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






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






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






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






6. The weight in grams of compound that can be substituted by 1 atom of Hydrogen. GEW = MW / # of acidic Hyrdogens






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






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






9. Alkali metals: highly reactive - therefore always compounds. - 1 valence electron +1 ion - Hydrogen H? - Lithium Li? - Sodium Na? - Potassium K? - Rubidium Rb? - Cesium Cs?






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






11. No two electrons or protons or neutrons in a given system can be in states characterized by the same set of quantum numbers






12. The reaction of the ions that characterize acids and the ions that characterize bases to form water molecules and a salt






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






14. 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






15. 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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16. 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






17. 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.






18. 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.






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






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






21. 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






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






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






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






25. 5 valence electrons -3 ions - Nitride N






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






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






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






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






30. Acids defined as electron - pair acceptors and bases as electron - pair donors.






31. 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.






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






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






34. 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.






35. A solution in which water is the solvent






36. When a solute is dissolved in a solvent - it will dissociate until reaching an equilibrium point at which the rate of dissociation equals the rate of precipitation of the solute - regardless of any additional solute introduced into the mixture






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






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






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. 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






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






42. 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






43. 2.18 x 10^-18 J/electron






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






45. The area of chemistry that is concerned with reaction rates and reaction mechanisms






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






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






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






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






50. Large molecular structures - strong covalent bonding - share qualities of IONIC And COVALENT