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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. The lowest allowable energy state of an atom






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






3. 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.






4. Simplest whole # ration of atoms in a compound






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






6. A definite stable energy that a physical system can have






7. Named after their cation and anion






8. Play- by- play showing the individual steps of a reaction - including the formation and destruction of any reaction intermediates that may occur.






9. Slightly less reactive than alkali metals - comprise group II






10. 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.






11. Process by which molecules tend to move from an area where they are more concentrated to an area where they are less concentrated






12. Product of the molar concentrations of dissociated ions in solution at saturation - where each ion is raised to the power of its stoichiometric coefficient. Denoted Ksp.






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






14. 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






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






16. Expression of auto - ionization of water into H+ and OH- at a certain temperature - given by the product of the ions' molar concentrations. Denoted by Kw and equal to 10-






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






18. The hypothetical equation showing only the species that is oxidized or reduced in a redox reaction and the correct number of electrons transferred between the species in the complete - balanced equation.






19. 5 valence electrons -3 ions - Nitride N






20. A solution in which water is the solvent






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






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






23. A graph of pressure versus temperature that shows the conditions under which the phases of a substance exist






24. Structure that occurs when it is possible to draw two or more valid electron dot structures that have the same number of electron pairs for a molecule or ion






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






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






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






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






29. 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.






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






31. 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.






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






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






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






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






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






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


39. 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






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






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






42. 5 different orbitals shaped like clover leaves and max electrons is 10






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






44. 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






45. 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






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






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






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






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






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