Chemistry Mid-Term Review: (HERBERHOLZ)
|
|
- Melina Chapman
- 6 years ago
- Views:
Transcription
1 Name: Hour: Chemistry Mid-Term Review: (HERBERHOLZ) This review is worth 5% extra credit to your mid-term exam. It is due the day you are scheduled to take your midterm. Your work must be hand written and it must be your own work. Copying answers from another student will not help you to be successful on this exam. Be sure to answer every question. For calculation questions, you must show your work to receive credit. Chapter 1: 1. What are the steps of the scientific method? 2. Explain the difference between the variable and control in an experiment. 3. Why should a hypothesis be developed before experiments take place? 4. What is the difference between a theory and scientific law? 5. What is the difference between a manipulated variable and a responding variable? 6. Explain how the results of many experiments lead to the development of a theory and scientific law? Chapter 2: 1. Compare the properties of solids, liquids, and gases. 2. Amongst solids, liquids, and gases, which have a definite volume? 3. Amongst solids, liquids, and gases, which take the shape of their container? 4. Amongst solids, liquids, and gases, which can be compressed? 1
2 5. How many phases exist in homogeneous and heterogeneous mixtures? 6. How is a compound different from an element? 7. How can you distinguish a substance from a mixture? 8. In a chemical reaction, how does the mass of the reactants compare with the mass of the products? 9. What is the difference between chemical and physical properties? Give examples. 10. What is the main difference between physical and chemical changes? 11. Classify each of the following as physical or chemical changes: a. Water boiling d. A metal rusts b. Milk turns sour e. Wood burns c. Salt dissolves in water f. ice melts 12. What are the differences between extensive and intensive properties? 13. Is a solution considered homogeneous or heterogeneous? How many phases does a solution have? 14. Explain the process of distillation and describe the goal of distillation. 15. How can you distinguish between elements and compounds? 16. Explain the compositions of the following substances by looking at their chemical formulas: a. H 2O c. C 6H 12O 6 b. NH 3 d. CH What are the properties of solids, liquids, and gases? Which have a definite volume? Which take the shape of their container? 2
3 Chapter 3: 1. Count the significant figures in each length a meters c meters b meters d meters 2. How many significant figures are in each measurement? a. 143 grams c meters b x 10-2 grams d meters 3. Round each measurement to three significant figures. Write your answers in scientific notation. a b x 10 8 meters c meter d meters e x 10-3 meters f meters 4. Perform each operation. Express your answers to the correct number of significant figures. a meters meters meters b meters meters c meters meters d meters 17.3 meters 5. Solve each problem. Give your answers to the correct number of significant figures and in scientific notation. a. 8.3 meters x 2.22 meters b meters / 12.5 c seconds x (1 minute / 60 seconds) 6. Solve the following and express each answer in scientific notation and to the correct number of significant figures. a. (5.3 x 10 4 ) + (1.3 x 10 4 ) b. (7.2 x 10-4 ) / (1.8 x 10 3 ) c x 10-3 x 10 6 d. (9.12 x 10-1 ) (4.7 x 10-2 ) e. (5.4 x 10 4 ) x (3.5 x 10 9 ) 7. Name the quantity measured by each of the seven SI base units and give the SI symbol of the unit. 8. State the difference between mass and weight. 9. State the relationship between degrees Celsius and kelvins. 10. Using tables from this chapter, convert the following. a km to meters 3
4 b mg to grams c g to centigrams 11. Covert the following a. 15 cm 3 to liters b. 6.7 s to milliseconds c g to micrograms 12. A 68-g bar of gold is cut into 3 equal pieces. How does the density of each piece compare to the density of the original gold bar? 13. Round off each of these measurements to three significant figures. a L b cg c m d C 14. What equation is used to determine the density of an object? 15. What is the difference between accuracy and precision? 16. Which is the estimated digit when using significant figures? 17. Using the density formula, how do you solve for mass, density, and volume? 18. What is the difference between the accepted and experimental value? 19. How do you use conversion factors? 20. What is dimensional analysis? 21. What is the order and values of the metric prefixes from largest to smallest? 4
