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






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






3. A solid made up of particles that are not arranged in a regular pattern.






4. The weight in grams of compound that can be substituted by 1 atom of Hydrogen. GEW = MW / # of acidic Hyrdogens






5. 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






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






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






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






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






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






11. 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






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






14. 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






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






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






17. 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






18. 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.






19. 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






20. A horizontal row of elements in the periodic table






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






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






23. Elements in the middle of the periodic table - in groups 3-12.






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






25. 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.






26. 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






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






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






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






30. 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






31. 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.






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






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






34. Chalcogens - - Oxide O






35. 5 valence electrons -3 ions - Nitride N






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






37. 2.18 x 10^-18 J/electron






38. 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.






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






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






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






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






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






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






45. Structure that occurs when it is possible to draw two or more valid electron dot structures that have the same number of electron pairs for a molecule or ion






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






48. The lowest allowable energy state of an atom






49. 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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50. 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