Chapter 3: Chemical Bonding Flashcards

(28 cards)

1
Q

What is ionic bonding?

A

Electrostatic attraction between oppositely charged ions.

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2
Q

How are ionic bonds formed?

A

Electrons are transferred from a metal to a non-metal, creating cations and anions.

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3
Q

What is a cation?

A

A positively charged ion.

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4
Q

What is an anion?

A

A negatively charged ion.

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5
Q

What is the effect of ionic charge on ionic bonding strength?

A

Higher charge = stronger attraction.

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6
Q

What is the effect of ionic radius on ionic bonding strength?

A

Smaller radius = ions are closer together = stronger bonding.

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7
Q

Which has stronger ionic bonding: MgO or NaCl?

A

MgO (Mg²⁺ and O²⁻) has stronger ionic bonding.

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8
Q

What are the properties of ionic compounds?

A
  • High melting/boiling points
  • Conduct electricity when molten or in solution
  • Often soluble in water
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9
Q

What is covalent bonding?

A

The sharing of electron pairs between non-metal atoms.

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10
Q

What is a dot-and-cross diagram?

A

A diagram showing how electrons are shared in covalent bonding.

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11
Q

What does a coordinate (dative) bond involve?

A

Both electrons come from one atom.

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12
Q

How is a coordinate bond represented?

A

With an arrow (→).

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13
Q

What causes bond polarity?

A

Differences in electronegativity between atoms.

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14
Q

What is a polar bond?

A

A bond where electrons are shared unequally, resulting in partial charges.

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15
Q

When is a bond non-polar?

A

When the atoms are the same (e.g., Cl–Cl).

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16
Q

What happens to dipoles in a symmetrical molecule?

A

The dipoles cancel out.

17
Q

What does VSEPR theory predict?

A

The shapes of molecules based on electron pair repulsion.

18
Q

What is the bond angle for a linear arrangement?

19
Q

What is the bond angle for a trigonal planar arrangement?

20
Q

What is the bond angle for a tetrahedral arrangement?

21
Q

What is the bond angle for a pyramidal arrangement?

22
Q

What is the bond angle for a bent arrangement?

23
Q

What are van der Waals’ forces?

A

Weak forces caused by temporary shifts in electron density.

24
Q

What are permanent dipole-dipole interactions?

A

Interactions between polar molecules with permanent partial charges.

25
What defines hydrogen bonding?
A strong dipole-dipole interaction between H (bonded to N, O, or F) and a lone pair on another N, O, or F atom.
26
How do intermolecular forces affect boiling points?
Stronger forces = higher boiling point.
27
How does hydrogen bonding affect water solubility?
Hydrogen bonding increases water solubility.
28
What is the solubility of non-polar molecules in water?
Tend to be insoluble in water due to weak forces.