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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. An ionic compound that resists changes in its pH
energy state
percent composition
Titration
Buffer
2. A base that can accept two moles of H+ per mole of itself (ex: SO4
Diprotic Base
Ion dipole interactions
Group 3A
The bohr model
3. When dipoles are dissolved in a solution where ions are present ions wil arrange themselves with the opposite charged end of the dipole.
single displacement reaction
Ion dipole interactions
Decomposition reaction
The bohr model
4. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
Bronsted Lowry
redox reaction
Octet Rule
indicator
5. 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
Avagadros number
Solution equilibrium
Lewis structure
electrolysis
6. Any sample of a given compound will contain the same elements in the identical mass ratio.
law of constant composition
Planck's Constant
periodic trends
Nucleus
7. A horizontal row of elements in the periodic table
electron configuration
Period
empirical formula
law of constant composition
8. Orbitals of equal energy are each occupied by one electron before any orbital is occupied by a second electron - and all electrons in singly occupied orbitals must have the same spin
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9. 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.
quanta
Group 5A
atomic radius
subshell
10. A structural formula in which electrons are represented by dots; dot pairs or dashes between two atomic symbols represent pairs in covalent bonds.
Charles and Gay Lussac's Law
Normality
Proton
Lewis structure
11. 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.
Neutralization reaction
Atomic absorption Spectra
Conjugate acids and Bases
Neutron
12. 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
Lyman series
Balmer series
pi bonds
13. Two or more atoms held together by covalent bonds
Atomic absorption Spectra
Lewis acid base reaction
bond length
molecule
14. The slowest elementary step which is the limit for the rate of the other steps
Rate determining step
Collision theory of chemical Kinetics
Diffusion
Henderson Hasselbalch Equation
15. Nh/2p The angular momentum changes only in discete amounts with respect to the quantum number. Also E=- R_h/n^2
angular momentum in the bohr model
Network covalent
s orbital
electron affinity
16. The process of decomposing a chemical compound by the passage of an electric current.
Molarity
quantum numbers
electrolysis
Avagadros number
17. At a constant pressure - the volume of an ideal gas is directly proportinal to its temperature: V (a) T
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18. An elementary particle with 0 charge and mass about equal to a proton
Neutron
molecular weight
Group 2A
bond length
19. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds
Mass number
empirical formula
pi bonds
Group 4A
20. 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.
Balmer series
Hydrogen bonding
Lyman series
Henry's Law
21. Sol - a chemical process in which solvent molecules and molecules or ions of the solute combine to form a compound
Electrolyte
solvation
sigma bond
Dipole
22. The weight in grams of one mole of a given elementand is expressedin tems of grams per mole.
Noble gases
Atomic weight
d orbital
polymer
23. Elements in the middle of the periodic table - in groups 3-12.
atomic emission spectrum
London forces
transition elements
Emperical Formula
24. The hypothetical equation showing only the species that is oxidized or reduced in a redox reaction and the correct number of electrons transferred between the species in the complete - balanced equation.
Redox Half Reaction
electron configuration
Principle quantum number
molecular weight
25. (chemistry) any theory in which all matter is composed of tiny discrete finite indivisible indestructible particles
Nucleus
single displacement reaction
atomic theory
lewis base
26. States that it is impossible to determine simultaneously both the position and momentum of an electron or any other particle
Resonance structure
single displacement reaction
Percent yield
heisenberg uncertainty principle
27. Property of the elements that can be predicted from the arrangement of the periodic table
Principle quantum number
periodic trends
Period
Resonance structure
28. Temperature is constant; effusion and temperature are proportional to the square root of their masses
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29. The ratio of the number of moles of solute dissolved in one kilogram of solvent. molality (M = moles solute/kg of solution)
Amphoteric
Bronsted - Lowry definition
Conjugate acids and Bases
Molality
30. 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
London forces
Magnetic quantum number
Equlibrium constant
Bronsted - Lowry definition
31. Process by which molecules tend to move from an area where they are more concentrated to an area where they are less concentrated
Diffusion
Molar solubility
indicator
compound
32. The amount of energy that reactants must absorb before a chemical reaction will start; also called free energy of activation.
Redox Half Reaction
Activation energy
Arrhenius Definition
transition elements
33. A set of frequencies of electromagnetic waves given off by atoms of an element; consists of a series of fine lines of individual colors
decomposition reaction
Ion
atomic emission spectrum
Equilibrium
34. Contains nonmetals - 7 valence electrons in it's outermost energy level. Very reactive
Strong acid
Principle quantum number
Halogens
Lewis definition
35. A naturally occurring or synthetic compound consisting of large molecules made up of a linked series of repeated simple monomers
electrolysis
polymer
Acid dissociation constant
bond energy
36. An atom - radical - or molecule that has gained or lost one or more electrons and has a negative or positive charge
Bronsted - Lowry definition
Concentration
Halogens
Ion
37. Common definition of acids as proton (H+) donors and bases as proton acceptors
Bronsted - Lowry definition
electromagnetic energy of photons emmited from electrons at ground state
Vapor pressure
Effusion
38. Alkali metals: highly reactive - therefore always compounds. - 1 valence electron +1 ion - Hydrogen H? - Lithium Li? - Sodium Na? - Potassium K? - Rubidium Rb? - Cesium Cs?
Equlibrium constant
amorphous solid
subshell
Group 1A
39. A subdivision of an energy level in an atom. They are divided into orbitals.
actinide series
Reaction mechanism
subshell
Titration
40. The process by which one or more substances change to produce one or more different substances
heisenberg uncertainty principle
chemical reaction
transition elements
Azeotrope
41. (chemistry) a substance formed by chemical union of two or more elements or ingredients in definite proportion by weight
compound
subshell
single displacement reaction
Solute
42. An acid that will completely dissociate in aqueous solution - like HCl - HI - HClO4 HBr.
Rate determining step
Electrolyte
Strong acid
energy state
43. A reaction in which two or more substances combine to form a single substance A+B>>>>>>>C
Rydberg constant
Molar solubility
Reaction mechanism
Combination Reaction
44. The percent by mass of each element in a compound
Free radical
Lyman series
atomic emission spectrum
percent composition
45. 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
Acid dissociation constant
gram equivalent weight
hydrogen bonding
Hydrogen bonding
46. 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
Triple point
single displacement reaction
polymer
Magnetic quantum number
47. 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
Effusion
Solute
crystalline solid
Ionic Bond
48. 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
Half equivalence point
Azeotrope
Vapor pressure
bond energy
49. (chemistry) a series from actinium to lawrencium of 15 radioactive elements with increasing atomic numbers
redox reaction
actinide series
decomposition reaction
Colligative properties
50. The maximum amount of product that can be produced from a given amount of reactant
amorphous solid
Dipole
Planck's Constant
theoretical yield