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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. 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






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






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






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






5. Spectrum of certain absorbed wavelengths of light corresponding to an atom's spectrum of emitted frequencies of light. Unique to each element. AAS can be used to indentify an element.






6. 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






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






8. 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






9. 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






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






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






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






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






14. The quantum number that indicates the main energy level occupied by the electron. Can theoretically take on any positive interger. Denoted by the letter n.






15. The formation of one or more covalent bonds between an electron pair donor and an electron pair acceptor






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. E=hc/?






18. The amount of energy that reactants must absorb before a chemical reaction will start; also called free energy of activation.






19. 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






20. A representation of a displacement reaction showing only the reactive species and omitting the spectator ions.






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






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






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






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






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






26. 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






27. Named after their cation and anion






28. 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.






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






30. 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






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






32. An equilibrium expression used to measure weak - acid strength - given by the ratio of the product of the products' molar concentrations to the product of the reactants' molar concentrations - with each term raised to the power of its stoichiometric






33. 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






34. 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






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






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






37. Substance in which a solute is dissolved to form a solution






38. 5 different orbitals shaped like clover leaves and max electrons is 10






39. Expression of auto - ionization of water into H+ and OH- at a certain temperature - given by the product of the ions' molar concentrations. Denoted by Kw and equal to 10-






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






41. The point on a phase diagram that represents the only set of conditions at which all three phases exist in equilibrium with one another






42. 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.






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






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






45. 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






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






47. 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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48. Simplest whole # ration of atoms in a compound






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






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