 3 Na = Cl= O= -3 PO 4 P = O = H 5P 3O 10 H = P = O = -1 SbF 6 Sb = F= 7
8 liter (giga) (mega) (kilo) (hecto) (deka) meter (deci) (centi) (milli) (micro) (nano) (pico) G- M- k- h- da- gram d- c- m- - n- p- byte 0 F = 9/5( 0 C) cm 3 = 1mL 0 C = ( 0 F-32)5/9 1 dm 3 = 1,000 ml = 1L K = 0 C m 3 = 1,000,000 ml = 1,000 L 1 lb 1 kg 1 m 1 in 1 mile 1 mile 2.54 cm 5,280 ft km g 2.2 lbs 3.28 ft density = mass volume Molarity = # moles # liters moles = # grams molar mass Electronegativity difference Ionic = > 1.7 Polar = 0.51 to 1.69 Nonpolar = < 0.5 8
Part A Answer all questions in this part.
Part A Directions (1-24): For each statement or question, record on your separate answer sheet the number of the word or expression that, of those given, best completes the statement or answers the question.
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 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 information5. [7 points] What is the mass of gallons (a fifth) of pure ethanol (density = g/cm 3 )? [1 gallon = Liters]
1 of 6 10/20/2009 3:55 AM Avogadro s Number, N A = 6.022 10 23 1. [7 points] Given the following mathematical expression: (15.11115.0)/(2.154 10 3 ) How many significant figures should the answer contain?
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 information2. Identify each of the following samples of matter as heterogeneous or homogeneous.
EOC REVIEW #1 1. List the following in order from smallest to largest. (A) 1 dm 3 (B) 1 ml (C) 1 cl (D) 1 L (E) 1 dl 2. Convert the following. Express your answer in standard scientific notation. (A) 36
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 information5. All isotopes of a given element must have the same (A) atomic mass (B) atomic number (C) mass number (D) number of neutrons
1. Which substance can be decomposed by a chemical change? (A) beryllium (B) boron (C) methanol (D) magnesium 2. The particles in a crystalline solid are arranged (A) randomly and far apart (B) randomly
More informationIn addition to the information at the end of the exam, you will be given a periodic table.
In addition to the information at the end of the exam, you will be given a periodic table. 1. Express 3143 in scientific notation. a. 3.143 x 10-3 b. 3143 x 10 +3 c. 3.143 x 10 +3 d. 3.143 x 10 +4 2. Express
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 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 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 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 informationHonor s Chemistry: Fall Semester Final
Honor s Chemistry: Fall Semester Final Name 1. Explain what is wrong with the statement My friend burned a piece of paper (a hydrocarbon) that had the final exam on it and it disappeared. (Be sure to use
More informationReactions in Aqueous Solutions
Reactions in Aqueous Solutions 1 Chapter 4 General Properties of Aqueous Solutions (4.1) Precipitation Reactions (4.2) Acid-Base Reactions (4.3) Oxidation-Reduction Reactions (4.4) Concentration of Solutions
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 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 informationVolume of water g g? 50.0 ml ?
MID-TERM EXAM REVIEW! KEY! Unit 1 Convert the following: 1.) 2.02 x 10 15 mg = g 2.02 x 10 15 mg 1 g = 2.02 x 10 12 g 1000 mg 2.) 1.29 x 10-7 m = cm 1.29 x 10-7 m 100 cm = 1.29 x 10-5 cm 1 m 3.) 13.5 dm
More informationChapter 4 Reactions in Aqueous Solution
Chapter 4 Reactions in Aqueous Solution Homework Chapter 4 11, 15, 21, 23, 27, 29, 35, 41, 45, 47, 51, 55, 57, 61, 63, 73, 75, 81, 85 1 2 Chapter Objectives Solution To understand the nature of ionic substances
More informationGas Laws. Bonding. Solutions M= moles solute Mass %= mass solute x 100. Acids and Bases. Thermochemistry q = mc T
Name Period Teacher Practice Test: OTHS Academic Chemistry Spring Semester 2017 The exam will have 100 multiple choice questions (1 point each) Formula sheet (see below) and Periodic table will be provided
More informationNATIONAL 5 CHEMISTRY
Farr High School NATIONAL 5 CHEMISTRY Unit 1 Chemical Changes and Structure Question Booklet 1 Rates of Reaction 1. Explain how the following would affect the rate of the reaction between 1.0 g of magnesium
More informationSOLUTIONS. Solutions - page
SOLUTIONS For gases in a liquid, as the temperature goes up the solubility goes. For gases in a liquid, as the pressure goes up the solubility goes. Example: What is the molarity of a solution with 2.0
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 informationnew experimental data, and can be modified
Mass in grams 10 20 30 40 50 Name: Date: Period: CP Chemistry Semester 1 Final Test Review CHAPTERS 1 & 2: Scientific Method, Density, Metric Conversions, Accuracy/Precision, Significant Figures 1. Know
More informationChemistry Released Questions
Name: Date: 1. What was Niels Bohr s prediction about the location of the electrons in an atom? 3. An atom with which atomic diagram has chemical properties most similar to calcium? A. Electrons pair with
More informationChemistry CRT Study Guide First Quarter
Number AL COS # 1. #1.0 Classify sodium chloride as an element, mixture, compound, or colloid. Compound 2. #1.0 Classify air as an element, mixture, compound, or colloid. Mixture 3. #1.0 Classify a blueberry
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 information2. 2 Complete this table of the parts of an atom: Particle Charge Location in atom Proton. Negative
Q Outcome 1. 1 Give a definition of the term matter 2. 2 Complete this table of the parts of an atom: Particle Charge Location in atom Proton In the nucleus Negative 3. 2 Draw an atom and label all particles.
