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






2. An ionic compound that resists changes in its pH






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






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






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






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






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






8. Nh/2p The angular momentum changes only in discete amounts with respect to the quantum number. Also E=- R_h/n^2






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






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






11. Named after their cation and anion






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






13. 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






14. 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






15. A fundamental constant - h - that relates the energy of light quanta to their frequency: h = 6.6 X 10^-34 joule


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






17. 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.






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






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






20. 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






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






22. Simplest whole # ration of atoms in a compound






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






24. 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






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






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






27. The weight in grams of compound that can be substituted by 1 atom of Hydrogen. GEW = MW / # of acidic Hyrdogens






28. 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.






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






30. A reaction in which two or more substances combine to form a single substance A+B>>>>>>>C






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






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






33. Chalcogens - - Oxide O






34. 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






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






36. 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






37. 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






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






39. 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


40. The process by which a gas escapes from one container to another at lower pressure through a tiny hole in the container.






41. 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






42. An uncharged molecule with a single unpaitred electron in its outer ring - very unstable - exists for only about 10 seconds






43. Numbers that specify the properties of atomic orbitals and of their electrons






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






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






46. 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






47. 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






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






49. The quantum number that indicates the main energy level occupied by the electron. Can theoretically take on any positive interger. Denoted by the letter n.






50. (chemistry) a substance formed by chemical union of two or more elements or ingredients in definite proportion by weight