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






2. 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.






3. Chalcogens - - Oxide O






4. 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






5. 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






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






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






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






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






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






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






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






13. A horizontal row of elements in the periodic table






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






15. 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






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






17. A graph of pressure versus temperature that shows the conditions under which the phases of a substance exist






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






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






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






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






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






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






24. Have the shape of a sphere - with the center of the sphere at the nucleus; completely symmetrical along all axes; 1s orbital is spherically symmetric and has no nodes; 2s orbital is also spherical but contains a node and is higher in energy






25. Two or more atoms held together by covalent bonds






26. 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.






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

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






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






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






31. A solution in which water is the solvent






32. 5 different orbitals shaped like clover leaves and max electrons is 10






33. Gram equivalent weight of solute per liter of solution - often denoted by N.






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






35. The slowest elementary step which is the limit for the rate of the other steps






36. 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.






37. A pair of equal and opposite electric charges or magnetic poles separated by a small distance






38. 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.






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






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






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






42. 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






43. A covalent bond in which the bonding electrons are shared equally by the bonded atoms - resulting in a balanced distribution of electrical charge






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






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






46. 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-






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






48. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds






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






50. The amount of a substance that contains as many particles as there are atoms in exactly 12g of carbon -12