1. Atoms and the Periodic Table
Chapter 3
Chapter Three
Atoms and the Periodic Table

2. Dalton’s Atomic Theory (1808)
Elements are composed of extremely small particles called atoms. All atoms of a given element are identical, having the same size,and chemical properties. The atoms of one element are different from the atoms of all other elements.
Compounds are composed of atoms of more than one element. The relative number of atoms of each element in a given compound is always the same.
Chemical reactions only involve the rearrangement of atoms. Atoms are not created or destroyed in chemical reactions.
2.1

3. What are atoms composed of?

4. The Structure of Atoms Cathode-Ray Tube (Thomson, 1856–1940):
Cathode rays consist of tiny negatively charged particles, now called electrons.

5. The Structure of Atoms
Oil Drop Experiment (Millikan, 1868–1953): Applied a voltage to oppose the downward fall of charged drops and suspend them.
Voltage on plates place x C of charge on each oil drop.
Millikan calculated the electron’s mass as x grams.

7. The Structure of Atoms Discovery of Nucleus (Rutherford, 1871 – 1937):
Rutherford irradiated gold foil with a beam of alpha () particles to search for positive charged particles.

8. The Structure of Atoms Discovery of Nucleus (Rutherford, 1871–1937):
Rutherford irradiated gold foil with a beam of alpha () particles to search for positive charged particles.
Atom must be mostly empty space except for a central positive mass concentration.

9. The Structure of Atoms
Structure of the Atom:

10. Atomic Number 11 Na Atomic Number Symbol
The atomic number is equal to the number of protons in an atom.
On the periodic chart, the atomic number appears above the symbol of an element. 11 Na
Atomic Number
Symbol

11. Atomic Numbers and Protons for Lithium and Carbon Atoms

12. Subatomic Particles
Chemists are interested in three particles in atoms: protons, electrons, and neutrons.
Protons have a positive (+) charge; electrons have a negative (-) charge.
Like charges repel and unlike charges attract.

13. Summary of Subatomic Particles

14. Structure of the Atom
An atom consists of a nucleus and a cloud of electrons.
The nucleus contains all of the protons and neutrons.
The rest of the atom, which is mostly empty space, is occupied by the electrons.

15. Learning Check State the number of protons in each. A. Nitrogen
1) 5 protons 2) 7 protons ) 14 protons
B. Sulfur
1) 32 protons 2) 16 protons ) 6 protons
C. Barium
1) 137 protons 2) 81 protons ) 56 protons

16. Solution State the number of protons in each. A. Nitrogen
2) Atomic number 7; 7 protons
B. Sulfur
2) Atomic number 16; 16 protons
C. Barium
3) Atomic number 56; 56 protons

17. Electrons in An Atom
An atom is electrically neutral; the net charge is zero.
In an atom, the number of protons is equal to the number of electrons. # protons = # electrons
Therefore, the atomic number is also equal to the number of electrons in a neutral atom.

18. Mass Number
The mass number gives the total number of protons and neutrons in the nucleus. Mass number = # protons # neutrons

19. Atomic Symbol
The atomic symbol represents a particular atom of an element.
The atomic symbol shows the mass number in the upper left corner and the atomic number in the lower left corner.
For example, an atom of sodium with atomic number 11 and a mass number 23 has the following atomic symbol: mass number 23 Na atomic number 11

20. Information from Atomic Symbols
When we know the atomic symbol of an atom, we can determine the number of protons (p+), neutrons, (n), and electrons (e-).
O P Zn
8 p+ 15 p p+
8 n 16 n 35 n
8 e e e-

21. Learning Check
Naturally occurring carbon consists of three isotopes, 12C, 13C, and 14C. State the number of protons, neutrons, and electrons in each of the following.
12C 13C C
protons ______ ______ ______
neutrons ______ ______ ______
electrons ______ ______ ______

22. Solution 12C 13C 14C 6 6 6 Protons 6 6 6 Neutrons 6 7 8
Protons
Neutrons
Electrons

23. Learning Check
Write the atomic symbols for atoms with the following subatomic particles:
A. 8 p+, 8 n, 8 e- ___________
B. 17p+, 20n, 17e- ___________
C. 47p+, 60 n, 47 e- ___________

