Chemistry STAAR Review Ladder to Success Rung 1 Reporting Category 1: Matter & Periodic Table

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1 Differentiate between physical and chemical changes and properties Chemistry STAAR Review Rung 1 Reporting Category 1: Matter & Periodic Table Physical and Chemical Properties Property Description Example Physical and Chemical Changes Change Description Example How can you recognize a chemical change? Identify extensive and intensive properties Types of Properties Physical and chemical properties of matter can be classified as either intensive or extensive. Extensive Properties Intensive Properties

2 Compare solids, liquids, and gases in terms of compressibility, structure, shape and volume States of Matter and Properties Property Solid Liquid Gas Compressible Shape Volume Structure Classify matter as pure substances or mixtures through investigation of their properties Matter Matter: anything that takes up space and has mass Pure Substance: Mixture: Element: Compound: Homogeneous: Heterogeneous: Solution:

3 Chemistry STAAR Review Rung 1: Homework Identify the following as physical or chemical properties. 1. The color of the house is red. 2. Oxygen is a gas. 3. A flagpole is 25 feet tall. 4. A ruby is red. Identify the following as physical or chemical changes: 5. Salt dissolving in water 6. Magnesium reacting with hydrochloric acid 7. Milk turning sour 8. Dry ice changing to a gas Identify the following as element, compound or mixture. 9. An unknown, clear liquid is given to you in a beaker. You transfer the liquid from the beaker to a clean, empty test-tube and begin to heat it. After a while, you see vapors (which on further analysis, you discover are vapors of water) rising from the test-tube, and pretty soon, all that's left are a few crystals of salt stuck to the edges! How would you classify this liquid? 10. You have won the world's biggest lottery, for which you are given a huge block of pure, metallic gold. How would you classify your prize? 11. A dish is given to you, which contains a blackish-yellow powder. When you move a magnet over it, you are amazed to see black particles (which you find out are iron) fly upwards and get stuck to the magnet. All that's left in the dish is a yellow powder, which you discover to be sulfur. How would you classify the initial blackish-yellow powder? 12. A substance is analyzed in a laboratory, and when viewed under an electron microscope, it is revealed that it contains only one kind of atom. How would you classify the substance? 13. A magnesium ribbon is burnt in the air to form the grayish oxide of magnesium - magnesium oxide (MgO). How would you classify this oxide? Answer the following: 14. What is the density at 20 C of 12.0 milliliters of a liquid that has a mass of 4.05 grams? 15. A sample of an element has a volume of 78.0 ml and a density of 1.85 g/ml. What is the mass in grams of the sample?

4 Understand the experimental design and conclusions used in the development of modern atomic theory. Including Dalton s postulates, Thomson s discovery of the electron properties, Rutherford s nuclear atom, and Bohr s nuclear atom. Chemistry STAAR Review Rung 2 Reporting Category 2: Atomic Structure and Nuclear Chemistry Scientist Contribution to Modern Atomic Theory Dalton Thomson Rutherford Bohr Understand the electromagnetic spectrum and the mathematical relationships between energy, frequency, and wavelength of light. Modern Atomic Theory A wave can be described by its frequency, wavelength and energy. Frequency: Wavelength: Energy:

What are the mathematical relationships between wavelength and frequency? What are the mathematical relationships between energy and frequency?

5 What are the mathematical relationships between wavelength and frequency? What are the mathematical relationships between energy and frequency? Calculate the wavelength, frequency, and energy using Planck s constant and the speed of light. Example #1: If a particular green light has a wavelength of 4.9 x 10-7 m, what is its frequency? Example #2: The human eye can see light with a frequency about as high as 7.9 x Hz, which appears violet. Calculate the energy that one photon of violet light carries. Example #3: Find the energy of violet light if the wavelength is 4 x 10-7 m. Use isotopic composition to calculate average atomic mass of an element. What is an isotope? Calculating Average Atomic Mass:

Express the arrangement of electrons in atoms through electron configurations and Lewis

6 Example: Calculate the avg. atomic mass of oxygen if its abundance in nature is 99.76% 16 O, 0.04% 17 O, and 0.20% 18 O. Express the arrangement of electrons in atoms through electron configurations and Lewis valence electron dot structures. Electron Configuration Longhand configuration: Shorthand configuration: Lewis Dot Diagrams represent the valence e -

