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MCAT Chemistry
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Subjects
:
mcat
,
science
Instructions:
Answer 50 questions in 15 minutes.
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.
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. Rare earth element group (elements 58-71)
lathanide series
Reaction mechanism
Rate determining step
pi bonds
2. Sol - a chemical process in which solvent molecules and molecules or ions of the solute combine to form a compound
Ion product
Charles and Gay Lussac's Law
solvation
gram equivalent weight
3. No two electrons or protons or neutrons in a given system can be in states characterized by the same set of quantum numbers
Charles and Gay Lussac's Law
Ion
Pauli exclusion principle
electron configuration
4. In a solution - the substance that dissolves in the solvent
Ground state
Acid dissociation constant
Buffer
Solute
5. Process by which molecules tend to move from an area where they are more concentrated to an area where they are less concentrated
Reaction order
theoretical yield
Diffusion
Group 4A
6. 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
Nucleus
Water dissociation Constant
Network covalent
Spin quantum number
7. A substance that - when dissolved in water - results in a solution that can conduct electricity
Effective nuclear charge
Electrolyte
electron configuration
polymer
8. The vapor pressure of solution is the product of the mole fraction of the solvent and the vapor pressure of the pure solvent. P_a=X_aP_total
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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.
Neutralization reaction
Ion product
Solubility Product Constant
Redox Half Reaction
10. 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
ionic cmpound
indicator
Ionization energy
azimuthal quantum number
11. States that if a stress is applied to a system at equilibrium - the system shifts in the direction that relieves the stress.
Combination Reaction
Le chateliers Principle
decomposition reaction
bond length
12. 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
Combination Reaction
Disproportionation
Azeotrope
Magnetic quantum number
13. The amount of a substance that contains as many particles as there are atoms in exactly 12g of carbon -12
Equivalence point
mole
energy state
Lewis structure
14. (chemistry) a substance that changes color to indicate the presence of some ion or substance
Alkaline earths
Proton
indicator
Pauli exclusion principle
15. Gram equivalent weight of solute per liter of solution - often denoted by N.
Buffer
Normality
energy state
pi bonds
16. A model of acids and bases which an acid is hydrogen ion donor and base is a hydrogen ion acceptor.
single displacement reaction
redox reaction
Bronsted Lowry
Amphoteric
17. Second quantum number - designated by the letter 'l.' This 'angular momentum' refers to the subshells within each principle quantum energy level. It can take on the value of an integer in the 0 to (n -1) range. The four subshellscorresponding to l=0
Alkaline earths
azimuthal quantum number
molecule
bond energy
18. An atom or group of atoms that has a positive or negative charge
quantum numbers
Nonpolar covalent bond
Ion
Vapor pressure
19. Play- by- play showing the individual steps of a reaction - including the formation and destruction of any reaction intermediates that may occur.
Neutralization reaction
Reaction mechanism
decomposition reaction
Theoretical yield
20. A structural formula in which electrons are represented by dots; dot pairs or dashes between two atomic symbols represent pairs in covalent bonds.
Bronsted - Lowry definition
Lewis structure
Alkaline earths
Neutron
21. 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
molecule
Alkaline earths
Formal Charge
Neutron
22. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
Free radical
Molarity
Planck's Constant
redox reaction
23. The energy required to break a chemical bond and form neutral isolated atoms
Neutralization reaction
Titration
redox reaction
bond energy
24. 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
The bohr model
molecular weight
gram equivalent weight
Intermolecular forces
25. 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.
Neutralization reaction
Diprotic Base
crystalline solid
Titration
26. (chemistry) a series from actinium to lawrencium of 15 radioactive elements with increasing atomic numbers
actinide series
Triple point
Lyman series
Lewis acid base reaction
27. Contains nonmetals - 7 valence electrons in it's outermost energy level. Very reactive
Rydberg constant
Halogens
Ionic Bond
Diffusion
28. An equilibrium expression used to measure weak - acid strength - given by the ratio of the product of the products' molar concentrations to the product of the reactants' molar concentrations - with each term raised to the power of its stoichiometric
Emperical Formula
Acid dissociation constant
Azeotrope
Nucleus
29. 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.
effective nuclear charge
Solubility Product Constant
Combination Reaction
Decomposition reaction
30. At a constant pressure - the volume of an ideal gas is directly proportinal to its temperature: V (a) T
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31. Small discrete increments of energy.
Group 1A
Atomic absorption Spectra
quanta
Network covalent
32. A dynamic condition in which two opposing changes occur at equal rates in a closed system
pi bonds
Equilibrium
heisenberg uncertainty principle
Dipole Dipole interaction
33. Common definition of acids as proton (H+) donors and bases as proton acceptors
Common ion effect
Bronsted - Lowry definition
Normality
Intermolecular forces
34. A naturally occurring or synthetic compound consisting of large molecules made up of a linked series of repeated simple monomers
Strong acid
polymer
physical reaction
Equivalence point
35. Property of the elements that can be predicted from the arrangement of the periodic table
Noble gases
Charles and Gay Lussac's Law
mole
periodic trends
36. An emperimentally determined mathmatical expression showing the rate of a reaction as a function of the concentration of its reactants
Lyman series
actinide series
compound
Rate law
37. A pair of equal and opposite electric charges or magnetic poles separated by a small distance
Redox Half Reaction
compound
Henry's Law
Dipole
38. Sum of all the masses - in AMU - present in one molecule of a molecular compound.
Formula weight
ionic cmpound
Net ionic equation
energy state
39. 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.
lewis base
solvation
electrolysis
Balmer series
40. An atom - ion - or molecule that donates an electron pair to form a covalent bond.
electrolysis
Equilibrium
Ground state
lewis base
41. 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.
percent composition
Redox Half Reaction
electron affinity
Net ionic equation
42. 5 valence electrons -3 ions - Nitride N
electromagnetic energy of photons emmited from electrons at ground state
Triple point
Group 5A
compound
43. Two or more atoms held together by covalent bonds
Covalent Bond
molecule
Combination Reaction
Free radical
44. (chemistry) the sum of the relative atomic masses of the constituent atoms of a molecule
Percent composition
Group 1A
redox reaction
molecular weight
45. An atom - radical - or molecule that has gained or lost one or more electrons and has a negative or positive charge
Ion
energy state
Neutron
atomic theory
46. The formation of one or more covalent bonds between an electron pair donor and an electron pair acceptor
Ground state
Nonpolar covalent bond
heisenberg uncertainty principle
Lewis acid base reaction
47. The molar solubility of one salt is reduced when another salt - having a common ion is brought into the same solution
Rate determining step
pH
Common ion effect
Atomic weight
48. 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
Water dissociation Constant
Titration
Aqueous Solution
atomic emission spectrum
49. Tells you how much solute is present compared to the amount of solvent
electrolysis
Molar solubility
atomic radius
Concentration
50. A solid made up of particles that are not arranged in a regular pattern.
percent composition
effective nuclear charge
amorphous solid
Bronsted - Lowry definition
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