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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. 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
Group 5A
Group 1A
Acid dissociation constant
atomic radius
2. The weight in grams of one mole of a given elementand is expressedin tems of grams per mole.
Equivalence point
Atomic weight
empirical formula
Proton
3. 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.
molecular weight
atomic radius
Rate determining step
Diffusion
4. A subatomic particle that has a positive charge and that is found in the nucleus of an atom Charge of +1 and mass of 1.0073 amu
Proton
VSEPR
Avagadros number
London forces
5. A physical property of a solution that depends on the number - but not the identity - of the disswolved solute particles; example properties include vapor pressure lowering - boiling point elevation - osmotic pressure - and frezzing point depression
quantum numbers
Effective nuclear charge
Colligative properties
Nucleus
6. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
lathanide series
azimuthal quantum number
redox reaction
Emperical Formula
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
percent composition
quantum numbers
Solution equilibrium
subshell
8. A chemical bond that involves sharing a pair of electrons between atoms in a molecule
Equlibrium constant
Covalent Bond
Solvent
Percent yield
9. 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
Nucleus
ionic cmpound
Lewis acid base reaction
Covalent Bond
10. The Percent by mass of each element in a compound.
Solution equilibrium
VSEPR
Percent composition
empirical formula
11. 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
STP
hydrogen bonding
indicator
angular momentum in the bohr model
12. 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
Lyman series
Resonance structure
Ionization energy
Period
13. Region in a molecule where atomic orbitals overlap - resulting in either a stable low - energy bonding orbital or an unstable high - energy antibonding orbital.
Charles and Gay Lussac's Law
lewis base
Molecular orbital
Rate law
14. Play- by- play showing the individual steps of a reaction - including the formation and destruction of any reaction intermediates that may occur.
molecular weight
Acid dissociation constant
Reaction mechanism
Concentration
15. The amount of energy that reactants must absorb before a chemical reaction will start; also called free energy of activation.
atomic emission spectrum
Activation energy
Molecular orbital
redox reaction
16. An uncharged molecule with a single unpaitred electron in its outer ring - very unstable - exists for only about 10 seconds
Atomic absorption Spectra
energy state
Free radical
Nonpolar covalent bond
17. A reaction in which two or more substances combine to form a single substance A+B>>>>>>>C
Combination Reaction
Group 3A
Collision theory of chemical Kinetics
gram equivalent weight
18. Orbitals of equal energy are each occupied by one electron before any orbital is occupied by a second electron - and all electrons in singly occupied orbitals must have the same spin
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19. Redox reaction - in which the same species is both oxidized and reduced.
The bohr model
Disproportionation
Acid dissociation constant
Redox Half Reaction
20. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
Molecular orbital
Reaction order
Aqueous Solution
redox reaction
21. 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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22. 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
Disproportionation
Group 3A
Rate law
Titration
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.
Triple point
Vapor pressure
Mass number
Redox Half Reaction
24. An atom - ion - or molecule that donates an electron pair to form a covalent bond.
lewis base
decomposition reaction
Equilibrium
Rate determining step
25. 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.
amorphous solid
Combination Reaction
electron affinity
Colligative properties
26. A reaction in which atoms of one element take the place of atoms of another element in a compound
Group 2A
Nonpolar covalent bond
Water dissociation Constant
single displacement reaction
27. A horizontal row of elements in the periodic table
und's rule
Period
empirical formula
Atomic absorption Spectra
28. Having characteristics of both an acid and a base and capable of reacting as either
Covalent Bond
Ion dipole interactions
Amphoteric
Acid dissociation constant
29. Chalcogens - - Oxide O
electron configuration
Group 6A
Disproportionation
molecule
30. A dynamic condition in which two opposing changes occur at equal rates in a closed system
Equilibrium
Molarity
redox reaction
Percent yield
31. 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
Bronsted - Lowry definition
Normality
Group 1A
Equlibrium constant
32. (chemistry) any theory in which all matter is composed of tiny discrete finite indivisible indestructible particles
empirical formula
atomic theory
Raoult's Law
Molarity
33. One - half the distance between the nuclei of two atoms of the same element when the atoms are joined
Balmer series
pi bonds
atomic radius
Octet Rule
34. 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.
Group 6A
Group 5A
gram equivalent weight
Principle quantum number
35. Rare earth element group (elements 58-71)
Ion
lathanide series
Azeotrope
Percent composition
36. The slowest elementary step which is the limit for the rate of the other steps
Balmer series
Net ionic equation
Ionization energy
Rate determining step
37. The amount of product that can be made in a chemical reaction based on the amount of limiting reactant
Azeotrope
Theoretical yield
Principle quantum number
Amphoteric
38. Common definition of acids as proton (H+) donors and bases as proton acceptors
Collision theory of chemical Kinetics
Rydberg constant
Bronsted - Lowry definition
compound
39. A graph of pressure versus temperature that shows the conditions under which the phases of a substance exist
Phase diagram
single displacement reaction
Free radical
Principle quantum number
40. An ionic compound that resists changes in its pH
Emperical Formula
Molarity
Group 2A
Buffer
41. Theory stating that the rate of a reaction is directly proportional to the number of collisions that take place between reactants per second.
Ion dipole interactions
Collision theory of chemical Kinetics
Solubility Product Constant
electron configuration
42. The pressure exerted by a vapor in equilibrium with its liquid or solid phase
Vapor pressure
STP
Net ionic equation
quantum
43. 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.
Alkaline earths
Atomic absorption Spectra
molecular weight
Halogens
44. Acids defined as electron - pair acceptors and bases as electron - pair donors.
electron configuration
Pauli exclusion principle
Solvent
Lewis definition
45. An elementary particle with 0 charge and mass about equal to a proton
law of constant composition
Ground state
Neutron
Group 1A
46. A solid made up of particles that are not arranged in a regular pattern.
crystalline solid
Solution equilibrium
amorphous solid
Atomic absorption Spectra
47. Named after their cation and anion
ionic cmpound
Phase diagram
sigma bond
Colligative properties
48. 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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49. 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
effective nuclear charge
Nucleus
STP
Hydrogen bonding
50. (chemistry) the sum of the relative atomic masses of the constituent atoms of a molecule
angular momentum in the bohr model
molecular weight
electron configuration
transition elements