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MCAT Chemistry

Subjects : mcat, science
Instructions:
  • Answer 50 questions in 15 minutes.
  • If you are not ready to take this test, you can study here.
  • 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. A subdivision of an energy level in an atom. They are divided into orbitals.






2. An atom or group of atoms that has a positive or negative charge






3. 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






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






5. (physics) the smallest discrete quantity of some physical property that a system can possess (according to quantum theory) E=hf






6. 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






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






8. The weight in grams of one mole of a given elementand is expressedin tems of grams per mole.






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






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






11. 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






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






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






14. Common definition of acids as proton (H+) donors and bases as proton acceptors






15. The solubility of a gas in a liquid is directly proportional to the partial pressure of that gas on the surface of the liquid

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






17. 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






18. Small discrete increments of energy.






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






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






21. 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






22. Keq describes the ratio of product concentration to reactant concentration - with each raised to the power corresponding ot its coefficient ion in the balanced equation






23. 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.






24. Acids defined as electron - pair acceptors and bases as electron - pair donors.






25. Having characteristics of both an acid and a base and capable of reacting as either






26. E=hc/?






27. 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.






28. Two or more atoms held together by covalent bonds






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






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






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






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






33. A horizontal row of elements in the periodic table






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






35. 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






36. 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.






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






38. 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






39. An ionic compound that resists changes in its pH






40. 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






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






42. The pressure exerted by a vapor in equilibrium with its liquid or solid phase






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






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






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






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






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






49. States that it is impossible to determine simultaneously both the position and momentum of an electron or any other particle






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