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






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






3. Small discrete increments of energy.






4. The percent by mass of each element in a compound






5. The amount of a substance that contains as many particles as there are atoms in exactly 12g of carbon -12






6. Spectrum of certain absorbed wavelengths of light corresponding to an atom's spectrum of emitted frequencies of light. Unique to each element. AAS can be used to indentify an element.






7. 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.






8. Simplest whole # ration of atoms in a compound






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






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






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






12. 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.






13. 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






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






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






16. An ionic compound that resists changes in its pH






17. 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






18. 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






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






20. 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.






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






22. The weight in grams of one mole of a given elementand is expressedin tems of grams per mole.






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






24. 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.






25. 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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26. 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-






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






28. 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






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

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






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






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






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






34. Substance in which a solute is dissolved to form a solution






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






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






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






38. 5 valence electrons -3 ions - Nitride N






39. The average distance between the nuclei of two bonded atoms






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






41. 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






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






43. The pressure exerted by a vapor in equilibrium with its liquid or solid phase






44. A solution in which water is the solvent






45. 5 different orbitals shaped like clover leaves and max electrons is 10






46. 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






47. 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.






48. A naturally occurring or synthetic compound consisting of large molecules made up of a linked series of repeated simple monomers






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






50. 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