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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. An ionic compound that resists changes in its pH






2. 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.






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






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






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






6. A horizontal row of elements in the periodic table






7. Set of spectral lines appearing in the UV region when a hydrogen atom undergoes a transition from energy levels n>1 to n=1.






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






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






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






11. 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






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






13. The quantum number that has only two possible values - +1/2 and -1/2 - which indicate the two fundamental spin states of an electron in an orbital






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






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






16. The quantum number that indicates the main energy level occupied by the electron. Can theoretically take on any positive interger. Denoted by the letter n.






17. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.






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






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






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






21. Standard Temperature and Pressure. 273 Kelvin (0 Celsius) - 1 atmosphere (760 torr - 760 kPA).






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






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






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






25. Keq describes the ratio of product concentration to reactant concentration - with each raised to the power corresponding ot its coefficient ion in the balanced equation






26. Two or more atoms held together by covalent bonds






27. 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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28. 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






29. The amount of product that can be made in a chemical reaction based on the amount of limiting reactant






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






31. 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.






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






33. Product of the molar concentrations of dissociated ions in solution at any point in the reaction other than equilibrium or saturation - where each ion is raised to the power of its stoichiometric coefficient. Denoted IP.






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






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






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






37. Valence Shell Electron Pair Repulsion theory - stating that the three - dimensional molecular geometry about some central atom is determined by the elctronic repulsion between its bonding and nonbonding electron pairs.






38. 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






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






40. An atom - ion - or molecule that donates an electron pair to form a covalent bond.






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






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






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






44. An atom - radical - or molecule that has gained or lost one or more electrons and has a negative or positive charge






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

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46. 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






47. A naturally occurring or synthetic compound consisting of large molecules made up of a linked series of repeated simple monomers






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






49. 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






50. 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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