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Chapter 4: Problem 65

According to Bohr, why do atoms in the same group in the periodic table have similar chemical properties?

Short Answer

Expert verified
According to Bohr's atomic model, atoms in the same group in the periodic table have similar chemical properties because they have the same number of valence electrons (outermost shell electrons), which play a significant role in determining the chemical properties of elements through interactions during chemical reactions.

Step by step solution

01

Briefly describe Bohr's atomic model

Niels Bohr's atomic model, proposed in 1913, states that electrons orbit the nucleus of an atom in distinct energy levels or "shells". Each shell can only hold a specific number of electrons. The arrangement of these electrons in the shells determines the chemical properties of the atoms.
02

Define the concept of groups in the periodic table

In the periodic table, elements are arranged in columns called "groups". Elements within the same group have similar chemical properties and generally exhibit a periodic pattern in their physical and chemical properties. This similarity and pattern arise due to the similar electron configurations of the elements in a group, particularly their outermost or valence electron configuration.
03

Explain the relationship between electron arrangement and chemical properties

In Bohr's atomic model, chemical properties of elements are determined by their electron configuration, particularly the outermost shell (valence shell). Elements in the same group have similar valence electron configurations, which means they have the same number of electrons in their outermost shell. This similarity in electron configuration results in similar chemical properties because chemical reactions typically involve the interaction of the valence electrons between atoms.
04

Example - Group 1 elements

For example, elements in the Group 1 of the periodic table, like lithium (Li), sodium (Na), and potassium (K), possess one electron in their outermost shell. Due to this similar electron configuration, they share similarities in their chemical properties such as high reactivity with water and relatively low ionization energies. In conclusion, according to Bohr's atomic model, atoms in the same group in the periodic table have similar chemical properties because they have the same number of valence electrons (outermost shell electrons), which play a significant role in determining the chemical properties of elements through interactions during chemical reactions.

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Most popular questions from this chapter

Write electron configurations for \(\mathrm{O}, \mathrm{O}^{2+}\), and \(\mathrm{O}^{2-}\). Which form would you expect to find in most compounds of oxygen? Why?

Name each element and tell how many valence electrons it has: (a) \(1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{2}\) (b) \([\mathrm{Ne}] 3 \mathrm{~s}^{1}\) (c) \([\mathrm{Ar}] 4 s^{2} 3 d^{10} 4 p^{3}\)

Consider the anion whose charge is \(2^{-}\) and whose electron configuration is identical to that of argon, Ar. What is the symbol for this anion?

Why are the \(s, p, d\), and \(f\) blocks in the periodic table \(2,6,10\), and 14 blocks wide, respectively?

A laser emits a beam of green light that has a wavelength of \(5.00 \times 10^{-5} \mathrm{~cm} .\) What is the wavelength of this light in nanometers?
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