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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. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance
decomposition reaction
Colligative properties
effective nuclear charge
Hydrogen bonding
2. The ratio of the number of moles of solute dissolved in one kilogram of solvent. molality (M = moles solute/kg of solution)
Titration
Molality
Neutralization reaction
crystalline solid
3. Theory stating that the rate of a reaction is directly proportional to the number of collisions that take place between reactants per second.
Azeotrope
Solute
heisenberg uncertainty principle
Collision theory of chemical Kinetics
4. One - half the distance between the nuclei of two atoms of the same element when the atoms are joined
STP
Rate law
theoretical yield
atomic radius
5. 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
amorphous solid
bond length
Rydberg constant
Hydrogen bonding
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
heisenberg uncertainty principle
d orbital
Mass number
7. The maximum amount of product that can be produced from a given amount of reactant
Strong acid
physical reaction
theoretical yield
Equivalence point
8. Redox reaction - in which the same species is both oxidized and reduced.
Group 3A
Disproportionation
polymer
Rate law
9. Tells you how much solute is present compared to the amount of solvent
Theoretical yield
Spin quantum number
Azeotrope
Concentration
10. The average distance between the nuclei of two bonded atoms
Group 6A
d orbital
bond length
Proton
11. The process by which a gas escapes from one container to another at lower pressure through a tiny hole in the container.
Noble gases
Ground state
Effusion
Molarity
12. E=hc/?
Molality
electromagnetic energy of photons emmited from electrons at ground state
polymer
Ion
13. The amount of a substance that contains as many particles as there are atoms in exactly 12g of carbon -12
mole
Group 4A
Alkaline earths
sigma bond
14. No two electrons or protons or neutrons in a given system can be in states characterized by the same set of quantum numbers
Acid dissociation constant
Pauli exclusion principle
effective nuclear charge
pi bonds
15. Named after their cation and anion
ionic cmpound
Lewis structure
Half equivalence point
atomic theory
16. A dynamic condition in which two opposing changes occur at equal rates in a closed system
Percent yield
Decomposition reaction
Equilibrium
Intermolecular forces
17. 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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18. 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
Aqueous Solution
molecular weight
Lewis definition
Formal Charge
19. 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
Ion product
atomic radius
Disproportionation
20. The sum of the exponents in a rate law - where each exponent provides the reaction order with respect to its reactants
angular momentum in the bohr model
Reaction order
molecular weight
Magnetic quantum number
21. Common definition of acids as proton (H+) donors and bases as proton acceptors
Bronsted - Lowry definition
percent composition
single displacement reaction
Disproportionation
22. Substance in which a solute is dissolved to form a solution
Electronegativity
Solvent
Atomic absorption Spectra
pH
23. A solid made up of particles that are not arranged in a regular pattern.
electromagnetic energy of photons emmited from electrons at ground state
d orbital
amorphous solid
Group 1A
24. 1913 - Niels Bohr - said that electrons formed specific layers instead or random ones - said atoms atoms absorb and give off energy when the electrons move from one shell to another
indicator
s orbital
The bohr model
Group 3A
25. 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.
Strong acid
periodic trends
transition elements
Principle quantum number
26. Temperature is constant; effusion and temperature are proportional to the square root of their masses
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27. The nuclear charge experienced by the outermost electrons of an atom (actual charge minus the shielding caused by inner shells: Z- eff)
hydrogen bonding
effective nuclear charge
actinide series
Formula weight
28. Large molecular structures - strong covalent bonding - share qualities of IONIC And COVALENT
Normality
Alkaline earths
Concentration
Network covalent
29. 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.
Balmer series
Emperical Formula
Reaction order
London forces
30. 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.
Concentration
Chemical Kinetics
und's rule
Henderson Hasselbalch Equation
31. 5 valence electrons -3 ions - Nitride N
Resonance structure
Rate determining step
Concentration
Group 5A
32. 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
lewis base
Rydberg constant
Colligative properties
Combination Reaction
33. (chemistry) a substance that changes color to indicate the presence of some ion or substance
indicator
Mass number
actinide series
Group 2A
34. Gram equivalent weight of solute per liter of solution - often denoted by N.
atomic radius
Normality
Neutron
decomposition reaction
35. 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
Covalent Bond
Formal Charge
Nucleus
Principle quantum number
36. A reaction in which two or more substances combine to form a single substance A+B>>>>>>>C
Rate determining step
Group 3A
Combination Reaction
energy state
37. 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
quantum
s orbital
atomic radius
effective nuclear charge
38. An elementary particle with 0 charge and mass about equal to a proton
Neutron
Molality
Lewis structure
Activation energy
39. Simplest whole # ration of atoms in a compound
atomic emission spectrum
Ion dipole interactions
Emperical Formula
amorphous solid
40. At a constant pressure - the volume of an ideal gas is directly proportinal to its temperature: V (a) T
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41. Systematic pairing of a deprotonated species (base) with its protonated form (conjugate acid). Conjugates appear on opposite sides of a chemical equation.
law of constant composition
Buffer
Conjugate acids and Bases
Ionic Bond
42. The lowest allowable energy state of an atom
STP
Ground state
representative elements
Graham's Law
43. Slightly less reactive than alkali metals - comprise group II
Percent yield
Avagadros number
Lyman series
Alkaline earths
44. 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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45. Alkali metals: highly reactive - therefore always compounds. - 1 valence electron +1 ion - Hydrogen H? - Lithium Li? - Sodium Na? - Potassium K? - Rubidium Rb? - Cesium Cs?
Solvent
Molecular orbital
Noble gases
Group 1A
46. A reaction where a compound does Not change its molecular structure.
Half equivalence point
und's rule
Electronegativity
physical reaction
47. An emperimentally determined mathmatical expression showing the rate of a reaction as a function of the concentration of its reactants
representative elements
Effusion
Rate law
Arrhenius Definition
48. Numbers that specify the properties of atomic orbitals and of their electrons
quantum numbers
electromagnetic energy of photons emmited from electrons at ground state
Rydberg constant
Ground state
49. A reaction in which atoms of one element take the place of atoms of another element in a compound
amorphous solid
Effective nuclear charge
single displacement reaction
Molality
50. 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.
amorphous solid
Ion product
London forces
The bohr model