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elements of life > structures and properties of bonded substances > Flashcards

structures and properties of bonded substances Flashcards

1
Q

how are ions held in ionic solids`

A

by opposite charges - each cation is attracted to several anions

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2
Q

what do the ions build up into

A

a giant ionic lattice

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3
Q

are the ions in fixed positions

A

yes

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4
Q

how is the sodium chloride lattice arranged

A

each Na+ is surrounded by 6 Cl- ions
each Cl- is surrounded by 6 Na+ ions
this adds up to an infinite series of attractions and repulsions

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5
Q

which are stronger attractions or repulsions

A

attractions

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6
Q

why do ionic solids have high mp and bp and are hard

A

due to the strong lattice arrangement

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7
Q

what does NaCl have a cubic shape

A

due to the cubic NaCl crystals

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8
Q

what happens when ionic substances dissolve in water

A

the ions become surrounded by water molecules and spread out through the water

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9
Q

what happens when NaCl dissolves in water

A

the dissolved Na+ and Cl- ions are regularly scattered anymore, they are scattered randomly through the water. both ions act independantly of each other

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10
Q

what is each ion surrounded by

A

water molecules.

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11
Q

describe water

A

polar with a bent shape. oxygen is more electronegative than hydrogen

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12
Q

how do ions dissolve in water

A

positive ends of the water are attracted to the negative ions and the negative ends of the water are attracted to the positive ions

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13
Q

why does hydration release energy

A

to compensate for the immense amount of energy needed to break the bonds within an ionic lattice

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14
Q

what happens to ionic substances in water

A

when dissolved, the positive and negative ions separate and behave independantly

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15
Q

what are ionic compounds at room temperature and pressure

A

solids

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16
Q

how is the ionic lattice arranged

A

consisting of repeating +ve and -ve ions in 3D and often form regularly shaped crystals

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17
Q

how is the ionic lattice held together

A

the electrostatic attraction of oppositely charged ions overcomes the repulsion of the same charge, holding together the ionic lattice structures

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18
Q

why do ionic compounds have high melting and boiling points

A

a large amount of energy is needed to overcome the electrostatic attraction forces and break the ionic bonds to pull the ions apart

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19
Q

what happens once an ionic compound has melted

A

the ions are free to move and then can carry charge and conduct electricity

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20
Q

when can ionic compounds conduct electricity

A

if molten or dissolved since the ions can move

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21
Q

what substances do ionic compounds dissolve in

A

soluble in polar substances

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22
Q

what is the difference between carbon dioxide and sillicon dioxide

A

both are in group 4 but carbon dioxide is a gas at room temperature and SiO2 is a hard solid with a high mp

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23
Q

why do CO2 and SiO2 have different physical properties even though they are in the same group

A

there is a difference between the bonding between carbon and oxygen and sillicon and oxygen

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24
Q

what type of compounds are SiO2 and CO2

25
what type of bonds can carbon form and why
the small size of the carbon atom makes it possible for carbon to form double bonds with oxygen so carbon dioxide is composed of individual molecules
26
why is carbon dioxide a gas at room temperature
the bonds between carbon dioxide molecules are weak so little energy is needed to separate individual molecules in the solid and liquid phases to form a gas.
27
how many oxygen atoms does sillicon bond to
four oxygen atoms (larger than carbon atoms)
28
what is quartz
an extended network of SiO4
29
describe some properties of SiO2
because of its giant covalent structure, SiO2 is insoluble in water and has a high mp and bp. this is due to the strong covalent bonding which exists throughout the SiO2 structure. lots of energy needed to break bonds within the structure
30
what are two types of covalent structures
covalent molecular/simple molecular covalent network/giant covalent
31
what are some properties of covalent molecular structures
- consists of discrete molecules. - strong covalent bonds within the molecules/between atoms (intramolecular forces) - weak covalent bonds between the molecules (intermolecular forces) - some dissolve in organic solvents
32
what do the strength of the IMF determine
the state of the substance
33
what are some properties of covalent network structures
- consists of a giant repeating lattice of covalently bonded atoms. - substances with network structures are insoluble - solids with high mp and bp
34
give some names of diatomic molecules
hydrogen, oxygen, nitrogen, fluorine, and chlorine
35
what is phosphorus (P4) made of
four phosphorous atoms
36
what is sulfur (S8) made of
8 sulfur atoms in a ring
37
what is similar about S8 and P4
both are soft, low melting solids
38
describe the bonds in network structures
bonds between individual atoms are strong covalent bonds and a lot of energy is needed to pull the atoms apart to form a liquid or gas
39
what is the structure of sillicon
every sillicon is bonded to four other sillicon atoms in a tetrahedral arrangement. the giant lattice repeats the structure indefinitely in all directions
40
what are the two allotropes of carbon
diamond and graphite
41
describe the structure of diamond
every carbon atom is joined tetrahedrically to four other carbon atoms by strong covalent bonds forming a giant lattice
42
why is diamond hard
due to its highly symmetrical structure and strong C-C bonds
43
what are industrial grade diamonds used for
on the tips of drills and crushed diamonds are used on high quality grinding and cutting wheels
44
describe the structure of graphite
made up of giant flat layers of carbon atoms. each layer is a two dimensional network. in layers each carbon atom is joined by strong covalent bonds to 3 others forming rings containing 6 carbon atoms
45
what are there extended delocalised electron clouds between the layers in graphite
only 3 of the four outer electrons of carbon are used to form the hexagonal rings. the 4th electron of each atom contributes to the cloud of delocalised electrons
46
what do the delocalised electrons do in graphite
causes the layers to be held together relatively weakly. the delocalised electrons are not attached to any particular carbon atom and are free to move around over the layers
47
why is graphite a good conductor of electricity
because of its delocalised electrons that are able to move through the structure and carry charge
48
why dont most covalent substances conduct electricity
all the electrons are held tightly in covalent bonds so they arent free to move from one molecule to the next through the structure
49
give some properties of graphite
soft, brittle solid. the layers are bonded weakly to eachother so can slide over one another used as a lubricant
50
what are simple molecular substances soluble in
non polar solvents
51
what are fullerenes
molecular form of carbon. dissolves in benzene to give a red solution.
52
formula of fullerenes
C60
53
what are the two types of fullerenes
buckminsterfullerene nanotubes
54
what is C60
optical limiter shining light on a solution of C60 causes it to turn darker instantly and the more light there is the darker it gets so that the intensity of the transmitted light is limited to a maximum value
55
describe metallic compounds
- strong bonds in regular structures - high mp and bp - hard and strong - electrostatic forces acting in all directions
56
how are metallic compounds formed
- in a metal, atom loses several of its outer electrons which drift around the metal ion as delocalised electrons
57
why are metallic compounds good conductors
- good conductor of heat and electricity because of large number of free electrons
58
why are metallic compounds malleable
- regular structure means layers of atoms can fairly slide over eachother without breaking bonds so metals are malleable

elements of life (15 decks)

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