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Chemistry 141 - Learning Objectives for Chapter 4 Questions & 100% Verified Correct Answers with complete solutions (Latest update CA$11.46   Add to cart
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Chemistry 141 - Learning Objectives for Chapter 4 Questions & 100% Verified Correct Answers with complete solutions (Latest update

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Chemistry 141 - Learning Objectives for Chapter 4 Questions & 100% Verified Correct Answers with complete solutions (Latest update

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  • August 15, 2024
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  • 2024/2025
  • Exam (elaborations)
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  • chemistry 141 learning objectives for chapter 4

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Chemistry 141 - Learning Objectives for Chapter 4
- ANS-Translate between different representations of simple molecules (for example, space
filling models, ball and stick models, perspective formulae, and Lewis structures).

- ANS-Draw structural isomers when given a molecular formula. Distinguish between structural
isomers and alternative representations of the same molecule.

- Since side-to-side overlap of atomic orbitals gives π bond, they cannot rotate freely.
- Since end-to-end overlap of atomic orbitals gives σ bond, they can rotate freely. - ANS-Explain
why rotation is (generally) easy around a sigma (single) bond, but more difficult around pi
bonds.

- ANS-Use Lewis structures and VSEPR to deduce electron pair geometry and molecular
shape of molecules

- ANS-Use Lewis structures to deduce the hybridization of the atoms in a molecule.

- ANS-Convert between Lewis structures and 3-dimensional representations of structure (and
vice versa).

- Ability of an element to attract electrons to itself in a bond.​
- Depends on effective nuclear charge and size of orbitals.​
- Electronegativity increases across the periodic table.​
- Electronegativity decreases down the periodic table. - ANS-Predict and explain the relative
electronegativity of different elements.

- When two atoms of different electronegativities bond, the electrons are not shared equally.​
- Results in a bond dipole. We say the bond is polar.​
- Because in this example (HF) the molecule only has one bond, the molecule also has a dipole.
The molecule is polar.​- ANS-Predict the polarity of bonds using atom electronegativity. Predict
the polarity of molecules using bond polarity and molecular shape.

- London dispersion forces (all molecules)​
- Dipole-dipole interactions (polar molecules)​
- Hydrogen bonding interactions (only very specific molecules)

LDFs < dipole-dipole < H-bonds​
weakest to strongest - ANS-Use molecular structure and the polarity of a molecule to predict the
type(s)of intermolecular forces (London dispersion forces, dipole-dipole interactions, and
hydrogen bonding interactions) present in molecules.

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