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






2. An element in an 'A' group in the periodic table; as a group these elements display a wide range of physical and chemical properties. In their atoms - the s and p sublevels in the highest occupied energy level are partially filled






3. 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.






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






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






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






7. The tendency for an atom to attract electrons to itself when it is chemically combined with another element






8. 5 valence electrons -3 ions - Nitride N






9. Numbers that specify the properties of atomic orbitals and of their electrons






10. 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






11. 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.






12. An ionic compound that resists changes in its pH






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






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






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






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






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






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






19. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds






20. The weak attractive forces between molecules resulting from the small - instantaneous dipoles that occur because of the varying positions of the electrons during their motion about nuclei






21. (physics) the smallest discrete quantity of some physical property that a system can possess (according to quantum theory) E=hf






22. Where half of the acid is neutralized by the base on a titration curveAn acid dissociation constant - Ka - (also known as acidity constant - or acid - ionization constant) is a quantitative measure of the strength of an acid in solution. It is the eq






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






24. 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






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






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






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






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






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






30. 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






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






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






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






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






35. 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.






36. 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






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






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






39. 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.






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






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






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. 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






44. E=hc/?






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






46. A chemical formula showing the ratio of elements in a compound rather than the total number of atoms






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






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






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






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