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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. The quantum number that indicates the main energy level occupied by the electron. Can theoretically take on any positive interger. Denoted by the letter n.






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

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






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






5. 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.






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






7. 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






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






10. A horizontal row of elements in the periodic table






11. Property of the elements that can be predicted from the arrangement of the periodic table






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






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






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






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






16. 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






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






18. Process by which molecules tend to move from an area where they are more concentrated to an area where they are less concentrated






19. E=hc/?






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






21. An acid that will completely dissociate in aqueous solution - like HCl - HI - HClO4 HBr.






22. 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






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






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






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






26. Chalcogens - - Oxide O






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






28. 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.






29. Keq describes the ratio of product concentration to reactant concentration - with each raised to the power corresponding ot its coefficient ion in the balanced equation






30. A definite stable energy that a physical system can have






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






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






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






34. The formation of one or more covalent bonds between an electron pair donor and an electron pair acceptor






35. 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.






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






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






38. 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






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






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






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






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






43. 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






44. 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.






45. 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






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






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






48. 1913 - Niels Bohr - said that electrons formed specific layers instead or random ones - said atoms atoms absorb and give off energy when the electrons move from one shell to another






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






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