can someone help me please? Approval workshop #12 Periodic Trends and Bondin A \

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can someone help me please?

Approval workshop #12 Periodic Trends and Bondin A "Trendy Workshop A1. write the chemical reactions for the following processes. Be sure to include states and 1. The electron affinity of O 2. The first ionization energy of Cu 3. The third ionization energy of Cl 4. The electron affinity of Xe Answer the questions. Justify your answer based on the relative positions in the periodic A2, 1. Greater first ionization energy 2. Larger radius 3, Greater second ionization energy Mg 4- Greater electronegativity 5. Smaller radius 6. Larger radius A3. Why is Ba larger than Ca? Your justification must include an explanation beyond their relative positions on the periodic table.

Explanation / Answer

A.1.

1. Electron affinity of Oxygen = O(g) + e- ------------> O-(g)

2. First ionisation energy of Cu = Cu(g) ---------------> Cu+ (g) + e-

3. Third ionisation energy of chlorine= Cl+2(g) -------------> Cl+3(g) + e-

4. Electron affinity of Xenon = Xe(g) + e- ------------> Xe-(g)

A.2.

1. Out of Al ans Si, the first ionisation energy of Al is more than Si because the size of Al is less than Si and they belong to same group, in a group from left to right size of elements decreases.

2. Out of Na and Al, Na has larger radius than Al, they belong to same period and with increase in atomic number the the radius of elements in the same group decreases from left to right due increase of effective nuclear charge.

3. Out of Mg and Li the second ionisation energy is more for Li, because Mg atomic number =12 =1s2 2s2 2p6 3s2 configuration, Li atomic number =3 , electronic configuration = 1s2 2s1. After removing one electron lithium attains stable electronic configuration of helium so it is difficult to remove the second electron hence hs high second ionisation enthalpy, it is not in case of magnesium.

4. Out of B and C, electronegativity is more for carbon because it is the tendency of attracting the bonded pair of electrons towards itself, which is dependent on size of atom, small is the size more is its electronegativity. The size of B is more than C, left to right size decreases due to increase of effective nuclear charge.

5. Mg and Ca belongs to two differnt periods but same group, in Mg three shells are occupied with electrons and Ca 4 shells, more the no.of shells occupied with electrons more is the size, so Ca has more size than Mg or Mg has less size than Ca.

6. Larger radius depends on effective nuclear charge in isoatomic species{ species with same no of electrons}, more electrons less protons has more size due to less effective nuclear charge, K+ and Cl- are isoelectronic with 18 electrons each, but Cl- has 17protons and K+ has 19 protons so K+ has more effective nuclear charge hence its size is less than Cl-.

A.3. Ba has atomic number = 56, its electronic configuration shows that 6 shells are occupied with electrons and Ca has atomic number =20, its electronic configuration shows that it has 4 shells occupied with electrons, more the number of shells occupied with electrons more is the size, hence it is Ba.

B [Kr]5s24d105p4 = atomic number =52, element = Tellurium, it belongs to Oxgen family or chalcogen family or 16 group, itsmetal because of its large size it can easily loose its valence electron to become cation, has metalic lustre, last electron quantum numbers : n=5, l=1, ml= -1, 0,+1, ms=+1/2 or -1/2.

A.4. Last electron is present in p-orbital it has dumb-bell shape.

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