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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. 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.






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






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






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






5. (chemistry) the sum of the relative atomic masses of the constituent atoms of a molecule






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






7. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance C>>>>A+B






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






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






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






11. Property of the elements that can be predicted from the arrangement of the periodic table






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






13. 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






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






15. Atoms react by gaining or losing electrons so as to acquire the stable electron structure of a noble gas - usually eight valence electrons






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






17. An ionic compound that resists changes in its pH






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






19. 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






20. 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






21. The percent by mass of each element in a compound






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






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






24. A reaction in which atoms of one element take the place of atoms of another element in a compound






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






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






27. 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.






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






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






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






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






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






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






34. Substance in which a solute is dissolved to form a solution






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






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






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






38. 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






39. 2.18 x 10^-18 J/electron






40. Chalcogens - - Oxide O






41. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds






42. 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






43. PH=pka+log[base/acid] Used in titration based problems that relates the pH or pOH of a solution to the pK and the ratio of the dissociated species.






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






45. 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






46. Process by which molecules tend to move from an area where they are more concentrated to an area where they are less concentrated






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






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






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






50. 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