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Chapter 3: Problem 19

What would the periodicity be if the transition metals, lanthanides, and actinides were removed from the periodic table?

Short Answer

Expert verified
If the transition metals, lanthanides, and actinides were removed from the periodic table, the new periodicity would be 6, as there would be 6 elements in periods 2 through 7 (excluding Period 1, which only contains 2 elements, hydrogen and helium).

Step by step solution

01

Determine the elements that will be removed

In this problem, we need to remove the transition metals, lanthanides, and actinides from the periodic table. The transition metals are the elements found in groups 3-12, the lanthanides are elements 57-70, and the actinides are elements 89-102.
02

Determine the remaining elements

If we remove the above-mentioned elements, we'll be left with elements from groups 1-2 (alkali and alkaline earth metals) and groups 13-18 (the p-block elements). These are also referred to as representative elements.
03

Understand the periodicity of the representative elements

Recall that the periodicity of a periodic table is determined by the number of elements in a period (row). In the modified table, we observe the following pattern for the number of elements in each period: Period 1: 2 elements (H, He) Period 2: 6 elements Period 3: 6 elements Period 4: 6 elements Period 5: 6 elements Period 6: (including f-block elements) 6 elements Period 7: (including f-block elements) 6 elements
04

Determine the new periodicity of the table

Based on the number of elements in each period after removing the transition metals, lanthanides, and actinides, we can conclude that the periodicity of the modified periodic table would be 6. There would be 6 elements in periods 2 through 7 (excluding Period 1, which only contains 2 elements, hydrogen and helium).

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Most popular questions from this chapter

While an atom's mass number and its atomic mass are not the same, they are often quite close to one another. Consider the following: Uranium- 235 has an atomic mass of \(235.04393\) amu and a percent abundance of \(0.73 \%\). Uranium-238 has an atomic mass of \(238.0508\) amu and a percent abundance of \(99.27 \%\). Without doing any calculations or consulting any other sources, which of the following do you think represents the atomic mass of naturally occurring uranium? (a) \(234.04 \mathrm{amu}\) (b) \(236.03 \mathrm{amu}\) (c) \(237.03\) amu (d) \(238.03\) amu (e) \(238.07\) amu Explain how you made your choice.

Explain why the first and second statements of Dalton's atomic theory are not exactly true.

What is the trend in first ionization energy as you go down a given group in the periodic table? As you go across a period from left to right?

It always takes energy to remove an electron from a neutral atom. Explain why, and name the minimum amount of energy it takes to do this.

Naturally occurring hydrogen on Earth has an atomic mass of \(1.0079\) amu. Suppose you were on another planet and found the atomic mass of hydrogen to be \(1.2000\) amu. How would you explain this? (The atomic mass of \({ }_{1}^{1} \mathrm{H}\) is \(1.0078252\) amu; the atomic mass of \({ }_{1}^{2} \mathrm{H}\) is \(2.1041022\) amu.)
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