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 definite shape. 4. is a state of matter found in outer space. 5. have definite volume and no definite shape. 6. has particles smaller than gas. 7. has the most energy of the 3 states of matter found on earth. It has no definite volume, and no definite shape. Use the word bank below to describe each. Evaporation Condensation Freezing Melting Sublimation 8. When a solid changes to a liquid: 9. When a liquid changes to a solid: 10. When a liquid changes a gas: 11. When a gas changes a liquid: 12. When a solid changes to a gas: 13. When a gas changes to a solid: 1 Page
14. Use an arrow to indicate in which direction the following processes occur. (Ex. A B, or B A) Evaporation = Freezing = Melting = Condensation = 15. Use an arrow to indicate in each state of matter on the graph above. (Ex. A B, or B A) Solid = Liquid= Gas = 2 Page
16. Fill in the Matter Flow Diagram below. Use the Word Bank below to fill in the blanks. (Not all the words are used) mixtures homogeneous heterogeneous atoms mass compound elements matter substances compounds element solutions 17. All matter consists of tiny particles called. 18. Matter is divided into 2 categories: and. 19. Substances can be broken down into 2 categories: and. 20. An is made up of only one type of atom. 21. Two or more different atoms combined chemically are called a. 22. A is made up of 2 or more substances physically combined. 3 Page
23. A mixture that is uniform throughout the sample is said to be. These types of mixtures are known as. 24. A mixture that has uneven distribution of 2 or more substances is called. 25. Fill in the following table. A. Determine if the following examples are Substances or Mixtures. B. If it s a substance, indicate if it s a compound or an element. C. If it s a mixture, indicate if it s homogenous or heterogeneous. Type of Matter Substance or Mixture? (Element or Compound) or (Homogeneous or Heterogeneous?) Ex 1: water Substance Compound Ex 2: sand & water Mixture Heterogenous Iron Sugar water Carbon dioxide Vegetable soup 26. Physical Changes only change the a of a substance, not it s identity! 27. Chemical Changes results in. List the 4 ways to show a chemical reaction takes place: a) b) c) d) 4 Page
28. Fill in the following chart. Physical or Chemical Change? Cutting paper Burning paper Freezing water Dissolving salt in water 5 Page
Unit 2: SI UNITS & MEASUREMENTS 1. Fill in the following metric prefixes. Use the Factor-Label Method to convert each of the following measurements. Show work and use appropriate labels. 2) 2.56 kilograms to grams 3) 17 millimeters to centimeters 4) 125 pounds to kilograms (2.2 pounds = 1 kilogram) 6 Page
DENSITY Write the formula to determine density, volume, and mass below. Density = Mass = Volume = Determine the value of the missing measurement. SHOW YOUR WORK! USE UNITS! 5. mass = 75 g; volume = 10 cm 3 ; density = 6. mass = 400 g; density = 15 g/cm 3 ; Volume = 7. volume = 25 cm 3 ; density = 5 g/cm 3 ; Mass = The density of water is 1.0 g/cm 3 Substance Density (g/cm 3 ) Sink or Float? 8. Mercury 13. 55 9. Soap 0.8 7 Page
Unit 3: Atoms and Isotopes 1. Label the nucleus, neutrons, protons, and electrons. 2. Fill in the following chart: Element Barium Chemical Symbol Atomic Number # Protons # Electrons # Neutrons 81 Mass Number Cr 52 Silver 47 61 3. Calculate the average atomic mass. Isotope Relative Abundance Atomic Mass Nitrogen-14 Nitrogen-15 99.63% 14.003 0.37% 15.000 8 Page
Unit 4 Nuclear Chemistry 1. Band of stability. (read a graph, identify elements that are stable and not stable) Use the graph above to identify the following elements as stable or not stable: 35 50 17 Cl 20 Ca 2. Put in order of most penetrating to least penetrating: beta, gamma, and alpha radiation. 3. Identify alpha and beta particles. Alpha Beta 4. Write nuclear equations that show alpha decay: U 238 92 9 Page
5. Write a nuclear equation that shows beta decay: 207 82 Pb Unit 6 Ions and Ionic Compounds 1. Draw a Bohr Model for the element Sulfur a) How many valence electrons? b) Lose or gain electrons to become stable? c) How many? d) Anion or Cation? d) Charge of ion? 2. The Octet Rule states that atoms want electrons in their valence shell to become stable. 3. What will Nitrogen do to become stable? a. Gain 3 electrons b. Lose 3 electrons c. Gain 3 protons 4. Atoms that gain or lose electrons and become charged particle are called. 10 Page
