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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. A set of frequencies of electromagnetic waves given off by atoms of an element; consists of a series of fine lines of individual colors






2. 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






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






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






5. 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






6. Second quantum number - designated by the letter 'l.' This 'angular momentum' refers to the subshells within each principle quantum energy level. It can take on the value of an integer in the 0 to (n -1) range. The four subshellscorresponding to l=0






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






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






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






10. 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






11. 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.






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






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






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






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






16. 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






17. Simplest whole # ration of atoms in a compound






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






19. A structural formula in which electrons are represented by dots; dot pairs or dashes between two atomic symbols represent pairs in covalent bonds.






20. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance C>>>>A+B






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






22. Expression of auto - ionization of water into H+ and OH- at a certain temperature - given by the product of the ions' molar concentrations. Denoted by Kw and equal to 10-






23. Acids defined as electron - pair acceptors and bases as electron - pair donors.






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






25. The reaction of the ions that characterize acids and the ions that characterize bases to form water molecules and a salt






26. 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






27. Small discrete increments of energy.






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






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






30. 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






31. 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






32. The hypothetical equation showing only the species that is oxidized or reduced in a redox reaction and the correct number of electrons transferred between the species in the complete - balanced equation.






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






34. 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






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






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






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






38. Attractive and repulsive forces between molecules that are weaker than forces within molecules.






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






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






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






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






43. Keq describes the ratio of product concentration to reactant concentration - with each raised to the power corresponding ot its coefficient ion in the balanced equation






44. 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






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






46. 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






47. Standard Temperature and Pressure. 273 Kelvin (0 Celsius) - 1 atmosphere (760 torr - 760 kPA).






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






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






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







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