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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. The weight in grams of compound that can be substituted by 1 atom of Hydrogen. GEW = MW / # of acidic Hyrdogens
ionic cmpound
Amphoteric
gram equivalent weight
s orbital
2. The amount of product that can be made in a chemical reaction based on the amount of limiting reactant
heisenberg uncertainty principle
Theoretical yield
Chemical Kinetics
redox reaction
3. A reaction in which two or more substances combine to form a single substance A+B>>>>>>>C
s orbital
Combination Reaction
Strong acid
electron configuration
4. 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
Ion product
Vapor pressure
representative elements
Decomposition reaction
5. (chemistry) a substance that changes color to indicate the presence of some ion or substance
Percent yield
s orbital
Dipole Dipole interaction
indicator
6. A horizontal row of elements in the periodic table
quantum
Redox Half Reaction
Period
Lewis acid base reaction
7. (chemistry) any theory in which all matter is composed of tiny discrete finite indivisible indestructible particles
atomic theory
Dipole
Effective nuclear charge
Diprotic Base
8. The process by which one or more substances change to produce one or more different substances
Chemical Kinetics
chemical reaction
Principle quantum number
Formula weight
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
Magnetic quantum number
mole
Group 4A
Percent yield
10. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance
Electrolyte
mole
Vapor pressure
decomposition reaction
11. A concentration unit of a solution expressed as moles of solute dissolved per liter of solution
Triple point
Concentration
Molarity
Le chateliers Principle
12. 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
Planck's Constant
theoretical yield
Arrhenius Definition
13. An emperimentally determined mathmatical expression showing the rate of a reaction as a function of the concentration of its reactants
Rate law
Electrolyte
Half equivalence point
crystalline solid
14. The lowest allowable energy state of an atom
molecular weight
Henry's Law
energy state
Ground state
15. An ionic compound that resists changes in its pH
atomic emission spectrum
Principle quantum number
heisenberg uncertainty principle
Buffer
16. Any sample of a given compound will contain the same elements in the identical mass ratio.
Effective nuclear charge
crystalline solid
atomic emission spectrum
law of constant composition
17. A solution in which water is the solvent
Free radical
Solution equilibrium
Group 3A
Aqueous Solution
18. The quantum number that indicates the main energy level occupied by the electron. Can theoretically take on any positive interger. Denoted by the letter n.
Principle quantum number
ionic cmpound
Net ionic equation
chemical reaction
19. Temperature is constant; effusion and temperature are proportional to the square root of their masses
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20. Sum of all the masses - in AMU - present in one molecule of a molecular compound.
Formula weight
Halogens
Principle quantum number
energy state
21. 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.
Charles and Gay Lussac's Law
crystalline solid
single displacement reaction
Group 5A
22. The ways in which electrons are arranged in various orbitals around the nuclei of atoms
Triple point
Nucleus
electron configuration
Equilibrium
23. Play- by- play showing the individual steps of a reaction - including the formation and destruction of any reaction intermediates that may occur.
Reaction mechanism
Lewis structure
physical reaction
Avagadros number
24. An acid that will completely dissociate in aqueous solution - like HCl - HI - HClO4 HBr.
d orbital
Strong acid
quantum
Equlibrium constant
25. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds
Electrolyte
Group 4A
Hydrogen bonding
Henry's Law
26. PH of a molecule at which it contains no net electric charge - isoelectric point.
law of constant composition
theoretical yield
Octet Rule
pI
27. Named after their cation and anion
Formal Charge
ionic cmpound
Buffer
decomposition reaction
28. Contains nonmetals that are non - reactive. Full outermost energy level except helium which has 2.
Reaction mechanism
Equivalence point
Concentration
Noble gases
29. 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
Proton
indicator
Ionic Bond
Solute
30. (chemistry) a substance formed by chemical union of two or more elements or ingredients in definite proportion by weight
Percent composition
quantum numbers
compound
Theoretical yield
31. Alkali metals: highly reactive - therefore always compounds. - 1 valence electron +1 ion - Hydrogen H? - Lithium Li? - Sodium Na? - Potassium K? - Rubidium Rb? - Cesium Cs?
Effective nuclear charge
Electrolyte
Principle quantum number
Group 1A
32. Atoms react by gaining or losing electrons so as to acquire the stable electron structure of a noble gas - usually eight valence electrons
gram equivalent weight
Octet Rule
actinide series
Free radical
33. Substance in which a solute is dissolved to form a solution
Neutralization reaction
Rydberg constant
Solvent
Molecular orbital
34. The number of atoms in exactly 12 g of pure 12c and equal to 6.022 x 10^23 is called
Molar solubility
Avagadros number
Percent composition
Lewis structure
35. A reaction in which atoms of one element take the place of atoms of another element in a compound
Henderson Hasselbalch Equation
Ion product
periodic trends
single displacement reaction
36. Set of spectral lines appearing in the UV region when a hydrogen atom undergoes a transition from energy levels n>1 to n=1.
actinide series
Bronsted - Lowry definition
Lyman series
Rate law
37. Property of the elements that can be predicted from the arrangement of the periodic table
redox reaction
periodic trends
Disproportionation
Group 5A
38. Tells you how much solute is present compared to the amount of solvent
Azeotrope
Noble gases
Ion
Concentration
39. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance C>>>>A+B
Decomposition reaction
Ion dipole interactions
Theoretical yield
atomic theory
40. 5 valence electrons -3 ions - Nitride N
solvation
Group 5A
Hydrogen bonding
Ion dipole interactions
41. 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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42. A graph of pressure versus temperature that shows the conditions under which the phases of a substance exist
Bronsted Lowry
single displacement reaction
Phase diagram
Lewis acid base reaction
43. Standard Temperature and Pressure. 273 Kelvin (0 Celsius) - 1 atmosphere (760 torr - 760 kPA).
STP
Dipole Dipole interaction
Rate determining step
chemical reaction
44. Redox reaction - in which the same species is both oxidized and reduced.
molecular weight
Disproportionation
redox reaction
Neutralization reaction
45. 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
Solution equilibrium
Reaction mechanism
atomic radius
Solute
46. Numbers that specify the properties of atomic orbitals and of their electrons
STP
quantum numbers
amorphous solid
Electrolyte
47. Acids defined as electron - pair acceptors and bases as electron - pair donors.
Solubility Product Constant
Group 4A
Conjugate acids and Bases
Lewis definition
48. The point on a phase diagram that represents the only set of conditions at which all three phases exist in equilibrium with one another
Solute
Triple point
gram equivalent weight
Percent yield
49. An uncharged molecule with a single unpaitred electron in its outer ring - very unstable - exists for only about 10 seconds
effective nuclear charge
Free radical
percent composition
Group 2A
50. A pair of equal and opposite electric charges or magnetic poles separated by a small distance
Dipole
Neutralization reaction
electromagnetic energy of photons emmited from electrons at ground state
Ionization energy