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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. 2.18 x 10^-18 J/electron






2. 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






3. 5 different orbitals shaped like clover leaves and max electrons is 10






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






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






6. Small discrete increments of energy.






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






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






10. Expression of auto - ionization of water into H+ and OH- at a certain temperature - given by the product of the ions' molar concentrations. Denoted by Kw and equal to 10-






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






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






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






14. 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






15. Slightly less reactive than alkali metals - comprise group II






16. An ionic compound that resists changes in its pH






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






18. Set of spectral lines appearing in the UV region when a hydrogen atom undergoes a transition from energy levels n>1 to n=1.






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






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






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






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






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. An elementary particle with 0 charge and mass about equal to a proton






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






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






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






28. A graph of pressure versus temperature that shows the conditions under which the phases of a substance exist






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






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






31. 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






32. Simplest whole # ration of atoms in a compound






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






34. 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.






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






36. 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






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






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






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

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






41. Alkali metals: highly reactive - therefore always compounds. - 1 valence electron +1 ion - Hydrogen H? - Lithium Li? - Sodium Na? - Potassium K? - Rubidium Rb? - Cesium Cs?






42. 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






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






44. A reaction in which two or more substances combine to form a single substance A+B>>>>>>>C






45. 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






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






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






48. No two electrons or protons or neutrons in a given system can be in states characterized by the same set of quantum numbers






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






50. 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