Respuesta :
Answer:
atomic radius decreases along the group.
atomic radius increases down the group.
ionization energy increases along the group and decreases down the group.
Explanation:
1. As we add an electron the effective nucleus charge increases because when electrons increase protons also increase so the net nuclear charge on the valence electron also increases therefore the size will tend to decrease.
2. As we move from top to bottom number of shell keeps adding on as a result the atom becomes bigger and bigger due to increase in number of shell.so the size increases.
3.as we move from top to bottom the size increases as a result total nuclear pull on the valence electron decreases so it becomes easy to remove an electron so ionization energy decreases down the group. As we move along the period the effective nuclear charge increases as mentioned above in 1 therefore it becomes difficult to remove an electron so ionization energy increases as we move along the group.
Ionization Energy decreases from top to bottom but atomic radius increases.
- The atomic radius decrease as electrons are added to a shell because the protons present in the nucleus attracts the new added electron due to its opposite charges which brings the valance shell nearer to the nucleus.
- The atomic radius increase as we go from the top to the bottom in a periodic table because more shells or orbits are added which takes the valance shell far from the nucleus.
- Ionization Energy is higher when we go from left to right in a periodic table but lower when we go from top to bottom which opposite to atomic radius.
- As we go from top to bottom atomic radius increase but Ionization Energy decreases because due to addition of more shells the valance electron go far from the nucleus.
- So weak force of attraction is present that needs lower ionization energy so we can conclude that Ionization Energy decreases from top to bottom.
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