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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. Any sample of a given compound will contain the same elements in the identical mass ratio.
Proton
law of constant composition
Lewis structure
Group 4A
2. A measured amount of a solution of unknown concentration is added to a known volume of a second solution until the reaction between them is just complete
Titration
mole
Resonance structure
Ion dipole interactions
3. A structural formula in which electrons are represented by dots; dot pairs or dashes between two atomic symbols represent pairs in covalent bonds.
Lewis structure
Electrolyte
Molar solubility
effective nuclear charge
4. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance
VSEPR
Buffer
Triple point
decomposition reaction
5. The molar solubility of one salt is reduced when another salt - having a common ion is brought into the same solution
pH
quanta
Molarity
Common ion effect
6. 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.
Activation energy
Spin quantum number
Group 3A
Formula weight
7. 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.
sigma bond
Formula weight
Atomic absorption Spectra
empirical formula
8. 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
Alkaline earths
Spin quantum number
Nucleus
Ion
9. When polar molecules orient themselves such that the positive region of one molecule is close to the negative region of another molecule.
Combination Reaction
Dipole Dipole interaction
Covalent Bond
Molecular orbital
10. Contains nonmetals that are non - reactive. Full outermost energy level except helium which has 2.
effective nuclear charge
Dispersion Forces
Normality
Noble gases
11. Mixture of 2 or more substances that distills at a constant temperature and with constant composition - even though seperately the components have different boiling points
Chemical Kinetics
Azeotrope
Charles and Gay Lussac's Law
atomic emission spectrum
12. Small discrete increments of energy.
quanta
empirical formula
Lyman series
redox reaction
13. 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
Period
bond energy
Magnetic quantum number
effective nuclear charge
14. No two electrons or protons or neutrons in a given system can be in states characterized by the same set of quantum numbers
Free radical
Neutron
Ion
Pauli exclusion principle
15. Temperature is constant; effusion and temperature are proportional to the square root of their masses
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16. The ways in which electrons are arranged in various orbitals around the nuclei of atoms
Bronsted - Lowry definition
electron configuration
Solute
Rydberg constant
17. 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
Group 6A
Chemical Kinetics
Ionic Bond
18. The nuclear charge experienced by the outermost electrons of an atom (actual charge minus the shielding caused by inner shells: Z- eff)
Neutralization reaction
Bronsted - Lowry definition
effective nuclear charge
Dipole
19. A solid made up of particles that are not arranged in a regular pattern.
Dispersion Forces
amorphous solid
Buffer
pi bonds
20. Charge assigned to an atom in a molecule or polyatmic ion - calculated by (# valence electrons) - (# 1/2 bonding electrons) - (# nonbonding electrons). Molecules containing atoms with lower formal charges tend to be more stable than those with higher
Graham's Law
Formal Charge
Noble gases
Neutralization reaction
21. Elements in the middle of the periodic table - in groups 3-12.
Mass number
Atomic weight
Molarity
transition elements
22. A representation of a displacement reaction showing only the reactive species and omitting the spectator ions.
bond length
Net ionic equation
d orbital
Atomic absorption Spectra
23. A naturally occurring or synthetic compound consisting of large molecules made up of a linked series of repeated simple monomers
Common ion effect
Percent composition
polymer
chemical reaction
24. The reaction of the ions that characterize acids and the ions that characterize bases to form water molecules and a salt
Emperical Formula
empirical formula
Neutralization reaction
bond length
25. A reaction in which atoms of one element take the place of atoms of another element in a compound
single displacement reaction
Solubility Product Constant
pI
Resonance structure
26. A reaction in which atoms of one element take the place of atoms of another element in a compound
hydrogen bonding
Equilibrium
single displacement reaction
Disproportionation
27. (chemistry) a substance that changes color to indicate the presence of some ion or substance
gram equivalent weight
indicator
Group 5A
percent composition
28. 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-
Aqueous Solution
s orbital
Network covalent
Water dissociation Constant
29. The sum of the exponents in a rate law - where each exponent provides the reaction order with respect to its reactants
Reaction order
single displacement reaction
Reaction mechanism
pI
30. 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
atomic radius
Solubility Product Constant
Ion
31. A reaction where a compound does Not change its molecular structure.
bond energy
The bohr model
Group 7A
physical reaction
32. States that if a stress is applied to a system at equilibrium - the system shifts in the direction that relieves the stress.
theoretical yield
Le chateliers Principle
Effective nuclear charge
subshell
33. The center of the atom which contains the protons and neutrons; in cells - structure that contains the cell's genetic material (DNA) and controls the cell's activities
Nucleus
crystalline solid
Dipole
Solvent
34. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance C>>>>A+B
Acid dissociation constant
Decomposition reaction
Covalent Bond
compound
35. Rare earth element group (elements 58-71)
lathanide series
decomposition reaction
bond energy
lewis base
36. The percent by mass of each element in a compound
Ground state
percent composition
Titration
Net ionic equation
37. Process by which molecules tend to move from an area where they are more concentrated to an area where they are less concentrated
Aqueous Solution
atomic theory
Diffusion
Planck's Constant
38. 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.
Avagadros number
Titration
Redox Half Reaction
Acid dissociation constant
39. (chemistry) a substance formed by chemical union of two or more elements or ingredients in definite proportion by weight
Vapor pressure
compound
Reaction order
Electrolyte
40. Property of the elements that can be predicted from the arrangement of the periodic table
Molar solubility
Principle quantum number
Percent yield
periodic trends
41. The slowest elementary step which is the limit for the rate of the other steps
actinide series
Rate determining step
Solubility Product Constant
Octet Rule
42. 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
Noble gases
Equlibrium constant
transition elements
single displacement reaction
43. A graph of pressure versus temperature that shows the conditions under which the phases of a substance exist
Graham's Law
Henderson Hasselbalch Equation
Phase diagram
Lewis definition
44. 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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45. 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
s orbital
Ground state
London forces
Rate determining step
46. A bond formed when two atomic orbitals combine to form a molecular orbital that is symmetrical around the axis connecting the two atomic nuclei
Molecular orbital
sigma bond
indicator
Dispersion Forces
47. The tendency for an atom to attract electrons to itself when it is chemically combined with another element
d orbital
Lewis acid base reaction
Electronegativity
Dispersion Forces
48. The lowest allowable energy state of an atom
Electrolyte
Decomposition reaction
solvation
Ground state
49. The energy required to remove an electron from a gaseous atom; generally increases in moving from left - to - right across a period and decreases in moving down a group
Collision theory of chemical Kinetics
Reaction mechanism
Ionization energy
quanta
50. 5 different orbitals shaped like clover leaves and max electrons is 10
lathanide series
d orbital
Ground state
Proton