Questions: Arrange the following set of elements in order of increasing atomic size: a. Sr, Te, Sn, Xe Sr<Xe<Sn<Te Xe<Te<Sn<Sr Xe<Sr<Te<Sn b. Sn, C, Si C<Pb<Si<Sn C<Si<Sn<Pb Sn<C<Si<Pb c. Rn, Po, Ba Rn<Po<Pb<Ba Rn<Ba<Po<Pb Ba<Pb<Rn<Po

Arrange the following set of elements in order of increasing atomic size: a. Sr, Te, Sn, Xe Sr<Xe<Sn<Te Xe<Te<Sn<Sr Xe<Sr<Te<Sn b. Sn, C, Si C<Pb<Si<Sn C<Si<Sn<Pb Sn<C<Si<Pb c. Rn, Po, Ba Rn<Po<Pb<Ba Rn<Ba<Po<Pb Ba<Pb<Rn<Po
Transcript text: Arrange the following set of elements in order of increasing atomic size: a. $\mathrm{Sr}, \mathrm{Te}, \mathrm{Sn}, \mathrm{Xe}$ $\mathrm{Sr}<\mathrm{Xe}<\mathrm{Sn}<\mathrm{Te}$ $\mathrm{Xe}<\mathrm{Te}<\mathrm{Sn}<\mathrm{Sr}$ $\mathrm{Xe}<\mathrm{Sr}<\mathrm{Te}<\mathrm{Sn}$ b. $\mathrm{Sn}, \mathrm{C}, \mathrm{Si}$ $\mathrm{C}<\mathrm{Pb}<\mathrm{Si}<\mathrm{Sn}$ $\mathrm{C}<\mathrm{Si}<\mathrm{Sn}<\mathrm{Pb}$ $\mathrm{Sn}<\mathrm{C}<\mathrm{Si}<\mathrm{Pb}$ c. $\mathrm{Rn}, \mathrm{Po}, \mathrm{Ba}$ $\mathrm{Rn}<\mathrm{Po}<\mathrm{Pb}<\mathrm{Ba}$ $\mathrm{Rn}<\mathrm{Ba}<\mathrm{Po}<\mathrm{Pb}$ $\mathrm{Ba}<\mathrm{Pb}<\mathrm{Rn}<\mathrm{Po}$
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Solution

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Solution Steps

Step 1: Understanding Atomic Size Trends

Atomic size generally increases as you move down a group in the periodic table because additional electron shells are added. Conversely, atomic size decreases as you move across a period from left to right due to increased nuclear charge pulling electrons closer to the nucleus.

Step 2: Analyzing the First Set of Elements

The elements given are Sr, Te, Sn, and Xe. These elements are located in the following positions on the periodic table:

  • Sr (Strontium) is in Group 2, Period 5.
  • Te (Tellurium) is in Group 16, Period 5.
  • Sn (Tin) is in Group 14, Period 5.
  • Xe (Xenon) is in Group 18, Period 5.

Since all these elements are in the same period, we compare them based on their group number. Atomic size decreases from left to right across a period. Therefore, the order of increasing atomic size is:

  • Xe < Te < Sn < Sr
Step 3: Analyzing the Second Set of Elements

The elements given are Sn, C, Si, and Pb. These elements are located in the following positions on the periodic table:

  • Sn (Tin) is in Group 14, Period 5.
  • C (Carbon) is in Group 14, Period 2.
  • Si (Silicon) is in Group 14, Period 3.
  • Pb (Lead) is in Group 14, Period 6.

Since these elements are in the same group, atomic size increases as you move down the group. Therefore, the order of increasing atomic size is:

  • C < Si < Sn < Pb

Final Answer

  • For the first set of elements: \(\boxed{\text{Xe < Te < Sn < Sr}}\)
  • For the second set of elements: \(\boxed{\text{C < Si < Sn < Pb}}\)
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