An atom of an element has 28 innermost electrons and 7 outermost electrons. In which period of the Periodic Table is this elemen
2 answers:
<u>Answer:</u> The given element belongs to Period 4.
<u>Explanation:</u>
We are given:
Number of innermost electrons = 28
Number of outermost electrons = 7
Total number of electrons = 28 + 7 = 35
Electronic configuration is defined as the representation of electrons around the nucleus of an atom.
Number of electrons in an atom is determined by the atomic number of that atom.
The electronic configuration of the element having atomic number '35' is:
To identify the period, we look at the highest occupied principle quantum number which is 'n'. Here, the value of highest occupied shell or 'n' is 4.
Hence, the given element belongs to Period 4.
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Answer:
a) 2-bromopyrrole
Explanation:
Our options for this questions are:
a) 2-bromopyrrole
b) 2,3-dibromopyrrole
c) N-bromopyrrole
d) 3-bromopyrrole
To understand how the reaction works we have to start with the <u>resonance structures</u>. (Figure 1), on these structures, we will obtain a n<u>egative charge on carbon 2</u> in the pyrrole ring, therefore on this carbon we can generate an attack to an electrophile.
The second step is to check how the mechanism take place. An <u>electrophile is generated</u> by the and
. This electrophile can be <u>attacked</u> by the negative charge on carbon 2 producing the 2-bromopyrrole. (See figure 2).
I hope it helps!
