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






2. 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






3. 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.






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






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






6. An atom - radical - or molecule that has gained or lost one or more electrons and has a negative or positive charge






7. 5 different orbitals shaped like clover leaves and max electrons is 10






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






9. The sum of the exponents in a rate law - where each exponent provides the reaction order with respect to its reactants






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






11. 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






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






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






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






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






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






17. Where half of the acid is neutralized by the base on a titration curveAn acid dissociation constant - Ka - (also known as acidity constant - or acid - ionization constant) is a quantitative measure of the strength of an acid in solution. It is the eq






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






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






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






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






22. 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.






23. Any sample of a given compound will contain the same elements in the identical mass ratio.






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






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






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






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






28. The reaction of the ions that characterize acids and the ions that characterize bases to form water molecules and a salt






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






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






31. A naturally occurring or synthetic compound consisting of large molecules made up of a linked series of repeated simple monomers






32. 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.






33. 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






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






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

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






37. Attractions between molecules caused by the electron motion on one molecule affecting the electron motion on the other through electrical forces; these are the weakest interactions between molecules






38. 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






39. Two or more atoms held together by covalent bonds






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






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






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






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






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






46. Chalcogens - - Oxide O






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






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






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






50. 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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