Bonding, structure and properties Flashcards

1
Q

Metallic bonding

A

the electrostatic force of attraction between positively charged ions and (negatively charged) delocalised outer electrons.

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2
Q

How are atoms in covalent bonds held together?

A

By the electrostatic forces of attraction between positively charged nuclei and the negatively charged shared electrons

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3
Q

What does the polarity of a covalent bond depend on?

A

On the difference in electronegativity of the bonded atoms

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4
Q

Ionic bonding

A

electrostatic force of attraction between positively and negatively charged ions.

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5
Q

what causes Van der Waals?

A

Electrostatic attraction between temporary dipoles and induced dipoles caused by movement of electrons in atoms or molecules.

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6
Q

Describe Van der Waals forces

A

Can operate between all types of molecules and atoms.
Are the weakest of all the other types of bonding.
Their strength depends on the sizes of the atoms or molecules.

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7
Q

polar molecule:

A

molecule with a permanent dipole.

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8
Q

what are permanent dipole-permanent dipole interactions?

A

they are additional electrostatic forces of attraction between polar molecules. they are stronger than VDW forces between molecules of the same size.

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9
Q

the spatial arrangement of polar covalent bonds results in a molecule being…

A

polar.

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10
Q

Between what elements can hydrogen bonding occur with?

A

Nitrogen, oxygen and fluorine

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11
Q

Describe hydrogen bonding

A

Stronger than permanent dipole-permanent dipole interactions but weaker than covalent.
(el.st. forces of ) Attraction between molecules which contain highly polar covalent bonds.

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12
Q

Describe a metallic structure

A

Lattice of positive ion and delocalised electrons

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13
Q

Describe covalent molecular structure

A

Discrete molecules held together by weak intermolecular forces.

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14
Q

Describe covalent network structure

A

A giant lattice of covalently bonded atoms.

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15
Q

Describe ionic molecular structure

A

A giant lattice of oppositely charged ions.

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16
Q

Describe monatomic structure

A

Discrete atoms held together by VDW forces.

17
Q

what does it mean if a molecule is discrete (don’t need to know for exam)

A

it is held together by VDW forces.

18
Q

compare melting and boiling points of polar molecules to those of non polar molecules.

A

The melting/boiling points are higher for polar molecules.

19
Q

What can these be related to?

  • melting/boiling points
  • hardness/softness
A

bonding and structures of elements

20
Q

What compounds are soluble in polar solutions such as water?

A

Polar molecular and ionic compounds.

21
Q

what is not soluble in water or polar compounds, but is in non-polar solutions?

A

Non-polar compounds.

22
Q

Give examples of anomalous boiling points due to hydrogen bonding.

A

Ammonia, water and hydrogen fluoride.

23
Q

Give 4 properties of compounds that are affected by hydrogen bonding.

A

higher boiling points and melting points, greater viscosity and miscibility with water.

24
Q

Why is the density of ice less than that of water?

A

Hydrogen bonding results in tunnels forming in the structure which are full of air.

25
Q

in what state is sulphur at room temperature?

A

Solid, 8 atoms bond together (discrete molecular solid)

26
Q

give another example of covalent molecular solid

A

Phosphorus (P4)

27
Q

are covalent molecular solids volatile? why?

A

yes, even if solid at room temperature. Because they have strong(er) intramolecular forces but intermolecular forces are very weak VDW.

28
Q

what happens between the layers of graphite?

A

there are free flowing electrons which make graphite able to conduct and flaky.

29
Q

what can you say about fullerenes?

A

under investigation- covalent molecular sructure

30
Q

why are metals malleable although their melting and boiling points are high?

A

because although the bonds are strong they are not directional.

31
Q

what forms a lattice, NOT a molecule?

A

Ionic compounds.

32
Q

give examples of covalent network structures

A

silicon carbide and silicon dioxide(quartz)

33
Q

a use of silicon carbide

A

abrasive in the cutting and grinding surfaces of tools

34
Q

which compounds conduct when molten?

A

Ionic compounds.