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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. 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.
energy state
Triple point
Atomic absorption Spectra
Group 6A
2. 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.
Phase diagram
Balmer series
Dipole Dipole interaction
Group 3A
3. Sol - a chemical process in which solvent molecules and molecules or ions of the solute combine to form a compound
Resonance structure
ionic cmpound
solvation
bond energy
4. Temperature is constant; effusion and temperature are proportional to the square root of their masses
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5. 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.
Neutralization reaction
Redox Half Reaction
Graham's Law
Buffer
6. The sum of the exponents in a rate law - where each exponent provides the reaction order with respect to its reactants
atomic emission spectrum
decomposition reaction
Reaction order
Phase diagram
7. An acid that will completely dissociate in aqueous solution - like HCl - HI - HClO4 HBr.
Percent yield
Normality
Neutralization reaction
Strong acid
8. Systematic pairing of a deprotonated species (base) with its protonated form (conjugate acid). Conjugates appear on opposite sides of a chemical equation.
Charles and Gay Lussac's Law
Conjugate acids and Bases
Ground state
azimuthal quantum number
9. 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
Hydrogen bonding
Lewis acid base reaction
sigma bond
electron configuration
10. (chemistry) a substance that changes color to indicate the presence of some ion or substance
atomic emission spectrum
indicator
Formal Charge
Molality
11. A reaction in which atoms of one element take the place of atoms of another element in a compound
Lyman series
Dispersion Forces
single displacement reaction
pI
12. Nh/2p The angular momentum changes only in discete amounts with respect to the quantum number. Also E=- R_h/n^2
Solubility Product Constant
Formula weight
angular momentum in the bohr model
Normality
13. 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
Nucleus
Resonance structure
Ion
und's rule
14. The amount of a substance that contains as many particles as there are atoms in exactly 12g of carbon -12
Henry's Law
molecular weight
Ion
mole
15. One - half the distance between the nuclei of two atoms of the same element when the atoms are joined
Disproportionation
atomic radius
Charles and Gay Lussac's Law
Noble gases
16. (chemistry) a series from actinium to lawrencium of 15 radioactive elements with increasing atomic numbers
Lyman series
actinide series
Phase diagram
single displacement reaction
17. A covalent bond in which the bonding electrons are shared equally by the bonded atoms - resulting in a balanced distribution of electrical charge
Concentration
Nonpolar covalent bond
Combination Reaction
molecular weight
18. The process by which one or more substances change to produce one or more different substances
London forces
atomic radius
Equlibrium constant
chemical reaction
19. The quantum number that indicates the main energy level occupied by the electron. Can theoretically take on any positive interger. Denoted by the letter n.
Electronegativity
Decomposition reaction
Combination Reaction
Principle quantum number
20. Theory stating that the rate of a reaction is directly proportional to the number of collisions that take place between reactants per second.
Effusion
Rydberg constant
Molarity
Collision theory of chemical Kinetics
21. 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
Spin quantum number
Solution equilibrium
Decomposition reaction
Conjugate acids and Bases
22. PH of a molecule at which it contains no net electric charge - isoelectric point.
Group 5A
Covalent Bond
Ion
pI
23. A set of frequencies of electromagnetic waves given off by atoms of an element; consists of a series of fine lines of individual colors
Arrhenius Definition
Percent yield
quantum
atomic emission spectrum
24. Property of the elements that can be predicted from the arrangement of the periodic table
chemical reaction
Lewis acid base reaction
periodic trends
Solubility Product Constant
25. The pressure exerted by a vapor in equilibrium with its liquid or solid phase
Vapor pressure
amorphous solid
polymer
Alkaline earths
26. A chemical formula showing the ratio of elements in a compound rather than the total number of atoms
Solution equilibrium
empirical formula
Strong acid
solvation
27. Redox reaction - in which the same species is both oxidized and reduced.
Free radical
Henderson Hasselbalch Equation
percent composition
Disproportionation
28. Chalcogens - - Oxide O
Solution equilibrium
Balmer series
Triple point
Group 6A
29. The tendency for an atom to attract electrons to itself when it is chemically combined with another element
Ionization energy
Electronegativity
Rydberg constant
single displacement reaction
30. 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-
Raoult's Law
Water dissociation Constant
Group 4A
Net ionic equation
31. Alkali metals: highly reactive - therefore always compounds. - 1 valence electron +1 ion - Hydrogen H? - Lithium Li? - Sodium Na? - Potassium K? - Rubidium Rb? - Cesium Cs?
Group 1A
compound
Magnetic quantum number
Molarity
32. 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
quanta
Atomic absorption Spectra
Group 2A
33. At a constant pressure - the volume of an ideal gas is directly proportinal to its temperature: V (a) T
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34. 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.
Henderson Hasselbalch Equation
Alkaline earths
Bronsted Lowry
Covalent Bond
35. (chemistry) p(otential of) H(ydrogen)
pH
Ionic Bond
electron configuration
heisenberg uncertainty principle
36. States that if a stress is applied to a system at equilibrium - the system shifts in the direction that relieves the stress.
Equlibrium constant
London forces
Rydberg constant
Le chateliers Principle
37. The number of atoms in exactly 12 g of pure 12c and equal to 6.022 x 10^23 is called
Avagadros number
solvation
Molarity
electromagnetic energy of photons emmited from electrons at ground state
38. (chemistry) the sum of the relative atomic masses of the constituent atoms of a molecule
molecular weight
Proton
Net ionic equation
Group 2A
39. The slowest elementary step which is the limit for the rate of the other steps
Rate determining step
Neutron
Molality
electromagnetic energy of photons emmited from electrons at ground state
40. Side - to side parallel orbitals overlap to share electrons - the 2nd/3rd covalent bond between two atoms - cannot rotate and maintain the bond.
Rydberg constant
pi bonds
Combination Reaction
sigma bond
41. The amount of product that can be made in a chemical reaction based on the amount of limiting reactant
Molar solubility
atomic emission spectrum
Solution equilibrium
Theoretical yield
42. 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
Titration
Equlibrium constant
atomic radius
43. 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
Neutralization reaction
Charles and Gay Lussac's Law
Equlibrium constant
representative elements
44. 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
Lewis definition
solvation
Equivalence point
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
Common ion effect
subshell
periodic trends
s orbital
46. A base that can accept two moles of H+ per mole of itself (ex: SO4
Equlibrium constant
Raoult's Law
STP
Diprotic Base
47. A subdivision of an energy level in an atom. They are divided into orbitals.
subshell
Rydberg constant
Ionization energy
angular momentum in the bohr model
48. Large molecular structures - strong covalent bonding - share qualities of IONIC And COVALENT
energy state
Network covalent
Diffusion
s orbital
49. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
redox reaction
Reaction mechanism
STP
Percent composition
50. Contains nonmetals - 7 valence electrons in it's outermost energy level. Very reactive
ionic cmpound
Activation energy
compound
Halogens