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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 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
Rate law
Common ion effect
ionic cmpound
hydrogen bonding
2. 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
Magnetic quantum number
lewis base
Resonance structure
azimuthal quantum number
3. (physics) the smallest discrete quantity of some physical property that a system can possess (according to quantum theory) E=hf
Ground state
Arrhenius Definition
hydrogen bonding
quantum
4. (chemistry) p(otential of) H(ydrogen)
actinide series
Group 5A
Colligative properties
pH
5. 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
Octet Rule
Free radical
Rate determining step
Titration
6. Have three valance electrons. In certain instances - some elements will loose three electrons - but they will also share electrons with another element to attain stability.
Group 3A
Common ion effect
Group 5A
Ionic Bond
7. Property of the elements that can be predicted from the arrangement of the periodic table
Equlibrium constant
Electronegativity
periodic trends
amorphous solid
8. One - half the distance between the nuclei of two atoms of the same element when the atoms are joined
Normality
Formal Charge
atomic radius
Rate law
9. Named after their cation and anion
Percent yield
Henderson Hasselbalch Equation
ionic cmpound
Dispersion Forces
10. Temperature is constant; effusion and temperature are proportional to the square root of their masses
11. 5 different orbitals shaped like clover leaves and max electrons is 10
heisenberg uncertainty principle
The bohr model
Molar solubility
d orbital
12. A structural formula in which electrons are represented by dots; dot pairs or dashes between two atomic symbols represent pairs in covalent bonds.
Raoult's Law
Lewis structure
Theoretical yield
molecule
13. When dipoles are dissolved in a solution where ions are present ions wil arrange themselves with the opposite charged end of the dipole.
Ion dipole interactions
bond length
empirical formula
lathanide series
14. Any sample of a given compound will contain the same elements in the identical mass ratio.
VSEPR
law of constant composition
Net ionic equation
atomic radius
15. 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
16. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
Molarity
Group 5A
molecule
redox reaction
17. One - half of the distance between the center of identical atoms that are not bonded together. Since effective nuclear charge increases when moving from left to right each additional electron is pulled more strogly toward the nucleus.
Ionic Bond
Molality
Alkaline earths
atomic radius
18. Tells you how much solute is present compared to the amount of solvent
amorphous solid
atomic radius
single displacement reaction
Concentration
19. (chemistry) a substance that changes color to indicate the presence of some ion or substance
Atomic absorption Spectra
Free radical
Raoult's Law
indicator
20. 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.
Arrhenius Definition
theoretical yield
decomposition reaction
crystalline solid
21. The percent by mass of each element in a compound
Diffusion
Equilibrium
Formal Charge
percent composition
22. PH=pka+log[base/acid] Used in titration based problems that relates the pH or pOH of a solution to the pK and the ratio of the dissociated species.
Lyman series
Henderson Hasselbalch Equation
Group 2A
Avagadros number
23. 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
Percent yield
Principle quantum number
Effusion
bond energy
24. The hypothetical equation showing only the species that is oxidized or reduced in a redox reaction and the correct number of electrons transferred between the species in the complete - balanced equation.
Half equivalence point
angular momentum in the bohr model
Redox Half Reaction
Lewis acid base reaction
25. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds
electron configuration
s orbital
Common ion effect
Group 4A
26. The process by which one or more substances change to produce one or more different substances
single displacement reaction
polymer
chemical reaction
representative elements
27. The tendency for an atom to attract electrons to itself when it is chemically combined with another element
Ion
Buffer
Electronegativity
Aqueous Solution
28. Contains nonmetals - 7 valence electrons in it's outermost energy level. Very reactive
quantum numbers
Theoretical yield
Halogens
lathanide series
29. In a solution - the substance that dissolves in the solvent
Solute
Dispersion Forces
Molar solubility
Group 3A
30. Chalcogens - - Oxide O
Hydrogen bonding
actinide series
Group 6A
Raoult's Law
31. The slowest elementary step which is the limit for the rate of the other steps
mole
Rate determining step
Lyman series
Nucleus
32. Redox reaction - in which the same species is both oxidized and reduced.
Bronsted - Lowry definition
Disproportionation
energy state
Molar solubility
33. The amount of energy that reactants must absorb before a chemical reaction will start; also called free energy of activation.
Activation energy
Alkaline earths
polymer
electron configuration
34. 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
Reaction mechanism
Strong acid
Molality
35. A concentration unit of a solution expressed as moles of solute dissolved per liter of solution
single displacement reaction
Dispersion Forces
Emperical Formula
Molarity
36. Rare earth element group (elements 58-71)
lathanide series
Raoult's Law
molecular weight
bond energy
37. The energy required to break a chemical bond and form neutral isolated atoms
bond energy
Arrhenius Definition
Collision theory of chemical Kinetics
Atomic weight
38. The amount of a substance that contains as many particles as there are atoms in exactly 12g of carbon -12
mole
und's rule
hydrogen bonding
Collision theory of chemical Kinetics
39. The sum of the exponents in a rate law - where each exponent provides the reaction order with respect to its reactants
chemical reaction
Planck's Constant
Electronegativity
Reaction order
40. The number of atoms in exactly 12 g of pure 12c and equal to 6.022 x 10^23 is called
Free radical
Ionization energy
Avagadros number
Spin quantum number
41. Alkali metals: highly reactive - therefore always compounds. - 1 valence electron +1 ion - Hydrogen H? - Lithium Li? - Sodium Na? - Potassium K? - Rubidium Rb? - Cesium Cs?
atomic theory
Group 1A
Half equivalence point
sigma bond
42. A solid made up of particles that are not arranged in a regular pattern.
indicator
Equlibrium constant
atomic radius
amorphous solid
43. Attractive and repulsive forces between molecules that are weaker than forces within molecules.
lewis base
Intermolecular forces
Redox Half Reaction
electromagnetic energy of photons emmited from electrons at ground state
44. The lowest allowable energy state of an atom
Vapor pressure
decomposition reaction
Ground state
Molarity
45. The process by which a gas escapes from one container to another at lower pressure through a tiny hole in the container.
Chemical Kinetics
Effusion
heisenberg uncertainty principle
Percent composition
46. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance
Rydberg constant
physical reaction
decomposition reaction
atomic radius
47. A horizontal row of elements in the periodic table
Planck's Constant
Effective nuclear charge
Period
decomposition reaction
48. A pair of equal and opposite electric charges or magnetic poles separated by a small distance
sigma bond
Rate determining step
Net ionic equation
Dipole
49. Play- by- play showing the individual steps of a reaction - including the formation and destruction of any reaction intermediates that may occur.
Bronsted Lowry
Reaction mechanism
Bronsted - Lowry definition
Electrolyte
50. The process of decomposing a chemical compound by the passage of an electric current.
polymer
electrolysis
ionic cmpound
Ground state