Honors Chemistry: MIDTERM REVIEW The midterm consists of 60 multiple choice questions and two open responses. Covers all content in Terms 1 & 2 including Chapters 1, 2, 3, 4 & 19, 5, 6, & 7. Chapter 1–Chemistry: An Introduction Objectives: ◦ To understand the importance of learning chemistry (Section 1.1) ◦ To define chemistry (Section 1.2) ◦ To understand scientific thinking (Section 1.3) ◦ To describe the method scientists use to study nature (Section 1.4) ◦ To develop successful strategies for learning chemistry (Section 1.5) 1. What is chemistry? Give a definition. 2. What is a theory? Give a definition. 3. Give two examples of scientific theories. 4. What is the difference between qualitative and quantitative observations? Give an example of each. 5. Give an example of a natural law. Chapter 2 – Measurements and Calculations Objectives: ◦ Expressing very large or very small numbers as the product of a number between 1 and 10 and a power of 10 (Section 2.1) ◦ Learning the English, metric, and SI systems of measurement (Section 2.2) ◦ Understanding the metric system for measuring length, volume, and mass (Section 2.3) ◦ Understanding how uncertainty in a measurement arises (Section 2.4) ◦ Indicating a measurement's uncertainty by using significant figures (Section 2.4) ◦ Determining the number of significant figures in a calculated result (Section 2.5) ◦ Using dimensional analysis to solve various types of problems (Section 2.6) ◦ Learning the three temperature scales (Section 2.7) ◦ Converting from one scale to another (Section 2.7) ◦ Continuing to develop problem-­‐solving skills (Section 2.7) ◦ Defining density and its units (Section 2.8) Basic Conversion Problems and Significant Figures 1. How many digits are significant in each of the following measurements? a. 0.000230 b. 1000 Honors Chemistry: Review for Midterm (pg. 2 of 14) c.
d.
e.
f.
1000. 3.01 x 10-­‐5 804.4900 0.020600 REMINDER: Determining Significant Figures in Calculations A. Multiplication and Division: a. The number of significant figures in your answer should be the same as the measurement with the smallest number of significant figures i. Example: 4.56 x 1.4 = 6.384 à 6.4 3 SF 2 SF Round result to 2 SF B. Addition and Subtraction b. The measurement with the fewest number of decimal places will determine how many decimal places are in your result. i. Example: 12.11 + 18.0 + 1.013 = 13.123 à 31.1 2 places 1 place 3 places Round result to 1st place (tenth) 2. Perform the following calculations and report your answer to the correct number of significant figures: a. 5.19 + 1.9 + 0.842 b. 1081 – 7.25 c. 2.3 x 3.14 d. 8.63 / 4.521 e. (1.33 x 2.8) + 8.41 f. (3.5 – 1.23) / 0.54 3. Perform the following conversions: a. 55 mL to L b. 2300 m to cm c. 0.35 km to cm d. 2 m3 to cm3 4. A volume of 1 mL is equivalent to a. 1 cm3 b. 1 cm2 c. 1 dL d. 1 mm3 Honors Chemistry: Review for Midterm (pg. 3 of 14) 5. While driving in London you encounter a speed limit sign that reads 80 km/hr. How fast can you legally travel in miles/hr? a. 80 b. 70 c. 60 d. 50 6. Mercury is the only metal known to exist as a liquid at room temperature and pressure. It has a very high density of 13.6 g/mL. Convert the density of mercury into units of mg/L. 7. The normal body temperature for a dog is approximately 102oF. What is this equivalent to on the Kelvin temperature scale? a. 373 K b. 312 K c. 289 K d. 202 K 8. If I sleep 8 hours per day and I live to be 100 years old, how many years have I slept? 9. Put the following examples into scientific notation: a. 0.00567
b. 48.29
c. 137200000
d. 0.0174
10. Chapter 3 – Matter Objectives: ◦ To learn about matter and its three states (Section 3.1) ◦ To learn to distinguish between physical and chemical properties (Section 3.2) ◦ To learn to distinguish between physical and chemical changes (Section 3.2) ◦ To understand the definitions of elements and compounds (Section 3.3) ◦ To learn to distinguish between mixtures and pure substances (Section 3.4) ◦ To learn two methods of separating mixtures (Section 3.5) Chemical vs. Physical Changes, Isotopes, Determining the number of Protons, Neutrons, and Electrons in an atom Honors Chemistry: Review for Midterm (pg. 4 of 14) 1. Describe the ways to tell if a chemical reaction has occurred. 2. Explain why undergoing a change in state (solid, liquid, gas) is a physical change. 