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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. In a solution - the substance that dissolves in the solvent






2. A pair of equal and opposite electric charges or magnetic poles separated by a small distance






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






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






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






6. Small discrete increments of energy.






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

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






9. 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






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






11. 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






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






13. Sum of the protons and neutrons in an element often denoted by the letter A






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






15. 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.






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






17. A solution in which water is the solvent






18. The Percent by mass of each element in a compound.






19. 2.18 x 10^-18 J/electron






20. 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






21. A horizontal row of elements in the periodic table






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






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






24. Two or more atoms held together by covalent bonds






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






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






27. 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.






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






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






30. 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.






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






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






33. 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






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






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






36. 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.






37. 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.






38. 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






39. 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






40. 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






41. (physics) the smallest discrete quantity of some physical property that a system can possess (according to quantum theory) E=hf






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






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






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






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






46. An ionic compound that resists changes in its pH






47. 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.






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






49. 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






50. 5 valence electrons -3 ions - Nitride N







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