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F321 Chemistry > Ionic and Covalent Bonding > Flashcards

Ionic and Covalent Bonding Flashcards

1
Q

When are ions formed?

A

When electrons are transferred from one atom to another. The simplest ions are single atoms which have either lost or gained 1, 2 or 3 electrons so they’ve got a full outer shell.

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2
Q

What ions do group 1 elements form?

A

1+

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3
Q

What ions do group 2 elements form?

A

2+

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4
Q

What ions do group 6 elements form?

A

2-

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5
Q

What ions do group 7 elements form?

A

1-

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6
Q

What are the compound ions I need to know?

A

Nitrate…NO3-
Carbonate…CO3 2-
Sulfate…SO4 2-
Ammonium…NH4+

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7
Q

What does an electrostatic attraction do?

A

It holds positive and negative ions together- its very strong.
When atoms are held together like this, its called ionic bonding.

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8
Q

What is an ionic bond?

A

An electrostatic attraction between two oppositely charged ions.

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9
Q

What do you get when oppositely charged ions form an ionic bond?

A

An ionic compound.

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10
Q

What are ionic crystals?

A

Giant lattices of ions.

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11
Q

What is a giant lattice?

A

A lattice is just a regular structure. The structure’s called giat because it’s made up of the same basic unit repeated over and over again.

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12
Q

What three physical properties can the structure of ionic compounds determine?

A

Electrical conductivity
Melting and boiling points
Solubility

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13
Q

What features of an ionic compound determines electrical conductivity?

A

Ionic compounds conduct electricity when they’re molten or dissolved- not when they’re solid.
The ions in a liquid are free to move (and they carry charge).
In a solid they’re fixed in position by the strong ionic bonds.

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14
Q

What features of an ionic compound determines melting and boiling points?

A

Ionic compounds have high melting and boiling points.
The giant ionic lattices are held together by strong electrostatic forces.
It takes loads of energy to overcome these forces, so melting and boiling points are very high.

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15
Q

What features of an ionic compound determines solubility?

A

Ionic compounds tend to dissolves in water.
Water molecules are polar- part of the molecule has a small negative charge, and the other bits have small positive charges.
The water molecules pull the ions away from the lattice and cause it to dissolve.

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16
Q

What are the smallest parts of compounds that can take part in chemical reactions?

A

Molecules.

17
Q

How are molecules formed?

A

When two or more atoms bond together.

18
Q

How are molecules held together?

A

By strong covalent bonds.

19
Q

What is a covalent bond?

A

A shared pair of electrons.

20
Q

What happens in dative covalent bonds?

A

One of the atoms provides both of the shared electrons.

21
Q

Why are simple covalent compounds mainly gases?

A

They have strong bonds within molecules by weak forces between the molecules.

22
Q

Explain the behaviour of electrical conductivity in simple covalent compounds.

A

Simple covalent compounds don’t conduct electricity because there are no free ions or electrons to carry the charge.

23
Q

Explain the behaviour of melting and boiling points in simple covalent compounds.

A

Simple covalent compounds have low melting and boiling points because the weak forces between molecules are easily overcome.

24
Q

Explain the behaviour of solubility in simple covalent compounds.

A

Simple covalent compounds dissolve in water depending on how polarised the molecules are.

25
Q

What are the two types of giant covalent carbon structures I need to know about?

A

Graphite and diamond.

26
Q

What are giant covalent structures?

A

Giant covalent structures have a huge network of covalently bonded atoms. Their atoms are arranged into giant lattices, which are strong structures because of the many bonds involved.

27
Q

Why can carbon atoms form a macromolecular/giant covalent structure?

A

They can form four strong, covalent bonds.

28
Q

What is the structure of graphite like?

A

The carbon atoms are arranged in sheets of flat hexagons covalently bonded with three bonds each.
The fourth outer electron of each carbon atom is delocalised.
The sheets of hexagons are bonded together by weak van der Waals forces.

29
Q

Graphites structure means it has certain properties. What are these?

A

The weak bonds between layers-easily broken so sheets can slide over each other- graphite feels slippery.
The delocalised electrons are free to move along the sheets- current can flow.
The layers are quite far apart compared to the length of the covalent bonds- so low density and used to make strong, lightweight sports equipment.
Because of the strong covalent bonds in the hexagon sheets- very high melting point.
Insoluble in any solvent- covalent bonds in sheets are too difficult to break.

30
Q

What is the structure of diamond like?

A

It is made up of carbon atoms.
Each carbon atom is bonded to four other carbon atoms.
The atoms arrange themselves in a tetrahedral shape- its crystal lattice structure.

31
Q

What properties of diamond are because of its strong covalent bonds?

A

Very high melting point.
Extremely hard.
Vibrations travel easily through the stiff lattice- good thermal conductor.
It can’t conduct electricity- all other electrons are held in localised bonds.
Like graphite, won’t dissolve in solvent.

32
Q

What is meant by the term ionic bonding?

A

Positive and negative ions attract one another and bind together forming a new substance, usually a metal and a non-metal through loosing or gaining an electron. The metal looses one or more electrons and the non-metal gains one or more electrons.

33
Q

Why does ammonium chloride conduct electricity when dissolved in water and not when it is solid?

A

In the solid state, it does not have the free ions flowing needed to conduct electricity. The atoms are locked in place.
However in the liquid state, it does have free ions. The free ions allow the conductivity of electricity.

34
Q

True or false, potassium fluoride exists as a molecule? Why?

A

Potassium fluoride exists as a lattice consisting of potassium and fluoride ions.

F321 Chemistry (25 decks)

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