2. Matter Unit
Learning Goal #4: Correlate atomic structure and the physical and chemical properties of an element to the position of the element on the periodic table.

3. The Periodic Table
Dmitri Mendeleev ( )

4. Discovering the Periodic TableNe Ar Kr Xe Po Rn Ra Eu Lu Pa Ac C S Fe Cu Ag Sn Au Hg Pb
Ancient Times Tc Hf Re At Fr Pm Np Pu Am Cm Bk Cf Es Fm Md No Lr He Sc Ga Ge Rb Ru In Cs Tl Pr Nd Sm Gd Dy Ho Tm Yb La Cr Mn Li K N O F Na B Be H Al Si Cl Ca Ti V Co Ni Se Br Sr Y Zr Nb Mo Rh Pd Cd Te I Ba Ta W Os Ir Mg Ce Tb Er Th U P Zn As Sb Pt Bi
Midd Rf Db Sg Bh Hs Mt
1965-
Journal of Chemical Education, Sept. 1989

5. Elements are arranged:
Vertically into Groups
Horizontally Into Periods

6. Why?

7. If you looked at one atom of every element in a group you would see…

8. Each atom has the same number of electrons in its outermost shell.
An example…

9. The group 2 atoms all have 2 electrons in their outer shells
Be (Beryllium)
Atom
Mg (Magnesium) Atom

10. The number of outer or “valence” electrons in an atom affects the way an atom bonds.
The way an atom bonds determines many properties of the element.
This is why elements within a group usually have similar properties.

11. If you looked at an atom from each element in a period
you would see…

12. Each atom has the same number of electron shells.
An example…

13. The period 4 atoms each have 4 electron containing shells
4th Shell
K (Potassium)
Atom
Kr (Krypton)
Atom
Fe (Iron) Atom

14. Each group has distinct properties
The periodic Table is divided into several groups based on the properties of different atoms.

15. Soft, silvery colored metals
Alkali Metals
Soft, silvery colored metals
Very reactive!!!

16. Group 1A: Alkali Metals Reaction of potassium + H2O
Cutting sodium metal

17. http://www. youtube. com/watch

18. Alkali Metals reacting with water:
Li (Lithium) – least reactive
Na (Sodium)
K (Potassium)
Rb (Rubidium)
Cs (Cesium) – more reactive
What would you expect from Francium?!?!

19. Group 2A: Alkaline Earth Metals
Magnesium
Magnesium oxide

20. Alkaline Earth Metals
Silvery-White Metals
Fairly reactive
Many are found in rocks in the earth’s crust

21. Transition Metals
Most are good conductors of electricity
Malleable (easily bent/hammered into wires or sheets)

22. How many things can you think of that have Transition Metals in them?

24. Metalloids lie on either side of the “staircase”
They share properties with both metals and non-metals
Si (Silicon) and Ge (Germanium) are very important “semi-conductors”

25. METALS Metals and Nonmetals Nonmetals Metalloids H He Li Be B C N O F1 He 2 1 Li 3 Be 4 B 5 C 6
Nonmetals N 7 O 8 F 9 Ne 10 2 Na 11 Mg 12 Al 13 Si 14 P 15 S 16 Cl 17 Ar 18 3 K 19 Ca 20 Sc 21 Ti 22 V 23 Cr 24 Mn 25 Fe 26 Co 27 Ni 28 Cu 29 Zn 30 Ga 31 Ge 32 As 33 Se 34 Br 35 Kr 36 4
METALS Rb 37 Sr 38 Y 39 Zr 40 Nb 41 Mo 42 Tc 43 Ru 44 Rh 45 Pd 46 Ag 47 Cd 48 In 49 Sn 50 Sb 51 Te 52 I 53 Xe 54 5
Metalloids Cs 55 Ba 56 Hf 72 Ta 73 W 74 Re 75 Os 76 Ir 77 Pt 78 Au 79 Hg 80 Tl 81 Pb 82 Bi 83 Po 84 At 85 Rn 86 6 * Fr 87 Ra 88 Rf
104 Db
105 Sg
106 Bh
107 Hs
108 Mt
109 7 W La 57 Ce 58 Pr 59 Nd 60 Pm 61 Sm 62 Eu 63 Gd 64 Tb 65 Dy 66 Ho 67 Er 68 Tm 69 Yb 70 Lu 71 Ac 89 Th 90 Pa 91 U 92 Np 93 Pu 94 Am 95 Cm 96 Bk 97 Cf 98 Es 99 Fm
100 Md
101 No
102 Lr
103

