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






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






3. 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






4. Chalcogens - - Oxide O






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






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






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






8. 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






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






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






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






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






14. 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






15. 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






16. 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






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






18. An element in an 'A' group in the periodic table; as a group these elements display a wide range of physical and chemical properties. In their atoms - the s and p sublevels in the highest occupied energy level are partially filled






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






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






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






22. 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






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






24. 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






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






26. The amount of a substance that contains as many particles as there are atoms in exactly 12g of carbon -12






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






28. 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






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






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






31. An atom - ion - or molecule that donates an electron pair to form a covalent bond.






32. 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.






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






34. An ionic compound that resists changes in its pH






35. Two or more atoms held together by covalent bonds






36. The weight in grams of compound that can be substituted by 1 atom of Hydrogen. GEW = MW / # of acidic Hyrdogens






37. A model of acids and bases which an acid is hydrogen ion donor and base is a hydrogen ion acceptor.






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






39. An atom - radical - or molecule that has gained or lost one or more electrons and has a negative or positive charge






40. A solid made up of particles that are not arranged in a regular pattern.






41. 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






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






43. 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






44. 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.






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






46. 5 different orbitals shaped like clover leaves and max electrons is 10






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






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






49. The solubility of a gas in a liquid is directly proportional to the partial pressure of that gas on the surface of the liquid

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