24. Solution
Write the atomic symbols for atoms with the following subatomic particles:
16O
A. 8 p+, 8 n, 8 e
B. 17p+, 20n, 17e- 37Cl 17
C. 47p+, 60 n, 47 e- 107Ag 47

25. Learning Check An atom of zinc has a mass number of 65.
A. How many protons are in this zinc atom?
1) ) ) 65
B. How many neutrons are in the zinc atom?
C. What is the mass number of a zinc atom
that has 37 neutrons?
1) ) ) 67

26. Solution An atom of zinc has a mass number of 65.
A. How many protons are in this zinc atom?
1) 30
B. How many neutrons are in the zinc atom?
2) 35
C. What is the mass number of a zinc atom
that has 37 neutrons?
3) 67

27. Learning Check An atom has 14 protons and 20 neutrons.
A. Its atomic number is
1) ) ) 34
B. Its mass number is
C. The element is
1) Si 2) Ca 3) Se

28. Solution An atom has 14 protons and 20 neutrons.
A. It has atomic number
1) 14
B. It has a mass number of
3) 34
C. The element is
1) Si

29. 2.5 Isotopes and Atomic Mass
24Mg 25Mg 26Mg

30. Isotopes
Isotopes are atoms of the same element that have different mass numbers.
Isotopes have the same number of protons, but different numbers of neutrons.
All elements have two or more isotopes.

31. Isotopes of Magnesium
In naturally occurring atoms of magnesium, there are three isotopes.
24Mg makes up 78.9% of magnesium atoms.
25Mg makes up 10.0% and 26Mg makes up 11.1%.
24Mg 25Mg 26Mg

32. Learning Check
Using the periodic table, specify the atomic mass of each element (round to the tenths place):
A. calcium __________
B. aluminum __________
C. lead __________
D. barium __________
E. iron __________

33. Solution
Using the periodic table, specify the atomic mass of each element (round to the tenths place):
A. calcium amu
B. aluminum amu
C. lead amu
D. barium amu
E. iron amu

34. 3. 6 Electronic Structure of Atoms
Quantum mechanical model of atomic structure:
Electrons are not perfectly free to move about in an atom.
Each electron is restricted to moving about only in a certain region of space within the atom, depending on the amount of energy the electron has.

35. Probability distribution ( 2) for an electron in a 1s orbital.7

36. Boundary surfaces of a 1s orbital and a 2s orbital.
A boundary surface encloses the region where the probability of finding an electron is high—on the order of 90-95% 1s 2s
Boundary surfaces of a 1s orbital and a 2s orbital. 7

37. Different orbitals have different shapes
Different orbitals have different shapes. Orbitals in s subshells are spherical (a), while orbitals in p subshells are roughly dumbbell shaped (b).

38. s and p Orbitals
In an atom, all the orbitals are centered around the nucleus. For example, the illustration of the combination of s and p orbitals is

39. Subshells and Orbitals
Each subshell has a specific number of orbitals.
Each s subshell contains one s orbital.
Each p subshell contains three p orbitals.
Each d subshell contains five d orbitals.
Each f subshell contains seven f orbitals.

40. d-Orbitals

41. f-Orbitals

42. The first shell has only an s subshell
The second shell has an s and a p subshell
The third shell has an s, a p, and a d subshell.
The fourth shell has an s, a p, a d, and an f subshell.

43. The number of subshells in a given shell is equal to the shell number
The number of subshells in a given shell is equal to the shell number. For example, shell number 3 has 3 subshells.
Within each subshell, electrons are further grouped into orbitals, regions of space within an atom where the specific electrons are more likely to be found.
There are different number of orbitals within the diff erent kinds of subshells.

44. Energy of Electrons
Different electrons have different amounts of energy and thus occupy different regions within the atom.
The energies of electrons are quantized, or restricted to having only certain values.
The electrons in an atom are grouped around the nucleus into shells.
Within the shells, electrons are further grouped into sub shells of four different types, identified as s, p, d, and f in order of increasing energy.

