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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. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
Effusion
law of constant composition
redox reaction
Bronsted - Lowry definition
2. Specifies the specific orbital in which the electron is most likely to be found. - Third quantum number - designated as ml. Describes a particular orbital within a subshell where an electron is very likely to be found. Possible values are integers in
polymer
angular momentum in the bohr model
d orbital
Magnetic quantum number
3. An atom or group of atoms that has a positive or negative charge
d orbital
sigma bond
Ion
Redox Half Reaction
4. The area of chemistry that is concerned with reaction rates and reaction mechanisms
percent composition
Group 5A
Chemical Kinetics
Lewis structure
5. An emperimentally determined mathmatical expression showing the rate of a reaction as a function of the concentration of its reactants
Rate law
Concentration
Avagadros number
quantum numbers
6. The amount of product that can be made in a chemical reaction based on the amount of limiting reactant
atomic radius
Theoretical yield
Ground state
quanta
7. The lowest allowable energy state of an atom
Octet Rule
Ground state
Dipole
Rydberg constant
8. 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
Theoretical yield
pI
Azeotrope
Arrhenius Definition
9. The Percent by mass of each element in a compound.
Percent composition
STP
subshell
Diffusion
10. A structural formula in which electrons are represented by dots; dot pairs or dashes between two atomic symbols represent pairs in covalent bonds.
VSEPR
The bohr model
Lewis structure
bond length
11. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds
Group 4A
atomic theory
Network covalent
Ion dipole interactions
12. A subatomic particle that has a positive charge and that is found in the nucleus of an atom Charge of +1 and mass of 1.0073 amu
Nonpolar covalent bond
periodic trends
Proton
Solution equilibrium
13. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance C>>>>A+B
d orbital
Decomposition reaction
electromagnetic energy of photons emmited from electrons at ground state
Theoretical yield
14. A reaction in which two or more substances combine to form a single substance A+B>>>>>>>C
und's rule
Combination Reaction
Noble gases
Rydberg constant
15. An atom - ion - or molecule that donates an electron pair to form a covalent bond.
Reaction mechanism
lewis base
Colligative properties
heisenberg uncertainty principle
16. An elementary particle with 0 charge and mass about equal to a proton
Half equivalence point
Neutron
Alkaline earths
actinide series
17. Temperature is constant; effusion and temperature are proportional to the square root of their masses
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18. The process by which a gas escapes from one container to another at lower pressure through a tiny hole in the container.
chemical reaction
empirical formula
Effusion
gram equivalent weight
19. A reaction in which atoms of one element take the place of atoms of another element in a compound
Vapor pressure
quanta
single displacement reaction
Normality
20. At a constant pressure - the volume of an ideal gas is directly proportinal to its temperature: V (a) T
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21. The energy required to remove an electron from a gaseous atom; generally increases in moving from left - to - right across a period and decreases in moving down a group
Redox Half Reaction
Mass number
Emperical Formula
Ionization energy
22. Tells you how much solute is present compared to the amount of solvent
Arrhenius Definition
Chemical Kinetics
Titration
Concentration
23. Redox reaction - in which the same species is both oxidized and reduced.
STP
Disproportionation
molecular weight
pH
24. A definite stable energy that a physical system can have
s orbital
energy state
redox reaction
hydrogen bonding
25. PH of a molecule at which it contains no net electric charge - isoelectric point.
pI
Acid dissociation constant
Electronegativity
Decomposition reaction
26. 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
Reaction order
lathanide series
Percent yield
molecule
27. A pair of equal and opposite electric charges or magnetic poles separated by a small distance
Group 2A
subshell
Alkaline earths
Dipole
28. Systematic pairing of a deprotonated species (base) with its protonated form (conjugate acid). Conjugates appear on opposite sides of a chemical equation.
Raoult's Law
Conjugate acids and Bases
Triple point
hydrogen bonding
29. 2.18 x 10^-18 J/electron
actinide series
Rydberg constant
Acid dissociation constant
Proton
30. The molar amount of a solute that can dissolve in 1L of solvent until equilibrium - saturation - is reached
The bohr model
Rydberg constant
Molar solubility
Concentration
31. Contains nonmetals that are non - reactive. Full outermost energy level except helium which has 2.
Group 3A
Noble gases
Planck's Constant
Solvent
32. 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
Reaction mechanism
Formal Charge
Ion dipole interactions
STP
33. 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
pI
Graham's Law
lewis base
Solution equilibrium
34. 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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35. A subdivision of an energy level in an atom. They are divided into orbitals.
Ion
subshell
Group 4A
The bohr model
36. 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
Spin quantum number
percent composition
Solute
single displacement reaction
37. Gram equivalent weight of solute per liter of solution - often denoted by N.
Normality
Rydberg constant
polymer
Lewis structure
38. Resulting positive nuclear charge an outer electron senses after accounting for the shielding effect of inner core electrons. Abbreviated as Z(eff). Increases from left to right - and bottom to top on the Periodic Table.
Bronsted Lowry
Noble gases
electron configuration
Effective nuclear charge
39. 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
Pauli exclusion principle
Colligative properties
Formal Charge
Lewis definition
40. The molar solubility of one salt is reduced when another salt - having a common ion is brought into the same solution
ionic cmpound
Common ion effect
Resonance structure
Buffer
41. 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
quantum
Ionic Bond
heisenberg uncertainty principle
Magnetic quantum number
42. Standard Temperature and Pressure. 273 Kelvin (0 Celsius) - 1 atmosphere (760 torr - 760 kPA).
Vapor pressure
periodic trends
Concentration
STP
43. (chemistry) a series from actinium to lawrencium of 15 radioactive elements with increasing atomic numbers
Planck's Constant
actinide series
physical reaction
percent composition
44. The ratio of the number of moles of solute dissolved in one kilogram of solvent. molality (M = moles solute/kg of solution)
Pauli exclusion principle
actinide series
Molality
Balmer series
45. 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.
bond length
Equivalence point
Group 5A
Principle quantum number
46. A chemical formula showing the ratio of elements in a compound rather than the total number of atoms
indicator
empirical formula
Group 3A
Neutron
47. (chemistry) a substance formed by chemical union of two or more elements or ingredients in definite proportion by weight
quanta
Group 5A
compound
Triple point
48. Set of spectral lines appearing in the UV region when a hydrogen atom undergoes a transition from energy levels n>1 to n=1.
Period
Avagadros number
Lyman series
electron affinity
49. Keq describes the ratio of product concentration to reactant concentration - with each raised to the power corresponding ot its coefficient ion in the balanced equation
Octet Rule
Equlibrium constant
periodic trends
Azeotrope
50. Alkaline Earth Metals - 2 valence electrons +2 ions - Magnesium Mg
decomposition reaction
Group 2A
Solubility Product Constant
Lyman series