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






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






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






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






6. 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






7. A subatomic particle that has a positive charge and that is found in the nucleus of an atom Charge of +1 and mass of 1.0073 amu






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






9. 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.






10. 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.






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






12. A solution in which water is the solvent






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. Resulting positive nuclear charge an outer electron senses after accounting for the shielding effect of inner core electrons. Abbreviated as Z(eff). Increases from left to right - and bottom to top on the Periodic Table.






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






16. 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






17. The sum of the exponents in a rate law - where each exponent provides the reaction order with respect to its reactants






18. 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






19. 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






20. The Percent by mass of each element in a compound.






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






22. When dipoles are dissolved in a solution where ions are present ions wil arrange themselves with the opposite charged end of the dipole.






23. 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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24. A definite stable energy that a physical system can have






25. 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






26. E=hc/?






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






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






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






30. The percent by mass of each element in a compound






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






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






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






34. 5 valence electrons -3 ions - Nitride N






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






36. PH=pka+log[base/acid] Used in titration based problems that relates the pH or pOH of a solution to the pK and the ratio of the dissociated species.






37. Two or more atoms held together by covalent bonds






38. 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.






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






40. 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.






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






42. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance C>>>>A+B






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






44. 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






45. 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






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






47. (chemistry) the sum of the relative atomic masses of the constituent atoms of a molecule






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






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






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.