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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. 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
Group 7A
theoretical yield
Redox Half Reaction
Graham's Law
2. The maximum amount of product that can be produced from a given amount of reactant
Ionic Bond
angular momentum in the bohr model
theoretical yield
Percent yield
3. Side - to side parallel orbitals overlap to share electrons - the 2nd/3rd covalent bond between two atoms - cannot rotate and maintain the bond.
Nucleus
Balmer series
Network covalent
pi bonds
4. Charge assigned to an atom in a molecule or polyatmic ion - calculated by (# valence electrons) - (# 1/2 bonding electrons) - (# nonbonding electrons). Molecules containing atoms with lower formal charges tend to be more stable than those with higher
Charles and Gay Lussac's Law
Diffusion
Bronsted Lowry
Formal Charge
5. An atom or group of atoms that has a positive or negative charge
Effective nuclear charge
Avagadros number
Group 3A
Ion
6. A chemical bond in which one atom loses an electron to form a positive ion and the other atom gains to electron to form a negative ion
Equivalence point
Ionic Bond
The bohr model
Hydrogen bonding
7. The area of chemistry that is concerned with reaction rates and reaction mechanisms
Henderson Hasselbalch Equation
Lewis structure
Concentration
Chemical Kinetics
8. The molar amount of a solute that can dissolve in 1L of solvent until equilibrium - saturation - is reached
azimuthal quantum number
Molar solubility
Group 7A
periodic trends
9. 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.
Vapor pressure
law of constant composition
Atomic absorption Spectra
Magnetic quantum number
10. A reaction in which two or more substances combine to form a single substance A+B>>>>>>>C
Normality
STP
Molecular orbital
Combination Reaction
11. 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
mole
energy state
azimuthal quantum number
representative elements
12. The weight in grams of one mole of a given elementand is expressedin tems of grams per mole.
Atomic weight
Arrhenius Definition
bond energy
Diffusion
13. Slightly less reactive than alkali metals - comprise group II
Alkaline earths
Bronsted - Lowry definition
Molecular orbital
heisenberg uncertainty principle
14. A solution in which water is the solvent
Titration
Electronegativity
Aqueous Solution
Group 7A
15. 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
theoretical yield
Free radical
Redox Half Reaction
16. (chemistry) a substance that changes color to indicate the presence of some ion or substance
Amphoteric
quantum numbers
Diprotic Base
indicator
17. Play- by- play showing the individual steps of a reaction - including the formation and destruction of any reaction intermediates that may occur.
theoretical yield
Reaction mechanism
Period
energy state
18. When a solute is dissolved in a solvent - it will dissociate until reaching an equilibrium point at which the rate of dissociation equals the rate of precipitation of the solute - regardless of any additional solute introduced into the mixture
Solution equilibrium
STP
Principle quantum number
Spin quantum number
19. 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.
sigma bond
atomic radius
London forces
Reaction mechanism
20. 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
Alkaline earths
Resonance structure
Pauli exclusion principle
Spin quantum number
21. E=hc/?
Equlibrium constant
electromagnetic energy of photons emmited from electrons at ground state
Decomposition reaction
Lewis structure
22. A naturally occurring or synthetic compound consisting of large molecules made up of a linked series of repeated simple monomers
Rydberg constant
polymer
Nucleus
Effective nuclear charge
23. A graph of pressure versus temperature that shows the conditions under which the phases of a substance exist
Lyman series
Group 4A
Phase diagram
Octet Rule
24. 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
Formula weight
Collision theory of chemical Kinetics
Redox Half Reaction
London forces
25. The process by which one or more substances change to produce one or more different substances
Buffer
Nucleus
chemical reaction
Reaction order
26. 2.18 x 10^-18 J/electron
Covalent Bond
Rydberg constant
Ion dipole interactions
ionic cmpound
27. The molar solubility of one salt is reduced when another salt - having a common ion is brought into the same solution
Common ion effect
Collision theory of chemical Kinetics
Buffer
Net ionic equation
28. The ways in which electrons are arranged in various orbitals around the nuclei of atoms
Ion
electron configuration
percent composition
Atomic weight
29. An ionic compound that resists changes in its pH
Raoult's Law
atomic theory
Normality
Buffer
30. A reaction in which atoms of one element take the place of atoms of another element in a compound
single displacement reaction
Nucleus
Dipole
Hydrogen bonding
31. The weight in grams of compound that can be substituted by 1 atom of Hydrogen. GEW = MW / # of acidic Hyrdogens
Ion dipole interactions
gram equivalent weight
Molar solubility
Group 4A
32. 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
Equlibrium constant
Molar solubility
Equilibrium
33. The amount of a substance that contains as many particles as there are atoms in exactly 12g of carbon -12
STP
mole
Atomic weight
solvation
34. A substance that - when dissolved in water - results in a solution that can conduct electricity
Ion
Electrolyte
Concentration
Effusion
35. 1913 - Niels Bohr - said that electrons formed specific layers instead or random ones - said atoms atoms absorb and give off energy when the electrons move from one shell to another
Lewis definition
The bohr model
percent composition
Equlibrium constant
36. A subdivision of an energy level in an atom. They are divided into orbitals.
Le chateliers Principle
Solute
subshell
Acid dissociation constant
37. Expression of auto - ionization of water into H+ and OH- at a certain temperature - given by the product of the ions' molar concentrations. Denoted by Kw and equal to 10-
Group 5A
bond energy
Reaction order
Water dissociation Constant
38. An emperimentally determined mathmatical expression showing the rate of a reaction as a function of the concentration of its reactants
Rate law
single displacement reaction
Group 3A
Equilibrium
39. Set of spectral lines appearing in the UV region when a hydrogen atom undergoes a transition from energy levels n>1 to n=1.
Lyman series
physical reaction
sigma bond
Le chateliers Principle
40. When dipoles are dissolved in a solution where ions are present ions wil arrange themselves with the opposite charged end of the dipole.
solvation
Ion dipole interactions
atomic theory
Effective nuclear charge
41. The nuclear charge experienced by the outermost electrons of an atom (actual charge minus the shielding caused by inner shells: Z- eff)
effective nuclear charge
Diffusion
Halogens
Lewis definition
42. An atom - ion - or molecule that donates an electron pair to form a covalent bond.
Redox Half Reaction
Dispersion Forces
quantum
lewis base
43. 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
Acid dissociation constant
Group 5A
Decomposition reaction
Formal Charge
44. Named after their cation and anion
Atomic absorption Spectra
ionic cmpound
Mass number
Normality
45. PH of a molecule at which it contains no net electric charge - isoelectric point.
lathanide series
pI
Emperical Formula
Reaction mechanism
46. The reaction of the ions that characterize acids and the ions that characterize bases to form water molecules and a salt
Solubility Product Constant
Neutralization reaction
single displacement reaction
hydrogen bonding
47. A chemical formula showing the ratio of elements in a compound rather than the total number of atoms
Free radical
empirical formula
azimuthal quantum number
electron affinity
48. At a constant pressure - the volume of an ideal gas is directly proportinal to its temperature: V (a) T
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49. The process by which a gas escapes from one container to another at lower pressure through a tiny hole in the container.
Mass number
Aqueous Solution
Effusion
Pauli exclusion principle
50. (chemistry) any theory in which all matter is composed of tiny discrete finite indivisible indestructible particles
Electronegativity
electron configuration
atomic theory
pI