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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 subdivision of an energy level in an atom. They are divided into orbitals.
Common ion effect
subshell
redox reaction
redox reaction
2. Alkali metals: highly reactive - therefore always compounds. - 1 valence electron +1 ion - Hydrogen H? - Lithium Li? - Sodium Na? - Potassium K? - Rubidium Rb? - Cesium Cs?
Strong acid
Group 1A
bond length
Nucleus
3. A dynamic condition in which two opposing changes occur at equal rates in a closed system
STP
Ion product
Activation energy
Equilibrium
4. States that if a stress is applied to a system at equilibrium - the system shifts in the direction that relieves the stress.
electromagnetic energy of photons emmited from electrons at ground state
effective nuclear charge
Le chateliers Principle
Ionic Bond
5. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance C>>>>A+B
Henderson Hasselbalch Equation
heisenberg uncertainty principle
Period
Decomposition reaction
6. Simplest whole # ration of atoms in a compound
Concentration
Lewis definition
Azeotrope
Emperical Formula
7. The area of chemistry that is concerned with reaction rates and reaction mechanisms
Equivalence point
The bohr model
s orbital
Chemical Kinetics
8. E=hc/?
Group 6A
Ion
Electrolyte
electromagnetic energy of photons emmited from electrons at ground state
9. A definite stable energy that a physical system can have
molecular weight
energy state
Diffusion
Atomic absorption Spectra
10. Chalcogens - - Oxide O
Net ionic equation
Solubility Product Constant
s orbital
Group 6A
11. The Percent by mass of each element in a compound.
Colligative properties
Percent composition
Rate law
single displacement reaction
12. A naturally occurring or synthetic compound consisting of large molecules made up of a linked series of repeated simple monomers
Mass number
angular momentum in the bohr model
Group 4A
polymer
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
Resonance structure
Octet Rule
lathanide series
Common ion effect
14. Numbers that specify the properties of atomic orbitals and of their electrons
Disproportionation
quantum numbers
Solute
energy state
15. The nuclear charge experienced by the outermost electrons of an atom (actual charge minus the shielding caused by inner shells: Z- eff)
Dispersion Forces
effective nuclear charge
Neutralization reaction
Arrhenius Definition
16. 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
empirical formula
Strong acid
Buffer
Ionization energy
17. The solubility of a gas in a liquid is directly proportional to the partial pressure of that gas on the surface of the liquid
18. Rare earth element group (elements 58-71)
Electrolyte
lathanide series
Concentration
Emperical Formula
19. 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
Group 7A
electron configuration
Ionic Bond
20. 2.18 x 10^-18 J/electron
Solubility Product Constant
Vapor pressure
Rydberg constant
Neutralization reaction
21. A solution in which water is the solvent
Vapor pressure
Aqueous Solution
Ion dipole interactions
Group 6A
22. 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.
polymer
Ion product
Solubility Product Constant
VSEPR
23. 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
single displacement reaction
Diprotic Base
s orbital
molecular weight
24. Slightly less reactive than alkali metals - comprise group II
Group 1A
Alkaline earths
Raoult's Law
Reaction order
25. Having characteristics of both an acid and a base and capable of reacting as either
Ionization energy
Equlibrium constant
Common ion effect
Amphoteric
26. A reaction in which atoms of one element take the place of atoms of another element in a compound
single displacement reaction
Atomic absorption Spectra
bond energy
percent composition
27. Tells you how much solute is present compared to the amount of solvent
Concentration
bond energy
Rydberg constant
Solute
28. The pressure exerted by a vapor in equilibrium with its liquid or solid phase
Conjugate acids and Bases
Magnetic quantum number
Vapor pressure
d orbital
29. 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.
Combination Reaction
Titration
Atomic absorption Spectra
sigma bond
30. Energy released when an atom or ion in the gaseous state gains an electron. Increases from left to right and from bottom to top on the Periodic Table.
Rate law
electron affinity
Group 1A
d orbital
31. 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
Concentration
Equlibrium constant
hydrogen bonding
Redox Half Reaction
32. 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
single displacement reaction
Solution equilibrium
Chemical Kinetics
Net ionic equation
33. 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.
crystalline solid
electron affinity
energy state
Solubility Product Constant
34. A reaction in which two or more substances combine to form a single substance A+B>>>>>>>C
Combination Reaction
Graham's Law
percent composition
Lewis acid base reaction
35. One - half the distance between the nuclei of two atoms of the same element when the atoms are joined
Strong acid
atomic radius
quantum
Molality
36. A concentration unit of a solution expressed as moles of solute dissolved per liter of solution
Spin quantum number
Atomic absorption Spectra
Group 1A
Molarity
37. 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
quanta
Covalent Bond
Molality
Group 7A
38. 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
Proton
Nonpolar covalent bond
molecular weight
azimuthal quantum number
39. Set of spectral lines appearing in the UV region when a hydrogen atom undergoes a transition from energy levels n>1 to n=1.
theoretical yield
London forces
Lyman series
Nucleus
40. An elementary particle with 0 charge and mass about equal to a proton
Neutron
Lewis acid base reaction
Bronsted - Lowry definition
Ion
41. The point on a phase diagram that represents the only set of conditions at which all three phases exist in equilibrium with one another
Triple point
Solubility Product Constant
Molecular orbital
Water dissociation Constant
42. An emperimentally determined mathmatical expression showing the rate of a reaction as a function of the concentration of its reactants
Rate law
Strong acid
Solubility Product Constant
Octet Rule
43. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
redox reaction
Formula weight
angular momentum in the bohr model
theoretical yield
44. Sol - a chemical process in which solvent molecules and molecules or ions of the solute combine to form a compound
indicator
Lyman series
solvation
law of constant composition
45. The process by which one or more substances change to produce one or more different substances
chemical reaction
und's rule
effective nuclear charge
Rydberg constant
46. The molar amount of a solute that can dissolve in 1L of solvent until equilibrium - saturation - is reached
Molar solubility
Atomic absorption Spectra
Theoretical yield
hydrogen bonding
47. The lowest allowable energy state of an atom
Proton
Ground state
Net ionic equation
Phase diagram
48. Contains nonmetals - 7 valence electrons in it's outermost energy level. Very reactive
Formula weight
Halogens
sigma bond
Pauli exclusion principle
49. A reaction where a compound does Not change its molecular structure.
Ion
Ionic Bond
periodic trends
physical reaction
50. (physics) the smallest discrete quantity of some physical property that a system can possess (according to quantum theory) E=hf
Rydberg constant
quantum
atomic radius
VSEPR