7 Chemistry STAAR Review Rung 2: Homework 1. If the wavelength of a certain light is 6.5X10-7 m what is the frequency? 2. The frequency of a wave is found to be 9.0X10 14 Hz. What is the wavelength? 3. The energy of one photon of light is 4.9X10-19 J. What is the frequency of this light? 4. The frequency of a wave is 4.0X10 14 Hz. Calculate the energy. 5. Electrons travel as waves within the atom. Calculate the wavelength of a wave if the energy is 6.9X10-19 J. 6. Determine the energy associated with a wave if the wavelength is 9.1X10-7 m. 7. Write the electron configuration for the following atoms: a. Bromine b. Zirconium c. Strontium d. Oxygen e. Silver 8. Draw the Lewis valence electron dot structures for the following atoms: a. Bromine b. Strontium c. Hydrogen d. Xenon e. Calcium

8 Name ionic compounds, covalent compounds, and acids using IUPAC nomenclature rules. Chemistry STAAR Review Rung 3 Reporting Category 3: Bonding and Chemical Reactions How are ionic compounds named using IUPAC rules? How are covalent compounds named using IUPAC rules? How are acids named using the IUPAC rules? Write the chemical formulas of common polyatomic ions, ionic compounds, covalent compounds and acids How do you write the chemical formulas of ionic compounds? How do you write the chemical formulas of covalent compounds? How do you write the chemical formulas of acids?

9 Construct electron dot formulas to illustrate ionic and covalent bonds How to construct electron dot formulas to illustrate ionic bonds: How to construct electron dot formulas to illustrate covalent bonds: Describe the nature of metallic bonding and apply the theory to explain metallic properties such as thermal and electrical conductivity, malleability, and ductility. How can you describe the nature of metallic bonding? How can you apply metallic bonding theory to explain metallic properties? Predict molecular structure for molecules with linear, trigonal planar or tetrahedral electron pair geometries using VSEPR theory. Molecular Structures Linear Trigonal planar Tetrahedral

10 Chemistry STAAR Review Rung 3: Homework Name the following: 1. BaSO 3 2. (NH 4 ) 3 PO 4 3. PBr 5 4. MgSO 4 5. CaO 6. H 3 PO 4 7. Na 2 Cr 2 O 7 8. MgO 9. SO Cu(NO 3 ) 2 Write the formula of the following: 11. hydrobromic acid 12. chromium(iii) carbonate 13. magnesium sulfide 14. iodine trichloride 15. lithium hydride 16. ammonium hydroxide 17. calcium chloride 18. hydroselenic acid 19. iron(ii) nitride 20. aluminum hydroxide Draw Lewis diagrams for the following and indicate the shape. 21. CBr N AlCl SF PCl 3

11 Describe and calculate the relations between volume, pressure, number of moles, and temperature for an ideal gas as described by Boyles law, Charles law, Avogadro s law, Dalton s law of partial pressure, and the Ideal gas law. Chemistry STAAR Review Rung 4 Reporting Category 4: Gases and Thermochemistry The following are variables in gas law calculations: P= V= n= R= T= Gas Law Equation Description Dalton s Law of Partial Pressures Boyles Charles Avogadro s Law Ideal Gas Law

12 Examples: The pressure on a balloon with a volume of 300 ml increases from 1.10 to 2.00 atm. Calculate the new volume of the balloon. The air in a balloon with a volume of 25 L is heated from 20 C to 60 C. If the pressure stays the same, what will be the new volume of the balloon? A sample of gas in a 1L flask at 1.5 atm contains 75% CO 2 and 25% H 2 O gas. Calculate the partial pressures of each gas. Calculate the temperaure of 5.85 mol N 2 gas in a 12 L steel bottle under 10 atm of pressure.

13 Perform stoichiometric calculations, including determination of mass and volume relationships between reactants and products for reactions involving gases. GAS STOICHIOMETRY Moles Liters of a Gas: STP - use 22.4 L/mol Non-STP - use ideal gas law Non-STP Given liters of gas? start with ideal gas law Looking for liters of gas? start with stoichiometry conv. EXAMPLES: What is the mass of oxygen gas produced when 29.2 g of water is decomposed by electrolysis according to the balanced equation? 2H 2 O 2H 2 + O 2 What volume in L of nitrogen dioxide gas is produced when 34 L of oxygen gas react with an excess of nitrogen monoxide? Assume conditions of STP. 2NO + O 2 2NO 2 Describe the postulates of kinetic molecular theory Gases are made of molecules in constant, random motion The volume is small Collisions are elastic Forces (attractive and repulsive) are small Average kinetic energy is proportional to temperature

