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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 structural formula in which electrons are represented by dots; dot pairs or dashes between two atomic symbols represent pairs in covalent bonds.
Lewis structure
Activation energy
Henry's Law
Dipole
2. Tells you how much solute is present compared to the amount of solvent
Vapor pressure
law of constant composition
Concentration
empirical formula
3. No two electrons or protons or neutrons in a given system can be in states characterized by the same set of quantum numbers
Molar solubility
Henry's Law
Pauli exclusion principle
Effective nuclear charge
4. Valence Shell Electron Pair Repulsion theory - stating that the three - dimensional molecular geometry about some central atom is determined by the elctronic repulsion between its bonding and nonbonding electron pairs.
Triple point
molecule
VSEPR
Solute
5. The sum of the exponents in a rate law - where each exponent provides the reaction order with respect to its reactants
Nucleus
Period
Lewis definition
Reaction order
6. 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
Equlibrium constant
Molar solubility
lathanide series
Equivalence point
7. The tendency for an atom to attract electrons to itself when it is chemically combined with another element
Electronegativity
Spin quantum number
ionic cmpound
Atomic absorption Spectra
8. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance
Alkaline earths
Mass number
decomposition reaction
Henry's Law
9. The amount of product that can be made in a chemical reaction based on the amount of limiting reactant
Theoretical yield
Mass number
lathanide series
decomposition reaction
10. 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
sigma bond
Solvent
electron affinity
Arrhenius Definition
11. In a solution - the substance that dissolves in the solvent
Acid dissociation constant
Raoult's Law
Solute
Group 6A
12. 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
Raoult's Law
Ionization energy
Lewis structure
Rydberg constant
13. The solubility of a gas in a liquid is directly proportional to the partial pressure of that gas on the surface of the liquid
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14. Side - to side parallel orbitals overlap to share electrons - the 2nd/3rd covalent bond between two atoms - cannot rotate and maintain the bond.
s orbital
single displacement reaction
sigma bond
pi bonds
15. 5 different orbitals shaped like clover leaves and max electrons is 10
d orbital
Activation energy
Molar solubility
Octet Rule
16. The ways in which electrons are arranged in various orbitals around the nuclei of atoms
bond length
electron configuration
Group 2A
STP
17. 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
Alkaline earths
atomic radius
hydrogen bonding
Solution equilibrium
18. Two or more atoms held together by covalent bonds
Normality
Water dissociation Constant
molecule
electron configuration
19. A substance that - when dissolved in water - results in a solution that can conduct electricity
Ionic Bond
Lewis definition
Electrolyte
Equilibrium
20. Standard Temperature and Pressure. 273 Kelvin (0 Celsius) - 1 atmosphere (760 torr - 760 kPA).
STP
Percent composition
The bohr model
Disproportionation
21. Contains nonmetals that are non - reactive. Full outermost energy level except helium which has 2.
Noble gases
quanta
atomic emission spectrum
Lewis definition
22. A subdivision of an energy level in an atom. They are divided into orbitals.
bond energy
Group 2A
subshell
Hydrogen bonding
23. An atom - radical - or molecule that has gained or lost one or more electrons and has a negative or positive charge
Ion
representative elements
Dispersion Forces
Chemical Kinetics
24. 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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25. The percent by mass of each element in a compound
percent composition
Rydberg constant
energy state
atomic radius
26. 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
Planck's Constant
azimuthal quantum number
London forces
Bronsted Lowry
27. Small discrete increments of energy.
electromagnetic energy of photons emmited from electrons at ground state
Lyman series
quanta
gram equivalent weight
28. A horizontal row of elements in the periodic table
Emperical Formula
Ionic Bond
quanta
Period
29. 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
Spin quantum number
representative elements
Effective nuclear charge
redox reaction
30. The molar amount of a solute that can dissolve in 1L of solvent until equilibrium - saturation - is reached
Molar solubility
Nucleus
decomposition reaction
chemical reaction
31. An atom or group of atoms that has a positive or negative charge
Group 1A
Triple point
Ion
Henry's Law
32. Sum of all the masses - in AMU - present in one molecule of a molecular compound.
effective nuclear charge
redox reaction
Avagadros number
Formula weight
33. Have the shape of a sphere - with the center of the sphere at the nucleus; completely symmetrical along all axes; 1s orbital is spherically symmetric and has no nodes; 2s orbital is also spherical but contains a node and is higher in energy
Ion dipole interactions
s orbital
Effective nuclear charge
Lewis acid base reaction
34. Temperature is constant; effusion and temperature are proportional to the square root of their masses
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35. Elements in the middle of the periodic table - in groups 3-12.
Free radical
transition elements
Azeotrope
Neutralization reaction
36. 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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37. The reaction of the ions that characterize acids and the ions that characterize bases to form water molecules and a salt
Reaction order
pI
transition elements
Neutralization reaction
38. A concentration unit of a solution expressed as moles of solute dissolved per liter of solution
Molarity
The bohr model
Aqueous Solution
Percent yield
39. 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
mole
STP
Colligative properties
40. 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.
Le chateliers Principle
Group 5A
Ion product
ionic cmpound
41. 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.
single displacement reaction
Aqueous Solution
Solubility Product Constant
Group 1A
42. 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.
Atomic absorption Spectra
Triple point
Common ion effect
atomic emission spectrum
43. 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
pI
molecular weight
Colligative properties
indicator
44. States that if a stress is applied to a system at equilibrium - the system shifts in the direction that relieves the stress.
electrolysis
Le chateliers Principle
The bohr model
actinide series
45. A set of spectral lines that appear in the visible light region when a hydrogen atom undergoes a transition from energy levels n>2 to n=2.
Graham's Law
Diffusion
Mass number
Balmer series
46. (chemistry) p(otential of) H(ydrogen)
angular momentum in the bohr model
Conjugate acids and Bases
Molarity
pH
47. 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.
Colligative properties
Activation energy
Aqueous Solution
Group 3A
48. The lowest allowable energy state of an atom
Ground state
Theoretical yield
Decomposition reaction
Bronsted Lowry
49. A dynamic condition in which two opposing changes occur at equal rates in a closed system
Planck's Constant
Equilibrium
Reaction mechanism
Solution equilibrium
50. The slowest elementary step which is the limit for the rate of the other steps
actinide series
quantum
atomic emission spectrum
Rate determining step