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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 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






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






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






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






5. 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


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






7. 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.






8. 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.






9. Chalcogens - - Oxide O






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






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






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






14. An ionic compound that resists changes in its pH






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






16. 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


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






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






19. 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.






20. 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






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






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






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






24. (chemistry) a substance that changes color to indicate the presence of some ion or substance






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






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






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






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






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






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






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






32. The ways in which electrons are arranged in various orbitals around the nuclei of atoms






33. Simplest whole # ration of atoms in a compound






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






35. The weight in grams of compound that can be substituted by 1 atom of Hydrogen. GEW = MW / # of acidic Hyrdogens






36. Atoms react by gaining or losing electrons so as to acquire the stable electron structure of a noble gas - usually eight valence electrons






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






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






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






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






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






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






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






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






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






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






48. Second quantum number - designated by the letter 'l.' This 'angular momentum' refers to the subshells within each principle quantum energy level. It can take on the value of an integer in the 0 to (n -1) range. The four subshellscorresponding to l=0






49. 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






50. 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