Lab 0. Periodic Trends PDF

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Lab report for lab 0.Periodic Trends...

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Lab 0. Periodic Trends Sanisha Lama 09/05/2021 Data Table: Element

F

Atomic number

Melting point (C)

melting point (K)

boiling point (C)

boiling point (K)

Density (g/mL)

Radius (A)

Ionization Energy (IE)(eV)

Electronegativity (EN)

Electron Affinity ((EA) kJ/mol)

9

-219.62

53.53

-188.14

85.01

0.00169

0.64

17.42282

4

328.164

Cl

17

-100.98

172.17

-33.97

239.18

0.00321

0.99

12.96764

3

348.575

Br

35

-7.3

265.85

58.78

331.93

3.12

1.14

11.81381

2.8

324.536

I

53

113.5

386.65

184.35

457.5

4.93

1.33

10.45126

2.5

295.153

Ts

117

522.73

795.88

610

883

7.1

At

85

302

575.15

337

610.15

Na

11

97.81

370.96

882.9

1156.05

K

19

63.65

336.8

774

1047.15

Rb

37

39

312.15

668

Fr

87

27

300.15

Cs

55

28.4

Be

4

B

5

C N

-

-

7.7

-

165.9

1.45

-

2.2

233.087

0.97

1.86

5.13908

0.9

52.867

0.86

2.31

4.34066

0.8

48.383

941.15

1.53

2.44

4.17713

0.8

46.884

677

950.15

2.4

2.7

4.0727

0.7

46.89

301.55

678.4

951.55

1.88

2.62

3.8939

0.7

45.505

1278

1551.15

2970

3243.15

1.85

1.11

9.3227

1.5

-48

2300

2573.15

3658

3931.15

2.34

0.88

8.29803

2

26.989

6

3527

3800.15

4827

5100.15

3.51

0.77

11.2603

2.5

121.776

7

-209.86

63.29

-195.8

77.35

0.00125

0.7

14.53414

3

121.775

Li

3

180.54

453.69

1347

1620.15

0.53

1.52

5.39172

1

59.632

O

8

-214.8

58.35

-182.96

90.19

0.00143

0.66

13.61806

3.5

140.976

F

9

-219.62

53.53

-188.14

85.01

0.00169

0.64

17.42282

4

328.164

Ca

20

839

1112.15

1484

1757.15

1.54

1.97

6.11316

Ne

10

-248.67

24.48

-246.05

27.1

0.0009

1.6

21.5646

1

Sc

21

1541

1814.15

2831

3104.15

3

1.44

6.5615

1.3

18

Ti

22

1660

1933.15

3287

3560.15

4.5

1.32

6.8281

1.5

7.289

V

23

1887

2160.15

3377

3650.15

6

1.22

6.7462

1.5

50.911

Cr

24

1857

2130.15

2672

2945.15

7.2

1.18

6.7665

1.6

65.21

Mn

25

1244

1517.15

1962

2235.15

7.2

1.17

7.43402

1.5

-50

Fe

26

1535

1808.15

2750

3023.15

7.9

1.17

7.9024

1.8

14.785

Co

27

1495

1768.15

2870

3143.15

8.9

1.16

7.6398

1.8

63.898

Ni

28

1453

1726.15

2732

3005.15

8.9

1.15

7.881

1.8

111.65

Cu

29

1083.4

1356.55

2567

2840.15

8.9

1.17

7.72638

1.9

119.235

Zn

30

419.58

692.73

907

1180.15

7.1

1.25

9.3942

1.6

-58

Ga

31

29.76

302.91

2204

2477.15

5.9

1.22

6

1.8

29.061

Ge

32

938.3

1211.45

2820

3093.15

5.3

1.22

7.9

2.01

118.935

As

33

817

1090.15

614

887.15

5.72

1.21

9.79

2.18

77.65

Se

34

221

494.15

685

958.15

4.81

1.17

9.75

2.55

194.958

Kr

36

-157.36

115.79

-153.22

119.93

3.75

2.0

14

3

-96

-

2.37 -116

1. electronegativity of halogens vs. atomic number

Figure 1. Electronegativity of halogens decreases as the atomic number increases. The atomic radius of the atom of each atom increases because more shells is added as we go down the group. This results in less attraction between the positive nucleus and the outer electrons.

2. Melting points and boiling points of the alkali metals vs. atomic number

Figure 2. Both the melting point and boiling point decreases as the atomic number increases. When any of the alkali metal in group 1 is melted, the metallic bond is weakened which is enough for the atoms to move around more freely, and it is completely broken when boiling point is reached. The decrease in the melting and boiling point is hence seen when there is decrease in the strength of each metallic bond.

3. Electronegativity of period 2 elements vs. atomic number

Figure 3. Electronegativity of period 2 elements increases as the atomic number increases. It is because as we move across the period from left to right, the number of protons in the nucleus also increases. And these positively charged proton attracts negatively charge electrons and hence the electronegativity also increases.

4. Density of Halogen vs. boiling point

Figure 4. The boiling point of the halogen increases as the density of the element increases. In the graph we can see that the higher the boiling point, the higher the density. It is because as the density increases the energy required to break the intermolecular forces also increases and the boiling point represents the amount needed to break those intermolecular forces from a solid to liquid....