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






2. A dynamic condition in which two opposing changes occur at equal rates in a closed system






3. A structural formula in which electrons are represented by dots; dot pairs or dashes between two atomic symbols represent pairs in covalent bonds.






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






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






6. One - half of the distance between the center of identical atoms that are not bonded together. Since effective nuclear charge increases when moving from left to right each additional electron is pulled more strogly toward the nucleus.






7. 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






8. The ratio of the actual yield to the theoretical yield for a chemical reaction expressed as a percentage; a measure of the efficiency of a reaction






9. 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.






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






11. 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






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






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






15. A bond formed when two atomic orbitals combine to form a molecular orbital that is symmetrical around the axis connecting the two atomic nuclei






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






17. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds






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






19. Expression of auto - ionization of water into H+ and OH- at a certain temperature - given by the product of the ions' molar concentrations. Denoted by Kw and equal to 10-






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






21. The amount of a substance that contains as many particles as there are atoms in exactly 12g of carbon -12






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






23. Simplest whole # ration of atoms in a compound






24. (chemistry) a substance formed by chemical union of two or more elements or ingredients in definite proportion by weight






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






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






27. 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.






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






29. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance C>>>>A+B






30. 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






31. Small discrete increments of energy.






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






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






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






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






37. 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






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






39. 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






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






41. Property of the elements that can be predicted from the arrangement of the periodic table






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






43. 5 valence electrons -3 ions - Nitride N






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






45. An uncharged molecule with a single unpaitred electron in its outer ring - very unstable - exists for only about 10 seconds






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






47. 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






48. PH=pka+log[base/acid] Used in titration based problems that relates the pH or pOH of a solution to the pK and the ratio of the dissociated species.






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






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