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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. 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
Rate law
representative elements
amorphous solid
2. No two electrons or protons or neutrons in a given system can be in states characterized by the same set of quantum numbers
Pauli exclusion principle
atomic theory
Bronsted - Lowry definition
compound
3. A naturally occurring or synthetic compound consisting of large molecules made up of a linked series of repeated simple monomers
decomposition reaction
polymer
Collision theory of chemical Kinetics
Solubility Product Constant
4. 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
Magnetic quantum number
Nucleus
Intermolecular forces
bond length
5. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds
Ion dipole interactions
Group 4A
Combination Reaction
Dipole Dipole interaction
6. The point on a phase diagram that represents the only set of conditions at which all three phases exist in equilibrium with one another
Triple point
Noble gases
empirical formula
Solubility Product Constant
7. Named after their cation and anion
Electrolyte
theoretical yield
und's rule
ionic cmpound
8. 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
VSEPR
hydrogen bonding
atomic radius
Acid dissociation constant
9. The area of chemistry that is concerned with reaction rates and reaction mechanisms
Vapor pressure
Chemical Kinetics
Phase diagram
Nucleus
10. In a solution - the substance that dissolves in the solvent
Effusion
Equivalence point
Solute
Diffusion
11. The weight in grams of compound that can be substituted by 1 atom of Hydrogen. GEW = MW / # of acidic Hyrdogens
Combination Reaction
pI
gram equivalent weight
single displacement reaction
12. (chemistry) a substance formed by chemical union of two or more elements or ingredients in definite proportion by weight
actinide series
Neutron
compound
pi bonds
13. An emperimentally determined mathmatical expression showing the rate of a reaction as a function of the concentration of its reactants
Combination Reaction
Spin quantum number
Reaction mechanism
Rate law
14. The molar solubility of one salt is reduced when another salt - having a common ion is brought into the same solution
decomposition reaction
Common ion effect
Acid dissociation constant
Alkaline earths
15. Attractive and repulsive forces between molecules that are weaker than forces within molecules.
Solute
Group 4A
Percent composition
Intermolecular forces
16. Region in a molecule where atomic orbitals overlap - resulting in either a stable low - energy bonding orbital or an unstable high - energy antibonding orbital.
Molecular orbital
Henderson Hasselbalch Equation
Resonance structure
Net ionic equation
17. PH of a molecule at which it contains no net electric charge - isoelectric point.
hydrogen bonding
Reaction mechanism
heisenberg uncertainty principle
pI
18. Specifies the specific orbital in which the electron is most likely to be found. - Third quantum number - designated as ml. Describes a particular orbital within a subshell where an electron is very likely to be found. Possible values are integers in
Equilibrium
Bronsted - Lowry definition
sigma bond
Magnetic quantum number
19. Numbers that specify the properties of atomic orbitals and of their electrons
Diffusion
Group 5A
Neutralization reaction
quantum numbers
20. A substance that - when dissolved in water - results in a solution that can conduct electricity
Ion
Mass number
electromagnetic energy of photons emmited from electrons at ground state
Electrolyte
21. An atom - ion - or molecule that donates an electron pair to form a covalent bond.
Ion product
atomic emission spectrum
Reaction order
lewis base
22. 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.
Redox Half Reaction
lathanide series
redox reaction
Group 6A
23. The ways in which electrons are arranged in various orbitals around the nuclei of atoms
electron configuration
Neutron
decomposition reaction
Molecular orbital
24. 2.18 x 10^-18 J/electron
Rydberg constant
lathanide series
Percent yield
energy state
25. 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-
Water dissociation Constant
Buffer
electron configuration
Formula weight
26. When dipoles are dissolved in a solution where ions are present ions wil arrange themselves with the opposite charged end of the dipole.
s orbital
Phase diagram
representative elements
Ion dipole interactions
27. The amount of energy that reactants must absorb before a chemical reaction will start; also called free energy of activation.
lewis base
Avagadros number
Activation energy
Solute
28. Sum of the protons and neutrons in an element often denoted by the letter A
Azeotrope
Dipole Dipole interaction
Mass number
Free radical
29. An atom or group of atoms that has a positive or negative charge
Solution equilibrium
Concentration
Nonpolar covalent bond
Ion
30. 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
azimuthal quantum number
single displacement reaction
Dispersion Forces
Acid dissociation constant
31. Gram equivalent weight of solute per liter of solution - often denoted by N.
Normality
Amphoteric
Colligative properties
azimuthal quantum number
32. 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
33. Side - to side parallel orbitals overlap to share electrons - the 2nd/3rd covalent bond between two atoms - cannot rotate and maintain the bond.
empirical formula
Concentration
pi bonds
Network covalent
34. Common definition of acids as proton (H+) donors and bases as proton acceptors
Henderson Hasselbalch Equation
Bronsted - Lowry definition
Halogens
Free radical
35. Property of the elements that can be predicted from the arrangement of the periodic table
Combination Reaction
Octet Rule
periodic trends
The bohr model
36. 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.
Ion product
Atomic weight
Group 3A
Amphoteric
37. Standard Temperature and Pressure. 273 Kelvin (0 Celsius) - 1 atmosphere (760 torr - 760 kPA).
pi bonds
Graham's Law
heisenberg uncertainty principle
STP
38. An atom - radical - or molecule that has gained or lost one or more electrons and has a negative or positive charge
Aqueous Solution
Ionic Bond
Ion
Percent yield
39. 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.
Magnetic quantum number
Equilibrium
Noble gases
electron affinity
40. A pair of equal and opposite electric charges or magnetic poles separated by a small distance
Dipole
Alkaline earths
Solution equilibrium
molecule
41. 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
Formula weight
Dispersion Forces
Rydberg constant
42. Small discrete increments of energy.
quanta
transition elements
Le chateliers Principle
s orbital
43. The maximum amount of product that can be produced from a given amount of reactant
Dipole Dipole interaction
lathanide series
theoretical yield
Bronsted Lowry
44. The formation of one or more covalent bonds between an electron pair donor and an electron pair acceptor
Octet Rule
Solvent
electron configuration
Lewis acid base reaction
45. 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
Principle quantum number
Proton
Electrolyte
Lewis acid base reaction
46. An acid that will completely dissociate in aqueous solution - like HCl - HI - HClO4 HBr.
Strong acid
Intermolecular forces
Ionization energy
Molecular orbital
47. An ionic compound that resists changes in its pH
Group 2A
Buffer
s orbital
electron configuration
48. Atoms react by gaining or losing electrons so as to acquire the stable electron structure of a noble gas - usually eight valence electrons
Aqueous Solution
theoretical yield
Octet Rule
Solution equilibrium
49. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
Aqueous Solution
Henderson Hasselbalch Equation
Rydberg constant
redox 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
London forces
electrolysis
Decomposition reaction
Lewis acid base reaction