14 Chemistry STAAR Review Rung 4: Homework 1. The total pressure of a homogenous gaseous mixture is 780mmHg. If the gas mixture contains helium at a pressure of 190mmHg, oxygen at a pressure of 200mmHg, and neon what is the partial pressure of the neon gas? 2. What is the volume, in L, of 4.0 moles of carbon dioxide gas at 10.0ºC and 867mmHg? 3. A given sample of gas has a volume of 4.20 L at 60.0 C and 1.00 atm. Calculate its pressure if the volume is changed to 5.00 L and the temperature to 27 C. 4. A gas sample contained in a cylinder equipped with a moveable piston occupied 300. ml at a pressure of 2.00 atm. What would be the final pressure if the volume were increased to 500. ml at constant temperature? 5. A fixed quantity of gas at 23.0 C exhibits a pressure of 748 torr and occupies a volume of 10.3 L. Calculate the volume the gas will occupy if the temperature is increased to 145 C while the pressure is held constant. 6. How many grams of AlCl 3 must decompose in order to produce 3.10 dm 3 of Cl 2 at 50.0 C and 98.4 kpa? (HINT: You must correct to STP.) 2AlCl 3 2Al + 3Cl 2 7. What volume of nitrogen can be produced by the decomposition of 50.0 g of NH 4 NO 2 at 25 C and 1.20 atm? (HINT: You must correct to STP.) NH 4 NO 2 N 2 + 2H 2 O

15 Describe the unique role of water in chemical and biological systems. Chemistry STAAR Review Rung 5 Reporting Category 5: Solutions Factors that contribute to water s unique properties: 1. Polarity: 2. Hydrogen bonding: Develop and use general rules regarding solubility through investigations with aqueous solutions Using the solubility curve: What is the solubility of KCl at 25 C? On the line = Below the line = Above the line= Using the solubility rules: ** Refer to your reference materials!! Example: Is Na 2 CrO 4 soluble in water? IS BaSO 4 soluble in water? Which product in the equation below is a precipitate? AlCl 3 + K 3 PO 4 3KCl + AlPO 4

16 Calculate the concentration of solutions in units of molarity How to calculate the molarity of a solution: Molarity= Example #1: What is the molarity of the solution if.25 moles of Na 2 SO 4 is dissolved in 1.5 L solution? Example #2: If you had a 2M solution of glucose (C6H12O6) how many liters of the solution would contain 3 moles glucose? Example #3: Calculate the molarity of.51l of solution that contains 110g of NaCl. Use molarity to calculate the dilutions of solutions Moles of solute before dilution = Moles of solute after dilution Example #1: What volume of.5m NaOH is needed to make a.075 M in 2L solution?

17 Distinguish between types of solutions such as electrolytes and nonelectrolytes and unsaturated, saturated, and supersaturated solutions. Solution Description Meaning Electrolyte Nonelectrolyte Unsaturated Saturated Supersaturated Investigate factors that influence solubilities and rates of dissolution such as temperature, agitation, and surface area. Factor Effect on solubility Effect on Rate of Dissolution Temperature Agitation Surface Area How does pressure influence solubilities and rates of dissolution?

18 Chemistry STAAR Review Rung 5: Homework 1. Calculate the amount in moles of hydrochloric acid needed to make 2000.mL of a 1.5M solution. 2. Find the volume of a solution if 5.00 moles of solute are present and the molarity is 2.25M. 3. If 88.0 grams of NaOH are dissolved in water and the volume of the solution is 3000.mL what is the molarity of the solution? 4. To prepare a dilute solution a student used 500.mL of a 12.0M HCl solution. The final volume of the dilute solution was 1750.mL. Calculate the molarity of the dilute solution L of a 3.0M solution was diluted to a concentration of 1.8M. What is the volume of the dilute solution? 6. Determine if the following ionic compounds are soluble or insoluble in water: a. Ba(CN) 2 b. BaSO 4 c. Al(OH) 3 d. Sr(OH) 2 e. CaCO 3 f. Na 2 CO 3

19 Chemistry STAAR Review Rung 6 Explain the use of chemical and physical properties in the historical development of the Periodic Table Reporting Category 1: Matter & Periodic Table How were chemical and physical properties used in the development of the periodic table? Word Definition What s so special? Group Period Atomic # Atomic mass Valence electrons Oxidation # Metal Nonmetal Metalloid

