Question

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

Short answer

The valence electrons for the given elements are: a. Ca: 2 valence electrons (4s^2) b. O: 6 valence electrons (2s^2 2p^4) c. Ts: 7 valence electrons (7s^2 7p^5) d. In: 3 valence electrons (5s^2 5p^1) e. Ar: 8 valence electrons (3s^2 3p^6) f. Bi: 5 valence electrons (6s^2 6p^3)

Step-by-step solution

Find the position of the elements in the periodic table

Locate the elements in the periodic table using their symbols. Note down their group numbers which will help in determining the valence electrons.

Determine the valence electrons

For most elements (except transition metals and inner transition metals), the group number (also called the family number) indicates the number of valence electrons. For example, elements in Group 1 have 1 valence electron, Group 2 elements have 2 valence electrons, and so on. Now, let's determine the valence electrons for the given elements. a. Calcium (Ca) is in Group 2. Therefore, it has 2 valence electrons (specifically 4s^2). b. Oxygen (O) is in Group 16. As Group 16 is called the chalcogens (also known as Group 6A), oxygen has 6 valence electrons (specifically 2s^2 2p^4). c. Element 117, Tennessine (Ts), is in Group 17, which is also known as the halogens (Group 7A). It has 7 valence electrons (specifically 7s^2 7p^5). d. Indium (In) is in Group 13, which is also called the boron family (Group 3A). It has 3 valence electrons (specifically 5s^2 5p^1). e. Argon (Ar) is in Group 18, known as the noble gases (Group 8A). It has 8 valence electrons (specifically 3s^2 3p^6). f. Bismuth (Bi) is in Group 15, known as the pnictogens (Group 5A). It has 5 valence electrons (specifically 6s^2 6p^3).

Key concepts

Periodic Table

The periodic table is a comprehensive chart that organizes all known elements by their atomic number, electron configuration, and recurring chemical properties. It places elements into rows called periods and columns called groups. Each element's position gives valuable information about its characteristics.
The periodic table is crucial for predicting element behavior and interactions in chemical reactions.

• It divides elements into metals, nonmetals, and metalloids based on shared properties.
• It helps chemists understand relationships between elements and predict potential properties and reactions.

By providing a structured visualization, the periodic table remains an essential tool in the field of chemistry.

Group Numbers

Group numbers in the periodic table indicate the number of valence electrons present in an element. Valence electrons are the electrons in the outermost shell and are vital for chemical bonding and reactions.
Every group number represents a column of the periodic table.

• Elements in Group 1 have one valence electron and are highly reactive.
• Group 2 elements have two valence electrons, often forming compounds like oxides.
• Groups 13 to 18 have increasing valence electrons, impacting their stability and bonding tendencies.

Knowing the group number helps in determining chemical reactivity and properties.

Electron Configuration

Electron configuration describes the distribution of electrons in an atom's orbitals. It determines an atom's chemical behavior and how it interacts with others. Electrons occupy energy levels or "shells," starting closest to the nucleus.
The configuration is expressed using for example the notation like 1s^2, where '1' is the energy level, 's' is the type of orbital, and '2' is the number of electrons in that orbital.

• This notation helps in identifying valence electrons which are involved in chemical bonds.
• Elements with similar electron configurations exhibit similar chemical properties.

Understanding electron configuration is key to mastering chemistry basics.

Elements

Elements are pure substances consisting of only one type of atom, characterized by a specific number of protons known as the atomic number. Each element has unique properties and symbol.

• Atoms of the same element share chemical properties.
• Elements can combine to form compounds through chemical bonds.

There are over 100 known elements, ranging from hydrogen, the simplest element, to more complex elements like uranium.
Each element's position in the periodic table provides insight into its properties and potential chemical interactions.

Chemical Properties

Chemical properties describe how a substance interacts with other substances, leading to chemical changes. They are influenced by the number of valence electrons and electron configuration.
Chemical properties determine how an element will behave in chemical reactions.

• Reactivity: Some elements, like alkali metals, are more reactive due to having one valence electron.
• Electronegativity: This is the tendency of an atom to attract electrons. It increases across a period and decreases down a group.
• Acidic or basic behavior: This is based on the ability to donate or accept protons in reactions.

These properties are essential for predicting how elements will interact in biological systems and industrial applications.