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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. An elementary particle with 0 charge and mass about equal to a proton
Ion product
Neutron
Hydrogen bonding
Diffusion
2. 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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3. (chemistry) a series from actinium to lawrencium of 15 radioactive elements with increasing atomic numbers
actinide series
Theoretical yield
atomic radius
effective nuclear charge
4. Numbers that specify the properties of atomic orbitals and of their electrons
lewis base
Lewis definition
quantum numbers
Lewis structure
5. Named after their cation and anion
quanta
Lewis structure
ionic cmpound
chemical reaction
6. A definite stable energy that a physical system can have
Strong acid
indicator
Colligative properties
energy state
7. Property of the elements that can be predicted from the arrangement of the periodic table
Theoretical yield
Neutralization reaction
Ion
periodic trends
8. 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.
electron affinity
Buffer
Ground state
Rate law
9. 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
und's rule
Percent yield
Ion product
Lewis definition
10. 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
Neutralization reaction
Colligative properties
VSEPR
11. 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
electrolysis
Colligative properties
Dipole Dipole interaction
Formula weight
12. (chemistry) a substance formed by chemical union of two or more elements or ingredients in definite proportion by weight
Solution equilibrium
Group 4A
compound
ionic cmpound
13. The process of decomposing a chemical compound by the passage of an electric current.
Activation energy
Group 1A
electrolysis
decomposition reaction
14. 5 different orbitals shaped like clover leaves and max electrons is 10
Chemical Kinetics
Principle quantum number
d orbital
Molality
15. 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
bond energy
Avagadros number
Ionic Bond
Titration
16. E=hc/?
actinide series
STP
electromagnetic energy of photons emmited from electrons at ground state
Group 6A
17. 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
Emperical Formula
s orbital
Concentration
Equlibrium constant
18. A bond formed when two atomic orbitals combine to form a molecular orbital that is symmetrical around the axis connecting the two atomic nuclei
Amphoteric
Principle quantum number
sigma bond
Effusion
19. Acids defined as electron - pair acceptors and bases as electron - pair donors.
redox reaction
Titration
Graham's Law
Lewis definition
20. 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
Phase diagram
Acid dissociation constant
Dispersion Forces
VSEPR
21. Chalcogens - - Oxide O
Water dissociation Constant
pH
Resonance structure
Group 6A
22. Sol - a chemical process in which solvent molecules and molecules or ions of the solute combine to form a compound
solvation
Titration
Dipole
Henderson Hasselbalch Equation
23. 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.
Activation energy
Reaction mechanism
Spin quantum number
Group 3A
24. 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
Percent composition
Electronegativity
mole
25. 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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26. The area of chemistry that is concerned with reaction rates and reaction mechanisms
Group 3A
Group 2A
Chemical Kinetics
periodic trends
27. 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
Solvent
Effective nuclear charge
single displacement reaction
28. 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
Titration
Octet Rule
Formal Charge
Common ion effect
29. An atom or group of atoms that has a positive or negative charge
redox reaction
Atomic absorption Spectra
Disproportionation
Ion
30. 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
Lewis definition
Half equivalence point
Theoretical yield
Neutralization reaction
31. A set of frequencies of electromagnetic waves given off by atoms of an element; consists of a series of fine lines of individual colors
Group 5A
empirical formula
atomic emission spectrum
amorphous solid
32. States that if a stress is applied to a system at equilibrium - the system shifts in the direction that relieves the stress.
Azeotrope
quantum
Le chateliers Principle
quanta
33. 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
Bronsted - Lowry definition
Group 7A
Amphoteric
Ion
34. Temperature is constant; effusion and temperature are proportional to the square root of their masses
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35. An ionic compound that resists changes in its pH
Buffer
Balmer series
azimuthal quantum number
Collision theory of chemical Kinetics
36. 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.
polymer
redox reaction
Henderson Hasselbalch Equation
Alkaline earths
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
molecule
Buffer
Azeotrope
Henry's Law
38. The amount of a substance that contains as many particles as there are atoms in exactly 12g of carbon -12
Bronsted - Lowry definition
subshell
mole
energy state
39. 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
periodic trends
Ionization energy
Solvent
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?
Net ionic equation
Common ion effect
Magnetic quantum number
Group 1A
41. 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
Activation energy
Dispersion Forces
Conjugate acids and Bases
single displacement reaction
42. 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.
Solute
Group 4A
crystalline solid
Diffusion
43. The number of atoms in exactly 12 g of pure 12c and equal to 6.022 x 10^23 is called
Group 5A
Electronegativity
Avagadros number
single displacement reaction
44. An emperimentally determined mathmatical expression showing the rate of a reaction as a function of the concentration of its reactants
Colligative properties
Covalent Bond
Rate law
Theoretical yield
45. A covalent bond in which the bonding electrons are shared equally by the bonded atoms - resulting in a balanced distribution of electrical charge
Nonpolar covalent bond
Lyman series
Triple point
Conjugate acids and Bases
46. Substance in which a solute is dissolved to form a solution
Group 5A
Bronsted Lowry
Solvent
azimuthal quantum number
47. The process by which one or more substances change to produce one or more different substances
chemical reaction
Group 1A
Henderson Hasselbalch Equation
atomic radius
48. 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
Phase diagram
Molecular orbital
bond length
The bohr model
49. Set of spectral lines appearing in the UV region when a hydrogen atom undergoes a transition from energy levels n>1 to n=1.
bond energy
Lyman series
heisenberg uncertainty principle
Rate law
50. Side - to side parallel orbitals overlap to share electrons - the 2nd/3rd covalent bond between two atoms - cannot rotate and maintain the bond.
STP
Magnetic quantum number
pi bonds
hydrogen bonding