Test your basic knowledge |

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 solid made up of particles that are not arranged in a regular pattern.






2. 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






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






4. 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






5. 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.






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






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






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






9. 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.






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






11. 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






12. A horizontal row of elements in the periodic table






13. 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






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






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






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






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






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






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


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






21. An ionic compound that resists changes in its pH






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






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






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






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






26. Theory stating that the rate of a reaction is directly proportional to the number of collisions that take place between reactants per second.






27. A dynamic condition in which two opposing changes occur at equal rates in a closed system






28. 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






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






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






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






32. The lowest allowable energy state of an atom






33. Specifies the specific orbital in which the electron is most likely to be found. - Third quantum number - designated as ml. Describes a particular orbital within a subshell where an electron is very likely to be found. Possible values are integers in






34. Named after their cation and anion






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






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






37. The vapor pressure of solution is the product of the mole fraction of the solvent and the vapor pressure of the pure solvent. P_a=X_aP_total


38. Small discrete increments of energy.






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






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






41. 2.18 x 10^-18 J/electron






42. 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.






43. Chalcogens - - Oxide O






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






45. 5 different orbitals shaped like clover leaves and max electrons is 10






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






47. 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






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






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






50. 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