5. Atoms that lose electrons have a (positive / negative) charge and are called (cations / anions). (Metals / Nonmetals) tend to lose electrons to become stable. [circle the correct answers of the pairs] 6. Atoms that gain electrons have a (positive / negative) charge and are called (cations / anions). (Metals / Nonmetals) tend to gain electrons to become stable. [circle the correct answers of the pairs] 7. What happened for Ca +2 to have a charge of +2? a) lost 2 electrons b) gained 2 electrons c) gained 2 protons 8. Complete the following table: Element Sodium Oxygen Chlorine Calcium Phosphorus Electron Dot Structure Ion Gained or lost electrons? How many? Cation or Anion? Metal or nonmetal? 11 Page
9. Word bank: Place the following formulas or chemical names in the appropriate spaces. NOT ALL COMPOUNDS ARE USED! a. O 3 F 9 i. Lead(II) sulfate b. CuCl 2 j. Diphosphorus pentoxide c. O 2 F 6 k. Dinitrogen tetroxide d. BaCO 3 l. Potassium oxide e. CCl 4 m. Aluminum phosphate f. MgBr 2 n. Aluminum phosphorus g. Mg 2 Br 3 o. Lead (I) sulfate h. BaCO 2 13. Dioxygen hexafluoride 14. Barium carbonate 15. Carbon tetrachloride 16. Copper (II) chloride 17. Magnesium bromide 18. PbSO 4 19. K 2 O 20. N 2 O 4 21. AlPO 4 22. P 2 O 5 12 Page
Unit 7 Chemical Equations and Reactions Write the Law of Conservation of Mass below: Terms to Know Match the correct term with it s definition. 1. a new solid formed from a chemical reaction 2. compounds present before a reaction 3. type of change that alters the appearance of a substance, but not it s composition 4. compounds present after a reaction 5. type of change that results in the formation of new substances 6. indicates the number of molecules a. products b. physical change c. coefficient d. reactants e. chemical change f. precipitate Match the Type of Reaction with it s description. 1. the burning of fuel with oxygen gas to create CO 2, H 2 O, and energy 2. two elements switch places to create 2 new compounds 3. the combining of substances into a more complex substance 4. one element takes the place of another to create a new compound 5. reaction that breaks down a compound into simpler products a. single replacement b. combustion c. double replacement d. synthesis e. decomposition 13 Page
CHEMICAL EQUATIONS A. Fill in the missing chemical symbols, or it s meaning. SYMBOL (s) MEANING reacts with (aq) Gaseous state C. Writing Chemical Equations/ Balancing Equations A. Balance each equation. Where necessary, use an ion sheet to write the chemical equation. B. Classify each reaction: Synthesis (S), Decomposition(D), Combustion(C), Single Replacement (SR), Double Replacement (DR) 1. P + O 2 PO 5 2. Al 2 O 3 Al + O 2 3. Fe + CuNO 3 Fe(NO 3 ) 2 + Cu 14 Page
4. C 6 H 5 OH + O 2 H 2 O + CO 2 6. Na 2 O 2 + HOH NaOH + H 2 O Unit 8 The Mole 1. The scientist that is credited for coming up with the Mole Concept: 2. One mole represents = 3. Formula Mass/ Molecular Mass/ Molar Mass are three different terms that can be used to express the (Write the definition on the line above!) 4. What is the percent composition of each element in KClO 3? 15 Page
Use the appropriate Mole Conversions to solve the problems below. USE UNITS! SHOW YOUR WORK! Round your answer to the nearest hundredth. 1. Convert ATOMS /MOLECULES MOLES. a) How many moles in 3.96 x 10 25 atoms of tin? b) How many atoms are in 1.97 moles of Barium? 2. Convert MASS (g) MOLES. a) 10.5 grams of KNO 3 b) 0.62 mole of H 2 O 16 Page
3. Convert MASS ATOMS a) What is the mass 4.2 x 10 26 molecules of H 2 SO 4? b) How many molecules are in 64 g of KMnO 4? 17 Page
Unit 5 Periodic Table Review 1. a. How did Mendeleev arrange the elements in his periodic table? b. How are elements arranged today in the modern periodic table? 2. Are the periods the horizontal rows or vertical columns? 3. Are the groups the horizontal rows or vertical columns? 4. On the periodic table: a. Number the PERIODS: 1 7 b. Number the GROUPS: 1-18 c. Draw a zig-zag line to separate the metals, nonmetals, and metalloids d. Locate the metals, nonmetals, and metalloids. 18 Page
5. What are the properties of metals? Name 3 metals. 6. What are the properties of nonmetals? Name 3 nonmetals. 7. What are the properties of metalloids? Name 3 metalloids 8. Locate the representative elements, transition elements, and inner transition elements. (Where are the lanthanides and actinides?) 9. Locate the alkali metals, alkaline earth metals, halogens, noble gases. 19 Page
10. What are the properties of the alkali metals? 12. What are the properties of the alkaline earth metals? 13. What are the properties of the halogens? 14. What are the properties of the noble gases? 20 Page