Regents Chemistry Midterm Study Guide



Regents Chemistry Midterm Study Guide

Midterm Exam Format:

The midterm exam was decided to follow the same exact format of a NYS regents exam. The exam consists of four parts and they are titled parts A, B-1, B-2 and C. The first two parts of the exam are multiple choice questions.

The first two parts of the exam are made up of 50 multiple choice questions all of which are worth 1 point each. Part A consists of 30 multiple choice questions that are designed to assess your knowledge of some of the basic chemistry concepts and definitions you have learned so far this year. Part B-1 is also made up of multiple choice questions, but these questions are designed to assess how well you can apply the concepts you have learned so far this year. These questions may require you to perform calculations, interpret a diagram or use information found on your reference tables.

The last two parts of the exam are made up of 31 short-answer (written) questions that can be worth either 1 or 2 points depending on the question asked. Part B-2 consists of 14 short answer questions that involve completing diagrams, and interpreting data given. The questions asked in this section may involve setting up and calculating answers based on equations you have learned so far this year as well as applying information given from your reference tables. Part C consists of 17 short answer (written) questions that involve the interpretation of data given. Some part C questions may require a longer response (no more than a sentence), but will also involve setting up and calculating answers based on equations you have learned so far this year. You may have to construct an appropriate graph or analyze a graph in this section and answer questions based on the graph constructed.

The exam has a total of 85 possible points between the 4 parts (some questions are worth 2 points) and your grade on the exam will be based on a scaled score not a straight percentage.

All of the questions on the midterm exam are questions that have been on old regents exams over the last several years. Feel free to look at the old exams in the back of your regents chemistry review books or online (google search regents chemistry exams) for examples of questions you could be asked just try to ignore questions on things we have not covered.

Reference Table Charts used on the Midterm Exam

Table A: Standard Temperature and Pressure (STP)

This data was used mainly during the “Gases” unit when using the combined gas law equation (table T).

Table B: Physical constants of water

This data was used mainly during the “energy and heat calculations unit” when using the heat equations (table T).

Table C: Selected prefixes

This data was used mainly during the “metric measurement unit” when performing metric unit conversions.

Table D: Selected Units

The units listed on the table were used in several units completed so far. The only units that are on table D that have not been covered yet are the last two “ppm” and “M” they will be used later in the year and will not be on the midterm.

Table E: Selected Polyatomic Ions

The data found on this chart was used during the “formula writing unit”. Polyatomic ions are essentially groups of atoms that have gained or lost electron(s) giving them a charge.

Table F: Solubility Guidelines for Aqueous Solutions

The data found on this chart was used during “part 2 of the chemical equations unit” when deciding weather or not the products from a double replacement reaction will dissolve in water or are soluble. Remember if soluble assign an (aq) symbol to show it is dissolved in water, if insoluble assign an (s) symbol to show it forms a precipitate. And also remember that only double replacement reactions that for an insoluble product (s) go to completion.

Table H: Vapor Pressure of Four Liquids

The data displayed on this graph was used during the “vapor pressure and boiling unit”. Remember a substances normal boiling point is the temperature at which vapor pressure is equal to standard atmospheric pressure. Any substance will boil when its vapor pressure is equal to the atmospheric or external pressure.

Table J: Activity or Reactivity Series

The data from this chart was used during “part 2 of the chemical equations unit” when deciding whether or not a single replacement reaction was spontaneous or would work. Remember the lone element will replace the element in compound with the same ionic charge only if the lone element is higher up on table J. If the lone element forms a positive ion it will replace positive ion in compound and form a new compound as long as it’s higher up on table J. If the lone element forms a negative ion then it will replace the negative ion in compound and form a new compound as long as it’s higher up on table J. When the lone element is more active than the ion it will replace then the reaction is spontaneous (will occur). If the lone element is less active than the ion it will replace then the reaction is non-spontaneous (will not occur).

The Periodic Table

The data from this table was used during several units covered throughout the first half of the year. It was used the most during the “atomic structure unit”, and the “formula writing unit.” Make sure you know the definitions of the atomic mass (different than mass number), atomic number and the electron configuration as well as the information you can obtain from these values.

Table S: Properties of Selected Elements

The data from this table was used during several units covered throughout the first half of the year. This table can be used to identify the symbol of an element or the name if given the symbol (do not guess when you can look it up). You can also find an elements melting and boiling points and density.

Table T: Important Formulas and Equations

All of the equations we have used for the first half of the year are found on this table. So far we have used the density equation, the mole calculation equation, the percent error equation, the percent composition (by mass) equation, the combined gas law equation, the heat equations, and the temperature conversion equation. All of the equations we have used are listed, but you will have to decided, based on what you have learned, when to use them.

