Skip to main content
Ch. 1 - Remembering General Chemistry: Electronic Structure and Bonding
Bruice - Organic Chemistry 8th Edition
Bruice8th EditionOrganic ChemistryISBN: 9780135213711당신이 사용하는 게 아니라요?교과서 변경
모든 교과서Bruice 8th EditionCh. 1 - Remembering General Chemistry: Electronic Structure and Bonding문제 16a,b
1장, 문제 16a,b

Give each atom the appropriate formal charge:
a.
b.

검증된 단계별 안내
1
Step 1: Recall the formula for calculating formal charge: Formal charge = (Valence electrons of the atom) - (Non-bonding electrons) - (1/2 × Bonding electrons).
Step 2: For the first molecule (CH3-O-CH3 with a hydrogen attached to oxygen), calculate the formal charge of each atom. Oxygen has 6 valence electrons, 4 non-bonding electrons (two lone pairs), and is involved in 3 bonds (6 bonding electrons). Use the formula to determine its formal charge.
Step 3: For the carbon atoms in the first molecule, each carbon has 4 valence electrons, no lone pairs, and is involved in 4 bonds (8 bonding electrons). Apply the formula to calculate their formal charges.
Step 4: For the second molecule (H-C-H with a lone pair on carbon), calculate the formal charge of the carbon atom. Carbon has 4 valence electrons, 2 non-bonding electrons (one lone pair), and is involved in 3 bonds (6 bonding electrons). Use the formula to determine its formal charge.
Step 5: For the hydrogen atoms in both molecules, each hydrogen has 1 valence electron, no lone pairs, and is involved in 1 bond (2 bonding electrons). Apply the formula to calculate their formal charges.

비슷한 문제에 대한 검증된 영상 답변:

이 영상 해법은 위 문제에 도움이 된다고 튜터들이 추천한 것입니다.
영상 길이:
5m
도움이 되었나요?

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 by comparing the number of valence electrons in the free atom to the number of electrons assigned to it in the molecule. It helps in determining the most stable structure of a molecule by minimizing the formal charges across the atoms.
추천 영상:
가이드 코스
01:34
Calculating formal and net charge.

Valence Electrons

Valence electrons are the outermost electrons of an atom that are involved in forming bonds with other atoms. Understanding the number of valence electrons is crucial for calculating formal charges and predicting how atoms will interact in a molecule.
추천 영상:
가이드 코스
03:40
Valence Electrons of Transition Metals

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 are essential for visualizing the arrangement of electrons, which aids in the calculation of formal charges and understanding molecular geometry.
추천 영상:
가이드 코스
04:12
Drawing the Lewis Structure for N2H4.
관련 실천
교과서 질문

An atom with a formal charge does not necessarily have more or less electron density than the atoms in the molecule without formal charges. We can see this by examining the potential maps for H2O, H3O+, and HO−.

<IMAGE>

a. Which atom bears the formal negative charge in the hydroxide ion?

b. Which atom has the greater electron density in the hydroxide ion?

1585
views
교과서 질문

Give each atom the appropriate formal charge:

c.

d.

862
views
교과서 질문

An atom with a formal charge does not necessarily have more or less electron density than the atoms in the molecule without formal charges. We can see this by examining the potential maps for H2O, H3O+, and HO−.

<IMAGE>

c. Which atom bears the formal positive charge in the hydronium ion?

d. Which atom has the least electron density in the hydronium ion?

1313
views
교과서 질문

Draw the Lewis structure for each of the following:

e. CH3N+H3

2305
views
교과서 질문

Draw the Lewis structure for each of the following:

d. +C2H5

1567
views
교과서 질문

a. Find potassium (K) in the periodic table and predict how many valence electrons it has.

b. What orbital does the unpaired electron occupy?

1872
views