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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. 5 valence electrons -3 ions - Nitride N






2. 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






3. 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.






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






5. Small discrete increments of energy.






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






7. An uncharged molecule with a single unpaitred electron in its outer ring - very unstable - exists for only about 10 seconds






8. 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-






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






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






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






13. 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.






14. The Percent by mass of each element in a compound.






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






16. 2.18 x 10^-18 J/electron






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






18. Chalcogens - - Oxide O






19. 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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20. Keq describes the ratio of product concentration to reactant concentration - with each raised to the power corresponding ot its coefficient ion in the balanced equation






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






22. 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






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






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






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






26. Named after their cation and anion






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






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






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






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






31. 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






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






33. 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






34. A measured amount of a solution of unknown concentration is added to a known volume of a second solution until the reaction between them is just complete






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






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






37. 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






38. 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






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






40. 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






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






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






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






44. When dipoles are dissolved in a solution where ions are present ions wil arrange themselves with the opposite charged end of the dipole.






45. 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






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






47. Simplest whole # ration of atoms in a compound






48. 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






49. 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.






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