45. Electrons fill orbitals in ascending order, from the lowest-energy orbitals upward. Generally, this means that lower-numbered shells fill before higher-numbered shells. However, some overlap in energy levels occurs starting in the third energy level.
Fig 3.5 order of orbital
energy levels

46. 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f, 5d, 6p, 7s, 5f, 6d, 7p

47. Some Electron Configurations
1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f, 5d, 6p, 7s, 5f, 6d, 7p
Some Electron Configurations
First Period
H 1s1
He 1s2
Second Period
Li s2 2s1
C 1s2 2s2 2p2
Third Period
Na 1s2 2s2 2p6 3s1
Al 1s2 2s2 2p6 3s2 3p1
S 1s2 2s2 2p6 3s2 3p4

48. Electronic configuration of a few elements are shown below:

50. Electron Configurations for Elements

51. 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f, 5d, 6p, 7s, 5f, 6d, 7p
Noble Gas Notation
A noble gas notation is used to abbreviate the completed subshells as [noble gas].
For example, the complete configuration of bromine is
1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p5
Ar configuration
The noble gas notation for bromine is
[Ar] 4s2 3d10 4p5

52. 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f, 5d, 6p, 7s, 5f, 6d, 7p
Learning Check
Write the complete electronic configuration and noble gas notation for each of the following elements:
A. Cl
B. Sr
C. I

53. Solution 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f, 5d, 6p,
A. Cl
1s2 2s2 2p6 3s2 3p5
[Ne] 3s23p5
B. Sr
1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2
[Kr] 5s2
C. I
1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p5
[Kr] 5s2 4d10 5p5

54. Group Numbers and Subshells
The Group Number is the sum of the s and p electrons in the outermost shell.

55. Fig 3.2 The periodic table

56. The table has 113 boxes, each of which tells the symbol, atomic number, and atomic weight of an element.
Last update: 117 elements known to date

57. Main Groups: The two large groups on the far left and the six on the far right are called the main groups.
Lanthanides: 14 elements following lanthanum in group 6.
Actinides: 14 elements following actinium in group 7.
Transition Metal Groups: Elements in the groups numbered 3 through 12 (Sc-Zn).
Inner Transition Metal Groups: The 14 groups shown separately at the bottom of the table and are not numbered.

58. 3.8 Electron Configuration and the Periodic table
The periodic table can be divided into four regions or blocks, of elements according to the shells and subshells as shown in Fig 3.6.
Valence Shell : Outermost shell of an atom.
Valence electrons: An electron in an outermost shell of an atom. These electrons are loosely held, they are most important in determining an element’s properties.

59. Group Numbers and Subshells
The Group Number is the sum of the s and p electrons in the outermost shell.

60. Electron Configuration and the Periodic Table
ns2np6
Electron Configuration and the Periodic Table
ns1
ns2np1
ns2np2
ns2np3
ns2np4
ns2np5
ns2
d10 d1 d5 4f 5f

61. Electron Configuration of Atoms 06

63. Using periodic table write Noble gas notation
for the following elements:
[Ne]3s23p4
a)S
[Ar] 4s23d6
b)Fe
[Ar] 4s23d104p4
c)Se
[Xe]6s2 5d1 4f7
d)Gd

65. Fig 3.6 electron configurations and the periodic table

66. Fig 3.2 The periodic table

67. Chapter Summary All matter is composed of atoms.
An atom is the smallest and simplest unit into which an element can be divided while maintaining the properties of the element.
Atoms are made up of subatomic particles called protons, neutrons and electrons. Protons have positive, electrons have negative, and neutrons have zero electrical charges.
Elements differ from each other according to the number of protons their atoms contain (Atomic number, Z)

68. Chapter Summary Contd.
Mass number (A): Total number of protons and neutrons in an atom.
Isotopes: Atoms with identical number of protons but different numbers of neutrons.
Periodic table: Tabular arrangement of elements according to their valence shells.
The electrons surrounding an atom are grouped into shells. Within each shell, electrons are grouped into subshells, and within subshells into orbitals – regions of space where electrons are more likely to be found.

69. Chapter Summary Contd.
s orbitals are spherical and p orbitals are bumbbell shaped.
Each orbital and each shell can hold a specific number of electrons.
- The first shell can hold only two electrons. 2 electrons in an s orbital (1S2).
- The second shell can hold 8 electrons electrons in an s orbital and 6 electrons in 3 p orbitals. (2S2 2p6).
- The third shell can hold 18 electrons. 2 electrons in an s orbital, 6 electrons in 3 p orbitals, and 10 electrons in 5 d orbitals (3S2 3p6 3d10); and so on.

70. End of Chapter 3