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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 molar solubility of one salt is reduced when another salt - having a common ion is brought into the same solution
redox reaction
Solvent
Common ion effect
Planck's Constant
2. 2.18 x 10^-18 J/electron
Normality
Rydberg constant
Molecular orbital
atomic emission spectrum
3. An atom - ion - or molecule that donates an electron pair to form a covalent bond.
atomic theory
Group 6A
Solubility Product Constant
lewis base
4. The sum of the exponents in a rate law - where each exponent provides the reaction order with respect to its reactants
Reaction order
Concentration
Charles and Gay Lussac's Law
Acid dissociation constant
5. In a solution - the substance that dissolves in the solvent
Solubility Product Constant
pI
Solute
molecular weight
6. (chemistry) any theory in which all matter is composed of tiny discrete finite indivisible indestructible particles
pI
Reaction mechanism
atomic theory
single displacement reaction
7. 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
Molecular orbital
Titration
Pauli exclusion principle
atomic radius
8. An uncharged molecule with a single unpaitred electron in its outer ring - very unstable - exists for only about 10 seconds
Net ionic equation
Free radical
pI
Aqueous Solution
9. 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.
molecule
Solution equilibrium
Henderson Hasselbalch Equation
Common ion effect
10. Large molecular structures - strong covalent bonding - share qualities of IONIC And COVALENT
Network covalent
Diprotic Base
Alkaline earths
Group 4A
11. Simplest whole # ration of atoms in a compound
Emperical Formula
Collision theory of chemical Kinetics
Lewis structure
single displacement reaction
12. 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
d orbital
atomic emission spectrum
Decomposition reaction
13. Having characteristics of both an acid and a base and capable of reacting as either
single displacement reaction
Phase diagram
Equivalence point
Amphoteric
14. (physics) the smallest discrete quantity of some physical property that a system can possess (according to quantum theory) E=hf
quantum
Alkaline earths
theoretical yield
Redox Half Reaction
15. Property of the elements that can be predicted from the arrangement of the periodic table
VSEPR
Ion
Diffusion
periodic trends
16. An atom - radical - or molecule that has gained or lost one or more electrons and has a negative or positive charge
Nonpolar covalent bond
Dispersion Forces
Ion
sigma bond
17. 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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18. 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
Electronegativity
Network covalent
d orbital
19. A pair of equal and opposite electric charges or magnetic poles separated by a small distance
Hydrogen bonding
Equlibrium constant
Dipole
solvation
20. Elements in the middle of the periodic table - in groups 3-12.
Alkaline earths
Dispersion Forces
transition elements
Rydberg constant
21. A reaction in which atoms of one element take the place of atoms of another element in a compound
Henry's Law
single displacement reaction
Charles and Gay Lussac's Law
Combination Reaction
22. The number of atoms in exactly 12 g of pure 12c and equal to 6.022 x 10^23 is called
Avagadros number
ionic cmpound
Nucleus
Equilibrium
23. Chalcogens - - Oxide O
Pauli exclusion principle
Group 6A
Covalent Bond
electron affinity
24. 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
hydrogen bonding
Strong acid
Formal Charge
Titration
25. 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
Rydberg constant
Phase diagram
electromagnetic energy of photons emmited from electrons at ground state
26. The weight in grams of compound that can be substituted by 1 atom of Hydrogen. GEW = MW / # of acidic Hyrdogens
Equivalence point
gram equivalent weight
Chemical Kinetics
empirical formula
27. A dynamic condition in which two opposing changes occur at equal rates in a closed system
Equilibrium
Formal Charge
Resonance structure
redox reaction
28. 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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29. 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
Diffusion
atomic radius
Ionization energy
30. Slightly less reactive than alkali metals - comprise group II
Dipole
Common ion effect
Theoretical yield
Alkaline earths
31. A graph of pressure versus temperature that shows the conditions under which the phases of a substance exist
Amphoteric
Dipole
Phase diagram
atomic theory
32. A reaction in which atoms of one element take the place of atoms of another element in a compound
Group 4A
single displacement reaction
Ion dipole interactions
polymer
33. The quantum number that has only two possible values - +1/2 and -1/2 - which indicate the two fundamental spin states of an electron in an orbital
gram equivalent weight
Azeotrope
Diprotic Base
Spin quantum number
34. 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.
Atomic absorption Spectra
Combination Reaction
Percent yield
lewis base
35. (chemistry) a series from actinium to lawrencium of 15 radioactive elements with increasing atomic numbers
sigma bond
actinide series
atomic radius
Ion dipole interactions
36. The slowest elementary step which is the limit for the rate of the other steps
Rate determining step
empirical formula
Electronegativity
VSEPR
37. Process by which molecules tend to move from an area where they are more concentrated to an area where they are less concentrated
Resonance structure
Lyman series
quanta
Diffusion
38. 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
angular momentum in the bohr model
quanta
crystalline solid
Half equivalence point
39. A solution in which water is the solvent
STP
Molar solubility
Aqueous Solution
Phase diagram
40. Have the shape of a sphere - with the center of the sphere at the nucleus; completely symmetrical along all axes; 1s orbital is spherically symmetric and has no nodes; 2s orbital is also spherical but contains a node and is higher in energy
s orbital
effective nuclear charge
chemical reaction
Emperical Formula
41. An elementary particle with 0 charge and mass about equal to a proton
decomposition reaction
molecule
amorphous solid
Neutron
42. Attractions between molecules caused by the electron motion on one molecule affecting the electron motion on the other through electrical forces; these are the weakest interactions between molecules
Aqueous Solution
Halogens
Dispersion Forces
Ionization energy
43. Gram equivalent weight of solute per liter of solution - often denoted by N.
energy state
mole
Normality
Reaction mechanism
44. A base that can accept two moles of H+ per mole of itself (ex: SO4
Group 3A
Avagadros number
Hydrogen bonding
Diprotic Base
45. States that it is impossible to determine simultaneously both the position and momentum of an electron or any other particle
Molecular orbital
heisenberg uncertainty principle
redox reaction
Percent composition
46. 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
Ion product
Normality
Colligative properties
Lyman series
47. The center of the atom which contains the protons and neutrons; in cells - structure that contains the cell's genetic material (DNA) and controls the cell's activities
Halogens
empirical formula
Nucleus
Solvent
48. Rare earth element group (elements 58-71)
Half equivalence point
physical reaction
mole
lathanide series
49. The process by which a gas escapes from one container to another at lower pressure through a tiny hole in the container.
pH
Common ion effect
lathanide series
Effusion
50. Side - to side parallel orbitals overlap to share electrons - the 2nd/3rd covalent bond between two atoms - cannot rotate and maintain the bond.
Colligative properties
pi bonds
Group 5A
Ionic Bond