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






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






3. 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.






4. 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






5. 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






6. 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






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






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






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






10. A substance that - when dissolved in water - results in a solution that can conduct electricity






11. The process of decomposing a chemical compound by the passage of an electric current.






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






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






14. 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






15. 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






16. Contains nonmetals - 7 valence electrons in it's outermost energy level. Very reactive






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






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






19. 5 valence electrons -3 ions - Nitride N






20. 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.






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






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






23. 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






24. Sum of all the masses - in AMU - present in one molecule of a molecular compound.






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






26. Standard Temperature and Pressure. 273 Kelvin (0 Celsius) - 1 atmosphere (760 torr - 760 kPA).






27. 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.






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






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






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






31. A reaction where a compound does Not change its molecular structure.






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






33. 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






34. Temperature is constant; effusion and temperature are proportional to the square root of their masses

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35. 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.






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






37. A horizontal row of elements in the periodic table






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






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






40. Energy released when an atom or ion in the gaseous state gains an electron. Increases from left to right and from bottom to top on the Periodic Table.






41. 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.






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






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






45. An ionic compound that resists changes in its pH






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






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






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






49. 2.18 x 10^-18 J/electron






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