Question

comprehension check questions chem 2.2_periodic table & atomic calculations use a periodic table and the information provided to complete the rest of the chart about the following four atoms. 1. element (nuclear notation) atomic # mass # # p⁺ #n⁰ #e⁻ ²⁷al 14 25 30 47 109 11 5 2 2. draw a bohr model for each main group element in the chart above (so skip any transition metals).

Explanation:

Step1: Recall atomic number and proton - neutron - electron relationships

The atomic number (\(Z\)) is equal to the number of protons (\(\#p^{+}\)). For 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 (\(A=\#p^{+}+\#n^{0}\)).

Step2: Analyze \(^{27}Al\)

• The atomic number of aluminum (\(Al\)) from the periodic table is \(13\). So, for \(^{27}Al\), \(\#p^{+}=13\). Since it is a neutral atom, \(\#e^{-}=13\). Given \(\#n^{0} = 14\), and the mass number \(A=\#p^{+}+\#n^{0}=13 + 14=27\). The atomic number is \(13\).

Step3: Analyze the second row

• Given \(\#p^{+}=25\), from the periodic table, the element is manganese (\(Mn\)). The atomic number \(Z = 25\). Given \(\#n^{0}=30\), the mass number \(A=\#p^{+}+\#n^{0}=25 + 30=55\). For a neutral atom, \(\#e^{-}=25\).

Step4: Analyze the third row

• Given atomic number \(Z = 47\), from the periodic table, the element is silver (\(Ag\)). Given mass number \(A = 109\), \(\#p^{+}=47\) (since \(Z=\#p^{+}\)). \(\#n^{0}=A-\#p^{+}=109 - 47 = 62\). For a neutral atom, \(\#e^{-}=47\).

Step5: Analyze the fourth row

• Given \(\#p^{+}=11\), from the periodic table, the element is sodium (\(Na\)). The atomic number \(Z = 11\). Given \(\#n^{0}=A-\#p^{+}\), and since \(\#p^{+}=11\) and \(\#e^{-}=2\) (assuming it is an ion, and it has lost \(9\) electrons), for a neutral \(Na\) atom \(\#e^{-}=11\). Given \(\#p^{+}=11\) and \(\#n^{0}=5\), the mass number \(A=\#p^{+}+\#n^{0}=11 + 5=16\).

The completed table:

Element (Nuclear notation)	Atomic #	Mass #	\(\#p^{+}\)	\(\#n^{0}\)	\(\#e^{-}\)
\(^{55}Mn\)	\(25\)	\(55\)	\(25\)	\(30\)	\(25\)
\(^{109}Ag\)	\(47\)	\(109\)	\(47\)	\(62\)	\(47\)
\(^{16}Na\) (assuming ion)	\(11\)	\(16\)	\(11\)	\(5\)	\(2\) (ion) or \(11\) (neutral)

For the second - part about drawing Bohr models, for \(Al\) (a main - group element):

• The atomic number of \(Al\) is \(13\). The first shell can hold \(2\) electrons, the second shell can hold \(8\) electrons, and the third shell holds \(3\) electrons. So, the Bohr model of \(Al\) has a nucleus with \(13\) protons and \(14\) neutrons, and three electron - shells: the first shell with \(2\) electrons, the second shell with \(8\) electrons, and the third shell with \(3\) electrons.

For \(Na\) (a main - group element), with atomic number \(11\):

• The first shell has \(2\) electrons, the second shell has \(8\) electrons, and the third shell has \(1\) electron. The Bohr model has a nucleus with \(11\) protons and \(5\) neutrons (from the table), and three electron - shells: \(2\) in the first, \(8\) in the second, and \(1\) in the third.

Answer:

Element (Nuclear notation)	Atomic #	Mass #	\(\#p^{+}\)	\(\#n^{0}\)	\(\#e^{-}\)
\(^{55}Mn\)	\(25\)	\(55\)	\(25\)	\(30\)	\(25\)
\(^{109}Ag\)	\(47\)	\(109\)	\(47\)	\(62\)	\(47\)
\(^{16}Na\) (assuming ion)	\(11\)	\(16\)	\(11\)	\(5\)	\(2\) (ion) or \(11\) (neutral)

Bohr model of \(Al\): Nucleus with \(13\) protons and \(14\) neutrons, \(2\) electrons in first shell, \(8\) in second, \(3\) in third.
Bohr model of \(Na\): Nucleus with \(11\) protons and \(5\) neutrons, \(2\) electrons in first shell, \(8\) in second, \(1\) in third.