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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. Theory stating that the rate of a reaction is directly proportional to the number of collisions that take place between reactants per second.
atomic radius
Collision theory of chemical Kinetics
Mass number
Intermolecular forces
2. 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
quantum
Balmer series
Diffusion
3. 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.
Effusion
Solubility Product Constant
London forces
Avagadros number
4. When dipoles are dissolved in a solution where ions are present ions wil arrange themselves with the opposite charged end of the dipole.
Covalent Bond
Ion dipole interactions
Proton
Reaction mechanism
5. Side - to side parallel orbitals overlap to share electrons - the 2nd/3rd covalent bond between two atoms - cannot rotate and maintain the bond.
crystalline solid
Atomic weight
pi bonds
quantum
6. A definite stable energy that a physical system can have
energy state
Atomic absorption Spectra
Noble gases
Graham's Law
7. A concentration unit of a solution expressed as moles of solute dissolved per liter of solution
Dipole
Diprotic Base
Intermolecular forces
Molarity
8. 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
Dispersion Forces
Octet Rule
decomposition reaction
Lewis acid base reaction
9. (chemistry) a substance formed by chemical union of two or more elements or ingredients in definite proportion by weight
Colligative properties
Alkaline earths
Lyman series
compound
10. PH of a molecule at which it contains no net electric charge - isoelectric point.
pI
pi bonds
energy state
effective nuclear charge
11. Chalcogens - - Oxide O
Neutron
decomposition reaction
Group 6A
Reaction order
12. The molar solubility of one salt is reduced when another salt - having a common ion is brought into the same solution
Common ion effect
subshell
Solution equilibrium
Collision theory of chemical Kinetics
13. 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
transition elements
lewis base
Group 6A
Proton
14. Tells you how much solute is present compared to the amount of solvent
Group 3A
Concentration
angular momentum in the bohr model
empirical formula
15. 5 different orbitals shaped like clover leaves and max electrons is 10
theoretical yield
d orbital
Free radical
Equilibrium
16. The pressure exerted by a vapor in equilibrium with its liquid or solid phase
Effusion
Vapor pressure
Graham's Law
Alkaline earths
17. The number of atoms in exactly 12 g of pure 12c and equal to 6.022 x 10^23 is called
Avagadros number
Resonance structure
Free radical
Solubility Product Constant
18. States that it is impossible to determine simultaneously both the position and momentum of an electron or any other particle
heisenberg uncertainty principle
Ionic Bond
polymer
Proton
19. An equilibrium expression used to measure weak - acid strength - given by the ratio of the product of the products' molar concentrations to the product of the reactants' molar concentrations - with each term raised to the power of its stoichiometric
Formal Charge
pi bonds
Acid dissociation constant
Arrhenius Definition
20. The process of decomposing a chemical compound by the passage of an electric current.
Dipole Dipole interaction
electrolysis
Azeotrope
heisenberg uncertainty principle
21. The average distance between the nuclei of two bonded atoms
Percent yield
quantum numbers
electrolysis
bond length
22. Contains nonmetals - 7 valence electrons in it's outermost energy level. Very reactive
Magnetic quantum number
lewis base
Halogens
Equilibrium
23. 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.
Net ionic equation
Hydrogen bonding
Solute
Principle quantum number
24. The process by which one or more substances change to produce one or more different substances
chemical reaction
Percent composition
Lewis acid base reaction
Amphoteric
25. A horizontal row of elements in the periodic table
Period
single displacement reaction
Redox Half Reaction
Molarity
26. A chemical bond in which one atom loses an electron to form a positive ion and the other atom gains to electron to form a negative ion
d orbital
compound
Ionic Bond
angular momentum in the bohr model
27. Acids defined as electron - pair acceptors and bases as electron - pair donors.
Balmer series
Pauli exclusion principle
Lewis definition
theoretical yield
28. A graph of pressure versus temperature that shows the conditions under which the phases of a substance exist
Ion
Phase diagram
bond energy
periodic trends
29. The sum of the exponents in a rate law - where each exponent provides the reaction order with respect to its reactants
azimuthal quantum number
Reaction order
electron configuration
Combination Reaction
30. 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
Ionization energy
Raoult's Law
periodic trends
31. Gram equivalent weight of solute per liter of solution - often denoted by N.
Normality
indicator
Percent composition
Lewis definition
32. A covalent bond in which the bonding electrons are shared equally by the bonded atoms - resulting in a balanced distribution of electrical charge
Pauli exclusion principle
Atomic absorption Spectra
Arrhenius Definition
Nonpolar covalent bond
33. Play- by- play showing the individual steps of a reaction - including the formation and destruction of any reaction intermediates that may occur.
Molecular orbital
Group 3A
Ion product
Reaction mechanism
34. Any sample of a given compound will contain the same elements in the identical mass ratio.
mole
Ion
law of constant composition
Ionic Bond
35. 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.
Nucleus
Atomic absorption Spectra
Mass number
Effective nuclear charge
36. 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
und's rule
Group 1A
Lewis definition
hydrogen bonding
37. 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
Network covalent
Percent yield
Collision theory of chemical Kinetics
Magnetic quantum number
38. 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
Theoretical yield
representative elements
STP
crystalline solid
39. An emperimentally determined mathmatical expression showing the rate of a reaction as a function of the concentration of its reactants
Rate law
Arrhenius Definition
Percent yield
Phase diagram
40. 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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41. A chemical bond that involves sharing a pair of electrons between atoms in a molecule
Covalent Bond
Azeotrope
atomic radius
Vapor pressure
42. A bond formed when two atomic orbitals combine to form a molecular orbital that is symmetrical around the axis connecting the two atomic nuclei
lewis base
Theoretical yield
Nonpolar covalent bond
sigma bond
43. (physics) the smallest discrete quantity of some physical property that a system can possess (according to quantum theory) E=hf
Ground state
Redox Half Reaction
Chemical Kinetics
quantum
44. Slightly less reactive than alkali metals - comprise group II
Alkaline earths
Ion product
Group 4A
Theoretical yield
45. An uncharged molecule with a single unpaitred electron in its outer ring - very unstable - exists for only about 10 seconds
Free radical
electromagnetic energy of photons emmited from electrons at ground state
Dipole Dipole interaction
single displacement reaction
46. Product of the molar concentrations of dissociated ions in solution at any point in the reaction other than equilibrium or saturation - where each ion is raised to the power of its stoichiometric coefficient. Denoted IP.
Group 4A
Collision theory of chemical Kinetics
Network covalent
Ion product
47. A pair of equal and opposite electric charges or magnetic poles separated by a small distance
Solvent
Rate law
Dipole
Mass number
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.
lathanide series
atomic theory
Lyman series
STP
49. One - half the distance between the nuclei of two atoms of the same element when the atoms are joined
Rydberg constant
Half equivalence point
atomic radius
gram equivalent weight
50. The lowest allowable energy state of an atom
Amphoteric
Collision theory of chemical Kinetics
electron affinity
Ground state