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






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






3. 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.






4. A chemical formula showing the ratio of elements in a compound rather than the total number of atoms






5. 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.






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






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






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






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






10. 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






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






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






13. 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






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






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






16. A representation of a displacement reaction showing only the reactive species and omitting the spectator ions.






17. A set of spectral lines that appear in the visible light region when a hydrogen atom undergoes a transition from energy levels n>2 to n=2.






18. Atoms react by gaining or losing electrons so as to acquire the stable electron structure of a noble gas - usually eight valence electrons






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






20. (chemistry) a series from actinium to lawrencium of 15 radioactive elements with increasing atomic numbers






21. Rare earth element group (elements 58-71)






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






23. 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






24. Contains nonmetals that are non - reactive. Full outermost energy level except helium which has 2.






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






26. 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.






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






28. 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






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






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






31. 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






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






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






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






35. Resulting positive nuclear charge an outer electron senses after accounting for the shielding effect of inner core electrons. Abbreviated as Z(eff). Increases from left to right - and bottom to top on the Periodic Table.






36. 2.18 x 10^-18 J/electron






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






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






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






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






41. Named after their cation and anion






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






43. 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






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






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






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






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






48. 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.






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






50. 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