SUBJECTS
|
BROWSE
|
CAREER CENTER
|
POPULAR
|
JOIN
|
LOGIN
Business Skills
|
Soft Skills
|
Basic Literacy
|
Certifications
About
|
Help
|
Privacy
|
Terms
|
Email
Search
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 weight in grams of compound that can be substituted by 1 atom of Hydrogen. GEW = MW / # of acidic Hyrdogens
pH
electron configuration
gram equivalent weight
Percent yield
2. Contains nonmetals that are non - reactive. Full outermost energy level except helium which has 2.
Nonpolar covalent bond
Noble gases
Ion
Ion dipole interactions
3. A definite stable energy that a physical system can have
energy state
quantum numbers
Alkaline earths
Half equivalence point
4. The amount of product that can be made in a chemical reaction based on the amount of limiting reactant
Atomic weight
Theoretical yield
atomic emission spectrum
Ion
5. 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.
Electronegativity
Group 6A
Balmer series
Henderson Hasselbalch Equation
6. The process of decomposing a chemical compound by the passage of an electric current.
Proton
Dipole Dipole interaction
Decomposition reaction
electrolysis
7. 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.
Bronsted Lowry
electron affinity
Atomic absorption Spectra
Group 3A
8. The weight in grams of one mole of a given elementand is expressedin tems of grams per mole.
Henderson Hasselbalch Equation
Lyman series
Atomic weight
actinide series
9. A representation of a displacement reaction showing only the reactive species and omitting the spectator ions.
bond energy
Chemical Kinetics
Net ionic equation
percent composition
10. 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
bond length
Arrhenius Definition
Balmer series
Normality
11. When dipoles are dissolved in a solution where ions are present ions wil arrange themselves with the opposite charged end of the dipole.
sigma bond
Amphoteric
Buffer
Ion dipole interactions
12. 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
Disproportionation
theoretical yield
London forces
Equivalence point
13. An atom or group of atoms that has a positive or negative charge
Bronsted - Lowry definition
Triple point
Ion
theoretical yield
14. Substance in which a solute is dissolved to form a solution
Atomic weight
Arrhenius Definition
Solvent
Water dissociation Constant
15. The pressure exerted by a vapor in equilibrium with its liquid or solid phase
Vapor pressure
Neutralization reaction
Lewis acid base reaction
Spin quantum number
16. Energy released when an atom or ion in the gaseous state gains an electron. Increases from left to right and from bottom to top on the Periodic Table.
Redox Half Reaction
physical reaction
electron affinity
Reaction mechanism
17. Alkaline Earth Metals - 2 valence electrons +2 ions - Magnesium Mg
Azeotrope
Group 2A
transition elements
Balmer series
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.
compound
Formal Charge
Solvent
crystalline solid
19. 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.
Percent composition
Activation energy
lathanide series
VSEPR
20. Elements in the middle of the periodic table - in groups 3-12.
Concentration
transition elements
Percent composition
und's rule
21. 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
Planck's Constant
Dispersion Forces
Azeotrope
Ionization energy
22. The amount of a substance that contains as many particles as there are atoms in exactly 12g of carbon -12
single displacement reaction
mole
Amphoteric
Diffusion
23. An uncharged molecule with a single unpaitred electron in its outer ring - very unstable - exists for only about 10 seconds
sigma bond
periodic trends
Free radical
Azeotrope
24. 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
Lewis definition
quantum
electron affinity
25. PH of a molecule at which it contains no net electric charge - isoelectric point.
pI
lathanide series
Theoretical yield
Period
26. At a constant pressure - the volume of an ideal gas is directly proportinal to its temperature: V (a) T
27. A dynamic condition in which two opposing changes occur at equal rates in a closed system
empirical formula
ionic cmpound
Henry's Law
Equilibrium
28. (chemistry) the sum of the relative atomic masses of the constituent atoms of a molecule
gram equivalent weight
Avagadros number
molecular weight
decomposition reaction
29. Theory stating that the rate of a reaction is directly proportional to the number of collisions that take place between reactants per second.
pI
Electrolyte
Electronegativity
Collision theory of chemical Kinetics
30. 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
Nonpolar covalent bond
Free radical
Halogens
31. Standard Temperature and Pressure. 273 Kelvin (0 Celsius) - 1 atmosphere (760 torr - 760 kPA).
STP
und's rule
energy state
electron configuration
32. Numbers that specify the properties of atomic orbitals and of their electrons
Redox Half Reaction
empirical formula
Ion
quantum numbers
33. 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
quanta
Combination Reaction
Disproportionation
34. Having characteristics of both an acid and a base and capable of reacting as either
Pauli exclusion principle
Group 1A
Amphoteric
atomic emission spectrum
35. An ionic compound that resists changes in its pH
Buffer
Lewis acid base reaction
d orbital
Ion
36. A structural formula in which electrons are represented by dots; dot pairs or dashes between two atomic symbols represent pairs in covalent bonds.
Ion dipole interactions
representative elements
Activation energy
Lewis structure
37. A reaction in which atoms of one element take the place of atoms of another element in a compound
lewis base
percent composition
single displacement reaction
atomic radius
38. The area of chemistry that is concerned with reaction rates and reaction mechanisms
Lewis structure
pi bonds
Chemical Kinetics
Acid dissociation constant
39. A subdivision of an energy level in an atom. They are divided into orbitals.
Solution equilibrium
sigma bond
subshell
Reaction mechanism
40. Named after their cation and anion
Alkaline earths
ionic cmpound
Azeotrope
Disproportionation
41. 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.
Acid dissociation constant
Bronsted Lowry
Redox Half Reaction
Ion
42. 5 valence electrons -3 ions - Nitride N
quantum numbers
Group 5A
Period
subshell
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
Dipole
VSEPR
Triple point
Ion
44. The process by which a gas escapes from one container to another at lower pressure through a tiny hole in the container.
Atomic absorption Spectra
electrolysis
Effusion
und's rule
45. (physics) the smallest discrete quantity of some physical property that a system can possess (according to quantum theory) E=hf
Ion product
quantum
Combination Reaction
Amphoteric
46. Simplest whole # ration of atoms in a compound
Emperical Formula
periodic trends
Group 7A
Group 6A
47. 2.18 x 10^-18 J/electron
redox reaction
effective nuclear charge
Rydberg constant
Ionization energy
48. A model of acids and bases which an acid is hydrogen ion donor and base is a hydrogen ion acceptor.
electron affinity
Arrhenius Definition
Bronsted Lowry
Dipole Dipole interaction
49. 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
Arrhenius Definition
Lewis definition
Group 7A
50. Rare earth element group (elements 58-71)
Normality
lathanide series
Rate determining step
Solubility Product Constant