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Chemistry Review

Chemistry Review. This is a review of the entire year, starting with Unit One and working up through Unit 15.

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Chemistry Review

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  1. Chemistry Review This is a review of the entire year, starting with Unit One and working up through Unit 15. The first page is the page is composed of Unit 1 through 15. Click on the bubble and it will take you to a quick review and reminder of that unit. From there you will go onto the questions for that chapter. Read the question, work out the answer and click on the first review bullet. There you will find multiple answers with only one being the correct one. If you click the correct an answer it will take you back to the first page and you can move onto the next chapter. If the answer you choose is incorrect, it will take you back to the question and you can start over. R A & K D

  2. Unit 2 Unit 1 Unit 3 Unit 5 Unit 4 Unit 7 Unit 6 Unit 8 Unit 9 Unit 10 Unit 12 Unit 13 Unit 11 Unit 14 Unit 15

  3. NEXT  Unit 1Symbols Memorize your symbols from the beginning of the year!

  4. Question for Unit 1 NEXT  Memorize Symbols for the Following: Potassium Calcium Iron Copper Sodium

  5. Answers for Unit 1 K Ca Fe Cu Na P Ca I Co S

  6. NEXT  Unit 2Atomic Theory Atomic number: The number of protons in the nucleus of an atom Atomic Mass: A weighted average mass Mass Number: The total number of protons and neutrons in nucleus of an atom

  7. Question for Unit 2 NEXT 

  8. Answers for Unit 2

  9. NEXT  Unit 3Periodic Table Elements are arranged by atomic number, there is a periodic repetition in their physical and chemical properties. Atomic radius Half the distance between the nuclei of two atoms. (Atoms are the same and bonded together) Electronegativity It is a measure of the element's ability to attract the electrons which are in a bond Horizontal rows:  Called “periods” 7 periods Show the number of the shell Vertical columns: Called “groups” Show the valance electrons Elements in a group have similar physical and chemical properties

  10. Question for Unit 3 NEXT      I                   II              III               IV              V               VI               VII           VIII 1.  The following elements belong in the same families             BFT---DGLZ   JNV   CMS   QXY   AEO   IPH   UKWR 2.  The charge on an ion of H is +4 and -4 3.  A neutral atom of C contains 8 electrons 4.  G is a noble gas 5.  U is an alkali metal 6.  E has 5 electrons in its outermost shell 7.  N is an alkaline earth metal 8.  T has 3 electrons in the fourth energy level 9.  Q is a halogen 10.  F has the smallest atomic mass in its family 11.  T is more metallic than B 12.  J has 20 protons 13.  P has the lowest ionization energy in its family 14.  N has 6 neutrons in its nucleus 15.  S’s atomic radius is greater than that of C 16.  C is more closely related to S than to M 17.  Y is a liquid whereas Q is a gas 18.  X has the lowest electronegativity in its family 19.  K has the largest radius in its family 20.  W is a gas 21.  R has a higher ionization energy than U 22.  Atom Z has 2 neutrons 23.  D contains 10 protons 24.  The electrons of atom G are distributed over 3 energy levels 25.  H is the least metallic element in its group 26.  The electrons of atom O are distributed over 3 energy levels 27.  A is more metallic than either O or E

  11. Answers for Unit 3 1 W Z R E N F H C Q D I G U V B O S Y K J T P A M X L 2 N Z C D V R F I E Q U A G J B H M Y L W K T P O S X

  12. Unit 4Formula Writing NEXT  Type 1 - metal and nonmetal:Cation is named first and anion named second Type 2 – contain a multivalent cation: These compounds include a multivalent cation, so we must identify the charge on the cation in the name of the compound Type 3 – two nonmetals: The first element is named with the full element name the second element is named as an anion (-ide) Prefixes denote the numbers of atoms present **mono- is not used for the first element NAMING ACIDS Binary acids contain only 2 elements. When naming binary acids, use the prefix hydro and the suffix ic Example:  HCl hydrochloric acid Ternary acids contain 3 elements. *Generally, the most common form of the ternary acid is given no prefix and a suffix of –ic Example:  HClO3 chloric acid * if a second acid is formed containing the same elements, but fewer oxygen atoms, the suffix is –ous Example: HClO2 chlorous acid *if a third acid containing still fewer oxygen atoms, it is given the prefix, hypo- and the suffix –ous Example: HClO hypochlorous acid *if the acid contains one more oxygen atom than the common form, the prefix is per- Example: HClO4 perchloric acid

