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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. Named after their cation and anion






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






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






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






5. Elements in the middle of the periodic table - in groups 3-12.






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






7. 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






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






9. Gram equivalent weight of solute per liter of solution - often denoted by N.






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






11. Chalcogens - - Oxide O






12. 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






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






14. The Percent by mass of each element in a compound.






15. 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.






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






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






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






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






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






21. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds






22. A set of spectral lines that appear in the visible light region when a hydrogen atom undergoes a transition from energy levels n>2 to n=2.






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






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






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






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






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






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






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






30. A horizontal row of elements in the periodic table






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






32. 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






33. A graph of pressure versus temperature that shows the conditions under which the phases of a substance exist






34. 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






35. 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






36. 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






37. 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






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






39. 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






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






41. 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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42. The lowest allowable energy state of an atom






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






44. 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






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

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






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






48. 5 different orbitals shaped like clover leaves and max electrons is 10






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






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