Question

2. An element has 2 naturally occurring isotopes with the following masses and abundances A. Calculate the atomic weight of the element. (20 pts) Isotope mass Percentage 34.97 amu 75.78% 36.97 amu 24.22% B. What is the element? C. How many neutrons does the heavier isotope have? (Round to whole number) D. How many electrons does the element have? E. What type(metal/nonmetal) of element is it? F. If the element above gains 1 electron what neutral element has the some number of electrons with it?

Answer 1

I have explained everything for better understanding...
IPAGE 1 e solution :- Gineu data in the question in Isotope mass percentage 34.97 amu 75.78 % 36.97 amu 24.22% (a) Atomic weight of the element can be calculated by calculating the average atomic mass atomic mass of both tu Isotopes. i. Average atomic mass= (Mass of Isotope I x fraction) + (Mass of Isotope 2 x fraction) (34.97 X0.7578 )+ ( 36.97 X0.2422) - 26.500266 + 8.954134 = 35.45 amu (b) Element name is chlorine. (Ce) - the atomic mass of chloine is 35.45 which is same as this element's average atomic mass. (c) Atomic mass of Heavier Isotope 36.97 ~ 37 Atomie number of chlorine u. number of protons .. Number of Neutoons = 17 17 37 - 17 20 - (d) Number of elections - Atomic number = 17

PAGE-2 (e) Type of element is [ Non-metal! (4) Aftu gaining 1 election, the number of eletons becomes (17+1)= 18. Oo Argon is the neutral element which has 18 electrons. Auswel in short :- (2) 35.45 amu. (b) chlorine (Ce). (c) 20 (d) 17. (e) Non-metal. (4) Argon.
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