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CEM 141 chapter 3 and 4 learning objectives Questions & 100% Verified Correct Answers with complete solutions (Latest update

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  • Chemistry 141

CEM 141 chapter 3 and 4 learning objectives Questions & 100% Verified Correct Answers with complete solutions (Latest update

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  • 15 de agosto de 2024
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  • cem 141 chapter 3 and 4 learning objectives

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CEM 141 chapter 3 and 4 learning objectives
Differences in properties displayed are due to differences in the ratio of surface area to volume,
that implies that intermolecular forces are important nano materials. As more and more particles
are clustered together properties of particle change. - ANS-Differentiate between properties of
atoms, nano-particles, and larger macroscale materials. Explain why is it that atoms don't have
macroscopic properties like melting point, boiling point, and color, while macroscopic materials
do (and can be identified by them).

The higher the boiling and melting points shows which bond is stronger because it requires so
much energy to overcome the forces. - ANS-Predict, draw models (pictures), and explain why
relative melting points and boiling points for substances that exist as molecules (like H2) differ
from those that exist as continuous extended networks (like diamond or metals).

Another atom is needed to create the bond because more energy is needed to overcome the
repulsion force and bring the atoms together. - ANS-Explain the force and energy changes that
occur when two atoms approach each other and form a bond. Explain why a third body (another
atom or molecule) is (almost always) needed to form a stable bond. (Think back to what we
learned in Chapter 1.)

A bond will form there are 2 electrons in a bonding molecular orbital. (these 2 electrons make up
one bond). However, if there are also 2 electrons in an antibonding, this cancels out the
stabilization from 2 electrons in bonding orbital and, therefore, no bonds are formed. Draw
picture - ANS-What determines whether a bond or interaction is stable? Explain how
temperature influences the stability of bonds and interactions.

Molecular orbital
-each orbital holds max 2 electrons
-electrons in bonding orbital stabilize system
-electrons delocalize
-electrons in antibonding less stable
-atomic orbitals combine to equal
Valence Bond
-atomic orbitals overlap to form bond
-stronger bond greater overlap
-Each bond made up of 2 electrons - ANS-Compare and contrast the molecular orbital bond
model and the valence bond model. What are the similarities? What are the differences?

For graphite the sp2 orbitals will overalap end to end making sigma bonds and the left over P
orbitals overlap side to side to make Pi bonds.

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