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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. Contains nonmetals - 7 valence electrons in it's outermost energy level. Very reactive
molecular weight
Halogens
Bronsted Lowry
Bronsted - Lowry definition
2. An acid that will completely dissociate in aqueous solution - like HCl - HI - HClO4 HBr.
Strong acid
Ionic Bond
Acid dissociation constant
Decomposition reaction
3. Process by which molecules tend to move from an area where they are more concentrated to an area where they are less concentrated
Solubility Product Constant
Electrolyte
Proton
Diffusion
4. 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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5. A horizontal row of elements in the periodic table
Group 5A
Period
Normality
molecular weight
6. An ionic compound that resists changes in its pH
Magnetic quantum number
Bronsted - Lowry definition
Buffer
atomic radius
7. A chemical bond that involves sharing a pair of electrons between atoms in a molecule
Covalent Bond
Equlibrium constant
Solution equilibrium
Buffer
8. The ratio of the actual yield to the theoretical yield for a chemical reaction expressed as a percentage; a measure of the efficiency of a reaction
Rate law
Percent yield
Concentration
Solution equilibrium
9. The molar solubility of one salt is reduced when another salt - having a common ion is brought into the same solution
pH
Henderson Hasselbalch Equation
Common ion effect
Arrhenius Definition
10. Expression of auto - ionization of water into H+ and OH- at a certain temperature - given by the product of the ions' molar concentrations. Denoted by Kw and equal to 10-
Free radical
Water dissociation Constant
Lyman series
Ion product
11. The number of atoms in exactly 12 g of pure 12c and equal to 6.022 x 10^23 is called
Avagadros number
Atomic absorption Spectra
Bronsted - Lowry definition
Charles and Gay Lussac's Law
12. A chemical formula showing the ratio of elements in a compound rather than the total number of atoms
empirical formula
polymer
Effective nuclear charge
lewis base
13. 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
amorphous solid
Resonance structure
Intermolecular forces
Titration
14. Attractions between molecules caused by the electron motion on one molecule affecting the electron motion on the other through electrical forces; these are the weakest interactions between molecules
Ion
Dispersion Forces
periodic trends
Formula weight
15. 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.
VSEPR
Acid dissociation constant
Dipole Dipole interaction
Diffusion
16. PH=pka+log[base/acid] Used in titration based problems that relates the pH or pOH of a solution to the pK and the ratio of the dissociated species.
Henderson Hasselbalch Equation
Proton
London forces
Effusion
17. (chemistry) any theory in which all matter is composed of tiny discrete finite indivisible indestructible particles
atomic theory
periodic trends
indicator
chemical reaction
18. The Percent by mass of each element in a compound.
Molarity
Percent composition
Ionization energy
Phase diagram
19. The weight in grams of one mole of a given elementand is expressedin tems of grams per mole.
Azeotrope
solvation
Atomic weight
Net ionic equation
20. Gram equivalent weight of solute per liter of solution - often denoted by N.
Pauli exclusion principle
Normality
s orbital
Water dissociation Constant
21. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
physical reaction
Ion product
Reaction order
redox reaction
22. An elementary particle with 0 charge and mass about equal to a proton
pi bonds
Effective nuclear charge
Neutron
electromagnetic energy of photons emmited from electrons at ground state
23. A concentration unit of a solution expressed as moles of solute dissolved per liter of solution
pi bonds
sigma bond
Molarity
crystalline solid
24. The amount of product that can be made in a chemical reaction based on the amount of limiting reactant
Half equivalence point
Percent yield
Vapor pressure
Theoretical yield
25. 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
Raoult's Law
STP
Balmer series
26. Large molecular structures - strong covalent bonding - share qualities of IONIC And COVALENT
pi bonds
transition elements
Network covalent
Octet Rule
27. Nh/2p The angular momentum changes only in discete amounts with respect to the quantum number. Also E=- R_h/n^2
Dispersion Forces
Group 6A
angular momentum in the bohr model
heisenberg uncertainty principle
28. The ratio of the number of moles of solute dissolved in one kilogram of solvent. molality (M = moles solute/kg of solution)
Molality
atomic theory
law of constant composition
und's rule
29. Named after their cation and anion
Phase diagram
indicator
Atomic weight
ionic cmpound
30. When polar molecules orient themselves such that the positive region of one molecule is close to the negative region of another molecule.
bond energy
Disproportionation
London forces
Dipole Dipole interaction
31. The sum of the exponents in a rate law - where each exponent provides the reaction order with respect to its reactants
Raoult's Law
Reaction order
single displacement reaction
Avagadros number
32. Theory stating that the rate of a reaction is directly proportional to the number of collisions that take place between reactants per second.
Emperical Formula
Collision theory of chemical Kinetics
Free radical
Octet Rule
33. 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.
Lyman series
electron affinity
Disproportionation
Principle quantum number
34. The molar amount of a solute that can dissolve in 1L of solvent until equilibrium - saturation - is reached
Ionization energy
Diprotic Base
Proton
Molar solubility
35. A base that can accept two moles of H+ per mole of itself (ex: SO4
Free radical
lathanide series
Diprotic Base
Atomic absorption Spectra
36. 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
Magnetic quantum number
atomic radius
The bohr model
electrolysis
37. The process of decomposing a chemical compound by the passage of an electric current.
electrolysis
single displacement reaction
Molarity
energy state
38. 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
polymer
Acid dissociation constant
Raoult's Law
Ionic Bond
39. The formation of one or more covalent bonds between an electron pair donor and an electron pair acceptor
Lewis acid base reaction
pI
atomic emission spectrum
single displacement reaction
40. The energy required to break a chemical bond and form neutral isolated atoms
empirical formula
bond energy
Titration
amorphous solid
41. Substance in which a solute is dissolved to form a solution
STP
effective nuclear charge
Halogens
Solvent
42. The slowest elementary step which is the limit for the rate of the other steps
Henry's Law
atomic theory
Rate determining step
Covalent Bond
43. Elements in the middle of the periodic table - in groups 3-12.
transition elements
Electronegativity
Redox Half Reaction
Activation energy
44. 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
Atomic absorption Spectra
Group 7A
Rate law
The bohr model
45. 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 3A
Group 2A
Phase diagram
Formal Charge
46. Any sample of a given compound will contain the same elements in the identical mass ratio.
Nucleus
Rydberg constant
law of constant composition
Neutron
47. Small discrete increments of energy.
quanta
Alkaline earths
Acid dissociation constant
Concentration
48. Alkaline Earth Metals - 2 valence electrons +2 ions - Magnesium Mg
bond energy
Group 2A
indicator
The bohr model
49. Contains nonmetals that are non - reactive. Full outermost energy level except helium which has 2.
single displacement reaction
Pauli exclusion principle
Noble gases
Formal Charge
50. The maximum amount of product that can be produced from a given amount of reactant
atomic emission spectrum
theoretical yield
Rate law
Le chateliers Principle