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Chemistry > Bonding, Structure and Properties of matter > Flashcards

Bonding, Structure and Properties of matter Flashcards

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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
Q

why do covalent compounds not conduct electricity

A

they have no delocalised electrons to carry the charge

26
Q

what is a metal crystal

A

grain/s

27
Q

what is covering iron with a protective layer of zinc

A

galvernising

28
Q

why does graphite have a high melting point

A

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

29
Q

why is graphite used in pencil

A

because it is soft and slippery

30
Q

why is graphite soft

A

layered structure, that are attracted to each other by weak forces which do not require a lot of energy to overcome this

31
Q

why does graphite conduct electricity

A

because 1 electron from each carbon atom becomes delocalised.

these electrons are free to move throughout the structure to carry the charge

32
Q

explain why diamond doesn’t conduct electricity but graphite does

A

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
Q

explain why diamond and graphite have high melting points

A

giant covalent structure

strong covalent bonds

requires a lot energy to break

34
Q

what are intermolecular forces

A

in between molecules

35
Q

describe Ionic Bonding

A

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
Q

describe covalent bonding

A

formed between two or more non metals

electrons are shared

neutral particles are formed

these are called molecules

37
Q

describe metallic bonding

A

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
Q

explain how the charge ion relates to its group number

A

for example 8 ions is group 0

group 1 means the elements have 1 ion

39
Q

how do the ions produced by elements in some groups have the electronic structure of a noble gas.

A

a noble gas also known as group 0 has a full outer shell (8 ions).

40
Q

using the examples chlorine and sodium answer

describe what is happening in this reaction

A

chlorine loses one electron
sodium gains one electron
both atoms achieve a full outer shell

41
Q

describe the properties of ionic compounds and explain why their structure effects these.

A

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
Q

what does aqueous mean

A

dissolved in water

43
Q

how does the structure of small molecules affect their properties

A

small molecules has strong electrostatic forces therefore need lots of heat energy to break them. therefore high melting and boiling points

44
Q

Explain how the structure of polymers affects their properties

A

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
Q

Explain how the structure of giant covalent structures affects their properties

A

substances with giant covalent structures are solid at room temperature.

they also have very high melting and boiling points

46
Q

Explain how the structure of metals and alloys affects their properties, including explaining why they are good conductors

A

they are electrical conductors because their delocalised electrons carry the charge through the metal.

47
Q

Explain why alloys are harder than pure metals in terms of the layers of atoms

A

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
Q

the disadvantages of nanoparticles

A

can be absorbed by the body and enter the body

no one knows the potential long term effects of this

49
Q

what is the mass number

A

protons and neutrons

50
Q

what is the atomic number

A

protons and electrons

51
Q

how to work out neutrons

A

mass number - protons = neutrons

52
Q

why do simple molecules no conduct electricity

A

they are not charged

no free electrons or ions

53
Q

why do metals conduct electricity

A

because they have delocalised electrons that carry the charge and thermal energy through the whole structure

54
Q

why does sodium chloride have a high boiling and melting point

A

giant lattice structure of na+ and cl- ions

a lot of energy needed to overcome this

55
Q

why would molton sodium chloride conduct electricty

A

because the ions are now free

they can carry the charge

56
Q

why has diamond got a higher boiling and melting point than sodium chloride

A

stronger attractive forces between atoms

each carbon atom is bonded to 4 other carbon atoms

by covalent bond

57
Q

explain a covalent bond using chlorine as an example

A

non metal atoms

each chlorine atoms needs one electron to get a full outer shell

they share electrons

covalent bond is formed

58
Q

explain a ionic bond using sodium chloride as an example

A

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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