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CEM 141 chapter 4 (1) Questions & 100% Verified Correct Answers with complete solutions (Latest update $7.99   Add to cart
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CEM 141 chapter 4 (1) Questions & 100% Verified Correct Answers with complete solutions (Latest update

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CEM 141 chapter 4 (1) Questions & 100% Verified Correct Answers with complete solutions (Latest update

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  • August 15, 2024
  • 2
  • 2024/2025
  • Exam (elaborations)
  • Questions & answers

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  • cem 141 chapter 4 1

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  • Chemistry 141
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CEM 141 chapter 4
the opposite charges of the metal and nonmetals attract - ANS-What is holding ions together in
the solid state? (Why don't they fly apart?)

the strength of the interaction between the ions is affected by the charges and atomic radii of
sodium and chlorine - ANS-What factors affect the strength of this interaction between ions?

there needs to be enough energy to overcome attractive forces between cations and anions -
ANS-What would happen if you wanted to melt NaCl?

NaCl is an ionic compound. It has ion-ion interactions not bonding. - ANS-How is bonding
different in an ionic substance like NaCl?

solid sodium chloride is an ionic compound in the solid state. In the solid state ionic molecules
do not conduct electricity because the charges do not have free movement. In solid aluminum
the electrons are de-localized and are free to move around therefore able to conduct electricity. -
ANS-Why doesn't solid sodium chloride conduct electricity, but solid aluminum does?

in the liquid state ions are free to move - ANS-Why does molten (liquid) sodium chloride conduct
electricity?

Single (sigma) bonds are formed when atomic or hybrid orbitals overlap directly between the
two nuclei (end-to-end overlap of orbitals). For example, sp3 + sp3, as shown above in C2H6.
When the bond rotates, the overlap stays the same so the bond is not broken.Double bonds
contain one sigma and one pi bond. Pi bonds are formed from the side-to-side overlap of
parallel p-orbitals and result in the overlap occurring above and below the plane of the nuclei.
For example, as shown in C2H4 above. If a pi bond were to rotate the overlap of the p-orbitals
would be broken and therefore the bond would break. - ANS-Use Valence Bond Theory to
explain why rotation is possible around single bonds, but not double bonds

are in a tug o war; bonds form because of the attractive forces between the atoms -
ANS-covalent bonds electrons...

strength of the bond - ANS-the depth of the well tells us the

overlap end to end; single bonds; rotate - ANS-sigma bonds

=8-#electrons - ANS-Valence

carbon atoms with single bonds - ANS-alkanes

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