Structure & Bonding Flashcards

1
Q

what does bonding mean/describe

A

how the electrons are distributed to make chemical bonds

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2
Q

what do noble gases do/have

A
  • a full outer shell
  • do not need to bond
  • exist as single atoms and all exist as gases at room temperature
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3
Q

what is a covalent bond

A

the attraction between the positive nuclei and a shared pair of electrons

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4
Q

bonding between individual molecules

A

is not covalent and is weak

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5
Q

why do simple covalent molecules have low melting and boiling points

A
  • attraction between molecules and are very weak

* easy to separate the molecules

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6
Q

carbon exists in two forms / allotropes

A

diamond and graphite

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7
Q

structure and bonding of diamond

A

covalent bond, giant molecular lattice structure

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8
Q

bond of carbon as diamond

A

each carbon atom is covalently bonded to 4 other carbon atoms in a tetrahedral arrangement

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9
Q

uses of diamond

A
  • drill bits to cut through rocks

* jewellery

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10
Q

why are large amounts of energy required to break diamond

A
  • covalent bonds extend through the crystal in a lattice
  • each diamond is a single giant molecule
  • large numbers of strong covalent bonds
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11
Q

graphite bonding and structure

A

covalent bond, layer lattice structure

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12
Q

how are the carbon atoms bonded in graphite

A

carbon atoms bonded covalently to 3 other carbons within layers to form a hexagon of atoms.

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13
Q

why is graphite soft and slippery

A

only weak intermolecular forces holding layers together so the layers of atoms can easily slide over eachother

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14
Q

what can graphite conduct

A

electricity

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15
Q

uses of graphite

A

lubricant, pencils, used as electrodes

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16
Q

what is metallic bonding

A

attraction between a lattice of positive ions and a sea of delocalised electrons

17
Q

why are metals strong and have high melting points and boiling points

A

strong electrostatic attraction between positive ions and negative electrons means that a lot of energy is required to separate the particles from the lattice

18
Q

why are metals malleable

A

less energy is required to slide one layer of positive metal ions over another layer

19
Q

why are metals good conductors of electricity

A

if a potential difference is applied across a piece of metal, the electrons will move, carrying an electrical current

20
Q

what is an alloy

A

mixture of metals

21
Q

why are alloys stronger and harder than normal metal

A

always contain atoms of different sizes, which distorts regular arrangements of atoms. makes it more difficult to slide over eachother, so alloys are harder

22
Q

what is ionic bonding

A

where ions are held together by strong electrostatic attractions between oppositely charged ions

23
Q

why are there high b/m points in ionic bonds

A

strong electrostatic attractions

24
Q

conductivity in ionic bonds

A
  • can only conduct when melted or dissolved when ions can move
  • when solid they cannot move so cannot conduct
25
Q

why is carbon dioxide a gas at room temperature but silicon dioxide is a solid

A
  • co2 has weak intermolecular forces between molecules

* sio2 is a giant molecular structure that only has strong covalent bonds that have to be broken

26
Q

why is diamond hard but granite soft

A
  • diamond is a giant molecular lattice. has strong covalent bonds which are hard to break
  • graphite is a layer latice. layers of atoms can slide over eachother
27
Q

what does structure mean/describe

A

it describes how the atoms, ions or molecules are arranged in a solid