Question

Order the following elements according to decreasing electronegativity: \(\mathrm{C}, \mathrm{Ca}, \mathrm{Cs}, \mathrm{Cl}, \mathrm{Cu}\).

Short answer

The order is: Cl > C > Cu > Ca > Cs.

Step-by-step solution

Understanding Electronegativity

Electronegativity is a measure of the tendency of an atom to attract a bonding pair of electrons. It generally increases across a period (from left to right in the periodic table) and decreases down a group (top to bottom).

Locating Elements on the Periodic Table

Identify the position of the elements on the periodic table: 1. Carbon (C) is in group 14, period 2. 2. Calcium (Ca) is in group 2, period 4. 3. Cesium (Cs) is in group 1, period 6. 4. Chlorine (Cl) is in group 17, period 3. 5. Copper (Cu) is in group 11, period 4.

Applying general trends in Electronegativity

Using the periodic table - Chlorine (Cl) is known to have high electronegativity as it is one of the halogens. - Carbon (C) also has relatively high electronegativity. - Copper (Cu) has moderate electronegativity being a transition metal. - Calcium (Ca) and Cesium (Cs) have lower electronegativities as they are metals, with Cesium being lower than Calcium due to it being further down the group.

Order Elements by Electronegativity

Using the known trends, we can order the elements from highest to lowest electronegativity: Chlorine (Cl), Carbon (C), Copper (Cu), Calcium (Ca), Cesium (Cs).

Key concepts

Periodic Table

The periodic table is an organized chart of elements, arranged based on increasing atomic number. It reveals important trends and properties of the elements. For instance, electronegativity, which is crucial for understanding how atoms bond, tends to increase as you move from left to right across a period. This is because elements on the right side of the table tend to have a greater number of protons, drawing electrons more strongly towards them. Conversely, as you move down a group, electronegativity decreases. This occurs because the additional electron shells cause the outer electrons to be farther from the nucleus, reducing the attractive force. Therefore, using the periodic table not only helps to locate elements like carbon (C), calcium (Ca), cesium (Cs), chlorine (Cl), and copper (Cu), but also to predict their relative electronegativities through their position in it.

Chemical Bonding

Chemical bonding describes the process of atoms joining to form molecules or compounds. It largely depends on the electronegativity of the elements involved. Electronegativity differences can dictate the type of bond formed. If two atoms have similar electronegativities, they are likely to share electrons equally, forming a covalent bond. For example, carbon atoms in organic compounds typically form covalent bonds due to their comparable electronegativity values with other nonmetals.

• If there is a noticeable difference in electronegativity, as seen between chlorine and many metals, the result is often an ionic bond. In such materials, electrons are transferred from one atom to another.
• Transition metals like copper present a unique case as they can display variable electronegativities, allowing for a variety of bonding possibilities, including metallic bonds.

Understanding these concepts helps to predict the structural characteristics and reactivity of substances.

Atomic Properties

Atomic properties include various attributes of atoms that dictate their chemical behavior. Electronegativity is one such property, impacting how an atom attracts electrons within bonds. Several factors affect electronegativity:

• Atomic Radius: As the atomic radius increases, the nucleus has less pull on the valence electrons, resulting in lower electronegativity.
• Nuclear Charge: A higher positive charge in the nucleus increases an atom's ability to attract electrons.
• Electron Shielding: Electrons in inner shells can shield outer electrons from the nucleus' pull, thus reducing electronegativity.

Moreover, each group and period in the periodic table affects these properties in predictable ways. Knowing the atomic properties allows us to understand why chlorine (Cl) has a much higher electronegativity than cesium (Cs), as Cl is smaller and experiences reduced electron shielding, enhancing its ability to attract electrons. Mastering these properties is key to understanding the behavior of elements in chemical reactions.