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MCAT Chemistry

Subjects : mcat, science
Instructions:
  • Answer 50 questions in 15 minutes.
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  • Match each statement with the correct term.
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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. Substance in which a solute is dissolved to form a solution






2. An element in an 'A' group in the periodic table; as a group these elements display a wide range of physical and chemical properties. In their atoms - the s and p sublevels in the highest occupied energy level are partially filled






3. 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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4. In a solution - the substance that dissolves in the solvent






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






6. 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






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






8. A base that can accept two moles of H+ per mole of itself (ex: SO4






9. Product of the molar concentrations of dissociated ions in solution at any point in the reaction other than equilibrium or saturation - where each ion is raised to the power of its stoichiometric coefficient. Denoted IP.






10. A horizontal row of elements in the periodic table






11. The quantum number that has only two possible values - +1/2 and -1/2 - which indicate the two fundamental spin states of an electron in an orbital






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






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






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






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






16. 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






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






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






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






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






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






22. 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






23. 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






24. E=hc/?






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






26. 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.






27. 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






28. Resulting positive nuclear charge an outer electron senses after accounting for the shielding effect of inner core electrons. Abbreviated as Z(eff). Increases from left to right - and bottom to top on the Periodic Table.






29. No two electrons or protons or neutrons in a given system can be in states characterized by the same set of quantum numbers






30. 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.






31. Expression of auto - ionization of water into H+ and OH- at a certain temperature - given by the product of the ions' molar concentrations. Denoted by Kw and equal to 10-






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






33. A reaction in which atoms of one element take the place of atoms of another element in a compound






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






35. Slightly less reactive than alkali metals - comprise group II






36. 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






37. An ionic compound that resists changes in its pH






38. States that it is impossible to determine simultaneously both the position and momentum of an electron or any other particle






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






40. 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.






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






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






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






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






45. 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.






46. When dipoles are dissolved in a solution where ions are present ions wil arrange themselves with the opposite charged end of the dipole.






47. (chemistry) any theory in which all matter is composed of tiny discrete finite indivisible indestructible particles






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






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






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