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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. A definite stable energy that a physical system can have
empirical formula
energy state
Ion
Ground state
2. The reaction of the ions that characterize acids and the ions that characterize bases to form water molecules and a salt
Neutron
compound
Neutralization reaction
amorphous solid
3. Process by which molecules tend to move from an area where they are more concentrated to an area where they are less concentrated
Neutralization reaction
Diffusion
Percent yield
Formula weight
4. 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 7A
Disproportionation
Amphoteric
5. (chemistry) a series from actinium to lawrencium of 15 radioactive elements with increasing atomic numbers
Raoult's Law
atomic radius
Azeotrope
actinide series
6. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
Half equivalence point
redox reaction
Group 2A
Ionic Bond
7. The area of chemistry that is concerned with reaction rates and reaction mechanisms
Raoult's Law
Bronsted Lowry
Chemical Kinetics
Activation energy
8. Slightly less reactive than alkali metals - comprise group II
Electrolyte
Alkaline earths
Activation energy
molecular weight
9. No two electrons or protons or neutrons in a given system can be in states characterized by the same set of quantum numbers
transition elements
atomic emission spectrum
Pauli exclusion principle
Lewis acid base reaction
10. (physics) the smallest discrete quantity of some physical property that a system can possess (according to quantum theory) E=hf
Ionic Bond
Reaction order
atomic radius
quantum
11. 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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12. The slowest elementary step which is the limit for the rate of the other steps
Activation energy
Neutralization reaction
Solution equilibrium
Rate determining step
13. Large molecular structures - strong covalent bonding - share qualities of IONIC And COVALENT
Lewis acid base reaction
Octet Rule
electron affinity
Network covalent
14. A graph of pressure versus temperature that shows the conditions under which the phases of a substance exist
Ionic Bond
Phase diagram
STP
Covalent Bond
15. 2.18 x 10^-18 J/electron
angular momentum in the bohr model
Rydberg constant
Nucleus
mole
16. 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
Water dissociation Constant
Redox Half Reaction
Activation energy
Spin quantum number
17. The pressure exerted by a vapor in equilibrium with its liquid or solid phase
law of constant composition
Network covalent
Diprotic Base
Vapor pressure
18. 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.
Atomic absorption Spectra
Reaction order
Molarity
electron affinity
19. (chemistry) the sum of the relative atomic masses of the constituent atoms of a molecule
pi bonds
Principle quantum number
molecular weight
Rate law
20. A chemical bond that involves sharing a pair of electrons between atoms in a molecule
Intermolecular forces
azimuthal quantum number
Covalent Bond
Group 4A
21. Common definition of acids as proton (H+) donors and bases as proton acceptors
Water dissociation Constant
amorphous solid
Acid dissociation constant
Bronsted - Lowry definition
22. The process of decomposing a chemical compound by the passage of an electric current.
Percent yield
Group 2A
azimuthal quantum number
electrolysis
23. (chemistry) a substance that changes color to indicate the presence of some ion or substance
molecule
Ion
electron affinity
indicator
24. 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
azimuthal quantum number
amorphous solid
effective nuclear charge
Balmer series
25. The number of atoms in exactly 12 g of pure 12c and equal to 6.022 x 10^23 is called
Avagadros number
solvation
Acid dissociation constant
Magnetic quantum number
26. 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
Henry's Law
Solubility Product Constant
representative elements
gram equivalent weight
27. 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
Noble gases
azimuthal quantum number
Reaction mechanism
Dispersion Forces
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
Pauli exclusion principle
Rydberg constant
Water dissociation Constant
Acid dissociation constant
29. Temperature is constant; effusion and temperature are proportional to the square root of their masses
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30. 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.
Covalent Bond
crystalline solid
Ion dipole interactions
Octet Rule
31. Contains nonmetals that are non - reactive. Full outermost energy level except helium which has 2.
Atomic weight
Neutralization reaction
Bronsted - Lowry definition
Noble gases
32. In a solution - the substance that dissolves in the solvent
Common ion effect
Solute
Solubility Product Constant
subshell
33. An ionic compound that resists changes in its pH
Ion product
Buffer
Dipole
Group 5A
34. A subatomic particle that has a positive charge and that is found in the nucleus of an atom Charge of +1 and mass of 1.0073 amu
Group 4A
Proton
Effective nuclear charge
Vapor pressure
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
Acid dissociation constant
The bohr model
Percent composition
solvation
36. 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
law of constant composition
Lewis structure
Noble gases
37. A reaction where a compound does Not change its molecular structure.
Lewis structure
physical reaction
Period
Bronsted - Lowry definition
38. Chalcogens - - Oxide O
Group 6A
Solubility Product Constant
STP
Colligative properties
39. States that it is impossible to determine simultaneously both the position and momentum of an electron or any other particle
heisenberg uncertainty principle
Molar solubility
Electrolyte
Neutron
40. 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.
heisenberg uncertainty principle
Balmer series
transition elements
Strong acid
41. A horizontal row of elements in the periodic table
redox reaction
lewis base
Period
pI
42. Sum of the protons and neutrons in an element often denoted by the letter A
Mass number
Henderson Hasselbalch Equation
Equivalence point
Lewis definition
43. 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.
redox reaction
Concentration
angular momentum in the bohr model
Solubility Product Constant
44. 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
Percent yield
Activation energy
Half equivalence point
Nucleus
45. 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.
Effective nuclear charge
chemical reaction
Atomic absorption Spectra
s orbital
46. An elementary particle with 0 charge and mass about equal to a proton
gram equivalent weight
Neutron
Percent composition
Half equivalence point
47. A reaction in which atoms of one element take the place of atoms of another element in a compound
und's rule
single displacement reaction
Solvent
Formal Charge
48. Any sample of a given compound will contain the same elements in the identical mass ratio.
amorphous solid
law of constant composition
hydrogen bonding
Alkaline earths
49. 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.
Strong acid
Neutralization reaction
Equivalence point
Redox Half Reaction
50. Standard Temperature and Pressure. 273 Kelvin (0 Celsius) - 1 atmosphere (760 torr - 760 kPA).
Intermolecular forces
Alkaline earths
pI
STP