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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. The amount of energy that reactants must absorb before a chemical reaction will start; also called free energy of activation.






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






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






4. 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






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






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






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






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






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






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






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






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






14. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance






15. 2.18 x 10^-18 J/electron






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






17. The maximum amount of product that can be produced from a given amount of reactant






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






19. Two or more atoms held together by covalent bonds






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






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






22. 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






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






24. The number of atoms in exactly 12 g of pure 12c and equal to 6.022 x 10^23 is called






25. 5 valence electrons -3 ions - Nitride N






26. 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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27. The process of decomposing a chemical compound by the passage of an electric current.






28. 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






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






30. E=hc/?






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






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






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






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






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

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36. 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






37. 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.






38. 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.






39. 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






40. 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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41. 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






42. The slowest elementary step which is the limit for the rate of the other steps






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






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






45. 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.






46. 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






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






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






49. Specifies the specific orbital in which the electron is most likely to be found. - Third quantum number - designated as ml. Describes a particular orbital within a subshell where an electron is very likely to be found. Possible values are integers in






50. 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.







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