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






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






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






4. 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






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






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






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






9. 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.






10. The process by which a gas escapes from one container to another at lower pressure through a tiny hole in the container.






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






12. Sol - a chemical process in which solvent molecules and molecules or ions of the solute combine to form a compound






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






14. 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.






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






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

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






18. 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






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






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






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






22. A model of acids and bases which an acid is hydrogen ion donor and base is a hydrogen ion acceptor.






23. 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






24. Theory stating that the rate of a reaction is directly proportional to the number of collisions that take place between reactants per second.






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






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






27. 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.






28. 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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29. In a solution - the substance that dissolves in the solvent






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






31. Named after their cation and anion






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






33. An equilibrium expression used to measure weak - acid strength - given by the ratio of the product of the products' molar concentrations to the product of the reactants' molar concentrations - with each term raised to the power of its stoichiometric






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






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






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






37. Temperature is constant; effusion and temperature are proportional to the square root of their masses

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38. States that if a stress is applied to a system at equilibrium - the system shifts in the direction that relieves the stress.






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






40. The lowest allowable energy state of an atom






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






42. 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






43. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance C>>>>A+B






44. 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






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






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






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






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






49. A dynamic condition in which two opposing changes occur at equal rates in a closed system






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