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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. 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






2. An ionic compound that resists changes in its pH






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






4. Valence Shell Electron Pair Repulsion theory - stating that the three - dimensional molecular geometry about some central atom is determined by the elctronic repulsion between its bonding and nonbonding electron pairs.






5. A pair of equal and opposite electric charges or magnetic poles separated by a small distance






6. One - half of the distance between the center of identical atoms that are not bonded together. Since effective nuclear charge increases when moving from left to right each additional electron is pulled more strogly toward the nucleus.






7. 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






8. A bond formed when two atomic orbitals combine to form a molecular orbital that is symmetrical around the axis connecting the two atomic nuclei






9. Orbitals of equal energy are each occupied by one electron before any orbital is occupied by a second electron - and all electrons in singly occupied orbitals must have the same spin

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10. 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






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






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






13. Attractions between molecules caused by the electron motion on one molecule affecting the electron motion on the other through electrical forces; these are the weakest interactions between molecules






14. 1913 - Niels Bohr - said that electrons formed specific layers instead or random ones - said atoms atoms absorb and give off energy when the electrons move from one shell to another






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






16. 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






17. A base that can accept two moles of H+ per mole of itself (ex: SO4






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






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






21. 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






22. The lowest allowable energy state of an atom






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






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






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






26. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds






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






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






29. 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






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






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






32. 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






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






34. 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






35. 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






36. Spectrum of certain absorbed wavelengths of light corresponding to an atom's spectrum of emitted frequencies of light. Unique to each element. AAS can be used to indentify an element.






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






38. 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.






39. 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.






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






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






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






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






44. 2.18 x 10^-18 J/electron






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






46. A horizontal row of elements in the periodic table






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






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






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






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