Question

Using the periodic table, arrange the atoms in each set in order of increasing electronegativity. a. \(\mathrm{Cl}, \mathrm{F}, \mathrm{Br}\) b. \(\mathrm{B}, \mathrm{O}, \mathrm{N}\) c. \(\mathrm{Mg}, \mathrm{F}, \mathrm{S}\)

Short answer

a) Br < Cl < F, b) B < N < O, c) Mg < S < F

Step-by-step solution

Title - Understanding Electronegativity Trend

Electronegativity increases across a period (left to right) and decreases down a group (top to bottom) in the periodic table.

Title - Order of Electronegativity for Set a

For the elements \(\text{Cl, F, Br}\), fluorine (F) is at the top-right of the periodic table, chlorine (Cl) is below fluorine, and bromine (Br) is below chlorine. The order is: increasing electronegativity is \(Br < Cl < F\).

Title - Order of Electronegativity for Set b

For the elements \(\text{B, O, N}\), boron (B) is farthest left in its period, nitrogen (N) is to the right of boron, and oxygen (O) is to the right of nitrogen. The order is: increasing electronegativity is \(B < N < O\).

Title - Order of Electronegativity for Set c

For the elements \(\text{Mg, F, S}\), magnesium (Mg) is on the far left, sulfur (S) is to the right of magnesium, and fluorine (F) is farthest right. The order is: increasing electronegativity is \(Mg < S < F\).

Key concepts

Periodic Table

The periodic table is a chart that organizes all known chemical elements based on their atomic number, electron configurations, and recurring chemical properties. The table is arranged in rows called periods and columns known as groups.
As you move from left to right across a period, the number of protons in the nucleus increases. This gives each element unique characteristics and allows scientists to predict chemical behaviors and trends.
Understanding the layout of the periodic table is crucial for determining trends like electronegativity, atomic radius, and ionization energy. Generally, elements in the same group (vertical column) share similar properties because they have the same number of valence electrons.

Electronegativity

Electronegativity refers to the ability of an atom to attract electrons towards itself in a chemical bond. This property is essential in predicting how atoms will interact when forming compounds. The most commonly used scale for electronegativity is the Pauling scale.
On the periodic table, electronegativity exhibits clear trends:

• It increases across a period from left to right.
• It decreases down a group from top to bottom.

Thus, the element fluorine (F), found at the top-right corner of the periodic table, is the most electronegative element. Electronegativity can influence the type of bond formed between two atoms, whether it's covalent or ionic.
Understanding these trends helps in predicting the behavior of different elements during chemical reactions.

Chemical Elements Order

In chemistry, arranging elements based on specific properties like electronegativity is an essential skill. It enables the prediction of chemical behaviors and the formation of compounds.
Let's look at how we order elements by their electronegativity:

• For \(\text{Cl, F, Br}\), we see that fluorine (F) is the most electronegative, followed by chlorine (Cl), and finally bromine (Br). Thus, the order is: \[ \text{Br < Cl < F} \].
• For \(\text{B, O, N}\), the sequence based on increasing electronegativity is boron (B), nitrogen (N), and then oxygen (O), i.e., \[ \text{B < N < O} \].
• For \(\text{Mg, F, S}\), magnesium (Mg) has the lowest electronegativity, followed by sulfur (S), with fluorine (F) being the highest: \[ \text{Mg < S < F} \].

By following these established trends and patterns, students can precisely arrange elements and anticipate their chemical properties.