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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. 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.
Charles and Gay Lussac's Law
Atomic absorption Spectra
Henderson Hasselbalch Equation
Titration
2. Play- by- play showing the individual steps of a reaction - including the formation and destruction of any reaction intermediates that may occur.
Reaction mechanism
Chemical Kinetics
London forces
Lyman series
3. 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.
atomic emission spectrum
Group 3A
Ion product
Emperical Formula
4. Side - to side parallel orbitals overlap to share electrons - the 2nd/3rd covalent bond between two atoms - cannot rotate and maintain the bond.
d orbital
Solubility Product Constant
electromagnetic energy of photons emmited from electrons at ground state
pi bonds
5. 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.
Group 5A
VSEPR
bond energy
Percent yield
6. Contains nonmetals - 7 valence electrons in it's outermost energy level. Very reactive
percent composition
pi bonds
Halogens
Nonpolar covalent bond
7. 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.
energy state
Balmer series
Free radical
Rate law
8. A subdivision of an energy level in an atom. They are divided into orbitals.
Titration
d orbital
Ionic Bond
subshell
9. Product of the molar concentrations of dissociated ions in solution at any point in the reaction other than equilibrium or saturation - where each ion is raised to the power of its stoichiometric coefficient. Denoted IP.
Half equivalence point
redox reaction
Ion product
pi bonds
10. An emperimentally determined mathmatical expression showing the rate of a reaction as a function of the concentration of its reactants
STP
Molecular orbital
Rate law
Electrolyte
11. 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.
Balmer series
Free radical
Chemical Kinetics
crystalline solid
12. Systematic pairing of a deprotonated species (base) with its protonated form (conjugate acid). Conjugates appear on opposite sides of a chemical equation.
gram equivalent weight
Neutron
Solvent
Conjugate acids and Bases
13. 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
Solvent
Formal Charge
Lyman series
Normality
14. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
Common ion effect
redox reaction
Group 4A
Graham's Law
15. The maximum amount of product that can be produced from a given amount of reactant
theoretical yield
Ion
Group 7A
pI
16. (chemistry) a series from actinium to lawrencium of 15 radioactive elements with increasing atomic numbers
redox reaction
Solution equilibrium
actinide series
Nonpolar covalent bond
17. The percent by mass of each element in a compound
Effective nuclear charge
solvation
percent composition
Half equivalence point
18. The number of atoms in exactly 12 g of pure 12c and equal to 6.022 x 10^23 is called
Avagadros number
STP
Group 5A
Theoretical yield
19. Common definition of acids as proton (H+) donors and bases as proton acceptors
Bronsted - Lowry definition
Alkaline earths
Acid dissociation constant
Ion
20. 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
Lyman series
angular momentum in the bohr model
Strong acid
21. Any sample of a given compound will contain the same elements in the identical mass ratio.
Atomic absorption Spectra
Colligative properties
law of constant composition
Combination Reaction
22. An uncharged molecule with a single unpaitred electron in its outer ring - very unstable - exists for only about 10 seconds
Bronsted Lowry
Free radical
gram equivalent weight
Solubility Product Constant
23. Having characteristics of both an acid and a base and capable of reacting as either
Amphoteric
Rydberg constant
Nonpolar covalent bond
Period
24. The slowest elementary step which is the limit for the rate of the other steps
Half equivalence point
pi bonds
Rate determining step
mole
25. Substance in which a solute is dissolved to form a solution
Lewis structure
Solvent
Rydberg constant
Mass number
26. The reaction of the ions that characterize acids and the ions that characterize bases to form water molecules and a salt
Titration
Neutralization reaction
The bohr model
pi bonds
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
heisenberg uncertainty principle
theoretical yield
London forces
s orbital
28. 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
azimuthal quantum number
s orbital
angular momentum in the bohr model
Group 7A
29. A chemical formula showing the ratio of elements in a compound rather than the total number of atoms
energy state
Concentration
empirical formula
Buffer
30. When dipoles are dissolved in a solution where ions are present ions wil arrange themselves with the opposite charged end of the dipole.
quantum numbers
Ion dipole interactions
Half equivalence point
Molecular orbital
31. A horizontal row of elements in the periodic table
Period
Neutralization reaction
Atomic absorption Spectra
Nucleus
32. The weight in grams of compound that can be substituted by 1 atom of Hydrogen. GEW = MW / # of acidic Hyrdogens
Spin quantum number
gram equivalent weight
Henderson Hasselbalch Equation
Equlibrium constant
33. Contains nonmetals that are non - reactive. Full outermost energy level except helium which has 2.
azimuthal quantum number
Arrhenius Definition
Noble gases
Buffer
34. A concentration unit of a solution expressed as moles of solute dissolved per liter of solution
Molarity
Decomposition reaction
hydrogen bonding
Disproportionation
35. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds
azimuthal quantum number
Group 4A
Diprotic Base
Ionic Bond
36. (chemistry) any theory in which all matter is composed of tiny discrete finite indivisible indestructible particles
atomic theory
azimuthal quantum number
Triple point
molecule
37. The process of decomposing a chemical compound by the passage of an electric current.
Reaction mechanism
pi bonds
electrolysis
Ion dipole interactions
38. The point on a phase diagram that represents the only set of conditions at which all three phases exist in equilibrium with one another
Equilibrium
periodic trends
Diprotic Base
Triple point
39. A model of acids and bases which an acid is hydrogen ion donor and base is a hydrogen ion acceptor.
Octet Rule
lathanide series
Bronsted Lowry
Rydberg constant
40. A covalent bond in which the bonding electrons are shared equally by the bonded atoms - resulting in a balanced distribution of electrical charge
atomic theory
Nonpolar covalent bond
Neutron
molecular weight
41. Large molecular structures - strong covalent bonding - share qualities of IONIC And COVALENT
Network covalent
Emperical Formula
Covalent Bond
Colligative properties
42. 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
Raoult's Law
Half equivalence point
Planck's Constant
redox reaction
43. Two or more atoms held together by covalent bonds
Molecular orbital
molecule
Balmer series
Network covalent
44. The Percent by mass of each element in a compound.
Percent composition
Group 3A
Hydrogen bonding
Colligative properties
45. 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
percent composition
Arrhenius Definition
Resonance structure
Spin quantum number
46. 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
redox reaction
Group 7A
Effusion
Covalent Bond
47. A bond formed when two atomic orbitals combine to form a molecular orbital that is symmetrical around the axis connecting the two atomic nuclei
redox reaction
Effective nuclear charge
Ion
sigma bond
48. 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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49. A solution in which water is the solvent
sigma bond
quantum
Aqueous Solution
Covalent Bond
50. An elementary particle with 0 charge and mass about equal to a proton
Reaction order
energy state
s orbital
Neutron