Brainscape's Knowledge GenomeTM


Top Flashcards (Certified)
All Flashcards

chemistry > bonding structure > Flashcards

bonding structure Flashcards

(93 cards)

Start Studying
1
Q

what are ions

A

charged particles

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

what can ions be

A

single atoms or groups of atoms

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

what happens when metals form ions

A

they lose electrons from their outer shell to form positive ions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

what happens when non metals form ions

A

they gain electrons into their outer shell to for negative ions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

how are ions formed

A

when atoms loose or gain electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

what are ionic bonds

A

when a metal and non metal react - the metal atom loses a electron to become positively charged and the non metal gains a electron to become negativity charged

they have opposite charges that attract by electrostatic forces and this attraction is called ionic bonds

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

what elements are most likley to form ions

A

1,2,6,7

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

what is the structure of ionic compounds

A

giant ionic lattice

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

what is a example of one giant ionic lattice

A

a crystal of sodium chloride

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

what are the properties of ionic compounds

A

they have high melting and boiling points - due to strong bonds - takes a lots of energy to overcome attraction

  • when soild cant conduct electricty
  • when melted free to move so they can carry electriity
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

Why can ionic compounds only conduct electricity when in liquid/molten, or aqueous form?

A

The ions are free to move and carry charge

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

in ionic bonding do the atoms transfer or share electrons

A

transfer

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

in covalent bonding to the atoms transfer or share electrons

A

share

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

what happens when non metals bond together

A

they share pairs of electrons to make covalent bonds

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

what are some examples of simple molecular strcutures

A

ammonia
methane
oxygen
chlorine

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

what type of structure do substances containing covalent bonds usually have

A

simple molecular strcutures

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

what are the forces of attractions like in the atoms within molecules with strong covalent bonds

A

weak forces of attraction

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

what is needed to melt or boil a simple molecular compound

A

low melting and pointing points becuase there are feeble intermolecular forces

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

what are most simple molecular substances liek a room temperature

A

liquid or gas

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

do simple molecular compounds conduct electricity

A

no because they do not have an overall electric charge because are no free electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

