Skip to main content
Ch.9 - Chemical Bonding I: The Lewis Model
Tro - Chemistry: A Molecular Approach 4th Edition
Tro4th EditionChemistry: A Molecular ApproachISBN: 9780134112831당신이 사용하는 게 아니라요?교과서 변경
모든 교과서Tro 4th EditionCh.9 - Chemical Bonding I: The Lewis Model문제 107a
9장, 문제 107a

Draw the Lewis structure for each compound. a. Cl2O7 (no Cl–Cl bond)

검증된 단계별 안내
1
Step 1: Count the total number of valence electrons. Chlorine (Cl) has 7 valence electrons and oxygen (O) has 6 valence electrons. Calculate the total for Cl2O7.
Step 2: Determine the central atom. In Cl2O7, chlorine atoms are typically central, with oxygen atoms surrounding them.
Step 3: Arrange the atoms. Place the two chlorine atoms in the center and connect each to three oxygen atoms, ensuring no Cl-Cl bond is formed.
Step 4: Distribute the electrons. Start by placing single bonds between the Cl and O atoms, then distribute the remaining electrons to satisfy the octet rule for each atom, starting with the outer atoms.
Step 5: Check for formal charges and resonance. Adjust the structure by forming double bonds if necessary to minimize formal charges, ensuring the most stable structure.

주요 개념

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

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 use dots to represent valence electrons and lines to represent bonds between atoms. Understanding how to draw Lewis structures is essential for visualizing molecular geometry and predicting the behavior of molecules in chemical reactions.
추천 영상:
가이드 코스
04:28
Lewis Dot Structures: Ions

Valence Electrons

Valence electrons are the outermost electrons of an atom and are crucial in determining how atoms bond with each other. The number of valence electrons influences the atom's reactivity and the types of bonds it can form. For example, chlorine has seven valence electrons, which allows it to form bonds with other elements, such as oxygen in Cl2O7.
추천 영상:
가이드 코스
02:12
Transition Metals Valence Electrons

Molecular Geometry

Molecular geometry refers to the three-dimensional arrangement of atoms within a molecule. It is influenced by the number of bonding pairs and lone pairs of electrons around the central atom, which can affect the molecule's polarity and reactivity. Understanding molecular geometry is important for predicting the properties and behavior of compounds like Cl2O7.
추천 영상:
가이드 코스
01:33
Molecular Geometry with Two Electron Groups
관련 실천
교과서 질문

If hydrogen were used as a fuel, it could be burned according to this reaction: H2(g) + 1/2 O2(g) → H2O(g) Which fuel yields more energy per gram?

828
views
교과서 질문

The azide ion, N3-, is a symmetrical ion, all of whose contributing resonance structures have formal charges. Draw three important contributing structures for this ion.

2357
views
교과서 질문

Draw the Lewis structure for each compound. c. H3AsO4

1206
views
교과서 질문

If hydrogen were used as a fuel, it could be burned according to this reaction: H2(g) + 1/2 O2(g) → H2O(g) Which fuel yields more energy per mole?

384
views
교과서 질문

Calculate ΔHrxn for the combustion of octane (C8H18), a component of gasoline, by using average bond energies and then calculate it using enthalpies of formation from Appendix IIB. What is the percent difference between your results? Which result would you expect to be more accurate?

2412
views
교과서 질문

Draw the Lewis structure for each compound. b. H3PO3 (two OH bonds)

1142
views