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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 all the masses - in AMU - present in one molecule of a molecular compound.
Formula weight
Atomic weight
atomic theory
Acid dissociation constant
2. A chemical bond in which one atom loses an electron to form a positive ion and the other atom gains to electron to form a negative ion
bond length
Ionic Bond
Azeotrope
crystalline solid
3. The maximum amount of product that can be produced from a given amount of reactant
Lyman series
physical reaction
theoretical yield
Molecular orbital
4. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
bond energy
physical reaction
redox reaction
Rate determining step
5. Side - to side parallel orbitals overlap to share electrons - the 2nd/3rd covalent bond between two atoms - cannot rotate and maintain the bond.
single displacement reaction
und's rule
pi bonds
s orbital
6. A model of acids and bases which an acid is hydrogen ion donor and base is a hydrogen ion acceptor.
effective nuclear charge
Group 7A
Arrhenius Definition
Bronsted Lowry
7. 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
Atomic absorption Spectra
Molecular orbital
Combination Reaction
8. 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
single displacement reaction
Arrhenius Definition
electrolysis
Net ionic equation
9. 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
Amphoteric
subshell
Normality
Percent yield
10. Property of the elements that can be predicted from the arrangement of the periodic table
periodic trends
transition elements
Concentration
Combination Reaction
11. 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
Lewis structure
sigma bond
Proton
Azeotrope
12. Having characteristics of both an acid and a base and capable of reacting as either
Nonpolar covalent bond
atomic radius
molecule
Amphoteric
13. The ratio of the number of moles of solute dissolved in one kilogram of solvent. molality (M = moles solute/kg of solution)
Diffusion
Group 2A
Molality
Redox Half Reaction
14. 5 valence electrons -3 ions - Nitride N
Formula weight
Group 5A
Balmer series
angular momentum in the bohr model
15. Sol - a chemical process in which solvent molecules and molecules or ions of the solute combine to form a compound
transition elements
solvation
bond energy
Avagadros number
16. At a constant pressure - the volume of an ideal gas is directly proportinal to its temperature: V (a) T
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17. Small discrete increments of energy.
Ground state
bond length
quanta
STP
18. The formation of one or more covalent bonds between an electron pair donor and an electron pair acceptor
Lewis acid base reaction
Triple point
Half equivalence point
solvation
19. An atom - radical - or molecule that has gained or lost one or more electrons and has a negative or positive charge
actinide series
Ion
empirical formula
London forces
20. (chemistry) a substance formed by chemical union of two or more elements or ingredients in definite proportion by weight
compound
Titration
molecule
physical reaction
21. PH of a molecule at which it contains no net electric charge - isoelectric point.
pI
heisenberg uncertainty principle
Emperical Formula
redox reaction
22. 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
Network covalent
Azeotrope
Ion
Vapor pressure
23. A reaction in which atoms of one element take the place of atoms of another element in a compound
Conjugate acids and Bases
Triple point
Diffusion
single displacement reaction
24. 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
single displacement reaction
theoretical yield
Ionic Bond
25. The area of chemistry that is concerned with reaction rates and reaction mechanisms
electron affinity
atomic theory
Chemical Kinetics
sigma bond
26. 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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27. Common definition of acids as proton (H+) donors and bases as proton acceptors
Nucleus
Bronsted - Lowry definition
Magnetic quantum number
Dipole
28. Atoms react by gaining or losing electrons so as to acquire the stable electron structure of a noble gas - usually eight valence electrons
pH
Azeotrope
Halogens
Octet Rule
29. The pressure exerted by a vapor in equilibrium with its liquid or solid phase
Vapor pressure
lathanide series
Le chateliers Principle
Group 6A
30. A chemical bond that involves sharing a pair of electrons between atoms in a molecule
Lewis definition
Proton
Covalent Bond
Graham's Law
31. 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.
Strong acid
Group 6A
Atomic absorption Spectra
Atomic weight
32. Set of spectral lines appearing in the UV region when a hydrogen atom undergoes a transition from energy levels n>1 to n=1.
Molecular orbital
Lyman series
Alkaline earths
angular momentum in the bohr model
33. The average distance between the nuclei of two bonded atoms
Molar solubility
bond length
chemical reaction
atomic radius
34. (physics) the smallest discrete quantity of some physical property that a system can possess (according to quantum theory) E=hf
Group 3A
Raoult's Law
Aqueous Solution
quantum
35. (chemistry) a substance that changes color to indicate the presence of some ion or substance
Molality
indicator
Free radical
Lewis definition
36. The tendency for an atom to attract electrons to itself when it is chemically combined with another element
Electronegativity
Neutralization reaction
Molarity
Rydberg constant
37. Standard Temperature and Pressure. 273 Kelvin (0 Celsius) - 1 atmosphere (760 torr - 760 kPA).
Acid dissociation constant
Bronsted Lowry
Percent composition
STP
38. Rare earth element group (elements 58-71)
Group 3A
lathanide series
percent composition
Activation energy
39. The amount of a substance that contains as many particles as there are atoms in exactly 12g of carbon -12
Neutron
Effusion
Reaction order
mole
40. 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
pI
Electronegativity
molecule
Titration
41. A naturally occurring or synthetic compound consisting of large molecules made up of a linked series of repeated simple monomers
Ground state
s orbital
polymer
redox reaction
42. 5 different orbitals shaped like clover leaves and max electrons is 10
amorphous solid
actinide series
d orbital
Lyman series
43. An uncharged molecule with a single unpaitred electron in its outer ring - very unstable - exists for only about 10 seconds
Free radical
Reaction mechanism
Equlibrium constant
Ion
44. 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
polymer
Ionization energy
single displacement reaction
London forces
45. Alkali metals: highly reactive - therefore always compounds. - 1 valence electron +1 ion - Hydrogen H? - Lithium Li? - Sodium Na? - Potassium K? - Rubidium Rb? - Cesium Cs?
Intermolecular forces
ionic cmpound
Group 1A
transition elements
46. 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
atomic radius
Hydrogen bonding
Group 3A
Azeotrope
47. Valence Shell Electron Pair Repulsion theory - stating that the three - dimensional molecular geometry about some central atom is determined by the elctronic repulsion between its bonding and nonbonding electron pairs.
VSEPR
Ionic Bond
Lewis definition
Equivalence point
48. Temperature is constant; effusion and temperature are proportional to the square root of their masses
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49. A solution in which water is the solvent
Aqueous Solution
atomic radius
Redox Half Reaction
crystalline solid
50. States that if a stress is applied to a system at equilibrium - the system shifts in the direction that relieves the stress.
crystalline solid
Le chateliers Principle
Ion
Collision theory of chemical Kinetics