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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 area of chemistry that is concerned with reaction rates and reaction mechanisms
redox reaction
Chemical Kinetics
pH
Molality
2. The average distance between the nuclei of two bonded atoms
molecule
Percent yield
Molarity
bond length
3. Process by which molecules tend to move from an area where they are more concentrated to an area where they are less concentrated
solvation
Diffusion
Covalent Bond
Solvent
4. The ways in which electrons are arranged in various orbitals around the nuclei of atoms
amorphous solid
physical reaction
Phase diagram
electron configuration
5. Second quantum number - designated by the letter 'l.' This 'angular momentum' refers to the subshells within each principle quantum energy level. It can take on the value of an integer in the 0 to (n -1) range. The four subshellscorresponding to l=0
heisenberg uncertainty principle
Ion
azimuthal quantum number
Covalent Bond
6. E=hc/?
Hydrogen bonding
Molarity
Theoretical yield
electromagnetic energy of photons emmited from electrons at ground state
7. Chalcogens - - Oxide O
Octet Rule
Redox Half Reaction
Charles and Gay Lussac's Law
Group 6A
8. A reaction in which atoms of one element take the place of atoms of another element in a compound
Lewis structure
angular momentum in the bohr model
single displacement reaction
solvation
9. (chemistry) the sum of the relative atomic masses of the constituent atoms of a molecule
periodic trends
Network covalent
Proton
molecular weight
10. 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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11. At a constant pressure - the volume of an ideal gas is directly proportinal to its temperature: V (a) T
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12. The amount of product that can be made in a chemical reaction based on the amount of limiting reactant
Theoretical yield
Strong acid
Nonpolar covalent bond
Emperical Formula
13. 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.
Theoretical yield
Atomic absorption Spectra
Vapor pressure
Buffer
14. The formation of one or more covalent bonds between an electron pair donor and an electron pair acceptor
Balmer series
Lewis acid base reaction
Covalent Bond
Triple point
15. The Percent by mass of each element in a compound.
Percent composition
VSEPR
Principle quantum number
Neutralization reaction
16. An atom or group of atoms that has a positive or negative charge
Formula weight
Ion
Intermolecular forces
Dipole Dipole interaction
17. 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
Alkaline earths
Electronegativity
atomic radius
Group 7A
18. (chemistry) a substance that changes color to indicate the presence of some ion or substance
Neutron
Balmer series
Chemical Kinetics
indicator
19. 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.
Collision theory of chemical Kinetics
theoretical yield
Titration
Principle quantum number
20. 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
Lewis structure
Bronsted Lowry
Period
Spin quantum number
21. 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
Equilibrium
Half equivalence point
und's rule
Percent composition
22. Nh/2p The angular momentum changes only in discete amounts with respect to the quantum number. Also E=- R_h/n^2
Activation energy
Redox Half Reaction
angular momentum in the bohr model
Pauli exclusion principle
23. Having characteristics of both an acid and a base and capable of reacting as either
atomic radius
law of constant composition
theoretical yield
Amphoteric
24. Play- by- play showing the individual steps of a reaction - including the formation and destruction of any reaction intermediates that may occur.
Reaction mechanism
Vapor pressure
sigma bond
STP
25. A definite stable energy that a physical system can have
Arrhenius Definition
Group 7A
energy state
STP
26. Sum of all the masses - in AMU - present in one molecule of a molecular compound.
Formula weight
lathanide series
pi bonds
Le chateliers Principle
27. Theory stating that the rate of a reaction is directly proportional to the number of collisions that take place between reactants per second.
molecular weight
Net ionic equation
Collision theory of chemical Kinetics
Solution equilibrium
28. A graph of pressure versus temperature that shows the conditions under which the phases of a substance exist
Group 4A
Atomic weight
Phase diagram
lewis base
29. (physics) the smallest discrete quantity of some physical property that a system can possess (according to quantum theory) E=hf
Nucleus
Azeotrope
Resonance structure
quantum
30. A bond formed when two atomic orbitals combine to form a molecular orbital that is symmetrical around the axis connecting the two atomic nuclei
Common ion effect
Decomposition reaction
Rate law
sigma bond
31. An elementary particle with 0 charge and mass about equal to a proton
Solution equilibrium
redox reaction
Water dissociation Constant
Neutron
32. Attractive and repulsive forces between molecules that are weaker than forces within molecules.
electrolysis
Intermolecular forces
Mass number
Molality
33. 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
Ion dipole interactions
Phase diagram
Raoult's Law
s orbital
34. 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.
pH
Period
crystalline solid
The bohr model
35. Systematic pairing of a deprotonated species (base) with its protonated form (conjugate acid). Conjugates appear on opposite sides of a chemical equation.
Common ion effect
Effective nuclear charge
Conjugate acids and Bases
Electronegativity
36. The slowest elementary step which is the limit for the rate of the other steps
Balmer series
Magnetic quantum number
Rate determining step
Percent composition
37. Slightly less reactive than alkali metals - comprise group II
Collision theory of chemical Kinetics
Alkaline earths
Electrolyte
effective nuclear charge
38. Set of spectral lines appearing in the UV region when a hydrogen atom undergoes a transition from energy levels n>1 to n=1.
energy state
Lyman series
Ion product
Ion
39. The process by which a gas escapes from one container to another at lower pressure through a tiny hole in the container.
Lewis structure
Half equivalence point
Effusion
percent composition
40. Common definition of acids as proton (H+) donors and bases as proton acceptors
Normality
Equlibrium constant
law of constant composition
Bronsted - Lowry definition
41. Sum of the protons and neutrons in an element often denoted by the letter A
atomic theory
Atomic absorption Spectra
Ground state
Mass number
42. When dipoles are dissolved in a solution where ions are present ions wil arrange themselves with the opposite charged end of the dipole.
Colligative properties
Ion dipole interactions
Conjugate acids and Bases
Le chateliers Principle
43. 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
law of constant composition
Disproportionation
Half equivalence point
44. Alkali metals: highly reactive - therefore always compounds. - 1 valence electron +1 ion - Hydrogen H? - Lithium Li? - Sodium Na? - Potassium K? - Rubidium Rb? - Cesium Cs?
Dispersion Forces
Magnetic quantum number
Intermolecular forces
Group 1A
45. In a solution - the substance that dissolves in the solvent
The bohr model
Solute
Network covalent
crystalline solid
46. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance
periodic trends
Conjugate acids and Bases
decomposition reaction
Bronsted Lowry
47. Any sample of a given compound will contain the same elements in the identical mass ratio.
angular momentum in the bohr model
bond length
law of constant composition
Dipole Dipole interaction
48. Contains nonmetals that are non - reactive. Full outermost energy level except helium which has 2.
Noble gases
Disproportionation
Planck's Constant
Principle quantum number
49. Alkaline Earth Metals - 2 valence electrons +2 ions - Magnesium Mg
Group 2A
Group 3A
Electronegativity
Graham's Law
50. 5 different orbitals shaped like clover leaves and max electrons is 10
Covalent Bond
Resonance structure
d orbital
redox reaction