Pre-AP Chemistry 1 st Nine Weeks Review Safety and Equipment

Transcription

1 Name _ Period Pre-AP Chemistry 1 st Nine Weeks Review Safety and Equipment 1) Match the safety symbols with their meaning: Symbol a) Radioactive materials being used. b) Danger to the eyes. c) Poisonous substances are being used. d) Substances used could stain or burn clothing. e) Substances used are corrosive to skin. f) Misuse of chemicals could cause an explosion g) Chemicals or chemical reactions could cause dangerous fumes. h) Danger of cuts or punctures caused by the use of sharp objects. i) Use of an open flame could cause a fire or explosion. 2) Hazardous Chemical Coding Diamond: The hazard numbers range from 0-4. The hazard in danger to health, flammability and reactivity increases from 0-4. a) Label the diamond below using the words Health, Flammable, Reactivity and Specific Hazard b) What hazard poses the greatest risk? c) What specific hazard does this chemical pose? d) If you place this chemical near a fire would it catch on fire? 1

2 3) Match the piece of equipment with their purpose: Equipment Name Purpose Beaker Ring Stand Evaporating Dish Wire Gauze Crucible and Cover a) Used to measure the volume of liquids. b) To move hot equipment that is light/small such as an evaporating dish or crucible. c) Used to heat small amounts of solids. d) Used to evaporate samples of liquids. Bunsen Burner Graduated Cylinder Funnel Iron Ring Buret e) Placed on the iron ring to support items being heated. f) Used to heat liquids. g) To deliver very accurately measured amounts of liquids. h) Heat source. i) Clamped to the ring stand and then supports the wire gauze or clay triangle j) For moving beakers of boiling water k) When used with filter paper, it can filter out solids from liquids. l) Used as a support and to clamp other equipment to. Crucible Tongs Beaker Tongs 2

3 Measurement 1) Write the following numbers in scientific notation: a) 23,000 _ b) _ c) _ d) ) Write the following numbers in standard notation: a) 4.5 x 10 3 b) 3.4 x 10-2 c) 6.02 x 10-6 _ 3) How many significant figures are in the following numbers? a) 4.30 d) 120 b) 1020 e) c) f) ) Round each of the following numbers to 3 significant figures a) d) b) 1028 e) c) f) ) Perform the following operations expressing the answer in the correct number of significant figures. a) 1.35 m x m = b) 1,035 m / 42 m = c) ml + (35.2 ml * 6 ml) = d) (1.278x10 3 m) / (1.4267x10 2 m) = e) 0.15 cm cm cm = 3

4 6) Which set of measurements is the most precise, most accurate? Each lab group is supposed to measure 7.00 ml of a liquid and repeat this 4 times. Below is each group s data. Group 1: 6.58mL, 7.06mL, 6.88 ml, 7.02mL Group 2: 7.03mL, 7.08mL, 6.97mL, 7.05 ml Group 3: 6.05 ml, 6.06mL, 6.05mL, 6.04mL Which group was the most precise? _ Which group was the most accurate? _ 7. The diagram below represents a portion of a buret. What is the reading of the meniscus (to the correct # of sig figs)? 8. The diagram below represents a portion of a triple beam balance. If the beams are in balance, with the riders in the position shown, what is the total mass in grams of the object being massed (to the correct # of sig figs)? ml g 9) What is the density of an object having a mass of 8 grams and a volume of 25 cm 3? 10) A substance has a density of 0.7 g/ml, if it has a volume of 3 ml, what is its mass? 11) A sample of iron has the dimensions of 2 cm x 3 cm x 2 cm. If the mass of this rectangularshaped object is 94 g, what is the density of iron? 12) An irregularly shaped stone was lowered into a graduated cylinder holding a volume of water equal to 2.0 ml. The height of the water rose to 7.0 ml. If the mass of the stone was 25 g, what was its density? 4

