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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. Simplest whole # ration of atoms in a compound
Emperical Formula
Diffusion
ionic cmpound
Net ionic equation
2. The process by which one or more substances change to produce one or more different substances
Acid dissociation constant
gram equivalent weight
heisenberg uncertainty principle
chemical reaction
3. 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.
Colligative properties
atomic radius
Period
Ion product
4. Process by which molecules tend to move from an area where they are more concentrated to an area where they are less concentrated
gram equivalent weight
Electrolyte
single displacement reaction
Diffusion
5. Property of the elements that can be predicted from the arrangement of the periodic table
azimuthal quantum number
Charles and Gay Lussac's Law
periodic trends
law of constant composition
6. Theory stating that the rate of a reaction is directly proportional to the number of collisions that take place between reactants per second.
Ionic Bond
pI
Collision theory of chemical Kinetics
Planck's Constant
7. Slightly less reactive than alkali metals - comprise group II
electromagnetic energy of photons emmited from electrons at ground state
representative elements
Alkaline earths
Nonpolar covalent bond
8. The amount of product that can be made in a chemical reaction based on the amount of limiting reactant
bond length
Theoretical yield
Network covalent
Percent yield
9. A reaction in which atoms of one element take the place of atoms of another element in a compound
Molar solubility
Dipole Dipole interaction
molecule
single displacement reaction
10. 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
energy state
Free radical
Titration
Bronsted Lowry
11. The tendency for an atom to attract electrons to itself when it is chemically combined with another element
decomposition reaction
Electronegativity
hydrogen bonding
Period
12. A horizontal row of elements in the periodic table
Concentration
Lyman series
Water dissociation Constant
Period
13. 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
hydrogen bonding
Electrolyte
Formula weight
azimuthal quantum number
14. 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-
Network covalent
Water dissociation Constant
Principle quantum number
pI
15. The pressure exerted by a vapor in equilibrium with its liquid or solid phase
Graham's Law
quantum
Vapor pressure
bond length
16. 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
Le chateliers Principle
Equlibrium constant
heisenberg uncertainty principle
Group 7A
17. 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
Noble gases
d orbital
Lewis structure
Azeotrope
18. A subdivision of an energy level in an atom. They are divided into orbitals.
subshell
Group 2A
Bronsted - Lowry definition
Molality
19. 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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20. The number of atoms in exactly 12 g of pure 12c and equal to 6.022 x 10^23 is called
Avagadros number
Strong acid
Network covalent
Lewis structure
21. Systematic pairing of a deprotonated species (base) with its protonated form (conjugate acid). Conjugates appear on opposite sides of a chemical equation.
Free radical
Conjugate acids and Bases
Molecular orbital
Solution equilibrium
22. The nuclear charge experienced by the outermost electrons of an atom (actual charge minus the shielding caused by inner shells: Z- eff)
Azeotrope
ionic cmpound
effective nuclear charge
Half equivalence point
23. 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
angular momentum in the bohr model
Half equivalence point
Spin quantum number
Azeotrope
24. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance
Reaction order
decomposition reaction
Planck's Constant
Period
25. 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
Hydrogen bonding
und's rule
Ion
Ion
26. The amount of energy that reactants must absorb before a chemical reaction will start; also called free energy of activation.
Henry's Law
Activation energy
Network covalent
Molar solubility
27. The average distance between the nuclei of two bonded atoms
bond length
s orbital
atomic theory
Ion
28. 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.
Solubility Product Constant
Formula weight
Group 2A
electrolysis
29. The process by which a gas escapes from one container to another at lower pressure through a tiny hole in the container.
Molality
Solution equilibrium
Effusion
Chemical Kinetics
30. A set of frequencies of electromagnetic waves given off by atoms of an element; consists of a series of fine lines of individual colors
law of constant composition
Dipole
atomic emission spectrum
Nonpolar covalent bond
31. Alkali metals: highly reactive - therefore always compounds. - 1 valence electron +1 ion - Hydrogen H? - Lithium Li? - Sodium Na? - Potassium K? - Rubidium Rb? - Cesium Cs?
Dipole
mole
Group 1A
Period
32. 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
Dispersion Forces
Lewis acid base reaction
quantum
quantum numbers
33. A set of spectral lines that appear in the visible light region when a hydrogen atom undergoes a transition from energy levels n>2 to n=2.
chemical reaction
Molality
Balmer series
Pauli exclusion principle
34. When polar molecules orient themselves such that the positive region of one molecule is close to the negative region of another molecule.
Solution equilibrium
Dipole Dipole interaction
single displacement reaction
polymer
35. A representation of a displacement reaction showing only the reactive species and omitting the spectator ions.
polymer
Net ionic equation
Concentration
physical reaction
36. The weight in grams of compound that can be substituted by 1 atom of Hydrogen. GEW = MW / # of acidic Hyrdogens
Group 4A
Lewis structure
solvation
gram equivalent weight
37. Gram equivalent weight of solute per liter of solution - often denoted by N.
Raoult's Law
Magnetic quantum number
Normality
Group 2A
38. The lowest allowable energy state of an atom
Group 3A
Ground state
Activation energy
redox reaction
39. 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.
actinide series
Dipole Dipole interaction
Redox Half Reaction
redox reaction
40. 5 valence electrons -3 ions - Nitride N
Diprotic Base
Group 5A
Amphoteric
pi bonds
41. The molar amount of a solute that can dissolve in 1L of solvent until equilibrium - saturation - is reached
Lewis definition
Period
Percent yield
Molar solubility
42. A substance that - when dissolved in water - results in a solution that can conduct electricity
atomic radius
Electrolyte
Ground state
electron configuration
43. 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
angular momentum in the bohr model
Principle quantum number
s orbital
Molarity
44. A graph of pressure versus temperature that shows the conditions under which the phases of a substance exist
und's rule
Phase diagram
atomic emission spectrum
molecule
45. The weight in grams of one mole of a given elementand is expressedin tems of grams per mole.
molecular weight
STP
Atomic weight
quantum
46. An emperimentally determined mathmatical expression showing the rate of a reaction as a function of the concentration of its reactants
Rate law
electron affinity
Nonpolar covalent bond
pi bonds
47. The vapor pressure of solution is the product of the mole fraction of the solvent and the vapor pressure of the pure solvent. P_a=X_aP_total
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48. PH=pka+log[base/acid] Used in titration based problems that relates the pH or pOH of a solution to the pK and the ratio of the dissociated species.
Charles and Gay Lussac's Law
bond energy
Redox Half Reaction
Henderson Hasselbalch Equation
49. A chemical bond that involves sharing a pair of electrons between atoms in a molecule
Ground state
Covalent Bond
Lewis structure
Graham's Law
50. An uncharged molecule with a single unpaitred electron in its outer ring - very unstable - exists for only about 10 seconds
single displacement reaction
Dispersion Forces
Spin quantum number
Free radical