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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. 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






2. The lowest allowable energy state of an atom






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






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






5. 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






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






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






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






9. 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.






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






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






12. States that it is impossible to determine simultaneously both the position and momentum of an electron or any other particle






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






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






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






16. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds






17. 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






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






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






20. 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






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

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22. 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






23. 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






24. 5 different orbitals shaped like clover leaves and max electrons is 10






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






26. PH of a molecule at which it contains no net electric charge - isoelectric point.






27. The nuclear charge experienced by the outermost electrons of an atom (actual charge minus the shielding caused by inner shells: Z- eff)






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






29. 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.






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






31. The energy required to remove an electron from a gaseous atom; generally increases in moving from left - to - right across a period and decreases in moving down a group






32. Small discrete increments of energy.






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






34. 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-






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






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






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






38. Contains nonmetals - 7 valence electrons in it's outermost energy level. Very reactive






39. 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






40. E=hc/?






41. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance C>>>>A+B






42. 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






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






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






45. The average distance between the nuclei of two bonded atoms






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






47. A solution in which water is the solvent






48. 5 valence electrons -3 ions - Nitride N






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






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