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Chapter 7: Problem 100

Arrange the following groups of atoms in order of increasing size. a. \(\mathrm{Rb}, \mathrm{Na}, \mathrm{Be}\) b. \(\mathrm{Sr}, \mathrm{Se}, \mathrm{Ne}\) c. \(\mathrm{Fe}, \mathrm{P}, \mathrm{O}\)

Short Answer

Expert verified
The order of increasing size for the given groups of atoms is: a. \(\mathrm{Be} < \mathrm{Na} < \mathrm{Rb}\) b. \(\mathrm{Ne} < \mathrm{Se} < \mathrm{Sr}\) c. \(\mathrm{O} < \mathrm{P} < \mathrm{Fe}\)

Step by step solution

01

Determine the position of elements in the periodic table

Rb is in Group 1 and Period 5, Na is in Group 1 and Period 3, and Be is in Group 2 and Period 2.
02

Compare the size based on group and period

We know that the atomic size increases down the group and decreases from left to right across a period. Comparing the given elements, we see that Be is the smallest due to being in Period 2, and Rb is the largest due to being in Period 5.
03

Arrange the atoms in order of increasing size

Based on the analysis, the order of increasing size is: \[\mathrm{Be} < \mathrm{Na} < \mathrm{Rb}.\] b. Arrange the atoms \(\mathrm{Sr}, \mathrm{Se}, \mathrm{Ne}\) in order of increasing size.
04

Determine the position of elements in the periodic table

Sr is in Group 2 and Period 5, Se is in Group 16 and Period 4, and Ne is in Group 18 and Period 2.
05

Compare the size based on group and period

Comparing the given elements, we see that Ne is the smallest due to being in Period 2, and Sr is the largest due to being in Period 5.
06

Arrange the atoms in order of increasing size

Based on the analysis, the order of increasing size is: \[\mathrm{Ne} < \mathrm{Se} < \mathrm{Sr}.\] c. Arrange the atoms \(\mathrm{Fe}, \mathrm{P}, \mathrm{O}\) in order of increasing size.
07

Determine the position of elements in the periodic table

Fe is in Group 8 and Period 4, P is in Group 15 and Period 3, and O is in Group 16 and Period 2.
08

Compare the size based on group and period

Comparing the given elements, we see that O is the smallest due to being in Period 2, and Fe is the largest due to being in Period 4.
09

Arrange the atoms in order of increasing size

Based on the analysis, the order of increasing size is: \[\mathrm{O} < \mathrm{P} < \mathrm{Fe}.\] So, the order of increasing size is as follows: a. \(\mathrm{Be} < \mathrm{Na} < \mathrm{Rb}\) b. \(\mathrm{Ne} < \mathrm{Se} < \mathrm{Sr}\) c. \(\mathrm{O} < \mathrm{P} < \mathrm{Fe}\)

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Most popular questions from this chapter

Which of elements 1-36 have one unpaired electron in the ground state?

Are the following statements true for the hydrogen atom only, true for all atoms, or not true for any atoms? a. The principal quantum number completely determines the energy of a given electron. b. The angular momentum quantum number, \(\ell\), determines the shapes of the atomic orbitals. c. The magnetic quantum number, \(m_{\ell}\), determines the direction that the atomic orbitals point in space.

Which of elements 1-36 have two unpaired electrons in the ground state?

How many valence electrons do each of the following elements have, and what are the specific valence electrons for each element? a. \(\mathrm{Ca}\) b. \(\mathrm{O}\) c. element 117 d. In e. Ar f. \(\mathrm{Bi}\)

Predict some of the properties of element 117 (the symbol is Uus, following conventions proposed by the International Union of Pure and Applied Chemistry, or IUPAC). a. What will be its electron configuration? b. What element will it most resemble chemically? c. What will be the formula of the neutral binary compounds it forms with sodium, magnesium, carbon, and oxygen? d. What oxyanions would you expect Uus to form?
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