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Chemistry > C3-Structure and Bonding > Flashcards

C3-Structure and Bonding Flashcards

1
Q

What are the three common states of matter ?

A

Solid , liquid , gas .

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2
Q

One fact about solids .

A

-Solids are extremely hard to compress (squeeze) , as particles in a solid are packed togteher in a regular pattern , with almost no spaces between the particles .

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3
Q

Another fact about soilds .

A

Solids have a fixed shpe and cannot flow from place to place ..
-Solid particles can virbate but can’t move place to place .

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4
Q

One fact about Liquids .

A

-Liquids are extremly hard to cpmress - as particles are close togetehr with not many spaces between them .

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5
Q

Another fact about Liquids .

A

-Unlike soilds , liquids tkae the shpe of their container , they flow from place to place , as particles in a liquid can mvoe .

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6
Q

Fact about gases .

A

-Gases are extremely easy to compress . As particles in gases are widely spaced .
-Gases spread out and fill the space of their container , As particles in a gas move quickkly and randomly .

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7
Q

How can we change the state of a substance ?

A

By puttign in or taking out energy .

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8
Q

How do we change a solid to a liquid .

A

Called melting , takes place at meltign point .
-Particles in a liquid moving , so hae more inetic energy than particles in a solid .
-Means have to put energy to convert solid to liquid , energy needed to break down forces of atraction between partciles in solid , ater broken , forces can move .

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9
Q

The stornger the ofrces of attraction between the particles …

A

The more energy we have to put in to break them and the higher the melting points .
Wax candle - low melting point s forces of attraction weak between particles easy to break .
-sodiumc hlrid e, storng ofrces of attraction between particles so high melting point .

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10
Q

Liquid to solid

A

freezing temperature at melting point .

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11
Q

Liquid to gas .

A

-Boiling point
-Stronger forces of atrraction between particles means boiling point high , as it takes a lot of enegry to break down forces to boil the liquid .
Gas to liquid condensing , the temperature for this is boiling point .

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12
Q

What is one limitation of the particle model ?

A

-Assumes all the particles are soild spheres , not true as the particles have lots of different shapes are not solid .

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13
Q

What is another limitation of the particle mdoel ?

A

Simple particle model assumes there are no forces between particle s, this is not the cses , forces have a major impact on melting and boiling point of a substance .

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14
Q

Whyd o elements react ?

A

-To gain an a full outer shell
-When a metal reacts with a non metal its called IONIC BONDING .

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15
Q

Do some ionic bonding questions .

A

:))

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16
Q

Check sheet ,
Describe what is happening in this reaction (4)

A

-One electron
-Passes from the sodium atom
-To Chlorine atom
-Both atoms achieve a full outer energy level .

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17
Q

What do ionic compounds form ?

A

The form giant structures (giant ionic lattices )
-Where a positive ion i surrounded in a negative ion .

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18
Q

More about giant ionic lattice’s

A

-They are 3 Dimensional
-Have very strong electrosatic forces of attraction , between positive and negative ions , holding them in place , and can act in all direction s.

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19
Q

What is one key property of ionic compounds >

A

-They have very high melting and boiling points , as thr strong electrostatic forces requrie a great deal of energy to break .

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20
Q

What is another kery property of ionic compounds ?

A

Ionic compounds cannot conduct electricity when theya re soilkds , as the ions can’t move , they are locked in place by the strong electrostaic forces of attraction .

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21
Q

Whenc an ionic compounds conduct electricity ?

A

-When they are melted or dissolved in water , as the ions can now move and carry the charge NOT ELECTRONS .

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22
Q

Practice some Covalent bonding questions .
-work out how manhy electrons outer shell UNLIKE IONIC.
-thuink how many each element needs for full outer shell

23
Q

What are the boiling points of small covalent moelcules ?

A

-Small covalnet molecules have a low melting and boiling point .
-Menaing they are are usually gases or liquids at room temperature .

24
Q

Why do small covalent bonds have low melting and boiling points .

A

-As threy have weak intermolecualr forces bettween the molecule to another molecule , which odn’t require a lot of energy to brek .

