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Chemistry > C2/Bonding > Flashcards

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
Q

true or false?

the stronger the forces between the particles the lower the melting point and boiling point of the substance

A

false.

the stronger the forces between the particles the higher the melting point and boiling point of the substance

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26
Q

name 3 limitations with the simple particle model for solids, liquids and gases

A

no forces are shown
all particles are represented as spheres
the spheres are solid and inelastic

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27
Q

what state of matter is represented by (l)?

A

liquids

28
Q

what state of matter is represented by (s)?

A

solids

29
Q

what state of matter is represented by (g)?

A

gas

30
Q

what state of matter is represented by (aq)?

A

aqueous solution

31
Q

ionic compounds form regular structures (giant ionic lattices) which have what type of forces of attraction?

A

strong electrostatic forces of attraction in all directions between oppositely charged ions

32
Q

why do compounds that form giant ionic lattices have high melting points and high boiling points?

A

because of large amounts of energy needed to break the many strong bonds

33
Q

when melted or dissolved in water ionic compounds conduct electricity?

A

conduct electricity

34
Q

why can melted or dissolved ionic compounds conduct electricity?

A

because the ions are free to move and so the charge can flow

35
Q

substances that consist of small molecules are usually gases or liquids. do they have relatively low or high melting points and boiling points?

A

low melting and boiling points

36
Q

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?

A

intermolecular forces

37
Q

true or false?
the intermolecular forces increase with the size of the molecules, so larger molecules have higher melting and boiling points

A

true

38
Q

polymers are what type of molecule?

A

very large molecules

39
Q

the atoms in the polymer molecules are linked to the other atoms by what type of bond?

A

strong covalent bonds

40
Q

true or false?
the intermolecular forces between polymer molecules are relatively strong and so these substances are gases at room temperature?

A

false.
the intermolecular forces between polymer molecules are relatively strong and so these substances are solids at room temperature

41
Q

substances that consist of giant covalent structures are solids with what type of melting point?

A

very high melting points

42
Q

all of the atoms in giant covalent structures are linked to other atoms by what type of bond?

A

strong covalent bonds

43
Q

why do metals have high melting and boiling points?

A

due to their strong metallic bonding

44
Q

in pure metals, atoms are arranged in layers, what does this allow to happen?

A

it allows metals to be bent and shaped

45
Q

pure metals are too soft for many uses and so are mixed with other metals to make harder what?

A

alloys

46
Q

why are metals good conductors of electricity?

A

because the delocalised electrons in the metal carry electrical charge through the metal

47
Q

why are metals good conductors of thermal energy?

A

because energy is transferred by the delocalised electrons

48
Q

diamond is a giant covalent structure.

how many covalent bonds form between each carbon atom?

A

four

49
Q

why is diamond very hard, with not a very high melting point and does not conduct electricity?

A

because the four covalent bonds between the carbon atoms

50
Q

in graphite how many covalent bonds form between each carbon atom?

A

three

51
Q

describe the layers in graphite

A

layers of hexagonal rings which have no covalent bonds between the layers

52
Q

why does graphite conduct electricity?

A

because one electron from each carbon atom is delocalised and free to move throughtout the whole structure

53
Q

what do we call a single layer of graphite that has properties that make it useful in electronics and composites?

A

graphene

54
Q

what are fullerenes?

A

molecules of carbon atoms with hollow shapes

55
Q

the structure of fullerenes is based on carbon atoms joined in what shape?

A

hexagonal rings

56
Q

the first fullerene to be discovered was Buckminsterfullerene (C60) which has what shape?

A

spherical shape

57
Q

what shape are carbon nanotubes?

A

cylindrical fullerenes with very high length to diameter ratios

58
Q

what are fullerenes used for?

A

nanotechnology
electronics
materials

59
Q

nanoscience refers to structures that are what size?

A

1-100 nm in size

60
Q

what type of particles are smaller than fine particles (PM2.5) which have diamters between 100 and 2500 nm.

A

nanoparticles

61
Q

what type of particles have diameters between 1 x 10-5m and 2.5 x 10-6m ?

A

coarse particles

62
Q

coarse particles are often referred to as what?

A

dust

63
Q

nanoparticles may have properties different from those for the same materials in bulk because of what?

A

their high surface area to volume ratio

64
Q

the high surface area to volume ratio of nanoparticles means how much can be used?

A

smaller quantities than normal sized particles

65
Q

nanoparticles have many applications.

name some of these.

A 
in medicine
in electronics
in cosmetics
in sun creams
in deodorants
in catalysts
66
Q

the applications for nanoparticles an important area of what?

A

research

Chemistry (10 decks)

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