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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. Small discrete increments of energy.






2. Simplest whole # ration of atoms in a compound






3. 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.






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






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






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






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






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






9. 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






10. An ionic compound that resists changes in its pH






11. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds






12. Large molecular structures - strong covalent bonding - share qualities of IONIC And COVALENT






13. The process by which one or more substances change to produce one or more different substances






14. 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






15. The lowest allowable energy state of an atom






16. Solids in which the particles are arranged in a repeating - 3- D pattern - has a specific melting point - classified as ionic network covalent - metallic or molecular.






17. 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






18. 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-






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






20. A horizontal row of elements in the periodic table






21. The number of atoms in exactly 12 g of pure 12c and equal to 6.022 x 10^23 is called






22. The formation of one or more covalent bonds between an electron pair donor and an electron pair acceptor






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






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






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






26. 2.18 x 10^-18 J/electron






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






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






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






31. 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






32. Second quantum number - designated by the letter 'l.' This 'angular momentum' refers to the subshells within each principle quantum energy level. It can take on the value of an integer in the 0 to (n -1) range. The four subshellscorresponding to l=0






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






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






35. 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






36. Chalcogens - - Oxide O






37. 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






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






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






40. 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






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






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






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






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






46. 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.






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






48. A pair of equal and opposite electric charges or magnetic poles separated by a small distance






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






Can you answer 50 questions in 15 minutes?



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