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Z/ HIGHER Chemistry > Chemical Bonding Summary > Flashcards

Chemical Bonding Summary Flashcards

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1
Q

What elements are involved in metallic bonding?

A

Metals

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2
Q

What elements are involved in covalent network bonding?

A

Non-metal elements form groups 3 and 4 or some of their compounds.

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3
Q

What elements are involved in Ionic bonding?

A

Usually metal/non-metal compound (i.e. elements with large differences in electronegativity).

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4
Q

What elements are involved in covalent molecular bonding?

A

Non-metal element or compound of non-metals.

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5
Q

What are examples of metallic bonding?

A

Na, Fe, Cu, Mg.

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6
Q

What are examples of covalent network bonding?

A

Diamond, graphite, SiO2, SiC, B, Si.

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7
Q

What are examples of Ionic bonding?

A

NaCl, CaO, K2CO3

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8
Q

What are examples of covalent molecular bonding?

A

Co2(g), I2(g), C8H18(I)

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9
Q

What is the structure of metallic bonding?

A

Giant lattice of positive metal cations in a “sea” of delocalised electrons.

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10
Q

What is the structure of covalent network bonding?

A

Giant lattice structure of covalently bonded atoms.

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11
Q

What is the structure of Ionic bonding?

A

Giant lattice of negative and positive ions.

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12
Q

What is the structure of covalent molecular bonding?

A

Discrete molecules.

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13
Q

How does the bonding work in a metallic bonding?

A

Attraction of DELOCALISED ELECTRONS and POSITIVE IONS hold the structure together with STRONG METALLIC BONDS.

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14
Q

How does the bonding work in a covalent network bonding?

A

Atoms linked throughout the structure by STRONG COVALENT BONDS.

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15
Q

How does the bonding work in Ionic bonding?

A

Electrostatic attraction of OPPOSITELY CHARGED IONS causes STRONG IONIC BONDS.

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16
Q

How does the bonding work in a covalent molecular bonding?

A

Strong covalent bonds hold atoms together inside the molecules. Molecules held together in liquid or solid by WEAK INTERMOLECULAR FORCES (Van der Waals forces): London Dispersion forces, permanent dipole-permanent dipole interactions or hydrogen bonding).

17
Q

What are the melting an boiling points of metallic bonding?

A

High

18
Q

What are the melting an boiling points of covalent network bonding?

A

Very High

19
Q

What are the melting an boiling points of Ionic bonding?

A

High

20
Q

What are the melting an boiling points of covalent molecular bonding?

A

Low (type of intermolecular bonding affects actual value: hydrogen bonding increases boiling point compared to Van der Waals forces).

21
Q

In what state are metallic bonds at room temperature?

A

Usually solid

22
Q

In what state are covalent network bonds at room temperature?

A

Solid

23
Q

In what state are ionic bonds at room temperature?

A

Solid

24
Q

In what state are covalent molecular at room temperature?

A

Solid, liquid or gas.

25
Q

How good is the electrical conductivity of metallic bonds and why is this?

A

Good conductors in solid or liquid state.

26
Q

How good is the electrical conductivity of covalent network bonds and why is this?

A

Non-conductors (except graphite).

27
Q

How good is the electrical conductivity of ionic bonds and why is this?

A

Non-conductors as solid, good conductors (electrolytes) When molten or in aqueous.

28
Q

How good is the electrical conductivity of covalent molecular and why is this?

A

Non-conductors, except those which react (dissolve) in water to produce electrolytes in solution (e.g. HCL, CO2).

29
Q

Is metallic bonding soluble and why is this?

A

Insoluble in polar and non-polar solvents.

30
Q

is covalent network bonding soluble and why is this?

A

Insoluble in all solvents.

31
Q

Is ionic bonding soluble and why is this?

A

Usually soluble in polar solvents (use DB to find out), insoluble in non-polar solvents.

32
Q

Is covalent molecular bonding soluble and why is this?

A

Generally insoluble in polar solvents, usually soluble in non-polar solvents.

Z/ HIGHER Chemistry (25 decks)

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