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






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






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






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






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






7. The molar amount of a solute that can dissolve in 1L of solvent until equilibrium - saturation - is reached






8. 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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9. 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






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






11. 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.






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






13. Two or more atoms held together by covalent bonds






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






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






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






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






20. A concentration unit of a solution expressed as moles of solute dissolved per liter of solution






21. A bond formed when two atomic orbitals combine to form a molecular orbital that is symmetrical around the axis connecting the two atomic nuclei






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






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

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






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






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






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






28. Energy released when an atom or ion in the gaseous state gains an electron. Increases from left to right and from bottom to top on the Periodic Table.






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






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






31. The ratio of the actual yield to the theoretical yield for a chemical reaction expressed as a percentage; a measure of the efficiency of a reaction






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






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






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






35. 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






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






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






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






39. 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






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






41. Charge assigned to an atom in a molecule or polyatmic ion - calculated by (# valence electrons) - (# 1/2 bonding electrons) - (# nonbonding electrons). Molecules containing atoms with lower formal charges tend to be more stable than those with higher






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






43. 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.






44. 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.






45. Named after their cation and anion






46. In a solution - the substance that dissolves in the solvent






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






48. 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






49. Specifies the specific orbital in which the electron is most likely to be found. - Third quantum number - designated as ml. Describes a particular orbital within a subshell where an electron is very likely to be found. Possible values are integers in






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