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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. Temperature is constant; effusion and temperature are proportional to the square root of their masses

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2. Redox reaction - in which the same species is both oxidized and reduced.






3. Structure that occurs when it is possible to draw two or more valid electron dot structures that have the same number of electron pairs for a molecule or ion






4. The ratio of the number of moles of solute dissolved in one kilogram of solvent. molality (M = moles solute/kg of solution)






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






6. When a solute is dissolved in a solvent - it will dissociate until reaching an equilibrium point at which the rate of dissociation equals the rate of precipitation of the solute - regardless of any additional solute introduced into the mixture






7. The area of chemistry that is concerned with reaction rates and reaction mechanisms






8. Tells you how much solute is present compared to the amount of solvent






9. 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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10. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds






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






12. At a constant pressure - the volume of an ideal gas is directly proportinal to its temperature: V (a) T

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






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






15. A solution in which water is the solvent






16. Side - to side parallel orbitals overlap to share electrons - the 2nd/3rd covalent bond between two atoms - cannot rotate and maintain the bond.






17. An ionic compound that resists changes in its pH






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






19. The weight in grams of one mole of a given elementand is expressedin tems of grams per mole.






20. Charge assigned to an atom in a molecule or polyatmic ion - calculated by (# valence electrons) - (# 1/2 bonding electrons) - (# nonbonding electrons). Molecules containing atoms with lower formal charges tend to be more stable than those with higher






21. The weak attractive forces between molecules resulting from the small - instantaneous dipoles that occur because of the varying positions of the electrons during their motion about nuclei






22. The amount of energy that reactants must absorb before a chemical reaction will start; also called free energy of activation.






23. A subdivision of an energy level in an atom. They are divided into orbitals.






24. Mixture of 2 or more substances that distills at a constant temperature and with constant composition - even though seperately the components have different boiling points






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






26. (physics) the smallest discrete quantity of some physical property that a system can possess (according to quantum theory) E=hf






27. One - half of the distance between the center of identical atoms that are not bonded together. Since effective nuclear charge increases when moving from left to right each additional electron is pulled more strogly toward the nucleus.






28. Sum of the protons and neutrons in an element often denoted by the letter A






29. 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.






30. A set of frequencies of electromagnetic waves given off by atoms of an element; consists of a series of fine lines of individual colors






31. The point during a titration when the number of H+ ions and OH- ions are equal. This is at the middle of the steepest part of the titration curve.






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






33. When polar molecules orient themselves such that the positive region of one molecule is close to the negative region of another molecule.






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






35. The process by which a gas escapes from one container to another at lower pressure through a tiny hole in the container.






36. Halogens; ns2np5 - - 2nd most reactive group - The Halogens; very active because of need to fill; form -1 ions; 7 electrons in valence shell; tend to form salts with elements from groups 1A and 2A






37. 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






38. 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






39. States that if a stress is applied to a system at equilibrium - the system shifts in the direction that relieves the stress.






40. Set of spectral lines appearing in the UV region when a hydrogen atom undergoes a transition from energy levels n>1 to n=1.






41. The solubility of a gas in a liquid is directly proportional to the partial pressure of that gas on the surface of the liquid

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42. The tendency for an atom to attract electrons to itself when it is chemically combined with another element






43. One - half the distance between the nuclei of two atoms of the same element when the atoms are joined






44. The intermolecular force in which a hydrogen atom that is bonded to a highly electronegative atom is attracted to an unshared pair of electrons of an electronegative atom in a nearby molecule






45. The lowest allowable energy state of an atom






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






47. Small discrete increments of energy.






48. Specifies the specific orbital in which the electron is most likely to be found. - Third quantum number - designated as ml. Describes a particular orbital within a subshell where an electron is very likely to be found. Possible values are integers in






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






50. Sum of all the masses - in AMU - present in one molecule of a molecular compound.