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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. The formation of one or more covalent bonds between an electron pair donor and an electron pair acceptor






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






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






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






5. 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






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






7. 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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8. 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






9. 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.






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






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






12. (chemistry) any theory in which all matter is composed of tiny discrete finite indivisible indestructible particles






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






14. 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.






15. Tells you how much solute is present compared to the amount of solvent






16. 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






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






18. 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.






19. 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-






20. Temperature is constant; effusion and temperature are proportional to the square root of their masses

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






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






23. 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






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






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






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






27. 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.






28. Simplest whole # ration of atoms in a compound






29. 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.






30. The tendency for an atom to attract electrons to itself when it is chemically combined with another element






31. (chemistry) a series from actinium to lawrencium of 15 radioactive elements with increasing atomic numbers






32. Two or more atoms held together by covalent bonds






33. (chemistry) p(otential of) H(ydrogen)






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






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






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






37. When polar molecules orient themselves such that the positive region of one molecule is close to the negative region of another molecule.






38. 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






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






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






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






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






43. 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






44. 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.






45. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds






46. 2.18 x 10^-18 J/electron






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






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






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






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







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