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






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






3. 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






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






5. Contains nonmetals that are non - reactive. Full outermost energy level except helium which has 2.






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






7. Halogens; ns2np5 - - 2nd most reactive group - The Halogens; very active because of need to fill; form -1 ions; 7 electrons in valence shell; tend to form salts with elements from groups 1A and 2A






8. 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






9. Chalcogens - - Oxide O






10. 2.18 x 10^-18 J/electron






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






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






13. The maximum amount of product that can be produced from a given amount of reactant






14. 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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15. The lowest allowable energy state of an atom






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






17. A structural formula in which electrons are represented by dots; dot pairs or dashes between two atomic symbols represent pairs in covalent bonds.






18. A set of frequencies of electromagnetic waves given off by atoms of an element; consists of a series of fine lines of individual colors






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






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






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






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






23. A bond formed when two atomic orbitals combine to form a molecular orbital that is symmetrical around the axis connecting the two atomic nuclei






24. The energy required to remove an electron from a gaseous atom; generally increases in moving from left - to - right across a period and decreases in moving down a group






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






26. A chemical formula showing the ratio of elements in a compound rather than the total number of atoms






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






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






29. 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






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






31. 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.






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






33. A horizontal row of elements in the periodic table






34. The tendency for an atom to attract electrons to itself when it is chemically combined with another element






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






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






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






38. Named after their cation and anion






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






40. 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






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






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






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






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






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






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






48. 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.






49. 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






50. An elementary particle with 0 charge and mass about equal to a proton