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






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






3. 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






4. Contains nonmetals that are non - reactive. Full outermost energy level except helium which has 2.






5. 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






6. 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






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






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






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






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






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






12. A fundamental constant - h - that relates the energy of light quanta to their frequency: h = 6.6 X 10^-34 joule

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13. 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.






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






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






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

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






19. (chemistry) a substance formed by chemical union of two or more elements or ingredients in definite proportion by weight






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






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






22. Sol - a chemical process in which solvent molecules and molecules or ions of the solute combine to form a compound






23. 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






24. A chemical bond that involves sharing a pair of electrons between atoms in a molecule






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






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






27. Chalcogens - - Oxide O






28. 5 valence electrons -3 ions - Nitride N






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






30. 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






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






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






33. 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.






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






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






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






37. 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.






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






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






40. 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.






41. Two or more atoms held together by covalent bonds






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






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






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






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






46. A bond formed when two atomic orbitals combine to form a molecular orbital that is symmetrical around the axis connecting the two atomic nuclei






47. The point on a phase diagram that represents the only set of conditions at which all three phases exist in equilibrium with one another






48. 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.






49. 5 different orbitals shaped like clover leaves and max electrons is 10






50. Named after their cation and anion