26. What are semiconductors used in?

27. Nonmetals
Brittle
Do not conduct electricity

28. Halogens
Most are poisonous
Fairly reactive – react with alkali metals (eg) Na+ and Cl-

29. Chlorine Gas was used as a chemical weapon during World War I.
It was used by the Germans in World War II.

30. Chlorine Gas
The Germans were the first to use Chlorine gas at Ypres in 1915
Chlorine gas is a lung irritant
The symptoms of gas poisoning are bright red lips, and a blue face
People affected die a slow death by suffocation
Decades later men who thought they had survived the war died from lung diseases such as Emphysema

31. CHLORINE

32. Noble Gases
Unreactive
Gases at room temperature

33. Jellyfish lamps made with noble gases artist- Eric Ehlenberger

34. Colors Noble Gases produce in lamp tubes:
Ne (Neon): orange-red
Ar (Argon): pale lavender
He (Helium): pale peach
Kr (Krypton): pale silver
Xe (Xenon): pale, deep blue

35. Lanthanide Series
Actinide Series

36. (A) Periods of the periodic table, and (B) groups of the periodic table.

37. ELEMENTS THAT EXIST AS DIATOMIC MOLECULES
Remember:
The “GENS”
These elements exist as PAIRS when ALONE.
Hydrogen (H2)
Nitrogen (N2)
Oxygen (O2)
Halogens
(F2, Cl2, Br2, I2)
(P4 and S8)

38. Diatomic Elements H2 He Li Be B C N2 O2 F2 Ne Na Mg Al Si P S S Cl2 ArK Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se
Br2 Kr Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te I2 Xe Cs Ba La Hf Ta W Re Os Ir Pt Au Hg Tl Tl Pb Bi Po At Rn Fr Ra Ac Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr

39. Melting Points H He Mg Symbol Melting point oC Li Be B C N O F Ne
-259.2 He
-269.7 1 1 Mg
650
Symbol
Melting point oC Li
180.5 Be
1283 B
2027 C
4100 N
-210.1 O
-218.8 F
-219.6 Ne
-248.6 2 2
> 3000 oC oC Na 98 Mg
650 Al
660 Si
1423 P
44.2 S
119 Cl
-101 Ar
-189.6 3 3 K
63.2 Ca
850 Sc
1423 Ti
1677 V
1917 Cr
1900 Mn
1244 Fe
1539 Co
1495 Ni
1455 Cu
1083 Zn
420 Ga
29.78 Ge
960 As
817 Se
217.4 Br
-7.2 Kr
-157.2 4 4 Rb
38.8 Sr
770 Y
1500 Zr
1852 Nb
2487 Mo
2610 Tc
2127 Ru
2427 Rh
1966 Pd
1550 Ag
961 Cd
321 In
156.2 Sn
231.9 Sb
630.5 Te
450 I
113.6 Xe
-111.9 5 5 Cs
28.6 Ba
710 La
920 Hf
2222 Ta
2997 W
3380 Re
3180 Os
2727 Ir
2454 Pt
1769 Au
1063 Hg
-38.9 Tl
303.6 Pb
327.4 Bi
271.3 Po
254 At Rn
-71 6 6
Ralph A. Burns, Fundamentals of Chemistry , 1999, page 1999