  13. Question for Unit 4 NEXT  • lithium sulfide            ____________________ •  beryllium fluoride      ____________________ magnesium oxide        ____________________ cesium phosphide        ____________________

  14. Answers for Unit 4 Li3S Be3F2 Mg3O2 Cs3P2 Li2S BeF2 MgO Cs3P

  15. Unit 5: Bonding NEXT  • BONDING and SHAPES XY • Shape: always linear • BONDING and SHAPES XY2 • Shape: Linear or bent • Depends on presence of unshared electrons • BONDING and SHAPE XY3 • Shape: Trigonal planar or Trigonal pyramidal • Depends on presence of unshared electrons • BONDING and SHAPE XY4 • Shape: Tetrahedral

  16. Question for Unit 5 NEXT  Match the following molecular shapes with the molecule description a) Linear b) bent c) trigonal pyramidal d) trigonal planar e) tetrahedral • ____ionic XY3 • ____ ionic XY • ____ covalent XY2 • ____covalent XY • ____ ionic XY2 • ____ ionic XY4 • ____ covalent XY4 • ____ covalent XY3

  17. Answers for Unit 5 • C ionic XY3 • A ionic XY • B covalent XY2 • D covalent XY • B ionic XY2 • A ionic XY4 • E covalent XY4 • E covalent XY3 • D ionic XY3 • A ionic XY • B covalent XY2 • A covalent XY • A ionic XY2 • E ionic XY4 • E covalent XY4 • C covalent XY3

  18. Unit 6Chemical Reaction NEXT  • Single Displacement:One element and one compound producing a different element and compound • Double Displacement:Two compounds producing two different compounds • Combustion:Ahydrocarbon reacts with oxygen to produce carbon dioxide and water • SOLUBILITY RULES • All common salts of Group I elements and ammonium are soluble • All common acetates and nitrates are soluble • All binary compounds of Group 7 (other than F) with metals are soluble except those of silver, mercury I and lead • All sulfates are soluble except those of barium, strontium, calcium, silver, mercury I and lead • Except for those in Rule 1, carbonates, hydroxides, oxides, sulfides and phosphates are insoluble

  19. Question for Unit 6 NEXT  Coefficient total Zn + Pb(NO3)2  Zn(NO3)2 + Pb ___________ Type of Reaction:__________________

  20. Answers for Unit 6 Coefficient total: 7 Type: Double Displacement Coefficient total: 4 Type: Single Displacement

  21. Unit 7The Mole NEXT  The unit all chemists use in describing numbers of atoms. Once you know the moles of atoms present, you can easily determine the number of atoms present.

  22. Question for Unit 7 NEXT  A compound is found to have a percent composition of 40.0% C, 6.71% H, and 53.3% O. What is its empirical formula?

  23. Answers for Unit 7 H2OC CH2O

  24. Unit 8Stoichiometry NEXT  The process of using a chemical equation to calculate the relative masses of reactants and products involved in a reaction. Step one: Balance the equation for the reaction Step two: Convert the masses of reactants or products to moles Step three: Use the balanced equations to set up the appropriate mole ratio(s) Step four: Use the mole ratio(s) to calculate the number of moles of the desired reactant or product Step five: convert from moles back to mass

  25. NEXT  Question for Unit 8 How much N2 in liters is needed to react completely with 12.4 grams of H2 in the following reaction?