Review Book Topics Covered On the Regents Chemistry Midterm

Your review book should be a very useful tool as you study for the chemistry midterm. All of the topics we have discussed in class are explained in detail, and there are a wide variety of practice questions that you can answer to see how well you understand what you have learned so far. Here is a list of the topics and pages in your review books that you should study to help prepare you for the chemistry midterm exam.

Topic 1: The Atom

Topic 2: Formulas and Equations

Topic 3: The Mathematics of Formulas and Equations

Topic 4: Physical Behavior of Matter

Things You MUST Know For Your Chemistry Midterm are

1. The relationship between gram formula mass of a substance and moles of a substance.

2. How to setup and answer an equation stoich problem mole to mole.

3. The conclusions made by Rutherford as a result of his famous experiment.

4. What an orbital is according to the modern model of an atom.

5. What information can be obtained from an isotopic symbol.

6. How to find or calculate the number of protons, neutrons or electrons a neutral atom has.

7. How to calculate atomic mass (using percentages and masses of the isotopes)

8. How does the energy of an electron change as it moves from a higher shell to a lower shell or from a lower shell to a higher shell.

9. Elements that form different molecules will have different structures and properties.

10. The difference between a chemical property and a physical property and examples of both, and the difference between chemical and physical changes and examples.

11. The difference between ground state and excited state.

12. What information can be obtained from an electron configuration and where to find it.

13. The definitions of matter, a substance, a mixture, a compound, and an element and the ability to identify examples of each.

14. How to calculate density and where to find the densities of elements in your reference tables.

15. How the particles are arranged in the solid, liquid and gas phases as well as the symbols used to represent each phase.

16. The properties used to separate mixtures during distillation, filtration, chromatography and other lab techniques used in class.

17. How to measure the average kinetic energy of matter.

18. The temperature and pressure conditions when gases behave like ideal gases.

19. The parts of the Kinetic Molecular Theory, and how to use them to explain the relationships between Temp & Pressure, Volume & Pressure and the number of gas particles and pressure.

20. Avagadro’s hypothesis on samples of gases there volumes and the number of particles.

21. When the potential energy of a substance increases or decreases and when the average kinetic energy of a substance increases or decreases during heating or cooling.

22. What happens to the external temperature during an exothermic reaction and an endothermic reaction.

23. Where to find Standard Temperature and Pressure or STP?

24. How to read table H.

25. What substances can be broken down by chemical reactions and what substances can not be broken down by chemical reactions.

26. The relationship between moles and grams and how to convert between the two units.

27. The difference between an ionic compound and a molecular compound.

28. How to count elements in a compound and the numbers of different atoms in a compound.

29. The properties of metals and nonmetals.

30. How to use reference table F.

31. How to identify the four major types of chemical reactions synthesis, decomposition, single replacement, and double replacement.

32. The difference between and definitions of empirical and molecular formulas.

33. How to find a compounds molecular formula when given the compounds empirical formula and its gram formula mass.

34. How to write formulas for ionic compounds and molecular compounds.

35. How to explain and or identify heat flow from one sample of matter to another.

36. The values for standard temperature and pressure and where to find them on your reference tables.

37. The definition of a substance melting/freezing point and boiling/condensing point and where to find them for the elements on the periodic table.

38. The definition of a diatomic element the seven elements that exist as diatomic elements (H,O,F, Br, I, N, Cl).

39. What the particle diagrams would look like for a pure substance (monoatomic or diatomic elements or compounds) and a mixture of elements, compounds or both.

40. How to read a bright-line emission spectrum and how to compare spectra of known samples to unknown samples.

41. How to perform metric conversions.

42. The relationships between pressure and volume, temperature and number of gas particles.

43. The relationship between volume and temperature when pressure is constant.

44. How to calculate the mass of an unknown product or reactant during a chemical reaction when the masses of all the other products and reactants are known. (law of conservation of mass)

45. How to calculate the percent composition of an element in a compound.

46. How to do temperature conversions.

47. How to balance a chemical equation.

48. The definition of the symbol (aq).

49. How and when to use the combined gas law equation.

50. In a closed system the number of gas particles never changes no matter what the conditions are.

51. The definition of an isotope in terms of subatomic particles, how isotopes are different and what do they have in common.

52. How to draw an electron dot diagram for atoms and ions.

53. How to calculate the weighted atomic mass of an element using the masses and the percent abundance of each isotope.

54. How and when to use the heat calculation equations on Table T.

55. How Rutherford and Thomson’s theories were different and how were they the same.

56. How to use the percent error equation on Table T.

57. How to find the charge of an ion from a formula or a name.

58. How to plot a graph and interpret the data.

59. Why light is emitted from atoms during an atomic emission in terms of electrons and energy states.

60. How to count significant figures.

61. How to calculate experimental percent composition.

62. How to interpret a phase change diagram.

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