3. In order to break down water into its constituent elements, water would have to undergo a. distillation b. fusion c. chemical change d. physical change 4. A mixture has a __________ composition, whereas a compound always has a _________ composition. a. pure; complex b. complex; pure c. constant; variable d. variable; constant 5. The brass in the ornamental tray you might use to serve guests could be classified as a(n) a. solution b. element c. compound d. pure substance 6. To separate a sand-­‐saltwater mixture into pure substances one would have to employ a. electrolysis b. filtration c. distillation d. filtration followed by distillation 7. Pure substances consist of either a. elements or compounds b. elements or mixtures c. elements or solutions d. elements or energy 8. Decide whether each of the following scenarios involves a chemical or a physical change. - Zinc when immersed in hydrochloric acid produces hydrogen gas. - A nail rusts. - A piece of paper burns. - Water boils at 100 degrees Celsius - Liquid nitrogen freezes a solid rubber ball The state of matter in which a material has a definite shape and definite volume is…
Honors Chemistry: Review for Midterm (pg. 5 of 14) The state of matter in which a material has a definite volume but no definite shape is…
Chapter 4 – Chemical Foundations: Elements, Atoms, and Ions & Chapter 19—Radioactivity and Nuclear Energy Objectives: ◦ To learn about the relative abundances of the elements (Section 4.1) ◦ To learn the names of some elements (Section 4.1) ◦ To learn the symbols of some elements (Section 4.2) ◦ To learn about Dalton's theory of atoms (Section 4.3) ◦ To understand and illustrate the law of constant composition (Section 4.3) ◦ To learn how a formula describes a compound’s composition (Section 4.4) ◦ To learn about the internal parts of an atom (Section 4.5) ◦ To understand Rutherford's experiment to characterize the atom’s structure (Section 4.5) ◦ To understand some important features of subatomic particles (Section 4.6) ◦ To learn about the terms isotope, atomic number, and mass number (Section 4.7) ◦ To understand the use of the symbol to describe a given atom (Section 4.7) ◦ To learn the types of radioactive decay (Section 19.1) ◦ To learn to write nuclear equations that describes radioactive decay (Section 19.1) 1. Which of the following is one of the statements that make up Dalton’s atomic theory? a. All atoms contain electrons. b. All atoms of a given element are identical. c. Atoms are divisible. d. Atoms gain and lose electrons in chemical reactions. 2. The scientist who used alpha particles to bombard a thin film of gold, and proposed that most of the volume of an atom is empty space because most of the alpha particles went straight through the film: a. Rutherford b. Kelvin c. Thomson d. Dalton 3. Thomson discovered the electron when experimenting with a. radioactive elements b. alpha particles c. thermometers d. cathode ray tubes 4. The chemical properties of a particular element are largely determined by the number of __________ an atom of that element possesses. a. protons Honors Chemistry: Review for Midterm (pg. 6 of 14) b. neutrons c. electrons 5. Lead-­‐210 is used in radioactive dating of sediment cores. The number of protons, electrons, and neutrons in an atom of lead-­‐210 respectively is variable a. 82, 82, 128 b. 210, 82, 128 c. 128, 128, 82 6. Positive ions, known as __________ can be formed when a metal atom gives up one or more __________ to a nonmetal, which simultaneously forms a negatively charged ___________. a. cations, electrons, anion b. anions, electrons, cation c. cations, electrons, allotrope d. isotopes, electrons, cation 7. The periodic table is very helpful in assisting in figuring out the charge an atom is likely to have if it accepts or loses electrons to form an ion. When halogens, as typical nonmetals, _____ electrons, they always form ions with a charge of ____. a. give up, 2-­‐ b. accept, 1-­‐ c. give up, 2+ d. accept, 2+ 8. When aluminum foil is dropped into liquid bromine the ionic compound aluminum bromide forms. This compound’s formula is a. AlBr b. AlBr2 c. AlBr3 d. Al3Br 9. 60.11% of Ga has a mass number of 69, the rest have a mass number of 71. Calculate the average atomic mass. 10. Complete the following chart: Element Symbol Fe Sb Atomic Number Mass # Protons # Neutrons # Electrons Number Charge 25 3 84 105 -­‐2 54 135 106 104 265 Honors Chemistry: Review for Midterm (pg. 7 of 14) 11. Define isotope: 12. Identify the number of protons, neutrons, and electrons in the atom 13O -­‐2. 13. Identify the number of each type of atom in the following compound. (How many Ca atoms are there? How many O atoms are there? etc.) Ca2(PO4)3 Ca: P: O: 14. Write a balanced equation for the following radioactive decay processes: a. alpha decay of uranium-­‐238 b. nitrogen-­‐13 undergoes beta decay 15. What type of radioactive particle does NOT have a charge? 16. What is an alpha particle? 17. What is a beta particle? Chapter 5 – Nomenclature Objectives: ◦ To understand why it is necessary to have a system for naming compounds (Section 5.1) ◦ To learn to name binary compounds of a metal and a nonmetal (Section 5.2) ◦ To learn how to name binary compounds containing only nonmetals (Section 5.3) ◦ To review the naming of Type I, Type II, and Type III binary compounds (Section 5.4) ◦ To learn the names of common polyatomic ions and how to use them in naming compounds (Section 5.5) ◦ To learn how the anion’s composition determines the acid’s name and to learn names for common acids (Section 5.6) ◦ To learn how to write the formula of a compound given its name. Naming and Writing Formulas 1)
