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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. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
Free radical
redox reaction
empirical formula
energy state
2. 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.
Principle quantum number
law of constant composition
Molar solubility
Network covalent
3. Chalcogens - - Oxide O
Reaction order
Dispersion Forces
Principle quantum number
Group 6A
4. 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.
physical reaction
Rate law
compound
Ion product
5. A horizontal row of elements in the periodic table
quantum
Period
Ground state
Ion
6. A set of frequencies of electromagnetic waves given off by atoms of an element; consists of a series of fine lines of individual colors
Buffer
atomic emission spectrum
transition elements
Water dissociation Constant
7. States that if a stress is applied to a system at equilibrium - the system shifts in the direction that relieves the stress.
Solution equilibrium
und's rule
d orbital
Le chateliers Principle
8. Property of the elements that can be predicted from the arrangement of the periodic table
periodic trends
Graham's Law
Theoretical yield
compound
9. The tendency for an atom to attract electrons to itself when it is chemically combined with another element
Dispersion Forces
Electronegativity
quantum numbers
chemical reaction
10. 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
Bronsted - Lowry definition
hydrogen bonding
quanta
chemical reaction
11. A representation of a displacement reaction showing only the reactive species and omitting the spectator ions.
Net ionic equation
heisenberg uncertainty principle
ionic cmpound
transition elements
12. (chemistry) the sum of the relative atomic masses of the constituent atoms of a molecule
Water dissociation Constant
Diffusion
Decomposition reaction
molecular weight
13. 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
Combination Reaction
atomic emission spectrum
Azeotrope
electrolysis
14. Having characteristics of both an acid and a base and capable of reacting as either
Henderson Hasselbalch Equation
Decomposition reaction
und's rule
Amphoteric
15. 2.18 x 10^-18 J/electron
Diprotic Base
lathanide series
gram equivalent weight
Rydberg constant
16. 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.
Solution equilibrium
Phase diagram
lathanide series
crystalline solid
17. 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
theoretical yield
Formula weight
representative elements
Collision theory of chemical Kinetics
18. 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.
Normality
Ion product
Diprotic Base
electron affinity
19. 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.
lathanide series
Atomic absorption Spectra
Bronsted - Lowry definition
Theoretical yield
20. The lowest allowable energy state of an atom
Effective nuclear charge
Amphoteric
molecular weight
Ground state
21. The process by which one or more substances change to produce one or more different substances
single displacement reaction
quantum numbers
chemical reaction
Disproportionation
22. Second quantum number - designated by the letter 'l.' This 'angular momentum' refers to the subshells within each principle quantum energy level. It can take on the value of an integer in the 0 to (n -1) range. The four subshellscorresponding to l=0
azimuthal quantum number
Solubility Product Constant
Period
Henderson Hasselbalch Equation
23. The area of chemistry that is concerned with reaction rates and reaction mechanisms
Pauli exclusion principle
Avagadros number
Atomic weight
Chemical Kinetics
24. Sum of the protons and neutrons in an element often denoted by the letter A
Mass number
indicator
Solvent
Equlibrium constant
25. The amount of energy that reactants must absorb before a chemical reaction will start; also called free energy of activation.
Ion
Activation energy
Proton
Concentration
26. 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
Effective nuclear charge
Nucleus
Group 3A
und's rule
27. In a solution - the substance that dissolves in the solvent
Principle quantum number
single displacement reaction
Solute
Lyman series
28. Process by which molecules tend to move from an area where they are more concentrated to an area where they are less concentrated
Aqueous Solution
Azeotrope
mole
Diffusion
29. 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
Activation energy
Lewis definition
decomposition reaction
30. 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-
Combination Reaction
Water dissociation Constant
Ground state
Solution equilibrium
31. 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
Raoult's Law
Dipole
Group 1A
Spin quantum number
32. Alkali metals: highly reactive - therefore always compounds. - 1 valence electron +1 ion - Hydrogen H? - Lithium Li? - Sodium Na? - Potassium K? - Rubidium Rb? - Cesium Cs?
Conjugate acids and Bases
percent composition
Strong acid
Group 1A
33. The slowest elementary step which is the limit for the rate of the other steps
Rate determining step
Net ionic equation
compound
Electrolyte
34. Small discrete increments of energy.
Group 3A
quanta
Intermolecular forces
Molality
35. 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
Group 7A
Formal Charge
Ion dipole interactions
redox reaction
36. 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
Henry's Law
Titration
Dispersion Forces
electron configuration
37. Rare earth element group (elements 58-71)
Dispersion Forces
Atomic absorption Spectra
Lewis definition
lathanide series
38. An equilibrium expression used to measure weak - acid strength - given by the ratio of the product of the products' molar concentrations to the product of the reactants' molar concentrations - with each term raised to the power of its stoichiometric
Acid dissociation constant
Resonance structure
Group 4A
Emperical Formula
39. The point on a phase diagram that represents the only set of conditions at which all three phases exist in equilibrium with one another
Group 5A
Combination Reaction
Group 4A
Triple point
40. Elements in the middle of the periodic table - in groups 3-12.
atomic emission spectrum
Lyman series
transition elements
Group 7A
41. 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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42. (chemistry) any theory in which all matter is composed of tiny discrete finite indivisible indestructible particles
molecule
atomic theory
atomic emission spectrum
ionic cmpound
43. Named after their cation and anion
Redox Half Reaction
ionic cmpound
Rate law
Net ionic equation
44. Theory stating that the rate of a reaction is directly proportional to the number of collisions that take place between reactants per second.
Solvent
Ionization energy
Collision theory of chemical Kinetics
Effusion
45. The process of decomposing a chemical compound by the passage of an electric current.
Ion
electrolysis
Molar solubility
Bronsted - Lowry definition
46. A graph of pressure versus temperature that shows the conditions under which the phases of a substance exist
Phase diagram
Normality
bond length
Ion
47. 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
s orbital
atomic radius
Ionic Bond
Charles and Gay Lussac's Law
48. 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.
Ionization energy
Molality
lathanide series
atomic radius
49. A substance that - when dissolved in water - results in a solution that can conduct electricity
Electrolyte
quantum numbers
Half equivalence point
physical reaction
50. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance C>>>>A+B
Ion
Hydrogen bonding
Ion product
Decomposition reaction
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