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






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






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






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






5. 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.






6. 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.






7. 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






8. 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






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






10. A chemical formula showing the ratio of elements in a compound rather than the total number of atoms






11. The hypothetical equation showing only the species that is oxidized or reduced in a redox reaction and the correct number of electrons transferred between the species in the complete - balanced equation.






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






13. Atoms react by gaining or losing electrons so as to acquire the stable electron structure of a noble gas - usually eight valence electrons






14. 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






15. 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






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






17. 5 valence electrons -3 ions - Nitride N






18. 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






19. 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






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






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






22. Expression of auto - ionization of water into H+ and OH- at a certain temperature - given by the product of the ions' molar concentrations. Denoted by Kw and equal to 10-






23. 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






24. 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.






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






26. Simplest whole # ration of atoms in a compound






27. 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






28. The formation of one or more covalent bonds between an electron pair donor and an electron pair acceptor






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






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






31. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds






32. 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






33. A horizontal row of elements in the periodic table






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






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






36. 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






37. 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.






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






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






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






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






42. 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






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






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






45. In a solution - the substance that dissolves in the solvent






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

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






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






49. Two or more atoms held together by covalent bonds






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






Can you answer 50 questions in 15 minutes?



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