40. Electronegativity
A measure of the ability of an atom in a chemical compound to attract electrons
  Electronegativities tend to increase across
a period
  Electronegativities tend to decrease down a
group or remain the same

41. Electronegativities Period H B P As Se Ru Rh Pd Te Os Ir Pt Au Po At
2.1 B
2.0 P As Se
2.4 Ru
2.2 Rh Pd Te Os Ir Pt Au Po At 1 1 2A 3A 4A 5A 6A 7A
Actinides: Li
1.0 Ca Sc
1.3 Sr Y
1.2 Zr
1.4 Hf Mg La
1.1 Ac
Lanthanides: * y Be
1.5 Al Si
1.8 Ti V
1.6 Cr Mn Fe Co Ni Cu
1.9 Zn
1.7 Ga Ge Nb Mo Tc Ag Cd In Sn Sb Ta W Re Hg Tl Pb Bi C
2.5 S Br
2.8 I N
3.0 O
3.5 F
4.0 Cl 2 2 Na
0.9 K
0.8 Rb Cs
0.7 Ba Fr Ra
Below 1.0 3 3 3B 4B 5B 6B 7B 8B 1B 2B
Period 4 4 5 5 6 6 7
Hill, Petrucci, General Chemistry An Integrated Approach 2nd Edition, page 373

42. Densities of Elements H He Li Be B C N O F Ne Na Mg Al Si P S Cl Ar K
0.071 He
0.126 1 1 Li
0.53 Be
1.8 B
2.5 C
2.26 N
0.81 O
1.14 F
1.11 Ne
1.204 2 2 Na
0.97 Mg
1.74 Al
2.70 Si
2.4 P
1.82w S
2.07 Cl
1.557 Ar
1.402 3 3 K
0.86 Ca
1.55 Sc
(2.5) Ti
4.5 V
5.96 Cr
7.1 Mn
7.4 Fe
7.86 Co
8.9 Ni
8.90 Cu
8.92 Zn
7.14 Ga
5.91 Ge
5.36 As
5,7 Se
4.7 Br
3.119 Kr
2.6 4 4 Rb
1.53 Sr
2.6 Y
5.51 Zr
6.4 Nb
8.4 Mo
10.2 Tc
11.5 Ru
12.5 Rh
12.5 Pd
12.0 Ag
10.5 Cd
8.6 In
7.3 Sn
7.3 Sb
6.7 Te
6.1 I
4.93 Xe
3.06 5 5 Cs
1.90 Ba
3.5 La
6.7 Hf
13.1 Ta
16.6 W
19.3 Re
21.4 Os
22.48 Ir
22.4 Pt
21.45 Au
19.3 Hg
13.55 Tl
11.85 Pb
11.34 Bi
9.8 Po
9.4 At
--- Rn
4.4 6 6
8.0 – 11.9 g/cm3
12.0 – 17.9 g/cm3
> 18.0 g/cm3 Mg
1.74
Symbol
Density in g/cm3C, for gases, in g/L W

43. Periodic Trends in Atomic Radius
  Radius decreases across a period
  Radius increases down a group

44. Atomic Radii = 1 Angstrom IA IIA IIIA IVA VA VIA VIIA Li Be B C N O F Na Mg Al Si P S Cl K Ca Ga Ge As Se Br Rb Sr In Sn Sb Te I Cs Ba Tl Pb Bi
= 1 Angstrom

45. Atomic Radii of Representative Elements (nm)
1A A A A A A A Li Be B C N O F Na Mg Al Si P S Cl K Ca Ga Ge As Se Br Rb Sr In Sn Sb Te I Cs Ba Tl Pb At Bi Po
LeMay Jr, Beall, Robblee, Brower, Chemistry Connections to Our Changing World , 1996, page 175

46. Increases for successive electrons taken from the same atom
Ionization Energy - the energy required to remove an electron from an atom
  Increases for successive electrons taken from
the same atom
  Tends to increase across a period
  Tends to decrease down a group

