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MCAT Chemistry

Subjects : mcat, science
Instructions:
  • Answer 50 questions in 15 minutes.
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  • Match each statement with the correct term.
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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) p(otential of) H(ydrogen)






2. Play- by- play showing the individual steps of a reaction - including the formation and destruction of any reaction intermediates that may occur.






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






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






5. The lowest allowable energy state of an atom






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






7. 5 valence electrons -3 ions - Nitride N






8. Sum of the protons and neutrons in an element often denoted by the letter A






9. 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






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






11. Product of the molar concentrations of dissociated ions in solution at any point in the reaction other than equilibrium or saturation - where each ion is raised to the power of its stoichiometric coefficient. Denoted IP.






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






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






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






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






16. Redox reaction - in which the same species is both oxidized and reduced.






17. 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.






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






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






20. 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






21. 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






22. The molar solubility of one salt is reduced when another salt - having a common ion is brought into the same solution






23. 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.






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






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






26. Simplest whole # ration of atoms in a compound






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






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






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






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






31. 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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32. Specifies the specific orbital in which the electron is most likely to be found. - Third quantum number - designated as ml. Describes a particular orbital within a subshell where an electron is very likely to be found. Possible values are integers in






33. At a constant pressure - the volume of an ideal gas is directly proportinal to its temperature: V (a) T

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






35. 1913 - Niels Bohr - said that electrons formed specific layers instead or random ones - said atoms atoms absorb and give off energy when the electrons move from one shell to another






36. The reaction of the ions that characterize acids and the ions that characterize bases to form water molecules and a salt






37. 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






38. 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






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






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






41. 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






42. 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-






43. An ionic compound that resists changes in its pH






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






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






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






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






48. When polar molecules orient themselves such that the positive region of one molecule is close to the negative region of another molecule.






49. Systematic pairing of a deprotonated species (base) with its protonated form (conjugate acid). Conjugates appear on opposite sides of a chemical equation.






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