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chemistry > ionic/covalent/metallic/ + Electrolysis P1 > Flashcards

ionic/covalent/metallic/ + Electrolysis P1 Flashcards

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1
Q

why arw group 3, group 4 and group 5 not usually ions

A

Because they would have to gain 5,4 or 3 electrons which would require a lot of energy

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2
Q

how is an ion formed

A

by loss or gain of electrons

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3
Q

When an atom becomes an ion what do you add to the end of the word

A

IDE

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4
Q

Why are metals positively charged(talk about prot aswell)

A

Because they lose electrons. So have more protons than electrons

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5
Q

What is an ionic bond

A

An electrostatic attraction between positive and negative ions

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6
Q

Explain how ionic bonding takes places

A

Electrons from the metal are transferred to the outer shell of the non metal,
because of strong electrostatic forces of attraction
between the oppositely charged ions.
both have a full outer shell

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7
Q

Are ionic compounds neutral or not?

A

Ionic compounds are neutral

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8
Q

Which groups have noble gas configuration [2,8] [2,8,8]

A

1,2,6,7

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9
Q

What does isoelectronic mean

A

Has the same number of electrons o same electronic configuration

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10
Q

What is an empirical formula

A

Simplest whole number ratio of atoms

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11
Q

What is a lattice

A

A regular arrangement of particles

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12
Q

What kind of lattice do ionic compounds have

A

giant ionic lattice

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13
Q

why does a magnesium oxide (Mg2+, O2-) have greater forces of attraction than Sodium Chloride (Na-, CL-)

A

Because ions in magnesium oxide are attracting 2+ and 2-, making thr electrostatic attractions stronger than (1+,1-)

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14
Q

Explain the arrangement of ions in an ionic lattice

A

Ions are arranged in a regular, repeating lattice

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15
Q

Why do ionic compounds have high melting and boiling points

A

-they have strong electrostatic forces of attraction between the oppositely charged ions so a lot of energy is required to break these forces.

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16
Q

In which way do forces of electrostatic attraction act in an ionic lattice?

A

Strong forces of electrostatic attraction act in all directions

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17
Q

Why do ionic compounds tend to be crystalline

A

Due to the regular arrangement of ions in the lattice

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18
Q

Why does magnesium oxide appear as a white powder

A

Because the crystals are too small to be seen with the naked eye

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19
Q

Why are ionic lattices brittle

A

Because any small distortion can cause ions of the same charge to become alongside each other.Like charges repels the crystal splits itself apart

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20
Q

What substance are ionic compounds soluble in

A

Soluble in water

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21
Q

what substances are ionic compounds insoluble in, (give 2 examples)

A

Organic solvents
Such as ethanol
Or HYDROCARBONS such as HEXANE in PETROL

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22
Q

Why do ionic substances not conduct electricity when solid

A

Because the IONS are in fixed positions
in the giant ionic lattice
And are not free to move around

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23
Q

Why do ionic substances conduct electricty once molten

A

Because the ions are no longer in fixed positions and are free to move around

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24
Q

What two things can you do to an ionic compound to make it conduct electricity

A

Make it molten (melted)
Make it an aqueous solution (dissolved in water)

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25
Q

What can ionic compounds contain which is an exception to them always consisting of a metal

A

Ammonium ions

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26
Q

What is an ion

A

An atom or group of atoms that carries a charge

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27
Q

What is ionic bonding

A

When there are electrons forces of attraction between positively charge and negatively charged ions
holding them together

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28
Q

draw a dot an cross diagram of lithium oxide

A

(Answer should have two lithium atoms on either side of an oxygen atom)

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29
Q

Draw dot and cross diagram of Calcium Bromide

A

(Two atoms of bromide on either side of an atom of calcium)
(Each Bromide should have 7 of its own electrons + one calcium)
(Calcium should have full outer shell)

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30
Q

Work out the Formula of magnesium sulfate

A

MgSO4

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31
Q

Work out the formula of calcium nitrate

A

Ca(NO3)2

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32
Q

Work out the formula of sodium sulfate

A

Na2SO4

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33
Q

Formula of ammonium Sulfide

A

(NH4)2S

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34
Q

How is a covalent bond formed

A

When two non metal atoms share electrons

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35
Q

What holds covalent bonds together

A

Strong electrostatic forces of attraction between positive nuclei of each atom
and negatively charged shared electrons

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36
Q

After covalent bonding, is a hydrogen molecule the same as a noble gas because it has the same electronic configuration?

