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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. 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






2. 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






3. 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






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






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






6. The ratio of the actual yield to the theoretical yield for a chemical reaction expressed as a percentage; a measure of the efficiency of a reaction






7. A horizontal row of elements in the periodic table






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






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






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






12. 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.






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






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






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






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






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






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






19. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds






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






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






22. 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






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






24. Alkali metals: highly reactive - therefore always compounds. - 1 valence electron +1 ion - Hydrogen H? - Lithium Li? - Sodium Na? - Potassium K? - Rubidium Rb? - Cesium Cs?






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






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






27. 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






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






29. 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






30. 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.






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






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






33. 5 valence electrons -3 ions - Nitride N






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






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






36. An equilibrium expression used to measure weak - acid strength - given by the ratio of the product of the products' molar concentrations to the product of the reactants' molar concentrations - with each term raised to the power of its stoichiometric






37. 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






38. The ratio of the number of moles of solute dissolved in one kilogram of solvent. molality (M = moles solute/kg of solution)






39. 5 different orbitals shaped like clover leaves and max electrons is 10






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






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






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






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






44. 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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45. 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.






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






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






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






49. 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






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