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Test your basic knowledge |
MCAT Chemistry
Start Test
Study First
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. 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-
Vapor pressure
atomic theory
d orbital
Water dissociation Constant
2. The weight in grams of compound that can be substituted by 1 atom of Hydrogen. GEW = MW / # of acidic Hyrdogens
Acid dissociation constant
atomic radius
gram equivalent weight
Solution equilibrium
3. (chemistry) the sum of the relative atomic masses of the constituent atoms of a molecule
representative elements
Solubility Product Constant
molecular weight
Ion dipole interactions
4. Chalcogens - - Oxide O
transition elements
lewis base
STP
Group 6A
5. When polar molecules orient themselves such that the positive region of one molecule is close to the negative region of another molecule.
Dipole Dipole interaction
Formula weight
Emperical Formula
Dispersion Forces
6. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance
law of constant composition
decomposition reaction
atomic theory
Henderson Hasselbalch Equation
7. PH of a molecule at which it contains no net electric charge - isoelectric point.
gram equivalent weight
sigma bond
indicator
pI
8. The process of decomposing a chemical compound by the passage of an electric current.
amorphous solid
Phase diagram
Aqueous Solution
electrolysis
9. Having characteristics of both an acid and a base and capable of reacting as either
Noble gases
Amphoteric
amorphous solid
d orbital
10. 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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11. The percent by mass of each element in a compound
Group 6A
percent composition
Rate determining step
decomposition reaction
12. 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
quanta
Group 6A
Spin quantum number
Rate law
13. The process by which a gas escapes from one container to another at lower pressure through a tiny hole in the container.
single displacement reaction
Effusion
Solvent
Alkaline earths
14. An atom - ion - or molecule that donates an electron pair to form a covalent bond.
Planck's Constant
empirical formula
lewis base
Solvent
15. A reaction in which atoms of one element take the place of atoms of another element in a compound
Solubility Product Constant
Network covalent
single displacement reaction
Lewis acid base reaction
16. The reaction of the ions that characterize acids and the ions that characterize bases to form water molecules and a salt
Neutralization reaction
law of constant composition
Atomic weight
Reaction mechanism
17. A substance that - when dissolved in water - results in a solution that can conduct electricity
gram equivalent weight
Ion product
Ground state
Electrolyte
18. Tells you how much solute is present compared to the amount of solvent
Electrolyte
Network covalent
Concentration
quantum
19. 5 valence electrons -3 ions - Nitride N
Phase diagram
d orbital
Group 5A
amorphous solid
20. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds
d orbital
Group 4A
quantum
Reaction mechanism
21. A reaction where a compound does Not change its molecular structure.
Proton
Triple point
Conjugate acids and Bases
physical reaction
22. Large molecular structures - strong covalent bonding - share qualities of IONIC And COVALENT
Azeotrope
subshell
Network covalent
electromagnetic energy of photons emmited from electrons at ground state
23. (chemistry) any theory in which all matter is composed of tiny discrete finite indivisible indestructible particles
atomic theory
Group 1A
Covalent Bond
Common ion effect
24. The point during a titration when the number of H+ ions and OH- ions are equal. This is at the middle of the steepest part of the titration curve.
Equivalence point
Ground state
Ionization energy
Azeotrope
25. A fundamental constant - h - that relates the energy of light quanta to their frequency: h = 6.6 X 10^-34 joule
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26. The molar amount of a solute that can dissolve in 1L of solvent until equilibrium - saturation - is reached
Atomic weight
Neutron
Equlibrium constant
Molar solubility
27. Rare earth element group (elements 58-71)
Resonance structure
Diprotic Base
lathanide series
energy state
28. 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.
Redox Half Reaction
sigma bond
Equilibrium
Balmer series
29. Region in a molecule where atomic orbitals overlap - resulting in either a stable low - energy bonding orbital or an unstable high - energy antibonding orbital.
amorphous solid
Molecular orbital
pI
bond energy
30. 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
Titration
Nucleus
azimuthal quantum number
Equivalence point
31. An uncharged molecule with a single unpaitred electron in its outer ring - very unstable - exists for only about 10 seconds
Rate law
atomic radius
Formal Charge
Free radical
32. The pressure exerted by a vapor in equilibrium with its liquid or solid phase
Vapor pressure
Henderson Hasselbalch Equation
Aqueous Solution
Conjugate acids and Bases
33. 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.
VSEPR
Principle quantum number
decomposition reaction
electron affinity
34. When dipoles are dissolved in a solution where ions are present ions wil arrange themselves with the opposite charged end of the dipole.
Intermolecular forces
Ion dipole interactions
Dispersion Forces
Molecular orbital
35. Property of the elements that can be predicted from the arrangement of the periodic table
pI
atomic radius
periodic trends
hydrogen bonding
36. 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.
angular momentum in the bohr model
single displacement reaction
Principle quantum number
Equivalence point
37. The Percent by mass of each element in a compound.
Alkaline earths
quantum
Formal Charge
Percent composition
38. The weight in grams of one mole of a given elementand is expressedin tems of grams per mole.
Dipole Dipole interaction
Atomic weight
quantum numbers
Network covalent
39. An atom - radical - or molecule that has gained or lost one or more electrons and has a negative or positive charge
Redox Half Reaction
Ion
Resonance structure
atomic theory
40. Redox reaction - in which the same species is both oxidized and reduced.
electron affinity
Disproportionation
Noble gases
Solution equilibrium
41. Alkaline Earth Metals - 2 valence electrons +2 ions - Magnesium Mg
Reaction order
atomic emission spectrum
Ion
Group 2A
42. The ratio of the actual yield to the theoretical yield for a chemical reaction expressed as a percentage; a measure of the efficiency of a reaction
Percent yield
Group 3A
und's rule
Buffer
43. (chemistry) p(otential of) H(ydrogen)
pH
Aqueous Solution
Nucleus
Lewis definition
44. The area of chemistry that is concerned with reaction rates and reaction mechanisms
Decomposition reaction
Chemical Kinetics
Nucleus
Noble gases
45. Alkali metals: highly reactive - therefore always compounds. - 1 valence electron +1 ion - Hydrogen H? - Lithium Li? - Sodium Na? - Potassium K? - Rubidium Rb? - Cesium Cs?
Lewis acid base reaction
Equivalence point
Group 1A
Reaction order
46. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
Atomic absorption Spectra
STP
redox reaction
crystalline solid
47. A representation of a displacement reaction showing only the reactive species and omitting the spectator ions.
Net ionic equation
Magnetic quantum number
Half equivalence point
molecular weight
48. Sum of all the masses - in AMU - present in one molecule of a molecular compound.
Formula weight
Ion product
decomposition reaction
quantum numbers
49. 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
Azeotrope
s orbital
Molar solubility
Resonance structure
50. An emperimentally determined mathmatical expression showing the rate of a reaction as a function of the concentration of its reactants
Alkaline earths
polymer
STP
Rate law