2. on the same graph, usi
he same graph using the following information, plot atomic number versus atomic radi
versity, electronegativity, and first ionization energy. draw a line graph by joining the points
hol draw a smooth curve. (20 comm
atomic number atomic radius
density
electronegativity first ionization energy
four lines
(nm)
(g/ml)
(kj/mol of atoms)
0.032
0.0899
2.1
1312
0.031
0.179
0
2372
0.123
0.534
1.0
520
0.09
1.85
1.5
899
0.082
2.34
2.0
801
0.077
2.26
2.5
1086
0.075
1.25
3.0
1402
0.073
1.43
3.5
1314
0.072
1.70
4.0
1681
10
0.071
0.900
o
2081
11
0.154
0.971
0.9
496
12
0.136
1.74
1.2
738
13
0.118
2.70
578
14
0.111
2.33
1.8
786
15
0.106
1.82
2.1
1012
16
0.102
2.07
2.5
1000
17
0.099
3.21
3.0
1251
18
0.098
1.78
1521
19
0.203
0.862
0.8
419
20
0.174
1.54
1.0
590
21
0.144
1.3
631
22
0.132
4.54
1.5
658
23
0.122
5.96
1.6
650
24
0.118
7.20
653
25
7.20
1.5
l
26
0.117
7.87
1.8
759
27
0.116
8.9
1.8
758
28
0.115
1.8
737
29
0.117
8.92
1.9
745
0.125
30
7.14
906
1.6
0.126
5.90
1.6
579
0.122
5.35
762
0.12
5.73
2.0
947
34
4.81 t
l
0.114
2.8
3.12
35
1140
1351
0.112
3.74
36
0
1.6
31
1.8
32
33

Start an single atom tab. observe the decay of polonium-211. after each decay, press the reset nucleus button to watch the process again. write a description of alpha decay for po-211

Astudent is given a sample of a blue copper sulfate hydrate. he weighs the sample in a dry covered porcelain crucible and got a mass of 23.875 g for the crucible, lid, and sample. the mass of the empty crucible and lid was found earlier to be 22.652 g. he then heats the crucible to expel the water of hydration, keeping the crucible at red heat for 10 minutes with the lid slightly ajar. on colling, he finds the mass of crucible, lid, and contents to be 23.403 g. the sample was changed in the process to very light clue anhydrous cuso4. if there are again 100.0 g of hydrate, how many grams of cuso4 are in it? how many moles of cuso4? (hint: molar mass of cuso4 = 159.6 g / mole. what per cent of the hydrate is cuso4? you may convert the mass of cuso4 to moles.)

Salicylic acid is a very important acid. it is used to synthesize the aspirin by treating with acetic anhydride. a 0.2015-g sample of salicylic acid was dissolved in a 100.00-ml volumetric flask, and the solution was diluted to the mark. a 10-ml aliquot of this solution was titrated with standard naoh (0.01130 + 0.2% n) to a phenolphthalein faint pink color end point at 19.81 ml. (a) (calculate the normality of the salicylic acid solution used in the titration. (b) assuming the salicylic acid is pure, what is the equivalent weight of the salicylic acid? practice problems for the final exam (continued) (c) (calculate the inherent error in the determination of the equivalent weight you calculated in part (b). use the following absolute errors in the equipment /glassware when calculating the inherent error. 5.00-ml pipet: + 0.02 ml 100-ml volumetric flask: + 0.08 ml analytical balance: + 0.2 mg 25-ml buret: + 0.03 ml