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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. The ratio of the number of moles of solute dissolved in one kilogram of solvent. molality (M = moles solute/kg of solution)






2. (chemistry) p(otential of) H(ydrogen)






3. 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.






4. 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






5. 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






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






7. 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






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






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






10. The energy required to remove an electron from a gaseous atom; generally increases in moving from left - to - right across a period and decreases in moving down a group






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






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






13. 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






14. 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.






15. 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.






16. 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






17. Slightly less reactive than alkali metals - comprise group II






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






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






20. 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






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. (chemistry) a substance that changes color to indicate the presence of some ion or substance






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






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






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






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






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






28. Standard Temperature and Pressure. 273 Kelvin (0 Celsius) - 1 atmosphere (760 torr - 760 kPA).






29. 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.






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






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






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






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






34. 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






35. 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






36. 5 valence electrons -3 ions - Nitride N






37. 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.






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






39. Specifies the specific orbital in which the electron is most likely to be found. - Third quantum number - designated as ml. Describes a particular orbital within a subshell where an electron is very likely to be found. Possible values are integers in






40. 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






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






42. The point during a titration when the number of H+ ions and OH- ions are equal. This is at the middle of the steepest part of the titration curve.






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






44. The amount of energy that reactants must absorb before a chemical reaction will start; also called free energy of activation.






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






46. 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






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






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






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






50. 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