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






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






3. The lowest allowable energy state of an atom






4. 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






5. 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






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






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






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






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






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






11. 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






12. 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






13. 5 valence electrons -3 ions - Nitride N






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






15. 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






16. 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






17. 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






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






19. States that if a stress is applied to a system at equilibrium - the system shifts in the direction that relieves the stress.






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






21. 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.






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






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






24. 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.






25. 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.






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






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






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






29. 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






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






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






32. Energy released when an atom or ion in the gaseous state gains an electron. Increases from left to right and from bottom to top on the Periodic Table.






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






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






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






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






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






38. 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






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






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






41. (chemistry) a substance that changes color to indicate the presence of some ion or substance






42. E=hc/?






43. Attractions between molecules caused by the electron motion on one molecule affecting the electron motion on the other through electrical forces; these are the weakest interactions between molecules






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






45. 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






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






47. 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






48. The weight in grams of one mole of a given elementand is expressedin tems of grams per mole.






49. (chemistry) the sum of the relative atomic masses of the constituent atoms of a molecule






50. 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.