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Chemistry > Topic 2 - Structure and Bonding > Flashcards

Topic 2 - Structure and Bonding Flashcards

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1
Q

What`s Ionic Bonding?

A

The electrostatic force of attraction between oppositely charged ions in a regular, ionic lattice.

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2
Q

What`s a covalent bond?

A

The electrostatic force of attraction between two oppositely charges nuclei and a shared pair of electrons.

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3
Q

What`s Metallic bonding?

A

The electrostatic force of attraction between cations and a sea of delocalized electrons.

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4
Q

What is a Dative Covalent bond?

A

A bond which contains a shared pair of electrons with both electrons supplied by one atom

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5
Q

Describe a Tetrahedral shape.

A

A molecule with 4 bonding pairs of electrons.
- No lone pairs
- Bond angle = 109.5
- e.g. CH4

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6
Q

Describe an Octahedral shape.

A

A molecule with 6 bonding pairs of electrons.
- No lone pairs
- Bond angle = 90
- e.g. SF6

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7
Q

Describe a Trigonal Planar shape.

A

A molecule with 3 bonding pairs of electrons.
- No lone pairs
- Bond angle = 120
- e.g. AlCl3

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8
Q

Describe a Linear Shape.

A

A molecule with 2 bonding pairs of electrons.
- No lone pairs
- Bond angle = 180
- e.g. CO2

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9
Q

Describe a Non-Linear Shape.

A

A molecule with 2 bonding pairs of electrons.
- 1 or more lone pairs
- Bond angle = 109.5 - 2.5 (per lp)
- e.g. SO2 - 107

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10
Q

Describe a Pyramidal shape.

A

A molecule with 3 bonding pairs of electrons.
- 1 lone pair
- Bond angle = 107
- e.g. NH3

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11
Q

Describe a Trigonal Bipyramidal shape.

A

A molecule with 5 bonding pairs of electrons.
- No lone pairs
- Bond angles 120 and 90
- e.g. PCl5

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12
Q

Define Electronegativity

A

The power of an atom to to attract the pair of electrons in a covalent bond.

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13
Q

What is the trend in electronegativity across a period?

A

Increases across a period.
- Nuclear charge increases
- Atomic radius decreases
- Shielding remains the same
-Bonding electrons are closer to attractive power of nucleus

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14
Q

What is the trend in electronegativity down a group ?

A

Decreases down a group.
- Atomic Radius increases
- Shielding increases
- Bonding electrons are further from attractive power of nucleus.

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15
Q

Properties of a polar molecule.

A
  • Bonds between atoms of elements with different electronegativity values are polar.
  • Polar molecules are asymmetric (contain a net dipole moment)
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16
Q

Van der Waal forces

A

IMFs that exist between all molecules.
- Electrons are always moving.
- Causing unequal distribution of electrons, resulting in temporary induced dipole.
- VDW forces are attractions between these induced dipoles
- The more electrons the greater the VDW forces

17
Q

Permanent dipole-dipole forces

A

Attractive forces between the delta +ve on one molecule and the delta -ve on another molecule. Occurs in polar molecules.

18
Q

Hydrogen Bonds

A

A strong intermolecular force between a delta +ve Hydrogen covalently bonded to O,F or N and a lone pair of electrons on the delta -ve O,F or N on a nearby molecule.

19
Q

Physical properties of an Ionic Crystal

A
  • Crystalline, hard, brittle - repulsion between ions if structure distorted
    -High mpt. and High bpt.
  • Conducts when molten or aqueous
  • Soluble in polar substances - contains +ve and -ve ions.
20
Q

Physical properties of a Metallic crystal

A
  • Hardness
  • High mpt. (strong attraction between +ve ions and -ve electrons)
  • Good electrical conductivity (delocalized electrons can move and carry charge)
21
Q

Physical properties of a simple molecular crystal

A
  • Low melting point (weak IMFs are broken)
  • Non-conductor of electricity (no free electrons)
  • Insoluble in water (they are non-polar so don`t interact with water)
  • soft
22
Q

Properties of Diamond

A
  • High melting point ( strong covalent bonds)
  • Very hard (Rigid 3 dimensional structure holding surface atoms in place)
  • Doesn`t conduct (No free electrons)
23
Q

Properties of Graphite

A

Chemistry (12 decks)

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