Unit 4The Periodic Table

Chemistry IMr. Patel

SWHS

Topic Outline

• Continue Learning Major Ions• Organization of the Periodic Table (6.1)• Classification of Elements (6.1)• Tour of the Periodic Table (6.2)• Periodic Trends (6.3)

Organizing the PT

• Properties of elements are used to sort them• Mendeleev – 1st periodic table– Arranged elements based on

atomic mass– Made predictions of new

elements

Organizing the PT

• Modern periodic table arranges elements based on atomic number

• Periodic Law: repetition of physical and chemical properties

Metals

• Most elements • Good conductors, high luster, ductile,

malleable• Most are solid (except Hg)• Found left of stair-step

line

Nonmetals

• Contains the gaseous elements• Mostly gas, few solids at room temp• Poor conductors• Brittle• Found to right of

stair-step line

Metalloids/Semimetals

• Properties of metals and nonmetals– Based on physical conditions

• Found above andbelow stair-step line

Periodic Table

• Each block gives information about the element

• Groups – columns• Periods – rows• Representative Elements – Groups 1A to 7A

1H

1.008

2He

4.003

3Li

6.941

4Be

9.012

5B

10.81

6C

12.01

7N

14.01

8O

16.00

9F

19.00

10Ne

20.18

11Na

22.99

12Mg

24.30

13Al

26.98

14Si

28.09

15P

30.97

16S

32.07

17Cl

35.45

18Ar

39.95

19K

39.10

20Ca

40.08

21Sc

44.96

22Ti

47.88

23V

50.94

24Cr

52.00

25Mn

54.94

26Fe

55.85

27Co

58.93

28Ni

58.69

29Cu

63.55

30Zn

65.39

31Ga

69.72

32Ge

72.61

33As

74.92

34Se

78.96

35Br

79.90

36Kr

83.80

37Rb

85.47

38Sr

87.62

39Y

88.91

40Zr

91.22

41Nb

92.91

42Mo

95.94

43Tc

(98)

44Ru

101.1

45Rh

102.9

46Pd

106.4

47Ag

107.9

48Cd

112.4

43In

114.8

50Sn

118.7

51Sb

121.7

52Te

127.6

53I

126.9

54Xe

131.3

55Cs

132.9

56Ba

137.3

57La

138.9

72Hf

178.5

73Ta

180.9

74W

183.8

75Re

186.2

76Os

190.2

77Ir

192.2

78Pt

195.1

79Au

197.0

80Hg

200.6

81Tl

204.4

82Pb

207.2

83Bi

209.0

84Po

(209)

85At

(210)

86Rn

(222)

87Fr

(223)

88Ra

(226)

89Ac

227.0

104Rf

(261)

105Db

(262)

106Sg

(263)

107Ns

(264)

108Hs

(265)

109Mt

(268)

110Ds

(281)

111Rg

(272)

112Uub(285)

58Ce

140.1

59Pr

140.9

60Nd

144.2

61Pm

(145)

62Sm

150.4

63Eu

152.0

64Gd

157.2

65Tb

158.9

66Dy

162.5

67Ho

164.9

68Er

167.3

69Tm

168.9

70Yb

173.0

71Lu

175.0

90Th

232.0

91Pa

231.0

92U

238.0

93Np

(237)

94Pu

(244)

95Am

(243)

96Cm

(247)

97Bk

(247)

98Cf

(251)

99Es

(252)

100Fm

(257)

101Md

(258)

102No

(259)

103Lr

(260)

Atomic NumberElement symbolWeighted average atomic mass

63Eu

152.0 Groups

Groups

Groups

Perio

ds Periods

Group 1A

• Called the Alkali Metals• Elements: Li, Na, K, Rb, Cs,

Fr (largest atom)• Very reactive with air

and water• Form Bases (alkali)

Group 2A

• Called the Alkaline-Earth Metals• Elements: Be, Mg, Ca, Sr (pic), Ba, Ra• Abundant in Earth Crust• Reactive with water - bases

Group 7A

• Called Halogens• Elements: F, Cl, Br, I, At• Form salts

Group 8A

• Called Noble Gases• Elements: He, Ne, Ar, Kr (pic), Xe, Rn• Full electron shell• Not Reactive• Gases

The Middle Ones

• Elements between 2A and 3A• Transition metals – colors• Inner Transition metals at

bottom of Periodic Table – Synthetic /Radioactive

IA IIA IIIA IVA VA VIA VIIA VIIIA

IIIB IVB VB VIB VIIB VIIIB IB IIB

Alka

li m

etal

s

Alka

line

eart

h m

etal

s

Nob

le g

ases

Hal

ogen

s

Transition metals

Lanthanoids

Actinoids

Inner Transition metals

1

2

4

3

5

7

6

Groups

Perio

dsThe Periodic Table of Elements

Periodic Trends

• Based on the organization of PT, trends in atomic parameters exist– Atomic Size– Ionization Energy– Electronegativity

Atomic Size

• Atomic Radius – one half the distance between two nuclei when joined (same element)

Atomic Size Trend

Atomic Size

• Atomic size:– Increases down a column– Decreases across a period

Increasing Atomic Size

Incr

easi

ng A

tom

ic S

ize

Ionization Energy

• Ionization Energy (IE) – energy required to remove an electron from an atom

First Ionization Energy Trend

First Ionization Energy

• Ionization Energy:– Decreases down a column– Increases across a period

Increasing Ionization Energy

Incr

easi

ng IE

Electronegativity

• Electronegativity – ability of an atom to attract/pull electrons

Electronegativity Trend

Electronegativity

• Electronegativity:– Decreases down a column– Increases across a period

Increasing Electronegativity

Incr

easi

ng E

N

Trend SummaryAtomic Size

Ionization Energy Electronegativity

Which is the larger atom?

1. Be or F

2. Ca or Ba

3. Rb or Cl

4. Largest atom?

1. Be

2. Ba

3. Rb

4. Fr

Which has higher IE?

1. Be or F

2. Ca or Ba

3. Rb or Cl

1. F

2. Ca

3. Cl

Which has higher Electronegativity?

1. Be or F

2. Ca or Ba

3. Rb or Cl

4. Highest EN?

1. F

2. Ca

3. Cl

4. F