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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.
  • 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 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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2. The lowest allowable energy state of an atom






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






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






6. 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






7. 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






8. The process of decomposing a chemical compound by the passage of an electric current.






9. 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






10. 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.






11. When dipoles are dissolved in a solution where ions are present ions wil arrange themselves with the opposite charged end of the dipole.






12. 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






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






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






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






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






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






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






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






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. 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






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






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






24. In a solution - the substance that dissolves in the solvent






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






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






27. 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






28. PH of a molecule at which it contains no net electric charge - isoelectric point.






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

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






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






32. 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.






33. 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






34. A set of frequencies of electromagnetic waves given off by atoms of an element; consists of a series of fine lines of individual colors






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






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






37. Slightly less reactive than alkali metals - comprise group II






38. 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






39. A concentration unit of a solution expressed as moles of solute dissolved per liter of solution






40. 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.






41. The percent by mass of each element in a compound






42. 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






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






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






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






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






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






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






49. Second quantum number - designated by the letter 'l.' This 'angular momentum' refers to the subshells within each principle quantum energy level. It can take on the value of an integer in the 0 to (n -1) range. The four subshellscorresponding to l=0






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