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Chemistry > Bonding > Flashcards

Bonding Flashcards

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1
Q

Ionic Bonding

A

Electrostatic attraction between oppositely charged ions in a lattice

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2
Q

Formulas of compound ions, eg sulfate, hydroxide, nitrate, carbonate and ammonium.

A

SO4 2-
OH-
NO3-
CO3 2-
NH4+

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3
Q

Co-ordinate/ (dative covalent)

A

Contains a shared pair of electrons with both electrons supplied by one atom.

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4
Q

Metallic Bonding

A

Attraction between delocalised electrons and positive ions arranged in a lattice

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5
Q

Examples of Ionic Crystal Structures as a Giant Ionic Lattice

A

Sodium chloride
Magnesium oxide

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6
Q

Examples of Structures with Covalent Bonding in a Simple Molecular

A

Iodine
Ice
Carbon dioxide
Water
Methane

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7
Q

Examples of Structures with Covalent Bonding in a Macromolecular

A

Diamond
Graphite
Silicon dioxide
Silicon

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8
Q

Examples of Metallic Bonding in a Giant Metallic Lattice

A

Magnesium, Sodium

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9
Q

Rules for Lone and Bonding Pairs in Shapes of Molecules

A

-Bonding pairs and lone (non-bonding) pairs of electrons as charge clouds that repel each other.

-Pairs of electrons in the outer shell of atoms arrange themselves as far apart as possible to minimise repulsion.

-Lone pair–lone pair repulsion is greater than lone pair–bond pair repulsion, which is greater than bond pair–bond pair repulsion.

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10
Q

Effect of electron pair repulsion on bond angles

A

The greater the force of repulsion between 2 pairs of e-, the further apart the electrons will be and the bigger the bond angle.

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11
Q

BP=2
LP=0

A

Linear

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12
Q

BP=3
LP=0

A

Trigonal Planar

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13
Q

BP=4
LP=0

A

Tetrahedral

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14
Q

BP=5
LP=0

A

Trigonal Bipyramidal

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15
Q

BP=6
LP=0

A

Octahedral

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16
Q

BP=3
LP=1

A

Pyramidal

17
Q

BP=2
LP=2

A

Bent

18
Q

BP=3
LP=2

A

Trigonal Planar

19
Q

BP=4
LP=2

A

Square Planar

20
Q

Electronegativity

A

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

21
Q

How is a permanent dipole produced?

A

The electron distribution in a covalent bond between elements with different electronegativities will be unsymmetrical. This produces a polar covalent bond, and may cause a molecule to have a permanent dipole.

22
Q

Why do some molecules with polar bonds do not have a permanent dipole

A

It contains polar bonds but is symmetrical, so the polar bonds cancel out, e.g H20 and CO2

23
Q

Properties of Ionic Bonding (Crystalline Solid)

A

-High Boiling and Melting Points- because
of giant lattice of ions with strong electrostatic forces between oppositely charged ions
-Good Solubility in Water
-SOLID- poor conductivity, ions fixed in lattice can’t move. MOLTEN- good conductivity, ions can move

24
Q

Properties of Simple Molecular Structures
(mostly gases and liquids)

A

low melting and boiling because of weak intermolecular forces between molecules (specify type e.g van der
Waals/hydrogen bond)
-Poor Solubility in water
-SOLID- Poor Conductor, as no ions to conduct and electrons are localised. MOLTEN- no ions

25
Q

Properties of Macromolecular
(Solids)

A

High Melting and Boiling Point because of many strong covalent bonds in macromolecular structure. Requires a lot of energy to overcome the many strong bonds.
-INSOLUBLE in water
-Conductivity in diamond and sand: poor, because electrons can’t move (localised) graphite: good as free delocalised electrons between layers carry a current, MOLTEN- poor conductivity

26
Q

Properties of Metallic Structure (Shiny Metals)

A

-Malleable, +ions in the lattice are all identical, planes of ions can easily slide over one another
-attractive forces in the lattice are all the same
-High Melting and Boiling Points- strong electrostatic forces between positive ions and a sea of delocalised electrons
-Insoluble in water
-SOLID: good conductivity due to delocalised e- which can move through the structure, MOLTEN: good conductor

Chemistry (6 decks)

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