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






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






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






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






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






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






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






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






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






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






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






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






13. Product of the molar concentrations of dissociated ions in solution at any point in the reaction other than equilibrium or saturation - where each ion is raised to the power of its stoichiometric coefficient. Denoted IP.






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






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






16. 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






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






18. 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






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






20. Sol - a chemical process in which solvent molecules and molecules or ions of the solute combine to form a compound






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






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






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






24. 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






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






26. A covalent bond in which the bonding electrons are shared equally by the bonded atoms - resulting in a balanced distribution of electrical charge






27. A model of acids and bases which an acid is hydrogen ion donor and base is a hydrogen ion acceptor.






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






29. When a solute is dissolved in a solvent - it will dissociate until reaching an equilibrium point at which the rate of dissociation equals the rate of precipitation of the solute - regardless of any additional solute introduced into the mixture






30. 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






31. 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






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






33. An emperimentally determined mathmatical expression showing the rate of a reaction as a function of the concentration of its reactants






34. 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






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






36. 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.






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






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






39. 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






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






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






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






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






44. 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.






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






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






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






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






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

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