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. No two electrons or protons or neutrons in a given system can be in states characterized by the same set of quantum numbers
Pauli exclusion principle
transition elements
atomic radius
Solution equilibrium
2. 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
Azeotrope
Ion product
Lyman series
Electrolyte
3. When dipoles are dissolved in a solution where ions are present ions wil arrange themselves with the opposite charged end of the dipole.
empirical formula
Solution equilibrium
Group 6A
Ion dipole interactions
4. An elementary particle with 0 charge and mass about equal to a proton
Neutron
Percent yield
Graham's Law
Azeotrope
5. (chemistry) a substance formed by chemical union of two or more elements or ingredients in definite proportion by weight
compound
Phase diagram
Redox Half Reaction
quantum
6. States that it is impossible to determine simultaneously both the position and momentum of an electron or any other particle
Formal Charge
Lewis definition
Group 3A
heisenberg uncertainty principle
7. The formation of one or more covalent bonds between an electron pair donor and an electron pair acceptor
Diprotic Base
Lewis acid base reaction
Lewis definition
representative elements
8. Named after their cation and anion
ionic cmpound
Collision theory of chemical Kinetics
Colligative properties
Half equivalence point
9. 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
atomic radius
Half equivalence point
Strong acid
Hydrogen bonding
10. The number of atoms in exactly 12 g of pure 12c and equal to 6.022 x 10^23 is called
Avagadros number
Planck's Constant
Combination Reaction
Rate determining step
11. A concentration unit of a solution expressed as moles of solute dissolved per liter of solution
Chemical Kinetics
Rate determining step
Molarity
solvation
12. 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
s orbital
Triple point
pH
electrolysis
13. Set of spectral lines appearing in the UV region when a hydrogen atom undergoes a transition from energy levels n>1 to n=1.
Magnetic quantum number
Lyman series
Lewis structure
compound
14. 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
Free radical
Disproportionation
atomic emission spectrum
Dispersion Forces
15. Process by which molecules tend to move from an area where they are more concentrated to an area where they are less concentrated
atomic emission spectrum
heisenberg uncertainty principle
Effusion
Diffusion
16. Alkaline Earth Metals - 2 valence electrons +2 ions - Magnesium Mg
Activation energy
Vapor pressure
Group 2A
Net ionic equation
17. States that if a stress is applied to a system at equilibrium - the system shifts in the direction that relieves the stress.
Henry's Law
molecule
Ionic Bond
Le chateliers Principle
18. Nh/2p The angular momentum changes only in discete amounts with respect to the quantum number. Also E=- R_h/n^2
compound
electron affinity
angular momentum in the bohr model
decomposition reaction
19. 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.
ionic cmpound
Solubility Product Constant
Colligative properties
Group 1A
20. Chalcogens - - Oxide O
Diprotic Base
Titration
Group 6A
Henderson Hasselbalch Equation
21. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance
decomposition reaction
theoretical yield
Rydberg constant
lewis base
22. 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.
Equlibrium constant
empirical formula
crystalline solid
Spin quantum number
23. The Percent by mass of each element in a compound.
Molecular orbital
Acid dissociation constant
Combination Reaction
Percent composition
24. Rare earth element group (elements 58-71)
Water dissociation Constant
Vapor pressure
quantum
lathanide series
25. 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
Redox Half Reaction
Nucleus
percent composition
Vapor pressure
26. A subdivision of an energy level in an atom. They are divided into orbitals.
Formal Charge
electron configuration
subshell
empirical formula
27. Sol - a chemical process in which solvent molecules and molecules or ions of the solute combine to form a compound
sigma bond
solvation
gram equivalent weight
Spin quantum number
28. A reaction in which atoms of one element take the place of atoms of another element in a compound
single displacement reaction
Le chateliers Principle
Aqueous Solution
Octet Rule
29. A definite stable energy that a physical system can have
sigma bond
percent composition
Alkaline earths
energy state
30. Side - to side parallel orbitals overlap to share electrons - the 2nd/3rd covalent bond between two atoms - cannot rotate and maintain the bond.
Solution equilibrium
sigma bond
Charles and Gay Lussac's Law
pi bonds
31. Contains nonmetals that are non - reactive. Full outermost energy level except helium which has 2.
Noble gases
Charles and Gay Lussac's Law
solvation
Intermolecular forces
32. An acid that will completely dissociate in aqueous solution - like HCl - HI - HClO4 HBr.
Half equivalence point
VSEPR
Strong acid
Free radical
33. The process of decomposing a chemical compound by the passage of an electric current.
Magnetic quantum number
Disproportionation
Neutralization reaction
electrolysis
34. PH of a molecule at which it contains no net electric charge - isoelectric point.
Disproportionation
Magnetic quantum number
Avagadros number
pI
35. One - half of the distance between the center of identical atoms that are not bonded together. Since effective nuclear charge increases when moving from left to right each additional electron is pulled more strogly toward the nucleus.
atomic radius
Phase diagram
Activation energy
Ionization energy
36. The slowest elementary step which is the limit for the rate of the other steps
Lewis definition
energy state
chemical reaction
Rate determining step
37. 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
Warning
: Invalid argument supplied for foreach() in
/var/www/html/basicversity.com/show_quiz.php
on line
183
38. 2.18 x 10^-18 J/electron
percent composition
The bohr model
angular momentum in the bohr model
Rydberg constant
39. 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
bond energy
Avagadros number
Conjugate acids and Bases
40. E=hc/?
Group 6A
electromagnetic energy of photons emmited from electrons at ground state
theoretical yield
VSEPR
41. The percent by mass of each element in a compound
und's rule
Mass number
percent composition
polymer
42. The ways in which electrons are arranged in various orbitals around the nuclei of atoms
Concentration
solvation
Conjugate acids and Bases
electron configuration
43. The ratio of the number of moles of solute dissolved in one kilogram of solvent. molality (M = moles solute/kg of solution)
Phase diagram
Molality
Water dissociation Constant
quanta
44. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
hydrogen bonding
redox reaction
subshell
Solute
45. The average distance between the nuclei of two bonded atoms
lewis base
periodic trends
atomic emission spectrum
bond length
46. Substance in which a solute is dissolved to form a solution
redox reaction
Water dissociation Constant
Solvent
heisenberg uncertainty principle
47. 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
Rate determining step
Aqueous Solution
Group 4A
48. Common definition of acids as proton (H+) donors and bases as proton acceptors
Bronsted - Lowry definition
molecule
Rate determining step
mole
49. A base that can accept two moles of H+ per mole of itself (ex: SO4
Spin quantum number
Diprotic Base
Bronsted Lowry
physical reaction
50. A horizontal row of elements in the periodic table
ionic cmpound
Period
Electronegativity
Azeotrope