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C2/Bonding Flashcards

1
Q

name 3 types of chemical bond

A

ionic bond
covalent bond
metallic bond

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2
Q

ionic bonds are formed between what type of particle?

A

by the attraction between oppositely charged ions

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3
Q

ionic bonds form between what type of elements?

A

they form between a metal and a non-metal element

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4
Q

how do covalent bonds form?

A

by the sharing of electrons

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5
Q

covalent bonds form between what type of elements?

A

they form between two non-metal elements

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6
Q

how do metallic bonds form?

A

by the sharing of delocalised electrons

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7
Q

metallic bonds form between what type of elements?

A

they form between two metal elements

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8
Q

in ionic bonding metal atoms gain electrons to become positively charged what?

A

ions

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9
Q

in ionic bonding non-metal atoms gain electrons to become ions with what charge?

A

a negative charge

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10
Q

group 1 metals commonly form ionic bonds with which group?

A

group 7

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11
Q

group 2 metals commonly form ionic bonds with which group?

A

group 6

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12
Q

ionic compounds form what type of structures?

A

giant ionic lattice structures

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13
Q

ionic compounds are held together by what?

A

strong electrostatic forces of attraction between oppositely charged ions

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14
Q

when atoms share pairs of electrons, they form what type of bonds?

A

covalent bonds

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15
Q

covalently bonded substances may consist of what size molecules?

A

small molecules

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16
Q

are covalent bonds strong or weak?

A

strong

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17
Q

some covalently bonded substances have very large molecules, such as what?

A

polymers

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18
Q

name 2 covalently bonded substances that have giant covalent structures

A

diamond

silicon dioxide

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19
Q

the electrons in the outer shell of metal atoms are delocalised and so are free to move to where?

A

throughout the whole structure

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20
Q

the sharing of delocalised electrons gives rise to what?

A

strong metallic bonds

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21
Q

name the three states of matter

A

solid, liquid and gas

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22
Q

both melting and freezing take place at what temperature?

A

the melting part of the substance

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23
Q

both boiling and condensing take place at what temperature?

A

the boling point of the substance

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24
Q

the amount of energy needed to change state from solid to liquid and from liquid to gas depends on what?

A

the strength of the forces between the particles of the substance

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25
true or false? | the stronger the forces between the particles the lower the melting point and boiling point of the substance
false. | the stronger the forces between the particles the higher the melting point and boiling point of the substance
26
name 3 limitations with the simple particle model for solids, liquids and gases
no forces are shown all particles are represented as spheres the spheres are solid and inelastic
27
what state of matter is represented by (l)?
liquids
28
what state of matter is represented by (s)?
solids
29
what state of matter is represented by (g)?
gas
30
what state of matter is represented by (aq)?
aqueous solution
31
ionic compounds form regular structures (giant ionic lattices) which have what type of forces of attraction?
strong electrostatic forces of attraction in all directions between oppositely charged ions
32
why do compounds that form giant ionic lattices have high melting points and high boiling points?
because of large amounts of energy needed to break the many strong bonds
33
when melted or dissolved in water ionic compounds conduct electricity?
conduct electricity
34
why can melted or dissolved ionic compounds conduct electricity?
because the ions are free to move and so the charge can flow
35
substances that consist of small molecules are usually gases or liquids. do they have relatively low or high melting points and boiling points?
low melting and boiling points
36
gases have only weak forces between the molecules (intermolecular forces) is it the intermolecular forces or the covalent bonds that are overcome when the substance melts or boils?
intermolecular forces
37
true or false? the intermolecular forces increase with the size of the molecules, so larger molecules have higher melting and boiling points
true
38
polymers are what type of molecule?
very large molecules
39
the atoms in the polymer molecules are linked to the other atoms by what type of bond?
strong covalent bonds
40
true or false? the intermolecular forces between polymer molecules are relatively strong and so these substances are gases at room temperature?
false. the intermolecular forces between polymer molecules are relatively strong and so these substances are solids at room temperature
41
substances that consist of giant covalent structures are solids with what type of melting point?
very high melting points
42
all of the atoms in giant covalent structures are linked to other atoms by what type of bond?
strong covalent bonds
43
why do metals have high melting and boiling points?
due to their strong metallic bonding
44
in pure metals, atoms are arranged in layers, what does this allow to happen?
it allows metals to be bent and shaped
45
pure metals are too soft for many uses and so are mixed with other metals to make harder what?
alloys
46
why are metals good conductors of electricity?
because the delocalised electrons in the metal carry electrical charge through the metal
47
why are metals good conductors of thermal energy?
because energy is transferred by the delocalised electrons
48
diamond is a giant covalent structure. | how many covalent bonds form between each carbon atom?
four
49
why is diamond very hard, with not a very high melting point and does not conduct electricity?
because the four covalent bonds between the carbon atoms
50
in graphite how many covalent bonds form between each carbon atom?
three
51
describe the layers in graphite
layers of hexagonal rings which have no covalent bonds between the layers
52
why does graphite conduct electricity?
because one electron from each carbon atom is delocalised and free to move throughtout the whole structure
53
what do we call a single layer of graphite that has properties that make it useful in electronics and composites?
graphene
54
what are fullerenes?
molecules of carbon atoms with hollow shapes
55
the structure of fullerenes is based on carbon atoms joined in what shape?
hexagonal rings
56
the first fullerene to be discovered was Buckminsterfullerene (C60) which has what shape?
spherical shape
57
what shape are carbon nanotubes?
cylindrical fullerenes with very high length to diameter ratios
58
what are fullerenes used for?
nanotechnology electronics materials
59
nanoscience refers to structures that are what size?
1-100 nm in size
60
what type of particles are smaller than fine particles (PM2.5) which have diamters between 100 and 2500 nm.
nanoparticles
61
what type of particles have diameters between 1 x 10-5m and 2.5 x 10-6m ?
coarse particles
62
coarse particles are often referred to as what?
dust
63
nanoparticles may have properties different from those for the same materials in bulk because of what?
their high surface area to volume ratio
64
the high surface area to volume ratio of nanoparticles means how much can be used?
smaller quantities than normal sized particles
65
nanoparticles have many applications. | name some of these.
``` in medicine in electronics in cosmetics in sun creams in deodorants in catalysts ```
66
the applications for nanoparticles an important area of what?
research

Chemistry (10 decks)

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