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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. 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.






2. A measured amount of a solution of unknown concentration is added to a known volume of a second solution until the reaction between them is just complete






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






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






5. 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-






6. Spectrum of certain absorbed wavelengths of light corresponding to an atom's spectrum of emitted frequencies of light. Unique to each element. AAS can be used to indentify an element.






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






8. 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






9. The average distance between the nuclei of two bonded atoms






10. (chemistry) a series from actinium to lawrencium of 15 radioactive elements with increasing atomic numbers






11. 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.






12. 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






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






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






15. An element in an 'A' group in the periodic table; as a group these elements display a wide range of physical and chemical properties. In their atoms - the s and p sublevels in the highest occupied energy level are partially filled






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






17. The number of atoms in exactly 12 g of pure 12c and equal to 6.022 x 10^23 is called






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






19. An ionic compound that resists changes in its pH






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

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21. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance C>>>>A+B






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






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






24. 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.






25. A chemical bond in which one atom loses an electron to form a positive ion and the other atom gains to electron to form a negative ion






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






27. Keq describes the ratio of product concentration to reactant concentration - with each raised to the power corresponding ot its coefficient ion in the balanced equation






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






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






30. 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






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






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






33. 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






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






35. 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






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






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






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






39. 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






40. Defined acids as subtsances that produced H ions in water - while bases produced OH ions. When they reacted together - H and OH neutralise to make water






41. 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.






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






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






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






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






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






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






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






49. 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.






50. Resulting positive nuclear charge an outer electron senses after accounting for the shielding effect of inner core electrons. Abbreviated as Z(eff). Increases from left to right - and bottom to top on the Periodic Table.