Bonding Flashcards

1
Q

What is ionic bonding

A

occurs between metal and non metal includes donation of electrons from metals to non metal positive and negative ions are formed

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2
Q

what is the structure and forces of attraction like in ionic bonding

A

each posutuve ion attracts all negative ions and all negative ions attract all positive ions this leads to electrostatic forces in all directions forming an ionic lattice

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3
Q

what is the properties of ionic compounds

A

they are always solid at room temperature as the strong electrostatic forces means a large amount of energy is required so have high melting points
in molten or aqueous conditions the ions are free to move and can can carry charge thus can conduct electricity

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4
Q

why do ionic compounds shatter easily

A

there is alternativing posutinve and negative ions held by electrostatic forces when given a sharp blow there is movement in the lattice which may make two ions of same charge come close togther causing repulsion and causes shattering

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5
Q

what is covalent bonding

A

bonding between two non metals
the atoms share some of their outer electron so that each atom has a stable electron structure
covalent bond is a shared pair of electron

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6
Q

how does sharing of electrons hold atoms together

A

the atoms are held by the forces of attraction between the electrons and the nucleasthis takes place wthin the molecules, molecules are not strongly attracted together only in molecules there are strong electrostatic forces

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7
Q

what is coordinate bonding

A

one atom provides both of the electron

the atom that accepts the pair is called electron deficient and the atom donative electron has a lone pair of electrons

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8
Q

what way does the arrow point

A

twoards the atom accepting the electron pair

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9
Q

what is metallic bonding

A

the outer electrons leave the main outer shell and fom a sea of delocalised electrons with positive ions the positive ions repel each other this is balanced out with the attraction between the negative particles and the electrons

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10
Q

what is the strength dependent on in metallic bonding

A

the shielding of electrons each atom and the positive charge on the positive ion

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11
Q

properties of metals and metallic bonding

A

they are good conductors of heat the vibrating causes allte delocalised electrons to vibrate and the closely packed ions
they are also good conductors of electricity the electron flows to the positive terminal

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12
Q

strength of metals

A

theya re ductil and can be pulled into wres and are mallaeble and dont shatter easily this is because the delocalised electrons are not associated with any particular ions and can move freely throught the strucure

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13
Q

what are crystals

A

they are solids which particleshave regular arrangement and are held together by forces of attractiob

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14
Q

iodine molecular crystals

A

van der waal forces hold the the pairs of iodine molecules together to hold the molecules together as a solid

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15
Q

what is diamond

A

made from pure carbon bonded to four other carbon atoms bond angle of 109.5 tetrahedral its very hard, high melting point doesnt conduct electricity as no free electrons to carry charge

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16
Q

what is graphite

A

pure carbon each carbon atom is covalently bonded to three other carbon atoms the carbon attoms are arranged in layers with weak intermolecult=ar forces between the layers the extra electron forms a layer above and below the hexagonal plane so electricity is conducted parallele to the plane as there are no convalent bonds between the layers only weak intermolecular forces the layers can slide over each other making graphite very slippery and flaky

17
Q

Why can metals be pulled into wired

A

They are in layer so can be pulled and slide over each other