47. Ionization Energies Period H He Mg Li Be B C N O F Ne Na Mg Al Si P S
Group 1 18 H
1312
Symbol
First Ionization Energy
(kJ/mol) He
2372 1 1 Mg
738 2 13 14 15 16 17 Li
520 Be
900 B
801 C
1086 N
1402 O
1314 F
1681 Ne
2081 2 2 Na
496 Mg
738 Al
578 Si
787 P
1012 S
1000 Cl
1251 Ar
1521 3 3 3 4 5 6 7 8 9 10 11 12
Period K
419 Ca
590 Sc
633 Ti
659 V
651 Cr
653 Mn
717 Fe
762 Co
760 Ni
737 Cu
746 Zn
906 Ga
579 Ge
762 As
947 Se
941 Br
1140 Kr
1351 4 4 Rb
403 Sr
550 Y
600 Zr
640 Nb
652 Mo
684 Tc
702 Ru
710 Rh
720 Pd
804 Ag
731 Cd
868 In
558 Sn
709 Sb
834 Te
869 I
1008 Xe
1170 5 5 Cs
376 Ba
503 La
538 * Hf
659 Ta
761 W
770 Re
760 Os
839 Ir
878 Pt
868 Au
890 Hg
1007 Tl
589 Pb
716 Bi
703 Po
812 At -- Rn
1038 6 6 Fr -- Ra
509 Ac
490 y Rf -- Db -- Sg -- Bh -- Hs -- Mt -- Ds --
Uuu --
Uub --
Uut --
Uuq --
Uup --
Uuo -- 7 *
Lanthanide series Ce
534 Pr
527 Nd
533 Pm
536 Sm
545 Eu
547 Gd
592 Tb
566 Dy
573 Ho
581 Er
589 Tm
597 Yb
603 Lu
523 y
Actinide series Th
587 Pa
570 U
598 Np
600 Pu
585 Am
578 Cm
581 Bk
601 Cf
608 Es
619 Fm
627 Md
635 No
642 Lr --

48. Essential Elements Elements in organic matter H He Major minerals Li1 He 2
Major minerals Li 3 Be 4 B 5 C 6 N 7 O 8 F 9 Ne 10
Trace elements Na 11 Mg 12 Al 13 Si 14 P 15 S 16 Cl 17 Ar 18 K 19 Ca 20 Sc 21 Ti 22 V 23 Cr 24 Mn 25 Fe 26 Co 27 Ni 28 Cu 29 Zn 30 Ga 31 Ge 32 As 33 Se 34 Br 35 Kr 36 Rb 37 Sr 38 Y 39 Zr 40 Nb 41 Mo 42 Tc 43 Ru 44 Rh 45 Pd 46 Ag 47 Cd 48 In 49 Sn 50 Sb 51 Te 52 I 53 Xe 54 Cs 55 Ba 56 La 57 Hf 72 Ta 72 W 74 Re 75 Os 76 Ir 77 Pt 78 Au 79 Hg 80 Tl 81 Pb 82 Bi 83 Po 84 At 85 Rn 86
Davis, Metcalfe, Williams, Castka, Modern Chemistry, 1999, page 748

49. The electron affinity is a measure of the energy change when an electron is added to a neutral atom to form a negative ion.

50. The End

51. Atomic Radii Ionic Radii = 1 Angstrom = 1 Angstrom
0.95
IA IIA IIIA IVA VA VIA VIIA
= 1 Angstrom
Li1+
Be2+
Na1+
Mg2+
Ba2+
Sr2+
Ca2+
K1+
Rb1+
Cs1+
Cl1-
N3-
O2-
F1-
S2-
Se2-
Br1-
Te2-
I1-
Al3+
Ga3+
In3+
Tl3+
IA IIA IIIA IVA VA VIA VIIA Li Na K Rb Cs Cl S P Si Al Br Se As Ge Ga I Te Sb Sn In Tl Pb Bi Mg Ca Sr Ba Be F O N C B
= 1 Angstrom

52. The Atom An atom consists of a nucleus (of protons and neutrons)
electrons in space about the nucleus.
Electron cloud
Nucleus

53. ATOM COMPOSITION The atom is mostly empty space
protons and neutrons in the nucleus.
the number of electrons is equal to the number of protons.
electrons in space around the nucleus.
extremely small. One teaspoon of water has 3 times as many atoms as the Atlantic Ocean has teaspoons of water.

