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Chemistry > Structure and bonding > Flashcards

Structure and bonding Flashcards

(65 cards)

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1
Q

what is an ionic bond

A

particles are oppositely charged ions
occurs in compounds formed in metals combined with non metals

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2
Q

what is a covalent bond

A

particles are atoms which share pairs of electrons
occurs in most non metallic elements and in compounds of non metals

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3
Q

what is a metallic bond

A

particles are atoms which share delocalised electrons
occurs in metallic elements and alloys

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4
Q

describe the bonding in magnesium oxide

A

magnesium loses 2 electrons to become 2+ ion
oxygen gains 2 electrons to become 2- ion
magnesium transfers the 2 electrons to oxygen
there is an electrostatic attraction between the oppositely charged ions
this forms an ionic bond

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5
Q

why do ionic compounds have a high melting point

A

strong electrostatic attraction between oppositely charged ions
stops them moving further apart
needs a lot of energy to break the bond

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6
Q

why are ionic compounds soluble

A

the ions can separate in water

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7
Q

why do ionic compounds not conduct electricity as a solid

A

ions are fixed in the lattice structure and can’t move

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8
Q

what are ionic compounds

A

giant lattice structure of ions
held together by electrostatic forces of attraction between oppositely charged ions

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9
Q

why do ionic compounds conduct electricity as a solution

A

ions can move in water

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10
Q

what is small covalent bonding

A

contain a few bonded atoms

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11
Q

what is giant covalent bonding

A

millions of atoms are joined together

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12
Q

describe the bonding between hydrogen and chlorine

A

hydrogen has 1 electron in outer shell
chlorine has 7 electrons in outer shell
to get full outer shell , hydrogen and chlorine share an electron each
the sharing of a pair of electrons is called a covalent bond

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13
Q

why do small covalent structures have a low melting point

A

weak intermolecular forces
takes a small amount of energy to break them

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14
Q

why do small covalent structures not conduct electricity

A

molecules have no charge and are neutral
molecules cannot move and conduct electricity

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15
Q

what are the properties of diamond

A

giant covalent
each carbon is bonded to 4 others
lots of strong bonds

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16
Q

why does diamond not conduct electricity

A

no delocalised electrons that can move

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17
Q

why does diamond have a high melting point

A

strong covalent bonds as each carbon bonded to 4 others, needs a lot of energy to break

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18
Q

what are the properties of graphite

A

soft/slippery
made of layers
weak intermolecular forces
each carbon bonded to 3 others
delocalised electrons

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19
Q

why is graphite soft and slippery

A

layers can slide over each other because there are weak forces between them

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20
Q

why can graphite conduct electriciy

A

delocalised electrons that can move through the whole structure

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21
Q

why does graphite have a high melting point

A

giant structure lots of covalent bonds
each carbon bonded to 3 others
needs a lot of energy to break bonds

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22
Q

what are the properties of silicon dioxide

A

each silicon is bonded to 4 oxygens

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23
Q

why is silicon dioxide hard

A

giant structure and has lots of covalent bonds

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24
Q

why does silicon dioxide not conduct electricity

A

no delocalised electrons that can move

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25
why does silicon dioxide have a high melting point
many strong covalent bonds and needs a lot of energy to break
26
what are the similarities between graphite and graphene
both giant covalent both made of carbon both have carbon bonded to 3 others both have delocalised electrons both have hexagonal structure
27
what are the differences between graphite and graphene
graphite has layers whereas graphene has only one layer
28
why is graphene strong
lots of strong covalent bonds carbon bonded to 3 others
29
why does graphene conduct electricity
delocalised electrons that can move through the structure
30
what is an allotrope
different physical forms of an element
31
what can carbon form
cage like structure called a bucky ball (buckminster fullerene)
32
what can graphene form
tube like structure called a nanotube
33
what are the properties of polymers
very large molecules atoms in polymer molecules are linked to other atoms by covalent bonds intermolecular forces are strong so they are solids at 20 degrees
34
how big are nanoparticles
1-100 nano meters across contain a few hundred atoms
35
how big is a nanometre
1 x 10-9
36
what are the properties of nanoparticles
large sa react faster than normal sized particles smaller than fine particles
37
what are nanoparticles used for
catalysts in socks suntan cream tennis balls sensors building materials lubricant coatings
38
how do you work out surface area
(length x width) x number of faces
39
why does a nanoparticle have different properties to the bulk chemical its made from
high surface area to volume ratio
40
what are the disadvantages of nanoparticles
may be toxic may be able to enter the brain from the bloodstream and cause harm
41
what are the structures of metallic substances
lattice structure electrons in outer shell of metal atoms are delocalised strong forces of attraction between positive metal ions and negative electrons
42
why do metallic substances have high melting and boiling points
strong electrostatic attraction between the metal atoms and delocalised electrons needs a lot of energy to break
43
why are metallic substances good electrical conductors
delocalised electrons can carry charge and move freely through the metal
44
why are metallic substances good thermal conductors
when a metal is heated the delocalised electrons gain kinetic energy and move faster this movement transfers the gained energy through the metal
45
why are metallic substances malleable
pure metals are soft layers of metal ions are able to slide
46
what is an alloy
a mixture of two or more different metals not a compound because the metals do not react together other metal distorts the layers so they cannot slide over each other now the alloy is harder
47
what are polymers
lots of small units linked together to form a long molecule that has repeating sections all the atoms in a polymer are joined by strong covalent bonds
48
what is a hydroxide ion
OH-
49
what is a nitrate ion
NO - 3
50
what is a sulfate ion
SO 2- 4
51
what is a carbonate ion
CO 2- 3
52
what three things affects how strong the forces of attraction are between particles
material temperature pressure
53
how close are the particles in solids
very close in a very regular pattern
54
what are the forces of attraction like between solid particles
strong forces of attraction
55
how do the particles move in a solid
can't move but vibrate around a fixed point
56
what are the energy levels like of a solid particle
low energy
57
how close are the particles in a liquid
close together but irregular pattern
58
what are the forces of attraction like in a liquid
small forces
59
how do the particles move in a liquid
move in any direction
60
what is the energy level of particles in a liquid
lower than gases higher than liquids
61
how close are particles in a gas
far apart
62
how close are particles of a gas
far apart
63
what are the forces of attraction like between gas particles
no forces of attraction
64
how do particles move in a gas
any direction
65
what is the energy level of particles in a gas
high

Chemistry (36 decks)

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