what type of atoms do covalent bonds form between

A

non-metallic

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

what are the atoms in polymers joined by

A

strong covalent bonds

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

what are polymers

A

they are long chains of small repeating units linked together

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

when drawing a polymer what do you draw

A

you draw the smallest repeating section called the repeating unit

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
what are most polymers like a room temperature
soilds because they have stronger inter molecular forces
26
what are the intermolecular forces like in between polymer molecules
the forces are larger than in between simple covalent molecules so more energy is needed to break them
27
what is the bonding like in giant covalent structures
all the atoms are bonded together by strong covalent bonds
28
what is the melting and boiling points like of giant covalent structures
they have high melting and boiling points because lots of energy is needed to break the bonds between atoms
29
do giant covalent structures conduct electricity
no because they dont contain charged particles
30
what are examples of giant covalent strcutures
dimond graphite silicon dioxide
31
how many covalent bonds does each carbon atom form in diamonds
4
32
what are the atoms arranged in in diamond and graphite
a regular repeating lattice
33
what element is diamond and graphite made from
carbon
34
Do giant covalent structures have high or low melting points?
high as the atoms are all held together by strong covalent bonds which require a large amount of energy to break.
35
what is the properties of diamond
hard very high melting point - strong covalent bonds doesn't conduct electricity - no free elctrons
36
why is diamond very hard
because each carbon atom in it each form 4 covalent bonds
37
how many covalent bonds does each carbon atom form in graphite
3
38
what is the shape of graphite
sheets of carbon atoms arranged in hexagons
39
are there covalent bonds between the layers of graphite
no so there only held together weakly
40
why si graphite a good lubricating material
there arent any covalent bonds between the layers of graphite to their only held together weakly. this means that they are free to move over each other which makes graphite slippery and soft - ideal lubricant
41
what is the melting point of graphite like
high - the covalent bonds in the layers need loads of energy to break
42
how many outer electrons does carbon have
4
43
why does graphite conduct electricity
only three out of 4 of its outer electrons are used for bonds so each carbon atom have one electron that is delocalised and can move. so it conducts electricity
44
what is graphene
one layer of graphite a sheet of carbon atoms joined in hexagons
45
how thick is graphene and what does this make it
it is one atom thick which makes it a two dimensional substance
46
is graphene strong or weak and why
strong because of teh network of covalent bonds but it si also weak because it is just one atom thick
47
what is a good use of graphene
can be added to composite materials to make it stronger without adding much weight
48
can graphene conduct electricity
yes because it is like graphite and contains delocalised electrons
49
what is a allotrope
different forms of the same element in the same physical state
50
what shapes are fullerenes
spheres and tubes
51
what are fullerenes
molecules of carbon shaped like spheres or tubes their Mainly atoms made up of hexagons
52
what was the first fullerene to be discovered
buck minster fullerene
53
what is the molecule formula of buckminsterfullerene
C60
54
what shape s buckministerfullerne
a hollow sphere
55
what are uses of fullerenes
lubricants deliver drugs industrial catalyst
56
why are fullerenes useful for delivering drugs
they can cage other molecules the fullerene structure forms around another atom or molecule trappng it inside
57
why are fullerenes useful for being industrial
they have a huge surface area - individual catalysts could be attached to the fullerene
58
what are nanotubes
tiny carbon cylinders
59
what can form nanotubes
fullerenes
60
what are the properties of nanotubes
the ratio between the length and the diameter of the nanotube is very high they can conduct thermal and electrical energy tensile strength - dont break when stretched
61
what can nanotubes be used for and why
electronics - delocaised electron tennis rackets - they can strengthen materials without adding much weightn
62
what kind of structure do metals consist of
giant structures
63
what does ionic bonding happen between
metals and non metals
64
what does covalent bonding happen betwee
two non-metals
65
what does metallic bonding happen between
metal elements where outer electrons are delocalised
66
what happens in metallic bonding
each metal becomes a ion with a positive charge because it shares its electrons with all the other atoms in the metal. because of this the electrons are then delocalised. - the strong electrostatic attraction between positive ions and negative electrons. - those forces hold everything together
67
why are most metals solid at room temperature
the electrostatic forces between metal atoms and the sea of delocalised electrons are very string so lots of energy is needed to be broken - high melting and boiling points
68
why are metals good conductors of heat
the delocalised electrons carry electrical charge and thermal energy through the whole structure
69
why are most metals malleable
the layers in a metal can slide over each other
70
why might pure metals not be suitable for certain jobs
they can be too soft when their pure
71
what are alloys
a mixture 2 or more different elements - 2 or more metals - a metal and another element
72
why do you use different sized atoms when making alloys
the different sized atoms mixed with the pure metal atoms disrupts the regular structure and the layers can no longer slide over each other which makes the alloy stronger
73
what are the three states of matter
solid liquid gas
74
at a certain temperature what does something depend on for which state it is at
how strong the forces of attraction is between particles of the material
75
in states of matter what do the strength of forces between particles depend on
temperature pressure material
76
what are particles like in soilds
strong forces of attraction which holds them close together in fixed positions to form a regular lattice arrangement - particles dont move - keep definate shape and volume - vibrate in positions - more heat = more vibrations
77
why do soilds expand slightly when their heated
the particles vibrate in their positions and the hotter a solid becomes the more they vibrate
78
what are particles like in liquids
- weak forces of attraction between particles - free to move past eachother but tend to stay close together - they have a definite volume but not a definite shape - particles are constantley moving with random motion
79
what happens to the particles when liquids are heated
they move faster which results in liquid expanding slightly
80
what are the particles like in gases
- forces of attraction are very weak - free to move and are far apart -they dont have a definite shape or volume - they move constantly with random motion
81
what direction do particles move in gases
in straight lines
82
what is the process of solid to liquid
melting - soild heated particles gain more energy - particles vibrate more which weakens forces that hold soild toghter - at melting point particles have enough energy to break free from position - soild turn to liquid
83
what is the process of liquid to gas
boiling - liquid heated and particles gain energy - energy makes particles move faster which weakens the bomds holding liquid togetther - at boiling point particles have enough energy to break the bonds holding liquid together
84
what is the process of gas to liquid
condensation - gas cools + particles dont have enough energy to overcome forces of attraction - bonds form between particles - at boiling point many bonds have formed - gas becomes liquid
85
what is the process of liquid to soild
freezing - liquid cools and particles have less energy so move around less - not enough energy to over come attraction so more bonds form - at melting point many bonds have formed that their held in place - liquid become soild
86
what does aqueous mean
dissolved in water
87
what is the state symbol for liquid
l
88
what is teh state symbol for gas
g
89
what is the state symbol for soild
s
90
what is the state symbol for aqueous
aq
91
when h20 changes state from water to steam do the covalent bonds break
no the weak intermoleuclar forces break not the bonds
92
why does diamond have a high melting point
it has strong covalent bonds where each carbon atom has 4 bonds so to melt it you need to overcome these strong covalent bonds, which requires a high amount of energy
93
what are the conditions for sodium chloride to conduct electricty
dissolve it in water so the ions are free to move

chemistry (5 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2025 Bold Learning Solutions. Terms and Conditions