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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 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
Redox Half Reaction
Proton
Emperical Formula
electromagnetic energy of photons emmited from electrons at ground state
2. No two electrons or protons or neutrons in a given system can be in states characterized by the same set of quantum numbers
single displacement reaction
Hydrogen bonding
Pauli exclusion principle
Solution equilibrium
3. 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
Theoretical yield
Half equivalence point
electron configuration
d orbital
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
Theoretical yield
decomposition reaction
Normality
5. An acid that will completely dissociate in aqueous solution - like HCl - HI - HClO4 HBr.
Ground state
law of constant composition
sigma bond
Strong acid
6. 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
Ion
polymer
transition elements
7. The process by which a gas escapes from one container to another at lower pressure through a tiny hole in the container.
Alkaline earths
Avagadros number
Effusion
transition elements
8. Tells you how much solute is present compared to the amount of solvent
Concentration
Rate determining step
Ground state
Lyman series
9. The slowest elementary step which is the limit for the rate of the other steps
Rydberg constant
Effusion
Rate determining step
Formal Charge
10. The solubility of a gas in a liquid is directly proportional to the partial pressure of that gas on the surface of the liquid
11. An atom - radical - or molecule that has gained or lost one or more electrons and has a negative or positive charge
Mass number
Ion
Pauli exclusion principle
Amphoteric
12. Have three valance electrons. In certain instances - some elements will loose three electrons - but they will also share electrons with another element to attain stability.
Neutron
Group 3A
Percent composition
Formula weight
13. 5 valence electrons -3 ions - Nitride N
Rydberg constant
Group 5A
Strong acid
angular momentum in the bohr model
14. 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.
Group 3A
VSEPR
lathanide series
electron configuration
15. The maximum amount of product that can be produced from a given amount of reactant
theoretical yield
Azeotrope
Group 6A
indicator
16. The process by which one or more substances change to produce one or more different substances
chemical reaction
Equilibrium
crystalline solid
gram equivalent weight
17. Contains nonmetals that are non - reactive. Full outermost energy level except helium which has 2.
Spin quantum number
Bronsted - Lowry definition
Formula weight
Noble gases
18. Sum of all the masses - in AMU - present in one molecule of a molecular compound.
transition elements
Planck's Constant
Halogens
Formula weight
19. A reaction in which atoms of one element take the place of atoms of another element in a compound
Network covalent
d orbital
angular momentum in the bohr model
single displacement reaction
20. (chemistry) a series from actinium to lawrencium of 15 radioactive elements with increasing atomic numbers
Period
actinide series
molecular weight
Diprotic Base
21. The process of decomposing a chemical compound by the passage of an electric current.
Ionization energy
Nucleus
Equlibrium constant
electrolysis
22. E=hc/?
pI
electromagnetic energy of photons emmited from electrons at ground state
ionic cmpound
Rate determining step
23. Common definition of acids as proton (H+) donors and bases as proton acceptors
Bronsted - Lowry definition
crystalline solid
Ion dipole interactions
Concentration
24. The area of chemistry that is concerned with reaction rates and reaction mechanisms
Phase diagram
Atomic weight
Common ion effect
Chemical Kinetics
25. 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.
pi bonds
Rydberg constant
Solubility Product Constant
atomic emission spectrum
26. 2.18 x 10^-18 J/electron
Rydberg constant
Formal Charge
Ion
Equilibrium
27. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
redox reaction
Group 3A
Concentration
bond length
28. The ratio of the number of moles of solute dissolved in one kilogram of solvent. molality (M = moles solute/kg of solution)
Molality
Triple point
Lyman series
physical reaction
29. The hypothetical equation showing only the species that is oxidized or reduced in a redox reaction and the correct number of electrons transferred between the species in the complete - balanced equation.
Free radical
Redox Half Reaction
Percent yield
Half equivalence point
30. (physics) the smallest discrete quantity of some physical property that a system can possess (according to quantum theory) E=hf
Ground state
solvation
quantum
single displacement reaction
31. Side - to side parallel orbitals overlap to share electrons - the 2nd/3rd covalent bond between two atoms - cannot rotate and maintain the bond.
pi bonds
Collision theory of chemical Kinetics
single displacement reaction
VSEPR
32. Numbers that specify the properties of atomic orbitals and of their electrons
Neutralization reaction
heisenberg uncertainty principle
Half equivalence point
quantum numbers
33. The number of atoms in exactly 12 g of pure 12c and equal to 6.022 x 10^23 is called
Solvent
Avagadros number
Ion
bond length
34. (chemistry) p(otential of) H(ydrogen)
pH
atomic emission spectrum
Reaction mechanism
Planck's Constant
35. Standard Temperature and Pressure. 273 Kelvin (0 Celsius) - 1 atmosphere (760 torr - 760 kPA).
STP
Nucleus
Balmer series
Ion dipole interactions
36. 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
s orbital
quantum
molecular weight
Solubility Product Constant
37. At a constant pressure - the volume of an ideal gas is directly proportinal to its temperature: V (a) T
38. Rare earth element group (elements 58-71)
redox reaction
Combination Reaction
Amphoteric
lathanide series
39. A definite stable energy that a physical system can have
Decomposition reaction
energy state
Group 6A
Common ion effect
40. Attractive and repulsive forces between molecules that are weaker than forces within molecules.
Lewis acid base reaction
Amphoteric
Intermolecular forces
Pauli exclusion principle
41. (chemistry) the sum of the relative atomic masses of the constituent atoms of a molecule
Emperical Formula
Rate determining step
Percent composition
molecular weight
42. The weak attractive forces between molecules resulting from the small - instantaneous dipoles that occur because of the varying positions of the electrons during their motion about nuclei
d orbital
Noble gases
London forces
Diprotic Base
43. Any sample of a given compound will contain the same elements in the identical mass ratio.
Normality
Equilibrium
law of constant composition
Formal Charge
44. The point on a phase diagram that represents the only set of conditions at which all three phases exist in equilibrium with one another
indicator
redox reaction
Group 2A
Triple point
45. Sol - a chemical process in which solvent molecules and molecules or ions of the solute combine to form a compound
decomposition reaction
solvation
Covalent Bond
Nonpolar covalent bond
46. A pair of equal and opposite electric charges or magnetic poles separated by a small distance
atomic radius
law of constant composition
heisenberg uncertainty principle
Dipole
47. A fundamental constant - h - that relates the energy of light quanta to their frequency: h = 6.6 X 10^-34 joule
48. A substance that - when dissolved in water - results in a solution that can conduct electricity
VSEPR
Electrolyte
Spin quantum number
actinide series
49. A structural formula in which electrons are represented by dots; dot pairs or dashes between two atomic symbols represent pairs in covalent bonds.
Lewis structure
Equlibrium constant
Lyman series
Molar solubility
50. The nuclear charge experienced by the outermost electrons of an atom (actual charge minus the shielding caused by inner shells: Z- eff)
Phase diagram
effective nuclear charge
Arrhenius Definition
Resonance structure