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






3. An element in an 'A' group in the periodic table; as a group these elements display a wide range of physical and chemical properties. In their atoms - the s and p sublevels in the highest occupied energy level are partially filled






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






5. Tells you how much solute is present compared to the amount of solvent






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






7. The process by which one or more substances change to produce one or more different substances






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






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






10. 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






11. 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






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

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13. Small discrete increments of energy.






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






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






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






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






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






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






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






22. 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






23. 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






24. Solids in which the particles are arranged in a repeating - 3- D pattern - has a specific melting point - classified as ionic network covalent - metallic or molecular.






25. 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.






26. A horizontal row of elements in the periodic table






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






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






29. 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






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






31. The area of chemistry that is concerned with reaction rates and reaction mechanisms






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






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






34. 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






35. 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.






36. An acid that will completely dissociate in aqueous solution - like HCl - HI - HClO4 HBr.






37. A solution in which water is the solvent






38. 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






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






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






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






42. The center of the atom which contains the protons and neutrons; in cells - structure that contains the cell's genetic material (DNA) and controls the cell's activities






43. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds






44. Alkali metals: highly reactive - therefore always compounds. - 1 valence electron +1 ion - Hydrogen H? - Lithium Li? - Sodium Na? - Potassium K? - Rubidium Rb? - Cesium Cs?






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






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






47. A measured amount of a solution of unknown concentration is added to a known volume of a second solution until the reaction between them is just complete






48. 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






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






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