5 Chapter 4: 1. How do we use shorthand notation to provide information about atoms of elements. *Give an example. 2. How did Democritus characterize atoms? 3. According to Dalton s Theory is it possible to convert atoms of one element into atoms of another? Explain! 4. What are the charges and relative masses of the three main subatomic particles? 5. Three isotopes of oxygen are oxygen-16, oxygen-17 and oxygen 18. Write the symbol for each including the atomic number and mass number. a. c. b. 6. What distinguishes the atoms of one element from the atoms of another? 7. What equation tells you how to calculate the number of neutrons in an atom? 8. What is the charge- positive or negative, of the nucleus of every atom? 9. Why is an atom electrically neutral? 10. What does the atomic number of each atom represent? 11. How are the elements on the modern periodic table arranged? 12. What are the parts of an atom? What are their charges? Where are they located? 13. What is the difference between mass number and atomic mass? 14. Which subatomic particle is mainly responsible for the properties of each element? 15. Which subatomic particle makes each atom unique? 5
6 Chapter 5 1. How do two sublevels of the same principle energy level differ from each other? 2. How can electrons in an atom move from one energy level to another? 3. How many orbitals are in the following sublevels? a. 3p sublevel- c. 4p sublevel- e. 4f sublevel- b. 2s sublevel- d. 3d sublevel- 4. What is an atomic orbital? 5. How many sublevels are contained in each of these principle energy levels? a. 1 st - b. 2 nd - c. 3 rd - d. 4 th - 6. How many electrons are in the highest occupied energy level of these atoms? a. Barium - b. Sodium- c. Aluminum- d. Oxygen- 7. What are the three rules that govern the filling of the atomic orbitals by electrons? a. b. c. 8. Give electron configurations for atoms of these elements: a. Na b. S c. Mg d. Ne e. K 9. What is the maximum number of electrons that can go into each of the following sublevels? a. 2s- c. 3p- e. 4s- g. 3d- b. 4p- d. 5s- f. 4f- h. 5p- 10. Give the symbol for the atom that corresponds to the following electron configurations: a. 1s 2 2s 2 2p 6 3s 2 3p 6 b. 1s 2 2s 2 2p 6 3s 2 3p 6 3d 10 4s 2 4p 6 4d 7 5s 1 c. 1s 2 2s 2 2p 6 3s 2 3p 6 3d 10 4s 2 4p 6 4d 10 4f 14 5s 2 5p 6 5d 1 6s An atom of an element has two electrons in the first energy level and five electrons in the second energy level. Write the electron configuration for this atom and name the element. How many unpaired electrons does an atom of this element have? a. Electron Configuration- 6
7 b. Name- c. Unpaired electrons- 12. What is the difference between a cation and an anion? 13. How many electrons fit into each principal quantum number? (also known as an energy level.) 14. How many orbitals will the s, p, d, & f sublevels hold? How many electrons in each orbital? 15. Compare Hund s rule, the Aufbau principle, and the Pauli Exclusion Principle. 16. Is it more stable for an atom to have 3 partially filled orbitals or 2 filled and 1 empty orbital? Chapter 6 1. How are the elements arranged on the modern periodic table? 2. Identify each element as a metal, nonmetal or metalloid: a. Gold- c. Siliconb. Sulfur- d. Barium- 3. Into what four classes can element be sorted based on their electron configurations? 4. Classify each element as a represented elements, transition metal or noble gas: a. 1s 2 2s 2 2p 6 3s 2 3p 6 3d 10 4s 2 4p 6 - b. 1s 2 2s 2 2p 6 3s 2 3p 6 3d 10 4s 2 - c. 1s 2 2s 2 2p 6 3s 2 3p 2-5. How does atomic size change within groups and across the periods? 6. When do ions form? 7. Compare the size of ions to the size of the atom from which they form. 8. How does electronegativity vary within groups and across periods? 7
8 9. Identify each property below as a characteristic of either a metal or nonmetal a. A gas at room temp- c. Malleable- d. Shiny- b. Brittle- d. Poor conductor of electric current- 10. Where are the alkaline metals, the alkaline earth metals, the halogens and the noble gases located on the periodic table? 11. Which noble gas does not have eight electrons in its highest occupied energy level? 12. Explain the difference between the first and second ionization energy of an element. 13. For groups 1A 7A, how many electrons fill the outermost sublevel? 14. How are the electron configurations for the atoms in each group of representative elements similar? 15. Where are the noble gases located on the periodic table? Why are these elements noble? 16. What is the difference between ionization energy and electronegativity? 17. Why does atomic size decrease across a period? 18. What are the group and period trends for atomic size, ionization energy, electronegativity, shielding effect, and ionic radius? 19. What is the difference between shielding electrons and valence electrons? 20. What is the difference between an anion and a cation? Why do they form? 21. How are the electron configurations of ions different than those of their neutral version? 22. What is the octet rule? 23. Why are copper, silver, and zinc likely to form pseudo-noble gas electron configurations? Chapter 7 1. How many electrons are lost or gained in the forming of each ion? a. Ba 2+ 8
