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Ch. 4 - Acids and Bases: Electron Flow
Mullins - Organic Chemistry: A Learner Centered Approach 1st Edition
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All textbooksMullins 1st EditionCh. 4 - Acids and Bases: Electron FlowProblem 6b
Chapter 3, Problem 6b

In each pair of atoms, which has the larger atomic radius? Which is more electronegative?
(b) C vs. O

Verified step by step guidance
1
Step 1: Understand the periodic trends for atomic radius and electronegativity. Atomic radius generally decreases across a period (left to right) in the periodic table, while electronegativity increases across a period.
Step 2: Locate the elements Carbon (C) and Oxygen (O) on the periodic table. Both are in the same period (Period 2), with Carbon in Group 14 and Oxygen in Group 16.
Step 3: Compare atomic radii. Since atomic radius decreases across a period, Carbon (C), being to the left of Oxygen (O), will have a larger atomic radius.
Step 4: Compare electronegativity. Electronegativity increases across a period, so Oxygen (O), being to the right of Carbon (C), will be more electronegative.
Step 5: Summarize the findings. Carbon has the larger atomic radius, while Oxygen is more electronegative. These trends are consistent with periodic table properties.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Atomic Radius

Atomic radius refers to the size of an atom, typically measured from the nucleus to the outermost electron shell. Generally, atomic radius increases down a group in the periodic table due to the addition of electron shells, while it decreases across a period from left to right due to increased nuclear charge, which pulls electrons closer to the nucleus.
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The difference between atomic numbers and atomic mass.

Electronegativity

Electronegativity is a measure of an atom's ability to attract and hold onto electrons in a chemical bond. It generally increases across a period from left to right and decreases down a group. This trend is important for predicting how atoms will interact in chemical reactions, particularly in determining bond polarity.
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Electronegativity

Periodic Trends

Periodic trends refer to the predictable patterns observed in the properties of elements as you move across or down the periodic table. Key trends include atomic radius, electronegativity, ionization energy, and electron affinity. Understanding these trends helps in comparing elements and predicting their chemical behavior.
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Related Practice
Textbook Question

In each pair of atoms, which has the larger atomic radius? Which is more electronegative?

(c) O vs. S

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Textbook Question

Sodium amide (NaNH₂) dissociates to give a sodium cation (Na+) and amide ion (NH2–) a very strong base. In the following three equations, identify which definition of base is being exemplified.

(b)

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Textbook Question

Sodium amide (NaNH2) dissociates to give a sodium cation (Na+) and amide ion (NH2-) a very strong base. In the following three equations, identify which definition of base is being exemplified.

(a)

Textbook Question

For the following acid–base pairs, (v) show a mechanism for the reaction;

(e)

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Textbook Question

Draw the molecular orbital picture of the following molecules and ions. In each, how many electrons are in the p orbital on the central atom? (b) BH3

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Textbook Question

Draw the molecular orbital picture of the following molecules and ions. In each, how many electrons are in the p orbital on the central atom? (c) AlCl3

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