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MCAT Chemistry
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Subjects
:
mcat
,
science
Instructions:
Answer 50 questions in 15 minutes.
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.
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. (chemistry) a substance that changes color to indicate the presence of some ion or substance
compound
STP
Percent composition
indicator
2. Elements in the middle of the periodic table - in groups 3-12.
solvation
Principle quantum number
VSEPR
transition elements
3. Chalcogens - - Oxide O
electron configuration
Group 6A
Hydrogen bonding
Ground state
4. Large molecular structures - strong covalent bonding - share qualities of IONIC And COVALENT
atomic theory
und's rule
s orbital
Network covalent
5. 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.
electron configuration
Atomic absorption Spectra
Theoretical yield
Concentration
6. The Percent by mass of each element in a compound.
Ion product
Solution equilibrium
Common ion effect
Percent composition
7. The weight in grams of compound that can be substituted by 1 atom of Hydrogen. GEW = MW / # of acidic Hyrdogens
Solution equilibrium
Formula weight
Intermolecular forces
gram equivalent weight
8. A chemical bond that involves sharing a pair of electrons between atoms in a molecule
London forces
Decomposition reaction
Covalent Bond
quantum
9. 5 different orbitals shaped like clover leaves and max electrons is 10
quantum
Ion product
Emperical Formula
d orbital
10. Temperature is constant; effusion and temperature are proportional to the square root of their masses
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11. An ionic compound that resists changes in its pH
Ground state
Buffer
Molality
Ion dipole interactions
12. 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
Diprotic Base
Group 7A
solvation
azimuthal quantum number
13. An atom or group of atoms that has a positive or negative charge
Network covalent
sigma bond
Conjugate acids and Bases
Ion
14. (physics) the smallest discrete quantity of some physical property that a system can possess (according to quantum theory) E=hf
atomic theory
quantum
Group 1A
crystalline solid
15. The molar amount of a solute that can dissolve in 1L of solvent until equilibrium - saturation - is reached
electromagnetic energy of photons emmited from electrons at ground state
Molar solubility
Amphoteric
Bronsted - Lowry definition
16. Named after their cation and anion
Ionization energy
Nonpolar covalent bond
ionic cmpound
Buffer
17. A solid made up of particles that are not arranged in a regular pattern.
Activation energy
amorphous solid
Lyman series
compound
18. Sum of the protons and neutrons in an element often denoted by the letter A
pi bonds
bond length
Buffer
Mass number
19. 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
representative elements
Azeotrope
Atomic absorption Spectra
molecule
20. Region in a molecule where atomic orbitals overlap - resulting in either a stable low - energy bonding orbital or an unstable high - energy antibonding orbital.
Proton
Buffer
Reaction order
Molecular orbital
21. Slightly less reactive than alkali metals - comprise group II
bond energy
Electrolyte
Alkaline earths
Strong acid
22. A measured amount of a solution of unknown concentration is added to a known volume of a second solution until the reaction between them is just complete
gram equivalent weight
Titration
electrolysis
molecular weight
23. Redox reaction - in which the same species is both oxidized and reduced.
periodic trends
polymer
Disproportionation
Lewis acid base reaction
24. 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
Equivalence point
Group 4A
Chemical Kinetics
Arrhenius Definition
25. 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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26. 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.
Vapor pressure
Formal Charge
pi bonds
VSEPR
27. E=hc/?
Noble gases
Net ionic equation
electromagnetic energy of photons emmited from electrons at ground state
Equivalence point
28. The process by which one or more substances change to produce one or more different substances
chemical reaction
Neutron
Buffer
empirical formula
29. One - half the distance between the nuclei of two atoms of the same element when the atoms are joined
theoretical yield
Half equivalence point
Activation energy
atomic radius
30. Contains nonmetals - 7 valence electrons in it's outermost energy level. Very reactive
electron affinity
Triple point
Mass number
Halogens
31. A dynamic condition in which two opposing changes occur at equal rates in a closed system
Reaction mechanism
Half equivalence point
Equilibrium
Intermolecular forces
32. Play- by- play showing the individual steps of a reaction - including the formation and destruction of any reaction intermediates that may occur.
Ion
Planck's Constant
Collision theory of chemical Kinetics
Reaction mechanism
33. Nh/2p The angular momentum changes only in discete amounts with respect to the quantum number. Also E=- R_h/n^2
Ionization energy
sigma bond
Period
angular momentum in the bohr model
34. The percent by mass of each element in a compound
percent composition
Mass number
Triple point
empirical formula
35. The lowest allowable energy state of an atom
Mass number
Atomic absorption Spectra
azimuthal quantum number
Ground state
36. A definite stable energy that a physical system can have
Buffer
energy state
Nucleus
azimuthal quantum number
37. (chemistry) p(otential of) H(ydrogen)
Lyman series
pH
Activation energy
solvation
38. An uncharged molecule with a single unpaitred electron in its outer ring - very unstable - exists for only about 10 seconds
atomic radius
pi bonds
Free radical
Percent composition
39. The nuclear charge experienced by the outermost electrons of an atom (actual charge minus the shielding caused by inner shells: Z- eff)
STP
lathanide series
effective nuclear charge
Ion
40. Alkali metals: highly reactive - therefore always compounds. - 1 valence electron +1 ion - Hydrogen H? - Lithium Li? - Sodium Na? - Potassium K? - Rubidium Rb? - Cesium Cs?
Collision theory of chemical Kinetics
Concentration
Chemical Kinetics
Group 1A
41. The ratio of the number of moles of solute dissolved in one kilogram of solvent. molality (M = moles solute/kg of solution)
Molecular orbital
actinide series
Molality
Collision theory of chemical Kinetics
42. A reaction in which atoms of one element take the place of atoms of another element in a compound
Arrhenius Definition
Effective nuclear charge
Group 7A
single displacement reaction
43. Two or more atoms held together by covalent bonds
indicator
Formula weight
molecule
Ground state
44. 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
Molar solubility
Period
Equlibrium constant
periodic trends
45. The center of the atom which contains the protons and neutrons; in cells - structure that contains the cell's genetic material (DNA) and controls the cell's activities
Theoretical yield
decomposition reaction
Diprotic Base
Nucleus
46. No two electrons or protons or neutrons in a given system can be in states characterized by the same set of quantum numbers
Pauli exclusion principle
Vapor pressure
pI
Group 2A
47. Process by which molecules tend to move from an area where they are more concentrated to an area where they are less concentrated
Diffusion
STP
Equivalence point
Molality
48. A graph of pressure versus temperature that shows the conditions under which the phases of a substance exist
Henderson Hasselbalch Equation
Solubility Product Constant
effective nuclear charge
Phase diagram
49. The point on a phase diagram that represents the only set of conditions at which all three phases exist in equilibrium with one another
Planck's Constant
Triple point
und's rule
Formal Charge
50. A set of frequencies of electromagnetic waves given off by atoms of an element; consists of a series of fine lines of individual colors
Solution equilibrium
Hydrogen bonding
Azeotrope
atomic emission spectrum
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