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Year 11 chemistry > Bonding > Flashcards

Bonding Flashcards

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1
Q

Metals have

A

Low ionisation energy meaning positive ions are formed, delocalised electrons meaning they can move freely in the lattice

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2
Q

Metallic bonding

A

Electrostatic attraction of the positively charge metal ions to the delocalised electrons, non-directional bond

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3
Q

Non-directional charge

A

Attraction is equal in all directions

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4
Q

Properties of metallic bonding

A

High melting and boiling points, high thermal and electrical conductivity, malleable and ductile

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5
Q

Why does metallic bonding cause high melting and boiling points

A

strength of metallic bonds between cations and delocalised electrons determined by No. delocalised electrons and atomic radius (Increased number of valence electrons= increased melting and boiling points, smaller atomic radius= stronger metallic bond

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6
Q

Why does metallic bonding cause high thermal and electrical conductivity

A

When heated, delocalised electrons gain energy and move faster, colliding with other electrons and transferring energy, delocalised electrons can move freely in a solid state

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7
Q

Why does metallic bonding mean metals are malleable and ductile

A

when force is applied, delocalised electrons shield the cations from each other to they slide past one another without breaking the bonds meaning it changes shape

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8
Q

Covalent bonding

A

Results from the electrostatic attraction between a shared pair(s) of electrons and adjacent positive nuclei, directional bonds

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9
Q

Directional bonding

A

not equal attraction between atoms

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10
Q

Covalent molecular substances

A

Made up of molecules with the atoms within the molecules held together by the electrostatic attraction between the shared electrons and positive nuclei, strong covalent bond but weak intermolecular forces

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11
Q

Properties of covalent bonding

A

Low melting and boiling points, form soft solids, non-conductors and insulators

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12
Q

Why does covalent bonding cause low melting and boiling points

A

Weak intermolecular forces meaning less energy is required to separate molecules

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13
Q

Why does covalent bonding form soft solids

A

Weak intermolecular forces

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14
Q

Why does covalent bonding cause non-conductors and insulators

A

No free electrons meaning molecules are uncharged

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15
Q

Examples of covalent bonding

A

Cl2- share 2 electrons, H2O- two single covalent bonds

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16
Q

Octet rule exceptions

A

Beryllium is stable with 4 electrons, Boron is stable with 6 electrons, Phosphorous has 10 electrons in its valence shell- PCl5, Sulfur has 12 electrons in its valence shell- SF6

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17
Q

Covalent network substances

A

Each atom is covalently bonded to each other to form a 3 dimensional lattice, no weak intermolecular forces because each atom is covalently bonded

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18
Q

Properties of covalent network structures

A

High melting and boiling points, hard and brittle, no conductivity

19
Q

Why do covalent network structures have a high melting and boiling point

A

Many strong covalent bonds which extend through the lattice which need a lot of energy to break apart

20
Q

Why are covalent network structures hard and brittle

A

Hard due to the strong covalent bonds in the lattice, shatter if hammered with enough energy

21
Q

Why do covalent network substances have no conductivity

A

No mobile ions or delocalised electrons

22
Q

Covalent network substance exeption

A

Graphite has conductivity as it has one delocalised electron per carbon atom

23
Q

Examples of covalent network substances

A

Diamond, silicon, carbide, quartz, granite

24
Q

Ionic bonding

A

Result of the electrostatic attraction between positive ions (cations) and negative ions (anions), non-directional

25
Q

What do metal atoms do to form cations

A

Lose elctrons

26
Q

What do non-metal atoms do to form cations

A

Gain electrons

27
Q

Stable arrangement in ionic bonding is achieved by

A

the transfer of electrons resulting in the formation of atoms held together in a 3 dimensional crystal lattice by electrostatic attraction

28
Q

Properties of ionic bonding

A

High melting and boiling points, poor electrical conductors when solid, good electrical conductors when molten or in aqueous solution, brittle

29
Q

Why do ionic bonds cause high melting and boiling points

A

strong electrostatic forces which extend through the lattice, through heating, ions vibrate faster and becomes less firmly held in place

30
Q

Why does ionic bonding cause poor electrical conductors when solid

A

When solid, ions are held tightly together by electrostatic bonds meaning ions can’t move

31
Q

Why does ionic bonding cause good electrical conductivity in a molten state or in an aqueous solution

A

Once the electrostatic forces are broken the ions are free to move meaning they carry charge, ionic compounds that are soluble in water means water molecules come between the ions breaking the lattice meaning the ions are mobile

32
Q

Why does ionic bonding cause susbtances to be brittle

A

When force is applied, the ions shift positions so the same charge may come together, likes charges repel each other meaning the ions repel each other meaning the latice breaks

33
Q

Examples of ionic bonding

A

NaCl, CaCl2

34
Q

Allotropes

A

Elements that can exist with their atoms in several different structure arrangements which give them different physical forms, bonded in different ways

35
Q

Examples of allotropes

A

Oxygen- O2 and O3, Carbon- diamond, graphite and amorphous carbon

36
Q

Properties of diamond

A

Very hard, sublimes, non-conductor, brittle

37
Q

Structure of diamond

A

Covalent network structure

38
Q

Structure of graphite

A

Covalent layer lattice

39
Q

Properties of graphite

A

soft, greasy, conductive, slippery

40
Q

Structure of amorphous carbon

A

irregular structure, many varieties

41
Q

Properties of amorphous carbon

A

Non-crystalline, cheap, conductive

42
Q

Nanomaterial

A

Molecule smaller than 100 nanometers

43
Q

Properties of nanomaterials

A

Increased strength, Increased chemical reactivity because of larger surface area, increased conductivity

44
Q

Example of a nanomaterial

A

Carbon nanotubes

Year 11 chemistry (10 decks)

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