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






2. 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






3. When dipoles are dissolved in a solution where ions are present ions wil arrange themselves with the opposite charged end of the dipole.






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






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






6. States that it is impossible to determine simultaneously both the position and momentum of an electron or any other particle






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






8. Named after their cation and anion






9. 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






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






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






12. 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






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






14. 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






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






16. Alkaline Earth Metals - 2 valence electrons +2 ions - Magnesium Mg






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






18. Nh/2p The angular momentum changes only in discete amounts with respect to the quantum number. Also E=- R_h/n^2






19. Product of the molar concentrations of dissociated ions in solution at saturation - where each ion is raised to the power of its stoichiometric coefficient. Denoted Ksp.






20. Chalcogens - - Oxide O






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






22. 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.






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






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






25. 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






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






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






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






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






30. Side - to side parallel orbitals overlap to share electrons - the 2nd/3rd covalent bond between two atoms - cannot rotate and maintain the bond.






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






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






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






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






35. One - half of the distance between the center of identical atoms that are not bonded together. Since effective nuclear charge increases when moving from left to right each additional electron is pulled more strogly toward the nucleus.






36. The slowest elementary step which is the limit for the rate of the other steps






37. 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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38. 2.18 x 10^-18 J/electron






39. 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






40. E=hc/?






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






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






43. The ratio of the number of moles of solute dissolved in one kilogram of solvent. molality (M = moles solute/kg of solution)






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






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






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






47. 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.






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






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






50. A horizontal row of elements in the periodic table