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Chapter 2: Problem 22

Define, with two examples, the following terms: (a) alkali metals, (b) alkaline earth metals, (c) halogens, (d) noble gases.

Short Answer

Expert verified
Alkali metals are highly reactive metals with one electron in their outer shell like Lithium and Sodium. Alkaline earth metals are less reactive with two outer shell electrons like Beryllium and Magnesium. Halogens are very reactive non-metals with seven outer shell electrons like Fluorine and Chlorine. Noble gases are the least reactive due to full outer shells, such as Helium and Neon.

Step by step solution

01

- Defining alkali metals with examples

Alkali metals are elements from Group 1 of the periodic table, excluding hydrogen. They have one electron in their outer shell and are highly reactive metals with low densities. Examples include Lithium (Li), Sodium (Na).
02

- Defining alkaline earth metals with examples

Alkaline earth metals are elements from Group 2 of the periodic table. They have two electrons in their outer shell and are less reactive than alkali metals but more reactive than most other elements. Examples include Beryllium (Be), Magnesium (Mg).
03

- Defining halogens with examples

Halogens are elements from Group 17 of the periodic table. They have seven electrons in their outer shell and are very reactive nonmetals. They are known to gain an electron to achieve a stable electron configuration. Examples include Fluorine (F), Chlorine (Cl).
04

- Defining noble gases with examples

Noble gases are elements from Group 18 of the periodic table. They have full electron shells, generally making them highly unreactive. Examples include Helium (He), Neon (Ne).

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Alkali Metals
Alkali metals are characterized by their single electron in the outermost shell, which contributes to their notable reactivity.

Found in Group 1 of the periodic table, these metals are shiny, soft, and have low melting points. Due to their high reactivity, they are usually not found in their elemental form in nature but rather in compounds. When interacting with water, they produce an alkaline solution; hence the name 'alkali'.

Common Examples

  • Lithium (Li): Used in batteries and as a treatment for bipolar disorder.
  • Sodium (Na): Extensively used in the culinary world as table salt and has applications in industry such as in the production of paper and soap.
Alkaline Earth Metals
Alkaline earth metals possess two electrons in their outer shell, offering them somewhat less reactivity compared to alkali metals.

These metals make up Group 2 on the periodic table and include several elements that are important to everyday life. They are also shiny and somewhat reactive, typically forming oxides or hydroxides when exposed to air or water.

Common Examples

  • Beryllium (Be): Used in aerospace materials for its light weight and high stiffness.
  • Magnesium (Mg): Important in biological systems, it is also used in products like flares and fireworks due to its bright white flame.
Halogens
Halogens are unique due to their seven valence electrons, which drive their high reactivity, particularly their tendency to gain an electron to form a complete octet.

Occupying Group 17 of the periodic table, these nonmetals are powerful oxidizing agents and have significant disinfectant properties. They are rarely encountered in their elemental form in the environment because they readily form compounds with metals.

Common Examples

  • Fluorine (F): Predominantly found in compounds like fluoride, which is added to toothpaste and water for dental health benefits.
  • Chlorine (Cl): Widely used to purify water, including in swimming pools, and as a bleaching agent.
Noble Gases
Noble gases are recognized for their filled electron shells and inherent lack of reactivity, making them very stable.

These odorless, colorless, and tasteless gases constitute Group 18 of the periodic table. Because of their low reactivity, they don't typically form compounds and are found in their pure form in the atmosphere. Their stability makes them ideal for use in non-reactive applications.

Common Examples

  • Helium (He): The lightest of the noble gases, used in balloons and as a cooling medium for superconducting magnets like those in MRI machines.
  • Neon (Ne): Best known for its use in neon signs, where it emits a characteristic bright red-orange light.

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Most popular questions from this chapter

What do we call atoms of the same elements with different mass numbers?

Name these compounds: (a) \(\mathrm{KClO}\) (b) \(\mathrm{Ag}_{2} \mathrm{CO}_{3}\) (c) \(\mathrm{FeCl}_{2}\), (d) \(\mathrm{KMnO}_{4}\), (e) \(\mathrm{CsClO}_{3}\), (f) \(\mathrm{HIO},(\mathrm{g}) \mathrm{FeO}\), (h) \(\mathrm{Fe}_{2} \mathrm{O}_{3}\) (i) \(\mathrm{TiCl}_{4},(\mathrm{j}) \mathrm{NaH},(\mathrm{k}) \mathrm{Li}_{3} \mathrm{~N},\) (1) \(\mathrm{Na}_{2} \mathrm{O}\) (m) \(\mathrm{Na}_{2} \mathrm{O}_{2},\) (n) \(\mathrm{FeCl}_{3} \cdot 6 \mathrm{H}_{2} \mathrm{O}\).

What are the empirical formulas of the following compounds? (a) \(\mathrm{Al}_{2} \mathrm{Br}_{6}\) (b) \(\mathrm{Na}_{2} \mathrm{~S}_{2} \mathrm{O}_{4}\) (c) \(\mathrm{N}_{2} \mathrm{O}_{5}\) (d) \(\mathrm{K}_{2} \mathrm{Cr}_{2} \mathrm{O}_{7}\)

Calculate the number of neutrons in \({ }^{239} \mathrm{Pu}\).

The elements in Group 8 A of the periodic table are called noble gases. Can you suggest what "noble" means in this context?
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