Periodic Table of Element

Mrs. Clendenon

The Periodic TableName as many things as you can about what you remember about the periodic table of

elements

1IA

18VIIIA

11H

1.00797

2IIA

Periodic Table 13IIIA

14IVA

15VA

16VIA

17VIIA

2He

4.0026

23

Li6.939

4Be

9.0122

5B

10.811

6C

12.0112

7N

14.0067

8O

15.9994

9F

18.9984

10Ne

20.179

311

Na22.9898

12Mg24.305

3IIIB

4IVB

5VB

6VIB

7VIIB

8 9VIIIB

10 11IB

12IIB

13Al

26.9815

14Si

28.086

15P

30.9738

16S

32.064

17Cl

35.453

18Ar

39.948

419K

39.102

20Ca40.08

21Sc

44.956

22Ti

47.90

23V

50.942

24Cr

51.996

25Mn

54.9380

26Fe

55.847

27Co

58.9332

28Ni58.71

29Cu63.54

30Zn65.37

31Ga65.37

32Ge72.59

33As

74.9216

34Se78.96

35Br

79.909

36Kr83.80

537

Rb85.47

38Sr87.62

39Y

88.905

40Zr91.22

41Nb

92.906

42Mo95.94

43Tc[99]

44Ru

101.07

45Rh

102.905

46Pd106.4

47Ag

107.870

48Cd

112.40

49In

114.82

50Sn

118.69

51Sb

121.75

52Te

127.60

53I

126.904

54Xe

131.30

655Cs

132.905

56Ba

137.34

57La

138.91

72Hf

178.49

73Ta

180.948

74W

183.85

75Re186.2

76Os190.2

77Ir

192.2

78Pt

195.09

79Au

196.967

80Hg200.59

81Tl

204.37

82Pb

207.19

83Bi

208.980

84Po[210]

85At[210]

86Rn[222]

787Fr[223]

88Ra[226]

89Ac[227]

104Ku[260]

105 106 107 108 109http://www.chemsoc.org/viselements/pages/periodic_table.html

Periodic Table: It is arranged by metals, nonmetals and metalloids

1IA

18VIIIA

12

IIA13

IIIA14

IVA15VA

16VIA

17VIIA

2

33

IIIB4

IVB5

VB6

VIB7

VIIB8 9

VIIIB10 11

IB12IIB

4

5

6

7

MetalsMetals

Metalloids

NonmetalsNonmetals

Metals How would you describe metals?

Metals are lustrous (shiny), malleable, ductile, and are good conductors of heat and electricity.

They are mostly solids at room temp.

Nonmetals – How would you describe these?

Nonmetals are the opposite.

They are dull, brittle, nonconductors (insulators).

Some are solid, but many are gases, and Bromine is a liquid.

Metalloids – How would you describe these?

Metalloids, aka semi-metals are just that.

They have characteristics of both metals and nonmetals.

They are shiny but brittle.

And they are semiconductors.

Across the Periodic Table

Elements are arranged horizontally across the periodic table (rows 1-7), what is

this arrangement called?

PeriodsPeriods

These elements have the same number of valence shells. How many shells are in

period 2? 6?

Period 2 would have two shells, while period 6 would have 6.Period 2 would have two shells, while period 6 would have 6.

1IA

18VIIIA

12

IIA13

IIIA14

IVA15VA

16VIA

17VIIA

2

33

IIIB4

IVB5

VB6

VIB7

VIIB8 9

VIIIB10 11

IB12IIB

4

5

6

7

2nd Period

6th Period

Down the Periodic Table Elements are arranged vertically down the periodic table (columns or group, 1- 18 or 1-8 A,B), what Elements are arranged vertically down the periodic table (columns or group, 1- 18 or 1-8 A,B), what are they called? are they called?

Family/Groups Family/Groups What do these elements have in common? What do these elements have in common?

Same number of valence electrons.Same number of valence electrons.

1IA

18VIIIA

12

IIA13

IIIA14

IVA15VA

16VIA

17VIIA

2

33

IIIB4

IVB5

VB6

VIB7

VIIB8 9

VIIIB10 11

IB12IIB

4

5

6

7

Alkali Family: 1 e- in the valence shell

Alkali Family: 1 e- in the valence shell

Halogen Family: 7 e- in the valence shell

Halogen Family: 7 e- in the valence shell

The roman numerals represent the number of valence electrons each family have.

How many valence electrons are in the Alkali Earth Family?

1IA

18VIIIA

12

IIA13

IIIA14

IVA15VA

16VIA

17VIIA

2

33

IIIB4

IVB5

VB6

VIB7

VIIB8 9

VIIIB10 11

IB12IIB

4

5

6

7

Alkali Family: Alkali Family:

Halogen Family: Halogen Family:

1 valence electron

1s1

1s22s1

1s22s22p63s1

1s22s22p63s23p64s1

1s22s22p63s23p64s23d104p65s1

1s22s22p63s23p64s23d104p65s24d10 5p66s1

1s22s22p63s23p64s23d104p65s24d105p66s2

4f145d106p67s1

H1

Li3

Na11

K19

Rb37

Cs55

Fr87

Do you notice any similarity in these configurations of the alkali metals?

