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






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






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






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






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






6. A solution in which water is the solvent






7. 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.






8. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds






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






10. Have three valance electrons. In certain instances - some elements will loose three electrons - but they will also share electrons with another element to attain stability.






11. 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.






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






13. 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






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






15. Gram equivalent weight of solute per liter of solution - often denoted by N.






16. 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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17. A dynamic condition in which two opposing changes occur at equal rates in a closed system






18. 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






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






20. 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






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






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






23. An ionic compound that resists changes in its pH






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






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






26. 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






27. The lowest allowable energy state of an atom






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






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






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






32. 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.






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






34. The process by which one or more substances change to produce one or more different substances






35. Region in a molecule where atomic orbitals overlap - resulting in either a stable low - energy bonding orbital or an unstable high - energy antibonding orbital.






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






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






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

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39. Named after their cation and anion






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






41. 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.






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






43. Having characteristics of both an acid and a base and capable of reacting as either






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






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






46. Chalcogens - - Oxide O






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






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






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







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