Chapter 6: The Periodic Table and Periodic Law Flashcards
(146 cards)
1
Q
Actinium
A
Ac, Element 89, 227.0278 a.m.u.
2
Q
Aluminium
A
Al, Element 13, 26.98154 a.m.u.
3
Q
Americium
A
Am, Element 95, 243 a.m.u.
4
Q
Antimony
A
Sb, Element 51, 121.75 a.m.u.
5
Q
Argon
A
Ar, Element 18, 39.948 a.m.u.
6
Q
Arsenic
A
As, Element 33, 74.9216 a.m.u.
7
Q
Astatine
A
At, Element 85, 210 a.m.u.
8
Q
Barium
A
Ba, Element 56, 137.33 a.m.u.
9
Q
Berkelium
A
Bk, Element 97, 247 a.m.u.
10
Q
Beryllium
A
Be, Element 4, 9.01218 a.m.u.
11
Q
Bismuth
A
Bi, Element 83, 208.9804 a.m.u.
12
Q
Bohrium
A
Bh, Element 107, 270 a.m.u.
13
Q
Boron
A
B, Element 5, 10.811 a.m.u.
14
Q
Bromine
A
Br, Element 35, 79.904 a.m.u.
15
Q
Cadmium
A
Cd, Element 48, 112.41 a.m.u.
16
Q
Caesium
A
Cs, Element 55, 132.9054 a.m.u.
17
Q
Calcium
A
Ca, Element 20, 40.078 a.m.u.
18
Q
Californium
A
Cf, Element 98, 251 a.m.u.
19
Q
Carbon
A
C, Element 6, 12.011 a.m.u.
20
Q
Cerium
A
Ce, Element 58, 140.12 a.m.u.
21
Q
Chlorine
A
Cl, Element 17, 35.453 a.m.u.
22
Q
Chromium
A
Cr, Element 24, 51.9961 a.m.u.
23
Q
Cobalt
A
Co, Element 27, 58.9332 a.m.u.
24
Q
Copernicium
A
Cn, Element 112, 285 a.m.u.
25
Copper
Cu, Element 29, 63.546 a.m.u.
26
Ciruim
Cm, Element 96, 247 a.m.u.
27
Darmstadtium
Ds, Element 110, 281 a.m.u.
28
Dubnium
Db, Element 105, 268 a.m.u.
29
Dysprosium
Dy, Element 66, 162.50 a.m.u.
30
Einsteinium
Es, Element 99, 252 a.m.u.
31
Erbium
Er, Element 68, 167.26 a.m.u.
32
Europium
Eu, Element 63, 151.96 a.m.u.
33
Fermium
Fm, Element 100, 257 a.m.u.
34
Fluorine
F, Element 9, 18.998403 a.m.u.
35
Francium
Fr, Element 87, 223 a.m.u.
36
Gadolinium
Gd, Element 64, 157.25 a.m.u.
37
Gallium
Ga, Element 31, 69.723 a.m.u.
38
Germanium
Ge, Element 32, 72.59 a.m.u.
39
Gold
Au, Element 79, 196.9665 a.m.u.
40
Hafnium
Hf, Element 72, 178.49 a.m.u.
41
Hassium
Hs, Element 108, 261 a.m.u.
42
Helium
He, Element 2, 4.002602 a.m.u.
43
Holmium
Ho, Element 67, 164.9304 a.m.u.
44
Hydrogen
H, Element 1, 1.00794 a.m.u.
45
Indium
In, Element 49, 114.82 a.m.u.
46
Iodine
I, Element 53, 126.9045 a.m.u.
47
Iridium
Ir, Element 77, 192.22 a.m.u.
48
Iron
Fe, Element 26, 55.847 a.m.u.
49
Krypton
Kr, Element 36, 83.80 a.m.u.
50
Lanthanum
La, Element 57, 138.9055 a.m.u.
51
Lawrencium
Lr, Element 103, 262 a.m.u.
52
Lead
Pb, Element 82, 207.2 a.m.u.
53
Lithium
Li, Element 3, 6.941 a.m.u.
54
Lutetium
Lu, Element 71, 174.967 a.m.u.
