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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. 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
single displacement reaction
Emperical Formula
Acid dissociation constant
Diprotic Base
2. One - half the distance between the nuclei of two atoms of the same element when the atoms are joined
Graham's Law
atomic radius
Ion
actinide series
3. Chalcogens - - Oxide O
Combination Reaction
Group 6A
Colligative properties
electromagnetic energy of photons emmited from electrons at ground state
4. Having characteristics of both an acid and a base and capable of reacting as either
Azeotrope
lathanide series
Amphoteric
Activation energy
5. Tells you how much solute is present compared to the amount of solvent
Concentration
law of constant composition
gram equivalent weight
Magnetic quantum number
6. 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
azimuthal quantum number
Network covalent
Group 1A
Concentration
7. Standard Temperature and Pressure. 273 Kelvin (0 Celsius) - 1 atmosphere (760 torr - 760 kPA).
STP
ionic cmpound
Group 4A
Group 2A
8. Property of the elements that can be predicted from the arrangement of the periodic table
Mass number
periodic trends
Covalent Bond
Group 6A
9. The process of decomposing a chemical compound by the passage of an electric current.
electrolysis
Molecular orbital
Rydberg constant
Balmer series
10. A dynamic condition in which two opposing changes occur at equal rates in a closed system
Ground state
Solute
Equilibrium
pi bonds
11. Atoms react by gaining or losing electrons so as to acquire the stable electron structure of a noble gas - usually eight valence electrons
electron configuration
lathanide series
Graham's Law
Octet Rule
12. States that it is impossible to determine simultaneously both the position and momentum of an electron or any other particle
Common ion effect
heisenberg uncertainty principle
lewis base
redox reaction
13. Structure that occurs when it is possible to draw two or more valid electron dot structures that have the same number of electron pairs for a molecule or ion
Group 7A
physical reaction
Solubility Product Constant
Resonance structure
14. When dipoles are dissolved in a solution where ions are present ions wil arrange themselves with the opposite charged end of the dipole.
effective nuclear charge
Ion dipole interactions
theoretical yield
Chemical Kinetics
15. Side - to side parallel orbitals overlap to share electrons - the 2nd/3rd covalent bond between two atoms - cannot rotate and maintain the bond.
redox reaction
Group 4A
Halogens
pi bonds
16. The molar solubility of one salt is reduced when another salt - having a common ion is brought into the same solution
pH
molecular weight
Electronegativity
Common ion effect
17. The ways in which electrons are arranged in various orbitals around the nuclei of atoms
Electronegativity
electron configuration
Ionization energy
Ion
18. A measured amount of a solution of unknown concentration is added to a known volume of a second solution until the reaction between them is just complete
Titration
d orbital
Group 2A
Period
19. A naturally occurring or synthetic compound consisting of large molecules made up of a linked series of repeated simple monomers
polymer
Le chateliers Principle
Free radical
Triple point
20. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance
Electronegativity
decomposition reaction
bond length
quantum numbers
21. The nuclear charge experienced by the outermost electrons of an atom (actual charge minus the shielding caused by inner shells: Z- eff)
Electrolyte
Percent composition
atomic radius
effective nuclear charge
22. The average distance between the nuclei of two bonded atoms
bond length
Reaction mechanism
gram equivalent weight
STP
23. At a constant pressure - the volume of an ideal gas is directly proportinal to its temperature: V (a) T
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24. A graph of pressure versus temperature that shows the conditions under which the phases of a substance exist
Phase diagram
Collision theory of chemical Kinetics
Formal Charge
Group 3A
25. Theory stating that the rate of a reaction is directly proportional to the number of collisions that take place between reactants per second.
Collision theory of chemical Kinetics
ionic cmpound
Formal Charge
empirical formula
26. (physics) the smallest discrete quantity of some physical property that a system can possess (according to quantum theory) E=hf
sigma bond
quantum
Octet Rule
Solvent
27. 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
quantum numbers
theoretical yield
Nucleus
Henry's Law
28. 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
Graham's Law
Proton
The bohr model
Ionic Bond
29. 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.
Solubility Product Constant
quantum numbers
Pauli exclusion principle
heisenberg uncertainty principle
30. The maximum amount of product that can be produced from a given amount of reactant
theoretical yield
Period
atomic emission spectrum
heisenberg uncertainty principle
31. When polar molecules orient themselves such that the positive region of one molecule is close to the negative region of another molecule.
Neutralization reaction
bond energy
Dipole Dipole interaction
Colligative properties
32. PH of a molecule at which it contains no net electric charge - isoelectric point.
Charles and Gay Lussac's Law
Half equivalence point
Percent composition
pI
33. 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
lewis base
Spin quantum number
actinide series
London forces
34. Alkaline Earth Metals - 2 valence electrons +2 ions - Magnesium Mg
VSEPR
Molar solubility
Group 2A
Free radical
35. (chemistry) any theory in which all matter is composed of tiny discrete finite indivisible indestructible particles
Henderson Hasselbalch Equation
atomic theory
actinide series
Azeotrope
36. A substance that - when dissolved in water - results in a solution that can conduct electricity
theoretical yield
Electrolyte
d orbital
Bronsted - Lowry definition
37. 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
crystalline solid
Solution equilibrium
Diprotic Base
percent composition
38. Numbers that specify the properties of atomic orbitals and of their electrons
Phase diagram
Neutralization reaction
Ion
quantum numbers
39. The point on a phase diagram that represents the only set of conditions at which all three phases exist in equilibrium with one another
Percent yield
atomic radius
Triple point
Noble gases
40. A reaction where a compound does Not change its molecular structure.
Free radical
hydrogen bonding
physical reaction
Lewis definition
41. A concentration unit of a solution expressed as moles of solute dissolved per liter of solution
Graham's Law
Molarity
transition elements
d orbital
42. A horizontal row of elements in the periodic table
Hydrogen bonding
Period
Mass number
Alkaline earths
43. A structural formula in which electrons are represented by dots; dot pairs or dashes between two atomic symbols represent pairs in covalent bonds.
Ion
Ionization energy
Strong acid
Lewis structure
44. The energy required to break a chemical bond and form neutral isolated atoms
Lewis structure
Raoult's Law
bond energy
atomic radius
45. Process by which molecules tend to move from an area where they are more concentrated to an area where they are less concentrated
Diffusion
Group 2A
Principle quantum number
mole
46. Region in a molecule where atomic orbitals overlap - resulting in either a stable low - energy bonding orbital or an unstable high - energy antibonding orbital.
molecule
Molarity
Molecular orbital
Nonpolar covalent bond
47. The ratio of the number of moles of solute dissolved in one kilogram of solvent. molality (M = moles solute/kg of solution)
energy state
Molality
Percent composition
Henry's Law
48. Elements in the middle of the periodic table - in groups 3-12.
transition elements
Resonance structure
Molality
pH
49. The amount of a substance that contains as many particles as there are atoms in exactly 12g of carbon -12
Group 6A
Arrhenius Definition
mole
Solvent
50. A reaction in which two or more substances combine to form a single substance A+B>>>>>>>C
Rate determining step
heisenberg uncertainty principle
Combination Reaction
Nonpolar covalent bond