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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 bond formed when two atomic orbitals combine to form a molecular orbital that is symmetrical around the axis connecting the two atomic nuclei
sigma bond
Atomic absorption Spectra
Chemical Kinetics
energy state
2. A pair of equal and opposite electric charges or magnetic poles separated by a small distance
Solute
Ion dipole interactions
Dipole
Ionization energy
3. The energy required to break a chemical bond and form neutral isolated atoms
bond energy
Theoretical yield
Amphoteric
Percent yield
4. The lowest allowable energy state of an atom
Buffer
Ionic Bond
Free radical
Ground state
5. The amount of energy that reactants must absorb before a chemical reaction will start; also called free energy of activation.
Planck's Constant
Activation energy
Noble gases
hydrogen bonding
6. Elements in the middle of the periodic table - in groups 3-12.
transition elements
Solute
Electrolyte
molecule
7. A set of frequencies of electromagnetic waves given off by atoms of an element; consists of a series of fine lines of individual colors
compound
Group 5A
atomic emission spectrum
Rate determining step
8. 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.
Equivalence point
STP
s orbital
Emperical Formula
9. A fundamental constant - h - that relates the energy of light quanta to their frequency: h = 6.6 X 10^-34 joule
10. Rare earth element group (elements 58-71)
Charles and Gay Lussac's Law
Collision theory of chemical Kinetics
lathanide series
Normality
11. At a constant pressure - the volume of an ideal gas is directly proportinal to its temperature: V (a) T
12. Systematic pairing of a deprotonated species (base) with its protonated form (conjugate acid). Conjugates appear on opposite sides of a chemical equation.
Conjugate acids and Bases
Amphoteric
Proton
Aqueous Solution
13. A physical property of a solution that depends on the number - but not the identity - of the disswolved solute particles; example properties include vapor pressure lowering - boiling point elevation - osmotic pressure - and frezzing point depression
Colligative properties
Theoretical yield
ionic cmpound
amorphous solid
14. Region in a molecule where atomic orbitals overlap - resulting in either a stable low - energy bonding orbital or an unstable high - energy antibonding orbital.
Theoretical yield
Balmer series
Molecular orbital
Spin quantum number
15. Redox reaction - in which the same species is both oxidized and reduced.
decomposition reaction
Disproportionation
Noble gases
Electrolyte
16. (chemistry) a substance that changes color to indicate the presence of some ion or substance
Covalent Bond
theoretical yield
indicator
Conjugate acids and Bases
17. Having characteristics of both an acid and a base and capable of reacting as either
lewis base
Amphoteric
Ionization energy
Henry's Law
18. An atom - ion - or molecule that donates an electron pair to form a covalent bond.
Emperical Formula
azimuthal quantum number
lewis base
Rate determining step
19. A solid made up of particles that are not arranged in a regular pattern.
law of constant composition
gram equivalent weight
Disproportionation
amorphous solid
20. Small discrete increments of energy.
Rate law
quanta
Intermolecular forces
electromagnetic energy of photons emmited from electrons at ground state
21. A substance that - when dissolved in water - results in a solution that can conduct electricity
Intermolecular forces
electrolysis
bond length
Electrolyte
22. Slightly less reactive than alkali metals - comprise group II
Alkaline earths
Solute
Decomposition reaction
indicator
23. 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.
Group 3A
Solution equilibrium
Diprotic Base
Pauli exclusion principle
24. A subdivision of an energy level in an atom. They are divided into orbitals.
subshell
pH
Planck's Constant
hydrogen bonding
25. The ways in which electrons are arranged in various orbitals around the nuclei of atoms
Triple point
Nucleus
Rate determining step
electron configuration
26. The tendency for an atom to attract electrons to itself when it is chemically combined with another element
solvation
law of constant composition
Electronegativity
Nucleus
27. Property of the elements that can be predicted from the arrangement of the periodic table
Resonance structure
periodic trends
decomposition reaction
Water dissociation Constant
28. The point on a phase diagram that represents the only set of conditions at which all three phases exist in equilibrium with one another
electron affinity
Lewis definition
Resonance structure
Triple point
29. A solution in which water is the solvent
Equlibrium constant
atomic radius
Dipole Dipole interaction
Aqueous Solution
30. An acid that will completely dissociate in aqueous solution - like HCl - HI - HClO4 HBr.
Ionization energy
Lewis acid base reaction
Effective nuclear charge
Strong acid
31. A chemical bond that involves sharing a pair of electrons between atoms in a molecule
Covalent Bond
s orbital
Reaction order
Henderson Hasselbalch Equation
32. 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.
Effective nuclear charge
Noble gases
Redox Half Reaction
azimuthal quantum number
33. Play- by- play showing the individual steps of a reaction - including the formation and destruction of any reaction intermediates that may occur.
atomic emission spectrum
STP
Reaction mechanism
Vapor pressure
34. (chemistry) the sum of the relative atomic masses of the constituent atoms of a molecule
Buffer
molecular weight
Balmer series
Group 5A
35. Alkali metals: highly reactive - therefore always compounds. - 1 valence electron +1 ion - Hydrogen H? - Lithium Li? - Sodium Na? - Potassium K? - Rubidium Rb? - Cesium Cs?
Resonance structure
Lyman series
Ionization energy
Group 1A
36. A dynamic condition in which two opposing changes occur at equal rates in a closed system
Equilibrium
Spin quantum number
ionic cmpound
Henry's Law
37. A concentration unit of a solution expressed as moles of solute dissolved per liter of solution
Net ionic equation
Molarity
law of constant composition
representative elements
38. Named after their cation and anion
ionic cmpound
Henry's Law
lathanide series
physical reaction
39. 2.18 x 10^-18 J/electron
Raoult's Law
pH
Electronegativity
Rydberg constant
40. A definite stable energy that a physical system can have
lewis base
azimuthal quantum number
energy state
Phase diagram
41. The solubility of a gas in a liquid is directly proportional to the partial pressure of that gas on the surface of the liquid
42. The slowest elementary step which is the limit for the rate of the other steps
energy state
Activation energy
Group 2A
Rate determining step
43. Any sample of a given compound will contain the same elements in the identical mass ratio.
law of constant composition
angular momentum in the bohr model
quantum
Reaction order
44. The average distance between the nuclei of two bonded atoms
ionic cmpound
Solution equilibrium
Ion
bond length
45. 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
law of constant composition
heisenberg uncertainty principle
angular momentum in the bohr model
46. A reaction where a compound does Not change its molecular structure.
VSEPR
Magnetic quantum number
Ionic Bond
physical reaction
47. 5 different orbitals shaped like clover leaves and max electrons is 10
Mass number
Net ionic equation
d orbital
Ground state
48. States that if a stress is applied to a system at equilibrium - the system shifts in the direction that relieves the stress.
single displacement reaction
The bohr model
pI
Le chateliers Principle
49. 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
Halogens
London forces
Equivalence point
Reaction mechanism
50. 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.
Molarity
Ground state
atomic radius
molecule