CHE2A Worksheet 5A PDF

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Worksheet 5A from CHE2A 2020W....

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Week 5A Worksheet Review: What is Periodic Law? Questions: 1. Which is a. The smallest atom in group 13?

b. The smallest of the following atoms: Te, In, Sr, Po, Sb?

c. Why?

2. Can two ions be isoelectronic (isoelectronic means they have the same number of electrons) without having noble-gas configurations?

3. The following species are isoelectronic with the noble gas Kr. Arrange them in order of increasing radius: Rb+, Y3+, Se2-, Br-, Sr2+

4. Compare the elements Na, O, Mg and P. Place the elements in order of increasing ionization energy.

5. Electron affinities can be negative, positive, or neutral. However, this is not the case with ionization energies. Why? (Hint: Think about what process is occurring in each.)

6. Which comparison of ionization energies is correct? A) Cs > Na B) Na > Mg C) Ca > Mg D) Ca+ > Ca E) Ar > He 7. Which of the following would you expect to be diamagnetic and which paramagnetic? a. K+ b. Cr3+ c. Zn2+ d. Cd e. Co3+ f. Sn2+ g. Br

8. Chlorine has a large negative electron affinity. Therefore, chlorine is most likely to: A) act as an oxidizing agent B) have a small first ionization energy C) act as a reducing agent D) form a basic oxide E) release electrons readily to other atoms

The following two pages contain conversions, constants, equations, and a periodic table which may be useful to you. You may remove them for easy access. Conversions: 1010 Å = 1 m = 1012 pm = 100 cm

1 atm = 760 Torr = 760 mmHg = 101,325 Pa 1.00 in = 2.54 cm

1 cm3 = 1 mL

101.325 J = 1 L atm

1 lb = 453.6 g

1 cal = 4.184 J

1 gal = 3.785 L

T(K) = t(°C) + 273.15

t(°F) =9/5 t(°C) + 32

Constants: c = 2.9979 x 108 m / s

R = 8.3145 J / mol K = 0.08206 L atm / mol K

NA = 6.022 x 1023 mol–1

h = 6.626 x 10–34 J s

g = 9.81 m / s

d (H2O) = 1.00 g / cm3

m(electron) = 9.109 x 10–31 kg

RH = 2.178 x 10–18 J

m(proton) = 1.673x10-27 kg

Equations:

n = m/M

d=

m V

M=

n V

P = dhg

E = h

=

c

=

h h = p mu

PV = nRT

urm s = u 2 =



 n 2a   P + 2  (V − nb ) = nRT V  

3RT M

Ptotal =  Pi

xp 

i

h 4

En = - Z2RH/n2

PiVi/Ti = PfVf/Tf

Zeff = Z − S

ΔE = Z2RH(1/ni2 – 1/nf2)

d = P(MM)/(RT)

ΧA = nA/ntotal

KE = ½mu2 = 3/2RT

rateA/rateB = (MMB/MMA)1/2

φ = hν

KE = hν – φ

tB/tA = (MMB/MMA)1/2

λ = h/p

p = mu

Ѱn(x) = (2/L)1/2sin(nπx/L)

P1/T1 = P2/T2

M1V1 = M2V2

V1/T1 = V2/T2

P1V1 = P2V2

Solubility Rules: 1. Salts of group 1 cations (with some exceptions for Li+) and the NH4+ cation are soluble 2. Nitrates, acetates, and perchlorates are soluble 3. Salts of silver, lead, and mercury(I) are insoluble 4. Chlorides, bromides, and iodides are soluble 5. Carbonates, phosphates, sulfides, oxides, and hydroxides are insoluble (sulfides of group 2 cations and hydroxides of Ca2+, Sr2+, and Ba2+ are slightly soluble) 6. Sulfates are soluble except for those of calcium, strontium, and barium PERIODIC TABLE Key

1

2

Atomic Number Symbol Atomic Mass Electronegativity

H

He

1.008 2.20 3

4

5

6

7

8

Li

Be

B

C

N

O

F

Ne

6.941 0.98

9.012 1.57

10.81 2.04

12.01 2.55

14.01 3.04

16.00 3.44

19.00 3.98

20.18 -

9

4.003 10

11

12

13

14

15

16

17

18

Na

Mg

Al

Si

P

S

Cl

Ar

22.99 0.93

24.31 1.31

26.98 1.61

28.09 1.90

30.97 2.19

32.06 2.58

35.45 3.16

39.95 36

19

20

21

22

23

24

25

26

27

28

29

30

31

32

33

34

35

K

Ca

Sc

Ti

V

Cr

Mn

Fe

Co

Ni

Cu

Zn

Ga

Ge

As

Se

Br

Kr

39.10 0.82

40.08 1.00

44.96 1.36

47.90 1.54

50.94 1.63

52.00 1.66

54.94 1.55

55.85 1.83

58.93 1.88

58.70 1.91

63.55 1.90

65.38 1.65

69.72 1.81

72.59 2.01

74.92 2.18

78.96 2.55

79.90 2.96

83.80 -

37

38

39

40

41

42

43

44

45

46

47

48

49

50

51

52

53

54

Rb

Sr

Y

Zr

Nb

Mo

Tc

Ru

Rh

Pd

Ag

Cd

In

Sn

Sb

Te

I

Xe

85.47 0.82

87.62 0.95

88.91 1.22

91.22 1.33

92.91 1.6

95.94 2.16

(98) 1.9

101.1 2.2

102.9 2.28

106.4 2.20

107.9 1.93

112.4 1.69

114.8 1.78

118.7 1.96

121.8 2.05

127.6 2.1

126.9 2.66

131.3 -

55

56

71

72

73

74

75

76

77

78

79

80

81

82

83

84

85

86

Cs

Ba

Lu

Hf

Ta

W

Re

Os

Ir

Pt

Au

Hg

Tl

Pb

Bi

Po

At

Rn

132.9 0.79 87

137.3 0.89 88

175.0 1.27 103

178.5 1.3 104

180.9 1.5 105

183.9 2.36 106

186.2 1.9 107

190.2 2.2 -

192.2 2.20 109

195.1 2.28

197.0 2.54

200.6 2.00

204.4 2.04

207.2 2.33

209.0 2.02

(209) 2.0

(210) 2.2

(222) -

Fr

Ra

Lr

Unq

Unp

Unh

Uns

(223) 0.7

(226) 0.9

(260) -

-

-

-

-

Une

57

58

59

60

61

62

63

64

65

66

67

68

69

70

La

Ce

Pr

Nd

Pm

Sm

Eu

Gd

Tb

Dy

Ho

Er

Tm

Yb

138.9 1.10

140.1 1.12

140.9 1.13

144.2 1.14

(145) 1.13

150.4 1.17

152.0 1.2

157.3 1.20

158.9 1.2

162.5 1.22

164.9 1.23

167.3 1.24

168.9 1.25

173.0 1.1 102

-

89

90

91

92

93

94

95

96

97

98

99

100

101

Ac

Th

Pa

U

Np

Pu

Am

Cm

Bk

Cf

Es

Fm

Md

No

(227) 1.1

232.0 1.3

(231) 1.5

238.0 1.38

(237) 1.36

(244) 1.28

(243) 1.3

(247) 1.3

(247) 1.3

(251) 1.3

(252) 1.3

(257) 1.3

(258) 1.3

(259) 1.3...