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Test your basic knowledge |
MCAT Chemistry
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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. Contains nonmetals - 7 valence electrons in it's outermost energy level. Very reactive
quantum numbers
Halogens
quanta
Triple point
2. 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.
effective nuclear charge
Henderson Hasselbalch Equation
electron affinity
angular momentum in the bohr model
3. Attractive and repulsive forces between molecules that are weaker than forces within molecules.
Amphoteric
Dispersion Forces
Magnetic quantum number
Intermolecular forces
4. Named after their cation and anion
Half equivalence point
ionic cmpound
solvation
crystalline solid
5. Gram equivalent weight of solute per liter of solution - often denoted by N.
Octet Rule
lathanide series
Molar solubility
Normality
6. Specifies the specific orbital in which the electron is most likely to be found. - Third quantum number - designated as ml. Describes a particular orbital within a subshell where an electron is very likely to be found. Possible values are integers in
Conjugate acids and Bases
Nonpolar covalent bond
Magnetic quantum number
Charles and Gay Lussac's Law
7. Sol - a chemical process in which solvent molecules and molecules or ions of the solute combine to form a compound
solvation
mole
The bohr model
Molality
8. The process by which one or more substances change to produce one or more different substances
chemical reaction
periodic trends
Vapor pressure
Rydberg constant
9. When dipoles are dissolved in a solution where ions are present ions wil arrange themselves with the opposite charged end of the dipole.
Le chateliers Principle
Arrhenius Definition
Ion dipole interactions
Lyman series
10. The amount of energy that reactants must absorb before a chemical reaction will start; also called free energy of activation.
Pauli exclusion principle
Group 5A
redox reaction
Activation energy
11. 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.
electrolysis
crystalline solid
electron affinity
Charles and Gay Lussac's Law
12. 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
Collision theory of chemical Kinetics
periodic trends
Equlibrium constant
Azeotrope
13. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
indicator
redox reaction
electrolysis
Strong acid
14. Any sample of a given compound will contain the same elements in the identical mass ratio.
law of constant composition
Ionization energy
hydrogen bonding
Lewis structure
15. A model of acids and bases which an acid is hydrogen ion donor and base is a hydrogen ion acceptor.
Aqueous Solution
crystalline solid
Bronsted Lowry
Colligative properties
16. Atoms react by gaining or losing electrons so as to acquire the stable electron structure of a noble gas - usually eight valence electrons
Octet Rule
The bohr model
physical reaction
subshell
17. The weight in grams of one mole of a given elementand is expressedin tems of grams per mole.
Octet Rule
Atomic weight
electromagnetic energy of photons emmited from electrons at ground state
Resonance structure
18. An atom - ion - or molecule that donates an electron pair to form a covalent bond.
Ionization energy
lewis base
Nucleus
Aqueous Solution
19. 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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20. The tendency for an atom to attract electrons to itself when it is chemically combined with another element
Dipole
Ionization energy
Electronegativity
Rate determining step
21. 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
Group 6A
Ion
ionic cmpound
azimuthal quantum number
22. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance
Amphoteric
Activation energy
decomposition reaction
atomic emission spectrum
23. 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
Buffer
representative elements
Effusion
Dispersion Forces
24. (chemistry) a series from actinium to lawrencium of 15 radioactive elements with increasing atomic numbers
ionic cmpound
actinide series
transition elements
Ionic Bond
25. An elementary particle with 0 charge and mass about equal to a proton
Theoretical yield
Arrhenius Definition
Electrolyte
Neutron
26. Resulting positive nuclear charge an outer electron senses after accounting for the shielding effect of inner core electrons. Abbreviated as Z(eff). Increases from left to right - and bottom to top on the Periodic Table.
Azeotrope
Solvent
bond length
Effective nuclear charge
27. 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
redox reaction
electron affinity
Phase diagram
28. 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
Octet Rule
Proton
Pauli exclusion principle
lathanide series
29. Nh/2p The angular momentum changes only in discete amounts with respect to the quantum number. Also E=- R_h/n^2
Formula weight
angular momentum in the bohr model
lewis base
Proton
30. Expression of auto - ionization of water into H+ and OH- at a certain temperature - given by the product of the ions' molar concentrations. Denoted by Kw and equal to 10-
Noble gases
Water dissociation Constant
Bronsted Lowry
Solution equilibrium
31. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds
Normality
Ion dipole interactions
Ion
Group 4A
32. A set of spectral lines that appear in the visible light region when a hydrogen atom undergoes a transition from energy levels n>2 to n=2.
Group 5A
Balmer series
Bronsted - Lowry definition
Chemical Kinetics
33. The number of atoms in exactly 12 g of pure 12c and equal to 6.022 x 10^23 is called
Equilibrium
Avagadros number
effective nuclear charge
Group 2A
34. Acids defined as electron - pair acceptors and bases as electron - pair donors.
Lewis acid base reaction
electron affinity
Decomposition reaction
Lewis definition
35. A bond formed when two atomic orbitals combine to form a molecular orbital that is symmetrical around the axis connecting the two atomic nuclei
Chemical Kinetics
atomic radius
Atomic weight
sigma bond
36. Alkali metals: highly reactive - therefore always compounds. - 1 valence electron +1 ion - Hydrogen H? - Lithium Li? - Sodium Na? - Potassium K? - Rubidium Rb? - Cesium Cs?
Chemical Kinetics
hydrogen bonding
Group 1A
electrolysis
37. A substance that - when dissolved in water - results in a solution that can conduct electricity
Phase diagram
indicator
Electrolyte
Dipole Dipole interaction
38. E=hc/?
Redox Half Reaction
Rate determining step
s orbital
electromagnetic energy of photons emmited from electrons at ground state
39. Chalcogens - - Oxide O
Disproportionation
Amphoteric
Group 6A
quantum numbers
40. 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.
Ground state
Neutron
Formula weight
electron affinity
41. 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
d orbital
Group 6A
Raoult's Law
42. Two or more atoms held together by covalent bonds
London forces
Disproportionation
molecule
gram equivalent weight
43. Alkaline Earth Metals - 2 valence electrons +2 ions - Magnesium Mg
Group 2A
Molar solubility
transition elements
heisenberg uncertainty principle
44. A structural formula in which electrons are represented by dots; dot pairs or dashes between two atomic symbols represent pairs in covalent bonds.
Lewis structure
Strong acid
Conjugate acids and Bases
Phase diagram
45. The slowest elementary step which is the limit for the rate of the other steps
Chemical Kinetics
Normality
Rate determining step
polymer
46. Where half of the acid is neutralized by the base on a titration curveAn acid dissociation constant - Ka - (also known as acidity constant - or acid - ionization constant) is a quantitative measure of the strength of an acid in solution. It is the eq
Half equivalence point
und's rule
Rate law
Azeotrope
47. A solution in which water is the solvent
Concentration
Aqueous Solution
Rate law
electron configuration
48. 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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49. A naturally occurring or synthetic compound consisting of large molecules made up of a linked series of repeated simple monomers
mole
Free radical
Principle quantum number
polymer
50. The formation of one or more covalent bonds between an electron pair donor and an electron pair acceptor
Lewis acid base reaction
Molar solubility
Diprotic Base
London forces