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Back to AI Flashcard MakerChemistry /OCR A-Level Chemistry: Chapter 6 - Shapes of Molecules Part 2

OCR A-Level Chemistry: Chapter 6 - Shapes of Molecules Part 2

Chemistry20 CardsCreated 2 months ago

A flashcard deck covering electronegativity, polar bonds, intermolecular forces, and hydrogen bonding.

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How is electronegativity measured?

On the Pauling scale.
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Key Terms

Term
Definition
How is electronegativity measured?
On the Pauling scale.
What does a higher Pauling value mean?
A higher electronegativity and thus a greater attraction for an electron pair in a covalent bond.
What makes a bond polar?
Two atoms with electronegativities differing by at least 0.5, causing the bonding electrons to be pulled towards the more electronegative atom and for...
What does a polar bond form?
A permanent dipole.
How is a dipole formed?
A difference in charge between the two atoms, caused by a shift in electron density in the bond.
Are diatomic gases polar or non-polar, why?
Non-polar.
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OCR A-Level Chemistry: Chapter 6 - Shapes of Molecules Part 2
TermDefinition
How is electronegativity measured?
On the Pauling scale.
What does a higher Pauling value mean?
A higher electronegativity and thus a greater attraction for an electron pair in a covalent bond.
What makes a bond polar?
Two atoms with electronegativities differing by at least 0.5, causing the bonding electrons to be pulled towards the more electronegative atom and forming a polar bond.
What does a polar bond form?
A permanent dipole.
How is a dipole formed?
A difference in charge between the two atoms, caused by a shift in electron density in the bond.
Are diatomic gases polar or non-polar, why?
Non-polar.
What happens if the polar bonds are arranged symmetrically in a molecule?
The dipoles cancel each other out, making the molecule non-polar.
What happens if the polar bonds are arranged unsymmetrically in a molecule?
Uneven distribution of charge and the molecule will have an overall dipole.
What can electronegativity be used to predict about bonding?
Whether it will be covalent or ionic bonding.
What is the general strength of intermolecular forces?
Very weak.
What is the order of the intermolecular forces from strongest to weakest?
Hydrogen bonding, dipole-dipole forces, and induced dipole-dipole forces.
What are induced dipole-dipole forces?
Electrons in clouds can at one moment be unevenly distributed, creating a temporary dipole. This dipole induces another dipole on a neighboring atom, and the two are attracted to each other. The dipoles can then be brought about in a domino effect, overall attracting the atoms to one another.
What is the effect of stronger induced dipole-dipole forces?
Higher boiling points.
How are permanent dipole-dipole interactions labelled?
With charges of delta+ and delta- on the atoms.
When can hydrogen bonding occur?
When hydrogen is covalently bonded to fluorine, nitrogen, or oxygen.
What effect does hydrogen bonding have on a molecule?
Soluble in water.
What is an interesting property of ice caused by hydrogen bonding?
In ice, water molecules are held together in a lattice. When ice melts, hydrogen bonds are broken, so ice has more of these than water, causing ice to be less dense than water.
How do intermolecular forces explain simple covalent compounds having low melting and boiling points?
Weak intermolecular forces to overcome.
How do intermolecular forces explain simple covalent compounds sometimes being soluble in water?
Water is also a polar molecule, and hydrogen bonded molecules can form these with water molecules, making them soluble.
How do intermolecular forces explain simple covalent compounds not conducting electricity?
Overall covalent molecules are uncharged, and permanent dipoles are not strong enough.