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






2. Small discrete increments of energy.






3. 5 different orbitals shaped like clover leaves and max electrons is 10






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






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






6. Solids in which the particles are arranged in a repeating - 3- D pattern - has a specific melting point - classified as ionic network covalent - metallic or molecular.






7. 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-






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






9. Elements in the middle of the periodic table - in groups 3-12.






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






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






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






13. 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.






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






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






16. 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






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






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






19. A solution in which water is the solvent






20. 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






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






22. At a constant pressure - the volume of an ideal gas is directly proportinal to its temperature: V (a) T

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






24. A graph of pressure versus temperature that shows the conditions under which the phases of a substance exist






25. 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






26. Process by which molecules tend to move from an area where they are more concentrated to an area where they are less concentrated






27. 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






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






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






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






31. 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.






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






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






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. 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






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






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






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






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






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






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






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






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






44. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds






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






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






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






48. The ratio of the actual yield to the theoretical yield for a chemical reaction expressed as a percentage; a measure of the efficiency of a reaction






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






50. 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