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Test your basic knowledge |
MCAT Chemistry
Start Test
Study First
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. 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
Ionic Bond
atomic theory
Aqueous Solution
2. Slightly less reactive than alkali metals - comprise group II
Alkaline earths
Water dissociation Constant
Reaction mechanism
transition elements
3. Acids defined as electron - pair acceptors and bases as electron - pair donors.
Noble gases
Triple point
Lewis definition
angular momentum in the bohr model
4. PH of a molecule at which it contains no net electric charge - isoelectric point.
Neutralization reaction
pI
hydrogen bonding
Common ion effect
5. Contains nonmetals that are non - reactive. Full outermost energy level except helium which has 2.
Noble gases
Ionization energy
Disproportionation
STP
6. An ionic compound that resists changes in its pH
Buffer
Atomic weight
London forces
Combination Reaction
7. A solid made up of particles that are not arranged in a regular pattern.
theoretical yield
amorphous solid
percent composition
Ionization energy
8. The lowest allowable energy state of an atom
Spin quantum number
Ground state
gram equivalent weight
effective nuclear charge
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
indicator
lathanide series
Percent yield
Buffer
10. (chemistry) any theory in which all matter is composed of tiny discrete finite indivisible indestructible particles
Ionic Bond
Free radical
Rate law
atomic theory
11. 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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12. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance
decomposition reaction
Conjugate acids and Bases
Ionization energy
redox reaction
13. 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.
Equivalence point
Group 7A
azimuthal quantum number
electron affinity
14. Elements in the middle of the periodic table - in groups 3-12.
Conjugate acids and Bases
redox reaction
Disproportionation
transition elements
15. 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
Le chateliers Principle
physical reaction
VSEPR
16. Numbers that specify the properties of atomic orbitals and of their electrons
Proton
Acid dissociation constant
Net ionic equation
quantum numbers
17. A graph of pressure versus temperature that shows the conditions under which the phases of a substance exist
indicator
Decomposition reaction
Phase diagram
Group 4A
18. 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
atomic radius
Titration
Charles and Gay Lussac's Law
Lewis definition
19. A physical property of a solution that depends on the number - but not the identity - of the disswolved solute particles; example properties include vapor pressure lowering - boiling point elevation - osmotic pressure - and frezzing point depression
Group 4A
Molar solubility
Colligative properties
pH
20. Play- by- play showing the individual steps of a reaction - including the formation and destruction of any reaction intermediates that may occur.
redox reaction
heisenberg uncertainty principle
Hydrogen bonding
Reaction mechanism
21. The process of decomposing a chemical compound by the passage of an electric current.
Dipole
lathanide series
Henderson Hasselbalch Equation
electrolysis
22. Sum of the protons and neutrons in an element often denoted by the letter A
energy state
Raoult's Law
Lewis definition
Mass number
23. 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
pI
Free radical
Ionization energy
und's rule
24. An atom - radical - or molecule that has gained or lost one or more electrons and has a negative or positive charge
Ion
Normality
Group 3A
Group 6A
25. 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
quanta
Group 3A
Lewis acid base reaction
26. An elementary particle with 0 charge and mass about equal to a proton
Neutron
Effective nuclear charge
Covalent Bond
Charles and Gay Lussac's Law
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.
Molecular orbital
Solubility Product Constant
actinide series
hydrogen bonding
28. Alkaline Earth Metals - 2 valence electrons +2 ions - Magnesium Mg
Group 7A
Group 2A
pI
Concentration
29. A substance that - when dissolved in water - results in a solution that can conduct electricity
Solvent
Water dissociation Constant
mole
Electrolyte
30. 2.18 x 10^-18 J/electron
Triple point
Spin quantum number
Rydberg constant
electrolysis
31. A reaction in which two or more substances combine to form a single substance A+B>>>>>>>C
Combination Reaction
Spin quantum number
chemical reaction
Principle quantum number
32. Substance in which a solute is dissolved to form a solution
single displacement reaction
Diffusion
Common ion effect
Solvent
33. The process by which a gas escapes from one container to another at lower pressure through a tiny hole in the container.
Principle quantum number
hydrogen bonding
Effusion
Solvent
34. The weight in grams of compound that can be substituted by 1 atom of Hydrogen. GEW = MW / # of acidic Hyrdogens
bond energy
gram equivalent weight
Equlibrium constant
Ion
35. A horizontal row of elements in the periodic table
Triple point
Period
effective nuclear charge
Formula weight
36. Simplest whole # ration of atoms in a compound
Nonpolar covalent bond
Lyman series
Magnetic quantum number
Emperical Formula
37. The sum of the exponents in a rate law - where each exponent provides the reaction order with respect to its reactants
transition elements
Ion
Percent yield
Reaction order
38. Two or more atoms held together by covalent bonds
Colligative properties
molecule
Group 2A
representative elements
39. Halogens; ns2np5 - - 2nd most reactive group - The Halogens; very active because of need to fill; form -1 ions; 7 electrons in valence shell; tend to form salts with elements from groups 1A and 2A
Solvent
STP
Principle quantum number
Group 7A
40. Property of the elements that can be predicted from the arrangement of the periodic table
periodic trends
Conjugate acids and Bases
Diprotic Base
redox reaction
41. The pressure exerted by a vapor in equilibrium with its liquid or solid phase
Vapor pressure
Alkaline earths
effective nuclear charge
Amphoteric
42. The reaction of the ions that characterize acids and the ions that characterize bases to form water molecules and a salt
physical reaction
Aqueous Solution
Formula weight
Neutralization reaction
43. An atom or group of atoms that has a positive or negative charge
The bohr model
Rydberg constant
Ion
Normality
44. 5 valence electrons -3 ions - Nitride N
Rydberg constant
Lewis structure
Group 5A
Electrolyte
45. Rare earth element group (elements 58-71)
lathanide series
angular momentum in the bohr model
electron configuration
Formula weight
46. Large molecular structures - strong covalent bonding - share qualities of IONIC And COVALENT
Network covalent
effective nuclear charge
London forces
percent composition
47. Nh/2p The angular momentum changes only in discete amounts with respect to the quantum number. Also E=- R_h/n^2
empirical formula
angular momentum in the bohr model
atomic radius
Common ion effect
48. Set of spectral lines appearing in the UV region when a hydrogen atom undergoes a transition from energy levels n>1 to n=1.
Effective nuclear charge
Lyman series
lewis base
Vapor pressure
49. The nuclear charge experienced by the outermost electrons of an atom (actual charge minus the shielding caused by inner shells: Z- eff)
Octet Rule
Concentration
quantum
effective nuclear charge
50. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds
Net ionic equation
Raoult's Law
Group 4A
Solution equilibrium