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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 atom or group of atoms that has a positive or negative charge
Group 7A
Activation energy
Ion
Common ion effect
2. 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
Titration
VSEPR
Aqueous Solution
Henderson Hasselbalch Equation
3. 5 valence electrons -3 ions - Nitride N
Solution equilibrium
energy state
Group 5A
Group 1A
4. When polar molecules orient themselves such that the positive region of one molecule is close to the negative region of another molecule.
Hydrogen bonding
Emperical Formula
Dipole Dipole interaction
electrolysis
5. An atom - ion - or molecule that donates an electron pair to form a covalent bond.
Alkaline earths
Network covalent
Bronsted Lowry
lewis base
6. A representation of a displacement reaction showing only the reactive species and omitting the spectator ions.
Net ionic equation
crystalline solid
London forces
redox reaction
7. The nuclear charge experienced by the outermost electrons of an atom (actual charge minus the shielding caused by inner shells: Z- eff)
lathanide series
decomposition reaction
Hydrogen bonding
effective nuclear charge
8. An acid that will completely dissociate in aqueous solution - like HCl - HI - HClO4 HBr.
Common ion effect
Solubility Product Constant
quantum
Strong acid
9. Small discrete increments of energy.
London forces
Free radical
quanta
Equivalence point
10. Sum of the protons and neutrons in an element often denoted by the letter A
Group 1A
Ground state
Mass number
redox reaction
11. Standard Temperature and Pressure. 273 Kelvin (0 Celsius) - 1 atmosphere (760 torr - 760 kPA).
STP
Pauli exclusion principle
Group 5A
Formula weight
12. When dipoles are dissolved in a solution where ions are present ions wil arrange themselves with the opposite charged end of the dipole.
Ion dipole interactions
Group 3A
quantum
Mass number
13. 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.
Amphoteric
Neutralization reaction
Atomic absorption Spectra
Hydrogen bonding
14. The formation of one or more covalent bonds between an electron pair donor and an electron pair acceptor
s orbital
Formula weight
Lewis acid base reaction
bond length
15. 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
Combination Reaction
Balmer series
Disproportionation
The bohr model
16. Chalcogens - - Oxide O
Hydrogen bonding
Dispersion Forces
atomic radius
Group 6A
17. Any sample of a given compound will contain the same elements in the identical mass ratio.
law of constant composition
physical reaction
Rate law
energy state
18. The weight in grams of compound that can be substituted by 1 atom of Hydrogen. GEW = MW / # of acidic Hyrdogens
Hydrogen bonding
Lewis acid base reaction
ionic cmpound
gram equivalent weight
19. Nh/2p The angular momentum changes only in discete amounts with respect to the quantum number. Also E=- R_h/n^2
angular momentum in the bohr model
Intermolecular forces
atomic radius
Ion dipole interactions
20. A reaction in which atoms of one element take the place of atoms of another element in a compound
single displacement reaction
Molecular orbital
compound
Theoretical yield
21. In a solution - the substance that dissolves in the solvent
Solute
Resonance structure
Group 4A
quantum numbers
22. A substance that - when dissolved in water - results in a solution that can conduct electricity
und's rule
Electrolyte
Water dissociation Constant
Theoretical yield
23. Process by which molecules tend to move from an area where they are more concentrated to an area where they are less concentrated
Atomic absorption Spectra
Octet Rule
Halogens
Diffusion
24. A fundamental constant - h - that relates the energy of light quanta to their frequency: h = 6.6 X 10^-34 joule
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25. Numbers that specify the properties of atomic orbitals and of their electrons
pI
quantum numbers
Hydrogen bonding
Electronegativity
26. A graph of pressure versus temperature that shows the conditions under which the phases of a substance exist
Phase diagram
Aqueous Solution
Dispersion Forces
Network covalent
27. 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
angular momentum in the bohr model
Common ion effect
redox reaction
28. The percent by mass of each element in a compound
Hydrogen bonding
Nucleus
Solubility Product Constant
percent composition
29. An elementary particle with 0 charge and mass about equal to a proton
Neutron
molecule
law of constant composition
Amphoteric
30. 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.
polymer
Le chateliers Principle
Henderson Hasselbalch Equation
lewis base
31. Region in a molecule where atomic orbitals overlap - resulting in either a stable low - energy bonding orbital or an unstable high - energy antibonding orbital.
Redox Half Reaction
Halogens
effective nuclear charge
Molecular orbital
32. 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
bond length
theoretical yield
molecular weight
Ionic Bond
33. A subdivision of an energy level in an atom. They are divided into orbitals.
Percent yield
subshell
actinide series
Group 2A
34. The weight in grams of one mole of a given elementand is expressedin tems of grams per mole.
Atomic weight
Rate determining step
heisenberg uncertainty principle
Electrolyte
35. 2.18 x 10^-18 J/electron
quantum numbers
Lewis structure
Rydberg constant
Hydrogen bonding
36. Having characteristics of both an acid and a base and capable of reacting as either
Amphoteric
Group 4A
atomic radius
Ion dipole interactions
37. 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
Formula weight
Group 3A
Group 7A
38. A concentration unit of a solution expressed as moles of solute dissolved per liter of solution
Diffusion
molecular weight
azimuthal quantum number
Molarity
39. Theory stating that the rate of a reaction is directly proportional to the number of collisions that take place between reactants per second.
Dispersion Forces
bond length
Atomic weight
Collision theory of chemical Kinetics
40. A dynamic condition in which two opposing changes occur at equal rates in a closed system
Equlibrium constant
single displacement reaction
Equilibrium
Spin quantum number
41. Set of spectral lines appearing in the UV region when a hydrogen atom undergoes a transition from energy levels n>1 to n=1.
pI
Lyman series
Principle quantum number
Alkaline earths
42. 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
Group 7A
Period
Net ionic equation
Free radical
43. A definite stable energy that a physical system can have
Solvent
polymer
solvation
energy state
44. An uncharged molecule with a single unpaitred electron in its outer ring - very unstable - exists for only about 10 seconds
energy state
Free radical
Resonance structure
quantum numbers
45. The molar solubility of one salt is reduced when another salt - having a common ion is brought into the same solution
Normality
Amphoteric
chemical reaction
Common ion effect
46. Contains nonmetals - 7 valence electrons in it's outermost energy level. Very reactive
Avagadros number
Halogens
Mass number
Octet Rule
47. (chemistry) any theory in which all matter is composed of tiny discrete finite indivisible indestructible particles
Ion
electromagnetic energy of photons emmited from electrons at ground state
Charles and Gay Lussac's Law
atomic theory
48. The point on a phase diagram that represents the only set of conditions at which all three phases exist in equilibrium with one another
Disproportionation
Planck's Constant
Triple point
quantum numbers
49. The sum of the exponents in a rate law - where each exponent provides the reaction order with respect to its reactants
Avagadros number
bond energy
Reaction order
Raoult's Law
50. E=hc/?
redox reaction
Reaction order
Molar solubility
electromagnetic energy of photons emmited from electrons at ground state