Cumulative Chemistry Review Packet
Chapter 1: 1. Define the following key terms. a. physical science ‐ the study of matter and energy and the changes they undergo b. hypothesis ‐ a possible answer to a scientific question c. manipulated (independent) variable ‐ the variable that we change in an experiment d. responding (dependent) variable ‐ the variable that is expected to change because of the manipulated variable. 2. In the graph at the right, how far did the car travel in 30 minutes? 30 km 3. In the graph at the right, how long did it take the car to travel 25 km? 25 min 4. List 3 lab safety rules. Ask the teacher if you have questions. Dispose of lab waste according to the teacher’s instructions. Yell safety alert if there is an emergency. 5. List the steps of the technology design process. Identify a need, research, design a solution, build a prototype, troubleshoot and redesign, communicate the solution Chapter 2: 1. Define the following key terms: a. matter ‐ anything that has mass and takes up space b. substance ‐ an element or compound that cannot be broken down further and still keep its original properties. c. mixture ‐ a material made up of two or more substances that are together in the same place, but not chemically combined. d. element ‐ a substance that cannot be broken down chemically into other substances e. compound ‐ a substance made up of two or more element that are chemically combined 2. Calculate the density of a 12g block of wood that has a volume of 3cm 3 . D = m/v 12/3 = 4 g/cm 3 3. You are given a flask that contains 250 mL of a clear liquid with a brownish tint. You examine a sample of the liquid under a microscope and notice that there are no visible particles. This sample could NOT be which of the following: homogeneous mixture, heterogeneous mixture, element, or compound. Heterogeneous mixture Explain why. It could not be this because you can see the different parts of a heterogeneous mixture. Chapter 3: 1. For each state of matter determine if it has a definite or indefinite shape and volume. Shape Volume definite definite Solid Liquid indefinite definite Gas indefinite indefinite 2. Double click the GOOGLE DRAWING to label all the phase changes in the diagram: 3. Indicate which of the states of matter AND phase changes are present in each section of the following heating curve . Section A: solid (least energy and motion) Section B: solid and liquid (melting) Section C: liquid Section D: liquid and gas (vaporization) Section E: gas (most energy and motion) 4. What is Boyle's Law? Give an example. As the volume of a gas decreases, the pressure increases. As the volume of a gas increases, the pressure decreases. Example: bursting water bottle 5. What is Charles's Law? Give an example. As the temperature of a gas increases, the volume increases. As the temperature of a gas decreases, the volume decreases. Example: Water bottle in cool and hot water. 6. What is the Pressure‐Temperature Law? Give an example. As the temperature of a gas increases, the pressure increases. As the temperature of a gas decreases, the pressure decreases. Example: Fizz keeper Chapter 4: 1. What does the electron cloud model of the atom tell us about the location and movement of electrons? The electrons are located around the nucleus moving freely in the electron cloud. 2. What are the three main parts of the atom, and what are their charges? proton‐‐positive charge electron‐‐negative charge neutron‐‐neutral charge 3. Read Straight From Periodic Table Name Titanium Symbol Ti Atomic Number 22 Average Atomic Mass 47.867 Determine From Periodic Table Mass Number 48 # of Protons 22 # of Neutrons 26 # of electrons (in neutral atoms) 22 4. What are 3 physical properties of metals? malleable, ductile, good conductors 5. What are 3 physical properties of nonmetals? solids are dull and brittle, most are gases at room temperature 6. What are metalloids? The have properties of both metals and nonmetals. They are used as semiconductors. 7. Which group contains the most reactive metals? Group 1 Alkali Metals 8. Which group contains the most reactive nonmetals? Group 17 Halogens 9. Which group is generally nonreactive? Group 18 Noble Gases 10. In the isotope Carbon‐14, what does the 14 represent? the mass number 11. A certain element has a mass # of 37 and 20 neutrons. Which element is it? 37‐20 = 17, Chlorine Chapter 5 1. What are valence electrons? The electrons with the most energy that are held most loosely and involved in chemical bonds. 2. List three properties of ionic compounds. made of a metal and a nonmetal have high melting points transfer electrons when forming bonds 3. What is the big difference between naming ionic compounds and covalent compounds? The covalent compounds have prefixes before each name. The ionic compounds do not have prefixes. 4. Element Symbol Ca N A) Dot Diagram B) How many electrons transferred? C) Ion symbol D) Chemical formula for compound E) Name of compound give 2 take 3 Ca +2 N ‐3 Ca 3 N 2 Calcium Nitride 5. List three properties of covalent molecules. made of all nonmetals have low melting points share electrons when forming bonds 6. What is the difference between a single, double, and triple bond? Single bonds share 1 pair of electrons Double bonds share 2 pairs of electrons Triple bonds share 3 pairs of electrons 7. Write the formula for carbon dioxide. Explain how you determined this formula. Is this ionic or covalent? CO 2 The prefixes in the name tell how many of each atom we have. If there is not prefix before the first element, it means there is one atom of that element. It is covalent. 8. Aluminum
a. # protons: 13
b. dot diagram (double click GOOGLE DRAWING) c. # neutrons: 14
d.
