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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. 5 valence electrons -3 ions - Nitride N






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






3. 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






4. A definite stable energy that a physical system can have






5. A horizontal row of elements in the periodic table






6. 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.






7. 5 different orbitals shaped like clover leaves and max electrons is 10






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






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






10. Expression of auto - ionization of water into H+ and OH- at a certain temperature - given by the product of the ions' molar concentrations. Denoted by Kw and equal to 10-






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






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






13. 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.






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






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






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






17. 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.






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






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






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






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






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






23. 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






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






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






26. 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






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






28. One - half the distance between the nuclei of two atoms of the same element when the atoms are joined






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






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






31. Theory stating that the rate of a reaction is directly proportional to the number of collisions that take place between reactants per second.






32. Attractive and repulsive forces between molecules that are weaker than forces within molecules.






33. 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.






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






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






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






37. Have the shape of a sphere - with the center of the sphere at the nucleus; completely symmetrical along all axes; 1s orbital is spherically symmetric and has no nodes; 2s orbital is also spherical but contains a node and is higher in energy






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






39. The tendency for an atom to attract electrons to itself when it is chemically combined with another element






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






41. An ionic compound that resists changes in its pH






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






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






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






45. 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






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






47. 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






48. 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






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






50. 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