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






2. Attractive and repulsive forces between molecules that are weaker than forces within molecules.






3. Structure that occurs when it is possible to draw two or more valid electron dot structures that have the same number of electron pairs for a molecule or ion






4. 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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5. Temperature is constant; effusion and temperature are proportional to the square root of their masses

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6. 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






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






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






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






10. Mixture of 2 or more substances that distills at a constant temperature and with constant composition - even though seperately the components have different boiling points






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






12. Rare earth element group (elements 58-71)






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






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






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






16. 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






17. Product of the molar concentrations of dissociated ions in solution at saturation - where each ion is raised to the power of its stoichiometric coefficient. Denoted Ksp.






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






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






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






21. 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






22. 5 different orbitals shaped like clover leaves and max electrons is 10






23. 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.






24. A model of acids and bases which an acid is hydrogen ion donor and base is a hydrogen ion acceptor.






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






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






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






28. 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






29. Sum of all the masses - in AMU - present in one molecule of a molecular compound.






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






31. Alkaline Earth Metals - 2 valence electrons +2 ions - Magnesium Mg






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






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






34. Two or more atoms held together by covalent bonds






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






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






37. The vapor pressure of solution is the product of the mole fraction of the solvent and the vapor pressure of the pure solvent. P_a=X_aP_total

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






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






40. 5 valence electrons -3 ions - Nitride N






41. 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






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






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






44. A physical property of a solution that depends on the number - but not the identity - of the disswolved solute particles; example properties include vapor pressure lowering - boiling point elevation - osmotic pressure - and frezzing point depression






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






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






47. Halogens; ns2np5 - - 2nd most reactive group - The Halogens; very active because of need to fill; form -1 ions; 7 electrons in valence shell; tend to form salts with elements from groups 1A and 2A






48. A solution in which water is the solvent






49. 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.






50. A measured amount of a solution of unknown concentration is added to a known volume of a second solution until the reaction between them is just complete