55
Magnesium
Mg, Element 12, 24.305 a.m.u.
56
Manganese
Mn, Element 25, 54.9380 a.m.u.
57
Meiterium
Mt, Element 109, 278 a.m.u.
58
Mendelevium
Md, Element 101, 258 a.m.u.
59
Mercury
Hg, Element 80, 200.59 a.m.u.
60
Molybdenum
Mo, Element 42, 95.94 a.m.u.
61
Neodymium
Nd, Element 60, 144.24 a.m.u.
62
Neon
Ne, Element 10, 20.179 a.m.u.
63
Neptunium
Np, Element 93, 237.0482 a.m.u.
64
Nickel
Ni, Element 28, 58.69 a.m.u.
65
Niobium
Nb, Element 41, 92.9064 a.m.u.
66
Nitrogen
N, Element 7, 14.0067 a.m.u.
67
Nobelium
No, Element 102, 259 a.m.u.
68
Osmium
Os, Element 76, 190.2 a.m.u.
69
Oxygen
O, Element 8, 15.9994 a.m.u.
70
Palladium
Pd, Element 46, 106.42 a.m.u.
71
Phosphorous
P, Element 15, 30.97376 a.m.u.
72
Platinum
Pt, Element 78, 195.08 a.m.u.
73
Plutonium
Pu, Element 94, 244 a.m.u.
74
Polonium
Po, Element 84, 209 a.m.u.
75
Potassium
K, Element 19, 39.0983 a.m.u.
76
Praseodymium
Pr, Element 59, 140.9077 a.m.u.
77
Promethium
Pm, Element 61, 145 a.m.u.
78
Protactinium
Pa, Element 91, 231.0359 a.m.u.
79
Radium
Ra, Element 88, 226.0254 a.m.u.
80
Radon
Rn, Element 86, 222 a.m.u.
81
Rhenium
Re, Element 75, 186.207 a.m.u.
82
Rhodium
Rh, Element 45, 102.9055 a.m.u.
83
Roentgenium
Rg, Element 111, 280 a.m.u.
84
Rubidium
Rb, Element 37, 85.4678 a.m.u.
85
Ruthenium
Ru, Element 44, 101.07 a.m.u.
86
Rutherfordium
Rf, Element 104, 261.11 a.m.u.
87
Samarium
Sm, Element 62, 150.36 a.m.u.
88
Scandium
Sc, Element 21, 44.95591 a.m.u.
89
Seaborgium
Sg, Element 106, 271 a.m.u.
90
Selenium
Se, Element 34, 78.96 a.m.u.
91
Silicon
Si, Element 14, 28.0855 a.m.u.
92
Silver
Ag, Element 47, 107.8682 a.m.u.
93
Sodium
Na, Element 11, 22.98977 a.m.u.
94
Strontium
Sr, Element 38, 87.82 a.m.u.
95
Sulfur
S, Element 16, 32.066 a.m.u.
96
Tantalum
Ta, Element 73, 180.9479 a.m.u.
97
Technetium
Tc, Element 43, 98 a.m.u.
98
Tellurium
Te, Element 52, 127.60 a.m.u.
99
Terbium
Tb, Element 65, 158.9254 a.m.u.
100
Thallium
Tl, Element 81, 204.383 a.m.u.
101
Thorium
Th, Element 90, 232.0381 a.m.u.
102
Thulium
Tm, Element 69, 168.9342 a.m.u.
103
Tin
Sn, Element 50, 118.710 a.m.u.
104
Titanium
Ti, Element 22, 47.88 a.m.u.
105
Tungsten
W, Element 74, 183.85 a.m.u.
106
Uranium
U, Element 92, 238.0289 a.m.u.
107
Vanadium
V, Element 23, 50.9415 a.m.u.
108
Xenon
Xe, Element 54, 131.29 a.m.u.
109
Ytterbium
Yb, Element 70, 173.04 a.m.u.
110
Yttrium
Y, Element 39, 88.9059 a.m.u.
111
Zinc
Zn, Element 30, 65.39 a.m.u.
112
Zirconium
Zr, Element 40, 91.224 a.m.u.