They all have 1 valence electron

Valence electrons for ElementsValence electrons for ElementsRecall that the valence electrons for the elements Recall that the valence electrons for the elements can be determined based on the elements position can be determined based on the elements position on the periodic table. This is based on the on the periodic table. This is based on the family/group they are found infamily/group they are found in

Infamous Families of the Periodic Table

Name all 6 families.

1IA

18VIIIA

12

IIA13

IIIA14

IVA15VA

16VIA

17VIIA

2

33

IIIB4

IVB5

VB6

VIB7

VIIB8 9

VIIIB10 11

IB12IIB

4

5

6

7

Alkali

Alkaline (earth)

Transition MetalsTransition Metals

Noble GasNoble GasHalogenHalogen

HalogensHalogens

Trend in Atomic Radius

Atomic Radius: Atomic Radius:

The size of at atomic radius decrease the closer the element are to the noble gases (to the right).

The atomic radius increases as the elements increase in the number of periods (moving down).

Which atom is larger in size? K or Kr? ___________

K In or Rb ? ________

Rb

Periodic Table: electron behaviorThe periodic table can be classified by the behavior of their electrons

1IA

18VIIIA

12

IIA13

IIIA14

IVA15VA

16VIA

17VIIA

2

33

IIIB4

IVB5

VB6

VIB7

VIIB8 9

VIIIB10 11

IB12IIB

4

5

6

7

METALS METALLOID NON-METALS Alkali

Alkaline Transition

Noble gas Halogens Halogens

These elements tend to give up

e- and form CATIONS become +

These elements will give up e- or accept e-

These elements tend to accept e- and form ANIONS

become negative

Trends in Atomic and Ionic Size

152

186

227

Li

Na

K

60

Li+

95

Na+

133

K+

e

e

e

F1-

136

Cl1-

181

Br-1-

195

F

Cl

Br

64

99

114

e

e

e

Metals NonmetalsGroup 1

Al

143

50

ee

e

Group 13 Group 17

Cations are smaller than parent atoms Anions are larger than parent atoms

Al3+

Trend in Electronegativity

Electronegativity: Electronegativity: •Electronegativity is a measure of an atom’s attraction for another atom’s electrons.•Elements with a high electronegatvity (EN) means it pulls the electron towards itself strongly! •Metals are electron givers and have low EN while nonmetals are electron takers and have high EN.

•What about the noble gases?•They have no EN because they have a full outer electron orbital

Electronegativity

F

Cs

Which element has the highest EN?

Fluorine

Which element has the least EN?

Cesium

1

2

3

4

5

6

1

2

3

4

5

6

Electronegativity

7

Be

1.5

Al

1.5

Si

1.8

Ti

1.5

V

1.6

Cr

1.6

Mn

1.5

Fe

1.8

Co

1.8

Ni

1.8

Cu

1.9

Zn

1.7

Ga

1.6

Ge

1.8

Nb

1.6

Mo

1.8

Tc

1.9

Ag

1.9

Cd

1.7

In

1.7

Sn

1.8

Sb

1.9

Ta

1.5

W

1.7

Re

1.9

Hg

1.9

Tl

1.8

Pb

1.8

Bi

1.9

1.5 - 1.9

N

3.0

O

3.5

F

4.0

Cl

3.0

3.0 - 4.0

C

2.5

S

2.5

Br

2.8

I

2.5

2.5 - 2.9

Na

0.9

K

0.8

Rb

0.8

Cs

0.7

Ba

0.9

Fr

0.7

Ra

0.9

Below 1.0

H

2.1

B

2.0

P

2.1

As

2.0

Se

2.4

Ru

2.2

Rh

2.2

Pd

2.2

Te

2.1

Os

2.2

Ir

2.2

Pt

2.2

Au

2.4

Po

2.0

At

2.2

2.0 - 2.4

Per

iod

Actinides: 1.3 - 1.5

Li

1.0

Ca

1.0

Sc

1.3

Sr

1.0

Y

1.2

Zr

1.4

Hf

1.3

Mg

1.2

La

1.1

Ac

1.1

1.0 - 1.4

Lanthanides: 1.1 - 1.3

1A

2A

3B 4B 5B 6B 7B 1B 2B

3A 4A 5A 6A 7A

8A

Hill, Petrucci, General Chemistry An Integrated Approach 2nd Edition, page 373

8B

Trend in Ionization Energy

Definition – amount energy needed to remove the outer most electronAs you go down a group, the first IE decreases because...The electron is further away from the attraction of the nucleus, and

The larger the atom is, the easier its electrons are to remove.Trend from left to right – increasesTrend from top to bottom – decreases

Firs

t Ion

izat

ion

ener

gy

Atomic number

H

HeHelium is a noble gas, the energy to

remove its outer valence electron will be extremely high

Why does Lithium have a low IE? Lithium would have a lower IE because it

has a larger atomic radius than H

Why do atoms steal electrons or give them away?

