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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. 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
Dispersion Forces
lathanide series
hydrogen bonding
Reaction order
2. A subdivision of an energy level in an atom. They are divided into orbitals.
subshell
lathanide series
Charles and Gay Lussac's Law
Acid dissociation constant
3. An atom or group of atoms that has a positive or negative charge
Ion
physical reaction
Octet Rule
Rate law
4. 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.
Formal Charge
Ion product
Pauli exclusion principle
single displacement reaction
5. Numbers that specify the properties of atomic orbitals and of their electrons
quantum numbers
Theoretical yield
atomic radius
law of constant composition
6. Small discrete increments of energy.
quanta
pi bonds
Rydberg constant
electron affinity
7. The slowest elementary step which is the limit for the rate of the other steps
Avagadros number
transition elements
Rate determining step
effective nuclear charge
8. At a constant pressure - the volume of an ideal gas is directly proportinal to its temperature: V (a) T
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9. The energy required to break a chemical bond and form neutral isolated atoms
bond energy
Lyman series
quanta
Theoretical yield
10. Standard Temperature and Pressure. 273 Kelvin (0 Celsius) - 1 atmosphere (760 torr - 760 kPA).
STP
quantum numbers
empirical formula
Halogens
11. The vapor pressure of solution is the product of the mole fraction of the solvent and the vapor pressure of the pure solvent. P_a=X_aP_total
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12. The reaction of the ions that characterize acids and the ions that characterize bases to form water molecules and a salt
Neutralization reaction
atomic radius
Emperical Formula
Intermolecular forces
13. 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 weight
Neutralization reaction
Spin quantum number
atomic radius
14. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds
lathanide series
Group 4A
effective nuclear charge
Water dissociation Constant
15. The process by which one or more substances change to produce one or more different substances
Hydrogen bonding
Decomposition reaction
sigma bond
chemical reaction
16. 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
Avagadros number
Concentration
Ion
Arrhenius Definition
17. Rare earth element group (elements 58-71)
Activation energy
lathanide series
Net ionic equation
pI
18. When dipoles are dissolved in a solution where ions are present ions wil arrange themselves with the opposite charged end of the dipole.
Ion dipole interactions
Group 4A
pi bonds
Activation energy
19. A graph of pressure versus temperature that shows the conditions under which the phases of a substance exist
Equlibrium constant
bond length
Phase diagram
Molecular orbital
20. Slightly less reactive than alkali metals - comprise group II
Alkaline earths
Ground state
electron configuration
Diprotic Base
21. The molar solubility of one salt is reduced when another salt - having a common ion is brought into the same solution
indicator
STP
Nucleus
Common ion effect
22. An elementary particle with 0 charge and mass about equal to a proton
Neutron
chemical reaction
Half equivalence point
Lyman series
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 4A
Percent yield
Period
Henry's Law
24. The amount of a substance that contains as many particles as there are atoms in exactly 12g of carbon -12
mole
pH
Dipole Dipole interaction
subshell
25. 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
Combination Reaction
Solution equilibrium
Molecular orbital
electron configuration
26. 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
Ionic Bond
Hydrogen bonding
Concentration
Ion
27. Theory stating that the rate of a reaction is directly proportional to the number of collisions that take place between reactants per second.
Balmer series
Collision theory of chemical Kinetics
Net ionic equation
percent composition
28. A horizontal row of elements in the periodic table
Period
Graham's Law
Lyman series
law of constant composition
29. 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.
physical reaction
crystalline solid
Dipole Dipole interaction
Le chateliers Principle
30. 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
Electronegativity
Atomic weight
Water dissociation Constant
Acid dissociation constant
31. Have three valance electrons. In certain instances - some elements will loose three electrons - but they will also share electrons with another element to attain stability.
Dipole
empirical formula
Conjugate acids and Bases
Group 3A
32. 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
sigma bond
Resonance structure
Azeotrope
Octet Rule
33. The formation of one or more covalent bonds between an electron pair donor and an electron pair acceptor
Lewis acid base reaction
Theoretical yield
Diprotic Base
quantum numbers
34. 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
Magnetic quantum number
Rate law
Chemical Kinetics
35. A solution in which water is the solvent
Chemical Kinetics
Hydrogen bonding
Aqueous Solution
Halogens
36. A chemical bond that involves sharing a pair of electrons between atoms in a molecule
Reaction order
Covalent Bond
Theoretical yield
Effective nuclear charge
37. 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
heisenberg uncertainty principle
Mass number
Henry's Law
38. 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-
sigma bond
quantum
amorphous solid
Water dissociation Constant
39. States that it is impossible to determine simultaneously both the position and momentum of an electron or any other particle
heisenberg uncertainty principle
molecular weight
ionic cmpound
Intermolecular forces
40. (chemistry) p(otential of) H(ydrogen)
Colligative properties
Nucleus
pH
Avagadros number
41. The amount of energy that reactants must absorb before a chemical reaction will start; also called free energy of activation.
Azeotrope
Activation energy
The bohr model
Strong acid
42. Large molecular structures - strong covalent bonding - share qualities of IONIC And COVALENT
Concentration
Proton
Network covalent
Vapor pressure
43. The amount of product that can be made in a chemical reaction based on the amount of limiting reactant
Theoretical yield
Buffer
electron affinity
ionic cmpound
44. PH of a molecule at which it contains no net electric charge - isoelectric point.
Redox Half Reaction
mole
single displacement reaction
pI
45. In a solution - the substance that dissolves in the solvent
single displacement reaction
Dipole Dipole interaction
Solute
Dispersion Forces
46. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance C>>>>A+B
pi bonds
Decomposition reaction
Bronsted - Lowry definition
Colligative properties
47. E=hc/?
atomic emission spectrum
Vapor pressure
electromagnetic energy of photons emmited from electrons at ground state
periodic trends
48. A reaction where a compound does Not change its molecular structure.
Vapor pressure
physical reaction
Titration
atomic theory
49. Having characteristics of both an acid and a base and capable of reacting as either
Intermolecular forces
Principle quantum number
Amphoteric
quantum
50. The percent by mass of each element in a compound
percent composition
angular momentum in the bohr model
chemical reaction
amorphous solid