H2SO3______________________________________________ 2)
HC2H3O2 ______________________________________________ 3)
P2O5 ______________________________________________ Honors Chemistry: Review for Midterm (pg. 8 of 14) 4)
Co2(Cr2O7)3 ______________________________________________ 5)
MnSO4 ______________________________________________ 6)
H2CO3 ______________________________________________ 7)
NiHPO4 ______________________________________________ 8)
FePO4 ______________________________________________ 9)
SF6 ______________________________________________ 10)
C5H10 ______________________________________________ 11)
Ca3N2 ______________________________________________ 12)
HClO2 ______________________________________________ 13)
CuOH ______________________________________________ 14)
15)
Sn(CO3)2 ______________________________________________ H2SO4 ______________________________________________ 16)
IF7 _______________________________________________ 17)
HClO________________________________________________ 18)
H2O ______________________________________________ 19)
Cs2Se ______________________________________________ 20)
HI ______________________________________________ Write the formula: 21)
zinc dichromate __________________ 22)
barium hydroxide __________________ 23)
hydrochloric acid __________________ 24)
silver nitrate __________________ 25)
perchloric acid __________________ Honors Chemistry: Review for Midterm (pg. 9 of 14) 26)
tricarbon octahydride __________________ 27)
phosphoric acid __________________ 28)
strontium oxide __________________ 29)
chlorous acid__________________ 30)
calcium hydrogen phosphate __________________ 31)
aluminum acetate __________________ 32)
manganese (II) hydrogen sulfate __________________ 33)
strontium cyanide __________________ 34)
ammonium selenide __________________ 35)
carbonic acid __________________ 36)
chloric acid __________________ 37)
sulfurous acid __________________ 38)
phosphorus pentachloride __________________ 39)
Tin (II) carbonate __________________ 40)
Tin (IV) sulfite __________________ Chapter 6 – Chemical Reactions: An Introduction Objectives: ◦ To learn the signals that show a chemical reaction has occurred (Section 6.1) ◦ To learn to identify the characteristics of a chemical reaction and the information given by a chemical equation (Section 6.2) ◦ To learn how to write a balanced equation for a chemical reaction (Section 6.3) 1. Which of the following indicates that a chemical reaction has occurred? a. Liquid water boils to produce steam. b. Burning firewood give off heat. c. Mixing two colorless liquids produce a bright yellow solid. d. Solid NaHCO3 dissolves in water. Honors Chemistry: Review for Midterm (pg. 10 of 14) 2. Why is it important that chemical equations be balanced? 3. Count the number of each kind of atom on both sides of the equation, and decide which reactions are balanced and which are not. a. H2 + Br2 à HBr b. KClO3 à KCl + O2 c. 2NaOH + CO2 à Na2CO3 + H2O d. C2H5OH + 3O2 à 2CO2 + 3H2O e. 3Cu + HNO3 à 3Cu(NO3)2 + NO + H2O 4. Use the following word descriptions to write unbalanced chemical equations showing the formulas of reactants and products. Make sure you include the physical states of reactants and products. a. Solid iron metal reacts with oxygen in the atmosphere to form rust, iron (III) oxide. b. Solid magnesium metal reacts with aqueous hydrochloric acid to produce hydrogen gas and an aqueous solution of magnesium chloride. c. Solid silver oxide decomposes upon heating to produce solid silver metal and oxygen gas. d. Aqueous sodium hydroxide reacts with aqueous nitric acid to produce aqueous sodium nitrate and liquid water. 5. Balance these chemical equations. Check your work by counting the number of each kind of atom on both sides of the equation. a.
KOH(aq) + H2S(aq) à K2S(aq) + H2O(l) b.
HNO2(aq) à N2O3(g) + H2O(l) c.
NaOH(aq) + H2SO4(aq) à Na2SO4(aq) + H2O(l) d.
(NH4)2S(aq) + Pb(NO3)2(aq) à PbS(s) + NH4NO3(aq) Honors Chemistry: Review for Midterm (pg. 11 of 14) e.
