Drill #6:11/11 & 11/12/13

Drill pd 3 11/17/14

Rank in order of increasing ionization energy. Si, C, S, F, Ca

Rank in order of decreasing atomic radii. F, S, N

Rank in order of increasing atomic radius As, Te, P, Al

Rank in order of increasing electronegativity. Ge, P, As, Cs

HINT: Look at group trends first, then period trends

Answers

Ca, Si, S, C, F F, N, S P, Al, As, Te Cs, Ge, As, P

Drill 4A/4B 11/17& 18/2014 Differentiate between ionization energy

and electronegativity. What types of periodic trends are you

noticing for atomic radius, ionization energy and electronegativity?

Ionization energy is the energy needed to REMOVE one of the atom’s outermost electrons while an atom’s electronegativity is its ability to ATTRACT electrons to itself in a chemical bond.

Announcement

Conclusions have been graded. You have one week to turn back into me for ½ credit.

PBIS stuff

SWBAT:

Analyze the trends of ionization energy, electronegativity and atomic radius by completing a graphing activity.

Homework

-2 Review and Reinforcement – pd 4A and 4B

Graph

PERIODIC TRENDS GRAPHING ACTIVITY

GRAPH DATA

Construct 1 graph for ionization energy, electronegativity and atomic radius. Answer questions on the Worksheet.

Octet Rule

Atoms tend to gain, lose, or share electrons so that each atom has a full outermost energy level, which typically consists of 8 electrons (called an octet)

Periodic Table Patterns

Nuclear Charge

Nuclear charge-the charge in the nucleus or the number of protons

Across – increases Down – increases

Atomic Mass

Weighted average (based on mass and percent abundance of each naturally occurring isotope)

Across – increases Down – increases Remember there are some exceptions to

this – like Te and I

Atomic Radius

One-half the distance between the nuclei of identical atoms that are bonded together.

Ionization Energy (IE)

Ionization energy is the energy needed to REMOVE one of the atom’s outermost electrons

Electronegativity

An atom’s electronegativity is its ability to attract electrons to itself in a chemical bond

Trend for Atomic Radius

Atomic radius decreases as you go from the left to the right across a period. This is because there is an increased nuclear charge (protons) but no additional “shielding” electrons come between valence electrons and nucleus.

Atomic radius increases as you go down a group. Increased distance of electrons and additional electron energy levels shield valence electrons.

Shielding Effect

The shielding effect is the reduction of attractive force between the nucleus (+) and its outer electrons (-) due to the blocking affect of the inner electrons

Nucleus

Shielding electrons

Valence electrons ‘shielded’ by inner electrons

Snowman analogy

Trend for Ionization Energy

Ionization energy increases as you go from the left to the right across a period this means it’s MORE DIFFICULT to remove

an electron because of increased positive nuclear charge.

Ionization energy decreases as you go down a group this means it’s EASIER to remove an

electron because as atomic radius increases, outermost electrons are further away from nucleus.

Trend for Electronegativity

Electronegativity increases as you go from the left to the right across a period

Electronegativity generally decreases as you go down a group in the periodic table

** Because the noble gases form very few compounds, they do not have an electronegativity value.

Trend for Electronegativity (cont) The highest electronegativity values

are located in the upper-right hand corner of the periodic table Fluorine has the highest electronegativity

value of 4.0 The lowest electronegativity values are

located in the lower-left hand corner of the periodic table

It is NOT an amount of energy

Ionization Energy (IE) - review Ionization energy – this is the energy

needed to remove one of the atom’s outermost electrons

Metals have low IE Nonmetals have high IE

Trend for IE

1) IE’s decrease as you move down a group why?

Why?

The electrons in larger atoms are held less strongly by the nucleus, therefore as you move down a group, the IE decreases

Trend for IE

2) IE’s increase as you move from the left to the right across a period why?

WHY?

As you move across a period, there is a decrease in atomic radius, therefore causing the IE to increase

Removing electrons from positive ions With sufficient energy, electrons can be

removed from positive ions. The energy required to remove a second

electron from an atom is called its second IE, and so on…

The second IE will be greater than the first IE, the third IE greater than the second, etc. because as electrons are removed, fewer electrons remain to shield the attractive nuclear force.

Electron Affinity (EA)

Neutral atoms can acquire electrons. An atom’s electron affinity is the

energy change that occurs when an electron is acquired by a neutral atom.

Trend for EA

They change in irregular ways across a period and down a group

General rules: nonmetals have higher electron

affinities than do metals (this means it’s usually easier to add an electron to a nonmetal)

The halogens gain electrons most readily – higher electron affinities.

Trends Across the Periodic Table

PERIODIC TABLE OF THE ELEMENTS1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 181

H1.008

2

He4.003

3

Li6.941

4

Be9.012

5

B10.81

6

C12.01

7

N14.01

8

O16.00

9

F19.00

10

Ne20.18

11

Na22.99

12

Mg24.31

13

Al26.98

14

Si28.09

15

P30.97

16

S32.07

17

Cl35.45

18

Ar39.95

19

K39.10

20

Ca40.08

21

Sc44.96

22

Ti47.87

23

V50.94

24

Cr52.00

25

Mn54.94

26

Fe55.85

27

Co58.93

28

Ni58.69

29

Cu63.55

30

Zn65.39

31

Ga69.72

32

Ge72.61

33

As74.92

34

Se78.96

35

Br79.90

36

Kr83.80

37

Rb85.47

38

Sr87.62

39

Y88.91

40

Zr91.22

41

Nb92.91

42

Mo95.94

43

Tc[98.9]