113
Nihonium
Nh, Element 113, 286 a.m.u.
114
Flerovium
Fl, Element 114, 289 a.m.u.
115
Moscovium
Mc, Element 115, 289 a.m.u.
116
Livermorium
Lv, Element 116, 293 a.m.u.
117
Tennessine
Ts, Element 117, 294 a.m.u.
118
Oganesson
Og, Element 118, 294 a.m.u.
119
John Newlands (1837-1898)
Law of Octaves
120
Lothar Meyer (1830-1895)
Made a prototype periodic table
121
Dmitri Mendeleev (1834-1907)
Made a prototype periodic table; Created the Periodic Law; Predicted properties of undiscovered elements; "Father of Periodic Table"; Arranged elements by increasing mass and chemical property; Left spaces for elements not yet discovered; If arrangement by mass didn't match arrangement by property, he arranged by property
122
Henry Moseley (1887-1915)
Discovered atomic number
123
Periodic Law
The chemical and physical properties of the elements are a periodic function of atomic mass*.
*Mendeleev said mass; modern definition is number
124
Metals
Tend to form cations in aqueous solutions; tend to be lustrous, malleable, ductile, and good conductors of heat and electricity; tend to lose electrons in reactions; typically solids
125
Nonmetals
Tend to form anions in aqueous solutions; tend to be dull, brittle, and bad conductors of heat and electricity; tend to gain electrons in reactions; often gases
126
Metalloids
Staircase elements (B, Si, Ge, As, Sb, Te); Some characteristics of metals and some of nonmetals
127
Alkali Metals
Family 1; Soft, metallic solids; found only in compounds in nature; low densities and melting points; low ionization energies; most reactive
128
Alkaline Earth Metals
Family 2; Very reactive metals
129
Transition Metals
Families 3-12
130
Boron Family
Family 13
131
Carbon Family
Family 14
132
Pnictogens/Nitrogen Family
Family 15
133
Chalcogens/Oxygen Family
Family 16
134
Halogens
Family 17; Salt formers; Most reactive nonmetals
135
Noble Gases
Family 18; Generally inert
136
Inner Transition Metals
Lanthanides & Actinides
137
Periodic Trends
1. Atomic Radius
2. Ionic Radius
3. Ionization Energy
4. Electronegativity
5. Electron Affinity
138
Driving Forces For Periodic Trends
1. Stable octet (atoms are most stable with 8 electrons in outer electron layers)
2. Electron shielding (equal within the same family, added electron layers reduce attraction between the nucleus and valence shell)
3. Nuclear charge (equal within the same period, number of electron layers does not change, but number of protons in nucleus increases from left to right, increasing nuclear charge and nuclear attraction)
139
Atomic Radius
Distance from nucleus to outer valence shell; increases top to bottom - more electron layers; decreases left to right - charge pulls electrons closer to nucleus as more protons are added
140
Electronegativity
Tendency of one element to remove electrons from other elements; decreases top to bottom - nuclear charge decreases due to electron shielding; increases left to right - effective nuclear charge increases, but not atomic size
141
Third Ionization Energy
Amount of energy needed to remove one mole of electrons from one mole of 2+ ions of the gas of the element; decreases top to bottom - electron shielding means easier to remove electrons; increases left to right - more energy to remove electrons from stable atoms (first 2 take more because removing electrons from stable octets)
142
Electron Affinity
Energy released when an electron is added to atom; decreases top to bottom - electron shielding; increases left to right - increasing nuclear charge
143
Principal Oxidation State
Typical charge of an ion of that element; increases to group 14, decreases to end; no top to bottom trend
144
First Ionization Energy
Energy required to remove highest electron from neutral atom; decreases top to bottom - electron shielding; increases left to right - increasing nuclear charge
145
Melting Point
Point at which element changes from solid to liquid; Metals - high melting point = metallic bonding; Metalloids - network solid = extremely high melting point; Nonmetals - lowest melting point = covalent bonding; lower melting points left to right - nonmetal bonds weaker
146
Second Ionization Energy
Energy needed to remove second electron after 1 electron already removed; decreases top to bottom - electron shielding; increases left to right - increasing nuclear charge (first group larger)
