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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. E=hc/?
Arrhenius Definition
heisenberg uncertainty principle
electromagnetic energy of photons emmited from electrons at ground state
Titration
2. The pressure exerted by a vapor in equilibrium with its liquid or solid phase
Proton
Equilibrium
lathanide series
Vapor pressure
3. A concentration unit of a solution expressed as moles of solute dissolved per liter of solution
Molarity
Group 4A
Group 1A
Normality
4. 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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5. Elements in the middle of the periodic table - in groups 3-12.
Nonpolar covalent bond
Network covalent
transition elements
Le chateliers Principle
6. Sol - a chemical process in which solvent molecules and molecules or ions of the solute combine to form a compound
pH
Decomposition reaction
solvation
theoretical yield
7. The Percent by mass of each element in a compound.
pH
Solubility Product Constant
Percent composition
electron affinity
8. Two or more atoms held together by covalent bonds
Planck's Constant
molecule
Ion product
pI
9. Standard Temperature and Pressure. 273 Kelvin (0 Celsius) - 1 atmosphere (760 torr - 760 kPA).
STP
Group 6A
percent composition
Covalent Bond
10. Set of spectral lines appearing in the UV region when a hydrogen atom undergoes a transition from energy levels n>1 to n=1.
Ion dipole interactions
Lyman series
Net ionic equation
Formula weight
11. In a solution - the substance that dissolves in the solvent
Solute
Avagadros number
empirical formula
mole
12. A graph of pressure versus temperature that shows the conditions under which the phases of a substance exist
Phase diagram
Group 6A
Ionic Bond
Period
13. Sum of all the masses - in AMU - present in one molecule of a molecular compound.
mole
bond energy
Formula weight
Decomposition reaction
14. PH of a molecule at which it contains no net electric charge - isoelectric point.
single displacement reaction
Colligative properties
Atomic absorption Spectra
pI
15. Nh/2p The angular momentum changes only in discete amounts with respect to the quantum number. Also E=- R_h/n^2
Ion
Equilibrium
angular momentum in the bohr model
Disproportionation
16. Any sample of a given compound will contain the same elements in the identical mass ratio.
Rate determining step
amorphous solid
Percent yield
law of constant composition
17. 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
Normality
Spin quantum number
Nucleus
compound
18. Chalcogens - - Oxide O
Group 6A
Alkaline earths
und's rule
polymer
19. A solid made up of particles that are not arranged in a regular pattern.
Effective nuclear charge
amorphous solid
Noble gases
Water dissociation Constant
20. Slightly less reactive than alkali metals - comprise group II
bond length
Phase diagram
Lewis acid base reaction
Alkaline earths
21. 5 valence electrons -3 ions - Nitride N
Bronsted - Lowry definition
Group 5A
actinide series
Molarity
22. Having characteristics of both an acid and a base and capable of reacting as either
Triple point
Magnetic quantum number
Ion product
Amphoteric
23. 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
Ionization energy
Solution equilibrium
Raoult's Law
Dipole Dipole interaction
24. A substance that - when dissolved in water - results in a solution that can conduct electricity
Electronegativity
Electrolyte
Molar solubility
Molecular orbital
25. (chemistry) a substance formed by chemical union of two or more elements or ingredients in definite proportion by weight
electron configuration
Triple point
Dipole
compound
26. 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.
Equivalence point
The bohr model
single displacement reaction
Solubility Product Constant
27. Simplest whole # ration of atoms in a compound
Octet Rule
Activation energy
Emperical Formula
Atomic weight
28. A naturally occurring or synthetic compound consisting of large molecules made up of a linked series of repeated simple monomers
und's rule
polymer
Group 6A
pH
29. The process by which one or more substances change to produce one or more different substances
Diffusion
Molarity
d orbital
chemical reaction
30. States that it is impossible to determine simultaneously both the position and momentum of an electron or any other particle
heisenberg uncertainty principle
Percent composition
Equlibrium constant
Mass number
31. The weight in grams of compound that can be substituted by 1 atom of Hydrogen. GEW = MW / # of acidic Hyrdogens
physical reaction
theoretical yield
quanta
gram equivalent weight
32. Atoms react by gaining or losing electrons so as to acquire the stable electron structure of a noble gas - usually eight valence electrons
atomic emission spectrum
Nucleus
molecule
Octet Rule
33. The point on a phase diagram that represents the only set of conditions at which all three phases exist in equilibrium with one another
Magnetic quantum number
Percent composition
subshell
Triple point
34. An atom or group of atoms that has a positive or negative charge
Ion
Planck's Constant
Lewis acid base reaction
Formal Charge
35. Property of the elements that can be predicted from the arrangement of the periodic table
periodic trends
Combination Reaction
Buffer
Group 3A
36. A subdivision of an energy level in an atom. They are divided into orbitals.
bond energy
Decomposition reaction
Ion product
subshell
37. Gram equivalent weight of solute per liter of solution - often denoted by N.
Equilibrium
Buffer
effective nuclear charge
Normality
38. Attractive and repulsive forces between molecules that are weaker than forces within molecules.
atomic theory
Intermolecular forces
Group 2A
Colligative properties
39. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance C>>>>A+B
Charles and Gay Lussac's Law
Decomposition reaction
Free radical
Phase diagram
40. 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
mole
Solution equilibrium
Phase diagram
Magnetic quantum number
41. Temperature is constant; effusion and temperature are proportional to the square root of their masses
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42. The weak attractive forces between molecules resulting from the small - instantaneous dipoles that occur because of the varying positions of the electrons during their motion about nuclei
Buffer
Solute
London forces
Graham's Law
43. An emperimentally determined mathmatical expression showing the rate of a reaction as a function of the concentration of its reactants
pH
effective nuclear charge
Rate law
Azeotrope
44. Large molecular structures - strong covalent bonding - share qualities of IONIC And COVALENT
und's rule
Period
single displacement reaction
Network covalent
45. An uncharged molecule with a single unpaitred electron in its outer ring - very unstable - exists for only about 10 seconds
Effusion
Free radical
Intermolecular forces
angular momentum in the bohr model
46. At a constant pressure - the volume of an ideal gas is directly proportinal to its temperature: V (a) T
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47. The weight in grams of one mole of a given elementand is expressedin tems of grams per mole.
Ionic Bond
Atomic weight
Lewis definition
amorphous solid
48. 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.
Proton
Group 3A
Neutralization reaction
Rydberg constant
49. Alkaline Earth Metals - 2 valence electrons +2 ions - Magnesium Mg
Spin quantum number
Group 2A
Halogens
Conjugate acids and Bases
50. 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
atomic radius
Dispersion Forces
electrolysis
Molar solubility