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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. A pair of equal and opposite electric charges or magnetic poles separated by a small distance
Dipole
Net ionic equation
azimuthal quantum number
solvation
2. Attractive and repulsive forces between molecules that are weaker than forces within molecules.
bond length
Neutron
Intermolecular forces
amorphous solid
3. 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
molecular weight
Disproportionation
Resonance structure
Phase diagram
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. Temperature is constant; effusion and temperature are proportional to the square root of their masses
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6. 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
Decomposition reaction
Electrolyte
Diffusion
Ionization energy
7. Nh/2p The angular momentum changes only in discete amounts with respect to the quantum number. Also E=- R_h/n^2
Colligative properties
Period
angular momentum in the bohr model
London forces
8. Contains nonmetals that are non - reactive. Full outermost energy level except helium which has 2.
percent composition
Noble gases
Concentration
gram equivalent weight
9. A graph of pressure versus temperature that shows the conditions under which the phases of a substance exist
Common ion effect
Phase diagram
Electrolyte
azimuthal quantum number
10. 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
amorphous solid
Azeotrope
electron configuration
Activation energy
11. A solid made up of particles that are not arranged in a regular pattern.
sigma bond
amorphous solid
actinide series
pI
12. Rare earth element group (elements 58-71)
Concentration
lathanide series
Molar solubility
representative elements
13. A chemical formula showing the ratio of elements in a compound rather than the total number of atoms
empirical formula
Formal Charge
Water dissociation Constant
Raoult's Law
14. (chemistry) a substance that changes color to indicate the presence of some ion or substance
Ionic Bond
Concentration
Resonance structure
indicator
15. In a solution - the substance that dissolves in the solvent
Solute
pI
Ionization energy
Ion
16. 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
bond energy
London forces
Le chateliers Principle
Solution equilibrium
17. 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.
lathanide series
Dipole
Solubility Product Constant
Balmer series
18. An elementary particle with 0 charge and mass about equal to a proton
Neutron
periodic trends
lathanide series
Colligative properties
19. A concentration unit of a solution expressed as moles of solute dissolved per liter of solution
redox reaction
bond energy
Molarity
Rydberg constant
20. A set of frequencies of electromagnetic waves given off by atoms of an element; consists of a series of fine lines of individual colors
Nonpolar covalent bond
atomic emission spectrum
quantum numbers
d orbital
21. 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
electron affinity
Covalent Bond
Nucleus
Ion
22. 5 different orbitals shaped like clover leaves and max electrons is 10
atomic radius
d orbital
Ion product
Amphoteric
23. Solids in which the particles are arranged in a repeating - 3- D pattern - has a specific melting point - classified as ionic network covalent - metallic or molecular.
Spin quantum number
crystalline solid
Rate determining step
Graham's Law
24. A model of acids and bases which an acid is hydrogen ion donor and base is a hydrogen ion acceptor.
Ion
chemical reaction
London forces
Bronsted Lowry
25. Process by which molecules tend to move from an area where they are more concentrated to an area where they are less concentrated
subshell
Molarity
Diffusion
pH
26. Common definition of acids as proton (H+) donors and bases as proton acceptors
single displacement reaction
quantum numbers
Lewis acid base reaction
Bronsted - Lowry definition
27. PH of a molecule at which it contains no net electric charge - isoelectric point.
electron configuration
Arrhenius Definition
pI
crystalline solid
28. A subatomic particle that has a positive charge and that is found in the nucleus of an atom Charge of +1 and mass of 1.0073 amu
Diffusion
Proton
Group 3A
STP
29. Sum of all the masses - in AMU - present in one molecule of a molecular compound.
Half equivalence point
Formula weight
indicator
Diprotic Base
30. Slightly less reactive than alkali metals - comprise group II
actinide series
Net ionic equation
Alkaline earths
ionic cmpound
31. Alkaline Earth Metals - 2 valence electrons +2 ions - Magnesium Mg
Group 2A
Percent yield
Rate determining step
Lyman series
32. Any sample of a given compound will contain the same elements in the identical mass ratio.
single displacement reaction
law of constant composition
redox reaction
Period
33. A covalent bond in which the bonding electrons are shared equally by the bonded atoms - resulting in a balanced distribution of electrical charge
Net ionic equation
Emperical Formula
Nonpolar covalent bond
und's rule
34. Two or more atoms held together by covalent bonds
Percent yield
Bronsted Lowry
molecule
Mass number
35. A base that can accept two moles of H+ per mole of itself (ex: SO4
solvation
quanta
atomic radius
Diprotic Base
36. A substance that - when dissolved in water - results in a solution that can conduct electricity
Neutralization reaction
decomposition reaction
bond length
Electrolyte
37. 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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38. Numbers that specify the properties of atomic orbitals and of their electrons
quantum numbers
Molar solubility
Lewis definition
Formula weight
39. Systematic pairing of a deprotonated species (base) with its protonated form (conjugate acid). Conjugates appear on opposite sides of a chemical equation.
Formal Charge
Ground state
Conjugate acids and Bases
Ionization energy
40. 5 valence electrons -3 ions - Nitride N
Group 5A
Titration
Collision theory of chemical Kinetics
compound
41. Where half of the acid is neutralized by the base on a titration curveAn acid dissociation constant - Ka - (also known as acidity constant - or acid - ionization constant) is a quantitative measure of the strength of an acid in solution. It is the eq
Emperical Formula
Ion
Equivalence point
Half equivalence point
42. The sum of the exponents in a rate law - where each exponent provides the reaction order with respect to its reactants
Electrolyte
Diffusion
Reaction order
Solubility Product Constant
43. The ratio of the number of moles of solute dissolved in one kilogram of solvent. molality (M = moles solute/kg of solution)
Free radical
redox reaction
Equlibrium constant
Molality
44. 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
Resonance structure
Colligative properties
Reaction order
Lewis structure
45. The nuclear charge experienced by the outermost electrons of an atom (actual charge minus the shielding caused by inner shells: Z- eff)
effective nuclear charge
hydrogen bonding
Group 4A
Ion product
46. Atoms react by gaining or losing electrons so as to acquire the stable electron structure of a noble gas - usually eight valence electrons
Octet Rule
Ground state
Aqueous Solution
Bronsted - Lowry definition
47. 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
Ion
electrolysis
Group 7A
Decomposition reaction
48. A solution in which water is the solvent
Aqueous Solution
azimuthal quantum number
Combination Reaction
Octet Rule
49. 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.
redox reaction
Strong acid
energy state
Atomic absorption Spectra
50. 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
s orbital
Spin quantum number
Neutralization reaction
Titration