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 informationNAME: Chemistry Final Exam Review *=equations not given on Reference Sheet Unit 1: Math & Measurement Main Topics: Conversions, Significant Figures,
Chemistry Final Exam Review *=equations not given on Reference Sheet Unit 1: Math & Measurement Main Topics: Conversions, Significant Figures, Density, Percent Error Density *Percent Error 1. How many
More informationCP Chemistry Midterm Topic List
CP Chemistry Midterm Topic List Converting SI Units (Kilo, Hecto, Deca, Base Unit, Deci, Centi, Milli) Scientific Notation Precision versus Accuracy Properties of Matter Classification of Matter (Element/Compound/Mixture)
More information1. How many protons, electrons, and neutrons are in one atom of the following isotopes (6 points)?
Chemistry 11 Department of Physical Sciences Kingsborough Community College City University of New York NAME Exam 1: Chapters 1-3 50 points 1. How many protons, electrons, and neutrons are in one atom
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 informationSPRING 2017 CHEMISTRY FINAL EXAM REVIEW
SPRING 2017 CHEMISTRY FINAL EXAM REVIEW Multiple Choice Identify the letter of the choice that best completes the statement or answers the question. 1. BONDING What is the formula for diphosphorus pentaoxide?
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 informationChemistry. Essential Standards Chemistry
Essential Standards Chemistry Chemistry Matter: Properties & Change 1.1 Students will analyze the structure of atoms and ions. 1.2 Student will understand the bonding that occurs in simple compounds in
More information11/3/09. Aqueous Solubility of Compounds. Aqueous Solubility of Ionic Compounds. Aqueous Solubility of Ionic Compounds
Aqueous Solubility of Compounds Not all compounds dissolve in water. Solubility varies from compound to compound. Chapter 5: Chemical Reactions Soluble ionic compounds dissociate. Ions are solvated Most
More informationChapter 4 Atoms Practice Problems
Chapter 4 Atoms Practice Problems 1) The primary substances of which all other things are composed are A) molecules. B) compounds. C) elements. D) electrons. E) protons. 2) Which of the following is a
More informationSilver nitrate solution is added to sodium dichromate solution
Chem. 110 50 Points Final Exam Part 1 Practice Write the chemical names or formulas for the following a H 2 SO 4 b NiNO 2 c Aluminum thiosulfate d Plumbic acetate e Ag 2 C 2 O 4 f P 2 O 5 g Cyanic acid
More informationChemistry Mid-Term Exam Review Spring 2017
Unit 1 Measurement & Math Accuracy & Precision (recognizing given lab data) Density calculations Number of SFs in a measurement, Round answers to correct number of SFs Percent Error Unit conversions in
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 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 informationCHEMISTRY 1A SPRING 2011 EXAM 1 KEY CHAPTERS 1-4
You might find the following useful. Electronegativities H 2.2 CHEMISTRY 1A SPRING 2011 EXAM 1 KEY CHAPTERS 1- Li Be B C N O F 0.98 1.57 2.0 2.55.0..98 Na Mg Al Si P S Cl 0.9 1.1 1.61 1.9 2.19 2.58.16
More informationUnit 4 - Periodic Table Exam Name: PRACTICE QUESTIONS Date: 2/23/2016
Name: PRACTICE QUESTIONS Date: 2/23/2016 1. Which pair of symbols represents a metalloid and a noble gas? 1) Si and Bi 2) As and Ar 3) Ge and Te 4) Ne and Xe 2. What determines the order of placement of
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 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 informationUnit Two Worksheet WS DC U2
Unit Two Worksheet WS DC U2 Name Period Short Answer [Writing]. Write skeleton equations representing the following reactions and then balance them. Then identify the reaction type. Include all needed
More informationChemistry Midterm Exam Review Sheet Spring 2012
Chemistry Midterm Exam Review Sheet Spring 2012 1. Know your safety rules 2. A shopping mall wanted to determine whether the more expensive Tough Stuff floor wax was better than the cheaper Steel Seal
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 informationH = Hydrogen atoms O = Oxygen atoms
CHEMISTRY CP Name: KEY Period: TEST DATE: Unit 8 Review Sheet KEY: Properties of Water, Solutions, Concentration, Acids and Bases PROPERTIES OF WATER 1. Define the following terms: polarity, surface tension,
More informationChemistry Spring Packet Study Guide for Benchmark Exam
Chemistry Spring Packet-1 --- Study Guide for Benchmark Exam 1. Which action will result in a new product with new chemical properties? A. shredding a newspaper B. cutting wood C. breaking a mirror D.