Atoms behave in ways to try and achieve a noble gas configuration.

Would Beryllium have a higher first or second ionization energy level?

Second

Li

Be

B

Ionization Energy

F

Cs

Noble

Gas

Summary of Trend

Atomic Radius: Largest toward SW corner of PTAtomic Radius: Largest toward SW corner of PT

Ionization Energy: Largest toward FluorineIonization Energy: Largest toward FluorineElectronegativity: Most favorable FluorineElectronegativity: Most favorable Fluorine

Review Game

Round 1

White board

How many valence electrons does Krypton have?

8

What is the family name of the group 2A elements?

Alkaline Earth Metals

Name three characteristics of a metal.

Metals are lustrous (shiny), malleable, ductile, and are good conductors of heat and electricity.

They are mostly solids at room temp.

What is the family name of the group 8A elements?

Nobel Gases

Draw the Lewis Dot structure for chlorine.

How many valence electrons does this element have?

Ca 1s22s22p63s23p64s2

2

Where are metalloids located?

They are the elements touching the staircase.

What is the family name of the group 7A elements?

Halogens

A vertical column ( ↓ ) of elements on the

periodic table may also be referred to as a:

Family or Groups

What is the family name of the group 1A elements?

Alkaline metals

Describe three characteristics of a nonmetal.

Nonmetals are the opposite.

They are dull, brittle, nonconductors (insulators).

Some are solid, but many are gases, and Bromine is a liquid

Draw the lewis dot structure for Bromide.

A horizontal row ( → ) of elements on the periodic table may also be referred to as a:

Period

Review Game

Round 2

clickers

Cations have a ______________ charge and are ______________ than the atoms from which they formed.

A. negative/larger

B. positive/smaller

C. positive/larger

D. negative/smaller

B

Given the representation of a chlorine atom, which circle might represent an atom of bromine?

A. Circle C

B. None of these

C. Circle D

D. Circle B

c

Of the following elements, which one would have the largest radius?

A. Hydrogen (H)

B. Potassium (K)

C. Sodium (Na)

D. Cesium (Cs)

d

The elements with the smallest atomic radii are found in the:

A. lower left-hand corner of the periodic table

B. lower right-hand corner of the periodic table

C. upper left-hand corner of the periodic table

D. upper right-hand corner of the periodic table

d

Anions have a ______________ charge and are ______________ than the atoms from which they formed.

A. positive/smaller

B. negative/smaller

C. positive/larger

D. negative/larger

d

Of the following elements, which one would have the largest ionization energy?

A. Hydrogen (H)

B. Potassium (K)

C. Cesium (Cs)

D. Sodium (Na)

a

The energy required to remove an electron from an atom is known as:

A. electronegatvity

B. radioactivity

C. electron affinity

D. ionization energy

D

Given the representation of a chlorine atom, which circle might represent an atom of fluorine?

A. Circle C

B. None of these

C. Circle B

D. Circle D

b

The most active metals are located in the:

A. upper right hand corner of the periodic table

B. lower left hand corner of the periodic table

C. upper left hand corner of the periodic table

D. lower right hand corner of the periodic table

B

Of the following elements, which one would have the smallest radius?

A. Bromine (Br)

B. Fluorine (F)

C. Chlorine (Cl)

D. Iodine (I)

B

As one moves down ( ↓ ) a group on the periodic table, the ionization energy of the elements encountered tends to:

A. stay the same

B. decrease

C. increase

B

Of the following elements, which one would have the largest electronegativity energy?

A. Chlorine (Cl)

B. Fluorine (F)

C. Iodine (I)

D. Bromine (Br)

B

Of the following elements, which one would have the largest radius?

A. Lithium (Li)

B. Nitrogen (N)

C. Boron (B)

D. Neon (Ne)

A

Given the representation of a chlorine atom, which circle might a chloride ion, Cl-?

A. Circle C

B. Circle B

C. Circle D

D. None of these

D

As one moves from left to right ( → ) within a

period across the periodic table, the atomic

radius of the elements encountered tends to:

A. increase

B. stay the same

C. decrease

C

Which of these elements would have the lowest first ionization energy?

A. Element D

B. Element C

C. Element A

D. Element B

A

The least electronegative elements are the:

A. Transition metals

B. Alkali metals

C. Halogens

D. Metalloids

B

As one moves from left to right ( → ) within a period across the periodic table, the ionization energy of the elements encountered tends to:

A. decrease

B. increase

C. stay the same

B

The measure of the attraction that an atom has for electrons involved in chemical bonds is known as:

A. electron affinity

B. radioactivity

C. electronegatvity

D. ionization energy

C