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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. 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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2. 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
Concentration
single displacement reaction
Resonance structure
3. The amount of energy that reactants must absorb before a chemical reaction will start; also called free energy of activation.
electron configuration
Activation energy
energy state
Molar solubility
4. Attractive and repulsive forces between molecules that are weaker than forces within molecules.
Intermolecular forces
single displacement reaction
sigma bond
effective nuclear charge
5. No two electrons or protons or neutrons in a given system can be in states characterized by the same set of quantum numbers
Pauli exclusion principle
Alkaline earths
Magnetic quantum number
molecule
6. The ratio of the number of moles of solute dissolved in one kilogram of solvent. molality (M = moles solute/kg of solution)
und's rule
Molality
quantum numbers
atomic radius
7. A substance that - when dissolved in water - results in a solution that can conduct electricity
Electrolyte
Group 7A
Rate determining step
Lewis acid base reaction
8. 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.
Atomic absorption Spectra
Group 6A
lathanide series
physical reaction
9. The process of decomposing a chemical compound by the passage of an electric current.
electrolysis
Alkaline earths
Spin quantum number
Pauli exclusion principle
10. An atom or group of atoms that has a positive or negative charge
physical reaction
atomic radius
Ion
single displacement reaction
11. PH of a molecule at which it contains no net electric charge - isoelectric point.
pI
electron configuration
amorphous solid
polymer
12. The area of chemistry that is concerned with reaction rates and reaction mechanisms
molecular weight
Chemical Kinetics
Intermolecular forces
Group 5A
13. Resulting positive nuclear charge an outer electron senses after accounting for the shielding effect of inner core electrons. Abbreviated as Z(eff). Increases from left to right - and bottom to top on the Periodic Table.
compound
Magnetic quantum number
Group 3A
Effective nuclear charge
14. Any sample of a given compound will contain the same elements in the identical mass ratio.
effective nuclear charge
Equivalence point
law of constant composition
chemical reaction
15. (chemistry) a substance formed by chemical union of two or more elements or ingredients in definite proportion by weight
Titration
Principle quantum number
compound
Theoretical yield
16. 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
Solution equilibrium
pI
Resonance structure
theoretical yield
17. States that it is impossible to determine simultaneously both the position and momentum of an electron or any other particle
Hydrogen bonding
Activation energy
single displacement reaction
heisenberg uncertainty principle
18. One - half of the distance between the center of identical atoms that are not bonded together. Since effective nuclear charge increases when moving from left to right each additional electron is pulled more strogly toward the nucleus.
Common ion effect
Combination Reaction
atomic radius
redox reaction
19. Where half of the acid is neutralized by the base on a titration curveAn acid dissociation constant - Ka - (also known as acidity constant - or acid - ionization constant) is a quantitative measure of the strength of an acid in solution. It is the eq
electron affinity
Half equivalence point
bond length
decomposition reaction
20. A representation of a displacement reaction showing only the reactive species and omitting the spectator ions.
Equivalence point
pI
Net ionic equation
pH
21. 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
single displacement reaction
und's rule
amorphous solid
22. 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
Henry's Law
hydrogen bonding
Free radical
The bohr model
23. Orbitals of equal energy are each occupied by one electron before any orbital is occupied by a second electron - and all electrons in singly occupied orbitals must have the same spin
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24. Sol - a chemical process in which solvent molecules and molecules or ions of the solute combine to form a compound
Concentration
solvation
Vapor pressure
Emperical Formula
25. 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.
Arrhenius Definition
Disproportionation
VSEPR
Balmer series
26. The slowest elementary step which is the limit for the rate of the other steps
Group 5A
heisenberg uncertainty principle
Rate determining step
quantum
27. Acids defined as electron - pair acceptors and bases as electron - pair donors.
Lewis definition
Effusion
s orbital
Ionization energy
28. An ionic compound that resists changes in its pH
Buffer
Lewis acid base reaction
pi bonds
The bohr model
29. The weight in grams of compound that can be substituted by 1 atom of Hydrogen. GEW = MW / # of acidic Hyrdogens
gram equivalent weight
Noble gases
Formal Charge
Conjugate acids and Bases
30. 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
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31. Chalcogens - - Oxide O
Group 6A
Group 3A
Molality
Diffusion
32. 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
STP
Nucleus
Azeotrope
quantum numbers
33. A solid made up of particles that are not arranged in a regular pattern.
Redox Half Reaction
Ion
The bohr model
amorphous solid
34. The point on a phase diagram that represents the only set of conditions at which all three phases exist in equilibrium with one another
molecule
Triple point
theoretical yield
Ion
35. Atoms react by gaining or losing electrons so as to acquire the stable electron structure of a noble gas - usually eight valence electrons
Solution equilibrium
Combination Reaction
Common ion effect
Octet Rule
36. (chemistry) a substance that changes color to indicate the presence of some ion or substance
indicator
Net ionic equation
Lewis definition
Diprotic Base
37. When polar molecules orient themselves such that the positive region of one molecule is close to the negative region of another molecule.
hydrogen bonding
Dipole Dipole interaction
Formula weight
physical reaction
38. The number of atoms in exactly 12 g of pure 12c and equal to 6.022 x 10^23 is called
solvation
Period
Avagadros number
amorphous solid
39. Large molecular structures - strong covalent bonding - share qualities of IONIC And COVALENT
atomic emission spectrum
Network covalent
law of constant composition
Group 4A
40. The reaction of the ions that characterize acids and the ions that characterize bases to form water molecules and a salt
Henderson Hasselbalch Equation
Acid dissociation constant
Neutralization reaction
Alkaline earths
41. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance C>>>>A+B
atomic radius
Decomposition reaction
Diprotic Base
chemical reaction
42. 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
decomposition reaction
Pauli exclusion principle
Electrolyte
43. (chemistry) any theory in which all matter is composed of tiny discrete finite indivisible indestructible particles
electrolysis
Covalent Bond
polymer
atomic theory
44. 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
Collision theory of chemical Kinetics
physical reaction
Principle quantum number
Equlibrium constant
45. 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
Alkaline earths
quanta
quantum
46. 5 valence electrons -3 ions - Nitride N
Group 5A
Percent composition
Balmer series
Group 4A
47. A base that can accept two moles of H+ per mole of itself (ex: SO4
Effusion
Diffusion
law of constant composition
Diprotic Base
48. Slightly less reactive than alkali metals - comprise group II
Alkaline earths
pH
Chemical Kinetics
Ion
49. 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
Proton
pI
Group 3A
Solute
50. 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
Pauli exclusion principle
Theoretical yield
Chemical Kinetics
Solution equilibrium