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






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






3. 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






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






5. The solubility of a gas in a liquid is directly proportional to the partial pressure of that gas on the surface of the liquid

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






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






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. 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






10. 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.






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






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






13. Have the shape of a sphere - with the center of the sphere at the nucleus; completely symmetrical along all axes; 1s orbital is spherically symmetric and has no nodes; 2s orbital is also spherical but contains a node and is higher in energy






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






16. 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






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






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






19. A horizontal row of elements in the periodic table






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






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






22. Having characteristics of both an acid and a base and capable of reacting as either






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






24. The molar solubility of one salt is reduced when another salt - having a common ion is brought into the same solution






25. 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






26. 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






27. 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






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






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






30. 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






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






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






33. An acid that will completely dissociate in aqueous solution - like HCl - HI - HClO4 HBr.






34. The pressure exerted by a vapor in equilibrium with its liquid or solid phase






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






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






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






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






40. 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






41. Small discrete increments of energy.






42. The slowest elementary step which is the limit for the rate of the other steps






43. 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






44. In a solution - the substance that dissolves in the solvent






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






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






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






48. The lowest allowable energy state of an atom






49. 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






50. 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.