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. An elementary particle with 0 charge and mass about equal to a proton
Effective nuclear charge
Neutron
Colligative properties
Ground state
2. The slowest elementary step which is the limit for the rate of the other steps
Ion product
heisenberg uncertainty principle
Normality
Rate determining step
3. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds
empirical formula
Group 4A
Phase diagram
Dispersion Forces
4. E=hc/?
Atomic weight
electromagnetic energy of photons emmited from electrons at ground state
Proton
Equivalence point
5. A model of acids and bases which an acid is hydrogen ion donor and base is a hydrogen ion acceptor.
quantum numbers
Formal Charge
Group 6A
Bronsted Lowry
6. 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
Atomic absorption Spectra
Nucleus
Percent composition
7. (chemistry) a substance that changes color to indicate the presence of some ion or substance
indicator
Rate law
Solution equilibrium
Planck's Constant
8. The number of atoms in exactly 12 g of pure 12c and equal to 6.022 x 10^23 is called
Pauli exclusion principle
atomic emission spectrum
Avagadros number
Group 3A
9. 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
Dipole Dipole interaction
redox reaction
Group 7A
Diffusion
10. An element in an 'A' group in the periodic table; as a group these elements display a wide range of physical and chemical properties. In their atoms - the s and p sublevels in the highest occupied energy level are partially filled
bond length
representative elements
amorphous solid
electrolysis
11. Gram equivalent weight of solute per liter of solution - often denoted by N.
Normality
Combination Reaction
Ionization energy
Acid dissociation constant
12. Rare earth element group (elements 58-71)
bond energy
Ion
Intermolecular forces
lathanide series
13. 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
Equlibrium constant
London forces
Bronsted - Lowry definition
mole
14. A naturally occurring or synthetic compound consisting of large molecules made up of a linked series of repeated simple monomers
bond length
Phase diagram
polymer
Group 7A
15. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance C>>>>A+B
Decomposition reaction
Dipole Dipole interaction
Rydberg constant
lewis base
16. The weight in grams of one mole of a given elementand is expressedin tems of grams per mole.
Triple point
Henry's Law
Atomic weight
mole
17. The sum of the exponents in a rate law - where each exponent provides the reaction order with respect to its reactants
s orbital
Redox Half Reaction
Reaction order
Proton
18. 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.
amorphous solid
atomic radius
electromagnetic energy of photons emmited from electrons at ground state
Atomic absorption Spectra
19. A reaction in which atoms of one element take the place of atoms of another element in a compound
Net ionic equation
Group 4A
Decomposition reaction
single displacement reaction
20. The molar solubility of one salt is reduced when another salt - having a common ion is brought into the same solution
Triple point
Effective nuclear charge
Common ion effect
theoretical yield
21. One - half the distance between the nuclei of two atoms of the same element when the atoms are joined
Neutralization reaction
Amphoteric
atomic radius
atomic theory
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.
Lyman series
electron affinity
decomposition reaction
Solubility Product Constant
23. 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
Group 1A
Group 3A
Percent yield
s orbital
24. The amount of product that can be made in a chemical reaction based on the amount of limiting reactant
Strong acid
Noble gases
bond energy
Theoretical yield
25. 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
Electronegativity
sigma bond
azimuthal quantum number
Disproportionation
26. 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
Rate determining step
Mass number
chemical reaction
27. (chemistry) a series from actinium to lawrencium of 15 radioactive elements with increasing atomic numbers
Group 3A
Intermolecular forces
actinide series
Octet Rule
28. The percent by mass of each element in a compound
Henry's Law
percent composition
Solute
pi bonds
29. A bond formed when two atomic orbitals combine to form a molecular orbital that is symmetrical around the axis connecting the two atomic nuclei
Diprotic Base
Solution equilibrium
Solubility Product Constant
sigma bond
30. The process by which a gas escapes from one container to another at lower pressure through a tiny hole in the container.
Dipole
Rydberg constant
Effusion
pI
31. At a constant pressure - the volume of an ideal gas is directly proportinal to its temperature: V (a) T
32. A reaction in which two or more substances combine to form a single substance A+B>>>>>>>C
Diffusion
Combination Reaction
molecular weight
Neutron
33. An ionic compound that resists changes in its pH
percent composition
VSEPR
polymer
Buffer
34. Tells you how much solute is present compared to the amount of solvent
Effusion
Free radical
Concentration
Percent yield
35. Nh/2p The angular momentum changes only in discete amounts with respect to the quantum number. Also E=- R_h/n^2
amorphous solid
mole
angular momentum in the bohr model
Phase diagram
36. 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
Nucleus
Reaction order
electromagnetic energy of photons emmited from electrons at ground state
hydrogen bonding
37. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
redox reaction
Principle quantum number
Octet Rule
Buffer
38. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
Rate determining step
Free radical
redox reaction
Lyman series
39. Slightly less reactive than alkali metals - comprise group II
Aqueous Solution
Colligative properties
Alkaline earths
polymer
40. Simplest whole # ration of atoms in a compound
Raoult's Law
Halogens
lathanide series
Emperical Formula
41. Substance in which a solute is dissolved to form a solution
effective nuclear charge
Solvent
Molecular orbital
Resonance structure
42. A definite stable energy that a physical system can have
energy state
electromagnetic energy of photons emmited from electrons at ground state
law of constant composition
Ionic Bond
43. Sol - a chemical process in which solvent molecules and molecules or ions of the solute combine to form a compound
Alkaline earths
hydrogen bonding
quantum numbers
solvation
44. Two or more atoms held together by covalent bonds
electromagnetic energy of photons emmited from electrons at ground state
STP
molecule
Equivalence point
45. A structural formula in which electrons are represented by dots; dot pairs or dashes between two atomic symbols represent pairs in covalent bonds.
Network covalent
Amphoteric
Hydrogen bonding
Lewis structure
46. Process by which molecules tend to move from an area where they are more concentrated to an area where they are less concentrated
polymer
Raoult's Law
Diffusion
Principle quantum number
47. A base that can accept two moles of H+ per mole of itself (ex: SO4
Henry's Law
Diprotic Base
Percent composition
Group 1A
48. Having characteristics of both an acid and a base and capable of reacting as either
Solubility Product Constant
Amphoteric
Decomposition reaction
Principle quantum number
49. Standard Temperature and Pressure. 273 Kelvin (0 Celsius) - 1 atmosphere (760 torr - 760 kPA).
representative elements
STP
Ionization energy
London forces
50. A fundamental constant - h - that relates the energy of light quanta to their frequency: h = 6.6 X 10^-34 joule