9 b. As 3- c. Cu How can you determine the number of valence electrons in an atom of a representative element? 3. Atoms of which element tend to gain electrons? Atoms of which elements tend to lose electrons? 4. How many valence electrons are in each atom? a. Potassium b. Carbon c. Magnesium d. Oxygen 5. Draw the electron dot structure for each atom. a. Potassium c. Carbon b. Magnesium d. Oxygen 6. Use the dot structure to determine formulas of the ionic compounds formed when a. Potassium reacts with iodine. b. Aluminum reacts with oxygen. 7. What properties characterize ionic compounds? 8. How many electrons must each atom lose to attain a noble-gas electron configuration? a. Ca b. Al c. Li d. Ba 9. How many electrons must each atom gain to attain a noble-gas electron configuration? a. N b. S c. Cl d. P 10. Which of the following pairs of atoms would you expect to combine chemically to form an ionic compound? a. Li and S b. O and S c. Al and O d. F and Cl e. I and K f. H and N 11. Explain why ionic compounds are electrically neutral. 12. Explain briefly why metals are good conductors of electricity. 13. Which of the following substances are most likely not ionic? a. H 2O 9
10 b. Na 2O c. CO 2 d. CaS e. SO 2 f. NH Which particle plays the most important role in chemistry? 15. What is an ionic bond? An ionic compound? 16. What are the characteristics of ionic compounds? 17. What are the properties of metals and metallic bonds? 18. What is a monatomic ion? 19. What is true about the charges of transition metal ions? Chapter 8 1. How are the melting points and boiling points of molecular compounds usually different from ionic compounds? 2. What information does the molecular formula provide? 3. The following molecules have single covalent bonds. Draw an electron dot structure for each. a. H 2O 2 b. PCl 3 4. What electron configurations do atoms usually achieve by sharing electrons to form covalent bonds? 5. How is a coordinate covalent bond different from other covalent bonds? 6. Draw the electron dot resonance structure for ozone (O 3) and explain how they describe its bonding. 10
11 7. Draw electron dot structures for the following molecules, which have only single covalent bonds. a. H 2S b. PH 3 c. ClF 8. Identify the bonds between atoms of each pair of elements as nonpolar covalent, moderately polar covalent, very covalent, or ionic. a. H and Br b. K and Cl c. C and O d. Cl and F e. Li and O f. Br and Br 9. Place the following covalent bonds in order from least to most polar. a. H-Cl b. H-Br c. H-S d. H-C 10. Which of the following gases in Earth s atmosphere would you expect to find as molecules and which as individual atoms? a. Nitrogen b. Oxygen c. Argon 11. Classify the following compounds as ionic or covalent. a. MgCl 2 b. Na 2S c. H 2O d. H 2S 12. How many electrons do two atoms in a double covalent bond share? How many in a triple covalent bond? 13. Characterize a coordinate covalent bond and give an example. 14. Using electron dot structure, draw at least two resonance structures for the nitrite ion (NO 2 -). The oxygen in NO 2 - are attached to the nitrogen. 15. How must the electronegativities of two atoms compare if a covalent bond between them is to be polar? 16. What are the diatomic elements? 11
12 17. What is the difference between single, double, and triple covalent bonds? 18. What does it mean when resonance structures occur? 19. Explain how phosphorus and sulfur are sometimes exceptions to the octet rule. 20. What is a polar covalent bond? 21. What is a polar molecule? 22. What is hydrogen bonding and how does it work? 23. How can elements achieve a noble gas configuration? 24. What are the bond angles of some common molecules using the VSEPR theory? Organic 1. What is an isomer? Give an example. 2. Define and give an example of each of the following. a. Alkane b. Alkene c. Alkyne 3. What is the molecular formula of each of the following? a. Methane b. Ethane 12
13 c. Propane d. Butane Chapter 9 1. Write the formulas for compounds formed from these pairs of ions. a. Ba 2+, S 2- b. Li +, O 2- c. Ca 2+, N 3- d. Cu 2+, I - 2. Write formulas for these compounds. a. Sodium iodide b. Tin (II) chloride c. Potassium sulfide d. Calcium iodide 3. Write formulas for compounds formed from these pairs of ions. a. NH 4 +, SO 3 2- b. Calcium ion, phosphate ion 4. Write formulas for these compounds. a. Lithium hydrogen sulfate b. Chromium (III) nitrite 5. Give the expected charge of the cations of these elements. a. Sr b. Ca c. Al d. Cs 6. What is the net ionic charge of every ionic compounds? Explain. 7. Which of the following compounds are binary ionic compounds? a. KBr b. K 3PO 4 c. Sodium nitride d. Calcium sulfate 8. Complete the table by writing correct formulas for the compounds formed by combining positive and negative ions. Then name each compound in the space below the table. NO 3 - CO 3 2- CN - PO
