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Lab 0 Melting point Boiling Density Atomic (K) point (K) (g/mL) Element Number F 9 53 85 0.001553 Cl 17 172 239 0.002898 Br 35 266 332 3.1028 I 53 387 457 4.933

Radius (Å) 60 100 117 136

Ionization Energy (IE), (eV) 1681 1251 1140 1008

Electronegativity (EN) 4 3.2 3 2.7

Electron Affinity ((EA)kJ/mol) 328 kJ/mol 349 kJ/mol 324.6 kJ/mol 295.2 kJ/mol

Li Na K Rb Cs

3 11 19 37 55

454 371 337 312 302

1615 1156 1032 961 944

0.534 0.97 0.89 1.53 1.873

130 160 200 215 238

520 496 419 403 376

1 0.9 0.8 0.8 0.8

59.6 kJ/mol 52.8 kJ/mol 48.4 kJ/mol 46.9 kJ/mol 45.5 kJ/mol

Li Be B C N O F Ne

3 4 5 6 7 8 9 10

454 1560 2348

1615 2744 4273

0.534 1.85 2.34

63 54 53 24

77 90 85 27

0.001145 0.001308 0.001553 0.000825

130 99 84 75 71 64 60 62

520 900 801 1086 1402 1314 1681 2081

1 1.6 2 2.6 3 3.4 4

59.6 kJ/mol 0 kJ/mol 26.7 kJ/mol 153.9 kJ/mol 7 kJ/mol 141 kJ/mol 328 kJ/mol

K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As

19 20 21 22 23 24 25 26 27 28 29 30 31 32 33

337 1115 1814 1941 2183 2180 1519 1811 1768 1728 1358 693 303 1211 1090

1032 1757 3109 3560 3680 2944 2334 3134 3200 3186 2835 1180 2477 3106

0.89 1.54 2.99 4.506 6 7.15 7.3 7.87 8.86 8.9 8.96 7.134 5.91 5.323 5.75

200 174 159 148 144 130 129 124 118 117 122 120 123 120 120

419 590 633 659 651 653 717 762 760 737 745 906 579 762 944

0.8 1 1.4 1.5 1.6 1.7 1.6 1.8 1.9 1.9 1.9 1.7 1.8 2 2.2

48.4 kJ/mol 2.37 kJ/mol 18.1 kJ/mol 7.6 kJ/mol 50.6 kJ/mol 64.3 kJ/mol 0 kJ/mol 15.7 kJ/mol 63.7 kJ/mol 112 kJ/mol 118.4 kJ/mol 0 kJ/mol 28.9 kJ/mol 119 kJ/mol 78 kJ/mol

34 35 36

494 266 116

958 332 120

4.809 3.102 0.0034

118 117 116

941 1140

2.6 195 kJ/mol 3 324.6 kJ/mol 0 kJ/mol

2.) Radius vs. Atomic Number PERIOD 4 ELEMENTS

Radius (Å)

Se Br Kr

200

200 190 180 170 160 150 140 130 120 110 100 18

174 159

148 144

130

124 129

20

22

24

120

118 117

123

122 26

28

120

30

118 117 116 120

32

34

36

38

Atomic Number

2.) As the atomic number of the elements in period 4 increase, the atomic radius decreases. The reasoning for this is as the numbr of protons increases, the nuclear charge attracts the electrons more strongly. This pulls the electrons closer to the nucleus resulting in a smaller radius.

6.) Melting points/Boiling points of Alkali metals vs. Atomic number 1800 1600

1615

1400

1156

1200

1032

1000

961

944

312

302

800 600

454

371

400

337

200 0 0

5

10

15

20

25

30

35

40

45

50

55

60

Atomic Number Melting point (K) Boiling point (K)

Linear (Melting point (K)) Exponential (Boiling point (K))

6.) As the atomic number increases, both the melting and boiling points decrease. When alkali metals are melted, the metallic bond is weakened enough for the atoms to move more freely

and is broken completely when the boiling point is reached. The boiling point is much higher than the melting point because a higher amount of energy is required to break the chemical bonds.

9.) Density vs. Boiling Point of Halogens 500

457

450

Boiling point (K)

400

332

350 300

239

250 200 150

85

100

50 0 0

0.5

1

1.5

2

2.5

3

3.5

4

4.5

5

Density (g/mL)

9.) The boiling point of halogens increases as the density of the element increases. Although density increases as atomic number increases, the density has no clear trend. However, as you go down the group, the boiling point increases due to the increasing strength of Van der Waals forces.

10.) Electronegativity vs. Atomic Number Period 2 Elements 4.5

4

Electronegativity (EN)

4

3.4

3.5

3 2.6

3 2.5

2 1.6

2 1.5

1

1 0.5 0 2

0 3

4

5

6

7

8

9

10

11

Atomic Number

10.) As you go down Period 2, the electronegativity increases. As the atomic number increases and the radius decreases, there is more attraction of the nucleus towards electron cloud. The effective nuclear charge increases. There is a drop at Neon because it is a noble gas, and it has no electronegativity because it has a full octet and does not need to pull electrons....