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MCAT Chemistry
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Subjects
:
mcat
,
science
Instructions:
Answer 50 questions in 15 minutes.
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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. Small discrete increments of energy.
Pauli exclusion principle
compound
quanta
Bronsted Lowry
2. Named after their cation and anion
electron affinity
Dipole Dipole interaction
Rydberg constant
ionic cmpound
3. Sum of all the masses - in AMU - present in one molecule of a molecular compound.
Formula weight
Colligative properties
STP
Reaction mechanism
4. The lowest allowable energy state of an atom
Concentration
azimuthal quantum number
Ground state
Dipole
5. Alkaline Earth Metals - 2 valence electrons +2 ions - Magnesium Mg
Group 2A
ionic cmpound
bond length
Group 6A
6. Redox reaction - in which the same species is both oxidized and reduced.
Aqueous Solution
Disproportionation
Lyman series
pI
7. 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
lathanide series
Solution equilibrium
Raoult's Law
Pauli exclusion principle
8. 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
Dipole
Equlibrium constant
Chemical Kinetics
Group 7A
9. Standard Temperature and Pressure. 273 Kelvin (0 Celsius) - 1 atmosphere (760 torr - 760 kPA).
theoretical yield
s orbital
STP
hydrogen bonding
10. A naturally occurring or synthetic compound consisting of large molecules made up of a linked series of repeated simple monomers
polymer
Group 6A
Spin quantum number
Avagadros number
11. 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.
ionic cmpound
d orbital
Lyman series
Balmer series
12. The amount of a substance that contains as many particles as there are atoms in exactly 12g of carbon -12
mole
Noble gases
Water dissociation Constant
VSEPR
13. Elements in the middle of the periodic table - in groups 3-12.
transition elements
Amphoteric
Lewis structure
Rydberg constant
14. Solids in which the particles are arranged in a repeating - 3- D pattern - has a specific melting point - classified as ionic network covalent - metallic or molecular.
crystalline solid
lathanide series
Ion
decomposition reaction
15. Property of the elements that can be predicted from the arrangement of the periodic table
actinide series
Lewis structure
Normality
periodic trends
16. (chemistry) the sum of the relative atomic masses of the constituent atoms of a molecule
VSEPR
molecular weight
Molecular orbital
Buffer
17. Numbers that specify the properties of atomic orbitals and of their electrons
quantum numbers
Formula weight
Amphoteric
heisenberg uncertainty principle
18. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
Net ionic equation
mole
Electrolyte
redox reaction
19. The average distance between the nuclei of two bonded atoms
percent composition
bond length
Phase diagram
Noble gases
20. An ionic compound that resists changes in its pH
Nucleus
Solute
sigma bond
Buffer
21. The slowest elementary step which is the limit for the rate of the other steps
Rate determining step
Combination Reaction
Intermolecular forces
molecular weight
22. A reaction in which atoms of one element take the place of atoms of another element in a compound
single displacement reaction
Formula weight
Titration
Lyman series
23. 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.
periodic trends
Group 1A
gram equivalent weight
Redox Half Reaction
24. The ways in which electrons are arranged in various orbitals around the nuclei of atoms
Mass number
electron configuration
Atomic weight
sigma bond
25. The point on a phase diagram that represents the only set of conditions at which all three phases exist in equilibrium with one another
Redox Half Reaction
quantum
Hydrogen bonding
Triple point
26. 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.
atomic radius
amorphous solid
STP
quantum
27. (chemistry) a substance formed by chemical union of two or more elements or ingredients in definite proportion by weight
compound
Ion
Lewis definition
chemical reaction
28. Common definition of acids as proton (H+) donors and bases as proton acceptors
Raoult's Law
Effective nuclear charge
Ionic Bond
Bronsted - Lowry definition
29. Chalcogens - - Oxide O
Acid dissociation constant
Group 6A
The bohr model
gram equivalent weight
30. 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
Effective nuclear charge
d orbital
representative elements
percent composition
31. The pressure exerted by a vapor in equilibrium with its liquid or solid phase
Vapor pressure
Ionic Bond
Group 3A
VSEPR
32. Theory stating that the rate of a reaction is directly proportional to the number of collisions that take place between reactants per second.
Collision theory of chemical Kinetics
Lyman series
Equlibrium constant
Neutron
33. Rare earth element group (elements 58-71)
Atomic weight
representative elements
Water dissociation Constant
lathanide series
34. In a solution - the substance that dissolves in the solvent
Disproportionation
Arrhenius Definition
Solute
Theoretical yield
35. The process of decomposing a chemical compound by the passage of an electric current.
electrolysis
Emperical Formula
Rydberg constant
Solution equilibrium
36. The formation of one or more covalent bonds between an electron pair donor and an electron pair acceptor
Percent yield
Hydrogen bonding
Equivalence point
Lewis acid base reaction
37. Gram equivalent weight of solute per liter of solution - often denoted by N.
electron configuration
Lewis definition
Nucleus
Normality
38. The nuclear charge experienced by the outermost electrons of an atom (actual charge minus the shielding caused by inner shells: Z- eff)
effective nuclear charge
Percent yield
Dipole Dipole interaction
Dispersion Forces
39. States that it is impossible to determine simultaneously both the position and momentum of an electron or any other particle
Redox Half Reaction
angular momentum in the bohr model
Bronsted - Lowry definition
heisenberg uncertainty principle
40. 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
Resonance structure
Effective nuclear charge
Ionic Bond
Group 7A
41. Atoms react by gaining or losing electrons so as to acquire the stable electron structure of a noble gas - usually eight valence electrons
single displacement reaction
Octet Rule
Principle quantum number
Proton
42. 2.18 x 10^-18 J/electron
Graham's Law
Rydberg constant
Effusion
Network covalent
43. The process by which a gas escapes from one container to another at lower pressure through a tiny hole in the container.
Effusion
d orbital
redox reaction
Solute
44. 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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45. Substance in which a solute is dissolved to form a solution
Decomposition reaction
pi bonds
redox reaction
Solvent
46. Sol - a chemical process in which solvent molecules and molecules or ions of the solute combine to form a compound
solvation
Group 3A
Alkaline earths
Bronsted - Lowry definition
47. 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.
lewis base
decomposition reaction
Network covalent
Ion product
48. (chemistry) a substance that changes color to indicate the presence of some ion or substance
Network covalent
atomic theory
molecular weight
indicator
49. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
Spin quantum number
Intermolecular forces
redox reaction
Group 3A
50. The percent by mass of each element in a compound
effective nuclear charge
representative elements
percent composition
Decomposition reaction
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