A

No, because a hydrogen atom still has the same number of protons in the nuclei

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37
Q

Explain How does an atom become more stable(in terms of bonds and energy)

A

If the atom makes more bonds than more energy is released so it will be much more stable

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38
Q

What does energy release between atoms do to the bond

A

Makes it more stable

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39
Q

Formula for ammonia

A

NH3

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40
Q

Formula for Methane

A

CH4

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41
Q

Formula of ETHANE

A

C2H6

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42
Q

Draw a stick diagram of nitrogen

A

N- - - N
(Triple bond)

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43
Q

Draw a stick diagram for ethene

A

C2H4 so
Two central carbon atoms with two bonds
2 hydrogen atoms surrounded by each carbon with single bonds

44
Q

Formula for ETHENE

A

C2H4
So two central carbon atoms with a double bond
And then two hydrogen atoms surrounding each carbon atom with a single bond

45
Q

Draw a dot and cross diagram for Chloroethene(CH2CHCL)

A

two central carbon atoms
With 2 hydrogen atoms around one carbon
And 1 hydrogen atom and one Cl atom around one carbon

46
Q

What is broken when you boil water

A

Weak intermolecular forces

47
Q

What holds a single water molecule together

A

Strong covalent bonds

48
Q

Why do substances with simple molecular structure have low melting and boiling points?

A

Because there are weak INTERMOLECULAR forces of attraction between the molecules which do not need a lot of energy to break

49
Q

Are covalent bonds strong or weak

A

Strong

50
Q

As you go down the group of halogens, why do you need to supply more energy to break the weak intermolecular forces of attraction?

A

Because the molecular mass increases so the intermolecular forces of attraction between the molecules become stronger

51
Q

Why do covalent molecules not conduct electricity (2)

A

Because the molecules do not have an overall charge,
And because all electrons are held tightly by covalent bonds so can not move around

52
Q

What does a molecule consist of

A

Consists of a fixed number of atoms
joined by covalent bonds

53
Q

Why is diamond not a molecule

A

Because the number of atoms are variable and are not fixed

54
Q

Why does diamond have a high melting point

A

Because of the strong covalent bonds which extend throughout the structure and require a lot of energy to break

55
Q

Give 3 substances that exist with a giant molecular structure

A

Silicon dioxide, diamond, graphite

56
Q

Why does diamond form a tetrahedron

A

Carbon has 4 atoms in its outershell so creates 4 bonds

57
Q

Why does diamond not conduct electricity

A

Each carbon atom is bonded to four other carbon atoms by four strong covalent bonds, leaving no delocalized electrons or no free ions

58
Q

Why does graphite conduct electricty

A

One carbon is joined to three other carbon atoms
so it has one delocalized electron
which is able to move between the layers and conduct a charge

59
Q

Why is graphite soft

A

Because the attractions between the layers are weak
and not much energy is needed to overcome them
And so they are able to Slide Over each other

60
Q

Does graphite have a high or low melting point and explain why

A

High melting and boiling point
because there are strong covalent bonds between the atoms IN EACH SEPEARTE LAYER
which require a lot of energy to break

61
Q

What is an allotrope

A

Different forms of the same element

62
Q

Describe the structure of c60 fullerene

A

Simple molecular structure
So consists of molecules with weak intermolecular forces of attraction between them
Where each molecule consists of 60 carbon atoms

63
Q

What kind of melting point does fullerene have and why

A

Low melting and boiling point because of simple molecular structure
So weak intermolecular forces of attraction between the molecules

64
Q

Name three allotropes of carbon

A

Diamond, graphite and fullerene

65
Q

How many bonds does C60 fullerene create

A

3

66
Q

Why can C60 fullerene not conduct electricity even though it only has three bonds

A

Because the fourth electron in one atom can only move around one molecule and is not able to jump to other molecules

67
Q

How is a metallic bond formed(4)

A

When metals atoms bond, their outer electrons become detached
Causing a sea of electrons
The atoms become positively charged ions
And it is the electrostatic forces of attraction between the positively charged ions and the electrons that keep the metallic bond

68
Q

Why do metals conduct electricity (in terms of metallic bonding)

A

Because they have delocalized ELECTRONS which are free to move

69
Q

What is metallic bonding

A

It is the electrostatic forces of attraction between each positive ion and the sea of delocalized electrons

70
Q

What type of structure do metals have

A

Giant structure

71
Q

Why are metals malleable

A

Because the layers of positive ions are able to slide over each other

72
Q

What two substances are exceptions of electrolysis of covalent compounds

A

Ammonia solution and hydrogen chloride(because hydrogen chloride gas dissolves in water to form hydrochloric acid

73
Q

Why can covalent compounds not be used in electrolysis

A

Because their electrons are tightly packed and are not able to move
and because their molecules do not have an overall charge

