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






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






5. A subdivision of an energy level in an atom. They are divided into orbitals.






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






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






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






9. 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






10. 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.






11. Spectrum of certain absorbed wavelengths of light corresponding to an atom's spectrum of emitted frequencies of light. Unique to each element. AAS can be used to indentify an element.






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






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

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14. 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






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






16. An atom or group of atoms that has a positive or negative charge






17. 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






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






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






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






21. A solution in which water is the solvent






22. Structure that occurs when it is possible to draw two or more valid electron dot structures that have the same number of electron pairs for a molecule or ion






23. 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






24. Attractions between molecules caused by the electron motion on one molecule affecting the electron motion on the other through electrical forces; these are the weakest interactions between molecules






25. 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






26. Named after their cation and anion






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






28. 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






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






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






31. Halogens; ns2np5 - - 2nd most reactive group - The Halogens; very active because of need to fill; form -1 ions; 7 electrons in valence shell; tend to form salts with elements from groups 1A and 2A






32. E=hc/?






33. The center of the atom which contains the protons and neutrons; in cells - structure that contains the cell's genetic material (DNA) and controls the cell's activities






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






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






36. 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






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






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






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






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






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






43. An equilibrium expression used to measure weak - acid strength - given by the ratio of the product of the products' molar concentrations to the product of the reactants' molar concentrations - with each term raised to the power of its stoichiometric






44. 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






45. 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






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






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






48. The average distance between the nuclei of two bonded atoms






49. 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






50. A representation of a displacement reaction showing only the reactive species and omitting the spectator ions.






Can you answer 50 questions in 15 minutes?



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