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






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






3. Energy released when an atom or ion in the gaseous state gains an electron. Increases from left to right and from bottom to top on the Periodic Table.






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






5. 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.






6. 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.






7. The process of decomposing a chemical compound by the passage of an electric current.






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






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






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






11. Region in a molecule where atomic orbitals overlap - resulting in either a stable low - energy bonding orbital or an unstable high - energy antibonding orbital.






12. The maximum amount of product that can be produced from a given amount of reactant






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






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






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

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16. 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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17. 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.






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






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






20. 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






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






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






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






24. 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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25. 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






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






27. Attractions between molecules caused by the electron motion on one molecule affecting the electron motion on the other through electrical forces; these are the weakest interactions between molecules






28. 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






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






30. A set of spectral lines that appear in the visible light region when a hydrogen atom undergoes a transition from energy levels n>2 to n=2.






31. 2.18 x 10^-18 J/electron






32. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance






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






34. (chemistry) any theory in which all matter is composed of tiny discrete finite indivisible indestructible particles






35. 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






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






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






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






39. Small discrete increments of energy.






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






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






42. 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






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






44. An acid that will completely dissociate in aqueous solution - like HCl - HI - HClO4 HBr.






45. 5 different orbitals shaped like clover leaves and max electrons is 10






46. The point during a titration when the number of H+ ions and OH- ions are equal. This is at the middle of the steepest part of the titration curve.






47. Simplest whole # ration of atoms in a compound






48. The lowest allowable energy state of an atom






49. States that it is impossible to determine simultaneously both the position and momentum of an electron or any other particle






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