More informationSettling? Filterable? Tyndall Effect? * 1 N N Y nm
Types of Mixtures Notes *What is the Tyndall Effect? When a light shines through a mixture, the beams of light scatter. Homogeneous or Heterogeneous # of visible phases Settling? Filterable? Tyndall Effect?
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 informationChemistry Final Exam Review
Chemistry Final Exam Review Multiple Choice Identify the letter of the choice that best completes the statement or answers the question. 1. All of the following are physical properties of matter EXCEPT.
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 informationChemistry Final Exam Study Guide Fall Semester
Chemistry Final Exam Study Guide Fall Semester Name: Date: Class: Basics of Science (Ch 1) 1. Briefly describe what occurs in each step of the scientific method: 1. Problem/Question 2. Research 3. Hypothesis
More informationPhysical Science Lecture Notes Chapters 17, 18 & 19
Physical Science Lecture Notes Chapters 17, 18 & 19 I. 17-1: Matter & Its Changes a. Changes in matter i. Physical Changes Alters form or appearance but doesn t change it into another substance ie. Water
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 informationChemistry Final Exam Review Multiple Choice Practice Questions
Chemistry Final Exam Review Multiple Choice Practice Questions Work through the following problems. Do your work in a neat orderly fashion either on this page or on another sheet. 1. Which of the following
More informationCHEMISTRY. Everything is made of matter. Matter is composed of tiny particles called atoms.
CHEMISTRY Everything is made of matter. Matter is composed of tiny particles called atoms. Everything in the world (every substance) is composed of one or more elements. Elements are pure substances, which
More informationAssignment 04 (A) a) ii and iii b) i, ii, and iii c) i, iv, and v d) iii e) ii (These are molecular compounds.)
Assignment 04 (A) 1- Which of the following are nonelectrolytes in water? (i) HF (ii) ethanol, C 2 H 5 OH (iii) C 12 H 22 O 11 (iv) KClO 3 (v) Cu(NO 3 ) 2 a) ii and iii b) i, ii, and iii c) i, iv, and
More informationChemistry FINAL: CONTENT Review Packet
Chemistry FINAL: CONTENT Review Packet Name: Period: Date: Classification of Matter & Chemical/ Physical Changes 1. are substances that are made up of two or more elements which are chemically combined
More informationChemistry Term 2 Review 1) Using the diagram above, answer the following question: How many electrons are in the valence shell of this atom? A. 2 B.
Name: Date: Chemistry Term 2 Review 1) Using the diagram above, answer the following question: How many electrons are in the valence shell of this atom? A. 2 C. 6 E. 13 2) Which formula represents an ionic
More informationUnit 8 Chemical Reactions- Funsheets
Part A- Balancing Equations and Types of Reactions Balance AND identify the following reactions: Unit 8 Chemical Reactions- Funsheets 1) Mg + Zn(NO 3) 2 Zn Mg(NO 3) 2 2) Ba + AgNO 3 Ag + Ba(NO 3) 2 3)
More informationChapter 6. Chemical Reactions. Sodium reacts violently with bromine to form sodium bromide.