20 Use the periodic table to identify and explain periodic trends, including atomic and ionic radii, electronegativity, and ionization energy Property Description Trend Atomic radius Ionic radius Electronegativity Ionization energy Use the periodic table to identify and explain the properties of chemical families, including alkali metals, alkaline earth metals, halogens, noble gases and transition metals Family Description Oxidation # Alkali metals Alkaline earth metals Halogen Noble gases Transition metals

Chemistry STAAR Review Rung 6: Homework 1. Label the following groups: alkali metals, alkaline earth metals, halogens, and noble gases. Also label the transition metals. List a few properties of each.

21 Chemistry STAAR Review Rung 6: Homework 1. Label the following groups: alkali metals, alkaline earth metals, halogens, and noble gases. Also label the transition metals. List a few properties of each. 2. Use the periodic table to identify/label and explain periodic trends, including atomic and ionic radii, electronegativity, and ionization energy a. Which has the larger atomic radii? Mg or Cl b. Which has the greater electronegativity? P or O c. Which has the lower ionization energy? K or Br

22 Chemistry STAAR Review Rung 7 Describe the characteristics of alpha, beta and gamma radiation Reporting Category 2: Atomic Structure and Nuclear Chemistry Particle Alpha Beta Gamma Symbols Charge Mass Speed Penetration Describe radioactive decay process in terms of balanced nuclear equations Alpha Example: Beta Example: Gamma: Gamma rays do not usually appear in nuclear equations since rays are emitted. Compare fission and fusion Fission Fusion

23 Chemistry STAAR Review Rung 7: Homework 1. Which particle is more massive: alpha, beta, or a neutron? 2. What can be used to shield (or protect) someone from alpha radiation? 3. What can be used to shield (or protect) someone from beta radiation? 4. What can be used to shield (or protect) someone from gamma radiation? 5. Complete the following nuclear radioactive decay equations: Po Pb U Np Md Md

24 Chemistry STAAR Review Rung 8 Reporting Category 3: Bonding and Chemical Reactions Define and use the How do chemist define a mole? concept of a mole Representative particles= Use the mole concept to calculate the number of atoms, ions or molecules in a sample of material Example #1: A sample consists of 6.85 x atoms of carbon. How many moles does the sample contain? Example #2: Another sample consists of 2.58 mol of water. What is the number of water molecules in the sample? Example #3: How many atoms are in 2 moles of He? Example #4: Find the number of chlorine ions in 5 grams of CaCl 2. Example #5: How many molecules are in 7.1 grams of water? Calculate percent composition and empirical and molecular formulas PERCENT COMPOSITION: Example #1: Calculate the percent composition of each element in MgCl 2

25 EMPIRICAL FORMULAS: Example #1: Find the empirical formula for a compound that is 79.8% C and 20.2% H. MOLECULAR FORMULAS: Example #1: The empirical formula for a molecule is NH 2. If its molecular weight is 32 amu, what is the compound s molecular formula? Use the law of conservation of mass to write and balance chemical equations LAW OF CONSERVATION OF MASS : Total mass of reactants = Total mass of products Balancing Equations: H 2 + N 2 NH 3 Perform stoichiometric calculations, including determination of mass relationships between reactants and products, calculation of limiting reagents and percent yield Example #1: Suppose 8.75 g of propane react with oxygen gas to produce carbon dioxide and water. How many grams of water are produced? C 3 H 4 + 5O 2 3CO 2 + 4H 2 O Example #2: What is the limiting reagent when 36 g of CH 4 when it reacts with 98 g O 2 to produce carbon dioxide and water? CH O 2 CO 2 + 2H 2 O Example #3: You calculate a theoretical yield of 55 g of water but the actual yield from your experimentation was 48.8 g of water. What is the percent yield?

