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