14 NH 4 + a. b. c. d. Sn 4+ e. f. g. h. Fe 3+ i. j. k. l. Mg 2+ m. n. o. p. a. h. n. b. i. o. c. j. p. d. k. e. l f. m. 9. What prefix indicates each of the following numbers of atoms in the formula of a molecular compound? a. 3 d. 6 b. 1 e. 5 c. 2 f Write the formula or name for these compounds. a. Boron trichloride b. N 2O 5 c. Dinitrogen tetrahydride d. CCl Give the name or the formula for these acids. a. HCl b. Sulfuric acid c. HNO 3 d. Acetic acid 12. Write names or formulas for these compounds. a. Iron (II) hydroxide b. Pb(OH) 2 c. Copper (II) hydroxide d. Co(OH )2 14
15 13. Write formulas for these compounds. a. Potassium permanganate b. Calcium hydrogen carbonate c. Dichlorine heptaoxide d. Trisilicon tetranitride e. Sodium dihydrogen phosphate f. Phosphours pentabromide g. Carbon tetrachloride 14. Name these compounds. a. NaClO 3 b. Hg 2Br 2 c. K 2CrO 4 d. HClO 4 e. SnO 2 f. Fe(C 2H 3O 2) 3 g. KHSO 4 h. Ca(OH) 2 i. BaS 15. Name each compound. a. Mg(MnO 4) 2 b. Be(NO 3) 2 c. K 2CO 3 d. N 2H 4 e. LiOH f. BaF 2 g. PI 3 h. ZnO 15
16 i. H 3PO A compound of general formula Q xr y contains no hydrogen and Q and R are both elements. Neither Q nor R is a metal. Is Q xr y an acid, a binary ionic compound, an ionic compound containing a polyatomic anion, or a binary molecular compound? 17. Explain what is wrong with each formula. a. CsCl 2 b. ZnO 2 c. LiNe d. Ba 2S What is the difference between a molecular and an ionic compound? 19. How can you tell from looking at the formula that a compound is ionic or molecular? 20. What is a salt? 21. When given the name of the compound, how do you write formulas for molecular compounds? 22. When given the formula, how do you name ionic and molecular compounds? 23. How do you name and write formulas for acids and bases? 24. What is a binary compound? When given the name of the compound or the formula of the ions, how do you write formulas for ionic compounds? Chapter How many moles is 2.80 x atoms of silicon? 2. How many moles is 2.17 x representative particles of bromine? 3. How many moles are in 4.65 x molecules of NO 2? 16
17 4. What is the mass of 1.00 mol of sodium hydrogen carbonate? 5. Find the number of moles in 3.70 x 10-1 g of boron. 6. Calculate the number of moles in 75.0 g of dinitrogen trioxide. 7. What is the volume of these gases at STP? a x 10-3 mol CO 2 b mol N 2 8. At STP, what volume do these gases occupy? a mol He b mol C 2H 6 9. A gaseous compound of sulfur and oxygen, which is linked to the formation of acid rain, has a density of 3.58 g/l at STP. What is the molar mass of this gas? 10. What is the density of krypton gas at STP? 11. A compound is formed when 9.03 g Mg combines completely with 3.48 g N. What is the percent composition of this compound? 12. When a 14.2 g sample of mercury (II) oxide is decomposed into its elements by heating, 13.2 g Hg is obtained. What is the percent composition of the compound? 13. Calculate the empirical formula of each compound. a. 94.1% O, 5.9% H b. 67.6% Hg, 10.8% S, 21.6% O 14. 1,6-diaminohexane is used to make nylon. What is the empirical formula of this compound if it is 62.1% C, 13.8% H, and 24.1% N? 17
18 15. Find the molecular formula of ethylene glycol, which is used as antifreeze. The molar mass is 62 g/mol and the empirical formula is CH 3O. 16. Which pair of molecules has the same empirical formula? a. C 2H 4O 2, C 6H 12O 6 b. NaCrO 4, Na 2Cr 2O Calculate the molar mass of each substance. a. H 2PO 4 b. N 2O 3 c. CaCO 3 d. (NH 4) 2SO 4 e. C 4H 9O 2 f. Br How many moles is each of the following? a g SiO 2 b g AgCl c G Cl 2 d g KOH e. 937 g Ca(C 2H 3O 2) 2 f g Ca 19. Find the mass of each substance. a mol C 5H 12 b mol F 2 18
19 c mol Ca(CN) 2 d mol H 2O 2 e mol NaOH f x 10-2 mol Ni 20. Calculate the percent composition of each compound. a. H 2S b. (NH 4) 2C 2O 4 c. Mg(OH) 2 d. Na 3PO Which of the following can be classified as an empirical formula? a. S 2Cl 2 b. C 6H 10O 4 c. Na 2SO What is the molecular formula for each compound? Each compound s empirical formula and molar mass is given. a. CH 2O, 90 g/mol b. HgCl, g/mol 23. Determine the molecular formula for each compound. a. 94.1% O and 5.9% H; molar mass = 34 g b. 50.7% C, 4.2% H, and 45.1% O; molar mass = 142 g 24. Determine the empirical formula of compounds with the following percent compositions. a. 42.9% C and 57.1% O b % C, 42.66% O, 18.67% N, and 6.67% H c % Cl, 16.16% O, and 12.12% C 19
