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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 definite stable energy that a physical system can have
pi bonds
molecular weight
energy state
theoretical yield
2. 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
pI
Charles and Gay Lussac's Law
Reaction order
Magnetic quantum number
3. 2.18 x 10^-18 J/electron
Group 5A
Octet Rule
Theoretical yield
Rydberg constant
4. Elements in the middle of the periodic table - in groups 3-12.
Henderson Hasselbalch Equation
transition elements
Colligative properties
Water dissociation Constant
5. 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
pH
electromagnetic energy of photons emmited from electrons at ground state
pi bonds
6. 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.
Theoretical yield
Henderson Hasselbalch Equation
Free radical
law of constant composition
7. The lowest allowable energy state of an atom
decomposition reaction
Ground state
Neutron
Intermolecular forces
8. 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
9. Large molecular structures - strong covalent bonding - share qualities of IONIC And COVALENT
Group 6A
Network covalent
Pauli exclusion principle
Covalent Bond
10. 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
Chemical Kinetics
quantum
Conjugate acids and Bases
11. The amount of a substance that contains as many particles as there are atoms in exactly 12g of carbon -12
Lyman series
Reaction order
mole
Halogens
12. Any sample of a given compound will contain the same elements in the identical mass ratio.
Vapor pressure
law of constant composition
Molar solubility
Decomposition reaction
13. The tendency for an atom to attract electrons to itself when it is chemically combined with another element
Ion
Phase diagram
gram equivalent weight
Electronegativity
14. Common definition of acids as proton (H+) donors and bases as proton acceptors
compound
Bronsted - Lowry definition
pH
Percent yield
15. The molar amount of a solute that can dissolve in 1L of solvent until equilibrium - saturation - is reached
Molar solubility
Ionic Bond
Group 6A
Azeotrope
16. 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.
Formal Charge
Atomic absorption Spectra
Molarity
Water dissociation Constant
17. 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.
Hydrogen bonding
Group 3A
molecule
Conjugate acids and Bases
18. Simplest whole # ration of atoms in a compound
Emperical Formula
Theoretical yield
Ion dipole interactions
Normality
19. The sum of the exponents in a rate law - where each exponent provides the reaction order with respect to its reactants
Group 1A
Reaction order
Ground state
Bronsted - Lowry definition
20. Named after their cation and anion
bond length
Equivalence point
ionic cmpound
Magnetic quantum number
21. 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
single displacement reaction
lathanide series
Diffusion
22. A chemical bond that involves sharing a pair of electrons between atoms in a molecule
Emperical Formula
Normality
Covalent Bond
Spin quantum number
23. 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
Reaction mechanism
Nonpolar covalent bond
Equlibrium constant
Bronsted - Lowry definition
24. (chemistry) p(otential of) H(ydrogen)
angular momentum in the bohr model
Planck's Constant
amorphous solid
pH
25. 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
Azeotrope
Rate determining step
Halogens
indicator
26. E=hc/?
Half equivalence point
Vapor pressure
electromagnetic energy of photons emmited from electrons at ground state
Lewis acid base reaction
27. A solid made up of particles that are not arranged in a regular pattern.
Percent composition
Pauli exclusion principle
amorphous solid
Intermolecular forces
28. An acid that will completely dissociate in aqueous solution - like HCl - HI - HClO4 HBr.
Ion
Strong acid
Mass number
Equlibrium constant
29. Process by which molecules tend to move from an area where they are more concentrated to an area where they are less concentrated
bond energy
Atomic weight
Diffusion
Normality
30. 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
redox reaction
lathanide series
Group 7A
Combination Reaction
31. 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
Mass number
Effusion
azimuthal quantum number
Molar solubility
32. The process by which one or more substances change to produce one or more different substances
heisenberg uncertainty principle
effective nuclear charge
Ion
chemical reaction
33. An atom or group of atoms that has a positive or negative charge
Molarity
Ion
Nucleus
Dipole Dipole interaction
34. 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
actinide series
Percent yield
Arrhenius Definition
theoretical yield
35. 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
Triple point
Solution equilibrium
hydrogen bonding
subshell
36. States that if a stress is applied to a system at equilibrium - the system shifts in the direction that relieves the stress.
Colligative properties
Rydberg constant
Group 5A
Le chateliers Principle
37. 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
Molar solubility
Le chateliers Principle
Titration
atomic emission spectrum
38. 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.
lathanide series
Ion product
Collision theory of chemical Kinetics
Graham's Law
39. Rare earth element group (elements 58-71)
Disproportionation
lathanide series
Percent yield
Ground state
40. The Percent by mass of each element in a compound.
pH
electron configuration
Percent composition
Avagadros number
41. 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.
Alkaline earths
bond length
Molality
VSEPR
42. 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.
atomic theory
atomic radius
Azeotrope
Dipole
43. Theory stating that the rate of a reaction is directly proportional to the number of collisions that take place between reactants per second.
Collision theory of chemical Kinetics
Alkaline earths
Aqueous Solution
Henderson Hasselbalch Equation
44. 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
Conjugate acids and Bases
pH
Dipole
Ionization energy
45. 5 valence electrons -3 ions - Nitride N
Conjugate acids and Bases
Bronsted - Lowry definition
Group 5A
subshell
46. Contains nonmetals that are non - reactive. Full outermost energy level except helium which has 2.
Nucleus
bond length
Vapor pressure
Noble gases
47. A bond formed when two atomic orbitals combine to form a molecular orbital that is symmetrical around the axis connecting the two atomic nuclei
Group 1A
Dipole Dipole interaction
sigma bond
Covalent Bond
48. PH of a molecule at which it contains no net electric charge - isoelectric point.
Solution equilibrium
pI
und's rule
Octet Rule
49. A pair of equal and opposite electric charges or magnetic poles separated by a small distance
Ion product
Resonance structure
Formula weight
Dipole
50. Alkaline Earth Metals - 2 valence electrons +2 ions - Magnesium Mg
Group 2A
Avagadros number
single displacement reaction
hydrogen bonding