Gifted Review Part 2 Final Exam Fall 2012
48. Balance the following reaction and write the ionic and next ionic equations:
Lead (II) nitrate solution reacts with lithium chloride solution to produce solid lead (II) chloride and lithium nitrate solution
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57.
Compare atomic versus ionic radii for cations and anions and their corresponding atoms.
What are the characteristics of alpha, beta and gamma radiation and what effect does each have on an element?
What is half life?
An isotope of cesium-137 has a half life of 30 years. If 1.0 g of cesium-137 disintegrates over a period of 90 years, how many grams
of cesium-137 would remain?
Name groups IA, IIA, VIIA and VIIIA in the periodic table.
Explain how atoms become anions or cations and what noble gas configuration do the ions resemble?
State the law of conservation of matter. Does it hold true for chemical reactions? Nuclear reactions?
Define mass and density.
What are the molecular shapes for molecules with central atoms with:
2 domains, 3 domains, 4 domains/no lone pairs, 4 domains/1 lone pair, 4 domains/2 lone pairs, 5 domains and 6 domains.
58. Write the following numbers in scientific notation:
0.000347, 229000000, 2, 473000.
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64.
What are the properties of ionic versus covalent compounds?
What shapes and s orbitals and p orbitals?
What determines the reactivity of elements?
List the 7 diatomic elements?
Identify s, p, d, f blocks and metal, non-metal, metalloids in the periodic table.
What are alkanes, alkenes and alkynes and what are the prefixes for hydrocarbons with 1 carbon, 2 carbons, 3 carbons, to 10
carbons.
65. How do you differentiate the name of compounds with elements with multiple oxidation states such as Fe +2 and Fe+3 and Cu+1 and
Cu+2?
66. How many electrons are held by:
Levels 1, 2, 3, 4, 5 (how do you calculate?) and orbitals s, p, d, f
67. Quantum numbers questions
Which of the following sets of quantum numbers are not allowed? For the sets of quantum numbers that are incorrect, indicate
what is wrong in each set.
(a) n = 2, l = 1, ml = -1
--allowed
--not allowed, n is not valid
--not allowed, l is not valid
--not allowed, ml is not valid
(b) n = 1, l = 1, ml = 0
--allowed
--not allowed, n is not valid
--not allowed, l is not valid
--not allowed, ml is not valid
(c) n = 8, l = 7, ml = -6
--allowed
--not allowed, n is not valid
--not allowed, l is not valid
--not allowed, ml is not valid
(d) n = 1, l = 0, ml = 2
--allowed
--not allowed, n is not valid
--not allowed, l is not valid
--not allowed, ml is not valid
48. 1 Pb(NO3)2 + 2 LiCl 1 PbCl2 + 2 LiNO3
49. cations: ionic radius is smaller than atomic radius because lost electrons
Anions: ionic radius is larger than atomic radius because gained electrons
50. Alpha= 42𝐻𝑒 = weakest; decreases mass by 4, decreases atomic number by 2
Beta = −10𝛽 = middle strength; no change to mass, increases atomic number by 1
Gamma = 00𝛾 = strongest; no change to mass nor atomic number
51. Half life = the time it takes for ½ of radioactive nuclei to decay
52. 0.125 g
53. IA = alkali metals, IIA = alkaline earth metals, VII A= halogens, VIIIA = noble gases
54. Cations = lose electrons therefore noble gas notation looks like previous noble gas (Na+1 configuration would be
the same as Ne)
Antions = gain electrons therefore noble gas notation looks like noble gas ahead (F-1 configuration would be the
same as Ar)
55. Law of Conservation = mass/matter can not be created nor destroyed, yes, yes
56. Mass = measurement of matter; density = mass/volume
57. 2 areas = linear; 3 areas = trigonal planar; 4 areas with 0 lone pairs = tetrahedral; 4 areas with 1 lone pair =
pyramidal; 4 areas with 2 lone pairs = bent
58. 3.74 x 10-4, 2.29 x 108, 4.73 x 105
59. Ionic = form strong crystals, high melting points, form electrolytes in solutions, bond between metal and nonmetal, electrons are transferred
Covalent = lower melting points, bonds between non-metals, polar covalent= un-equal sharing of electrons, nonpolar covalent = equal sharing of electrons
60. S = sphere with one orientation; p = dumbbell with 3 orientations
61. Reactivity is based on the number of valence electrons. Think octet rule….so elements with 1 or 7 valence
electrons are very reactive
62. Hydrogen, nitrogen, oxygen, fluorine, chlorine, bromine, iodine
63. S block = alkali metals & alkaline earth metals; p-block = group IIIA down and to the right; d-block = transition
metals; f-block = 2 rows on the bottom
Metals = to the left of stair steps; metalloids= on stair step; non-metals = to right of stair step + hydrogen
64. Alkanes = hydrocarbons with single bonds between carbons; alkenes = hydrocarbons with double bonds
between carbons; alkynes= hydrocarbons with triple bonds between carbons
Methane, ethane, propane, butane, pentane, hexane, heptanes, octane, nonane, decane
65. Use roman numerals to represent the charges
66. Use 2n2. Level 1 = 2, level 2 = 8, level 3 = 18, level 4 = 32, level 5 = 50
S orbital holds 2 electrons max; p orbitals hold 6 electrons max; d orbitals hold 10 electrons max; f orbitals hold
14 electrons max
67. (a) allowed, (b) not allowed, l is not valid (no 1p ortbial), (c) not allowed, ml is not valid (ml ranges from –l to +l),
(d) not allowed, mL is not valid