54. Compounds composed of 2 or more elements in a fixed ratio
properties differ from those of individual elements
EX: table salt (NaCl)

55. Composition of molecules is given by a MOLECULAR FORMULA
A MOLECULE is 2 more atoms bonded together – they may be the same element (ie diatomic molecule) or they may be different elements (ie caffeine)
Composition of molecules is given by a MOLECULAR FORMULA
H2O
C8H10N4O2 - caffeine

56. Isotopes
Atoms of the same element (same Z) but different mass number (A).
Boron-10 (10B) has 5 p and 5 n
Boron-11 (11B) has 5 p and 6 n
10B
11B

57. Isotopes & Their Uses
Bone scans with radioactive technetium-99.

58. CARBON-14 – RADIOACTIVE ISOTOPE
Occurs in trace amounts in the atmosphere
Absorbed into living organisms
The half-life of carbon-14 is approx 5700 years (when half the C-14 is converted to N-14)

59. Atomic Symbols sodium-23
Show the name of the element, a hyphen, and the mass number in hyphen notation
sodium-23
Show the mass number and atomic number in nuclear symbol form
mass number
23 Na
atomic number

60. Isotopes?
Which of the following represent isotopes of the same element?
Which element is it?
234 X X 235 X 238 X

61. IONS
IONS are atoms or groups of atoms with a positive or negative charge.
Donating an electron from an atom gives a CATION with a positive charge
Accepting an electron to an atom gives an ANION with a negative charge
To tell the difference between an atom and an ion, look to see if there is a charge in the superscript! Examples: Na+ Ca+2 I- O-2 Na Ca I O

62. Forming Cations & Anions
A CATION forms when an atom loses one or more electrons.
An ANION forms when an atom gains one or more electrons
F + e- --> F-
Mg --> Mg e-

63. PREDICTING ION CHARGES
In general
metals (Mg) lose electrons ---> cations (Mg2+)
nonmetals (F) gain electrons ---> anions (F-)

64. When an atom or molecule gain or loses an electron it becomes an ion.
A cation has lost an electron and therefore has a positive charge
An anion has gained an electron and therefore has a negative charge.

65. Charges on Common Ions -3 -2 -1 +1 +2
By losing or gaining e-, atom has same number of e-’s as nearest Group 8A atom.

66. Learning Check – Counting
State the number of protons, neutrons, and electrons in each of these ions.
39 K O Ca +2
#p+ ______ ______ _______
#no ______ ______ _______
#e- ______ ______ _______

67. Elements with 1, 2, or 3 electrons in their outer shell tend to lose electrons to fill their outer shell and become cations.
These are the metals which always tend to lose electrons.
Elements with 5 to 7 electrons in their outer shell tend to gain electrons to fill their outer shell and become anions.
These are the nonmetals which always tend to gain electrons.
Semiconductors (metalloids) occur at the dividing line between metals and nonmetals.

68. EXAMPLE So the charge would be +1
What would the charge be on a sodium ion?
Since sodium in in Group IA it is a metal and so would
LOSE an electron
You can tell how many would be lost by the group number
Group 1A elements lose 1 electron
So the charge would be +1
Remember an electron is negatively charged. When you lose them atom becomes positively charged…
when you gain them it becomes negatively charged

69. Na +1 EXAMPLE It has 1…remember the group number!
How would you right the symbol for the sodium CATION? Na +1
How many outer electrons does sodium have before it loses one?
It has 1…remember the group number!