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






2. 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






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






4. 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.






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






6. 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.






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






8. The ratio of the actual yield to the theoretical yield for a chemical reaction expressed as a percentage; a measure of the efficiency of a reaction






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






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






11. The amount of product that can be made in a chemical reaction based on the amount of limiting reactant






12. 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






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






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






15. A reaction in which two or more substances combine to form a single substance A+B>>>>>>>C






16. A solution in which water is the solvent






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






18. Orbitals of equal energy are each occupied by one electron before any orbital is occupied by a second electron - and all electrons in singly occupied orbitals must have the same spin

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19. 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






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






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






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






23. 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.






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






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






26. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds






27. 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






28. 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.






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






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. 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.






32. (chemistry) any theory in which all matter is composed of tiny discrete finite indivisible indestructible particles






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






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






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






36. Numbers that specify the properties of atomic orbitals and of their electrons






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






38. The weak attractive forces between molecules resulting from the small - instantaneous dipoles that occur because of the varying positions of the electrons during their motion about nuclei






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






40. 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






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






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






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






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






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






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






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






48. 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.






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






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