Chemistry Lab Methods Final Exam Study Guide 2012

Below are sample questions that will help you focus on key topics to be covered on this year’s final exam. This is not completely inclusive. Reviewing copies your past unit exams will strengthen this study guide.

  1. Define an observation?
  2. Dialysis tubing is like a screen door because:

For questions 3 – 16, identify the particle (s)

  1. The lightest particle of the atom
  2. The particle that determines what element an atom is (not an electron)
  3. Has a negative charge
  4. Has a positive charge
  5. Has a neutral charge
  6. Used to formulate atomic mass
  7. Particle used in chemical reactions
  8. Moves around the nucleus in energy level cloud
  9. An atom has an equal number of these two particles if it is a neutral atom
  10. What particle has a mass > 1 amu?
  11. What particle has a mass of 1/2000 amu?
  12. Makes up 99.9% of the mass of the atom
  13. Two particles that have opposite charges
  14. As you move down the periodic table, what is true of mass, atomic number, etc?

Match the following answers to statements 17 – 24.

Purpose, Materials, Analysis/Interpretations, Procedures, Hypothesis, Data, Conclusion, Error Statement

  1. List at least three things that could have affected your results.
  2. All measurements recorded during the experiment.
  3. A brief statement of what was done in a step by step fashion
  4. A list of equipment and chemicals used.
  5. Statement of the reason for doing the lab.
  6. Your prediction as to the outcome of the experiment.
  7. Answer all questions that have been handed out or written on the board.
  8. Makes a statement of the relationship between the variables after the experiment.

Identify Questions 25 - 37 as True or False

  1. The meter is greater than the length of 10 centimeters
  2. Liters are used to measure volume
  3. Feet are part of the metric system
  4. A kilometer is bigger than 10 meters
  5. Milliliter is an appropriate unit of measurement for the volume of a glass of water
  6. When converting 10.5 cm to m the decimal place moves to the right
  7. Meter sticks measure grams
  8. 10 meters = 1 decimeter
  9. 10 decimeters fit into 1 meter
  10. Graduated cylinders and beakers are used to measure volume
  11. Measure mass of a dog in kg
  12. Measure the length of a dog’s tail in inches in the metric system
  13. There are 100 centimeters in one meter

For # 38 – 47, answer the following questions in complete sentences

  1. What are the decimal equivalents for: milli , Kilo, deci, centi, meter, hecto
  2. In Dialysis Tubing, the molecule that traveled through the tubing was:
  3. In the Mystery powders lab Iodine reacted with what substance?
  4. When viewing milk fat, the molecules of fat behaved:
  5. The behavior of the milk fat can be explained by:
  6. The powders in the Mystery powders lab that conducted electricity where (ionically bonded/covalently bonded)
  7. How did we use PPH in the myster powders lab? Which substances did it help us identify?
  8. In the solubility lab where there any substances that were soluble in alcohol but not water?
  9. What reacted with vinegar? Why?
  10. The half life of a substance describes what?
  11. Oil ______(sinks/floats) water because oil’s density is ______(more/less) than water.
  12. ______Observations include numbers while ______Observations do not. (Quantitative vs. Qualitative)

Over

The green leaf is 4.0 centimeters long. Use A) Qualitative and B) Quantitative (for Q’s 50 and 51)

  1. Green refers to a ______observation.
  2. 4 centimeters refers to a ______observation.

For questions # 52 – 62, complete the statement

  1. Mg is a ______forms ______when becoming an ion?
  2. The element ____ has 3 protons.
  3. The element __ has both its 1st and 2nd shells full.
  4. Gold has _ electrons.
  5. Radon is a __ gas.
  6. When you determine the # of neutrons of an atom simply by looking at the periodic table? Explain.
  7. Chlorine – 37 has _ electrons, __protons, _ neutrons.
  8. 91. Boron has _ electrons, __protons& a mass of __.
  9. 92. Hydrogen has _ electrons, _protons, & a mass of __.
  10. Helium has _ electrons, _protons, & a mass of_.
  11. When comparing two atoms, an isotope of the same element has:

For #s 63 – 78 identify the statement or formula as indicating the substance as either an acid, base, both, orneither?

  1. Conducts electricity
  2. Stays red with phenol thalanine
  3. Turns yellow with bromothyml blue
  4. Stays blue with bromothyml blue
  5. Turns green with bromothyml blue
  6. Contains H+ ions
  7. Contains OH- ions
  8. NaOH
  9. HCl
  10. H2O
  11. KOH
  12. H2SO4
  13. pH of 0-6
  14. pH of 7
  15. pH of 8-14
  16. stomach juice

In the equation: HCl + NaOH -> H2O + NaCl

  1. Label the acid, base, water, and salt in the reaction above. What type of reaction is this?

Use the following words and your experience from our labs/activities to complete80 - 96.