  26. Answers for Unit 8 45.8 L M 36.8 L M

  27. NEXT  Unit 9Heat Heat: the transfer of energy from one substance to another. The nature of energy. The ability to produce heat or do work. Potential energy: stored energy Kinetic energy: energy due to the motion of objects and depends on the mass of the object and its velocity

  28. Question for Unit 9 NEXT  An 18.5g piece of metal with an initial temp. of 100.9˚C is added to 75.3 g of water with an initial temperature of 22.9˚C. The final temperature is 27.0˚C. Calculate the specific heat of the metal.

  29. Answers for Unit 9 .94 J/G˚C .24 J/G˚C

  30. NEXT  • Heat Unit 10Gas Laws • Energy transferred due to differences in temperature • Temperature • Measure of the average kinetic energy of particles composing a material • Pressure • Force per unit area • Volume • The amount of space a material occupies • Temp and volume are directly related • Temp and pressure are directly related • Pressure and volume are indirectly related

  31. Question for Unit 10 NEXT  A gas at 500. K occupies a volume of 50. mL. what temperature is needed to increase the volume to 500 mL?

  32. Answers for Unit 10 5000K 6000K

  33. Unit 11Solutions NEXT  • “Like dissolves Like” • Polar molecules dissolve polar molecules • Nonpolar molecules dissolve nonpolar molecules Saturated:–When a solution contains the maximum amount of solute Supersaturated:–When the solution contains more solute than a saturated solution will hold at that temperature Unsaturated:–When a solvent can dissolve more solute Concentrated:–When a relatively large amount of solute is dissolved Dilute:–When a relatively small amount of solute is dissolved

  34. Question for Unit 11 NEXT  At what temperature is the solubility of KNO3 20g/100cm3 H2O?

  35. Answers for Unit 11 20.0°C 25.0°C

  36. Unit 12Reaction Rates NEXT  • Reaction Rate: The rate of disappearance of a reactant or appearance of a product • Temperature: Increasing temperature increases the average kinetic energy of particles This increases the number of collisions between reactants This increases the collision energy

  37. Question for Unit 12 NEXT  Write the equilibrium constant expression for the following: H2(g)     +   O2(g)   ↔   H2O(g)

  38. Answers for Unit 12 [H20]2 ———————— [H2]2[O2] [O2] ———————— [H2O]2[H2]

  39. Unit 13Solubility Rates NEXT  SOLUBILITY PRODUCT CONSTANT • The equilibrium constant for the dissolving of a slightly soluble salt REVIEW LeCHATLIER’S PRINCIPLE • If a system at equilibrium is subjected to a stress, the system will adjust to relieve that stress

  40. Question for Unit 13 NEXT  Determine the concentration of Barium Carbonate in the saturated solution.

  41. Answers for Unit 13 5.08 x 105 6.08 x 10-5

  42. Unit 14Acids and Bases NEXT Acids, bases and salts conduct electricity when dissolved in water Acids, bases and salts are considered to be electrolytes Acids– substances that ionize in water to produce hydrogen ions (protons) Bases- substances that ionize in water to produce hydroxide ions Salts- substances that ionize in water to produce something other than hydrogen and hydroxide ions

  43. Question for Unit 14 NEXT  What is the hydronium ion concentration of a .100M solution of formic acid, HCOOH? (Ka = 1.77 x 10-4)

  44. Answers for Unit 14 .00421 M .0421 M

  45. Unit 15Redox NEXT  • THE APPARENT CHARGE ON AN ATOM • RULES –The oxidation number on any free element is zero –The oxidation number of a monatomic ion is equal to the charge on the ion –The oxidation number of Hydrogen in most compounds is +1 –The oxidation number of Oxygen in most compounds is -2 –The sum of the oxidation numbers of all the atoms in a particle must be equal to the apparent charge of that particle.

  46. Question for Unit 15 NEXT  1. assign each one an oxidation number to all species in the equation 2. is the reaction redox 3. add up all the oxidation numbers and fill in the blank 4. if yes, name the oxidizing agent and reducing agent CuO + H2  Cu + H20

  47. Answers for Unit 15 redox-yes sum of all oxidation number- 3 oxidizing agent- H2 reducing agent- CuO redox-yes sum of all oxidation number- 1 oxidizing agent- CuO reducing agent- H2 Not a Redox Reaction

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