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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.
  • 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 chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.






2. 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






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






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






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






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






7. The lowest allowable energy state of an atom






8. 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






9. The Percent by mass of each element in a compound.






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






11. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds






12. 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






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






15. An atom - ion - or molecule that donates an electron pair to form a covalent bond.






16. An elementary particle with 0 charge and mass about equal to a proton






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

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






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






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

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21. 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






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






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






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






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






26. 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






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






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






29. 2.18 x 10^-18 J/electron






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






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






32. 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






33. 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






34. The vapor pressure of solution is the product of the mole fraction of the solvent and the vapor pressure of the pure solvent. P_a=X_aP_total

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






36. 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






37. Gram equivalent weight of solute per liter of solution - often denoted by N.






38. 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.






39. 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






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






41. 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






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






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






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






45. 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.






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






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






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






49. 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






50. Alkaline Earth Metals - 2 valence electrons +2 ions - Magnesium Mg