Which of the following symbolic representations is correct for an atom X with 22 electrons and 43 neutrons?
\(^{43}_{22}X\)
\(^{22}_{43}X\)
\(^{65}_{43}X\)
\(^{65}_{22}X\)
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Here is an explanation:
Mass number is the total number of proton and neutron of an element-and number of proton=number of electron. 43+22=65 that's the mass number which should be untop of the X while atomic number is the electron or proton number which should be under
REF: OSIE YAW ABABIO page 69
to cut the whole story short,
u can see that X here represent an element.
from the question there is no indication that the element X is positively charged or negatively charged. therefore, the laws for this condition includes the following:
1. when an atom is positively charged, it means that it loses an electron (s).
2. atoms gains electrons and become negatively charged.
3. for positivity charged atom, the number of electrons is less than the number of protons.
4. for negativity charged atom, the number of electrons is greater than the number of protons
5. for neutral atoms, the number of electrons is equal to the number of protons.
now back to our question
we were given the following values
neutrons= 43
electrons = 22
proton = 22
now why is it that we recognized proton to be 22 why it is not given in the question?????
answer: it is because from the rule I stated above, it says for neutral atoms the number of electrons is equal to no of protons.
meanwhile we don't know the value of mass number yet.
how do we found that??
we can found that using the formula below.
recall:
mass no. = neutron + proton
mass no. = 22+43
mass no. = 65.
so ooo from the look of things, option D is very correct 💯.
