3. An element “X” has mass number 35 and the number of neutrons, is 18. Identify
the group number and period of “X”.
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Answered by
1
given mass no. = 35
no. of neutrons = 18
therefore no. of protons = atomic no. = 35-18 = 17
so the element X has atomic no. 17
so its group no. is 17 and period is 3
no. of neutrons = 18
therefore no. of protons = atomic no. = 35-18 = 17
so the element X has atomic no. 17
so its group no. is 17 and period is 3
tasneemprzd10:
how do we get to know the period
IT is the number of shells
so how do we get to know tat it has 3 shells
by the electronic configuration
plzz explain it I m very poor at tat
no worries. see, they have given that mass number is 35 and number of neutrons is 18. we know that mass number= sum of neutrons + protons. so we find proton by subtracting 35-18 =17 . so 17 is the atomic number of element X. now we need to find its electronic configuration . for that we distribute the electrons into K,L,M shells. hence we get the electric configuration as 2,8,7
k tq but how does it show tat it belongs to the third period
because it has three shells. that determines that it belongs to period 3
k k I get I now
Answered by
0
Number of protons= 35-18=17
The atom is chlorine
Electronic configuration- 2,8,7
group number- 17
period-3
The atom is chlorine
Electronic configuration- 2,8,7
group number- 17
period-3
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