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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. An emperimentally determined mathmatical expression showing the rate of a reaction as a function of the concentration of its reactants






2. 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






3. 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






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






5. 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






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






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






8. An ionic compound that resists changes in its pH






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






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






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. Process by which molecules tend to move from an area where they are more concentrated to an area where they are less concentrated






13. An acid that will completely dissociate in aqueous solution - like HCl - HI - HClO4 HBr.






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






15. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds






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






17. 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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18. Small discrete increments of energy.






19. The process by which a gas escapes from one container to another at lower pressure through a tiny hole in the container.






20. 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.






21. 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






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






23. 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






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






25. Have the shape of a sphere - with the center of the sphere at the nucleus; completely symmetrical along all axes; 1s orbital is spherically symmetric and has no nodes; 2s orbital is also spherical but contains a node and is higher in energy






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






27. 2.18 x 10^-18 J/electron






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 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






30. The ways in which electrons are arranged in various orbitals around the nuclei of atoms






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






32. A solution in which water is the solvent






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






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






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






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

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






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






39. 5 valence electrons -3 ions - Nitride N






40. 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.






41. 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






42. (chemistry) p(otential of) H(ydrogen)






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






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






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






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






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






48. 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.






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






50. An uncharged molecule with a single unpaitred electron in its outer ring - very unstable - exists for only about 10 seconds