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Chemistry GCSE > Topic 2 - Structure and Bonding > Flashcards

Topic 2 - Structure and Bonding Flashcards

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1
Q

bonds

A

forces of attraction that can hold atoms together

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2
Q

when are atoms more stable

A

when they have a full outer shell

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3
Q

how do you make atoms more stable

A

by transferring electrons between atoms forming charged particles called ions

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4
Q

ion

A

an atom or group of atoms that carries a positive or negative electric charge as a result of having lost or gained one or more electrons

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5
Q

cation

A

when the atom looses an electron and forms a positive ion

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6
Q

anion

A

when an atom gains electrons and forms negative ions

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7
Q

ionic bond

A

formed from the electrostatic attraction between oppositely charged ions in a chemical compound

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8
Q

if an atom (e.g. Mg) looses 2 electrons, how do you write the atom symbol

A

Mg2+ because you lost electrons so the atom turns positive

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9
Q

how are ionic compounds formed

A

from the loss and gain of electrons

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10
Q

how are ionic compounds held together

A

by the strong electrostatic forces of attraction between oppositely charged ions

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11
Q

lattice structure

A

a regular repeating arrangement of ions

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12
Q

when solid what does ionic compounds form

A

crystals

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13
Q

how do you work out an ionic formulae

A

use the cross over method

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14
Q

sodium sulphate contains Na+and S2-, what’s the ionic formulae

A

Na+ S2-
✖️
Na2- S+
= Na2S

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15
Q

polyatomic ion

A

set of two or more atoms ((e.g. (SO4)2-)

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16
Q

how do you know the ion is polyatomic and contains oxygen

A

ion name ends in ‘-ate’ or ‘-ite’

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17
Q

at what state can ionic compounds conduct electricity

A

once melted or dissolved in water

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18
Q

what two things have to happen for a substance to conduct electricity

A
  • must be charged particles
  • these particles must be free to move
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19
Q

name the process to create an ionic bond

A

the ions loose or gain and electron to each other and produce oppositely charged ions; these ions are then attracted to each other by electrostatic forces forming an ionic bond (this whole thing is an ionic compound)

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20
Q

in an electric current, which way do the anions move

A

to the anode (positive electrode)

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21
Q

in an electric current, which way do the cations move

A

to the cathode (the negative electrode)

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22
Q

how do you show the number of each element bonded together in a simple molecule

A

using a molecular formula

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23
Q

where are convolent bonds found

A

between two non-metals

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24
Q

how are convent bonds formed

A

two atoms share an electron to create a full outer shell - this makes the atom more stable

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25
Q

how can we show a covalent bond

A

using dot and cross diagram

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26
Q

what’s a double covalent bond

A

where atoms share two pair of electrons to fill their outer shells

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27
Q

in a molecule what is the bond between the positive nuclei and the negative electrons

A

electrostatic forces of attraction

28
Q

molecule

A

two or more atoms connected by COVALENT bonds

29
Q

in group 1, what’s the charge of the elements

A

+1

30
Q

in group 2, what’s the charge of the elements

A

+2

31
Q

in group 3, what’s the charge of the elements

A

+3

32
Q

in group 5, what’s the charge of the elements

A

-3

33
Q

in group 6, what’s the charge of the elements

A

-2

34
Q

in group 7, what’s the charge of the elements

A

-1

35
Q

in group 8/0, what’s the charge of the elements

A

0

36
Q

what are the WEAK forces of attraction between molecules

A

intermolecular forces

37
Q

monomers and what can it form

A

small simple molecules that can be joined in a chain to form a polymer

38
Q

properties of simple covalent molecules

A

low boiling and melting points due to weak intermolecular forces

39
Q

allotrope

A

different form of the same element

40
Q

what are the different allotropes of carbon

A
  • diamond
  • graphite
  • graphene
  • fullerene (C60)
41
Q

how is a fullerene (C60) structured and its properties

A
  • each carbon atom is covalently bonded to 3 other carbon atoms
  • spherical shape
  • low melting point due to weak intermolecular forces
  • soft and slippery
42
Q

how is graphene structured and its properties

A
  • it’s a sheet of carbon atoms (one atom thick) with 3 covalent bonds between each atom which forms a hexagon - you can roll this up to form a tube
  • good electrical conductors as it allows free electrons to move across its surface
43
Q

giant covalent molecular structures

A

huge three dimensional networks of carbon atoms linked together by covalent bonds

44
Q

giant covalent molecular structure examples and properties (of carbon)

A
  • diamond and graphite
  • high melting points because of the many strong covalent bonds that need to be broken to melt the solids
  • very strong
45
Q

how many covalent bonds are there for each carbon atom in graphite

A

3

46
Q

how many covalent bonds are there for each carbon atom in diamond

A

4

47
Q

graphite structure

A

layered structure (sheets of graphene that are held together by strong covalent bonds) that are held together on top of one another by weak forces or attraction meaning they’re able to slide over each other - making graphite soft

48
Q

why can graphite carry an electrical current

A
  • because it only has 3 bonds for each carbon atoms meaning there is one electron that is not being used in covalent bonding
  • this one electron is called a delocalised electron (free to move around)
  • this means it’s free to move and carry a current
49
Q

diamond structure and properties

A
  • network of carbon atoms in a tetrahedral arrangement, joined by strong covalent bonds
  • very hard
50
Q

why can metals conduct electricity

A
  • because metal’s outer shell electrons are lost from each atom and become free to move randomly throughout the metal
  • when voltages applied between two points on a piece of metal these delocalised electrons will flow towards the positive side which transfers energy and forms an electrical current
51
Q

metallic bonding

A

electrostatic attraction between the positive metal ions and the negative delocalised electrons

52
Q

why do metals have high melting and boiling points

A

because the metallic bonding is so strong it needs a lot of energy to break these bonds

53
Q

why are metals malleable (they can be hammered or rolled into shape without shattering)

A

because when you hit the metal the layers of ions slide over each other and the ‘sea’ of electrons hold the ions together that’s why it changes shape instead of breaking

54
Q

how do you know when the metal can conduct more or less electricity

A

because of the charge of the metal (e.g. +1 or +2)
- this +1 means it contributes 1 delocalised electron and +2 means it contributes 2 delocalised electrons
- the element that contributes more electrons conducts more electricity

55
Q

what are the negatives for showing covalent bonds in a dot and cross diagram

A

positives:
- show how electrons shared in covalent bonds
negatives:
- do not show the structure formed
- they suggest that the electrons in different atoms are different when they are actually the same

56
Q

what are the positives and negatives for showing covalent bonds in a 3D ball and stick model

A

positives:
- shows which atoms are joined together
- shows the shape of the structure
negatives:

57
Q

what is released when bonds form

A

energy

58
Q

when do non-metal make endings change to -ide

A

when they form negative ions

59
Q

What does it mean if an ion ends in -ate or -ite?

A

It contains oxygen as well as another element

60
Q

what enables ionic compounds to conduct electricity

A

charged ions that are free to move (NOT ELECTRONS)

61
Q

what state does the iconic compounds have to be in to conduct electricity

A
  • molten or dissolved in water (in aqueous solution)
62
Q

What substances contain covalent bonds

A

Molecular

63
Q

what is an electric current?

A

Flow of charged particles

64
Q

how does the electrical conductivity increase?

A

When the number of delocalised electrons increase

65
Q

What are the 4 different types of bonding

A
  • ionic
  • simple molecular (covalent)
  • giant covalent
  • metallic

Chemistry GCSE (8 decks)

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