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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. 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






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






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






4. 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






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






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






7. 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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8. An ionic compound that resists changes in its pH






9. 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.






10. 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






11. Play- by- play showing the individual steps of a reaction - including the formation and destruction of any reaction intermediates that may occur.






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






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






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






15. Attractions between molecules caused by the electron motion on one molecule affecting the electron motion on the other through electrical forces; these are the weakest interactions between molecules






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






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






18. 5 different orbitals shaped like clover leaves and max electrons is 10






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






20. 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.






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






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






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






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






25. Set of spectral lines appearing in the UV region when a hydrogen atom undergoes a transition from energy levels n>1 to n=1.






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






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






29. Two or more atoms held together by covalent bonds






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






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






32. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.






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






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






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






36. 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.






37. Defined acids as subtsances that produced H ions in water - while bases produced OH ions. When they reacted together - H and OH neutralise to make water






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






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






40. Simplest whole # ration of atoms in a compound






41. 5 valence electrons -3 ions - Nitride N






42. 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






43. An atom - ion - or molecule that donates an electron pair to form a covalent bond.






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






45. 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






46. 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






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






48. 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






49. Property of the elements that can be predicted from the arrangement of the periodic table






50. Sum of all the masses - in AMU - present in one molecule of a molecular compound.