44

Ru101.1

45

Rh102.9

46

Pd106.4

47

Ag107.9

48

Cd112.4

49

In114.8

50

Sn118.7

51

Sb121.8

52

Te127.6

53

I126.9

54

Xe131.3

55

Cs132.9

56

Ba137.3

57-70*

71

Lu175.0

72

Hf178.5

73

Ta180.9

74

W183.8

75

Re186.2

76

Os190.2

77

Ir192.2

78

Pt195.1

79

Au197.0

80

Hg200.6

81

Tl204.4

82

Pb207.2

83

Bi209.0

84

Po[209]

85

At[210]

86

Rn[222]

87

Fr[223]

88

Ra[226]

89-102**

103

Lr[262]

104

Rf[261]

105

Db[262]

106

Sg[263]

107

Bh[264]

108

Hs[265]

109

Mt[268]

110

Uun[269]

111

Uuu[272]

112

Uub[277]

114

Uuq[289]

116

Uuh[289]

118

Uuo[293]

*lanthanoids 57

La138.9

58

Ce140.0

59

Pr140.9

60

Nd144.2

61

Pm[145]

62

Sm150.4

63

Eu152.0

64

Gd157.3

65

Tb158.9

66

Dy162.5

67

Ho164.9

68

Er167.3

69

Tm168.9

70

Yb173.0

**actinoids 89

Ac[227]

90

Th232.0

91

Pa231.0

92

U238.0

93

Np[237]

94

Pu[244]

95

Am[243]

96

Cm[247]

97

Bk[247]

98

Cf[251]

99

Es[252]

100

Fm[257]

101

Md[258]

102

No[259]

Version Date 29 February 2000

Shielding Effect Stays the SameAtomic Radius decreasesIonization Energy IncreasesElectronegativity Increases

Trends Down the Periodic Table

PERIODIC TABLE OF THE ELEMENTS1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 181

H1.008

2

He4.003

3

Li6.941

4

Be9.012

5

B10.81

6

C12.01

7

N14.01

8

O16.00

9

F19.00

10

Ne20.18

11

Na22.99

12

Mg24.31

13

Al26.98

14

Si28.09

15

P30.97

16

S32.07

17

Cl35.45

18

Ar39.95

19

K39.10

20

Ca40.08

21

Sc44.96

22

Ti47.87

23

V50.94

24

Cr52.00

25

Mn54.94

26

Fe55.85

27

Co58.93

28

Ni58.69

29

Cu63.55

30

Zn65.39

31

Ga69.72

32

Ge72.61

33

As74.92

34

Se78.96

35

Br79.90

36

Kr83.80

37

Rb85.47

38

Sr87.62

39

Y88.91

40

Zr91.22

41

Nb92.91

42

Mo95.94

43

Tc[98.9]

44

Ru101.1

45

Rh102.9

46

Pd106.4

47

Ag107.9

48

Cd112.4

49

In114.8

50

Sn118.7

51

Sb121.8

52

Te127.6

53

I126.9

54

Xe131.3

55

Cs132.9

56

Ba137.3

57-70*

71

Lu175.0

72

Hf178.5

73

Ta180.9

74

W183.8

75

Re186.2

76

Os190.2

77

Ir192.2

78

Pt195.1

79

Au197.0

80

Hg200.6

81

Tl204.4

82

Pb207.2

83

Bi209.0

84

Po[209]

85

At[210]

86

Rn[222]

87

Fr[223]

88

Ra[226]

89-102**

103

Lr[262]

104

Rf[261]

105

Db[262]

106

Sg[263]

107

Bh[264]

108

Hs[265]

109

Mt[268]

110

Uun[269]

111

Uuu[272]

112

Uub[277]

114

Uuq[289]

116

Uuh[289]

118

Uuo[293]

*lanthanoids 57

La138.9

58

Ce140.0

59

Pr140.9

60

Nd144.2

61

Pm[145]

62

Sm150.4

63

Eu152.0

64

Gd157.3

65

Tb158.9

66

Dy162.5

67

Ho164.9

68

Er167.3

69

Tm168.9

70

Yb173.0

**actinoids 89

Ac[227]

90

Th232.0

91

Pa231.0

92

U238.0

93

Np[237]

94

Pu[244]

95

Am[243]

96

Cm[247]

97

Bk[247]

98

Cf[251]

99

Es[252]

100

Fm[257]

101

Md[258]

102

No[259]

Version Date 29 February 2000

Shielding Effect IncreasesAtomic Radius IncreasesIonization Energy DecreasesElectronegativity Decreases

Drill 11/19/14

Comparison of Na and Cl atoms1. Both atoms are in the same period.

Explain the differences in their sizes.

2. Predict the charge that an ion of each would have. Explain your answer.

3. Compare the ionization energy required to remove the first electron from each of these atoms.

4. Draw the ion for each atom. Make sure to represent their sizes relative to their original sizes.

Ignore sizes of atoms:

Answers to Drill1. Cl is smaller than Na because the increased

positive nuclear charge exerts a stronger pull on the e- shrinking the cloud.

2. A Na ion would have a charge of +1 and Cl ion, a charge of -1 because Na must lose an e- to have a full octet and Cl must gain an e-.

3. The IE of Cl would be higher because nonmetals hold on to their valence e- more tightly.

4. The Cl ion is now larger than the Na ion. Sodium lost its outermost orbital. The positive nuclear charge is felt more strongly.