20 25. What does the term STP mean? 26. What is the volume of 1 mole of any gas at STP? 27. When given the name of the compound or the formula of the ions, how do you write formulas for ionic compounds? 28. What is Avogadro s number? 29. What is a mole? 30. What are representative particles of elements? Molecular compounds? Ionic compounds? 31. How do you convert from representative particles to moles? 32. How do you convert from moles to representative particles? 33. What is molar mass? 34. How do you convert moles to mass? Mass to moles? 35. What is standard temperature and pressure? 36. How do you convert moles of a gas to STP? 37. How do you find the density of a STP when you know the formula? 38. How do you find percent composition? 39. How do you determine the empirical formula and the molecular formula of a compound? Additional Topics to Review Review the correct use of parentheses ( ) in formulas Know these molecular shapes: tetrahedral, pyramidal, bent, linear Study the stock and classical names for transition metal ions (p 255) Review the polyatomic ions (p. 257) Study p. 277 and p. 278 for extra help in naming and writing formulas of compounds Look over the note cards for all chapters. 20
Mid-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 informationCh. 1: Introduction to Chemistry. Ch. 2: Matter and Change
Review Sheet for Chemistry First Semester Final Refer to your class notes, worksheets, and the textbook to complete this review sheet. Study early so that you will have time to ask questions about what
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 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 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 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 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 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 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 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 informationMIDTERM STUDY GUIDE. Chapter 1 Introduction to Chemistry
MIDTERM STUDY GUIDE Chapter 1 Introduction to Chemistry What is chemistry? Chemical properties vs. physical properties examples of both States of matter Scientific method Chapter 2 Data Analysis SI measurement
More informationRegents review Atomic & periodic
2011-2012 1. The diagram below represents the nucleus of an atom. What are the atomic number and mass number of this atom? A) The atomic number is 9 and the mass number is 19. B) The atomic number is 9
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 informationUnit Five Practice Test (Part I) PT C U5 P1
Unit Five Practice Test (Part I) PT C U5 P1 Name Period LPS Standard(s): --- State Standard(s): 12.3.1 Short Answers. Answer the following questions. (5 points each) 1. Write the electron configuration
More informationPeriodic Table Workbook
Key Ideas: The placement or location of elements on the Periodic Table gives an indication of physical and chemical properties of that element. The elements on the Periodic Table are arranged in order
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 informationPeriodic Table Practice 11/29
Periodic Table Practice 11/29 1. The arrangement of the elements from left to right in Period 4 on the Periodic Table is based on A) atomic mass B) atomic number C) the number of electron shells D) the
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 informationHonors Chemistry Semester 1 Final Review
Honors Chemistry Semester 1 Final Review Ch. 1 Introduction to Chemistry Chemistry: its branches, technology, scientific method, and problem solving. 1. Know the definition of matter. 2. Know the definition
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 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 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 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 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 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 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 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 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 informationA) first electron shell D) are located in orbitals outside the nucleus A) 2-3 D) 18 A) K and Na C) a mixture C) Sb2O5
1. In a calcium atom in the ground state, the electrons that possess the least amount of energy are located in the A) first electron shell B) second electron shell C) third electron shell D) fourth electron
More informationName Midterm Review Date
Name Midterm Review Date 1. In which process does a solid change directly into a vapor? A) sublimation B) deposition C) condensation D) solidification 2. What is the molecular formula of a compound that
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 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 informationName: Midterm Review Date:
Name: Midterm Review Date: 1. Which statement concerning elements is true? A) Different elements must have different numbers of isotopes. B) Different elements must have different numbers of neutrons.
