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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. Solids in which the particles are arranged in a repeating - 3- D pattern - has a specific melting point - classified as ionic network covalent - metallic or molecular.
crystalline solid
Dipole
Atomic weight
Ground state
2. Sum of the protons and neutrons in an element often denoted by the letter A
Rate determining step
Combination Reaction
Mass number
Molar solubility
3. PH of a molecule at which it contains no net electric charge - isoelectric point.
pI
ionic cmpound
atomic theory
Titration
4. Elements in the middle of the periodic table - in groups 3-12.
Effusion
Acid dissociation constant
transition elements
Free radical
5. 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.
Balmer series
Normality
London forces
Formula weight
6. 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.
Atomic weight
Nonpolar covalent bond
Resonance structure
Atomic absorption Spectra
7. The molar solubility of one salt is reduced when another salt - having a common ion is brought into the same solution
Colligative properties
Theoretical yield
empirical formula
Common ion effect
8. Contains nonmetals - 7 valence electrons in it's outermost energy level. Very reactive
Equlibrium constant
Disproportionation
periodic trends
Halogens
9. A reaction in which two or more substances combine to form a single substance A+B>>>>>>>C
crystalline solid
Network covalent
Lewis acid base reaction
Combination Reaction
10. A structural formula in which electrons are represented by dots; dot pairs or dashes between two atomic symbols represent pairs in covalent bonds.
Equivalence point
hydrogen bonding
compound
Lewis structure
11. 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-
law of constant composition
Lyman series
Water dissociation Constant
Amphoteric
12. 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
Resonance structure
Triple point
Water dissociation Constant
Rydberg constant
13. 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
London forces
bond length
Half equivalence point
Azeotrope
14. 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.
Buffer
Reaction order
Effective nuclear charge
Triple point
15. The tendency for an atom to attract electrons to itself when it is chemically combined with another element
Le chateliers Principle
Formula weight
Conjugate acids and Bases
Electronegativity
16. The pressure exerted by a vapor in equilibrium with its liquid or solid phase
Covalent Bond
Vapor pressure
Nonpolar covalent bond
Ion dipole interactions
17. 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
Lewis definition
Vapor pressure
Hydrogen bonding
sigma bond
18. Nh/2p The angular momentum changes only in discete amounts with respect to the quantum number. Also E=- R_h/n^2
Electronegativity
angular momentum in the bohr model
Equlibrium constant
The bohr model
19. The amount of energy that reactants must absorb before a chemical reaction will start; also called free energy of activation.
atomic radius
compound
empirical formula
Activation energy
20. Slightly less reactive than alkali metals - comprise group II
Dipole
Dispersion Forces
Alkaline earths
Rate law
21. Standard Temperature and Pressure. 273 Kelvin (0 Celsius) - 1 atmosphere (760 torr - 760 kPA).
STP
ionic cmpound
Solubility Product Constant
Ionization energy
22. 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
Ion product
Magnetic quantum number
Principle quantum number
atomic radius
23. A solution in which water is the solvent
bond length
Aqueous Solution
redox reaction
decomposition reaction
24. (chemistry) a series from actinium to lawrencium of 15 radioactive elements with increasing atomic numbers
Graham's Law
actinide series
Principle quantum number
Group 6A
25. Chalcogens - - Oxide O
subshell
Percent composition
Group 6A
Triple point
26. Property of the elements that can be predicted from the arrangement of the periodic table
Phase diagram
atomic radius
periodic trends
Group 5A
27. An ionic compound that resists changes in its pH
Colligative properties
azimuthal quantum number
Buffer
single displacement reaction
28. 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.
Diffusion
STP
Henderson Hasselbalch Equation
Percent yield
29. 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.
Redox Half Reaction
molecular weight
Principle quantum number
redox reaction
30. Sum of all the masses - in AMU - present in one molecule of a molecular compound.
Chemical Kinetics
Formula weight
ionic cmpound
London forces
31. When polar molecules orient themselves such that the positive region of one molecule is close to the negative region of another molecule.
Molecular orbital
Dipole Dipole interaction
pI
Arrhenius Definition
32. The average distance between the nuclei of two bonded atoms
bond length
Diprotic Base
Planck's Constant
Normality
33. Product of the molar concentrations of dissociated ions in solution at saturation - where each ion is raised to the power of its stoichiometric coefficient. Denoted Ksp.
Amphoteric
Planck's Constant
Buffer
Solubility Product Constant
34. A set of frequencies of electromagnetic waves given off by atoms of an element; consists of a series of fine lines of individual colors
Lyman series
Period
Network covalent
atomic emission spectrum
35. 1913 - Niels Bohr - said that electrons formed specific layers instead or random ones - said atoms atoms absorb and give off energy when the electrons move from one shell to another
Molecular orbital
The bohr model
Solution equilibrium
pI
36. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
hydrogen bonding
Acid dissociation constant
redox reaction
Balmer series
37. The percent by mass of each element in a compound
solvation
und's rule
s orbital
percent composition
38. The slowest elementary step which is the limit for the rate of the other steps
crystalline solid
Lyman series
Rate determining step
Titration
39. 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
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40. 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 radius
quantum numbers
molecular weight
Concentration
41. Alkaline Earth Metals - 2 valence electrons +2 ions - Magnesium Mg
Ground state
Equivalence point
Group 2A
crystalline solid
42. Side - to side parallel orbitals overlap to share electrons - the 2nd/3rd covalent bond between two atoms - cannot rotate and maintain the bond.
Mass number
The bohr model
pH
pi bonds
43. 5 different orbitals shaped like clover leaves and max electrons is 10
Charles and Gay Lussac's Law
bond energy
d orbital
Collision theory of chemical Kinetics
44. When a solute is dissolved in a solvent - it will dissociate until reaching an equilibrium point at which the rate of dissociation equals the rate of precipitation of the solute - regardless of any additional solute introduced into the mixture
Group 3A
Titration
Solution equilibrium
Decomposition reaction
45. A pair of equal and opposite electric charges or magnetic poles separated by a small distance
Dipole
Lewis definition
Half equivalence point
Rydberg constant
46. The amount of product that can be made in a chemical reaction based on the amount of limiting reactant
lewis base
Theoretical yield
Emperical Formula
Azeotrope
47. 5 valence electrons -3 ions - Nitride N
energy state
Group 5A
Decomposition reaction
molecular weight
48. A chemical bond that involves sharing a pair of electrons between atoms in a molecule
law of constant composition
Magnetic quantum number
Covalent Bond
Bronsted Lowry
49. Two or more atoms held together by covalent bonds
Dipole Dipole interaction
molecule
Solute
Arrhenius Definition
50. A fundamental constant - h - that relates the energy of light quanta to their frequency: h = 6.6 X 10^-34 joule
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