bonding Flashcards

1
Q

Graphite

A

consists of carbon atoms bonded to 3 other carbon atoms in a 2-D lattice. Delocalised valence electrons are between the layers and the forces of attraction between the layers are weak.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

Diamond

A

Consists of carbon atoms covalently bonded in 4 other carbon atoms in a tetrahedral 3-D lattice structure. The covalent bonds are strong so atoms cannot be easily removed.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

Ion

A

Consists on ions, ionic bonds

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

Metal

A

cations and electrons, metallic bonds

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

Molecule

A

atoms, covalent bonds, covalent network solid

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

Metal conduction

A

3-D lattice of positively charged metal cations, with delocalised valence electrons bonded to all the metal cations. As these electrons move the metal will conduct electricity as solid & molten

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

Requirement for conduction

A

Free moving charged particles

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

Ion conduction

A

ionic solid is a 3-D lattice of cations and anions. In solid, charged particles (ions) are in fixed position and as they do not move, the solid cannot conduct electricity. Molten, ions can move and is able to conduct electricity.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

Melt ice

A

endothermic to absorb

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

Heat pack heats up

A

exothermic as heat is released

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

Shape

A

_ regions of electron density around the central _ atom. These regions are arranged as far apart as possible to minimise repulsion. They take a _ arrangement with a bond angle of _.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

All Bonding regions

A

all regions are bonding therefore the shape is _

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

Not all bonding regions

A

_ regions are bonded and _ non-bonding lone pair of electrons, therefore the observed shape is _

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

Polarity factors

A

presence of polar bonds (due to electronegativity differences of the atoms in a bond)
distribution of polar bonds around a central atom
symmetrical/asymmetrical to cancel dipole

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

Polarity

A

bonded atoms are different and have different electronegativity so there is a bond dipole and the bonds are polar. If symmetrical, the dipole cancels and is non-polar.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

metal description

A

_ is a metallic solid made up of atoms that take a regular 3-D arrangement. The valence electrons of the atoms are delocalised, resulting in a regular array of cations held in place by the strong attractions between cations and valence electrons (metallic bond)

17
Q

metal conductivity

A

_ can conduct electricity as the valence electrons are able to move.

18
Q

metal ductility

A

the metal is able to be stretched into a wire as when it is hammered, the layers of cations are able to slide over each other without disrupting the strong bonding, this is because metallic bonds are multi directional

19
Q

molecule in high temp

A

_ has a molecular structure made up of _ molecules held together by weak intermolecular forces of attraction. These forces are easily broken with a small amount of energy.

20
Q

graphite in high temp

A

graphite is a strong covalent network made up of a regular 2-D arrangement of carbon atoms covalently bonded to each other. A large amount of energy is required to break all the strong covalent bonds.

21
Q

Solubility

A

for a solute to dissolve in a solvent, the new attractions formed between the solute and solvent molecules must be strong enough to release sufficient energy to overcome the bonds between molecules in the solute and between the molecules in the solvent.

22
Q

non polar solubility in water

A

water is polar, so there are only weak forces of attraction between water and _. The energy released when these attractions form is not sufficient to overcome the polar water molecules and allow them to separator. _ will not dissolve

23
Q

polar solubility in water

A

the + and - molecules are strongly attracted to polar water molecules. + is attracted to slightly negative O- atoms. - is attracted to slightly positive H+ atoms. Forming these attractions releases sufficient energy to overcome the attractive forces between water molecules in solvent and in the solute. the molecule will dissolve.

24
Q

force on metal

A

Metallic solid in 3-D lattice of cations surrounded by free moving electrons. Delocalised electrons hold structure together, as they are attracted to the cations/atoms in the lattice. As force is applied, layers of ions move but do not seperate as the bonding between electrons and ions in non-directional and not disrupted by rearrangement. (is malleable)

25
Q

force on ion

A

3-D arrangement of alternating + and - ions. When force is applied, layers of lattice slide over each other, causing + ions to align with + ions and - ions to align with - ions. This introduces repulsive forces to lattice and bonding is disrupted as the lattice breaks apart (shatters)

26
Q

non-polar / non-polar solubility

A

both are non-polar, so attractions are strong enough to overcome existing attractions/bonds, allowing it to dissolve

27
Q

molecule vs covalent network melting/subliming

A

difference in attractive forces leads to difference in energy needed to break these bonds