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AP Chemistry

Subjects : science, ap, chemistry
Instructions:
  • Answer 50 questions in 15 minutes.
  • If you are not ready to take this test, you can study here.
  • Match each statement with the correct term.
  • Don't refresh. All questions and answers are randomly picked and ordered every time you load a test.

This is a study tool. The 3 wrong answers for each question are randomly chosen from answers to other questions. So, you might find at times the answers obvious, but you will see it re-enforces your understanding as you take the test each time.
1. The amount of energy/heat required to raise some substance 1 degree C






2. The entropy of a pure perfectly formed crystal @0K is 0






3. Cl¹?






4. If needed - indicate charge of metal(cation) by...






5. An equilibrium expression






6. Faraday's constant






7. 120° - sp^2






8. Reactant that's completely used up in a chemical reaction






9. Atoms with the same number of protons but a different number of neutrons






10. neutron (symbol)






11. An element with several different forms - each with different properties (i.e. graphite & diamond)






12. Mols A/ total mols - XA






13. Oxidation # of Compounds






14. The total energy of the universe is constant - all systems tend towards minimum energy






15. The part of the universe one is focused upon (in thermodynamics)






16. HCl - HBr - HI - HNO3 - HClO4 - H2SO4






17. If K>1 - then Gº<0 and reaction will be...at chemical equilibrium






18. Liquid to solid






19. Solid to gas






20. Carbonates - Hydroxides - Oxides - Phosphates - Sulfides






21. Releases/gives off heat (negative value)






22. Solution in flask being titrated






23. Group 1 - Ammonium - Nitrates - Acetates - Sulfates - Halides






24. Elements on staircase on periodic table






25. Color of Ba (flame test)






26. Mass #






27. H?+OH??H2O






28. Anything occupying space and with mass






29. Has values from -l to l - including zero; tells orientation of the orbital relative to other orbitals






30. Phase change from gas to solid






31. 1 sigma bond






32. For significant digits - leading zeros ____ significant






33. Negative enthalpy - heat flows into surroundings






34. Energy involved in gaining an electron to become a negative ion






35. Mol/kg of solvent - used in calculating colligative properties






36. Idea Gas Law (actual rules)






37. A neutral molecule/ion having a lone e- pair that can be used to form a bond to a metal ion






38. I=moles of particles/moles of solute dissolved


39. How to Find a Weighted Average






40. A weak acid that changes color at or near the equivalence point






41. Ionizes to produce H+ ions






42. Degree of disorder in a system






43. Experimental yield/theoretical yieldx100






44. Puts H? into solution






45. 1 sigma bond - 2 pi bonds






46. The lowest energy configuration for an atom is the one having the max number of unpaired electrons allowed by the Pauli principle in a set of degenerate orbitals


47. Heat capacity formula






48. Molecules' tendency to stick to one another






49. States molecules at a given temp. vary in kinetic energy along a bell-curve of molecular velocities






50. (organics) ten carbons