Question

atomic structure
protons
neutrons
electrons
atomic calculation
atomic # = #p
#p = #e
mass # = #p + #n
determine the atomic number and identify the atom by using the periodic table.
isotope
symbol - mass
isotope notation
mass#px
#protons = 5
atomic # =
#electrons =
#neutrons =
mass # =
#protons =
atomic # =
#electrons =
#neutrons =
mass # =
14 6c

Explanation:

Step1: Recall atomic - structure relationships

The atomic number (\(Z\)) is equal to the number of protons (\(\#P\)). In a neutral atom, the number of electrons (\(\#e\)) is equal to the number of protons. The mass number (\(A\)) is the sum of the number of protons and neutrons (\(\#N\)), i.e., \(A=\#P+\#N\).

Step2: First - row calculations

Given \(\#P = 5\). The atomic number \(Z=\#P = 5\). Since \(\#e=\#P\), \(\#e = 5\). Counting the neutrons in the diagram, \(\#N=6\). Then the mass number \(A=\#P+\#N=5 + 6=11\).

Step3: Second - row calculations

For the isotope \(^{14}_6C\), the sub - script is the atomic number \(Z = 6\), so \(\#P=Z = 6\). Since \(\#e=\#P\), \(\#e = 6\). The mass number \(A = 14\), and \(\#N=A-\#P=14 - 6=8\).

Answer:

First row: Atomic \(\#=5\), \(\#\)electrons \( = 5\), \(\#\)neutrons \(=6\), Mass \(\# = 11\)
Second row: \(\#\)Protons \(=6\), Atomic \(\#=6\), \(\#\)electrons \( = 6\), \(\#\)neutrons \(=8\), Mass \(\# = 14\)