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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 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






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






3. 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






4. 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






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






6. Expression of auto - ionization of water into H+ and OH- at a certain temperature - given by the product of the ions' molar concentrations. Denoted by Kw and equal to 10-






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






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






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






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


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






12. Have three valance electrons. In certain instances - some elements will loose three electrons - but they will also share electrons with another element to attain stability.






13. 5 valence electrons -3 ions - Nitride N






14. 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.






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






16. The process by which one or more substances change to produce one or more different substances






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






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






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






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






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






22. E=hc/?






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






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






25. 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.






26. 2.18 x 10^-18 J/electron






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






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






29. 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.






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






31. Side - to side parallel orbitals overlap to share electrons - the 2nd/3rd covalent bond between two atoms - cannot rotate and maintain the bond.






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






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






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






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






36. 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






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


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






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






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






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






42. 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






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






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






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






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






47. A fundamental constant - h - that relates the energy of light quanta to their frequency: h = 6.6 X 10^-34 joule


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






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






50. The nuclear charge experienced by the outermost electrons of an atom (actual charge minus the shielding caused by inner shells: Z- eff)