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Chemistry > Structure and bonding > Flashcards

Structure and bonding Flashcards

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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
Q

why does silicon dioxide have a high melting point

A

many strong covalent bonds and needs a lot of energy to break

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26
Q

what are the similarities between graphite and graphene

A

both giant covalent
both made of carbon
both have carbon bonded to 3 others
both have delocalised electrons
both have hexagonal structure

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27
Q

what are the differences between graphite and graphene

A

graphite has layers whereas graphene has only one layer

28
Q

why is graphene strong

A

lots of strong covalent bonds carbon bonded to 3 others

29
Q

why does graphene conduct electricity

A

delocalised electrons that can move through the structure

30
Q

what is an allotrope

A

different physical forms of an element

31
Q

what can carbon form

A

cage like structure called a bucky ball (buckminster fullerene)

32
Q

what can graphene form

A

tube like structure called a nanotube

33
Q

what are the properties of polymers

A

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
Q

how big are nanoparticles

A

1-100 nano meters across
contain a few hundred atoms

35
Q

how big is a nanometre

A

1 x 10-9

36
Q

what are the properties of nanoparticles

A

large sa
react faster than normal sized particles
smaller than fine particles

37
Q

what are nanoparticles used for

A

catalysts
in socks
suntan cream
tennis balls
sensors
building materials
lubricant coatings

38
Q

how do you work out surface area

A

(length x width) x number of faces

39
Q

why does a nanoparticle have different properties to the bulk chemical its made from

A

high surface area to volume ratio

40
Q

what are the disadvantages of nanoparticles

A

may be toxic
may be able to enter the brain from the bloodstream and cause harm

41
Q

what are the structures of metallic substances

A

lattice structure
electrons in outer shell of metal atoms are delocalised
strong forces of attraction between positive metal ions and negative electrons

42
Q

why do metallic substances have high melting and boiling points

A

strong electrostatic attraction between the metal atoms and delocalised electrons
needs a lot of energy to break

43
Q

why are metallic substances good electrical conductors

A

delocalised electrons can carry charge and move freely through the metal

44
Q

why are metallic substances good thermal conductors

A

when a metal is heated the delocalised electrons gain kinetic energy and move faster
this movement transfers the gained energy through the metal

45
Q

why are metallic substances malleable

A

pure metals are soft
layers of metal ions are able to slide

46
Q

what is an alloy

A

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
Q

what are polymers

A

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
Q

what is a hydroxide ion

A

OH-

49
Q

what is a nitrate ion

A

NO -
3

50
Q

what is a sulfate ion

A

SO 2-
4

51
Q

what is a carbonate ion

A

CO 2-
3

52
Q

what three things affects how strong the forces of attraction are between particles

A

material
temperature
pressure

53
Q

how close are the particles in solids

A

very close in a very regular pattern

54
Q

what are the forces of attraction like between solid particles

A

strong forces of attraction

55
Q

how do the particles move in a solid

A

can’t move but vibrate around a fixed point

56
Q

what are the energy levels like of a solid particle

A

low energy

57
Q

how close are the particles in a liquid

A

close together but irregular pattern

58
Q

what are the forces of attraction like in a liquid

A

small forces

59
Q

how do the particles move in a liquid

A

move in any direction

60
Q

what is the energy level of particles in a liquid

A

lower than gases
higher than liquids

61
Q

how close are particles in a gas

A

far apart

62
Q

how close are particles of a gas

A

far apart

63
Q

what are the forces of attraction like between gas particles

A

no forces of attraction

64
Q

how do particles move in a gas

A

any direction

65
Q

what is the energy level of particles in a gas

A

high

Chemistry (36 decks)

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