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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. The center of the atom which contains the protons and neutrons; in cells - structure that contains the cell's genetic material (DNA) and controls the cell's activities






2. The energy required to remove an electron from a gaseous atom; generally increases in moving from left - to - right across a period and decreases in moving down a group






3. Sol - a chemical process in which solvent molecules and molecules or ions of the solute combine to form a compound






4. Two or more atoms held together by covalent bonds






5. Nh/2p The angular momentum changes only in discete amounts with respect to the quantum number. Also E=- R_h/n^2






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






7. A pair of equal and opposite electric charges or magnetic poles separated by a small distance






8. Named after their cation and anion






9. The reaction of the ions that characterize acids and the ions that characterize bases to form water molecules and a salt






10. The molar solubility of one salt is reduced when another salt - having a common ion is brought into the same solution






11. The pressure exerted by a vapor in equilibrium with its liquid or solid phase






12. The lowest allowable energy state of an atom






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






14. A reaction in which two or more substances combine to form a single substance A+B>>>>>>>C






15. An ionic compound that resists changes in its pH






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






17. An atom - radical - or molecule that has gained or lost one or more electrons and has a negative or positive charge






18. An emperimentally determined mathmatical expression showing the rate of a reaction as a function of the concentration of its reactants






19. A reaction where a compound does Not change its molecular structure.






20. Standard Temperature and Pressure. 273 Kelvin (0 Celsius) - 1 atmosphere (760 torr - 760 kPA).






21. Systematic pairing of a deprotonated species (base) with its protonated form (conjugate acid). Conjugates appear on opposite sides of a chemical equation.






22. The amount of product that can be made in a chemical reaction based on the amount of limiting reactant






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






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






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






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






27. (chemistry) a substance formed by chemical union of two or more elements or ingredients in definite proportion by weight






28. Large molecular structures - strong covalent bonding - share qualities of IONIC And COVALENT






29. A structural formula in which electrons are represented by dots; dot pairs or dashes between two atomic symbols represent pairs in covalent bonds.






30. 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






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






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






33. The hypothetical equation showing only the species that is oxidized or reduced in a redox reaction and the correct number of electrons transferred between the species in the complete - balanced equation.






34. 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






35. 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.






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






37. 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.






38. Having characteristics of both an acid and a base and capable of reacting as either






39. The percent by mass of each element in a compound






40. PH of a molecule at which it contains no net electric charge - isoelectric point.






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

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






43. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance C>>>>A+B






44. A set of spectral lines that appear in the visible light region when a hydrogen atom undergoes a transition from energy levels n>2 to n=2.






45. The point on a phase diagram that represents the only set of conditions at which all three phases exist in equilibrium with one another






46. The ratio of the actual yield to the theoretical yield for a chemical reaction expressed as a percentage; a measure of the efficiency of a reaction






47. Have the shape of a sphere - with the center of the sphere at the nucleus; completely symmetrical along all axes; 1s orbital is spherically symmetric and has no nodes; 2s orbital is also spherical but contains a node and is higher in energy






48. PH=pka+log[base/acid] Used in titration based problems that relates the pH or pOH of a solution to the pK and the ratio of the dissociated species.






49. 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






50. 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