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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. 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






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






3. A dynamic condition in which two opposing changes occur at equal rates in a closed system






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






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






6. 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.






7. Alkali metals: highly reactive - therefore always compounds. - 1 valence electron +1 ion - Hydrogen H? - Lithium Li? - Sodium Na? - Potassium K? - Rubidium Rb? - Cesium Cs?






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






9. 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.






10. Defined acids as subtsances that produced H ions in water - while bases produced OH ions. When they reacted together - H and OH neutralise to make water






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






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






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






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






15. An uncharged molecule with a single unpaitred electron in its outer ring - very unstable - exists for only about 10 seconds






16. 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






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






18. 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.






19. Orbitals of equal energy are each occupied by one electron before any orbital is occupied by a second electron - and all electrons in singly occupied orbitals must have the same spin

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20. A measured amount of a solution of unknown concentration is added to a known volume of a second solution until the reaction between them is just complete






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

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22. A representation of a displacement reaction showing only the reactive species and omitting the spectator ions.






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






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






25. 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






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






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






28. 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






29. 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






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






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. A substance that - when dissolved in water - results in a solution that can conduct electricity






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






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






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






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






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






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






39. 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






40. The maximum amount of product that can be produced from a given amount of reactant






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






42. 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






43. A covalent bond in which the bonding electrons are shared equally by the bonded atoms - resulting in a balanced distribution of electrical charge






44. An ionic compound that resists changes in its pH






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






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






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






49. The molar amount of a solute that can dissolve in 1L of solvent until equilibrium - saturation - is reached






50. Rare earth element group (elements 58-71)