Chapter 6 Chemical Reactions Sodium reacts violently with bromine to form sodium bromide. Evidence of Chemical Reactions Chemical Equations Reactants Products Reactant(s): Substance(s) present before the
More informationUnit 4: Reactions and Stoichiometry
Unit 4: Reactions and Stoichiometry Reactions Chemical equation Expression representing a chemical reaction Formulas of reactants on the left side Formulas of products on the right side Arrow(s) connect(s)
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 informationOPTIONAL PRACTICE PROBLEMS
OPTIONAL PRACTICE PROBLEMS 1 DIMENSIONAL ANALYSIS AND PROPERTIES OF MATTER (1) List the base (fundamental) SI units: (2) Fill in the following table: Object Weight, g Mass, g Piece of iron 50 g? Huge container
More informationExplain freezing-point depression and boiling-point elevation at the molecular level.
Solutions 1 UNIT4: SOLUTIONS All important vocabulary is in Italics and bold. Describe and give examples of various types of solutions. Include: suspension, emulsion, colloid, alloy, solute, solvent, soluble,
More informationChemistry Utica Community Schools Semester One Review
Directions: Chemistry Utica Community Schools Semester One Review You may prepare your own hand-written 3x5 note card which will be collected on your exam day. You must bring a pencil and calculator to
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 informationMid-Term Review (HERBERHOLZ - Honors Chemistry) Chapter 2: 1. How many significant digits are in the following numbers?
Name Hour Mid-Term Review 2017-2018 (HERBERHOLZ - Honors Chemistry) Chapter 2: 1. How many significant digits are in the following numbers? a. 417.0 b. 0.0005 c. 500 000 d. 0.30034 e. 3.970 x 10 5 f. 200.10
More informationTopics to Expect: Periodic Table: s, p, d, f blocks Metal, Metalloid, Non metal, etc. Periodic Trends, Family names Electron Configuration: Orbitals a
Chemistry Final Exam Review and Practice Chapters Covered ESSENTIALLY CUMMULATIVE List of Chapters: Ch: 6, 7, 8, 9, 10, 13, 14, 15, 16, 19, 20 Topics to Expect: Periodic Table: s, p, d, f blocks Metal,
More informationCHEMISTRY REVIEW REVIEW WORKSHEET
The student should be able to:. 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 atom
More informationJanuary Semester Exam Practice B This exam will be given over 2 days. Part 1: Objectives 1-13 Part 2: Objectives 14-24
Name Hour January Semester Exam Practice B 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
More informationSample. Test Booklet. Subject: SC, Grade: HS MCAS 2007 HS Chemistry. - signup at to remove - Student name:
Test Booklet Subject: SC, Grade: HS Student name: Author: Massachusetts District: Massachusetts Released Tests Printed: Thursday February 14, 2013 1 Which of the following Lewis dot structures represents
More informationed. Brad Collins Aqueous Chemistry Chapter 5 Some images copyright The McGraw-Hill Companies, Inc. Sunday, August 18, 13
ed. Brad Collins Aqueous Chemistry Chapter 5 Some images copyright The McGraw-Hill Companies, Inc. A solution is a homogenous mixture of 2 or more substances at the molecular level The solute(s) is(are)
More informationCHEMISTRY 102B Practice Hour Exam I. Dr. D. DeCoste T.A (30 pts.) 16 (15 pts.) 17 (15 pts.) Total (60 pts)
CHEMISTRY 102B Practice Hour Exam I Spring 2016 Dr. D. DeCoste Name Signature T.A. This exam contains 17 questions on 5 numbered pages. Check now to make sure you have a complete exam. You have one hour
More information3. What is the smallest particle of an element that has the properties of that element?
2009-2010 semester one exam review Name Date Hr 1. What is the difference between elements, molecules and compounds? 2. What is the difference between compounds and molecules? 3. What is the smallest particle
More informationCHAPTER 4 TYPES OF CHEMICAL REACTIONS & SOLUTION STOICHIOMETRY
Advanced Chemistry Name Hour Advanced Chemistry Approximate Timeline Students are expected to keep up with class work when absent. CHAPTER 4 TYPES OF CHEMICAL REACTIONS & SOLUTION STOICHIOMETRY Day Plans
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 information2. If a gas is released in a reaction (ex: Hydrogen gas bubbles off), is it written as a reactant or a product?
PRE-AP CHEMISTRY SPRING FINAL EXAM REVIEW Name _ Period Exam Date 100% COMPLETION OF THIS REVIEW BY THE DAY OF YOUR FINAL EXAM WILL COUNT AS A 5 POINT BONUS ADDED TO YOUR FINAL EXAM SCORE. THERE WILL BE
More informationCHAPTER 8 CHEMICAL REACTIONS AND EQUATIONS
CHAPTER 8 CHEMICAL REACTIONS AND EQUATIONS CHEMICAL REACTIONS Occurs when matter combines or breaks apart to produce new kinds of matter with different properties with a change in energy. EVIDENCE FOR
More informationHONORS CHEMISTRY. Chapter 1 Introduction to Chemistry 1. What is chemistry?