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 informationAP Chemistry Summer Assignment
AP Chemistry Summer Assignment 1) Name this compound: Cr 3 (PO 4 ) 2 a) Chromium Diphosphate b) Trichromium Phosphate c) Chromium (II) Phosphate d) Chromium (II) Diphosphate 2) How many significant figures
More informationBonding Mrs. Pugliese. Name March 02, 2011
Bonding Mrs. Pugliese Name March 02, 2011 1. Atoms of which element have the greatest tendency to gain electrons? 1. bromine 3. fluorine 2. chlorine 4. iodine 2. Which polyatomic ion contains the greatest
More informationUnit 7 Study Guide: Name: KEY Atomic Concepts & Periodic Table
Unit 7 Study Guide: Name: KEY Atomic Concepts & Periodic Table Focus Questions for the unit... How has the modern view of the atom changed over time? How does a chemist use symbols and notation to communicate
More informationFirst 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 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 informationSecond Semester Chemistry Study Guide
Second Semester Chemistry Study Guide All of the information on this review is fair game for the final Some information will be more prevalent on the test (Think about which topics we spent more time on
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 informationELECTRONS. Construct your own electron dot diagram Choose one element & drag the correct number of VALENCE Br electrons around it.
Ch. 6 - Chemical Bonds Chemical reactivity depends on electron configuration. Remember the Stable Octet rule: when the highest energy level occupied is filled with electrons (8 electrons for most atoms),
More informationQuestions 1 to 58 must be answered on the Scantron sheets.
Questions 1 to 58 must be answered on the Scantron sheets. Base your answers to questions 1 to 5 on the heating curve for a pure substance that is shown below. 1. The freezing point of the substance is
More informationCHAPTER 8 Ionic and Metallic Bonds
CHAPTER 8 Ionic and Metallic Bonds Shows the kind of atoms and number of atoms in a compound. MgCl 2 NaCl CaCO 3 Al 2 O 3 Ca 3 (PO 4 ) 2 Chemical Formulas Al: Cl: counting atoms AlCl 3 Pb: N: O: Pb(NO
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 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 informationPractice Periodic Table Review
Practice Periodic Table Review Name 1. An electron will emit energy in quanta when its energy state changes from 4p to A) 5s B) 5p C) 3s D) 6p 2. Which electron configuration represents an atom in the
More informationAnswers to SNC 2DI Exam Review: Chemistry Unit 1. Understand the meaning of the following terms. Be able to recognize their definitions:
Answers to SNC 2DI Exam Review: Chemistry Unit 1. Understand the meaning of the following terms. Be able to recognize their definitions: Protons Chemical amily or Group Ionic compound Double displacement
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 informationName: 1. The mass of a proton is approximately equal to the mass of (1) an alpha particle (2) a beta particle (3) a positron (4) a neutron
Chemistry Section Name: MID TERM STUDY GUIDE Date: A. Multiple Choice. 1. The mass of a proton is approximately equal to the mass of (1) an alpha particle (2) a beta particle (3) a positron (4) a neutron
More informationUNIT 5.1. Types of bonds
UNIT 5.1 Types of bonds REVIEW OF VALENCE ELECTRONS Valence electrons are electrons in the outmost shell (energy level). They are the electrons available for bonding. Group 1 (alkali metals) have 1 valence
More information1 st Semester Final Review Sheet (Chapters 2-7)
CP Chemistry Name: Period: 1 st Semester Final Review Sheet (Chapters 2-7) Matter (Chapter 2) 1. What is the definition of an element? 2. What is the definition of a compound? 3. What is the definition
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 informationTest Review # 4. Chemistry: Form TR4-5A 6 S S S
