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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. Named after their cation and anion






2. 5 different orbitals shaped like clover leaves and max electrons is 10






3. 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






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






5. 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






6. 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






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






8. A horizontal row of elements in the periodic table






9. Small discrete increments of energy.






10. 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.






11. Theory stating that the rate of a reaction is directly proportional to the number of collisions that take place between reactants per second.






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






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






15. Sol - a chemical process in which solvent molecules and molecules or ions of the solute combine to form a compound






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

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17. Large molecular structures - strong covalent bonding - share qualities of IONIC And COVALENT






18. 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






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






20. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance






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






23. 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






24. A physical property of a solution that depends on the number - but not the identity - of the disswolved solute particles; example properties include vapor pressure lowering - boiling point elevation - osmotic pressure - and frezzing point depression






25. 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.






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






27. The quantum number that indicates the main energy level occupied by the electron. Can theoretically take on any positive interger. Denoted by the letter n.






28. 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






29. 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.






30. One - half of the distance between the center of identical atoms that are not bonded together. Since effective nuclear charge increases when moving from left to right each additional electron is pulled more strogly toward the nucleus.






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






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






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






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






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






36. 2.18 x 10^-18 J/electron






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






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






39. The lowest allowable energy state of an atom






40. 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






41. 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






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






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






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






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






46. 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






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






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






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






50. 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