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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. Elements in the middle of the periodic table - in groups 3-12.
Group 3A
Collision theory of chemical Kinetics
transition elements
Planck's Constant
2. The Percent by mass of each element in a compound.
pi bonds
Principle quantum number
Arrhenius Definition
Percent composition
3. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance
molecule
sigma bond
decomposition reaction
Henderson Hasselbalch Equation
4. The slowest elementary step which is the limit for the rate of the other steps
pI
theoretical yield
physical reaction
Rate determining step
5. (chemistry) any theory in which all matter is composed of tiny discrete finite indivisible indestructible particles
Graham's Law
atomic theory
Reaction order
single displacement reaction
6. A naturally occurring or synthetic compound consisting of large molecules made up of a linked series of repeated simple monomers
polymer
Molarity
Conjugate acids and Bases
Group 2A
7. A representation of a displacement reaction showing only the reactive species and omitting the spectator ions.
Group 6A
compound
Net ionic equation
Water dissociation Constant
8. The pressure exerted by a vapor in equilibrium with its liquid or solid phase
Vapor pressure
Lewis structure
Amphoteric
Reaction order
9. Attractive and repulsive forces between molecules that are weaker than forces within molecules.
hydrogen bonding
polymer
Principle quantum number
Intermolecular forces
10. 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
Triple point
Graham's Law
lewis base
Dispersion Forces
11. 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
percent composition
Group 7A
Lewis definition
Acid dissociation constant
12. An ionic compound that resists changes in its pH
Balmer series
hydrogen bonding
Equivalence point
Buffer
13. Having characteristics of both an acid and a base and capable of reacting as either
Redox Half Reaction
single displacement reaction
Amphoteric
Percent composition
14. States that if a stress is applied to a system at equilibrium - the system shifts in the direction that relieves the stress.
redox reaction
indicator
Rydberg constant
Le chateliers Principle
15. A definite stable energy that a physical system can have
energy state
indicator
Octet Rule
Free radical
16. 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
Electrolyte
atomic radius
azimuthal quantum number
Balmer series
17. The number of atoms in exactly 12 g of pure 12c and equal to 6.022 x 10^23 is called
quantum
Avagadros number
Reaction mechanism
ionic cmpound
18. 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.
Covalent Bond
indicator
quantum
Henderson Hasselbalch Equation
19. Set of spectral lines appearing in the UV region when a hydrogen atom undergoes a transition from energy levels n>1 to n=1.
Dipole
Azeotrope
Acid dissociation constant
Lyman series
20. An atom or group of atoms that has a positive or negative charge
Ion
Formal Charge
Amphoteric
effective nuclear charge
21. 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
Atomic weight
Spin quantum number
molecular weight
Lewis acid base reaction
22. 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
Combination Reaction
Hydrogen bonding
Pauli exclusion principle
Group 7A
23. An acid that will completely dissociate in aqueous solution - like HCl - HI - HClO4 HBr.
pi bonds
Strong acid
Halogens
Raoult's Law
24. The process by which one or more substances change to produce one or more different substances
Colligative properties
chemical reaction
redox reaction
Percent composition
25. An atom - radical - or molecule that has gained or lost one or more electrons and has a negative or positive charge
Redox Half Reaction
Molality
Ion
Effective nuclear charge
26. 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-
Molarity
Formal Charge
Proton
Water dissociation Constant
27. Named after their cation and anion
Solubility Product Constant
bond energy
ionic cmpound
redox reaction
28. E=hc/?
Free radical
electromagnetic energy of photons emmited from electrons at ground state
effective nuclear charge
law of constant composition
29. 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
compound
Nonpolar covalent bond
Solution equilibrium
Network covalent
30. Standard Temperature and Pressure. 273 Kelvin (0 Celsius) - 1 atmosphere (760 torr - 760 kPA).
Mass number
redox reaction
electrolysis
STP
31. A covalent bond in which the bonding electrons are shared equally by the bonded atoms - resulting in a balanced distribution of electrical charge
Ionic Bond
Nonpolar covalent bond
Ion product
hydrogen bonding
32. (physics) the smallest discrete quantity of some physical property that a system can possess (according to quantum theory) E=hf
Common ion effect
Principle quantum number
law of constant composition
quantum
33. Alkali metals: highly reactive - therefore always compounds. - 1 valence electron +1 ion - Hydrogen H? - Lithium Li? - Sodium Na? - Potassium K? - Rubidium Rb? - Cesium Cs?
Group 1A
Molecular orbital
atomic radius
molecular weight
34. Rare earth element group (elements 58-71)
lathanide series
Le chateliers Principle
Lewis structure
quantum numbers
35. No two electrons or protons or neutrons in a given system can be in states characterized by the same set of quantum numbers
empirical formula
compound
Titration
Pauli exclusion principle
36. 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
Free radical
Arrhenius Definition
Reaction order
Group 5A
37. Process by which molecules tend to move from an area where they are more concentrated to an area where they are less concentrated
Solubility Product Constant
sigma bond
Aqueous Solution
Diffusion
38. An atom - ion - or molecule that donates an electron pair to form a covalent bond.
lewis base
lathanide series
Planck's Constant
Electronegativity
39. The percent by mass of each element in a compound
percent composition
decomposition reaction
Solution equilibrium
angular momentum in the bohr model
40. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
redox reaction
molecular weight
Group 4A
single displacement reaction
41. Tells you how much solute is present compared to the amount of solvent
Hydrogen bonding
Dispersion Forces
Vapor pressure
Concentration
42. 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.
Disproportionation
Raoult's Law
Equivalence point
Buffer
43. When dipoles are dissolved in a solution where ions are present ions wil arrange themselves with the opposite charged end of the dipole.
pH
molecular weight
Ion dipole interactions
Free radical
44. 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
Group 2A
Titration
Decomposition reaction
theoretical yield
45. The molar amount of a solute that can dissolve in 1L of solvent until equilibrium - saturation - is reached
Molar solubility
Ion
Reaction mechanism
Reaction order
46. 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
Planck's Constant
Hydrogen bonding
Electronegativity
s orbital
47. (chemistry) a substance that changes color to indicate the presence of some ion or substance
molecule
Molecular orbital
indicator
law of constant composition
48. Contains nonmetals that are non - reactive. Full outermost energy level except helium which has 2.
atomic radius
Solvent
Noble gases
Group 1A
49. (chemistry) a substance formed by chemical union of two or more elements or ingredients in definite proportion by weight
compound
pi bonds
Dipole
atomic radius
50. A graph of pressure versus temperature that shows the conditions under which the phases of a substance exist
Phase diagram
Atomic absorption Spectra
Ground state
Ion