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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.
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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. 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






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






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






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






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






6. 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






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






8. Named after their cation and anion






9. 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






10. Simplest whole # ration of atoms in a compound






11. Play- by- play showing the individual steps of a reaction - including the formation and destruction of any reaction intermediates that may occur.






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






13. An ionic compound that resists changes in its pH






14. 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.






15. 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






16. 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.






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






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






19. A chemical bond that involves sharing a pair of electrons between atoms in a molecule






20. The intermolecular force in which a hydrogen atom that is bonded to a highly electronegative atom is attracted to an unshared pair of electrons of an electronegative atom in a nearby molecule






21. The point during a titration when the number of H+ ions and OH- ions are equal. This is at the middle of the steepest part of the titration curve.






22. 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.






23. The solubility of a gas in a liquid is directly proportional to the partial pressure of that gas on the surface of the liquid


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






25. 5 valence electrons -3 ions - Nitride N






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






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






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






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






30. 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






31. A solution in which water is the solvent






32. 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.






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






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






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






36. 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






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






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






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






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






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






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






43. A fundamental constant - h - that relates the energy of light quanta to their frequency: h = 6.6 X 10^-34 joule


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






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






46. A subdivision of an energy level in an atom. They are divided into orbitals.






47. Sol - a chemical process in which solvent molecules and molecules or ions of the solute combine to form a compound






48. The ways in which electrons are arranged in various orbitals around the nuclei of atoms






49. The intermolecular force in which a hydrogen atom that is bonded to a highly electronegative atom is attracted to an unshared pair of electrons of an electronegative atom in a nearby molecule






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