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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 definite stable energy that a physical system can have






2. The solubility of a gas in a liquid is directly proportional to the partial pressure of that gas on the surface of the liquid

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3. 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






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






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






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






7. The center of the atom which contains the protons and neutrons; in cells - structure that contains the cell's genetic material (DNA) and controls the cell's activities






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






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






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






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






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






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






14. 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






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






16. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance






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






18. Valence Shell Electron Pair Repulsion theory - stating that the three - dimensional molecular geometry about some central atom is determined by the elctronic repulsion between its bonding and nonbonding electron pairs.






19. A bond formed when two atomic orbitals combine to form a molecular orbital that is symmetrical around the axis connecting the two atomic nuclei






20. 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






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






22. 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






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






24. 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.






25. 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






26. (chemistry) any theory in which all matter is composed of tiny discrete finite indivisible indestructible particles






27. 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.






28. 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.






29. 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.






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






31. 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






32. 2.18 x 10^-18 J/electron






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






34. A model of acids and bases which an acid is hydrogen ion donor and base is a hydrogen ion acceptor.






35. 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






36. 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






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






38. No two electrons or protons or neutrons in a given system can be in states characterized by the same set of quantum numbers






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






40. An atom - radical - or molecule that has gained or lost one or more electrons and has a negative or positive charge






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






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






44. 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






45. Mixture of 2 or more substances that distills at a constant temperature and with constant composition - even though seperately the components have different boiling points






46. 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.






47. 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






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






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