25
Expalin porcess of breaking bonds in small covalnet sturctures .
-Atoms in each molecule held togther by strong covalne tbonds . -but weak intermolecular forces , one movleucle to another , don;t requrie a lot of nergy to break . -Increas the temperature anf the vibrations increase , at a point , vibrations strong enough to break the waeak intermolecular forces holding mollecules togther - turn into a gas .
26
As we increase the size of the covlent molecules ...
intermolecular forces increase .
27
Why don't small covalnet molecules no conduct electriciy ?
As the molecules do not have an overall electric charge .
28
State of giant covalent moelcules at room tempeature ?
Giant covalent molecules are always solid at room temperature . As giant covalent molecules have millions of strong covalent bonds . -Menaing they have high melting and boiling ponts . /
29
Example of a giant covalentmolecule .
Diamond is a form of the elemnt carbon . -Each carbon atom forms four strong covalnet bonds to four other carbon atoms . -Diamond have a huge number of covalent bonds , these hae o be broken when diamond melted ,reequiring a great dela of energy . Melting point 3700 degrees .
30
Why can't diamond conduct electricity ?
As there are no free elctrons to carry elecrical charge .
31
Another covalent molecule ?
Silicon Dioxide (Silica /Sand ) . -Silicion dioixide has a very high melting and oiling point . -As the number of strong covalent bonds mus e broken , this takes a great deal of energy .
32
Give a few propertie of graphite .
-Has a high metlign and boilign point . -Is soft and slippery . -escvellent conductor of both electricty and heat .
33
Structure of graphite .
-Grpahite formed from the elemnt Carbon . Each carbona toms froms three covalent bonds . -Carbon atoms from heaxagonal rings .
34
Why does graphite have a high mp and bp ?
-As graphite has many strong covalent bonds , takes a great deal of energy to break these , so graphite has a high mp and bp .
35
Why is graphite slippery ?
-The hexagonal rings are in layers . NO covalent bonds betwen layes so can slide , making graphite slippery .
36
Why can graphite conduct electricity ?
Carboon froms three bonds , single elctron on outer shell that isn''t ina covalent bond . -These are delocalised electrons meanin they can move and conduct therml energy and electircity .
37
is graphite a metal ?
NO , graphite is based on the elemtn carbon and not a metal . -Grpahite is similar to metals as both ar good condcutors of heat and electricity , as both have delocalised electrons that can move .
38
What is graphene ?
Grpahene is a single layer of graphite . -Graphene is one atom thick .
39
Propertieis of graphene .
-Excellent conductors of electricity as it has delocalised electrons . -Graphene is extremely strong .
40
What are fullerenes ?
-Fullernes are moelcules of crbon stoms with hollow shapes . -Usually fullerenes have hexagnoal rings of carbona toms but also or 7 rings of carbon toms .
41
What is te first fullerene discoevred ?
Buckminster Fullerne , ahs 60 carbon atoms - carbon atoms form rings orf 5 or 6 carbons .
42
What are some uses of Fullerenes .
-Pharmacueticla delivery into bodiey . -Lubricant -Catalysts .
43
What are Carbon nano tubes .
Fullernes hsaped into long cylidners .
44
What are two properites of carbon nano tubes .
-High tensile strength (strech without breaking ) -Excellent conductors of hea and electricty and used to reinforce metals like tennis rackets .
45
Structure of metals .
Metals consitis of a giant structrue of atoms arranged regularly - electrons in the outer energy leevel of each atom is delocalised
46
structure of metals .
Strong electrostatic attracting between the sea of delocalsied negative electros and positive ions . the electrostatic attracts in metla sare the metalic bonds - which are strong .
47
Properties of meals .
Metals have high metling and boiling points ,a s a great deal of energy is required to break the strong metallic bonds .
48
Why are metals good conductors of hear and electricity .
-As the sea of delcoalised electrons can mov e, and as electrons are charged , means electrons can carry electric current and thermal energy allowign the them to conduct heat .
49
Why can metals be bent and hsaped ?
As in metals , layers of atoms are able to slie over eachother . due to deloaclised electron allowing layers to distort a little . PROBLEM - some pure metals aren't hard enough to be useufl (copper and gold) SO HAVE TO MAKE AN ALLOY . to make them harder .
50
What is an alloy , and how is is stronger than a pure metal ?
An alloy is a mixture of metals . -The different sizes of the atoms , distorts hte layers , making it more difficult for them to slide over eachtoehr . Hence why allys harder than pure metals .
51
What are nano particles .
Have a diameter of 1-100 nanometres , onlyc ontain a few hundred atoms . -As the particle size decreasesby ten times , the surface area to volume ratioio increasees byt en times . do surface area/volume
52
Nano particles have a huge surace area to volume ratio :
Small amount of nanoparticles have massive surface aea . -Much smaller quanitty of nano particles compaered tonano particle s.
53
Ues of nanoparticles .
cosemtic , sunscreen ,catlayast RISK -nanoparticles going into surroundings can damage the lungs when breathing in tinny particles as it possible for them to be absorbed into body and cells adn can enter blood stream . possibly .
54
problems with dot and cross diagrams
-dosent shwo the strucutre of compoud -the size of the ions -or how the ions are arranged

Chemistry (20 decks)

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