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Questions and Answers
What is responsible for physical properties, such as boiling and melting points?
What is a measure of unequal sharing of electrons in a covalent bond?
What increases from left to right across a period and decreases down a group in the periodic table?
What influences the strength of dipole-dipole forces?
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What type of molecules have a higher dipole moment than linear molecules?
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What increases boiling point?
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What can decrease boiling point?
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What influences boiling point trends?
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Study Notes
Dipole-Dipole Forces
Intermolecular Forces
- Weak attractive forces between molecules
- Responsible for physical properties, such as boiling and melting points
- Includes:
- Dipole-dipole forces
- Hydrogen bonding
- London dispersion forces
Polarity
- Measure of unequal sharing of electrons in a covalent bond
- Results in a partial positive charge (δ+) on one atom and a partial negative charge (δ-) on the other
- Caused by differences in electronegativity between atoms in a bond
Electronegativity
- Ability of an atom to attract electrons in a covalent bond
- Increases from left to right across a period and decreases down a group in the periodic table
- Electronegativity differences between atoms in a bond lead to polarity
Molecular Shape
- Influences the strength of dipole-dipole forces
- Bent or V-shape molecules have a higher dipole moment than linear molecules
- Dipole-dipole forces are stronger when molecules are polar and have a bent or V-shape
Boiling Point Trends
- Dipole-dipole forces increase boiling point
- As molecular weight increases, boiling point also increases
- Branching or complexity in molecular shape can decrease boiling point
- Boiling point trends are influenced by a combination of molecular weight and dipole-dipole forces
Intermolecular Forces
- Weak attractive forces between molecules responsible for physical properties like boiling and melting points
- Comprise dipole-dipole forces, hydrogen bonding, and London dispersion forces
Polarity
- Measures unequal sharing of electrons in a covalent bond
- Results in partial positive (δ+) and partial negative (δ-) charges on atoms
- Caused by electronegativity differences between atoms in a bond
Electronegativity
- Ability of an atom to attract electrons in a covalent bond
- Increases from left to right across a period and decreases down a group in the periodic table
- Electronegativity differences lead to polarity in a bond
Molecular Shape
- Influences dipole-dipole force strength
- Bent or V-shape molecules have a higher dipole moment than linear molecules
- Dipole-dipole forces are stronger when molecules are polar and have a bent or V-shape
Boiling Point Trends
- Dipole-dipole forces increase boiling point
- Boiling point increases with molecular weight
- Branching or complexity in molecular shape can decrease boiling point
- Boiling point trends result from a combination of molecular weight and dipole-dipole forces
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Description
Understanding intermolecular forces, including dipole-dipole forces, hydrogen bonding, and London dispersion forces, and their role in determining physical properties.
