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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 amount of energy that reactants must absorb before a chemical reaction will start; also called free energy of activation.
Activation energy
Solution equilibrium
theoretical yield
Water dissociation Constant
2. Sum of the protons and neutrons in an element often denoted by the letter A
Lewis acid base reaction
Vapor pressure
Mass number
sigma bond
3. A horizontal row of elements in the periodic table
Nucleus
Group 1A
Proton
Period
4. 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.
Ion
angular momentum in the bohr model
Triple point
Henderson Hasselbalch Equation
5. Property of the elements that can be predicted from the arrangement of the periodic table
molecule
Titration
periodic trends
sigma bond
6. No two electrons or protons or neutrons in a given system can be in states characterized by the same set of quantum numbers
Chemical Kinetics
Ionization energy
Pauli exclusion principle
Atomic absorption Spectra
7. A dynamic condition in which two opposing changes occur at equal rates in a closed system
Ion product
Magnetic quantum number
Half equivalence point
Equilibrium
8. (chemistry) the sum of the relative atomic masses of the constituent atoms of a molecule
molecule
Electronegativity
molecular weight
Network covalent
9. Slightly less reactive than alkali metals - comprise group II
Bronsted - Lowry definition
Concentration
Alkaline earths
Solvent
10. The Percent by mass of each element in a compound.
Noble gases
Ion product
periodic trends
Percent composition
11. The slowest elementary step which is the limit for the rate of the other steps
Dispersion Forces
Rate determining step
Group 7A
physical reaction
12. A structural formula in which electrons are represented by dots; dot pairs or dashes between two atomic symbols represent pairs in covalent bonds.
Strong acid
Lewis structure
atomic theory
Charles and Gay Lussac's Law
13. A reaction in which two or more substances combine to form a single substance A+B>>>>>>>C
Combination Reaction
percent composition
s orbital
Period
14. States that if a stress is applied to a system at equilibrium - the system shifts in the direction that relieves the stress.
Le chateliers Principle
energy state
lathanide series
Octet Rule
15. Nh/2p The angular momentum changes only in discete amounts with respect to the quantum number. Also E=- R_h/n^2
angular momentum in the bohr model
Formula weight
Solubility Product Constant
hydrogen bonding
16. The pressure exerted by a vapor in equilibrium with its liquid or solid phase
Vapor pressure
Neutron
Net ionic equation
Theoretical yield
17. Large molecular structures - strong covalent bonding - share qualities of IONIC And COVALENT
Common ion effect
Raoult's Law
Aqueous Solution
Network covalent
18. Solids in which the particles are arranged in a repeating - 3- D pattern - has a specific melting point - classified as ionic network covalent - metallic or molecular.
crystalline solid
Group 2A
Molality
Disproportionation
19. An emperimentally determined mathmatical expression showing the rate of a reaction as a function of the concentration of its reactants
representative elements
Avagadros number
Rate law
Molar solubility
20. The ratio of the number of moles of solute dissolved in one kilogram of solvent. molality (M = moles solute/kg of solution)
ionic cmpound
pI
Molality
Bronsted - Lowry definition
21. 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.
Buffer
amorphous solid
redox reaction
Redox Half Reaction
22. The formation of one or more covalent bonds between an electron pair donor and an electron pair acceptor
Octet Rule
Titration
Atomic weight
Lewis acid base reaction
23. Substance in which a solute is dissolved to form a solution
Water dissociation Constant
Diffusion
Solvent
Chemical Kinetics
24. (physics) the smallest discrete quantity of some physical property that a system can possess (according to quantum theory) E=hf
Noble gases
quantum numbers
quantum
Bronsted Lowry
25. The percent by mass of each element in a compound
percent composition
Molar solubility
Buffer
Le chateliers Principle
26. A pair of equal and opposite electric charges or magnetic poles separated by a small distance
Decomposition reaction
und's rule
Dipole
Magnetic quantum number
27. Elements in the middle of the periodic table - in groups 3-12.
transition elements
representative elements
Principle quantum number
Arrhenius Definition
28. One - half the distance between the nuclei of two atoms of the same element when the atoms are joined
Proton
Atomic weight
Concentration
atomic radius
29. The energy required to remove an electron from a gaseous atom; generally increases in moving from left - to - right across a period and decreases in moving down a group
Ion product
amorphous solid
Ionization energy
Neutralization reaction
30. 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
bond energy
Half equivalence point
Rate law
decomposition reaction
31. Contains nonmetals that are non - reactive. Full outermost energy level except helium which has 2.
chemical reaction
Charles and Gay Lussac's Law
Half equivalence point
Noble gases
32. An elementary particle with 0 charge and mass about equal to a proton
Phase diagram
Theoretical yield
Net ionic equation
Neutron
33. The process by which a gas escapes from one container to another at lower pressure through a tiny hole in the container.
sigma bond
Effusion
heisenberg uncertainty principle
d orbital
34. A naturally occurring or synthetic compound consisting of large molecules made up of a linked series of repeated simple monomers
redox reaction
Electrolyte
Concentration
polymer
35. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds
Planck's Constant
Emperical Formula
Group 4A
d orbital
36. 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
Half equivalence point
Strong acid
Lewis acid base reaction
Acid dissociation constant
37. A base that can accept two moles of H+ per mole of itself (ex: SO4
Diprotic Base
Acid dissociation constant
Henderson Hasselbalch Equation
solvation
38. A model of acids and bases which an acid is hydrogen ion donor and base is a hydrogen ion acceptor.
Bronsted Lowry
Reaction mechanism
Network covalent
redox reaction
39. A substance that - when dissolved in water - results in a solution that can conduct electricity
gram equivalent weight
Molarity
single displacement reaction
Electrolyte
40. The reaction of the ions that characterize acids and the ions that characterize bases to form water molecules and a salt
Emperical Formula
crystalline solid
Neutralization reaction
quantum numbers
41. 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.
Ion product
ionic cmpound
Lewis structure
Charles and Gay Lussac's Law
42. 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
azimuthal quantum number
mole
Electronegativity
hydrogen bonding
43. 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
Percent composition
Formal Charge
Group 5A
Azeotrope
44. At a constant pressure - the volume of an ideal gas is directly proportinal to its temperature: V (a) T
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45. 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
Electrolyte
Colligative properties
Group 3A
molecule
46. Theory stating that the rate of a reaction is directly proportional to the number of collisions that take place between reactants per second.
subshell
Collision theory of chemical Kinetics
Atomic absorption Spectra
Lewis definition
47. Process by which molecules tend to move from an area where they are more concentrated to an area where they are less concentrated
Acid dissociation constant
Charles and Gay Lussac's Law
Diffusion
Nonpolar covalent bond
48. The molar solubility of one salt is reduced when another salt - having a common ion is brought into the same solution
Acid dissociation constant
Triple point
Atomic absorption Spectra
Common ion effect
49. A covalent bond in which the bonding electrons are shared equally by the bonded atoms - resulting in a balanced distribution of electrical charge
Reaction order
Raoult's Law
Nonpolar covalent bond
Rydberg constant
50. Small discrete increments of energy.
quanta
Group 2A
Buffer
Water dissociation Constant