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






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






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






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






5. 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






6. 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






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






8. 1913 - Niels Bohr - said that electrons formed specific layers instead or random ones - said atoms atoms absorb and give off energy when the electrons move from one shell to another






9. 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






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






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






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






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






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






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






16. 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






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






18. Redox reaction - in which the same species is both oxidized and reduced.






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






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






22. 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






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






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






25. 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.






26. 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.






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






28. 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






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






30. 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






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






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






33. 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






34. Simplest whole # ration of atoms in a compound






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






36. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds






37. 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






38. 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






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






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






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






42. 2.18 x 10^-18 J/electron






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






44. The reaction of the ions that characterize acids and the ions that characterize bases to form water molecules and a salt






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






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






47. 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.






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






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






50. 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.