Test your basic knowledge |

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. 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






2. 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






3. 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






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






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






6. 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






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






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






9. Have three valance electrons. In certain instances - some elements will loose three electrons - but they will also share electrons with another element to attain stability.






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






11. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds






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






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






14. 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.






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






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






17. Product of the molar concentrations of dissociated ions in solution at any point in the reaction other than equilibrium or saturation - where each ion is raised to the power of its stoichiometric coefficient. Denoted IP.






18. Simplest whole # ration of atoms in a compound






19. A reaction where a compound does Not change its molecular structure.






20. A base that can accept two moles of H+ per mole of itself (ex: SO4






21. A representation of a displacement reaction showing only the reactive species and omitting the spectator ions.






22. 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






23. A bond formed when two atomic orbitals combine to form a molecular orbital that is symmetrical around the axis connecting the two atomic nuclei






24. Chalcogens - - Oxide O






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






26. An ionic compound that resists changes in its pH






27. 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






28. 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.






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






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






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






32. 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.






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






34. 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






35. The Percent by mass of each element in a compound.






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






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






38. Structure that occurs when it is possible to draw two or more valid electron dot structures that have the same number of electron pairs for a molecule or ion






39. Named after their cation and anion






40. Region in a molecule where atomic orbitals overlap - resulting in either a stable low - energy bonding orbital or an unstable high - energy antibonding orbital.






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






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






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






44. 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






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






46. 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






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






48. 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






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






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







Sorry!:) No result found.

Can you answer 50 questions in 15 minutes?


Let me suggest you:

Browse all subjects

Browse all tests

Most popular tests



Major Subjects

Tests & Exams


AP
CLEP
DSST
GRE
SAT
GMAT

Browse all subjects

Browse all tests

Most popular tests