Chemistry: Form TR4-5A REVIEW Name Date Period Test Review # 4 Development of the Periodic Table. Dmitri Mendeleev (1869) prepared a card for each of the known elements listing the symbol, the atomic mass,
More information1. The elements on the Periodic Table are arranged in order of increasing A atomic mass C molar mass
1. The elements on the Periodic Table are arranged in order of increasing A atomic mass C molar mass A Br, Ga, Hg C O, S, Se B atomic number D oxidation number 2. Which list includes elements with the
More informationName: Unit 1: Nature of Science
Name: Unit 1: Nature of Science 1. Using the picture above, list lab safety rules that are being ignored. 2. What are the steps to the scientific method? 3. Convert the following into scientific notation:
More informationNOTES PACKET COLLIER CHEMISTRY PRE-AP
SECOND NINE WEEKS NOTES PACKET COLLIER CHEMISTRY PRE-AP 1 2 UNIT 5 CHEMICAL NAMING & BALANCING Chapter 6, 15.1, 16.1 3 NOMENCLATURE: Atoms of elements combine to form that are represented by. All compounds
More informationChapter 2. The Components of Matter
Chapter 2. The Components of Matter 1 The Periodic Table (Section 2.6) 13 Al 26.981 Main Idea: 1. Groups: Old numbering system: New IUPAC numbering system: 2. Periods: 3. Know the names and properties
More information1. The elements on the Periodic Table are arranged in order of increasing A atomic mass C molar mass
1. The elements on the Periodic Table are arranged in order of increasing A atomic mass C molar mass A Br, Ga, Hg C O, S, Se B atomic number D oxidation number 2. Which list includes elements with the
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 informationBonding Practice Exam
Bonding Practice Exam Matching Match each item with the correct statement below. a. halide ion e. valence electron b. octet rule f. coordination number c. ionic bond g. metallic bond d. electron dot structure
More informationPractice Multiple Choice
Practice Multiple Choice 1. A theory differs from a hypothesis in that a theory A. cannot be disproved C. always leads to the formation of a law B. represents an educated guess D. has been subjected to
More informationMid-Term Review Multiple Choice: Ch. 3 Identify the letter of the choice that best completes the statement or answers the question.
HONORS CHEMISTRY MID-TERM PRACTICE January 2013 Mrs. Allen from HS North put together a collection of multiple choice questions for you to use as a study tool. Not all of the midterm topics are covered
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 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 informationFirst 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 4 1. Explain the law of conservation of mass. 2. What mass of product is produced in the following
More informationNaming and Counting Atoms and Molecules. Chemistry--Unit 2
Naming and Counting Atoms and Molecules Chemistry--Unit 2 Masses of 22.4 L O 2, N 2, & HCl N 2 28 g O 2 32 g HCl 36.5 g Observation: At 1 atmosphere pressure and 0 o C, 22.4 L of 3 different gases have
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 information2 A ruler is marked in.1 cm intervals. What is the uncertainty associated with the ruler? a) 1 cm b) 0.1 cm c) 0.01 cm d) cm
Practice Final (Print) Name last First Signature Introduction to General Chemistry, Ch152 Practice Final Exam 1 Who was first responsible for presenting the planetary model of the atom? a) Dalton b) Millikan
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 information1. The arrangement of the elements from left to right in Period 4 on the Periodic Table is based on
1. The arrangement of the elements from left to right in Period 4 on the Periodic Table is based on A) atomic mass B) atomic number C) the number of electron shells D) the number of oxidation states 2.
