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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. Halogens; ns2np5 - - 2nd most reactive group - The Halogens; very active because of need to fill; form -1 ions; 7 electrons in valence shell; tend to form salts with elements from groups 1A and 2A






2. Small discrete increments of energy.






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






4. 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.






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






6. A solution in which water is the solvent






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






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






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






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






11. 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.






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






13. Charge assigned to an atom in a molecule or polyatmic ion - calculated by (# valence electrons) - (# 1/2 bonding electrons) - (# nonbonding electrons). Molecules containing atoms with lower formal charges tend to be more stable than those with higher






14. An atom or group of atoms that has a positive or negative charge






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






16. Simplest whole # ration of atoms in a compound






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






18. 5 different orbitals shaped like clover leaves and max electrons is 10






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






20. 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.






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






22. 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






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






24. 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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25. A set of spectral lines that appear in the visible light region when a hydrogen atom undergoes a transition from energy levels n>2 to n=2.






26. 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






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






28. 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.






29. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds






30. E=hc/?






31. A chemical bond that involves sharing a pair of electrons between atoms in a molecule






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






33. 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






34. Have three valance electrons. In certain instances - some elements will loose three electrons - but they will also share electrons with another element to attain stability.






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






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






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






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






39. (chemistry) the sum of the relative atomic masses of the constituent atoms of a molecule






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






41. The amount of product that can be made in a chemical reaction based on the amount of limiting reactant






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






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






44. Any sample of a given compound will contain the same elements in the identical mass ratio.






45. A dynamic condition in which two opposing changes occur at equal rates in a closed system






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






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. Named after their cation and anion






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






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