5 13) A student used a balance and graduated cylinder to collect the following data: Volume of water Volume of water and sample Sample mass 15.0 ml 28.4 ml 10.8 g a) Calculate the density of the sample. Include the appropriate number of significant figures and proper units. b) If the accepted value is 1.27 grams per milliliter, calculate the percent error. (put answer in 3 significant figures) 14) Consider the following data and determine which objects would float or sink in water. Object A has a density of 1.35 g/cm 3 Object B has a density of g/cm 3 Object C has a density of 2.65 g/cm 3 Float or Sink in H 2 O 15) Fill in the following table with the metric prefixes Prefix Abbreviation Scientific notation equivalent Prefix Abbreviation Scientific notation equivalent Tera- Centi- Giga- Milli- Mega- Micro- Kilo- Nano- Pico- 16) Convert the following. a) 36 cm to meters 5

6 b) 78 nm to pm c) 8.02 x mm to km d) The number of seconds in 6.78 days e) 0.44mL/min to micro liters per second Matter 1) Matter can be defined as anything that has_ and takes up. 2) Which of the following can NOT be considered matter? (circle all that apply) a. Air d. natural gas b. Electricity e. snow c. Table Salt f. heat 3) Label the following pictures as: element, compound, mixture of two elements, mixture of two compounds or mixture of elements and compounds. Some answer choices may be used more than once. 6

7 4) Identify the following as a pure substance (S) or mixture (M) Glucose mustard Oxygen gas grapes 5) Identify the following items as an element, compound, heterogeneous or homogeneous mixture: Copper (II) bromide: Beach sand: Vegetable oil: Titanium: Tap water: Copper Pipe 6) Define physical property 7) Define chemical property 8) What is the difference between intensive and extensive physical properties? 9) Classify the following as Physical or Chemical property: Color Reactivity Smell Density Mass Length Volume Flammability Melting point 10) Which of the above properties are intensive physical and which are extensive physical? Intensive: Extensive: 7

8 11) Use the heating curve to answer the following questions. a. Label the solid, liquid and gas regions on the heating curve. b. What is the boiling point (in o C) of this substance? c. What is the freezing point (in o C) of this substance? d. As energy is released from point D to point C, what phase change is occurring? e. As energy is added from point C to point D, what phase change is occurring? f. The phase changes from point B to point A and from point D to point C are both _ processes? g. At what point does melting begin? h. At what point does vaporization begin? i. Does melting or vaporization take more energy and how can you tell? 8

9 12) Are the following processes endothermic or exothermic? a. Freezing: b. Deposition: c. Condensation: d. Melting: 13) Use the phase diagram to answer the following questions. a. Label the solid, liquid and gas regions on the phase diagram. b. What phase change(s) would occur if we decrease the pressure of point A at a constant temperature? c. What phase change(s) would occur if we raise the pressure of point C at a constant temperature? d. What phase change(s) would occur if we lower the pressure of point B at a constant temperature? e. What phases are present at point E? f. Draw a point on the diagram to represent the triple point. What does the triple point represent? 14) What is the difference between physical and chemical changes? 15) Identify each of the following as a chemical or physical change: a) Ice cracking b) Sugar dissolving c) Water freezing d) Milk souring e) Lead melting _ f) Wood burning _ g) Sublimation _ 9

10 16) A chemical change occurs when a piece of wood. (circle all that apply) a. is painted d. decays (decomposes) b. is burned e. is split into two pieces c. is cut into multiple pieces f. floats on water 17) Changing from a solid directly to a gas is called: a. Deposition c. Sublimation b. Vaporization d. Condensation 18) When a gas turns into a liquid this is called. This is a type of change. a. sublimation / physical c. condensation / physical b. condensation / chemical d. sublimation / chemical 19) Fill in the following table: 3 basic Physical states of matter Definite shape? Yes or No Definite volume? Yes or No Circle the example of each Water vapor/steam Ice Water Water vapor/steam Ice Water Water vapor/steam Ice Water 20) If you have a mixture of sand and salt what process can be used to separate the two? Atomic Structure 1) Identify the major accomplishment of each of the following scientists: a. Dalton 1. All matter is made up of tiny _ particles called _. 2. Atoms of a given element are the same in,, and _. Atoms of different elements are _. 3. Atoms are neither nor in a chemical reaction. Atoms are _, _ or _. 4. Atoms of different elements combine in simple ratios to form _. b. Ernest Rutherford - Discovered the nucleus by using the gold foil experiment. He concluded that the atom is mostly space and that the nucleus of the atom has a charge. 10

