SUBJECTS
|
BROWSE
|
CAREER CENTER
|
POPULAR
|
JOIN
|
LOGIN
Business Skills
|
Soft Skills
|
Basic Literacy
|
Certifications
About
|
Help
|
Privacy
|
Terms
|
Email
Search
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 set of spectral lines that appear in the visible light region when a hydrogen atom undergoes a transition from energy levels n>2 to n=2.
Graham's Law
Balmer series
hydrogen bonding
Resonance structure
2. An atom or group of atoms that has a positive or negative charge
energy state
Ion
redox reaction
Group 6A
3. Contains nonmetals - 7 valence electrons in it's outermost energy level. Very reactive
Bronsted Lowry
Principle quantum number
Halogens
Ion dipole interactions
4. The molar solubility of one salt is reduced when another salt - having a common ion is brought into the same solution
Nonpolar covalent bond
Rydberg constant
atomic radius
Common ion effect
5. Attractive and repulsive forces between molecules that are weaker than forces within molecules.
Rydberg constant
Intermolecular forces
quanta
Molarity
6. An atom - radical - or molecule that has gained or lost one or more electrons and has a negative or positive charge
d orbital
Ion
lathanide series
Molecular orbital
7. A solid made up of particles that are not arranged in a regular pattern.
amorphous solid
pH
physical reaction
Rydberg constant
8. Alkaline Earth Metals - 2 valence electrons +2 ions - Magnesium Mg
Nonpolar covalent bond
empirical formula
Group 2A
redox reaction
9. A reaction where a compound does Not change its molecular structure.
physical reaction
Spin quantum number
Solute
Effusion
10. A subdivision of an energy level in an atom. They are divided into orbitals.
und's rule
Bronsted - Lowry definition
Free radical
subshell
11. Rare earth element group (elements 58-71)
lathanide series
Disproportionation
Molar solubility
Rate law
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
Ground state
Effusion
Concentration
13. Slightly less reactive than alkali metals - comprise group II
Alkaline earths
ionic cmpound
solvation
Equivalence point
14. The pressure exerted by a vapor in equilibrium with its liquid or solid phase
effective nuclear charge
Vapor pressure
Percent composition
crystalline solid
15. 5 different orbitals shaped like clover leaves and max electrons is 10
Ion product
und's rule
d orbital
empirical formula
16. 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.
Period
solvation
Henderson Hasselbalch Equation
physical reaction
17. A naturally occurring or synthetic compound consisting of large molecules made up of a linked series of repeated simple monomers
decomposition reaction
polymer
Triple point
Decomposition reaction
18. An acid that will completely dissociate in aqueous solution - like HCl - HI - HClO4 HBr.
Strong acid
Lewis definition
crystalline solid
atomic emission spectrum
19. Process by which molecules tend to move from an area where they are more concentrated to an area where they are less concentrated
Group 1A
Arrhenius Definition
Diffusion
Lyman series
20. In a solution - the substance that dissolves in the solvent
Solute
Group 4A
Acid dissociation constant
representative elements
21. Nh/2p The angular momentum changes only in discete amounts with respect to the quantum number. Also E=- R_h/n^2
Arrhenius Definition
d orbital
angular momentum in the bohr model
Diffusion
22. 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
Group 5A
law of constant composition
indicator
23. A base that can accept two moles of H+ per mole of itself (ex: SO4
Resonance structure
transition elements
Free radical
Diprotic Base
24. 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
Bronsted Lowry
Disproportionation
Combination Reaction
25. 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
VSEPR
quantum numbers
Strong acid
26. 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
Octet Rule
crystalline solid
Combination Reaction
27. (chemistry) any theory in which all matter is composed of tiny discrete finite indivisible indestructible particles
molecule
Period
atomic theory
Strong acid
28. Chalcogens - - Oxide O
Effective nuclear charge
indicator
quantum numbers
Group 6A
29. 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
electrolysis
heisenberg uncertainty principle
Arrhenius Definition
und's rule
30. The maximum amount of product that can be produced from a given amount of reactant
bond energy
theoretical yield
Henderson Hasselbalch Equation
solvation
31. 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
Group 4A
indicator
Rate determining step
Magnetic quantum number
32. A solution in which water is the solvent
Formal Charge
Aqueous Solution
polymer
indicator
33. Alkali metals: highly reactive - therefore always compounds. - 1 valence electron +1 ion - Hydrogen H? - Lithium Li? - Sodium Na? - Potassium K? - Rubidium Rb? - Cesium Cs?
Percent yield
Group 1A
Group 4A
Group 5A
34. An atom - ion - or molecule that donates an electron pair to form a covalent bond.
Group 1A
lewis base
Rate law
compound
35. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
Rydberg constant
redox reaction
Alkaline earths
effective nuclear charge
36. A fundamental constant - h - that relates the energy of light quanta to their frequency: h = 6.6 X 10^-34 joule
37. The slowest elementary step which is the limit for the rate of the other steps
molecule
Octet Rule
Atomic weight
Rate determining step
38. A reaction in which two or more substances combine to form a single substance A+B>>>>>>>C
Reaction order
Combination Reaction
Water dissociation Constant
Lyman series
39. States that it is impossible to determine simultaneously both the position and momentum of an electron or any other particle
und's rule
single displacement reaction
heisenberg uncertainty principle
Octet Rule
40. An uncharged molecule with a single unpaitred electron in its outer ring - very unstable - exists for only about 10 seconds
Ground state
VSEPR
Hydrogen bonding
Free radical
41. A concentration unit of a solution expressed as moles of solute dissolved per liter of solution
Rydberg constant
Ion
Dipole
Molarity
42. 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
Phase diagram
atomic radius
Half equivalence point
bond energy
43. 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.
VSEPR
atomic emission spectrum
Phase diagram
molecule
44. 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.
Octet Rule
Ion product
Dipole Dipole interaction
Buffer
45. An element in an 'A' group in the periodic table; as a group these elements display a wide range of physical and chemical properties. In their atoms - the s and p sublevels in the highest occupied energy level are partially filled
single displacement reaction
representative elements
Electrolyte
Henry's Law
46. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds
quanta
Pauli exclusion principle
Group 4A
Aqueous Solution
47. The amount of product that can be made in a chemical reaction based on the amount of limiting reactant
Activation energy
crystalline solid
Theoretical yield
Amphoteric
48. 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
Rate law
Henry's Law
Group 7A
Formula weight
49. (chemistry) a substance formed by chemical union of two or more elements or ingredients in definite proportion by weight
physical reaction
compound
STP
molecule
50. A structural formula in which electrons are represented by dots; dot pairs or dashes between two atomic symbols represent pairs in covalent bonds.
Aqueous Solution
subshell
Lewis structure
transition elements