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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. 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.






2. 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.






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






4. Small discrete increments of energy.






5. Chalcogens - - Oxide O






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






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






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






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






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






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






12. A solution in which water is the solvent






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






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






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






16. 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






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. 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






19. 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






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






21. 5 different orbitals shaped like clover leaves and max electrons is 10






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






24. 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






25. A subatomic particle that has a positive charge and that is found in the nucleus of an atom Charge of +1 and mass of 1.0073 amu






26. When polar molecules orient themselves such that the positive region of one molecule is close to the negative region of another molecule.






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






28. 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.






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






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






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






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






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

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34. 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.






35. Atoms react by gaining or losing electrons so as to acquire the stable electron structure of a noble gas - usually eight valence electrons






36. Nh/2p The angular momentum changes only in discete amounts with respect to the quantum number. Also E=- R_h/n^2






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






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






39. An ionic compound that resists changes in its pH






40. 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






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






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






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






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






45. Product of the molar concentrations of dissociated ions in solution at any point in the reaction other than equilibrium or saturation - where each ion is raised to the power of its stoichiometric coefficient. Denoted IP.






46. 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






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






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






49. 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






50. 2.18 x 10^-18 J/electron