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bonding, structure and the properties of matter Flashcards

1
Q

process from solid to gas and vice versa

A

sublimation

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2
Q

difference between evaporation and boiling

A

evaporation - particles leave liquid from surface only

boiling - bubbles of gas form throughout liquid

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3
Q

what is stronger, ionic bonds or bonds between simple molecules

A

ionic bonds

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4
Q

2 limitations of the particle model

A
  • particles mostly empty space

- not spherical

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5
Q

how is an ionic bond formed

A

when a metal and a non-metal react with each other

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6
Q

what is an ionic lattice

A

the regular arrangement of irons in an ionic substance

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7
Q

how are ionic lattices held together

A

with strong electrostatic forces

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8
Q

which direction do forces of attraction from ions act in

A

all directions

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9
Q

why do ionic compounds have high boiling and melting points

A

because of their strong electrostatic forces of attraction

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10
Q

what do strength of ionic bonds depend on

A

the charge of ions, higher charge will have stronger forces

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11
Q

when can a substance conduct electricity

A
  • if it contains charged particles such as ions

- can move place to place

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12
Q

when can an ionic compound conduct electricity

A
  • when it’s melted to form a liquid

- dissolved in liquid to form aqueous solution

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13
Q

where does covalent bonding mostly occure

A

in non-metal elements

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14
Q

what is a double and triple bond in covalent bonding

A

double - 2 shared pairs of electrons

triple - 3 shared pairs of electrons

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15
Q

why do small molecular substances have low melting and boiling points

A

they have weak intermolecular forces in comparison to the covalent bonds in the molecules

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16
Q

how to change strength of intermolecular forces

A

bigger the molecule, stronger the intermolecular force

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17
Q

can covalent bonds conduct electricity

A

no

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18
Q

what happens to covalent bonds when substances melt or boil

A

they don’t change

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19
Q

what are melting and boiling points on giant covalent structures

A

very high, large amounts of energy needed to overcome strong covalent bonds

20
Q

can giant covalent structures conduct electricity

A

no except for graphite

21
Q

how is diamond structured

A
  • each carbon atom joined to four others by strong covalent bonds
  • repeating tetrahedal structure
  • no free electrons
22
Q

how is graphite structured

A
  • each carbon atom jointed to 3 others by strong covalent bonds
  • carbon atoms form layers of hexagonal rings
  • no bonds between layers
  • one delocalised electron from each atom
23
Q

why is graphite good as a lubricant

A

it’s slippery as the forces between layers are weak so easily slip off

24
Q

why does graphite conduct electricity

A

has delocalised electrons that are free to move between layers

25
Q

properties of graphene

A
  • very high melting point

- very strong

26
Q

uses of graphene

A

electronics because delocalised electrons can move freely

27
Q

what are fullerenes

A

molecules of carbon atoms with hollow shapes

28
Q

what is buckminsterfullerene

A

molecules made of 60 carbon atoms which are spherical

29
Q

why is buckminsterfullerene slippery

A

weak intermolecular forces between each molecule that need little energy to overcome, also has low melting point

30
Q

what is a nanotube

A

like a layer of graphene rolled into a cylinder

31
Q

properties of nanotubes

A
  • strong in tension resist being stretched

- conduct electricity

32
Q

uses of nanotubes

A

nanotechnology and electronics

33
Q

what is a polymer

A

a large molecule formed by many smaller molecules known as monomers

34
Q

what are the intermolecular forces between polymer molecules

A

strong compared to forces between small molecules, high melting and boiling point solid at room temp

35
Q

what is metallic bonding

A

giant structure of metal atoms and delocalised electrons moving between them

36
Q

why are metals good conductors of thermal energy

A

delocalised electrons transfer their energy

37
Q

why do metals have high melting and boiling points

A

large amounts of energy are needed to overcome metalling bonds in melting and boiling

38
Q

what is an alloy

A

a mixture of two or more elements where at least one is a metal

39
Q

why are alloys formed

A

many pure metals are too soft so combining with another makes it harder

40
Q

why is an alloy stronger than a pure metal

A

atoms of different sizes, distort the layers of atoms, greater force required for layers to slide, alloy is harder and stronger

41
Q

what is nanoscience

A

study of structures between 1 and 100nm in size (nanoparticles)

42
Q

what is a substance made of nanoparticles called

A

nanoparticulate

43
Q

uses of nanoparticulates

A

zinc oxide is invisible when a nanoparticulate used in suncream, rather than white when in bulk

44
Q

why are nanoparticulates used as catalysts

A

they have a large surface area to volume ratio

  • more efficient
  • catalyse different reactions producing different products
45
Q

possible risks of nanoparticles

A
  • small size makes it easy to breathe in
  • can catalyse harmful reactions in body
  • toxic substances can bind because of large SA:VOL ratio

other (19 decks)

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