FALL SEMESTER REVIEW NAME: PERIOD: 1. (Unit 7) When the equation Cu + AgNO 3 Cu(NO3) 2 + Ag is balanced the coefficient of Ag NO 3 is? 2. (Unit 7) Balance the following equation: AgNO 3 + BaCl 2 AgCl + Ba(NO 3 ) 2 3. (Unit 2) Is the following picture representing accuracy, precision or both? Explain the difference. 4. (Unit 2) Determine the amount of liquid in the following graduated cylinders. (remember to use correct significant figures. 100 ml 50 ml 50 ml 40 ml 30 ml 20 ml 10 ml A)_ml B) _ml General Chemistry, 2011-2012 Page 1
FALL SEMESTER REVIEW NAME: PERIOD: 5. (Unit 7) True/False: According to the law of conservation of mass, the total mass of the reactant substances is always equal to the mass of the products. 6. (Unit 3) Of the following examples, circle the ones that are physical changes. a) Boiling water b) Burning charcoal c) Food rotting d) Churning butter (stirring) 7. (Unit 7) Write the balanced equation for the reaction of a solution of Magnesium Hydroxide and Nitric Acid that produces Magnesium Nitrate and water. 8. (Unit 3) First label the phase change diagram with the following phase changes: Sublimation, condensation, melting, evaporation, freezing and deposition. Second, highlight the phase changes that are losing energy. General Chemistry, 2011-2012 Page 2
FALL SEMESTER REVIEW NAME: PERIOD: 9-10: (Unit 1) Using the following scenario, answer the quest: Hypothesis: If you give children a reward then they are more likely to draw with magic markers. Experiment: Some children were told that they would be given a special award for drawing with magic markers (an activity they already enjoyed). Other children were simply asked to draw with the magic markers. One week later, the children were unobtrusively observed for how much time they spent drawing with the markers. Result: The children who expected and received a reward for drawing with the markers were less likely to draw with them later. 9. What is the: a)independent Variable: b)dependent Variable: 10. Did the results confirm or refute the hypothesis? Explain. 11. (Unit 4) Determine which family from the periodic table is represented by the following characteristics: a) Inert (unreactive) gases: b) silver in color, 2 nd most reactive metals:_ c) most reactive nonmetals which usually form salts with metals: d) most reactive metals that must be stored in mineral oil:_ 12. (Unit 3) Describe the characteristics of each of the following including: shape and volume, molecule movement and closeness, compressibility. Solid: Liquid: Gas: General Chemistry, 2011-2012 Page 3
FALL SEMESTER REVIEW NAME: PERIOD: 13. (Unit 2) Convert the following to scientific notation: a) 75,100,000 b) 0.000 002 31 14. (Unit 2) Determine the number of significant figures in each of the following: a) 4000 b) 0.004 5 c)2.050 10 24 d)100.0 e) 3.990 15. (Unit 2) Four lab groups performed the same experiment three times to determine the boiling point of mercury. The accepted melting point is 358 C. Indicate whether the following sets of data are precise, accurate, both or neither. Precise, Accurate, Both or Neither Reasoning Group Trial 1 Trial 2 Trial 3 1 347.3 C 358.9 C 363.6 C 2 340.1 C 370.8 C 364.2 C 3 357.9 C 358.1 C 358.3 C 4 370.1 C 370.3 C 369.8 C 16. (Unit 2) Volume can be expressed as 1L which is equivalent to 1_ or 1. 17. (Unit 2) Convert the following using dimensional analysis : a) 125 g = Kg b) 3.34 mm = cm c).898 g = mg 18. (Unit 2) Convert the following to miles per hour (mi/hr) 850 m/s = mph? 19. (Unit 2) The density of silver nitrate is 13.6 g/ml. What is the mass of 35.0 ml of silver nitrate? General Chemistry, 2011-2012 Page 4
FALL SEMESTER REVIEW NAME: PERIOD: 20. (Unit 4) JJ Thompson discovered using the experiment. Using the Gold Foil experiment Ernest Rutherford discovered most particles went through the foil and some alpha particles were _ because they were hitting a dense charged nucleus. 21. (Unit 4) Compare the masses of protons, neutrons and electrons. 22. (Unit 4) Describe where the subatomic particles (protons, neutrons and electrons) can be found in the atom. 23-24. (Unit 4) When an atom has more electrons than protons, the charge is (positive / negative / neutral). When an atom has more protons than electrons, the charge is (positive / negative / neutral). When the number of protons and electrons is equal, the charge is (positive / negative / neutral). 25-26. (Unit 4) An atom has an atomic number of 15, a mass number of 32, a charge of +3 and an atomic mass of 31.97 amu. What is the identity of the element? Which type of number should you use to identify the element? Write the chemical configuration for this element. _ 27. (Unit 4) What is the atomic number of silver? 28-29. (Unit 4) Describe what is different between the isotopes carbon-12 and carbon-14 in terms of the number of subatomic particles. Calculate the number of protons and neutrons in each isotope. 30. (Unit 4) In terms of the information printed on your periodic chart, explain why nitrogen (N) comes after carbon (C) on the periodic chart. 31. (Unit 5) According to your understanding of the Electromagnetic Spectrum, list the colors of the Visible Spectrum in order of increasing frequency. What is the relathip between frequency and wavelength? General Chemistry, 2011-2012 Page 5
