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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. The amount of a substance that contains as many particles as there are atoms in exactly 12g of carbon -12
Le chateliers Principle
Henderson Hasselbalch Equation
electron configuration
mole
2. Gram equivalent weight of solute per liter of solution - often denoted by N.
Decomposition reaction
Emperical Formula
Phase diagram
Normality
3. Numbers that specify the properties of atomic orbitals and of their electrons
decomposition reaction
quantum numbers
polymer
atomic radius
4. A naturally occurring or synthetic compound consisting of large molecules made up of a linked series of repeated simple monomers
atomic theory
polymer
Reaction order
solvation
5. 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
Hydrogen bonding
London forces
Dispersion Forces
Period
6. 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
Balmer series
Aqueous Solution
Hydrogen bonding
Noble gases
7. A subdivision of an energy level in an atom. They are divided into orbitals.
subshell
Concentration
Dipole Dipole interaction
London forces
8. 1913 - Niels Bohr - said that electrons formed specific layers instead or random ones - said atoms atoms absorb and give off energy when the electrons move from one shell to another
Pauli exclusion principle
Atomic weight
Titration
The bohr model
9. 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
s orbital
Atomic absorption Spectra
Alkaline earths
Theoretical yield
10. Standard Temperature and Pressure. 273 Kelvin (0 Celsius) - 1 atmosphere (760 torr - 760 kPA).
STP
VSEPR
Equilibrium
Molarity
11. PH of a molecule at which it contains no net electric charge - isoelectric point.
pI
pi bonds
Titration
Percent yield
12. An atom or group of atoms that has a positive or negative charge
Equilibrium
Group 1A
single displacement reaction
Ion
13. The energy required to break a chemical bond and form neutral isolated atoms
bond energy
Half equivalence point
Aqueous Solution
Hydrogen bonding
14. A reaction in which atoms of one element take the place of atoms of another element in a compound
single displacement reaction
Aqueous Solution
Molarity
quantum
15. The percent by mass of each element in a compound
Concentration
Charles and Gay Lussac's Law
Group 5A
percent composition
16. 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
Group 7A
redox reaction
Solvent
Half equivalence point
17. The tendency for an atom to attract electrons to itself when it is chemically combined with another element
Electronegativity
Ion product
Rydberg constant
Colligative properties
18. Redox reaction - in which the same species is both oxidized and reduced.
Pauli exclusion principle
molecule
Disproportionation
quantum
19. The process by which one or more substances change to produce one or more different substances
chemical reaction
Lewis acid base reaction
empirical formula
pI
20. 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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21. The ratio of the number of moles of solute dissolved in one kilogram of solvent. molality (M = moles solute/kg of solution)
Molality
Titration
Ion product
crystalline solid
22. 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
Alkaline earths
Balmer series
und's rule
23. Acids defined as electron - pair acceptors and bases as electron - pair donors.
Proton
Lewis definition
compound
Titration
24. The weight in grams of compound that can be substituted by 1 atom of Hydrogen. GEW = MW / # of acidic Hyrdogens
atomic emission spectrum
Lyman series
gram equivalent weight
Balmer series
25. Resulting positive nuclear charge an outer electron senses after accounting for the shielding effect of inner core electrons. Abbreviated as Z(eff). Increases from left to right - and bottom to top on the Periodic Table.
Graham's Law
Molality
Effective nuclear charge
hydrogen bonding
26. 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.
Nucleus
Magnetic quantum number
energy state
Balmer series
27. (chemistry) any theory in which all matter is composed of tiny discrete finite indivisible indestructible particles
Reaction order
atomic theory
Half equivalence point
Molecular orbital
28. 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
Nonpolar covalent bond
Ionization energy
Reaction order
Ion product
29. A structural formula in which electrons are represented by dots; dot pairs or dashes between two atomic symbols represent pairs in covalent bonds.
Diffusion
Lewis structure
Solvent
Electrolyte
30. 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
gram equivalent weight
Combination Reaction
quantum numbers
Resonance structure
31. (physics) the smallest discrete quantity of some physical property that a system can possess (according to quantum theory) E=hf
quantum
Concentration
Neutron
redox reaction
32. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance
Molarity
periodic trends
single displacement reaction
decomposition reaction
33. 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
s orbital
Rate law
Formula weight
Arrhenius Definition
34. Simplest whole # ration of atoms in a compound
Emperical Formula
Ion dipole interactions
Halogens
Buffer
35. (chemistry) p(otential of) H(ydrogen)
pI
indicator
mole
pH
36. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds
lewis base
Molality
Group 4A
lathanide series
37. 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
Effective nuclear charge
Group 6A
Azeotrope
Reaction mechanism
38. 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
atomic radius
Equivalence point
Colligative properties
Lewis definition
39. The nuclear charge experienced by the outermost electrons of an atom (actual charge minus the shielding caused by inner shells: Z- eff)
Principle quantum number
Covalent Bond
effective nuclear charge
Alkaline earths
40. A solid made up of particles that are not arranged in a regular pattern.
Ion product
STP
Ground state
amorphous solid
41. Tells you how much solute is present compared to the amount of solvent
Concentration
Bronsted - Lowry definition
molecule
Charles and Gay Lussac's Law
42. 2.18 x 10^-18 J/electron
Balmer series
Rydberg constant
Equilibrium
Group 3A
43. The process of decomposing a chemical compound by the passage of an electric current.
physical reaction
molecule
Magnetic quantum number
electrolysis
44. The reaction of the ions that characterize acids and the ions that characterize bases to form water molecules and a salt
Dipole
Ion dipole interactions
Neutralization reaction
percent composition
45. Large molecular structures - strong covalent bonding - share qualities of IONIC And COVALENT
Decomposition reaction
Atomic weight
Network covalent
Diffusion
46. The number of atoms in exactly 12 g of pure 12c and equal to 6.022 x 10^23 is called
lewis base
Hydrogen bonding
Avagadros number
Intermolecular forces
47. The point during a titration when the number of H+ ions and OH- ions are equal. This is at the middle of the steepest part of the titration curve.
Ion product
Atomic weight
Arrhenius Definition
Equivalence point
48. A chemical bond that involves sharing a pair of electrons between atoms in a molecule
Covalent Bond
Reaction mechanism
Rate law
lathanide series
49. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
Solvent
redox reaction
Diffusion
Water dissociation Constant
50. 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.
Planck's Constant
atomic radius
Reaction order
Decomposition reaction