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MCAT Chemistry

Subjects : mcat, science
Instructions:
  • Answer 50 questions in 15 minutes.
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  • Match each statement with the correct term.
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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. Theory stating that the rate of a reaction is directly proportional to the number of collisions that take place between reactants per second.






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






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






4. 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.






5. An uncharged molecule with a single unpaitred electron in its outer ring - very unstable - exists for only about 10 seconds






6. A reaction where a compound does Not change its molecular structure.






7. A fundamental constant - h - that relates the energy of light quanta to their frequency: h = 6.6 X 10^-34 joule

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8. 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.






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






10. Any sample of a given compound will contain the same elements in the identical mass ratio.






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






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






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






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






15. A bond formed when two atomic orbitals combine to form a molecular orbital that is symmetrical around the axis connecting the two atomic nuclei






16. In a solution - the substance that dissolves in the solvent






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






18. 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.






19. 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.






20. 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






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






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






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






24. When a solute is dissolved in a solvent - it will dissociate until reaching an equilibrium point at which the rate of dissociation equals the rate of precipitation of the solute - regardless of any additional solute introduced into the mixture






25. 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






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






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






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






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






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






31. Spectrum of certain absorbed wavelengths of light corresponding to an atom's spectrum of emitted frequencies of light. Unique to each element. AAS can be used to indentify an element.






32. The Percent by mass of each element in a compound.






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






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






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






36. 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






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






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






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






40. 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






41. 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






42. Chalcogens - - Oxide O






43. An ionic compound that resists changes in its pH






44. Temperature is constant; effusion and temperature are proportional to the square root of their masses

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






46. (physics) the smallest discrete quantity of some physical property that a system can possess (according to quantum theory) E=hf






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






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






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






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