Complete the table-Outermost electronic configurationGroup NumberOxidation state3s-2- 3p-4-16underline - a - 3s-1-underline - b - -12s-2- 2p-5-underline - c - underline - d - 3d-10-4s-2-underline - e - underline - f -

Question

Toppr Admin · Accepted Answer

-text-Group number- -Rightarrow -text-no- of valence electron-oxidation state - refer imagea- -2-b- -1-c- -17-d- -1-e- -12-f- -2-

Outermost electronic configuration	Group Number	Oxidation state
$$3s^{2}\ 3p^{4}$$	$$16$$	$$\underline { a }$$
$$3s^{1}$$	$$\underline { b }$$	$$+1$$
$$2s^{2}\ 2p^{5}$$	$$\underline { c } $$	$$\underline { d } $$
$$3d^{10}4s^{2}$$	$$\underline { e } $$	$$\underline { f } $$

Outermost electronic configuration	Group Number	Oxidation state
$$3s^{2}\ 3p^{4}$$	$$16$$	$$\underline { a }$$
$$3s^{1}$$	$$\underline { b }$$	$$+1$$
$$2s^{2}\ 2p^{5}$$	$$\underline { c } $$	$$\underline { d } $$
$$3d^{10}4s^{2}$$	$$\underline { e } $$	$$\underline { f } $$

Complete the table.
Outermost electronic configuration Group Number Oxidation state
$$3s^{2}\ 3p^{4}$$ $$16$$ $$\underline { a }$$
$$3s^{1}$$ $$\underline { b }$$ $$+1$$
$$2s^{2}\ 2p^{5}$$ $$\underline { c } $$ $$\underline { d } $$
$$3d^{10}4s^{2}$$ $$\underline { e } $$ $$\underline { f } $$

$$\text{Group number} \Rightarrow \text{no. of valence electron}$$
oxidation state : refer image
a. $$-2$$
b. $$1$$
c. $$17$$
d. $$-1$$
e. $$12$$
f. $$+2$$

Complete the table.Outermost electronic configurationGroup NumberOxidation state$$3s^{2}\ 3p^{4}$$$$16$$$$\underline { a }$$ $$3s^{1}$$$$\underline { b }$$ $$+1$$$$2s^{2}\ 2p^{5}$$$$\underline { c } $$$$\underline { d } $$$$3d^{10}4s^{2}$$$$\underline { e } $$$$\underline { f } $$

$$\text{Group number} \Rightarrow \text{no. of valence electron}$$oxidation state : refer imagea. $$-2$$b. $$1$$c. $$17$$d. $$-1$$e. $$12$$f. $$+2$$

Complete the table.
Outermost electronic configuration Group Number Oxidation state
$$3s^{2}\ 3p^{4}$$ $$16$$ $$\underline { a }$$
$$3s^{1}$$ $$\underline { b }$$ $$+1$$
$$2s^{2}\ 2p^{5}$$ $$\underline { c } $$ $$\underline { d } $$
$$3d^{10}4s^{2}$$ $$\underline { e } $$ $$\underline { f } $$

$$\text{Group number} \Rightarrow \text{no. of valence electron}$$
oxidation state : refer image
a. $$-2$$
b. $$1$$
c. $$17$$
d. $$-1$$
e. $$12$$
f. $$+2$$