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






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






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






4. Two or more atoms held together by covalent bonds






5. A reaction where a compound does Not change its molecular structure.






6. 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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7. Slightly less reactive than alkali metals - comprise group II






8. The process by which one or more substances change to produce one or more different substances






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






10. A substance that - when dissolved in water - results in a solution that can conduct electricity






11. 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






12. 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.






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






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






15. 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






16. A physical property of a solution that depends on the number - but not the identity - of the disswolved solute particles; example properties include vapor pressure lowering - boiling point elevation - osmotic pressure - and frezzing point depression






17. 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






18. 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






19. 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.






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






21. Energy released when an atom or ion in the gaseous state gains an electron. Increases from left to right and from bottom to top on the Periodic Table.






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






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






24. 5 valence electrons -3 ions - Nitride N






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






26. The maximum amount of product that can be produced from a given amount of reactant






27. 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






28. 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.






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






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






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






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






33. The vapor pressure of solution is the product of the mole fraction of the solvent and the vapor pressure of the pure solvent. P_a=X_aP_total

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






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






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






37. Chalcogens - - Oxide O






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






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






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






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






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






43. 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






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






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






46. Elements in the middle of the periodic table - in groups 3-12.






47. 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






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






49. 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






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