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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. Substance in which a solute is dissolved to form a solution
Neutralization reaction
Decomposition reaction
quanta
Solvent
2. 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
Ion product
Balmer series
representative elements
Percent composition
3. The solubility of a gas in a liquid is directly proportional to the partial pressure of that gas on the surface of the liquid
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4. In a solution - the substance that dissolves in the solvent
Azeotrope
Solute
Concentration
Resonance structure
5. (chemistry) p(otential of) H(ydrogen)
energy state
pH
Reaction order
Group 4A
6. 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
London forces
Halogens
Charles and Gay Lussac's Law
Equivalence point
7. The percent by mass of each element in a compound
percent composition
Rydberg constant
electron configuration
lathanide series
8. A base that can accept two moles of H+ per mole of itself (ex: SO4
Acid dissociation constant
Redox Half Reaction
Diprotic Base
Le chateliers Principle
9. 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.
Ion product
Nucleus
Ion
crystalline solid
10. A horizontal row of elements in the periodic table
Resonance structure
solvation
Period
Noble gases
11. The quantum number that has only two possible values - +1/2 and -1/2 - which indicate the two fundamental spin states of an electron in an orbital
Noble gases
Alkaline earths
molecule
Spin quantum number
12. Sum of all the masses - in AMU - present in one molecule of a molecular compound.
Reaction order
Formula weight
lewis base
energy state
13. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance C>>>>A+B
Noble gases
Dipole
Decomposition reaction
Resonance structure
14. The number of atoms in exactly 12 g of pure 12c and equal to 6.022 x 10^23 is called
Avagadros number
Spin quantum number
Ion dipole interactions
decomposition reaction
15. The molar solubility of one salt is reduced when another salt - having a common ion is brought into the same solution
Group 6A
Percent composition
Spin quantum number
Common ion effect
16. 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
Theoretical yield
Reaction mechanism
Covalent Bond
17. Sum of the protons and neutrons in an element often denoted by the letter A
Graham's Law
Lewis structure
Mass number
azimuthal quantum number
18. Sol - a chemical process in which solvent molecules and molecules or ions of the solute combine to form a compound
solvation
Group 2A
Solute
Hydrogen bonding
19. A graph of pressure versus temperature that shows the conditions under which the phases of a substance exist
Phase diagram
Effusion
compound
ionic cmpound
20. A reaction where a compound does Not change its molecular structure.
physical reaction
single displacement reaction
molecular weight
energy state
21. Redox reaction - in which the same species is both oxidized and reduced.
London forces
Ground state
Disproportionation
indicator
22. 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
bond length
Effective nuclear charge
Resonance structure
sigma bond
23. The ratio of the actual yield to the theoretical yield for a chemical reaction expressed as a percentage; a measure of the efficiency of a reaction
Henry's Law
Equivalence point
Percent yield
Halogens
24. E=hc/?
electromagnetic energy of photons emmited from electrons at ground state
Ionic Bond
Principle quantum number
Ion
25. A solid made up of particles that are not arranged in a regular pattern.
amorphous solid
Effusion
Strong acid
Mass number
26. 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.
Rate determining step
Network covalent
chemical reaction
Equivalence point
27. 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
Henderson Hasselbalch Equation
Decomposition reaction
hydrogen bonding
Ionic Bond
28. 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.
Activation energy
ionic cmpound
Effective nuclear charge
Disproportionation
29. No two electrons or protons or neutrons in a given system can be in states characterized by the same set of quantum numbers
ionic cmpound
bond energy
Redox Half Reaction
Pauli exclusion principle
30. 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.
Group 3A
electron affinity
Water dissociation Constant
Raoult's Law
31. 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-
Group 2A
quanta
Rate law
Water dissociation Constant
32. Tells you how much solute is present compared to the amount of solvent
Concentration
Group 6A
Rydberg constant
Solution equilibrium
33. A reaction in which atoms of one element take the place of atoms of another element in a compound
single displacement reaction
Electronegativity
hydrogen bonding
Electrolyte
34. The average distance between the nuclei of two bonded atoms
effective nuclear charge
bond length
quantum
electron configuration
35. Slightly less reactive than alkali metals - comprise group II
Vapor pressure
electron configuration
und's rule
Alkaline earths
36. Attractions between molecules caused by the electron motion on one molecule affecting the electron motion on the other through electrical forces; these are the weakest interactions between molecules
Group 4A
Magnetic quantum number
Equivalence point
Dispersion Forces
37. An ionic compound that resists changes in its pH
quantum numbers
Mass number
Buffer
Water dissociation Constant
38. States that it is impossible to determine simultaneously both the position and momentum of an electron or any other particle
molecular weight
Solute
Diffusion
heisenberg uncertainty principle
39. A set of frequencies of electromagnetic waves given off by atoms of an element; consists of a series of fine lines of individual colors
atomic emission spectrum
Decomposition reaction
Colligative properties
atomic radius
40. 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.
London forces
Henderson Hasselbalch Equation
azimuthal quantum number
Le chateliers Principle
41. An atom or group of atoms that has a positive or negative charge
bond length
Combination Reaction
Ion
Ionic Bond
42. A chemical formula showing the ratio of elements in a compound rather than the total number of atoms
sigma bond
electron configuration
Resonance structure
empirical formula
43. The tendency for an atom to attract electrons to itself when it is chemically combined with another element
Electronegativity
Percent composition
Phase diagram
Net ionic equation
44. Side - to side parallel orbitals overlap to share electrons - the 2nd/3rd covalent bond between two atoms - cannot rotate and maintain the bond.
azimuthal quantum number
pi bonds
theoretical yield
Solvent
45. 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.
solvation
Atomic absorption Spectra
Raoult's Law
empirical formula
46. 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
Group 1A
Octet Rule
Solute
47. (chemistry) any theory in which all matter is composed of tiny discrete finite indivisible indestructible particles
atomic theory
Molality
Graham's Law
mole
48. PH of a molecule at which it contains no net electric charge - isoelectric point.
Group 3A
angular momentum in the bohr model
pI
electron affinity
49. 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
Diprotic Base
redox reaction
Formal Charge
50. Common definition of acids as proton (H+) donors and bases as proton acceptors
Bronsted - Lowry definition
law of constant composition
pI
Ion dipole interactions