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Ch. 2 - General Chemistry Translated: Finding the Electrons
Mullins - Organic Chemistry: A Learner Centered Approach 1st Edition
Mullins1st EditionOrganic Chemistry: A Learner Centered ApproachISBN: 9780137566471당신이 사용하는 게 아니라요?교과서 변경
모든 교과서Mullins 1st EditionCh. 2 - General Chemistry Translated: Finding the Electrons문제 28d
1장, 문제 28d

Calculate the formal charge of the indicated atom in the following molecules or ions.
(d) Structural formula of a molecule with an arrow pointing to a nitrogen atom, indicating where to calculate formal charge.

검증된 단계별 안내
1
Step 1: Recall the formula for calculating formal charge: Formal Charge = (Valence Electrons) - (Non-bonding Electrons) - (1/2 × Bonding Electrons).
Step 2: Identify the atom in question and determine the number of valence electrons it has based on its position in the periodic table.
Step 3: Count the number of non-bonding electrons (lone pairs) around the atom. Each lone pair contributes 2 electrons.
Step 4: Count the number of bonding electrons (shared electrons in bonds) around the atom. Each bond contributes 2 electrons, but only half of these are assigned to the atom in question.
Step 5: Substitute the values for valence electrons, non-bonding electrons, and bonding electrons into the formula to calculate the formal charge of the atom.

비슷한 문제에 대한 검증된 영상 답변:

이 영상 해법은 위 문제에 도움이 된다고 튜터들이 추천한 것입니다.
영상 길이:
1m

주요 개념

질문에 올바르게 답하기 위해 반드시 이해해야 하는 핵심 개념들은 다음과 같습니다.

Formal Charge

Formal charge is a theoretical charge assigned to an atom in a molecule, calculated based on the number of valence electrons, the number of non-bonding electrons, and the number of bonds. The formula is: Formal Charge = Valence Electrons - (Non-bonding Electrons + 1/2 Bonding Electrons). This concept helps in understanding the distribution of electrons in a molecule and assessing the stability of different resonance structures.
추천 영상:
01:34
Calculating formal and net charge.

Lewis Structures

Lewis structures are diagrams that represent the bonding between atoms in a molecule and the lone pairs of electrons that may exist. They provide a visual representation of the arrangement of electrons and help in predicting the formal charge of atoms. Understanding how to draw and interpret Lewis structures is essential for calculating formal charges accurately.
추천 영상:
04:12
Drawing the Lewis Structure for N2H4.

Resonance Structures

Resonance structures are different ways of drawing the same molecule that show the delocalization of electrons. They are used when a single Lewis structure cannot adequately represent the electron distribution. Recognizing resonance structures is important for understanding the stability of a molecule and the implications for formal charge, as the actual structure is a hybrid of all possible resonance forms.
추천 영상:
03:04
Drawing Resonance Structures
관련 실천
교과서 질문

Calculate the formal charge of the indicated atom in the following molecules or ions.

(e)

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교과서 질문

Draw the Lewis structure for the following molecules. Be sure to calculate the formal charge of each atom as a way of confirming your structure is correct.

(b) HOBr

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교과서 질문

Using only your intuition, rank the following covalent bonds in terms of their polarity (1 = most polar; 6 = least polar). [You can use the periodic trend of electronegativity, but don't use actual numbers.]

(a) C―C

(b) C―O

(c) C―H

(d) C―F

(e) C―Cl

(f) C―S

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교과서 질문

Calculate the formal charge of the indicated atom in the following molecules or ions.

(f)

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교과서 질문

Draw the Lewis structure for the following ions. Be sure to calculate the formal charge of each atom to confirm that your structure is correct.

(b) H+

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교과서 질문

Draw the Lewis structure for the following molecules. Be sure to calculate the formal charge of each atom as a way of confirming your structure is correct.

(c) CF4

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