HONORS CHEMISTRY FIRST SEMESTER EXAM REVIEW Chapter 1 Introduction to Chemistry 1. What is chemistry? 2. Identify the independent and dependent variables using the graph to the right. IV: DV: 3. Write
More informationChemistry 104 Final Exam Content Evaluation and Preparation for General Chemistry I Material
Chemistry 104 Final Exam Content Evaluation and Preparation for General Chemistry I Material What is 25 mph in mm s 1? Unit conversions What is 1025 K in o F? Which is larger 1 ft 3 or 0.1 m 3? What is
More informationName Chemistry Pre-AP. Notes: Solutions
Name Chemistry Pre-AP Notes: Solutions Period I. Intermolecular Forces (IMFs) A. Attractions Between Molecules Attractions between molecules are called and are very important in determining the properties
More informationChapter 4 Types of Chemical Reaction and Solution Stoichiometry
Chapter 4 Types of Chemical Reaction and Solution Stoichiometry Water, the Common Solvent One of the most important substances on Earth. Can dissolve many different substances. A polar molecule because
More informationExperiment 8 - Double Displacement Reactions
Experiment 8 - Double Displacement Reactions A double displacement reaction involves two ionic compounds that are dissolved in water. In a double displacement reaction, it appears as though the ions are
More informationYear 10 Chemistry Exam June 2011 Multiple Choice. Section A Multiple Choice
Year 10 Chemistry Exam June 2011 Multiple Choice Section A Multiple Choice 1 An aqueous solution is obtained when: a. a substance dissolves in any liquid b. a substance is dissolved in water c. when a
More informationReactions in aqueous solutions Redox reactions
Reactions in aqueous solutions Redox reactions Redox reactions In precipitation reactions, cations and anions come together to form an insoluble ionic compound. In neutralization reactions, H + ions and
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 informationChapter 1: Matter and Energy 1-1. Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display.
Chapter 1: Matter and Energy Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. 1-1 1.1 Matter and Its Classification Matter is anything that occupies space and
More informationCHEM 60 Spring 2016 Exam 2 Ch 5-8, 100 points total.
Name Exam No. F CHEM 60 Spring 2016 Exam 2 Ch 5-8, 100 points total. Multiple Choice. (20 questions, 3 points each = 60 points total) Mark the letter on the scantron form corresponding to the one best
More informationChapter 4. Aqueous Reactions and Solution Stoichiometry
Sample Exercise 4.1 (p. 127) The diagram below represents an aqueous solution of one of the following compounds: MgCl 2, KCl, or K 2 SO 4. Which solution does it best represent? Practice Exercise 1 (4.1)
More informationAdvanced Chemistry Final Review
Advanced Chemistry Final Review 1. What are the products of complete combustion of hydrocarbons? Hydrocarbons are compounds made of carbon and oxygen. When they burn (combine with oxygen) they form carbon
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 informationGCSE Additional Science
GCSE Additional Science Module C5 Chemicals of the Natural Environment: What you should know Name: Science Group: Teacher: each of the statements to help focus your revision: R = Red: I don t know this
More informationAnswers for UNIT ONE NAT 5 Flash Cards
Answers for UNIT ONE NAT 5 Flash Cards 1. (a) rate increases (b) rate increases (c) rate increases (d) rate increases 2. Average rate = change in property / change in time Where property = concentration,
More informationELEMENTS AND COMPOUNDS
C03 04/19/2013 13:31:38 Page 20 CHAPTER 3 ELEMENTS AND COMPOUNDS SOLUTIONS TO REVIEW QUESTIONS 1. Silicon 25:7% Hydrogen 0:9% In 100 g 25:7g Si 0:9g H ¼ 30 g Si=1 g H ð 1 sig: fig: Þ Si is 28 times heavier
More informationChapter 4; Reactions in Aqueous Solutions. Chapter 4; Reactions in Aqueous Solutions. V. Molarity VI. Acid-Base Titrations VII. Dilution of Solutions
Chapter 4; Reactions in Aqueous Solutions I. Electrolytes vs. NonElectrolytes II. Precipitation Reaction a) Solubility Rules III. Reactions of Acids a) Neutralization b) Acid and Carbonate c) Acid and
More information