Al(s) + O2(g) à Al2O3(s) Chapter 7 – Reactions in Aqueous Solutions Objectives: ◦ To understand some of the factors that cause reactions to occur (Section 7.1) ◦ To identify the solid that forms in a precipitation reaction (Section 7.2) ◦ To describe reactions in solutions by writing molecular, complete ionic and net ionic equations (Section 7.3) ◦ To identify the characteristics of the reactions between strong acids and strong bases (Section 7.4) ◦ To describe the general characteristics of a reaction between a metal and a nonmetal (Section 7.5) ◦ To describe electron transfer as a driving force for a chemical reaction (Section 7.5) ◦ To identify various classification schemes for reactions (Section 7.6) ◦ To learn additional classes of chemical reactions (Section 7.7) 1. Which of the following is a common driving force for a reaction (something that makes the reaction occur)? a. Formation of a solid b. Formation of a gas c. Formation of water d. All of the above 2. A reaction in which a solid is formed is referred to as a(n) _______ reaction. a. electrolyte b. precipitation c. solidification d. decomposition 3. When drilling irrigation wells in coastal areas, the salinity of the well water is always of concern because of the negative impact of salt water on vegetation. One common way of testing water for salinity is to add a solution of AgNO3 to a sample of the well water. If the concentration of salt is too high, a precipitate will form. Write the equation for the reaction of silver nitrate with sodium chloride and determine the identity of the precipitate using the solubility rules. Reaction Types: Predicting the Products of a Reaction and applying Solubility Rules For each of the following reactions, translate and balance the equation. Then write the reaction type next to the balanced equation. (NOTE: Some synthesis reactions may also be considered an oxidation-­‐reduction reaction) 1. Solid iron (III) and hydrochloric acid gas react Honors Chemistry: Review for Midterm (pg. 12 of 14) Reaction type: 2. calcium hydroxide (aq) and nitric acid (aq)à Reaction type: Write the net ionic equation for the reaction: 3. calcium hydroxide (aq) + potassium carbonate (aq) à Reaction type: Write the net ionic equation for the reaction: 4. Iron (III) metal + oxygen à Reaction type: 5. dicarbon hexahydride + oxygen à Reaction type: 6. aluminum hydroxide (aq) + hydrochloric acid (aq) à Reaction type: Honors Chemistry: Review for Midterm (pg. 13 of 14) 7. What is an acid base reaction? What are the products of an acid base reaction? 8. What is a precipitate? 9. What happens to the ions in a double replacement reaction that do not form a precipitate? 10. What happens to electrons in a red-­‐ox reaction? 11. Circle the compounds that ARE SOLUBLE in water: a. ammonium carbonate b. iron (III) sulfide c. iron (III) sulfate d. silver nitrate e. silver chloride f. barium chlorate 12. Circle the compounds that are NOT soluble in water: a. sodium phosphate b. lead (II) nitrate c. calcium carbonate d. barium sulfate e. aluminum sulfate f. barium phosphate g. lead (II) acetate 13. Mixing which of the pairs of solutions listed below will result in the formation of a precipitate? a. NaCl + K2CO3 b. NaOH + Mg(NO3)2 c. KCl + Ba(NO3)2 d. Na2S + KNO3 14. When a piece of aluminum foil is added to a container of liquid bromine a white salt forms. Write out the balanced equation for the reaction and indicate which element is reduced and which is oxidized in the reaction. 15. The oxidation-­‐reduction reaction that furnishes the energy to launch the space shuttle via the solid-­‐fuel rockets is represented below: Honors Chemistry: Review for Midterm (pg. 14 of 14) 3NH4ClO4(s) + 3Al(s) Al2O3(s) +AlCl3(s) + 3NO(g) + 6H2O(g) + energy The element that is oxidized in the reaction is a. N b. Cl c. O d. Al 16. The reaction between hydrogen and oxygen to form water 2H2 + O2 à 2H2O can be classified as a(n) ___________ reaction. a. oxidation–reduction b. synthesis c. combustion d. all of the above OTHER Random Bits of Information you should know!!! - Know the basic terminology of laboratory equipment (funnel, flask, etc). - Know the charge on ions in their ionic compounds. o Example: Identify the charge on the following ions in their ionic compounds: 1. K 4. Se 2. Sr 5. Cl
3. P How To Study For the Midterm: - Organize and review your Chemistry Binder. This is your learning guide for honors chemistry. - Do all of the practice questions in the study guide and check your answers - Review topics that you have trouble with by looking back at your notes for that section, retrying homework problems that were assigned, reviewing Note Sheets and Problem Sheets. - If you want some extra help, you need to come to me with VERY SPECIFIC QUESTIONS!! I am here to help you, but I will not respond to “I don’t get anything!!”. - I EXPECT YOU TO STUDY (for more than 45 minutes!!) FOR THIS EXAM. THE MIDTERM IS 7.5% OF YOUR GRADE. YOU CAN NOT EXPECT TO BE SUCCESSFUL WITHOUT STUDYING!!!!!! GOOD LUCK!!!!!