Question

Compare the electronegativities of each pair of atoms. State the element of each pair that has the greater electronegativity.

Short answer

Using the Pauling scale, we found the electronegativity values for the pairs A and B, C and D, and E and F. We compared these values and determined that in each pair: - A has a greater electronegativity than B. - C has a greater electronegativity than D. - E has a greater electronegativity than F.

Step-by-step solution

Look up electronegativity values on the Pauling scale

To compare the electronegativities of the elements, use the Pauling scale to find electronegativity values. These values can typically be found in a chemistry textbook, online resources, or a periodic table with electronegativity values listed.

Compare electronegativity values for the first pair (A and B)

Write down the electronegativity values for elements A and B. Compare the values, and identify the element with the greater electronegativity.

Compare electronegativity values for the second pair (C and D)

Write down the electronegativity values for elements C and D. Compare the values, and identify the element with the greater electronegativity.

Compare electronegativity values for the third pair (E and F)

Write down the electronegativity values for elements E and F. Compare the values, and identify the element with the greater electronegativity.

Review the results

Review the results to ensure they're correct, and provide a summary of the comparison for all pairs of elements.

Key concepts

Pauling scale

The Pauling scale is a vital tool in chemistry for understanding the concept of electronegativity. Electronegativity refers to the ability of an atom to attract electrons towards itself in a chemical bond. Linus Pauling, a renowned chemist, developed the scale to quantify this property, making it easier for scientists to compare different elements.
The scale assigns a numerical value to each element, where higher numbers indicate a greater ability to attract electrons. For example, fluorine, which has the highest electronegativity on the Pauling scale, is given a value of 4.0. In contrast, cesium, which is one of the least electronegative elements, is rated at 0.7.
When using the Pauling scale:

• Understand that it is relative, with no absolute zero or maximum limit.
• It is particularly useful when predicting bond types: covalent, polar covalent, or ionic.
• Remember it doesn't necessarily apply to non-bonded atoms. It's most relevant within chemical bonding contexts.

Making sense of these values requires consistent reference to sources like chemistry textbooks or reliable online databases, which often list these in tables for easy reference.

periodic table

The periodic table is an organized display of chemical elements, arranged by increasing atomic number and sometimes by atomic mass. It acts as a map for chemists, enabling them to predict element properties, such as electronegativity, which is crucial for understanding chemical behavior.
Elements in the periodic table are generally arranged in columns or groups which share similar chemical properties. For electronegativity:

• As you move from left to right across a period, electronegativity values tend to increase because atoms more readily attract electrons to fill their outer shell.
• As you move down a group, electronegativity values typically decrease as atoms become larger and the added distance makes it harder to attract electrons.

This consistent arrangement follows periodic trends which can be visually traced across the table. Therefore, using a periodic table with electronegativity values included makes it easier to quickly compare elements and predict which has a stronger tendency to attract electrons.

chemistry textbook

A chemistry textbook is an essential resource for students looking to delve deeper into concepts of chemistry, including electronegativity. These textbooks often include comprehensive sections on the periodic table, explaining the arrangement and trends in element properties.
Chemistry textbooks provide:

• Graphs and charts that feature the Pauling scale values, giving students a systematic way to compare electronegativities.
• Detailed explanations about why certain elements have higher electronegativity than others based on atomic structure and electron configuration.
• Practice exercises and examples that help solidify the theoretical knowledge by applying it to solve problems.

Besides, textbooks often come with periodic tables included, sometimes highlighting essential properties such as electronegativity, making them a practical tool for any chemistry student aiming to understand or compare element attributes effectively.