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 informationChapter 9 Periodic Law The structure of molecules and describing reactions
Chapter 9 Periodic Law The structure of molecules and describing reactions Reading Assignment: Read the entire chapter. Homework: see the web site for homework. http://web.fccj.org/~smilczan/psc/homework7_11.htm
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 informationNAME: DATE: CLASS: Chapter Metallic Bonding
Chapter 7 7.3 Metallic Bonding Ionic & Metallic Bonding 1. LESSON REVIEW Use the diagram of metallic bonding to answer the following questions. 1. What is the name of the model of metallic bonding that
More informationTest Review # 4. Chemistry: Form TR4-9A
Chemistry: Form TR4-9A REVIEW Name Date Period Test Review # 4 Location of electrons. Electrons are in regions of the atom known as orbitals, which are found in subdivisions of the principal energy levels
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 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 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 informationCHEMISTRY HONORS LEOCE Study Guide
BENCHMARK: N.1.1-1.2, N.1.6, N.3.1, N.3.3, N.3.4 CHEMISTRY HONORS CHEMISTRY AND SCIENTIFIC MEASUREMENT TEXTBOOK: Glencoe, Chemistry: Matter and Change, Chapters 1-3 ESSENTIAL QUESTION: How is measurement
More informationDescription Computer Bonding. Late Lab Stamp (this stamp means you are not qualified to do lab and test corrections) Name: Period:
Chemistry: Hood River Valley High School Unit 4 Note Pack and Goals Name: Period: Unit 4 Metals, Non-Metals, Metalloids, Ions, and Ionic compounds. Unit Goals- As you work through this unit, you should
More informationSymbol Atomic Number
Name: Date: Chemistry ~ Ms. Hart Class: Anions or Cations February Break Review Sheets - /150 Chemistry has a LOT of words. Take this break to review and strengthen your knowledge of the vocabulary you
More informationOrganizing the Periodic Table
Organizing the Periodic Table How did chemists begin to organize the known elements? Chemists used the properties of the elements to sort them into groups. The Organizers JW Dobereiner grouped the elements
More informationWrite the name or formula for:
Do Now Date: Tuesday, November 2, 2015 Objective: Name and write formulas for ionic and molecular (covalent) compounds. Write the name or formula for: K 2 SO 4 NaNO 3 Calcium Hydroxide Tuesday, November
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 informationRed Hook Central High School. Honors CHEMISTRY. Midterm Examination. Thursday, January 25, :30 to 2:30 p.m., only. Notice...
Red Hook Central High School Honors CHEMISTRY Midterm Examination Thursday, January 25, 2018 11:30 to 2:30 p.m., only This is a test of your knowledge of chemistry. Use that knowledge to answer all questions
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 informationACCELERATED CHEMISTRY SEMESTER 1 PROBLEM SHEET
ACCELERATED CHEMISTRY SEMESTER 1 PROBLEM SHEET 100. Determine the number of significant figures in the following numbers: a. 100 b. 0.000123 c. 1.00300 d. 1.2300 e. 1.20 x 10 16 f..00010100 Write the following
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 informationCHEMICAL NAMES AND FORMULAS
CHEMICAL NAMES AND FORMULAS Practice Problems In your notebook, solve the following problems. SECTION 9.1 NAMING IONS What is the charge on the ion typically formed by each element? a. oxygen c. sodium
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 informationA1 Models of the atom. A2 Size of the atom
A1 Models of the atom 1. Describe the improvements to our understanding of the atom from each of the following scientists: 1.1. Democritus 1.2. Dalton 1.3. Thomson 1.4. Rutherford 1.5. Bohr 1.6. Chadwick
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 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 informationSemester II Final Exam Study Questions Answer Key
Semester II Final Exam Study Questions Answer Key Unit 5: Matter Standards: Standard 1: Structure and Properties of Matter All matter is made up of atoms. Its structure is made up of repeating patterns
More informationTHE ST. MICHAEL SCHOOL THIRD FORM CHEMISTRY MANUAL 3 SYMBOLS AND FORMULAE, CHEMICAL BONDING AND CHEMICAL EQUATIONS
1 THE ST. MICHAEL SCHOOL THIRD FORM CHEMISTRY MANUAL 3 SYMBOLS AND FORMULAE, CHEMICAL BONDING AND CHEMICAL EQUATIONS COMPILED BY G.WALKER, L.WORRELL, T. HARDING REFERENCE BOOKS Anne Tindale Chemistry A
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 informationHomework Packet Unit 2. b. Al 3+, F, Na +, Mg 2+, O 2
Name Period Homework Packet Unit 2 1. Which of the following is the correct empirical formula for a compound that has 37.5% C, 12.6% H, and 49.9% O? (A) C 2 H 4 O (B) CH 4 O 2 (C) CH 5 O 2 (D) CH 4 O (E)
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 informationH 2 O. Chapter 9 Chemical Names and Formulas
H 2 O Chapter 9 Chemical Names and Formulas Section 9.1 Naming Ions OBJECTIVES: Identify the charges on monatomic ions by using the periodic table, and name the ions. Section 9.1 Naming Ions OBJECTIVES:
More information