CHAPTER 3 : PERIODIC TABLE
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1. Trends in group
1.1. Down a group, the electronegativity decreases.
1.2. atom size increase also attraction between nucleus and outer become weaker.
1.3. so, its has smaller relative to attract electron to itself.
2. Size of anion
2.1. size of anion > size neutral atoms
2.2. it is because electron are added to an atom, repulsion between electron increase and it size of anion became larger.
3. Ionic radius
3.1. Down a group, ionic radius increase
3.2. The ionic size decreases across a period but increases significantly from cation to anion
4. Ionization energy (IE)
4.1. Down a group, ionization energy decreases.
4.2. Across a period, ionization energy increases.
5. EXAMPLE
5.1. IE is the minimum energy to remove an electron from gaseous atom or ion
6. Electronegativity
6.1. electronegativity is relative ability of an atom to attract electrons towards itself
7. Trends in period
7.1. Across a period, the electronegativity increase
7.2. because proton number increase
7.3. so, effective nucleus charge, Zeff also increase
7.4. atom radius increase also attraction between nucleus and outer become stronger.
7.5. so, its has greater relative to attract electron to itself.
8. PERIOD
8.1. Periodic Table are numbered 1 to 7
8.2. Period number can be determined based on principle quantum number, n, of the electrons in the valence shell.
9. electrons configuration
10. BLOCK
10.1. Block s ( Group 1 and 2 )
10.1.1. ns^1 to ns^2
10.2. Block p ( Group 13 to 18 )
10.2.1. ns^2 np^1 to ns^2 np^6
10.3. Block d ( Group 3 to 12 )
10.3.1. ns^2 (n-1)d^1 to ns^2 (n-1)^10
10.4. Block p ( Group 13 to 18 )
11. GROUP
11.1. Periodic Table have name the group from 1 to 18.
11.2. Elements in the same group have the same number of valence electron.
11.3. Main Groups in Periodic Table :
11.3.1. GROUP 1 - alkali metals
11.3.2. GROUP 2 - alkali earth metals
11.3.3. GROUP 3 to 12 - transition metals
11.3.4. GROUP 17 - halogens
11.3.5. GROUP 18 - inert gases