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Chemistry > Bonding, Structure and Properties of matter > Flashcards

Bonding, Structure and Properties of matter Flashcards

1
Q

what is ionic bonding

A

electrostatic attraction between oppositely charged ions

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2
Q

what happens to electrons in ionic bonding

A

electrons are given away and gained

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3
Q

explain why an ionic compound is solid at room temperature

A

high melting points

giant lattice structure

strong electrostatic attraction between oppositely charged ions

a lot of energy is needed to overcome this

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4
Q

where do ionic compounds conduct electricity

A

water or molton

ions are now free

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5
Q

what is covalent bonding

A

formed between two or more non metals, electrons are shared, neutral particles are formed called molecules

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6
Q

what are formed in ionic bonding

A

positive and negative ions

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7
Q

what is metallic bonding

A

electrostatic attraction between metal ions and delocalised electrons

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8
Q

what are alloys

A

mixture of metals with other elements

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9
Q

what is wrong with a 3D ball and stick diagram

A

it shows the actual bond of the molecule

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10
Q

what is wrong with a 2D ball and stick diagram

A

shows which atom is bonded, it shows a 90 degree angle when it is 109 degrees

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11
Q

what is wrong with a dot and cross diagram

A

shows different electrons in different forms when they all look the same

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12
Q

what is wrong with a displayed formula diagram

A

the electrons are in a fixed position when they actually move

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13
Q

why do metals have high melting points

A

giant lattice structure

strong electrostatic attraction between metal ions and delocalised electrons

requires a lot of energy to overcome this

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14
Q

what is a giant lattice

A

structure - ions are packed together in an ordered, regular structure

positive and negative ions

strong electrostatic forces between oppositely charged ions

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15
Q

describe the structure of graphite

A

giant structure of carbon atoms and hexagonal layered structure

each atom is attached to 3 more carbon atoms by strong covalent bonds

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16
Q

why does diamond have a high melting point

A

Giant structure of strong covalent bonds which require a lot of energy to break

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17
Q

why is diamond used in cutting drills

A

it is strong and hard

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18
Q

why is diamond hard

A

it has a giant structure of strong covalent bonds which require a lot of energy to break

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19
Q

how many more carbon atoms are attached to a carbon molecule

A

4

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20
Q

why does diamond not conduct electricity

A

all the outer shell electrons in carbon are fixed in bonding no free electrons to carry the charge

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21
Q

is carbon a metal

A

no carbon is a non metal

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22
Q

what bond is used when carbon atoms bond to make diamond

A

covalent bond

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23
Q

what arrangement of carbon atoms do diamond have

A

tetrahedral

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24
Q

why do covalent compounds have low boiling points

A

because they have simple and small structures

weak intermolecular molecules that need little energy to overcome

25
why do covalent compounds not conduct electricity
they have no delocalised electrons to carry the charge
26
what is a metal crystal
grain/s
27
what is covering iron with a protective layer of zinc
galvernising
28
why does graphite have a high melting point
it has a giant structure of strong covalent bonds which require a lot of energy to break
29
why is graphite used in pencil
because it is soft and slippery
30
why is graphite soft
layered structure, that are attracted to each other by weak forces which do not require a lot of energy to overcome this
31
why does graphite conduct electricity
because 1 electron from each carbon atom becomes delocalised. these electrons are free to move throughout the structure to carry the charge
32
explain why diamond doesn't conduct electricity but graphite does
in diamond all the outer shell electrons of carbon are fixed in bonding so no free electrons to carry the charge in graphite each carbon is bonded to 3 atoms so there is 1 free delocalised electron
33
explain why diamond and graphite have high melting points
giant covalent structure strong covalent bonds requires a lot energy to break
34
what are intermolecular forces
in between molecules
35
describe Ionic Bonding
formed between metal and non metal if formed between metal electrons are given away and positive ions are formed. if formed between non metals electrons are gained and negative ions are formed
36
describe covalent bonding
formed between two or more non metals electrons are shared neutral particles are formed these are called molecules
37
describe metallic bonding
metal atoms lose outer shell electrons to form delocalised electrons amongst different sized atoms but they cannot slide over each other making it harder
38
explain how the charge ion relates to its group number
for example 8 ions is group 0 group 1 means the elements have 1 ion
39
how do the ions produced by elements in some groups have the electronic structure of a noble gas.
a noble gas also known as group 0 has a full outer shell (8 ions).
40
using the examples chlorine and sodium answer describe what is happening in this reaction
chlorine loses one electron sodium gains one electron both atoms achieve a full outer shell
41
describe the properties of ionic compounds and explain why their structure effects these.
very high melting and boiling points because the strong electrostatic forces need lots of heat energy to break cannot conduct electricity when solid because the ions can not move and carry the charge however can when melted or dissolved in water because the ions can now move and carry the charge
42
what does aqueous mean
dissolved in water
43
how does the structure of small molecules affect their properties
small molecules has strong electrostatic forces therefore need lots of heat energy to break them. therefore high melting and boiling points
44
Explain how the structure of polymers affects their properties
polymers have very long carbon molecules, they too are held together by strong electrostatic forces they have bigger intermolecular forces than smaller molecules this means that polymers have higher melting and boiling points than any other organic molecule
45
Explain how the structure of giant covalent structures affects their properties
substances with giant covalent structures are solid at room temperature. they also have very high melting and boiling points
46
Explain how the structure of metals and alloys affects their properties, including explaining why they are good conductors
they are electrical conductors because their delocalised electrons carry the charge through the metal.
47
Explain why alloys are harder than pure metals in terms of the layers of atoms
alloys contain different sizes of atoms. these different sizes the regular arrangements of atoms this makes it more difficult for the layers to slide over each other
48
the disadvantages of nanoparticles
can be absorbed by the body and enter the body no one knows the potential long term effects of this
49
what is the mass number
protons and neutrons
50
what is the atomic number
protons and electrons
51
how to work out neutrons
mass number - protons = neutrons
52
why do simple molecules no conduct electricity
they are not charged no free electrons or ions
53
why do metals conduct electricity
because they have delocalised electrons that carry the charge and thermal energy through the whole structure
54
why does sodium chloride have a high boiling and melting point
giant lattice structure of na+ and cl- ions a lot of energy needed to overcome this
55
why would molton sodium chloride conduct electricty
because the ions are now free | they can carry the charge
56
why has diamond got a higher boiling and melting point than sodium chloride
stronger attractive forces between atoms each carbon atom is bonded to 4 other carbon atoms by covalent bond
57
explain a covalent bond using chlorine as an example
non metal atoms each chlorine atoms needs one electron to get a full outer shell they share electrons covalent bond is formed
58
explain a ionic bond using sodium chloride as an example
metal and non metal atoms sodium loses one electron to chlorine to get a full outer shell Na+ and Cl- ions are formed

Chemistry (7 decks)

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