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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 average distance between the nuclei of two bonded atoms






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






3. 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






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

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






6. 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






7. 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.






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






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






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






11. 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.






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






13. Tells you how much solute is present compared to the amount of solvent






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






15. 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.






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






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






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






20. E=hc/?






21. A naturally occurring or synthetic compound consisting of large molecules made up of a linked series of repeated simple monomers






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






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






24. The intermolecular force in which a hydrogen atom that is bonded to a highly electronegative atom is attracted to an unshared pair of electrons of an electronegative atom in a nearby molecule






25. Two or more atoms held together by covalent bonds






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






27. (chemistry) a series from actinium to lawrencium of 15 radioactive elements with increasing atomic numbers






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






29. Acids defined as electron - pair acceptors and bases as electron - pair donors.






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






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






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






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. 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






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






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






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






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






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






40. 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






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






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






43. 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.






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






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






46. 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.






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






48. Defined acids as subtsances that produced H ions in water - while bases produced OH ions. When they reacted together - H and OH neutralise to make water






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






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