26 Chemistry STAAR Review Rung 8: Homework 1. During a reaction 15.0g of magnesium reacted with excess oxygen. After the reaction students collected 20.2g of magnesium oxide powder. Determine the percent yield for this reaction. 2Mg(s) + O 2 (g) 2MgO(s) 2. When 60.0L of F 2 react how many L of Cl 2 are produced? 3F 2 (g) + 2AlCl 3 (s) 3Cl 2 (g) + 2AlF 3 (s) 3. How many particles are in 10.0 moles of CaCO 3? 4. How many ions are in 10.0 moles of K 2 SO 4? 5. How many moles of particles are in 3.01X10 24 CaCO 3 particles? 6. How many moles of atoms are in 3.01X10 24 K 2 SO 4 particles? 7. How many moles of ions are in 3.01X10 24 NaCl particles? 8. Balance the following chemical equations: a. CH 4 + O 2 H 2 O + CO 2 b. LiOH Li 2 O + H 2 O c. Mg + Al 2 (CO 3 ) 2 Al + MgCO 3

27 Chemistry STAAR Review Rung 9 Understand energy and its forms including kinetic, potential, chemical and thermal energies Reporting Category 4: Gases and Thermochemistry What is energy? Form Description Kinetic Potential Chemical Thermal Understand the law of conservation of energy and the processes of heat transfer Law of Conservation of Energy: Heat Transfer: Conduction: Convection: Radiation: Use thermochemical equations to calculate energy changes that occur in chemical reactions and classify reactions as exothermic or endothermic Enthalpy: Reaction Enthalpy Change Description Exothermic Endothermic

Perform calculations involving heat, mass, temperature change, and specific heat Example #1: Calculate the heat absorbed by a 20 g piece of copper metal that is heated from 25 C to 125 C.

28 Example #1: Calculate the change in energy for the following reaction at standard conditions. Is the is reaction exothermic or endothermic? Example #2: Calculate the change in energy for the following reaction. Is this reaction endothermic or exothermic? Perform calculations involving heat, mass, temperature change, and specific heat Example #1: Calculate the heat absorbed by a 20 g piece of copper metal that is heated from 25 C to 125 C. The specific heat of copper is.385. Example #2: The specific heat of water is A 1200 g water sampel at 19 C loses 10,000 J of heat. What is the final temperature? Use calorimetry to calculate the heat of a chemical process Calorimeter: tool used to measure heat of a chemical process Energy released by the reaction = Energy absorbed by the solution

29 Chemistry STAAR Review Rung 9: Homework 1. The reaction of zinc with nitric acid was carried out in a calorimeter. This reaction caused the temperature of 72.0 grams of liquid water, within the calorimeter, to raise from 25.0 C to 100. C. If the specific heat of water is 4.18 J/(g K) calculate the energy associated with this reaction. 2. A 4.00 gram sample of solid gold was heated from 274K to 314K. If the specific heat of gold is J/(g K) how much energy was involved in this change? 3. Calculate the change in enthalpy for the following reaction given that the standard enthalpy of formation for water is kJ/mol, 0.0 kj/mol for oxygen, and kJ/mol for hydrogen peroxide. 2H 2 O(l) + O 2 (g) 2H 2 O(l) 4. Calculate the H value for the following reaction: CaSO 4 (s) CaO(s) + SO 3 (g) H =? kj/mol Substance H f (kj/mol) SO 3 (g) CaSO 4 (s) CaO(s) Draw a graph to indicate exothermic and endothermic reactions.

30 Chemistry STAAR Review Rung 10 Define acids and bases and distinguish between Arhennius and Bronsted-Lowry definitions and predict the products in acidbase reactions that form water. Reporting Category 5: Solutions Theory Definition Arrhenius Acid Arrhenius Base Bronsted-Lowry Acid Bronsted- Lowry Base Identifying Conjugate Acid: Identifying Conjugate Base: Understand and differentiate among acid-base reactions, precipitation reactions, and oxidationreduction reactions. Reaction Acid-Base Precipitation Description and Example Oxidation-Reduction (Redox)

31 Define ph and use the hydrogen and hydroxide ion concentrations to calculate the ph of a solution What is ph? Example 1: What is the ph of a solution with a H + concentration of 1 x 10-5 M. Example 2: What is the hydrogen concentration of a solution with a ph of 11. Example 3: What is the ph of a solution with a hydroxide concentration of 1.3 x Example 4: What is the ph if [OH] = 8 x 10-5 M Distinguish between degrees of dissociation for strong and weak acids and bases Strong Acid/Base: Weak Acid/Base:

Chemistry Assessment. Eligible Texas Essential Knowledge and Skills

Chemistry Assessment. Eligible Texas Essential Knowledge and Skills Chemistry Assessment Eligible Texas Essential Knowledge and Skills STAAR Chemistry Assessment Reporting Category 1: Matter and the Periodic Table The student will demonstrate an understanding of the properties