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. 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






2. 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.






3. 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






4. 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






5. An element in an 'A' group in the periodic table; as a group these elements display a wide range of physical and chemical properties. In their atoms - the s and p sublevels in the highest occupied energy level are partially filled






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






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






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






9. 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






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






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






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






13. Substance in which a solute is dissolved to form a solution






14. The slowest elementary step which is the limit for the rate of the other steps






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






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






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






18. 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






19. An ionic compound that resists changes in its pH






20. 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.






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






22. The maximum amount of product that can be produced from a given amount of reactant






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






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






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






27. (chemistry) the sum of the relative atomic masses of the constituent atoms of a molecule






28. An emperimentally determined mathmatical expression showing the rate of a reaction as a function of the concentration of its reactants






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






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






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






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






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






34. The area of chemistry that is concerned with reaction rates and reaction mechanisms






35. 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.






36. 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






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






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






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






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






42. Chalcogens - - Oxide O






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






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






45. Resulting positive nuclear charge an outer electron senses after accounting for the shielding effect of inner core electrons. Abbreviated as Z(eff). Increases from left to right - and bottom to top on the Periodic Table.






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






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






48. Simplest whole # ration of atoms in a compound






49. 5 valence electrons -3 ions - Nitride N






50. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds







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