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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 area of chemistry that is concerned with reaction rates and reaction mechanisms
Chemical Kinetics
STP
Rate law
polymer
2. 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
Aqueous Solution
pH
Ion dipole interactions
Ionic Bond
3. A solid made up of particles that are not arranged in a regular pattern.
lathanide series
amorphous solid
Balmer series
Ground state
4. 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
The bohr model
heisenberg uncertainty principle
bond energy
Decomposition reaction
5. Process by which molecules tend to move from an area where they are more concentrated to an area where they are less concentrated
Titration
Diffusion
electromagnetic energy of photons emmited from electrons at ground state
Octet Rule
6. The maximum amount of product that can be produced from a given amount of reactant
Vapor pressure
molecule
theoretical yield
Group 3A
7. Alkaline Earth Metals - 2 valence electrons +2 ions - Magnesium Mg
Ground state
Colligative properties
Group 2A
molecular weight
8. An atom or group of atoms that has a positive or negative charge
Strong acid
Ion
d orbital
actinide series
9. Small discrete increments of energy.
Raoult's Law
Free radical
compound
quanta
10. The process by which a gas escapes from one container to another at lower pressure through a tiny hole in the container.
percent composition
Concentration
Effusion
Lewis structure
11. 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
transition elements
redox reaction
und's rule
Group 7A
12. Large molecular structures - strong covalent bonding - share qualities of IONIC And COVALENT
Raoult's Law
Network covalent
Hydrogen bonding
redox reaction
13. A physical property of a solution that depends on the number - but not the identity - of the disswolved solute particles; example properties include vapor pressure lowering - boiling point elevation - osmotic pressure - and frezzing point depression
d orbital
Group 4A
Colligative properties
Magnetic quantum number
14. A graph of pressure versus temperature that shows the conditions under which the phases of a substance exist
Formal Charge
Phase diagram
Solubility Product Constant
STP
15. A substance that - when dissolved in water - results in a solution that can conduct electricity
molecule
Electrolyte
Solubility Product Constant
Group 1A
16. 2.18 x 10^-18 J/electron
Bronsted Lowry
Rydberg constant
Electronegativity
Molarity
17. 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.
molecular weight
molecule
Arrhenius Definition
Solubility Product Constant
18. 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
Solute
Azeotrope
Electrolyte
Electronegativity
19. 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
Molar solubility
solvation
azimuthal quantum number
hydrogen bonding
20. 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
Arrhenius Definition
ionic cmpound
s orbital
Solution equilibrium
21. Named after their cation and anion
ionic cmpound
Theoretical yield
Vapor pressure
Resonance structure
22. The average distance between the nuclei of two bonded atoms
atomic radius
bond length
Free radical
atomic emission spectrum
23. Standard Temperature and Pressure. 273 Kelvin (0 Celsius) - 1 atmosphere (760 torr - 760 kPA).
Redox Half Reaction
polymer
Percent yield
STP
24. 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 3A
Nonpolar covalent bond
Water dissociation Constant
bond energy
25. Acids defined as electron - pair acceptors and bases as electron - pair donors.
Lewis definition
lathanide series
decomposition reaction
Theoretical yield
26. Property of the elements that can be predicted from the arrangement of the periodic table
Molarity
periodic trends
Planck's Constant
Atomic weight
27. The ways in which electrons are arranged in various orbitals around the nuclei of atoms
electron configuration
physical reaction
Equilibrium
Effective nuclear charge
28. A fundamental constant - h - that relates the energy of light quanta to their frequency: h = 6.6 X 10^-34 joule
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29. A covalent bond in which the bonding electrons are shared equally by the bonded atoms - resulting in a balanced distribution of electrical charge
Solubility Product Constant
Nonpolar covalent bond
pi bonds
mole
30. An ionic compound that resists changes in its pH
Buffer
Network covalent
pH
Henderson Hasselbalch Equation
31. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds
Chemical Kinetics
VSEPR
Collision theory of chemical Kinetics
Group 4A
32. 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
Phase diagram
Acid dissociation constant
Chemical Kinetics
Percent yield
33. Systematic pairing of a deprotonated species (base) with its protonated form (conjugate acid). Conjugates appear on opposite sides of a chemical equation.
single displacement reaction
Conjugate acids and Bases
Redox Half Reaction
Raoult's Law
34. An atom - radical - or molecule that has gained or lost one or more electrons and has a negative or positive charge
Ion
Vapor pressure
actinide series
Lewis definition
35. 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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36. PH=pka+log[base/acid] Used in titration based problems that relates the pH or pOH of a solution to the pK and the ratio of the dissociated species.
Henderson Hasselbalch Equation
Planck's Constant
crystalline solid
heisenberg uncertainty principle
37. A reaction where a compound does Not change its molecular structure.
Period
electrolysis
Normality
physical reaction
38. One - half the distance between the nuclei of two atoms of the same element when the atoms are joined
atomic radius
Percent composition
Planck's Constant
Principle quantum number
39. The amount of energy that reactants must absorb before a chemical reaction will start; also called free energy of activation.
Neutron
Bronsted Lowry
Activation energy
Equlibrium constant
40. (physics) the smallest discrete quantity of some physical property that a system can possess (according to quantum theory) E=hf
Ion
Net ionic equation
azimuthal quantum number
quantum
41. The molar amount of a solute that can dissolve in 1L of solvent until equilibrium - saturation - is reached
Molar solubility
Resonance structure
und's rule
Buffer
42. 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
periodic trends
Solvent
Titration
representative elements
43. Theory stating that the rate of a reaction is directly proportional to the number of collisions that take place between reactants per second.
molecular weight
Collision theory of chemical Kinetics
Emperical Formula
Titration
44. Atoms react by gaining or losing electrons so as to acquire the stable electron structure of a noble gas - usually eight valence electrons
Le chateliers Principle
electrolysis
Octet Rule
The bohr model
45. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance
decomposition reaction
Solution equilibrium
sigma bond
Normality
46. The quantum number that indicates the main energy level occupied by the electron. Can theoretically take on any positive interger. Denoted by the letter n.
Intermolecular forces
Principle quantum number
electron configuration
atomic radius
47. Contains nonmetals that are non - reactive. Full outermost energy level except helium which has 2.
azimuthal quantum number
redox reaction
Molar solubility
Noble gases
48. (chemistry) any theory in which all matter is composed of tiny discrete finite indivisible indestructible particles
atomic theory
energy state
Theoretical yield
Half equivalence point
49. A reaction in which two or more substances combine to form a single substance A+B>>>>>>>C
polymer
Combination Reaction
quantum
Lewis definition
50. (chemistry) a substance formed by chemical union of two or more elements or ingredients in definite proportion by weight
compound
redox reaction
Neutron
Electronegativity