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MCAT Chemistry

Subjects : mcat, science
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. Atoms react by gaining or losing electrons so as to acquire the stable electron structure of a noble gas - usually eight valence electrons






2. Named after their cation and anion






3. The lowest allowable energy state of an atom






4. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance






5. Attractive and repulsive forces between molecules that are weaker than forces within molecules.






6. Elements in the middle of the periodic table - in groups 3-12.






7. (chemistry) the sum of the relative atomic masses of the constituent atoms of a molecule






8. Acids defined as electron - pair acceptors and bases as electron - pair donors.






9. A physical property of a solution that depends on the number - but not the identity - of the disswolved solute particles; example properties include vapor pressure lowering - boiling point elevation - osmotic pressure - and frezzing point depression






10. Attractions between molecules caused by the electron motion on one molecule affecting the electron motion on the other through electrical forces; these are the weakest interactions between molecules






11. Substance in which a solute is dissolved to form a solution






12. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.






13. A concentration unit of a solution expressed as moles of solute dissolved per liter of solution






14. (chemistry) a substance that changes color to indicate the presence of some ion or substance






15. Contains nonmetals that are non - reactive. Full outermost energy level except helium which has 2.






16. The nuclear charge experienced by the outermost electrons of an atom (actual charge minus the shielding caused by inner shells: Z- eff)






17. A chemical bond in which one atom loses an electron to form a positive ion and the other atom gains to electron to form a negative ion






18. A chemical formula showing the ratio of elements in a compound rather than the total number of atoms






19. Numbers that specify the properties of atomic orbitals and of their electrons






20. Play- by- play showing the individual steps of a reaction - including the formation and destruction of any reaction intermediates that may occur.






21. Product of the molar concentrations of dissociated ions in solution at saturation - where each ion is raised to the power of its stoichiometric coefficient. Denoted Ksp.






22. Energy released when an atom or ion in the gaseous state gains an electron. Increases from left to right and from bottom to top on the Periodic Table.






23. Region in a molecule where atomic orbitals overlap - resulting in either a stable low - energy bonding orbital or an unstable high - energy antibonding orbital.






24. The process by which one or more substances change to produce one or more different substances






25. 2.18 x 10^-18 J/electron






26. A graph of pressure versus temperature that shows the conditions under which the phases of a substance exist






27. A horizontal row of elements in the periodic table






28. The Percent by mass of each element in a compound.






29. The average distance between the nuclei of two bonded atoms






30. Any sample of a given compound will contain the same elements in the identical mass ratio.






31. Common definition of acids as proton (H+) donors and bases as proton acceptors






32. Chalcogens - - Oxide O






33. Spectrum of certain absorbed wavelengths of light corresponding to an atom's spectrum of emitted frequencies of light. Unique to each element. AAS can be used to indentify an element.






34. (chemistry) p(otential of) H(ydrogen)






35. Solids in which the particles are arranged in a repeating - 3- D pattern - has a specific melting point - classified as ionic network covalent - metallic or molecular.






36. The number of atoms in exactly 12 g of pure 12c and equal to 6.022 x 10^23 is called






37. A subatomic particle that has a positive charge and that is found in the nucleus of an atom Charge of +1 and mass of 1.0073 amu






38. A solid made up of particles that are not arranged in a regular pattern.






39. Have three valance electrons. In certain instances - some elements will loose three electrons - but they will also share electrons with another element to attain stability.






40. A naturally occurring or synthetic compound consisting of large molecules made up of a linked series of repeated simple monomers






41. A chemical bond that involves sharing a pair of electrons between atoms in a molecule






42. An atom or group of atoms that has a positive or negative charge






43. (chemistry) a series from actinium to lawrencium of 15 radioactive elements with increasing atomic numbers






44. A model of acids and bases which an acid is hydrogen ion donor and base is a hydrogen ion acceptor.






45. The energy required to break a chemical bond and form neutral isolated atoms






46. A fundamental constant - h - that relates the energy of light quanta to their frequency: h = 6.6 X 10^-34 joule

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47. The process of decomposing a chemical compound by the passage of an electric current.






48. Theory stating that the rate of a reaction is directly proportional to the number of collisions that take place between reactants per second.






49. The slowest elementary step which is the limit for the rate of the other steps






50. The vapor pressure of solution is the product of the mole fraction of the solvent and the vapor pressure of the pure solvent. P_a=X_aP_total

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