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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. Property of the elements that can be predicted from the arrangement of the periodic table






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






3. A representation of a displacement reaction showing only the reactive species and omitting the spectator ions.






4. The area of chemistry that is concerned with reaction rates and reaction mechanisms






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






6. Alkali metals: highly reactive - therefore always compounds. - 1 valence electron +1 ion - Hydrogen H? - Lithium Li? - Sodium Na? - Potassium K? - Rubidium Rb? - Cesium Cs?






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






8. 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






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






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






11. 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






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






13. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds






14. 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






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






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






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






18. 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.






19. 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






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






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






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






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






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






25. 5 valence electrons -3 ions - Nitride N






26. 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.






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






28. 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






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






30. A reaction in which two or more substances combine to form a single substance A+B>>>>>>>C






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






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






33. The point on a phase diagram that represents the only set of conditions at which all three phases exist in equilibrium with one another






34. 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






35. Chalcogens - - Oxide O






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






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






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






39. 2.18 x 10^-18 J/electron






40. 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






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






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






43. 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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44. 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.






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






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






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






49. A horizontal row of elements in the periodic table






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