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






2. 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.






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






4. An atom - radical - or molecule that has gained or lost one or more electrons and has a negative or positive charge






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






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






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






9. Contains nonmetals - 7 valence electrons in it's outermost energy level. Very reactive






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






11. 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.






12. Small discrete increments of energy.






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






14. (chemistry) a substance that changes color to indicate the presence of some ion or substance






15. 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






16. The process by which a gas escapes from one container to another at lower pressure through a tiny hole in the container.






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






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






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






20. 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.






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






22. An elementary particle with 0 charge and mass about equal to a proton






23. Named after their cation and anion






24. 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






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






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






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






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






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






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

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32. A measured amount of a solution of unknown concentration is added to a known volume of a second solution until the reaction between them is just complete






33. 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






34. 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






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






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






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






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






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






40. 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.






41. 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






42. 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






43. 2.18 x 10^-18 J/electron






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






45. 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.






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






47. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds






48. 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






49. The nuclear charge experienced by the outermost electrons of an atom (actual charge minus the shielding caused by inner shells: Z- eff)






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