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






2. 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






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






4. The vapor pressure of solution is the product of the mole fraction of the solvent and the vapor pressure of the pure solvent. P_a=X_aP_total

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5. The sum of the exponents in a rate law - where each exponent provides the reaction order with respect to its reactants






6. An atom - ion - or molecule that donates an electron pair to form a covalent bond.






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






8. Property of the elements that can be predicted from the arrangement of the periodic table






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






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






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






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






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






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






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






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






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






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






19. When polar molecules orient themselves such that the positive region of one molecule is close to the negative region of another molecule.






20. 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






21. A representation of a displacement reaction showing only the reactive species and omitting the spectator ions.






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






23. A solution in which water is the solvent






24. 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.






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






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






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

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






30. Attractive and repulsive forces between molecules that are weaker than forces within molecules.






31. When a solute is dissolved in a solvent - it will dissociate until reaching an equilibrium point at which the rate of dissociation equals the rate of precipitation of the solute - regardless of any additional solute introduced into the mixture






32. 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






33. 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






34. Named after their cation and anion






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






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. 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.






38. 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






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






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






41. 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






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






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






44. A horizontal row of elements in the periodic table






45. A reaction where a compound does Not change its molecular structure.






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






47. Have three valance electrons. In certain instances - some elements will loose three electrons - but they will also share electrons with another element to attain stability.






48. 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.






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






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