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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. Simplest whole # ration of atoms in a compound






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. The solubility of a gas in a liquid is directly proportional to the partial pressure of that gas on the surface of the liquid

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4. 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






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






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






7. 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






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






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






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






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






12. Alkaline Earth Metals - 2 valence electrons +2 ions - Magnesium Mg






13. 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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14. 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






15. 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






16. 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






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






18. 5 different orbitals shaped like clover leaves and max electrons is 10






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






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






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






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






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






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






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






26. 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






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






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






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






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






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






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






33. An ionic compound that resists changes in its pH






34. E=hc/?






35. 2.18 x 10^-18 J/electron






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






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






38. The slowest elementary step which is the limit for the rate of the other steps






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






40. Set of spectral lines appearing in the UV region when a hydrogen atom undergoes a transition from energy levels n>1 to n=1.






41. 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






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






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






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






46. A reaction where a compound does Not change its molecular structure.






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

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48. Tells you how much solute is present compared to the amount of solvent






49. The quantum number that has only two possible values - +1/2 and -1/2 - which indicate the two fundamental spin states of an electron in an orbital






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