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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. Simplest whole # ration of atoms in a compound
electron affinity
Octet Rule
Emperical Formula
und's rule
2. Property of the elements that can be predicted from the arrangement of the periodic table
Pauli exclusion principle
actinide series
periodic trends
Proton
3. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance C>>>>A+B
Ionization energy
Octet Rule
London forces
Decomposition reaction
4. Defined acids as subtsances that produced H ions in water - while bases produced OH ions. When they reacted together - H and OH neutralise to make water
Arrhenius Definition
Diffusion
azimuthal quantum number
Strong acid
5. States that if a stress is applied to a system at equilibrium - the system shifts in the direction that relieves the stress.
Henry's Law
Bronsted Lowry
Le chateliers Principle
Network covalent
6. The energy required to remove an electron from a gaseous atom; generally increases in moving from left - to - right across a period and decreases in moving down a group
Ionization energy
Rydberg constant
periodic trends
VSEPR
7. 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-
amorphous solid
Water dissociation Constant
Spin quantum number
energy state
8. Slightly less reactive than alkali metals - comprise group II
Equivalence point
Alkaline earths
Lewis acid base reaction
Net ionic equation
9. E=hc/?
Atomic weight
redox reaction
pi bonds
electromagnetic energy of photons emmited from electrons at ground state
10. Alkali metals: highly reactive - therefore always compounds. - 1 valence electron +1 ion - Hydrogen H? - Lithium Li? - Sodium Na? - Potassium K? - Rubidium Rb? - Cesium Cs?
Activation energy
Neutralization reaction
redox reaction
Group 1A
11. A concentration unit of a solution expressed as moles of solute dissolved per liter of solution
Theoretical yield
Conjugate acids and Bases
Molarity
Noble gases
12. A subdivision of an energy level in an atom. They are divided into orbitals.
subshell
periodic trends
molecular weight
Intermolecular forces
13. 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
lewis base
angular momentum in the bohr model
Raoult's Law
Dispersion Forces
14. Theory stating that the rate of a reaction is directly proportional to the number of collisions that take place between reactants per second.
quanta
Buffer
Collision theory of chemical Kinetics
atomic emission spectrum
15. In a solution - the substance that dissolves in the solvent
Strong acid
Solute
Concentration
Formula weight
16. A bond formed when two atomic orbitals combine to form a molecular orbital that is symmetrical around the axis connecting the two atomic nuclei
Ion dipole interactions
Solvent
sigma bond
angular momentum in the bohr model
17. (chemistry) a substance that changes color to indicate the presence of some ion or substance
crystalline solid
Reaction order
single displacement reaction
indicator
18. The process by which a gas escapes from one container to another at lower pressure through a tiny hole in the container.
Intermolecular forces
Chemical Kinetics
Effusion
Half equivalence point
19. A representation of a displacement reaction showing only the reactive species and omitting the spectator ions.
Net ionic equation
Hydrogen bonding
decomposition reaction
Water dissociation Constant
20. Numbers that specify the properties of atomic orbitals and of their electrons
atomic theory
quantum numbers
electrolysis
Rate law
21. PH=pka+log[base/acid] Used in titration based problems that relates the pH or pOH of a solution to the pK and the ratio of the dissociated species.
Effective nuclear charge
Henderson Hasselbalch Equation
Network covalent
Titration
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.
electron affinity
electrolysis
periodic trends
Neutralization reaction
23. 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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24. Tells you how much solute is present compared to the amount of solvent
Formal Charge
Concentration
Reaction mechanism
physical reaction
25. 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
Noble gases
quanta
hydrogen bonding
Bronsted Lowry
26. A chemical bond in which one atom loses an electron to form a positive ion and the other atom gains to electron to form a negative ion
Lewis acid base reaction
Electronegativity
Half equivalence point
Ionic Bond
27. 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
Solvent
und's rule
Percent yield
Colligative properties
28. The nuclear charge experienced by the outermost electrons of an atom (actual charge minus the shielding caused by inner shells: Z- eff)
Hydrogen bonding
Intermolecular forces
effective nuclear charge
Ionic Bond
29. A model of acids and bases which an acid is hydrogen ion donor and base is a hydrogen ion acceptor.
atomic emission spectrum
Alkaline earths
representative elements
Bronsted Lowry
30. The percent by mass of each element in a compound
gram equivalent weight
atomic radius
percent composition
Solute
31. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
redox reaction
Ion dipole interactions
Ion product
pH
32. Elements in the middle of the periodic table - in groups 3-12.
Vapor pressure
Planck's Constant
redox reaction
transition elements
33. A graph of pressure versus temperature that shows the conditions under which the phases of a substance exist
Magnetic quantum number
Conjugate acids and Bases
Lewis definition
Phase diagram
34. A dynamic condition in which two opposing changes occur at equal rates in a closed system
Octet Rule
Equilibrium
energy state
periodic trends
35. The ratio of the number of moles of solute dissolved in one kilogram of solvent. molality (M = moles solute/kg of solution)
Phase diagram
Molality
Bronsted - Lowry definition
Diprotic Base
36. 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
Phase diagram
lewis base
Pauli exclusion principle
37. Region in a molecule where atomic orbitals overlap - resulting in either a stable low - energy bonding orbital or an unstable high - energy antibonding orbital.
electrolysis
single displacement reaction
Molecular orbital
decomposition reaction
38. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance
decomposition reaction
Reaction mechanism
Half equivalence point
Combination Reaction
39. Contains nonmetals that are non - reactive. Full outermost energy level except helium which has 2.
Reaction mechanism
Lyman series
electron configuration
Noble gases
40. An emperimentally determined mathmatical expression showing the rate of a reaction as a function of the concentration of its reactants
Rate law
electrolysis
Triple point
bond energy
41. Common definition of acids as proton (H+) donors and bases as proton acceptors
Bronsted - Lowry definition
Formula weight
Octet Rule
percent composition
42. An atom or group of atoms that has a positive or negative charge
atomic theory
Halogens
Ion
quantum numbers
43. (chemistry) the sum of the relative atomic masses of the constituent atoms of a molecule
Halogens
molecular weight
Normality
Disproportionation
44. The sum of the exponents in a rate law - where each exponent provides the reaction order with respect to its reactants
Alkaline earths
Vapor pressure
Reaction order
Redox Half Reaction
45. 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.
Henderson Hasselbalch Equation
Ion product
Ion dipole interactions
redox reaction
46. (physics) the smallest discrete quantity of some physical property that a system can possess (according to quantum theory) E=hf
law of constant composition
quantum
Redox Half Reaction
ionic cmpound
47. Chalcogens - - Oxide O
physical reaction
Charles and Gay Lussac's Law
pi bonds
Group 6A
48. The formation of one or more covalent bonds between an electron pair donor and an electron pair acceptor
Spin quantum number
single displacement reaction
Lewis acid base reaction
Phase diagram
49. An acid that will completely dissociate in aqueous solution - like HCl - HI - HClO4 HBr.
Rate determining step
Strong acid
Amphoteric
sigma bond
50. A pair of equal and opposite electric charges or magnetic poles separated by a small distance
Titration
Dipole
Water dissociation Constant
Dispersion Forces