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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. E=hc/?






2. 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






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






4. Small discrete increments of energy.






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






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






7. An atom - ion - or molecule that donates an electron pair to form a covalent bond.






8. 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






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






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






11. The reaction of the ions that characterize acids and the ions that characterize bases to form water molecules and a salt






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






13. Simplest whole # ration of atoms in a compound






14. Halogens; ns2np5 - - 2nd most reactive group - The Halogens; very active because of need to fill; form -1 ions; 7 electrons in valence shell; tend to form salts with elements from groups 1A and 2A






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






16. 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.






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






18. 1913 - Niels Bohr - said that electrons formed specific layers instead or random ones - said atoms atoms absorb and give off energy when the electrons move from one shell to another






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






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






21. 5 different orbitals shaped like clover leaves and max electrons is 10






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






23. 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.






24. Having characteristics of both an acid and a base and capable of reacting as either






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






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






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






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. 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






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






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






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

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33. Named after their cation and anion






34. The lowest allowable energy state of an atom






35. Mixture of 2 or more substances that distills at a constant temperature and with constant composition - even though seperately the components have different boiling points






36. Two or more atoms held together by covalent bonds






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






38. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.






39. 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.






40. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds






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






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






43. 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






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






45. 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






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






47. 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






48. The hypothetical equation showing only the species that is oxidized or reduced in a redox reaction and the correct number of electrons transferred between the species in the complete - balanced equation.






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






50. A model of acids and bases which an acid is hydrogen ion donor and base is a hydrogen ion acceptor.







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