FALL SEMESTER REVIEW NAME: PERIOD: 32. (Unit 5) In your own words, describe what is happening as an electron moves from the excited state to the ground state. Describe this in terms of energy. 33. (Unit 5) Write the correct electron configuration for the following elements: a. Fe b. Ca c. S 34. (Unit 5) Put the following sublevels in order of increasing energy (Lowest to Highest) 1s 5p 2s 2p 3p 3s 4s 4p 4d 3d 5s 35. (Unit 5) 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 6 is the electron configuration for which element? 36. (Unit 5) If the s and p sublevels are filled for an element, how many valence electrons would the element contain? 37.(Unit 5) Define Hund s rule in your own words and explain why it is important: 38. (Unit 5) Write the correct orbital notation for the following elements: a. Ca b. Fe c. S 39.(Unit 5) Where do you find the valence electrons for an element using the Periodic Table? General Chemistry, 2011-2012 Page 6
FALL SEMESTER REVIEW NAME: PERIOD: 40. (Unit 4) List the elements that would have similar chemical and physical properties to those in Ca and explain why? 41. (Unit 4): Define the periodic trend of electronegativity: What is the most electronegative element? Use arrows to depict the trend for electronegativity on the periodic table below: 42. (Unit 4): Define the periodic trend for atomic radii: What is the element with the largest atomic radius (largest element)? Use arrows to depict the trend for atomic radius on the periodic table below: General Chemistry, 2011-2012 Page 7
FALL SEMESTER REVIEW NAME: PERIOD: 43. (Unit 6): An ionic bond is created between a (positive ion) and a (negative ion). Electrons are and create an attraction that holds the elements together. 44. (Unit 6): Circle the ionic compound(s): LiF H 2 O BCl 3 CH 4 NaCl CO 2 MgBr 2 NH 3 NaNO 3 NH 4 ClO 3 45. (Unit 6): Draw an example of each of the following VSEPR shapes: **Remember, all elements want 8 valence electrons except for Hydrogen (H) and Helium (He) that only want 2. Also, Boron (B) can have only 6 electrons (or 3 bonds)** VSEPR Shape: AXE formula: Lewis Dot Molecule Example: Linear AX Bent Trigonal Planar AX3 Trigonal Pyramidal AX3E1 Tetrahedral General Chemistry, 2011-2012 Page 8
FALL SEMESTER REVIEW NAME: PERIOD: 46-50. (Unit 6) Fill in the following table: Group # Group Name # Valence Electrons Example Lewis Dot Structure of Atom 1 K Charge (Oxidation #) Example Lewis Dot Structure of Ion 2 +2 [Mg] 3-12 Transition Metals 13 +3 14 15 16 6 17 18 General Chemistry, 2011-2012 Page 9
FALL SEMESTER REVIEW NAME: PERIOD: 51-60 (Unit 7) Make a chemical compound using the /atoms given and fill in the chart sodium & sulfide Ionic, Molecule or Acid Chemical Formula Formula Name calcium & fluoride write own formula using a group 1 or 2 metal ion & a non-metal ion Iron(II) & oxide Lead(IV) & iodide write own formula using a metal ion from group 3-14 & a non-metal ion hydrogen & sulfate hydrogen & perchlorite hydrogen & sulfide write own formula for an acid sodium and acetate ammonium & nitrite write own formula using polyatomic three carbon atoms and six oxygen atoms General Chemistry, 2011-2012 Page 10
FALL SEMESTER REVIEW NAME: PERIOD: two nitrogen atoms & two fluorine atoms write own molecular formula using two different non-metal atoms Determine how many (number) of each atom is in the given compound. HClO 4 C 2 H 12 O 6 Pb(MnO 4 ) 2 V 2 (SO 4 ) 5 H Cl O C H O Pb Mn O V S O Word Bank Chemical formula Coefficient Atom Superscript Subscript 4H 2 + 2O 2 4H 2 O Mg +2 Place the word (found in Word Bank) that describes each item the arrow is pointing to on the arrow. Match the word with the following descript. _ Indicates the oxidation number, or the charge _ Indicates the number of moles of that compound _ the number of atoms or of each type that are combined I the simplest unit. _ the smallest unit of an element that maintains the properties of the element General Chemistry, 2011-2012 Page 11
FALL SEMESTER REVIEW NAME: PERIOD: Fill out the following table: Cation Anion # cat in compound # an in compound Cation oxidation # * # cat Anion oxidation # * # an Total charge on compound MgCl 2 Rb 2 O The oxidation # of all in a compound add up to so that the total charge on a compound is. General Chemistry, 2011-2012 Page 12