# electrons: 13 9. How can you determine if a compound is ionic or covalent? If it is made of a metal or a nonmetal, then it is ionic. If it is made of all nonmetals, the it is covalent 10. For each of the following compounds highlight ionic or covalent AND write their chemical names. a) S 4 N 2 ionic / covalent Name: tetrasulfur dinitride b) MgCl 2 ionic / covalent Name: Magnesium Chloride 9. For each of the following compounds highlight ionic or covalent AND write their chemical formulas. a) sodium nitride ionic / covalent Formula: Na 3 N b) triphosphorus pentachloride ionic / covalent Formula: P3 Cl 5 Chapter 6: 1. What is the difference between a physical property and a chemical property? We can observe physical properties with our five senses just by looking at the substance. We can only observe chemical properties during a chemical reaction. 2. What is the difference between a physical change and a chemical change? Physical changes do not change the properties of a substance. Chemical changes create new substances with new properties. 3. Indicate whether each of the following is a physical property, chemical property, physical change, or chemical change. a. red truck physical property b. flammable liquid chemical property c. burning wood chemical change d. chopping wood physical change 4. What are four kinds of evidence you can use to determine if a chemical reaction has occurred? Fizzing and bubbling, sound produced, light produced, heat produced, order produced 5. How are endothermic and exothermic reactions the same? How are they different? Endothermic and exothermic reactions both involve heat. Endothermic reactions take in heat to make the reaction happen. Exothermic reactions produce heat during a chemical reaction. 6. Check to see if the following equations are balanced and classify the reaction as synthesis, decomposition, single replacement or double replacement: a. 2 Fe 2 O 3 + 3 C Fe + 3 CO 2 Type of reaction: Single replacement Balanced? no b. 3 AgNO 3 + FeCl 3 → AgCl + Fe(NO 3 ) 3
Type of reaction: Double replacement Balanced? no 7. Determine if the following equations are synthesis, decomposition, single replacement or double replacement reactions. double replacement a.
b.
c.
d.
decomposition single replacement synthesis Chapter 7: 1. What is a solution? A well‐mixed mixture that contains a solvent and at least one solute. 2. How are solutions different from colloids and suspensions? Solutions have dissolved particles, where colloids and suspensions have undissolved particles 3. What is concentration and how can you change it? Concentration indicates the amount of solute in a solvent. Altering the amount of solute or solvent can change concentration . 4. What are 3 factors that affect solubility? pressure, temperature, and type of solvent. 5. What happens to red and blue litmus paper in an acidic solution? They turn red. 6. What happens to red and blue litmus paper in a basic solution? They turn blue. 7. What happens to red and blue litmus paper in a neutral solution? Stay their original colors. 8. Explain what phenolphthalein will do in acidic, basic, and neutral solutions. Phenolphthalein will be clear or cloudy in acids and neutral solutions, but pink in basic solutions. 9. How do carbonates and metals react with acidic, basic, and neutral solutions? Both will react with acids, but do not react with basic or neutral solutions. 10. What is the difference between using pH paper and phenolphthalein indicator to test an acid and base? PH paper will change colors corresponding to different pH values where phenolphthalein will only change in a base . 11. List 3 characteristics of a base. slippery, bitter, smooth, strong base high electrical conductivity 12. List 3 characteristics of an acid. f eels like water, stings in open cuts, sour, strong acid high electrical conductivity