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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. Sum of the protons and neutrons in an element often denoted by the letter A
VSEPR
Equivalence point
Net ionic equation
Mass number
2. The maximum amount of product that can be produced from a given amount of reactant
theoretical yield
Dipole Dipole interaction
Strong acid
representative elements
3. A pair of equal and opposite electric charges or magnetic poles separated by a small distance
redox reaction
Group 3A
Dipole
Neutron
4. The amount of a substance that contains as many particles as there are atoms in exactly 12g of carbon -12
Ionization energy
STP
mole
Proton
5. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds
Molarity
Solubility Product Constant
Group 4A
Azeotrope
6. Slightly less reactive than alkali metals - comprise group II
Charles and Gay Lussac's Law
Alkaline earths
pi bonds
bond length
7. The process by which a gas escapes from one container to another at lower pressure through a tiny hole in the container.
Effusion
Activation energy
Water dissociation Constant
Vapor pressure
8. PH of a molecule at which it contains no net electric charge - isoelectric point.
pI
Equivalence point
Ion
decomposition reaction
9. At a constant pressure - the volume of an ideal gas is directly proportinal to its temperature: V (a) T
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10. 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
Bronsted - Lowry definition
Spin quantum number
Equivalence point
Collision theory of chemical Kinetics
11. The percent by mass of each element in a compound
representative elements
Rate determining step
percent composition
pH
12. 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
Ground state
physical reaction
Solution equilibrium
amorphous solid
13. The tendency for an atom to attract electrons to itself when it is chemically combined with another element
atomic radius
Electronegativity
Dipole Dipole interaction
Nucleus
14. 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
Molar solubility
Proton
hydrogen bonding
ionic cmpound
15. 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.
Covalent Bond
STP
Collision theory of chemical Kinetics
Solubility Product Constant
16. The reaction of the ions that characterize acids and the ions that characterize bases to form water molecules and a salt
Neutralization reaction
Activation energy
transition elements
Rate determining step
17. Process by which molecules tend to move from an area where they are more concentrated to an area where they are less concentrated
Diffusion
Ion dipole interactions
Le chateliers Principle
mole
18. 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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19. A chemical formula showing the ratio of elements in a compound rather than the total number of atoms
Redox Half Reaction
Molality
atomic emission spectrum
empirical formula
20. 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-
Water dissociation Constant
Molecular orbital
lathanide series
Electrolyte
21. The formation of one or more covalent bonds between an electron pair donor and an electron pair acceptor
Balmer series
hydrogen bonding
Lewis acid base reaction
Neutralization reaction
22. Any sample of a given compound will contain the same elements in the identical mass ratio.
Equivalence point
Group 2A
Strong acid
law of constant composition
23. Atoms react by gaining or losing electrons so as to acquire the stable electron structure of a noble gas - usually eight valence electrons
Octet Rule
VSEPR
redox reaction
Formula weight
24. A representation of a displacement reaction showing only the reactive species and omitting the spectator ions.
Hydrogen bonding
Pauli exclusion principle
Chemical Kinetics
Net ionic equation
25. (chemistry) a series from actinium to lawrencium of 15 radioactive elements with increasing atomic numbers
atomic radius
effective nuclear charge
atomic emission spectrum
actinide series
26. States that it is impossible to determine simultaneously both the position and momentum of an electron or any other particle
azimuthal quantum number
heisenberg uncertainty principle
bond energy
Molality
27. An acid that will completely dissociate in aqueous solution - like HCl - HI - HClO4 HBr.
theoretical yield
Raoult's Law
Henderson Hasselbalch Equation
Strong acid
28. When polar molecules orient themselves such that the positive region of one molecule is close to the negative region of another molecule.
pi bonds
lewis base
Chemical Kinetics
Dipole Dipole interaction
29. 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
Aqueous Solution
Solubility Product Constant
und's rule
s orbital
30. (chemistry) the sum of the relative atomic masses of the constituent atoms of a molecule
molecular weight
representative elements
chemical reaction
Colligative properties
31. Rare earth element group (elements 58-71)
Equlibrium constant
lathanide series
Alkaline earths
Rydberg constant
32. Standard Temperature and Pressure. 273 Kelvin (0 Celsius) - 1 atmosphere (760 torr - 760 kPA).
compound
Pauli exclusion principle
Spin quantum number
STP
33. 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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34. 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
Acid dissociation constant
pI
Reaction order
Bronsted - Lowry definition
35. Elements in the middle of the periodic table - in groups 3-12.
electron affinity
Molarity
transition elements
Formal Charge
36. A horizontal row of elements in the periodic table
Molarity
atomic theory
Rydberg constant
Period
37. 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
transition elements
Halogens
atomic theory
Azeotrope
38. Theory stating that the rate of a reaction is directly proportional to the number of collisions that take place between reactants per second.
Collision theory of chemical Kinetics
chemical reaction
Group 1A
actinide series
39. Two or more atoms held together by covalent bonds
Ground state
molecule
Ion dipole interactions
periodic trends
40. 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
angular momentum in the bohr model
Vapor pressure
Equlibrium constant
percent composition
41. The molar amount of a solute that can dissolve in 1L of solvent until equilibrium - saturation - is reached
Percent yield
single displacement reaction
Molar solubility
Atomic weight
42. 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
solvation
Collision theory of chemical Kinetics
Activation energy
43. Property of the elements that can be predicted from the arrangement of the periodic table
Lyman series
Equlibrium constant
periodic trends
Rydberg constant
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
Ionization energy
indicator
pI
45. 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
Pauli exclusion principle
Solution equilibrium
46. A covalent bond in which the bonding electrons are shared equally by the bonded atoms - resulting in a balanced distribution of electrical charge
Nonpolar covalent bond
Molarity
Dispersion Forces
Acid dissociation constant
47. 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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48. The Percent by mass of each element in a compound.
Group 1A
Percent composition
Titration
und's rule
49. 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.
Phase diagram
Ion dipole interactions
Redox Half Reaction
electron affinity
50. Region in a molecule where atomic orbitals overlap - resulting in either a stable low - energy bonding orbital or an unstable high - energy antibonding orbital.
Molecular orbital
Neutron
Spin quantum number
Ion product