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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.
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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. Simplest whole # ration of atoms in a compound
Emperical Formula
angular momentum in the bohr model
Decomposition reaction
Dipole
2. Standard Temperature and Pressure. 273 Kelvin (0 Celsius) - 1 atmosphere (760 torr - 760 kPA).
Balmer series
sigma bond
STP
quanta
3. 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
Group 2A
Formal Charge
mole
Lewis structure
4. Gram equivalent weight of solute per liter of solution - often denoted by N.
Normality
Chemical Kinetics
Mass number
Group 7A
5. A representation of a displacement reaction showing only the reactive species and omitting the spectator ions.
Net ionic equation
compound
Dipole
pI
6. 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.
Solubility Product Constant
Water dissociation Constant
Vapor pressure
Buffer
7. A bond formed when two atomic orbitals combine to form a molecular orbital that is symmetrical around the axis connecting the two atomic nuclei
sigma bond
Mass number
Half equivalence point
Dipole Dipole interaction
8. Numbers that specify the properties of atomic orbitals and of their electrons
atomic radius
quantum numbers
s orbital
The bohr model
9. One - half the distance between the nuclei of two atoms of the same element when the atoms are joined
Molarity
atomic radius
Solute
Redox Half Reaction
10. A reaction where a compound does Not change its molecular structure.
physical reaction
Percent composition
Equlibrium constant
Emperical Formula
11. The amount of energy that reactants must absorb before a chemical reaction will start; also called free energy of activation.
Activation energy
Henderson Hasselbalch Equation
The bohr model
Chemical Kinetics
12. 5 different orbitals shaped like clover leaves and max electrons is 10
Titration
d orbital
hydrogen bonding
Equlibrium constant
13. The process by which a gas escapes from one container to another at lower pressure through a tiny hole in the container.
Principle quantum number
quantum
Phase diagram
Effusion
14. A graph of pressure versus temperature that shows the conditions under which the phases of a substance exist
Neutron
Solute
Phase diagram
Effusion
15. 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.
sigma bond
Ion product
Redox Half Reaction
Group 6A
16. 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
atomic emission spectrum
Graham's Law
Lewis definition
17. Nh/2p The angular momentum changes only in discete amounts with respect to the quantum number. Also E=- R_h/n^2
London forces
heisenberg uncertainty principle
angular momentum in the bohr model
Network covalent
18. Systematic pairing of a deprotonated species (base) with its protonated form (conjugate acid). Conjugates appear on opposite sides of a chemical equation.
Nucleus
Nonpolar covalent bond
Conjugate acids and Bases
Henderson Hasselbalch Equation
19. At a constant pressure - the volume of an ideal gas is directly proportinal to its temperature: V (a) T
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20. Tells you how much solute is present compared to the amount of solvent
Equivalence point
Concentration
Aqueous Solution
London forces
21. 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.
Group 3A
Equivalence point
Neutron
periodic trends
22. 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
decomposition reaction
Group 7A
Diffusion
empirical formula
23. Common definition of acids as proton (H+) donors and bases as proton acceptors
Bronsted - Lowry definition
Neutralization reaction
Dipole Dipole interaction
theoretical yield
24. A naturally occurring or synthetic compound consisting of large molecules made up of a linked series of repeated simple monomers
Diprotic Base
polymer
sigma bond
Mass number
25. 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
electron affinity
Azeotrope
Electrolyte
Group 7A
26. Alkali metals: highly reactive - therefore always compounds. - 1 valence electron +1 ion - Hydrogen H? - Lithium Li? - Sodium Na? - Potassium K? - Rubidium Rb? - Cesium Cs?
Group 1A
Effective nuclear charge
Lyman series
Alkaline earths
27. A pair of equal and opposite electric charges or magnetic poles separated by a small distance
polymer
Bronsted Lowry
Dipole
pI
28. Sol - a chemical process in which solvent molecules and molecules or ions of the solute combine to form a compound
Electrolyte
Balmer series
solvation
Triple point
29. The intermolecular force in which a hydrogen atom that is bonded to a highly electronegative atom is attracted to an unshared pair of electrons of an electronegative atom in a nearby molecule
pH
Avagadros number
amorphous solid
Hydrogen bonding
30. 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.
Ionization energy
und's rule
Ion product
redox reaction
31. An atom or group of atoms that has a positive or negative charge
Planck's Constant
Principle quantum number
subshell
Ion
32. An uncharged molecule with a single unpaitred electron in its outer ring - very unstable - exists for only about 10 seconds
Proton
electron affinity
bond length
Free radical
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
Solution equilibrium
Redox Half Reaction
atomic theory
atomic emission spectrum
34. Elements in the middle of the periodic table - in groups 3-12.
angular momentum in the bohr model
STP
transition elements
Nonpolar covalent bond
35. Small discrete increments of energy.
und's rule
quanta
percent composition
molecule
36. PH of a molecule at which it contains no net electric charge - isoelectric point.
hydrogen bonding
Halogens
pI
Lewis definition
37. 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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38. The lowest allowable energy state of an atom
Magnetic quantum number
quantum numbers
Ground state
Molarity
39. A solid made up of particles that are not arranged in a regular pattern.
redox reaction
Effusion
Octet Rule
amorphous solid
40. The molar amount of a solute that can dissolve in 1L of solvent until equilibrium - saturation - is reached
Bronsted - Lowry definition
Group 5A
Molar solubility
Dipole Dipole interaction
41. 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.
Group 1A
Atomic absorption Spectra
Buffer
Dispersion Forces
42. The percent by mass of each element in a compound
Molecular orbital
Azeotrope
Group 1A
percent composition
43. When polar molecules orient themselves such that the positive region of one molecule is close to the negative region of another molecule.
periodic trends
STP
Dipole Dipole interaction
pi bonds
44. 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.
Molecular orbital
lewis base
bond length
Principle quantum number
45. The number of atoms in exactly 12 g of pure 12c and equal to 6.022 x 10^23 is called
Acid dissociation constant
hydrogen bonding
Avagadros number
Solution equilibrium
46. (physics) the smallest discrete quantity of some physical property that a system can possess (according to quantum theory) E=hf
quantum
Principle quantum number
Ion
quantum numbers
47. Substance in which a solute is dissolved to form a solution
Solvent
Formula weight
Solubility Product Constant
Water dissociation Constant
48. (chemistry) a substance formed by chemical union of two or more elements or ingredients in definite proportion by weight
Mass number
atomic emission spectrum
Ground state
compound
49. An ionic compound that resists changes in its pH
Free radical
Buffer
indicator
quanta
50. 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
Acid dissociation constant
Ion product
Colligative properties
ionic cmpound
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