The reason why Br has a greater magnitude of electron affinity than that of I is that there is a greater attraction between an added electron and the nucleus in Br than in I.
In the periodic table, there are trends that increase down the group and across the period. Electron affinity is a trend that increases across the period but decreases down the group.
Recall that the ability of an atom to accept an electron depends on the size of the atom. The smaller the atom, the greater the attraction between an added electron and the nucleus.
Since Br is smaller than I, there is a greater attraction between an added electron and the nucleus in Br than in I which explains why Br has a greater magnitude of electron affinity than I.
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Homogeneous mixture. (all of the different components of the salad are shown)
Answer:
Explanation:
2Al + 3Cl2 --> 2AlCl3
Ag2O + Be -----> 2Ag + BeO
4K + O2 ---> 2K2O
CoP + 3NaBr ---> CoBr3 + Na3P
Si + Hg2S ---> SiS2 + Hg
6Li + Ni3N2 --- > 2Li3N + 3Ni
3Ca + 2K3N --> Ca3N2 + 6K
SnS2 + 2F2 --> SnF4 + 2S
Answer: Correct option is (D).
Explanation:
Given that unknown element has larger atomic radii than potassium atoms and its valence electrons feel an effective nuclear charge of +1 which means that this unknown element belongs to group(I) of the periodic table.
In periodic table:
- As we move down the group the value of ionization energy decreases down the group. This is due to increase in the size of an element.With increase in size valence electrons gets far away from the nucleus by which less energy will require to ionize the element.
- Electronegative characters also decreases when we move down the group.This is due to increase in size of an element by which electrons present in valence shells are far away from the nucleus.
So,It would have lower ionization energies than K and a lower electronegativity value than K.
Answer:
C: The atomic nucleus contains most of the mass.
