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MCAT Chemistry
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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. The slowest elementary step which is the limit for the rate of the other steps
Rate determining step
electromagnetic energy of photons emmited from electrons at ground state
Planck's Constant
Diprotic Base
2. (chemistry) a series from actinium to lawrencium of 15 radioactive elements with increasing atomic numbers
lathanide series
The bohr model
actinide series
subshell
3. 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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4. No two electrons or protons or neutrons in a given system can be in states characterized by the same set of quantum numbers
Electronegativity
Pauli exclusion principle
Normality
Vapor pressure
5. A reaction in which atoms of one element take the place of atoms of another element in a compound
single displacement reaction
Group 6A
actinide series
Period
6. 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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7. 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
single displacement reaction
und's rule
Noble gases
8. 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.
Activation energy
Henderson Hasselbalch Equation
Rate determining step
STP
9. An emperimentally determined mathmatical expression showing the rate of a reaction as a function of the concentration of its reactants
Group 7A
energy state
STP
Rate law
10. 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
law of constant composition
Collision theory of chemical Kinetics
Percent yield
Rate determining step
11. A set of frequencies of electromagnetic waves given off by atoms of an element; consists of a series of fine lines of individual colors
Rydberg constant
Mass number
atomic emission spectrum
Group 2A
12. Acids defined as electron - pair acceptors and bases as electron - pair donors.
Lewis definition
Free radical
atomic theory
atomic radius
13. The area of chemistry that is concerned with reaction rates and reaction mechanisms
pH
STP
electron affinity
Chemical Kinetics
14. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds
Group 3A
Group 4A
Bronsted Lowry
Graham's Law
15. Property of the elements that can be predicted from the arrangement of the periodic table
Ion dipole interactions
periodic trends
Spin quantum number
Diffusion
16. A solid made up of particles that are not arranged in a regular pattern.
Rate law
Avagadros number
pi bonds
amorphous solid
17. Defined acids as subtsances that produced H ions in water - while bases produced OH ions. When they reacted together - H and OH neutralise to make water
Decomposition reaction
ionic cmpound
Pauli exclusion principle
Arrhenius Definition
18. Process by which molecules tend to move from an area where they are more concentrated to an area where they are less concentrated
Network covalent
effective nuclear charge
Diffusion
Theoretical yield
19. A horizontal row of elements in the periodic table
Ground state
Nonpolar covalent bond
Period
Resonance structure
20. 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
Lewis acid base reaction
quantum
electromagnetic energy of photons emmited from electrons at ground state
The bohr model
21. Small discrete increments of energy.
Graham's Law
quanta
Alkaline earths
atomic emission spectrum
22. The weak attractive forces between molecules resulting from the small - instantaneous dipoles that occur because of the varying positions of the electrons during their motion about nuclei
transition elements
Rydberg constant
Equilibrium
London forces
23. 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
azimuthal quantum number
Group 2A
solvation
Effusion
24. A pair of equal and opposite electric charges or magnetic poles separated by a small distance
Dipole
bond length
Effusion
Formal Charge
25. 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
Ionic Bond
Effective nuclear charge
electron affinity
26. Numbers that specify the properties of atomic orbitals and of their electrons
Group 7A
electron affinity
Theoretical yield
quantum numbers
27. Side - to side parallel orbitals overlap to share electrons - the 2nd/3rd covalent bond between two atoms - cannot rotate and maintain the bond.
Rate determining step
atomic emission spectrum
pi bonds
Dipole Dipole interaction
28. 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
d orbital
atomic radius
STP
29. Temperature is constant; effusion and temperature are proportional to the square root of their masses
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30. (chemistry) a substance that changes color to indicate the presence of some ion or substance
indicator
effective nuclear charge
Charles and Gay Lussac's Law
gram equivalent weight
31. 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
Solvent
chemical reaction
Disproportionation
32. Attractive and repulsive forces between molecules that are weaker than forces within molecules.
VSEPR
London forces
Intermolecular forces
Arrhenius Definition
33. 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
Resonance structure
polymer
Rydberg constant
Hydrogen bonding
34. 2.18 x 10^-18 J/electron
Rydberg constant
Titration
subshell
bond length
35. The weight in grams of one mole of a given elementand is expressedin tems of grams per mole.
Group 4A
STP
Atomic weight
Nonpolar covalent bond
36. Mixture of 2 or more substances that distills at a constant temperature and with constant composition - even though seperately the components have different boiling points
Balmer series
Reaction order
Azeotrope
Water dissociation Constant
37. Two or more atoms held together by covalent bonds
Equilibrium
molecule
gram equivalent weight
theoretical yield
38. 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
hydrogen bonding
Raoult's Law
law of constant composition
actinide series
39. A structural formula in which electrons are represented by dots; dot pairs or dashes between two atomic symbols represent pairs in covalent bonds.
Group 5A
Ion dipole interactions
Lewis structure
Activation energy
40. Substance in which a solute is dissolved to form a solution
Solvent
single displacement reaction
compound
Group 6A
41. A base that can accept two moles of H+ per mole of itself (ex: SO4
Diprotic Base
Group 1A
Charles and Gay Lussac's Law
Resonance structure
42. 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-
percent composition
Water dissociation Constant
Graham's Law
Chemical Kinetics
43. The point on a phase diagram that represents the only set of conditions at which all three phases exist in equilibrium with one another
atomic radius
Solute
theoretical yield
Triple point
44. Gram equivalent weight of solute per liter of solution - often denoted by N.
Molality
physical reaction
subshell
Normality
45. Region in a molecule where atomic orbitals overlap - resulting in either a stable low - energy bonding orbital or an unstable high - energy antibonding orbital.
indicator
Redox Half Reaction
Half equivalence point
Molecular orbital
46. A dynamic condition in which two opposing changes occur at equal rates in a closed system
effective nuclear charge
pH
Group 4A
Equilibrium
47. Halogens; ns2np5 - - 2nd most reactive group - The Halogens; very active because of need to fill; form -1 ions; 7 electrons in valence shell; tend to form salts with elements from groups 1A and 2A
single displacement reaction
Group 4A
Conjugate acids and Bases
Group 7A
48. Any sample of a given compound will contain the same elements in the identical mass ratio.
electrolysis
und's rule
law of constant composition
molecule
49. Play- by- play showing the individual steps of a reaction - including the formation and destruction of any reaction intermediates that may occur.
Octet Rule
electrolysis
Reaction mechanism
Charles and Gay Lussac's Law
50. 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.
Ground state
Redox Half Reaction
sigma bond
Arrhenius Definition
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