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Chemistry > Bonding and structure Y10 > Flashcards

Bonding and structure Y10 Flashcards

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1
Q

What ia an isotope

A

Atoms of the same element that have different numbers of neutrons

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2
Q

definition of relative atomic mass(RAM)

A

is the avarage mass of one atom compared to the mass of an atom of carbon-12

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3
Q

when do atoms become negatively charged?

A

If they gain electrons, non-metals

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4
Q

name of positive ions

A

cations

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5
Q

when do atoms becomo positively charged

A

when they lose an electron, metals

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6
Q

name of negative ions

A

anions

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7
Q

what is the force of an ionic bound

A

electrostatic force of attraction

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8
Q

how are ionic compound held togheter

A

bys trong forces of attraction between their oppositevely charged ions. called ionic bonding

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9
Q

why do ionic compound have high melting points

A

takes lot of energy to break the many strong ionic bonds, operating in all directions, that hold a giant ionic lattice togheter.

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10
Q

can ionic compound conduct electricity

A

only when molten or dissolved in water because their ions can then become mobile and can carry charge through the liquid.

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11
Q

What is a covalent bond?

A

A chemical bond formed when two or atoms share electrons.

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12
Q

what is the structure of an ionic compund?

A

Giant ionic lattice that is held togethere by the strong bonds.

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13
Q

covalent bonding can only happen with

A

NON METALS

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14
Q

what is a simple molecular structure?

A

a substance made up of simple molecules which contain only a few atoms held together by covalent bonds

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15
Q

What is a giant covalent structure?

A

All the atoms are linked by strong covalent bonds

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16
Q

Why do simple molecules have low melting points and boiling points?

A

the forces between simple molecules are weak. there are weak intermulecular forces

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17
Q

Can simple molecular substances conduct electricity?

A

nope because they have no overall charge,

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18
Q

how are the atoms arranged in in a diamond?

A

tetrahedrally, each carbon is bonded covalently to 4 other carbon atoms

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19
Q

structure of a diamond

A

giant molecuar structure

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20
Q

can a diamond conduct electricity

A

No because there are no free electrons to carry the electrical charge

21
Q

why is a diamond rigid?

A

because of the strong covalant bonds

22
Q

How are carbon atoms arranged in the graphite?

A

it has a giant structure and the atoms are arrenged in layers in which the carbon atoms are arranged hexagonally.

23
Q

How are carbon atoms arranged in the graphite?

i

A

ach atom form 3 covalant bonds, which are strong

24
Q

why are there weak intermolecular forces in a graphite

A

here are no covalant bons between the layers

25
Q

why can layers of graphite slide over each other

A

there are no covalant bons between the layers so there are weak intermolecular forces that can be easily broken

26
Q

Why graphite conducts electricity

A

because only 3 of the four electrons needed for the bonding, there is a delocalised electron who can move andcarries a charge through the substance

27
Q

What is buckminsterfullerene?

A

Also known as C60, where 60 carbon atoms form a ball, made up of hexagons and pentagons, with the formula C60. third family of carbon allotrop

28
Q

what are carbon nanotubes

A

A nanotube resembles a layer of graphene, rolled into a tube shape, they are strong and conduct electricity

29
Q

Properties of buckyballs

A

They are made up of large molecules but do not have a giant covalent structure. Weak intermolecular forces exist between individual buckyballs. Little energy is needed to overcome these forces, so substances consisting of buckyballs are slippery and have lower melting points than graphite or diamond.

30
Q

grephene structure

A

A single layer of graphite one atom thick.

31
Q

Graphene properties

A

strong and high melting point= atoms joined by covalent bonds.
conduct electricity because of the delocalised electrob

32
Q

uses of fuelleneres

A

transport mechanism for drugs to specific sites in the body, catalysts, reinforcement for composite materials

33
Q

uses of graphene

A

electronic industry

34
Q

structure of metallic bonding

A

giant metallic lattice

35
Q

what is metallic bonding

A

the chemical bonding that results from the attraction between the positive metal ions and the surrounding sea of electrons

36
Q

what is the force between the positive ions and the delocalised electrons in the metallic bonding

A

electrostatic force of attraction

37
Q

why are metallic substances good conductors

A

delocalised electrons are free to move and carry a charge through the whole structure

38
Q

why are metallic substances malleable and ductile

A

because the metal ions/atoms are arranged in neat rows that can slide over each other

39
Q

what is an alloy

A

mixture of two different types of metal (metal and non metal)

40
Q

why are alloys stronger than pure metals

A

because there are different sized atoms, it’s not easy to push one row of atom over another

41
Q

examples of alloys

A

aluminium-titanium for aereoplanes
nickel-copper for coins
titanium-cobalt for hip joints

42
Q

what is steel

A

the most common alloy

43
Q

different types of steel

A

low carbon steel-malleable, so easy shaped
high carbon steel- hard, more brittle
stainless steel- resists rust and shiny

44
Q

what is nanotube

A

study of nanopartclles that are between 1 and 100 nanometres in size

45
Q

characteristic about nanoparticles

A

high surface area to volume ratio, with a high percentage of atoms eposed at their surface

46
Q

what happen when when the side of a cube decreases, in size by a factor of 10

A

its surface area to volume ratio increases by 10

47
Q

uses of nanoparticles

A

-suncream which helps to prevent skin cancer but the
nanoparticles could potentially cause brin damage.
- side of a milk cartoon

48
Q

what is a compound

A

two or more elements that are chemically bonded togheter

Chemistry (14 decks)

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