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chemistry > structure and bonding > Flashcards

structure and bonding Flashcards

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1
Q

what is an ion?

A

an atom or group of atoms that has lost or gained electrons and therefore has a positive or negative charge.

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2
Q

what is a covalent bond?

A

a bond involving shared pairs of electrons between atoms- molecules are held together by covalent bonds

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3
Q

what is metallic bonding?

A

when positively charged metal ions are surrounded by delocalised outer electrons

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4
Q

what are electrostatic forces of attraction?

A

strong forces of attraction between oppositely charged particles eg Na+ and Cl-

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5
Q

what bonds do metals and non-metals form?

A

ionic

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6
Q

what elements form covalent bonds?

A

non-metals

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7
Q

what elements form metallic bonds?

A

metals and alloys

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8
Q

what are examples of giant covalent structures?

A

diamond, graphite, silicon dioxide

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9
Q

what is a monomer?

A

a small compound whose molecules can join together to form polymers

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10
Q

what is a polymer?

A

a long molecule consisting of many similar or identical monomers linked together.

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11
Q

what is a limitation of dot and cross diagrams?

A

they do not show the 3D shape of a molecule

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12
Q

how are group numbers and charges linked?

A

the group of an element tells us the charge on that atom- eg barium is in group 2 so it has a charge of 2+, iodine is in group 7 so it has a change of -1

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13
Q

what is a giant atomic lattice?

A

a huge, 3D, regular structure of oppositely charged ions, held together by electrostatic forces.

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14
Q

what is a delocalised electron?

A

an electron that is able to move freely throughout a structure- enables charge to be carried through

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15
Q

how do ions become positive?

A

by losing outer shell electrons- number of protons in nucleus > number of electrons in shells

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16
Q

how are metals bonded?

A

they are in a lattice shape- positive ions surrounded by a sea od delocalised electrons

17
Q

why are metals malleable?

A

the layers of metal ions can slide over each other

18
Q

why are alloys harder than pure metal?

A

the differently sized atoms disrupt the layers of ions and prevent the layers from sliding

19
Q

how can ionic compounds not carry charge when solid but can when molten/in solution?

A

when they are molten the ions are free to move and carry charge whereas they are fixed in their solid state

20
Q

why do ionic substances have high boiling/melting points?

A

strong electrostatic forces between opposite ions need lots of energy to break

21
Q

what is an allotrope?

A

different forms/shapes of the same element eg diamond and graphite are carbon allotropes.

22
Q

why is diamond so hard?

A

each of the carbon atoms form 4 other covalent bonds in a tetrahedral structure, so it is very hard to break.

23
Q

how many bonds are in graphite?

A

each carbon bonds forms 3 other bonds, leaving one electron delocalised and free to carry charge

24
Q

why is graphite so soft?

A

there are strong bonds between atoms but weak IMF between layers of atoms, which means that they can slide over each other.

25
Q

what is graphene?

A

a single layer of graphite that is one atom thick. it is used in electronics and composites

26
Q

what is a composite?

A

materials made of two or more different materials, containing a matrix and a reinforcement- often used to combine desirable properties of each

27
Q

what is buckminsterfullerene?

A

carbon c60- 60 carbon atoms arranged as a hollow sphere. useful for drug administration

28
Q

what are carbon nanotubes?

A

tiny, hollow tubes made of carbon atoms with a high length to diameter ratio

29
Q

what are some properties of carbon nanotubes?

A

high tensile strength, high electrical + thermal conductivity. used in electronics and strong materials

30
Q

what are nanoparticles?

A

very very small particles- usually between 1 and 100 nanometres in size and contain only a few hundred atoms

chemistry (10 decks)

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