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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 emperimentally determined mathmatical expression showing the rate of a reaction as a function of the concentration of its reactants
Rate law
Molecular orbital
s orbital
electron configuration
2. The amount of a substance that contains as many particles as there are atoms in exactly 12g of carbon -12
mole
Solute
Equlibrium constant
molecule
3. The ratio of the actual yield to the theoretical yield for a chemical reaction expressed as a percentage; a measure of the efficiency of a reaction
Group 6A
Covalent Bond
amorphous solid
Percent yield
4. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance C>>>>A+B
Decomposition reaction
electrolysis
Free radical
Vapor pressure
5. The process of decomposing a chemical compound by the passage of an electric current.
heisenberg uncertainty principle
electrolysis
Activation energy
Rydberg constant
6. Standard Temperature and Pressure. 273 Kelvin (0 Celsius) - 1 atmosphere (760 torr - 760 kPA).
STP
atomic theory
Azeotrope
effective nuclear charge
7. 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
8. The ratio of the number of moles of solute dissolved in one kilogram of solvent. molality (M = moles solute/kg of solution)
polymer
Molality
Normality
Henry's Law
9. Process by which molecules tend to move from an area where they are more concentrated to an area where they are less concentrated
Diffusion
Neutron
atomic radius
Atomic absorption Spectra
10. 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
Equilibrium
atomic radius
Resonance structure
Group 7A
11. Simplest whole # ration of atoms in a compound
Bronsted Lowry
single displacement reaction
law of constant composition
Emperical Formula
12. Substance in which a solute is dissolved to form a solution
Solute
Solvent
Effusion
The bohr model
13. Play- by- play showing the individual steps of a reaction - including the formation and destruction of any reaction intermediates that may occur.
Noble gases
Charles and Gay Lussac's Law
Reaction mechanism
bond energy
14. 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.
azimuthal quantum number
Atomic absorption Spectra
Lewis structure
indicator
15. The percent by mass of each element in a compound
periodic trends
amorphous solid
Equilibrium
percent composition
16. 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
London forces
Hydrogen bonding
Electronegativity
Colligative properties
17. A structural formula in which electrons are represented by dots; dot pairs or dashes between two atomic symbols represent pairs in covalent bonds.
Combination Reaction
Lewis structure
representative elements
Ionization energy
18. A base that can accept two moles of H+ per mole of itself (ex: SO4
Group 5A
redox reaction
Disproportionation
Diprotic Base
19. 5 valence electrons -3 ions - Nitride N
Lewis acid base reaction
Neutron
Group 5A
electron configuration
20. 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-
Atomic weight
Water dissociation Constant
Atomic absorption Spectra
percent composition
21. Chalcogens - - Oxide O
physical reaction
Neutron
Group 6A
Triple point
22. 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.
Pauli exclusion principle
gram equivalent weight
electron affinity
Redox Half Reaction
23. 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
Magnetic quantum number
bond length
hydrogen bonding
polymer
24. Common definition of acids as proton (H+) donors and bases as proton acceptors
Reaction order
Bronsted - Lowry definition
molecule
Ion product
25. Any sample of a given compound will contain the same elements in the identical mass ratio.
Electrolyte
chemical reaction
law of constant composition
Reaction mechanism
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
s orbital
Le chateliers Principle
Nucleus
Phase diagram
27. 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
heisenberg uncertainty principle
Diffusion
Equlibrium constant
Molality
28. A model of acids and bases which an acid is hydrogen ion donor and base is a hydrogen ion acceptor.
Alkaline earths
Le chateliers Principle
molecular weight
Bronsted Lowry
29. The area of chemistry that is concerned with reaction rates and reaction mechanisms
atomic emission spectrum
Chemical Kinetics
indicator
Le chateliers Principle
30. 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.
Net ionic equation
Diffusion
heisenberg uncertainty principle
Solubility Product Constant
31. (chemistry) a series from actinium to lawrencium of 15 radioactive elements with increasing atomic numbers
actinide series
Acid dissociation constant
Group 3A
Buffer
32. A subdivision of an energy level in an atom. They are divided into orbitals.
Common ion effect
Group 6A
subshell
Principle quantum number
33. 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
Magnetic quantum number
Equlibrium constant
Effective nuclear charge
molecular weight
34. 1913 - Niels Bohr - said that electrons formed specific layers instead or random ones - said atoms atoms absorb and give off energy when the electrons move from one shell to another
The bohr model
Ion product
Solubility Product Constant
quanta
35. The weight in grams of compound that can be substituted by 1 atom of Hydrogen. GEW = MW / # of acidic Hyrdogens
solvation
Aqueous Solution
gram equivalent weight
Phase diagram
36. A reaction where a compound does Not change its molecular structure.
physical reaction
Arrhenius Definition
Redox Half Reaction
Le chateliers Principle
37. Numbers that specify the properties of atomic orbitals and of their electrons
angular momentum in the bohr model
quantum numbers
solvation
Dipole
38. 5 different orbitals shaped like clover leaves and max electrons is 10
d orbital
Decomposition reaction
quantum numbers
Reaction order
39. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
redox reaction
Solution equilibrium
Effusion
electron affinity
40. The Percent by mass of each element in a compound.
Emperical Formula
molecular weight
energy state
Percent composition
41. Rare earth element group (elements 58-71)
periodic trends
Magnetic quantum number
Percent yield
lathanide series
42. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds
Nucleus
Group 4A
Vapor pressure
VSEPR
43. A chemical formula showing the ratio of elements in a compound rather than the total number of atoms
crystalline solid
Water dissociation Constant
empirical formula
atomic radius
44. A pair of equal and opposite electric charges or magnetic poles separated by a small distance
Noble gases
Ionic Bond
Dipole
Hydrogen bonding
45. The lowest allowable energy state of an atom
London forces
Bronsted Lowry
Ground state
Group 7A
46. 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
Diffusion
s orbital
Free radical
47. The sum of the exponents in a rate law - where each exponent provides the reaction order with respect to its reactants
Reaction order
hydrogen bonding
actinide series
Half equivalence point
48. States that it is impossible to determine simultaneously both the position and momentum of an electron or any other particle
Atomic absorption Spectra
heisenberg uncertainty principle
hydrogen bonding
atomic emission spectrum
49. 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.
Atomic weight
crystalline solid
Arrhenius Definition
azimuthal quantum number
50. A reaction in which atoms of one element take the place of atoms of another element in a compound
single displacement reaction
effective nuclear charge
Molarity
Vapor pressure