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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. A horizontal row of elements in the periodic table






2. The lowest allowable energy state of an atom






3. 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






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






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






6. 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






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






8. E=hc/?






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






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






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






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






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






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






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






16. A definite stable energy that a physical system can have






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






18. In a solution - the substance that dissolves in the solvent






19. 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






20. An ionic compound that resists changes in its pH






21. Named after their cation and anion






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






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






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






25. The ways in which electrons are arranged in various orbitals around the nuclei of atoms






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






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






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






29. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds






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






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






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






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






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






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






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






37. 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


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






39. 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.






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






41. An atom - radical - or molecule that has gained or lost one or more electrons and has a negative or positive charge






42. The quantum number that indicates the main energy level occupied by the electron. Can theoretically take on any positive interger. Denoted by the letter n.






43. 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.






44. Small discrete increments of energy.






45. A solution in which water is the solvent






46. 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






47. The solubility of a gas in a liquid is directly proportional to the partial pressure of that gas on the surface of the liquid


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






49. 5 valence electrons -3 ions - Nitride N






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