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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. The molar solubility of one salt is reduced when another salt - having a common ion is brought into the same solution
Atomic absorption Spectra
Common ion effect
Charles and Gay Lussac's Law
Effective nuclear charge
2. 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
Rate determining step
representative elements
Disproportionation
Henry's Law
3. Sol - a chemical process in which solvent molecules and molecules or ions of the solute combine to form a compound
solvation
Group 5A
Planck's Constant
Covalent Bond
4. The formation of one or more covalent bonds between an electron pair donor and an electron pair acceptor
Group 4A
Colligative properties
Lewis acid base reaction
Electrolyte
5. 2.18 x 10^-18 J/electron
Lewis structure
Rydberg constant
Decomposition reaction
Ion
6. 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
atomic emission spectrum
hydrogen bonding
d orbital
s orbital
7. A reaction in which atoms of one element take the place of atoms of another element in a compound
single displacement reaction
Colligative properties
molecular weight
Amphoteric
8. 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
Electrolyte
Percent yield
Proton
Dipole
9. 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
actinide series
Network covalent
VSEPR
10. Tells you how much solute is present compared to the amount of solvent
physical reaction
angular momentum in the bohr model
Amphoteric
Concentration
11. One - half the distance between the nuclei of two atoms of the same element when the atoms are joined
Equivalence point
Lewis structure
Aqueous Solution
atomic radius
12. 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
Redox Half Reaction
Graham's Law
Titration
Rydberg constant
13. A definite stable energy that a physical system can have
Ground state
Rydberg constant
energy state
Phase diagram
14. A dynamic condition in which two opposing changes occur at equal rates in a closed system
Proton
Equilibrium
redox reaction
Bronsted - Lowry definition
15. When polar molecules orient themselves such that the positive region of one molecule is close to the negative region of another molecule.
Resonance structure
Dipole Dipole interaction
energy state
bond length
16. Gram equivalent weight of solute per liter of solution - often denoted by N.
Titration
Pauli exclusion principle
Bronsted - Lowry definition
Normality
17. 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.
Effusion
Redox Half Reaction
Equlibrium constant
single displacement reaction
18. The percent by mass of each element in a compound
Aqueous Solution
percent composition
Raoult's Law
polymer
19. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
redox reaction
actinide series
Theoretical yield
Conjugate acids and Bases
20. The molar amount of a solute that can dissolve in 1L of solvent until equilibrium - saturation - is reached
Molar solubility
Resonance structure
Atomic absorption Spectra
Noble gases
21. In a solution - the substance that dissolves in the solvent
Group 1A
Solute
Formula weight
Atomic absorption Spectra
22. The ratio of the number of moles of solute dissolved in one kilogram of solvent. molality (M = moles solute/kg of solution)
Activation energy
Solution equilibrium
Molality
Molarity
23. At a constant pressure - the volume of an ideal gas is directly proportinal to its temperature: V (a) T
24. Set of spectral lines appearing in the UV region when a hydrogen atom undergoes a transition from energy levels n>1 to n=1.
Lyman series
Conjugate acids and Bases
Reaction order
Covalent Bond
25. No two electrons or protons or neutrons in a given system can be in states characterized by the same set of quantum numbers
Ion dipole interactions
Pauli exclusion principle
Phase diagram
Percent composition
26. The point during a titration when the number of H+ ions and OH- ions are equal. This is at the middle of the steepest part of the titration curve.
molecular weight
Spin quantum number
Equivalence point
Activation energy
27. 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
Normality
Molar solubility
Magnetic quantum number
Activation energy
28. 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.
Balmer series
Diprotic Base
Alkaline earths
Molecular orbital
29. Play- by- play showing the individual steps of a reaction - including the formation and destruction of any reaction intermediates that may occur.
Titration
Mass number
Triple point
Reaction mechanism
30. The pressure exerted by a vapor in equilibrium with its liquid or solid phase
Vapor pressure
Molarity
Triple point
energy state
31. The nuclear charge experienced by the outermost electrons of an atom (actual charge minus the shielding caused by inner shells: Z- eff)
Colligative properties
effective nuclear charge
Effusion
Alkaline earths
32. The tendency for an atom to attract electrons to itself when it is chemically combined with another element
crystalline solid
Electronegativity
Strong acid
Phase diagram
33. A pair of equal and opposite electric charges or magnetic poles separated by a small distance
energy state
Neutralization reaction
representative elements
Dipole
34. Simplest whole # ration of atoms in a compound
Nucleus
Emperical Formula
atomic radius
Neutron
35. A base that can accept two moles of H+ per mole of itself (ex: SO4
Diprotic Base
Net ionic equation
Principle quantum number
Bronsted Lowry
36. Alkaline Earth Metals - 2 valence electrons +2 ions - Magnesium Mg
Emperical Formula
Group 2A
Acid dissociation constant
Net ionic equation
37. Having characteristics of both an acid and a base and capable of reacting as either
quantum
Amphoteric
Normality
Concentration
38. 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 Bond
Conjugate acids and Bases
chemical reaction
39. 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
Rate law
empirical formula
Lewis acid base reaction
Spin quantum number
40. 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.
physical reaction
Reaction mechanism
Solubility Product Constant
Diffusion
41. Contains nonmetals that are non - reactive. Full outermost energy level except helium which has 2.
Disproportionation
Noble gases
Lewis acid base reaction
Solute
42. Elements in the middle of the periodic table - in groups 3-12.
transition elements
Conjugate acids and Bases
Nonpolar covalent bond
mole
43. 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
Hydrogen bonding
Resonance structure
Percent yield
Colligative properties
44. The process by which a gas escapes from one container to another at lower pressure through a tiny hole in the container.
periodic trends
Effusion
sigma bond
Concentration
45. 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
Titration
Azeotrope
polymer
hydrogen bonding
46. A subdivision of an energy level in an atom. They are divided into orbitals.
subshell
Percent composition
Molarity
Solubility Product Constant
47. Valence Shell Electron Pair Repulsion theory - stating that the three - dimensional molecular geometry about some central atom is determined by the elctronic repulsion between its bonding and nonbonding electron pairs.
periodic trends
Dipole Dipole interaction
electron configuration
VSEPR
48. (physics) the smallest discrete quantity of some physical property that a system can possess (according to quantum theory) E=hf
Azeotrope
Bronsted - Lowry definition
quantum
STP
49. The number of atoms in exactly 12 g of pure 12c and equal to 6.022 x 10^23 is called
Avagadros number
Graham's Law
electrolysis
compound
50. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
Halogens
redox reaction
physical reaction
Diprotic Base