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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. 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.






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






3. 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






4. The vapor pressure of solution is the product of the mole fraction of the solvent and the vapor pressure of the pure solvent. P_a=X_aP_total

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5. A set of frequencies of electromagnetic waves given off by atoms of an element; consists of a series of fine lines of individual colors






6. 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






7. 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






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






9. A solution in which water is the solvent






10. Halogens; ns2np5 - - 2nd most reactive group - The Halogens; very active because of need to fill; form -1 ions; 7 electrons in valence shell; tend to form salts with elements from groups 1A and 2A






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






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






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






14. The reaction of the ions that characterize acids and the ions that characterize bases to form water molecules and a salt






15. The weight in grams of compound that can be substituted by 1 atom of Hydrogen. GEW = MW / # of acidic Hyrdogens






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






17. Process by which molecules tend to move from an area where they are more concentrated to an area where they are less concentrated






18. A chemical bond that involves sharing a pair of electrons between atoms in a molecule






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






20. A subdivision of an energy level in an atom. They are divided into orbitals.






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






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






23. The process of decomposing a chemical compound by the passage of an electric current.






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






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






26. 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






27. 5 valence electrons -3 ions - Nitride N






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






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






30. The point on a phase diagram that represents the only set of conditions at which all three phases exist in equilibrium with one another






31. 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






32. Two or more atoms held together by covalent bonds






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






34. 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.






35. Temperature is constant; effusion and temperature are proportional to the square root of their masses

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






37. 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






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






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






40. 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






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






42. Chalcogens - - Oxide O






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






44. 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






45. 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






46. 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.






47. Simplest whole # ration of atoms in a compound






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






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






50. 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.