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






2. 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






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






4. Where half of the acid is neutralized by the base on a titration curveAn acid dissociation constant - Ka - (also known as acidity constant - or acid - ionization constant) is a quantitative measure of the strength of an acid in solution. It is the eq






5. Solids in which the particles are arranged in a repeating - 3- D pattern - has a specific melting point - classified as ionic network covalent - metallic or molecular.






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






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






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






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






10. A concentration unit of a solution expressed as moles of solute dissolved per liter of solution






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






12. 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






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






14. The slowest elementary step which is the limit for the rate of the other steps






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






17. 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






18. Named after their cation and anion






19. The hypothetical equation showing only the species that is oxidized or reduced in a redox reaction and the correct number of electrons transferred between the species in the complete - balanced equation.






20. 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






21. The point on a phase diagram that represents the only set of conditions at which all three phases exist in equilibrium with one another






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






23. 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.






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






25. An equilibrium expression used to measure weak - acid strength - given by the ratio of the product of the products' molar concentrations to the product of the reactants' molar concentrations - with each term raised to the power of its stoichiometric






26. (physics) the smallest discrete quantity of some physical property that a system can possess (according to quantum theory) E=hf






27. 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.






28. 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.






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






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






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






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






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






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






35. 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






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






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






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






40. Product of the molar concentrations of dissociated ions in solution at saturation - where each ion is raised to the power of its stoichiometric coefficient. Denoted Ksp.






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






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






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






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






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






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






47. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds






48. 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






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






50. 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