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Chemistry IGCSE > Chapter #3 - Chemical Bonding > Flashcards

Chapter #3 - Chemical Bonding Flashcards

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1
Q

What is the definition of bonding?

A

Forces that cause particles to stick together.

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2
Q

What is the definition of ionic bonding?

A

A bonding which occurs in compounds containing a metal and non-metal. The electrostatic attraction of oppositely charged ions.

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3
Q

What forces are present in ionic bonding?

A

Electrostatic forces of attraction between oppositely charged ions.

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4
Q

What is the meaning of structure in chemistry?

A

3D arrangement of particles as a consequence of bonding.

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5
Q

What is a lattice?

A

A repeating pattern (of particles).

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6
Q

What is a discrete structure?

A

Individual particles not arranged in a pattern.

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7
Q

What is the structure of ionic bonded ions description?

A

Lattice of alternating cations(+) and anions(-) held together with electrostatic forces.

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8
Q

What is the general mpt/bpt of ionic bonds and why?

A

High mpt because of strong electrostatic forces between ions and each ion has multiple forces. lots of energy is needed to weaken forces

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9
Q

What does mpt/bpt depend on?

A

The strength of the forces between particles.

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10
Q

What does the strength of the forces depend on in ionic bonds?

A

1) Magnitude of charge
ex. Forces between -2 & +2 are stronger than forces between -1 & +1

2) Radius of ions. the bigger they are the weaker the forces are because the charge is more dispersed.

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11
Q

What should you look at first and second when comparing mpt/bpt of ionic bonds?

A

1) Magnitude
2) Radius of ion

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12
Q

What is the general electrical conductivity of ionic bonds and why?

A

Conduct in only (l) and (aq) because the particles are charged and can move but in (s), they are charged but can’t move.

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13
Q

What is the general solubility of ionic bonds?

A

They dissolve in water.

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14
Q

What does conductivity depend on?

A

Weather the substance has charged particles which can move.

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15
Q

What is the general malleability of ionic bonds and why?

A

brittle, because when ions shift position, they will repel each other.

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16
Q

Where does covalent bonding occur?

A

In substances containing two (or more) non-metals. The non-metals can be of the same type of atom (element) or different (compound).

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17
Q

What happens when non-metals share electrons?

A

The outer valence (energy levels) overlap.

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18
Q

What is the definition of a covalent bond?

A

the electrostatic attraction of two nuclei for a shared pair of electrons.

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19
Q

What are the two different types of covalent bond structures?

A

Discrete/Simple/Molecular

Covalent lattice/Giant lattice/Macromolecular

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20
Q

What are the forces present in covalent discrete bonds?

A

Very strong covalent bonds (stronger than ionic bonds) between the atoms in the molecule which are only affected during chemical reactions.

Very weak intermolecular forces (IMFs) The forces between molecules which are affected during physical processes.

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21
Q

What is the general mpt/bpt of discrete covalent bonds?

A

very low, because weak IMFs require little energy to break.

22
Q

What does the mpt/bpt of discrete covalent bonds depend on?

A

The physical size of the molecules. larger molecules have higher IMFs because they are larger, therefor the mpt is higher.

23
Q

What is the general electrical conductivity of discrete covalent bonds?

A

They do not conduct because they have no charged particles.

24
Q

What is the general solubility of discrete covalent bonds?

A

Insoluble in water but soluble in oil-like substances.

25
Q

What happens when discrete covalent bonds are dissolved?

A

During dissolving, molecules do NOT dissociate. The molecules separate from each other (atoms remain bonded).

26
Q

What is the description of a covalent lattice?

A

a lattice of atoms held together with strong covalent bonds. There are NO IMFs because it is NOT a molecule.

27
Q

What is the general mpt/bpt of SiO2?

A

Very high, because the only forces present are very strong covalent bonds which require lots of energy to break.

28
Q

What is the general conductivity of SiO2?

A

Does not conduct, no charged particles.

29
Q

What is the general solubility of SiO2?

A

insoluble in all solvents as strong covalent bonds cannot be broken.

30
Q

What is the general malleability of SiO2?

A

They are brittle.

31
Q

What are the three most important covalent substances with a lattice structure?

A
  • SiO2 (sand)
  • C in diamond
  • C in graphite
32
Q

What does testing for solubility in water find out?

A

Soluble: Ionic (lots of exceptions)

Insoluble: Metallic/Covalent

33
Q

What does testing for mpt find out?

A

melts: covalent (discrete) (very hard to find exacts mpt)

not melt: Lattices (covalent, ionic or metallic)

34
Q

What does testing for conductivity (aq) find out?

A

Conducts: Ionic (not many dissolve or conduct)

Not conducts: Metallic, covalent, ionic (insoluble)

35
Q

What does testing for conductivity (l)

A

(Not possible with school apparatus to reach such high temps)

Conducts: ionic, metallic

Not conducts: Covalent

36
Q

What does testing for solubility in oil like substances find out?

A

Soluble: Covalent discrete (exceptions)

Insoluble: metallic, ionic, covalent lattice

37
Q

What does testing for conductivity as (s) find out?

A

Conducts: metallic, graphite

No Conducts: ionic, covalent discrete, carbon

38
Q

What is the name of the shape a carbon diamond makes?

A

A tetrahedron

39
Q

What is the mpt of carbon (diamond)?

A

Very high mpt. (aprox. 3500)

40
Q

What is the conductivity of carbon (diamond)?

A

Does not conduct, no charged particles.

41
Q

What is the solubility of carbon (diamond)?

A

Does not dissolve in any solvent (because it only has strong covalent bonds)

42
Q

What is the mpt of carbon (graphite)?

A

Very high, like SiO2

43
Q

What is the conductivity of carbon (graphite)?

A

conducts electricity as a solid due to delocalized electrons that can move and carry charge.

44
Q

What is the solubility of carbon (graphite)?

A

Insoluble in all solvents.

45
Q

Is carbon (graphite) malleable?

A

They are lubricant-layers can slide over each other without affecting the rest of the structure.

46
Q

Where does metallic bonding occur?

A

In metallic elements, and alloys (mixtures of metals)(metals cannot form compounds)

47
Q

What is the description of metallic bonding?

A

A lattice of cations surrounded by delocalized electrons, held together with strong electrostatic forces.

48
Q

What is the mpt of metallic bonds?

A

High mpt due to strong electrostatic forces between cations and delocalized electrons

49
Q

What is the conductivity of metallic bonds?

A

Conduct electricity as (s) and (l) as delocalized electrons move and carry charge.

50
Q

What is the solubility of metallic bonds?

A

Insoluble in all solvents but some react with water.

51
Q

What does the mpt. of metallic bonds depend on?

A

It depends on how many delocalised electrons there are per ion

Chemistry IGCSE (12 decks)

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