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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. An uncharged molecule with a single unpaitred electron in its outer ring - very unstable - exists for only about 10 seconds
Triple point
Lewis definition
Equilibrium
Free radical
2. A structural formula in which electrons are represented by dots; dot pairs or dashes between two atomic symbols represent pairs in covalent bonds.
Octet Rule
Group 2A
Lewis structure
transition elements
3. 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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4. States that it is impossible to determine simultaneously both the position and momentum of an electron or any other particle
Molality
polymer
heisenberg uncertainty principle
Ionic Bond
5. 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
Arrhenius Definition
Group 6A
pH
Dipole Dipole interaction
6. Structure that occurs when it is possible to draw two or more valid electron dot structures that have the same number of electron pairs for a molecule or ion
Activation energy
Molar solubility
Resonance structure
polymer
7. 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.
Balmer series
Period
VSEPR
Redox Half Reaction
8. The amount of energy that reactants must absorb before a chemical reaction will start; also called free energy of activation.
amorphous solid
chemical reaction
Vapor pressure
Activation energy
9. 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.
Water dissociation Constant
Lewis structure
Ion product
Amphoteric
10. Nh/2p The angular momentum changes only in discete amounts with respect to the quantum number. Also E=- R_h/n^2
Effusion
Percent composition
angular momentum in the bohr model
Balmer series
11. Redox reaction - in which the same species is both oxidized and reduced.
Electrolyte
Resonance structure
Halogens
Disproportionation
12. Systematic pairing of a deprotonated species (base) with its protonated form (conjugate acid). Conjugates appear on opposite sides of a chemical equation.
percent composition
Chemical Kinetics
Henderson Hasselbalch Equation
Conjugate acids and Bases
13. The pressure exerted by a vapor in equilibrium with its liquid or solid phase
Formal Charge
angular momentum in the bohr model
Halogens
Vapor pressure
14. Sum of the protons and neutrons in an element often denoted by the letter A
Disproportionation
angular momentum in the bohr model
single displacement reaction
Mass number
15. A representation of a displacement reaction showing only the reactive species and omitting the spectator ions.
Net ionic equation
Ground state
Balmer series
Concentration
16. A base that can accept two moles of H+ per mole of itself (ex: SO4
Percent composition
Diprotic Base
Percent yield
periodic trends
17. 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
Emperical Formula
Molar solubility
Titration
theoretical yield
18. The molar solubility of one salt is reduced when another salt - having a common ion is brought into the same solution
Dipole Dipole interaction
Balmer series
Ion product
Common ion effect
19. 5 different orbitals shaped like clover leaves and max electrons is 10
Network covalent
d orbital
Reaction mechanism
Group 6A
20. Numbers that specify the properties of atomic orbitals and of their electrons
quantum numbers
Intermolecular forces
Hydrogen bonding
Reaction mechanism
21. A horizontal row of elements in the periodic table
Electronegativity
crystalline solid
Period
Solvent
22. 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.
crystalline solid
Group 2A
und's rule
Solubility Product Constant
23. (physics) the smallest discrete quantity of some physical property that a system can possess (according to quantum theory) E=hf
Normality
Titration
quantum
chemical reaction
24. Contains nonmetals that are non - reactive. Full outermost energy level except helium which has 2.
Halogens
indicator
Noble gases
Avagadros number
25. 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
Amphoteric
Raoult's Law
Molality
London forces
26. An emperimentally determined mathmatical expression showing the rate of a reaction as a function of the concentration of its reactants
Noble gases
Rate law
Ionization energy
decomposition reaction
27. 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
Henry's Law
law of constant composition
Water dissociation Constant
Spin quantum number
28. Valence Shell Electron Pair Repulsion theory - stating that the three - dimensional molecular geometry about some central atom is determined by the elctronic repulsion between its bonding and nonbonding electron pairs.
VSEPR
single displacement reaction
Concentration
compound
29. Substance in which a solute is dissolved to form a solution
Solvent
Effusion
Net ionic equation
Titration
30. The weight in grams of one mole of a given elementand is expressedin tems of grams per mole.
energy state
bond energy
Solvent
Atomic weight
31. The point on a phase diagram that represents the only set of conditions at which all three phases exist in equilibrium with one another
Triple point
Acid dissociation constant
Colligative properties
The bohr model
32. The number of atoms in exactly 12 g of pure 12c and equal to 6.022 x 10^23 is called
Avagadros number
Buffer
heisenberg uncertainty principle
atomic theory
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
empirical formula
s orbital
subshell
Hydrogen bonding
34. The formation of one or more covalent bonds between an electron pair donor and an electron pair acceptor
Lewis acid base reaction
bond length
Group 2A
Electronegativity
35. A subdivision of an energy level in an atom. They are divided into orbitals.
Atomic absorption Spectra
quanta
Nucleus
subshell
36. Process by which molecules tend to move from an area where they are more concentrated to an area where they are less concentrated
Dispersion Forces
Diffusion
Equilibrium
lathanide series
37. 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
Disproportionation
Phase diagram
electrolysis
azimuthal quantum number
38. 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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39. A definite stable energy that a physical system can have
energy state
Pauli exclusion principle
molecule
Rate law
40. Having characteristics of both an acid and a base and capable of reacting as either
Vapor pressure
Amphoteric
Aqueous Solution
Octet Rule
41. Simplest whole # ration of atoms in a compound
Emperical Formula
Combination Reaction
Decomposition reaction
Redox Half Reaction
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
azimuthal quantum number
quantum numbers
quantum
sigma bond
43. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance C>>>>A+B
Ionic Bond
representative elements
atomic radius
Decomposition reaction
44. The sum of the exponents in a rate law - where each exponent provides the reaction order with respect to its reactants
polymer
Normality
representative elements
Reaction order
45. 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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46. (chemistry) the sum of the relative atomic masses of the constituent atoms of a molecule
molecular weight
Ion dipole interactions
Half equivalence point
Octet Rule
47. Gram equivalent weight of solute per liter of solution - often denoted by N.
Covalent Bond
Normality
Chemical Kinetics
Titration
48. States that if a stress is applied to a system at equilibrium - the system shifts in the direction that relieves the stress.
representative elements
Electrolyte
Buffer
Le chateliers Principle
49. The reaction of the ions that characterize acids and the ions that characterize bases to form water molecules and a salt
Triple point
Avagadros number
Theoretical yield
Neutralization reaction
50. 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
Solvent
und's rule
Group 7A
heisenberg uncertainty principle