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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. E=hc/?






2. A set of frequencies of electromagnetic waves given off by atoms of an element; consists of a series of fine lines of individual colors






3. The lowest allowable energy state of an atom






4. 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






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






6. An atom or group of atoms that has a positive or negative charge






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. 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.






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






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






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






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






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






14. Simplest whole # ration of atoms in a compound






15. An element in an 'A' group in the periodic table; as a group these elements display a wide range of physical and chemical properties. In their atoms - the s and p sublevels in the highest occupied energy level are partially filled






16. Two or more atoms held together by covalent bonds






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






18. Large molecular structures - strong covalent bonding - share qualities of IONIC And COVALENT






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






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






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






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






23. Having characteristics of both an acid and a base and capable of reacting as either






24. 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






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






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






27. 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






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






29. Process by which molecules tend to move from an area where they are more concentrated to an area where they are less concentrated






30. 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.






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. A solution in which water is the solvent






33. A reaction where a compound does Not change its molecular structure.






34. The sum of the exponents in a rate law - where each exponent provides the reaction order with respect to its reactants






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






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






37. 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.






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






40. One - half the distance between the nuclei of two atoms of the same element when the atoms are joined






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






42. 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






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






44. Contains nonmetals - 7 valence electrons in it's outermost energy level. Very reactive






45. The formation of one or more covalent bonds between an electron pair donor and an electron pair acceptor






46. 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

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47. 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






48. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds






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






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






Can you answer 50 questions in 15 minutes?



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