74
Q

What is the positive electrode called

A

Anode

75
Q

What is the name of a positive ion

A

Cation

76
Q

What is the name of a negative ion

A

Anion

77
Q

What is the name of the negative electrode

A

Cathode

78
Q

What is electrolysis

A

A chemical change caused by passing an electric current through a compound which is either molten or in solution

79
Q

What are the electrodes usually made of and why

A

Carbon
because it conducts electricity well
and is also inert

80
Q

if a solution is insoluble, will you melt it or dissolve it in water for electrolysis

A

Melt it

81
Q

What is another substance used before aluminum oxide can be an electrolyte and what does it do

A

Mix it with molten cryolite to lower melting point of aluminum

82
Q

What are three examples of electrolyte

A

Molten salts
Aqueous solutions of ionic compounds
Molten metals

83
Q

If you electrolyse a molten ionic compound, which substance will form at the cathode and why

A

The metal because it has a positive charge

84
Q

What state must an ionic compound be in if it is to be used as an electrolyte

A

Must be molten or dissolved

85
Q

When labeling an electrolysis diagram, what 4 things should you include

A

-DC power supply
-inert anode(positive electrode)
-inert cathode (negative electrode)
-electrolyte

86
Q

Write the half equation for copper sulfate at the cathode

A

Cu(2+) + 2e—— Cu

87
Q

If you are observing hydroxide being formed in electrolysis, what will you observe

A

Bubbling around the electrode

88
Q

If you are observing chlorine being formed at the electrode, what will you observe?

A

Green/yellowish bubbling

89
Q

How is carbon dioxide formed as a waste gas in electrolysis of molten aluminum oxide

A

When oxide goes to the anode, oxygen gas is formed
Because it reacts with the carbon electrode to form carbon dioxide

90
Q

2 properties of aluminum that make it suitable for food and drink

A

Malleable
Low density

91
Q

During electrolysis of aluminum oxide, apart from oxygen, what else is formed at the anode and why

A

Carbon dioxide
Because the oxygen reacts with the carbon of the electrode

92
Q

Write the ionic hard equation of the equation at the anode of aluminum oxide

A

2O2+ —-) O2 + 4e

(Oxygen is being oxidized
And because it is a diatonic molecule the number of electrons needs to be doubled)

(So would start as O2- —-) O2 + e-

Then you would need to balance the oxygen on left and on right so would become 2O2—-) O2 + e-

And then would need to balance the charges so 2O2- —-) O2 + 4e-

93
Q

During electrolysis of aluminum oxide, why must the anode be constantly replaced

A

Because the anode is being oxidized
As the carbon form the anode reacts with the oxygen to form carbon dioxide

94
Q

Suggest why the melting point of silicon dioxide is higher than the melting point of sodium chloride

A

Because the covalent bonding in silicon dioxide is higher than the ionic bonding of sodium chloride

95
Q

Can diamond conduct electricity when molten

A

No

96
Q

Describe the structure and bonding in the group three metal indium

A

Has a metallic lattice structure
Held together by strong electrostatic forces of attraction
Between the positively charged ions
And delocalized electrons

97
Q

Why would you have H+ and OH- ions in an aqeous solution

A

Because water in solutions splits up into its ions

98
Q

Describe the structure of an ionic substance, and then the structure of a giant covalent substance

A

Ionic:
-arranged in a giant ionic lattice
-ions are tightly packed and regularly arranged
-repeating pattern of positive and negative ions

Giant covalent:
-arranged in giant lattice structure
-where the number of atoms is variable
-repeats in 3 dimensions

99
Q

Why is diamond hard

A

Because of the rigid tetrahedral structure

100
Q

Which of the allotropes of carbon can conduct electricity, and which can’t,

A

graphite is the only one that can
Fullerene and diamond cant

101
Q

Describe the structure of metallic substances

A

Giant metallic attic structure
So ions are in variable amounts
And held together between positively charged ions and delocalized electrons

102
Q

Give the names of two compounds that can be split up using the molten way of electrolysis

A

Aluminum oxide
Lead bromide

103
Q

During the electrolysis of aluminum oxide, state what deposits at the bottom

A

Molten aluminum

104
Q

In the electrolysis of lead bromide, state two observations made and explain what they are

A

Grey solid deposits at the bottom which is lead
Bubbling at the anode because bromide gas formed

105
Q

Why do you need rules to determine what forms at what electrode, when talking about aqeous solutions

A

Because water in soltuion splits up into its ions
Therefore you have four different ions to choose from

106
Q

If using an aqueous solution in electrolysis, and turns out that hydroxide ions will be discharged at the anode, what are the two products formed
And state the equation

A

Oxygen and water
4OH- ——-) 2H2O + O2 + 4e-

chemistry (18 decks)

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