Level 3 Chemistry Crossword

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Across
  1. 2. The species formed when a base gains a proton.
  2. 7. Shape where atoms form a straight line (180° bond angle)
  3. 8. The point in a titration when the moles of acid and base are equal.
  4. 9. A charged species formed when a metal ion bonds with ligands such as ammonia.
  5. 10. When two organic molecules join together and eliminate a small molecule
  6. 15. A substance containing no water – usually added as a drying agent to removes water to help purify a substance e.g. CaCl2 or SiO2
  7. 16. Total enthalpy change independent of reaction pathway, _______ Law
  8. 17. Measure of disorder or randomness in a system
  9. 19. A measure of how well a solution carries electrical current due to mobile charged particles.
  10. 22. Reaction that releases heat, ____thermic
  11. 25. A side chain off the main parent chain of an organic compound. E.g. a methyl group.
  12. 28. A substance that changes colour over a particular pH range.
  13. 29. A method of heating with a vertical condenser to speed up the rate of reaction and prevent the loss of volatile substances.
  14. 30. The presence of this type of ion decreases the solubility of a sparingly soluble ionic solid.
  15. 31. The process by which a weak acid or base reacts with water to form ions.
  16. 32. Average kinetic energy of particles in a substance
  17. 33. Type of bond formed by the sharing of electron pairs
  18. 34. The state in which the forward and reverse reactions occur at equal rates.
  19. 38. A reaction with water in either acidic or basic condition used to split up a larger organic molecule (usually ester or amide)
  20. 40. KS need to be smaller than this for a precipitate to form
  21. 42. Charge separation in a molecule causes a __________ moment
  22. 44. The process of distributing electrons evenly to minimize potential repulsion, ___________ theory
  23. 45. Distance from nucleus to outermost electron; ________ radius
  24. 46. The pH at the halfway point of a weak acid–strong base titration is equal to this.
  25. 48. The equilibrium constant for the ionisation of water.
  26. 49. The product that forms when 2 amino acids join together to make one amide bond between them.
  27. 50. Shape of H₂O molecule due to two lone pairs on oxygen
  28. 53. Calculating bond _______ uses the formular: bonds broken-bonds formed
  29. 54. Attractive forces between molecules are ____________ forces
  30. 57. Total heat content of a system; negative for exothermic reactions
  31. 59. The equilibrium constant for a saturated solution of a sparingly soluble ionic solid.
  32. 62. The reactant that is completely consumed first in a chemical reaction.
  33. 63. Energy needed to remove an electron from an atom in gaseous state ______________ energy
  34. 66. Type of bond formed through the transfer of electrons
  35. 68. Difference in electronegativity forms a _______ bond
  36. 69. When an organic molecule has the same molecular formula (number and type of atoms) but different structural formula (arrangement of atoms).
  37. 70. An insoluble solid that forms when ions in solution react.
Down
  1. 1. A method used to separate a mixture made of substances with different boiling points. It uses a condenser attached on an angle so that when one compound evaporates over its bp then when it condenses again it drips into a separate flask.
  2. 3. Atoms in Period 3 can exhibit this to enable more than 4 pairs of electrons _______________ octet
  3. 4. Heat energy associated with melting a solid to a liquid, enthalpy of ______________
  4. 5. The process of decreasing concentration by adding more solvent.
  5. 6. A blue solution containing Cu2+ ions which when heated will react to form a brick red precipitate with aldehydes.
  6. 11. Molecular shape with 90° bond angles
  7. 12. The ion, H₃O⁺, whose concentration is used to calculate the pH of an acidic solution.
  8. 13. Usually special situations that occur alongside a reagent added – common examples include heat, acidic, basic conditions.
  9. 14. A blue solution containing Cu2+ ions which when heated will react to form a brick red precipitate with aldehydes.
  10. 18. A graph showing how pH changes as titrant is added.
  11. 20. Easily is able to turn from liquid to a gas due to weak attractions holding the molecules together.
  12. 21. The equation used to calculate buffer pH from pKa and the ratio of conjugate base to weak acid.
  13. 23. The equilibrium constant describing the ionisation of a weak acid in water.
  14. 24. A molecule that has both an amine and carboxylic acid bonded to the same carbon. 20 amino acids make up the building blocks of life.
  15. 26. The part of a titration curve where pH changes relatively little as titrant is added.
  16. 27. A molecule with a double bond and each double bonded C has 2 different atoms or groups can form cis/trans isomers due to the different special arrangements because of the restricted rotation of a double bond.
  17. 35. Orange coloured bromine (Br2) dissolved in water.
  18. 36. The ion, OH⁻, whose concentration is used to calculate the pH of a strong base solution.
  19. 37. Heat energy required to vaporize a liquid, enthalpy of _________________
  20. 38. Strong intermolecular force between molecules with H bonded to N, O, or F, _____________ bonding
  21. 39. An organic compound that just has one long chain of carbons (no branched chains)
  22. 41. The species formed when an acid loses a proton.
  23. 43. The shape of XeF₄ molecule
  24. 47. A colourless solution containing Ag+ ions which when heated will react to form a silver mirror (Ag) with an aldehyde.
  25. 51. Energy required to raise 1 g of a substance by 1°C, specific _________ capacity
  26. 52. Reaction that absorbs heat, _____thermic
  27. 55. Preferred position for non-bonded pairs
  28. 56. Electronegativity is the tendency of an atom to attract __________ electrons
  29. 58. Minimum energy required for a reaction to occur ________________ energy
  30. 60. A long repeating chain made of multiple monomers that have bonded together
  31. 61. A molecule containing a chiral carbon can have two different arrangements of the atoms as they are non-superimposable mirror images.
  32. 64. The chemical you add to make a reaction occur.
  33. 65. Calculating change in entalpy by measuring the change in temperature of water
  34. 67. A solution that resists changes in pH when small amounts of acid or base are added.