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






2. 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.






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






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






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






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






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






8. 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






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






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






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






12. 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






13. 2.18 x 10^-18 J/electron






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






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






16. A horizontal row of elements in the periodic table






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






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






19. 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.






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






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






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






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






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






25. The lowest allowable energy state of an atom






26. Small discrete increments of energy.






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






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






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






32. 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






33. Named after their cation and anion






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






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






36. A covalent bond in which the bonding electrons are shared equally by the bonded atoms - resulting in a balanced distribution of electrical charge






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






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






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






40. 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






41. Simplest whole # ration of atoms in a compound






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

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






45. The energy required to remove an electron from a gaseous atom; generally increases in moving from left - to - right across a period and decreases in moving down a group






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






47. 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






48. 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






49. 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






50. 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







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