11 c. J.J. Thomson Discovered the _ by using a cathode ray tube. d. Niels Bohr Developed the _ model of the atom. 2) The overall charge of an atom is neutral. Why? 3) What does the atomic number tell us? 4) How would you find the number of neutrons in an atom? 5) How are the isotopes carbon 12 and carbon 14 the same? How are they different? Same: _ Different: 6) Decide if the following are isotopes (yes or no) a) 5 protons and 6 neutrons b) protons and 6 neutrons 7) How many protons, neutrons, and electrons are in the following neutral atoms? a) 40 K 19 b) 238 U 92 c) 207 Pb 82 d) 20 Ne 10 e) 25 Mg 12 p + = n 0 = e - = p + = n 0 = e - = p + = n 0 = e - = p + = n 0 = e - = p + = n 0 = e - = 8) Subatomic Particle Charge Location Mass Proton Neutron Electron 11

12 9) Complete the chart: Element Protons Neutrons Electrons Mass # Carbon Krypton 45 Plutonium Mercury Mendelevium Fluorine 9 10) Calculate the average atomic mass of a fake element named sony. The two isotopes for sony have atomic masses relative abundances of amu (50.69%) and amu (49.31%). 11) What is the average atomic mass of an element that has 2 isotopes with the following percent abundances: a mass number of 20 that is 25% abundant and a mass number of 22 that is 75% abundant. 12) An element has two isotopes, one with a mass of 109 and the other with a mass of 112. Calculate the % abundance for each isotope if the average mass of the element is amu. 13) An element has two isotopes, one with a mass of 88 and the other with a mass of 89. Calculate the % abundance for each isotope if the average mass of the element is amu. 12

13 Nuclear 1) Define the following terms: a) Fission _ b) Fusion _ b) Half-life _ 2) Fill in the table with the three types of natural radiation: Type of Radiation Beta Isotopic Notation Material needed to stop/shield radiation Alpha Gamma Proton Neutron Positron 3) Write the equation for the beta decay of radon-138 4) Write the equation for the alpha decay of Uranium-238 5) Write the equation when Pu-236 absorbs a neutron. 6) Write the equation when thorium-234 absorbs a proton and emits a beta particle. 7) Write the equation when carbon-14 is bombarded with a positron and emits a neutron. 13

14 8) Complete the following nuclear equations and state the type of radiation emitted. Radiation Type Si Al Na Ne 1 1 H P 0 e ) A patient is administered 20 mg of iodine-131. How much of this isotope will remain in the body after 40 days if the half-life for iodide -131 is 8 days? 10) What is the half-life of Thorium-92 if, after 56 days, g remains from a 10 g starting sample? 11) If the half-life of carbon-14 is 5230 years, how much remains of a 10 g sample after years? 12) The half-life of Co-60 is 5.3 years. How much of a 24 gram sample of this isotope will remain after 10.6 years? 14

15 13) Use the nuclear decay graph below to answer the following questions. a) What is the half-life of this substance? b) After 6 hours what is the activity of the substance? c) Will the activity ever reach zero? 14) What did the following scientists do? a) Fermi: b) Curie: c) Becquerel: Periodic Table 1) In each of the following sets, which atom has the smallest atomic radius? a) Si, Na, Cl b) S, Sn, P c) Al, Cl, B 2) Arrange the following groups of atoms in order of decreasing atomic radius. a) P, Ge, As, S b) Br, Cs, Sn, Sr 3) Label the following on the periodic table: Group Period Alkali metals Halogens noble gases Transition metals Alkaline Earth Metals 15