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Chapter 2: Problem 61

(a) Without looking at a periodic table, list as many alkali metals as you can. (There are five common ones.) (b) Without looking at a periodic table, list as many alkaline earth metals as you can. (There are five common ones.)

Short Answer

Expert verified
Alkali metals: Li, Na, K, Rb, Cs. Alkaline earth metals: Be, Mg, Ca, Sr, Ba.

Step by step solution

01

Recall Alkali Metals

Alkali metals are characterized by having one electron in their outermost shell, which makes them highly reactive. They are found in Group 1 of the periodic table. The common alkali metals include: Lithium (Li), Sodium (Na), Potassium (K), Rubidium (Rb), and Cesium (Cs). Francium is also an alkali metal, but it is less common.
02

Recall Alkaline Earth Metals

Alkaline earth metals have two electrons in their outer shell and are found in Group 2 of the periodic table. The common alkaline earth metals include: Beryllium (Be), Magnesium (Mg), Calcium (Ca), Strontium (Sr), and Barium (Ba). Radium is also an alkaline earth metal, but it is radioactive and less frequently discussed.

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Key Concepts

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

Alkaline Earth Metals
Alkaline earth metals have a unique spot on the periodic table, residing in Group 2. These elements are known for their two electrons in the outermost shell, which defines their chemical characteristics. Because of this electron configuration, alkaline earth metals are less reactive than alkali metals but are still quite reactive. Alkaline earth metals include:
  • Beryllium (Be)
  • Magnesium (Mg)
  • Calcium (Ca)
  • Strontium (Sr)
  • Barium (Ba)
Remembering these elements can be made easier with the mnemonic: "Bears Might Catch Strange Balls." Maybe not the most famous metals, but they play significant roles in fields like industry and biology.
For instance, calcium is crucial for healthy bones!
Periodic Table
The periodic table is a structured chart that organizes all known elements based on increasing atomic number and recurring chemical properties. It is a powerful tool that helps scientists predict the behavior of elements and their compounds.
  • The periodic table is divided into groups (vertical columns) and periods (horizontal rows).
  • Elements in the same group share similar properties since they have the same number of electrons in their outer shell.
  • The table allows us to understand relationships between elements and recognize patterns, such as reactivity and electronegativity.
The structure of the periodic table aids in memorizing elemental properties and predicting how they might react chemically.
Electron Configuration
Electron configuration refers to the arrangement of electrons in an atom's electron shells. Each element has a unique electron configuration that influences its chemical behavior and reactivity.
  • Electrons are arranged in shells around the nucleus, occupying subshells designated as 's', 'p', 'd', and 'f'.
  • The configuration follows a specific order: starting from the lowest energy level to higher ones.
  • A full outer shell implies stability, influencing whether an element is likely to gain, lose, or share electrons during chemical interactions.
Understanding electron configurations helps explain the placement of elements in the periodic table and their role in chemical reactions.
Group 1 Elements
Group 1 elements, also known as alkali metals, are highly reactive and found on the far left of the periodic table. They include:
  • Lithium (Li)
  • Sodium (Na)
  • Potassium (K)
  • Rubidium (Rb)
  • Cesium (Cs)
  • Francium (Fr)
All alkali metals have one electron in their outermost shell, which they readily lose to form positive ions (cations). This tendency makes them highly reactive, particularly with water, often resulting in explosive reactions!
These metals are typically soft and can be cut with a knife.
Group 2 Elements
Group 2 elements, known as alkaline earth metals, boast two electrons in their outer shell. Located next to the alkali metals, these elements share some similarities, yet have distinct characteristics.
  • They are less reactive than Group 1 elements, but will still react, especially with water and acids.
  • Their two outer electrons make them more likely to form compounds by losing two electrons, leading to the creation of divalent cations (2+ charge).
  • Some common uses include magnesium in alloys and dietary supplements, along with calcium playing a vital role in biological systems like bone formation.
Understanding the characteristics of Group 2 elements can help in various fields such as chemistry, biology, and material science.

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Most popular questions from this chapter

In methane, one part hydrogen combines with three parts carbon by mass. If a sample of a compound containing only carbon and hydrogen contains \(32.0 \mathrm{~g}\) of carbon and \(8.0 \mathrm{~g}\) of hydrogen, could the sample be methane? If the sample is not methane, show that the law of multiple proportions is followed for methane and this other substance.

In an alternate universe, the smallest negatively charged particle, analogous to our electron, is called a blorvek. To determine the charge on a single blorvek, an experiment like Millikan's with charged oil droplets was carried out and the following results were recorded: $$ \begin{array}{cl} \hline \text { Droplet Number } & \text { Charge(C) } \\ \hline 1 & 7.74 \times 10^{-16} \\ 2 & 4.42 \times 10^{-16} \\ 3 & 2.21 \times 10^{-16} \\ 4 & 4.98 \times 10^{-16} \\ 5 & 6.64 \times 10^{-16} \\ \hline \end{array} $$ (a) Based on these observations, what is the largest possible value for the charge on a blorvek? (b) Further experiments found a droplet with a charge of \(5.81 \times 10^{-16} \mathrm{C}\). Does this new result change your answer to part (a)? If so, what is the new largest value for the blorvek's charge?

At room temperature, a certain element is a colorless, unreactive gas. Is the element likely to be a metal, a nonmetal, or a semimetal?

If the atomic weight of an element is \(x\), what is the mass in grams of \(6.02 \times 10^{23}\) atoms of the element? How does your answer compare numerically with the atomic weight of element \(x ?\)

A sample of mercury with a mass of \(114.0 \mathrm{~g}\) was combined with \(12.8 \mathrm{~g}\) of oxygen gas, and the resulting reaction gave \(123.1 \mathrm{~g}\) of mercury(II) oxide. How much oxygen was left over after the reaction was complete?
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