NeutralizeLikeOppositePlasticAttractCovalent BondingGroups

Ionic Bonding RepelNomenclatureMetal NonmetalPeriodsWool

  1. When a base and an acid are added together they ______.
  2. Wool had a ______charge than the plastic ruler.
  3. Iodine would be attracted to the ______electrode of a battery.
  4. Plastic rulers had a ______charge when both rubbed with wool.
  5. The wool in the electric charge lab was attracted to the ______.
  6. The plastic rulers in the electric charge lab ______each other when one was rubbed with wool and the other plastic .
  7. Opposite electrical charges ______.
  8. Like electrical charges will ______.
  9. The vertical columns are called ___.
  10. The horizontal rows are called ______.
  11. Nonmetal + Nonmetal =
  12. Nonmetal + Metal =
  13. Naming chemical compounds is called:
  14. What conducts heat and electricity well?
  15. What are mostly solids at room temperature?
  16. What are mostly gases at room temperature?
  17. What are ductile and malleable?

Match the following words with statements 97 – 103

Transition MetalsHalogensBoronCarbonNitrogen

Noble GasesAlkaline Earth MetalsAlkali Earth Metals

  1. Group 3-12
  2. Most reactive nonmetals
  3. Most reactive metals
  4. Will form a charge of 4- or 4+ in a chemical reaction
  5. Will form a charge of 3- in a chemical reaction
  6. Does not bond with other elements
  7. Will form a 3+ charge in a chemical reaction

For #s 104 & 105, count

  1. Determine the number of H’s, O’s, and S’s and total number of atoms in H2SO4
  2. Determine the number of Si’s, Cl’s and total # of atoms represented by: 2 SiCl4

Identify the following representations of chemical reactions as: Synthesis, Decomposition, Single replacement, Double replacement

  1. A + B -> C
  2. A -> B + C
  3. A + BC -> AC + B
  4. AB + CD -> AD + CB
  5. Grouping Elements By Chemical Behavior/Properties gives us much more______about the elements than if they are grouped by ___.

WRITE the correct CHEMICAL FORMULAS for #s 111 -115:

  1. Magnesium Oxide
  2. Magnesium Phosphate
  3. Cobalt III sulfite

BALANCE THE CHEMICAL EQUATIONS for #s 116 - 121

  1. ___H2O --> ___H2 + ___O2
  2. ___H2 + ___N2 --> ___NH3
  3. ___KCl + ___O2 --> ____KClO3
  4. ___Al + ___O2 --> _____Al2O3
  5. ___Pb(NO3)2 + _____AlI3 --> _____Al(NO3)3 + ______PbI2
  6. _____ Li + _____ CaCl2 --> _____ LiCl + _____Ca

Heat and Temperature (thermodynamics): Demonstrate your knowledge of thermodynamics by answering statement #s 122 - 131.

  1. What is the kinetic molecular theory?
  2. What does temperature measure?
  3. What is thermodynamics?
  4. What is heat?
  5. Which has more heat, a cup of water at 100ºC or a lake of water at 50ºC? Why? Which has a greater temperature? Why?
  6. Explain how heat moves.
  7. What happens as water is heated, compared to when a metal is heated, like lead. Which stores more heat?
  8. What happens to the distance between molecules of a gas as they absorb calories of heat?
  9. Compare the potential energy of molecules of steam, liquid water, and ice (or any other gas/ liquid/ solid) at the same temperature.
  10. From a thermodynamics stand point, why is ice/water/steam so unique?
  11. What are the phase changes and which are exothermic vs. endothermic?
  12. Be able to use Q = C x m x ΔT , Q = Heat of ______(a specific phase change) x mass that changes phase, and Qgain = - Qlost

Radioactivity: answer questions 132-136 in complete sentences.

  1. If an atom undergoes alpha decay how does its mass and atomic number change?
  2. If an atom undergoes beta decay how does its mass and atomic number change?
  3. If an atom undergoes gamma decay how does its mass and atomic number change?
  4. If there is 200g of a substance how much will be left after 1 half life? 2? 3? 6?
  5. If the half life of a substance is 100 years and there is 500 g to start with 62.5 g left how many years have passed?

Do not forget to make a note sheet, have a calculator, complex ion sheet, periodic table, and a #2 pencil!