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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
Period
energy state
pI
Magnetic quantum number
2. A dynamic condition in which two opposing changes occur at equal rates in a closed system
und's rule
Disproportionation
Equilibrium
Molarity
3. A reaction in which two or more substances combine to form a single substance A+B>>>>>>>C
Combination Reaction
Equilibrium
Formal Charge
lewis base
4. Simplest whole # ration of atoms in a compound
Conjugate acids and Bases
Rate law
Magnetic quantum number
Emperical Formula
5. The sum of the exponents in a rate law - where each exponent provides the reaction order with respect to its reactants
Lewis structure
Reaction order
Strong acid
effective nuclear charge
6. 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
Common ion effect
Hydrogen bonding
Group 7A
Vapor pressure
7. A chemical bond that involves sharing a pair of electrons between atoms in a molecule
Octet Rule
molecule
Net ionic equation
Covalent Bond
8. An ionic compound that resists changes in its pH
pH
Charles and Gay Lussac's Law
Mass number
Buffer
9. Elements in the middle of the periodic table - in groups 3-12.
transition elements
Concentration
Effusion
Arrhenius Definition
10. The process of decomposing a chemical compound by the passage of an electric current.
atomic radius
electrolysis
Ionization energy
Atomic weight
11. In a solution - the substance that dissolves in the solvent
Diprotic Base
Solute
Molality
mole
12. Any sample of a given compound will contain the same elements in the identical mass ratio.
molecular weight
Arrhenius Definition
Solution equilibrium
law of constant composition
13. (chemistry) a substance formed by chemical union of two or more elements or ingredients in definite proportion by weight
pH
compound
empirical formula
atomic radius
14. The area of chemistry that is concerned with reaction rates and reaction mechanisms
Chemical Kinetics
Reaction order
single displacement reaction
Reaction mechanism
15. Substance in which a solute is dissolved to form a solution
Theoretical yield
bond length
Solvent
redox reaction
16. The pressure exerted by a vapor in equilibrium with its liquid or solid phase
Ion
transition elements
Vapor pressure
Strong acid
17. A structural formula in which electrons are represented by dots; dot pairs or dashes between two atomic symbols represent pairs in covalent bonds.
Mass number
Halogens
Group 4A
Lewis structure
18. Common definition of acids as proton (H+) donors and bases as proton acceptors
Resonance structure
atomic theory
Graham's Law
Bronsted - Lowry definition
19. 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.
Phase diagram
Rate determining step
Intermolecular forces
VSEPR
20. 5 different orbitals shaped like clover leaves and max electrons is 10
molecular weight
Group 7A
Lewis definition
d orbital
21. 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
percent composition
gram equivalent weight
Equlibrium constant
Rate law
22. The formation of one or more covalent bonds between an electron pair donor and an electron pair acceptor
Redox Half Reaction
Lewis acid base reaction
Theoretical yield
Group 7A
23. The ways in which electrons are arranged in various orbitals around the nuclei of atoms
Ion dipole interactions
quantum
Network covalent
electron configuration
24. A base that can accept two moles of H+ per mole of itself (ex: SO4
law of constant composition
energy state
Diprotic Base
Ionization energy
25. Acids defined as electron - pair acceptors and bases as electron - pair donors.
Lewis definition
Lewis acid base reaction
Proton
electron configuration
26. Large molecular structures - strong covalent bonding - share qualities of IONIC And COVALENT
Bronsted Lowry
Network covalent
Triple point
Theoretical yield
27. 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.
pI
quanta
Solubility Product Constant
amorphous solid
28. 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.
Equivalence point
Half equivalence point
Nonpolar covalent bond
Ionic Bond
29. 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.
Intermolecular forces
Atomic absorption Spectra
Equilibrium
polymer
30. 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.
Rate law
Graham's Law
electron affinity
Molality
31. Side - to side parallel orbitals overlap to share electrons - the 2nd/3rd covalent bond between two atoms - cannot rotate and maintain the bond.
Percent composition
Acid dissociation constant
pi bonds
Conjugate acids and Bases
32. 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
Equivalence point
Dipole
bond length
33. 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
Diprotic Base
Rate law
Ionization energy
Formal Charge
34. Process by which molecules tend to move from an area where they are more concentrated to an area where they are less concentrated
Diffusion
amorphous solid
heisenberg uncertainty principle
Buffer
35. Nh/2p The angular momentum changes only in discete amounts with respect to the quantum number. Also E=- R_h/n^2
Covalent Bond
Graham's Law
Pauli exclusion principle
angular momentum in the bohr model
36. Property of the elements that can be predicted from the arrangement of the periodic table
Arrhenius Definition
Redox Half Reaction
periodic trends
Effective nuclear charge
37. Play- by- play showing the individual steps of a reaction - including the formation and destruction of any reaction intermediates that may occur.
Percent yield
Spin quantum number
ionic cmpound
Reaction mechanism
38. Standard Temperature and Pressure. 273 Kelvin (0 Celsius) - 1 atmosphere (760 torr - 760 kPA).
STP
Reaction mechanism
molecule
Le chateliers Principle
39. Gram equivalent weight of solute per liter of solution - often denoted by N.
Normality
hydrogen bonding
atomic radius
Nonpolar covalent bond
40. A set of frequencies of electromagnetic waves given off by atoms of an element; consists of a series of fine lines of individual colors
atomic emission spectrum
Graham's Law
Emperical Formula
subshell
41. 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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42. A representation of a displacement reaction showing only the reactive species and omitting the spectator ions.
Net ionic equation
electromagnetic energy of photons emmited from electrons at ground state
theoretical yield
amorphous solid
43. An acid that will completely dissociate in aqueous solution - like HCl - HI - HClO4 HBr.
Strong acid
Formal Charge
Net ionic equation
Lewis acid base reaction
44. Rare earth element group (elements 58-71)
lathanide series
Water dissociation Constant
STP
effective nuclear charge
45. The weight in grams of compound that can be substituted by 1 atom of Hydrogen. GEW = MW / # of acidic Hyrdogens
Spin quantum number
gram equivalent weight
Period
Percent yield
46. PH of a molecule at which it contains no net electric charge - isoelectric point.
Chemical Kinetics
Collision theory of chemical Kinetics
Nucleus
pI
47. The tendency for an atom to attract electrons to itself when it is chemically combined with another element
Electronegativity
Chemical Kinetics
mole
electron configuration
48. Chalcogens - - Oxide O
periodic trends
chemical reaction
Group 6A
Reaction mechanism
49. The molar solubility of one salt is reduced when another salt - having a common ion is brought into the same solution
und's rule
Raoult's Law
Common ion effect
Redox Half Reaction
50. E=hc/?
Group 3A
periodic trends
electromagnetic energy of photons emmited from electrons at ground state
Theoretical yield