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Chemistry > Bonding, Structure And The Properties Of Matter > Flashcards

Bonding, Structure And The Properties Of Matter Flashcards

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1
Q

What is ionic bonding

A
  • When a metal reacts with a non metal
  • the outer electrons are transferred from a metal atom to the non metal atom
  • ionic bonding produces ions which have the electronic structure of a noble gas
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2
Q

What happens to groups during ionic bonding

A
  • group 1 metals lose 1 electron forming a 1+ ion
  • group 2 metals lose 2 electrons forming a 2+ ion
  • group 6 non metals gain 2 electrons forming a 2- ion
  • group 7 non metals gain 1 electron forming a 1- ion
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3
Q

Describe what is happening in the reaction when

Na* + CI*** —> [ Na]+ + [CI**]-

A
  • sodium loses one electron to become a positively charged ion
  • chlorine gains this electron to form a negatively charged ion
  • opposite charges attract and a strong ionic bond is formed
  • both atoms achieve a full outer-energy level
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4
Q

What do you do in dot and cross diagrams

A

Only show the outer levels (only electrons are showed)

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5
Q

What is involved in covalent bonding

A

Only the outer energy levels

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6
Q

What is covalent bonding

A
  • Takes place between non metal elements

- a covalent bond is a shared pair of electrons

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7
Q

How does a stick diagram look like for H2O

A

O
/ \
H H

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8
Q

What is a double covalent bond

A

Two shared pairs of electrons (a single covalent bond would be one shared pair of electrons)

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9
Q

What does a double covalent bond stick diagram look like

A

O = O (two lines)

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10
Q

What do non metals and metals do when they react together

A

Form a giant ionic lattice which have strong electrostatic forces (3 dimensional)

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11
Q

What does metallic bonding consist of

A

Positive ions and delocalised electrons

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12
Q

What are examples of giant covalent structures

A
  • diamond
  • graphite
  • graphene
  • silicon dioxide
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13
Q

What is an ionic bond

A

A strong electrostatic attraction between positive and negative ions

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14
Q

What happens in metallic bonding

A

Metals lose electrons to form positive ions and delocalised electrons

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15
Q

What is a metallic bond

A

A strong electrostatic attraction between positive metal ions and negative delocalised electrons

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16
Q

What are the electrons in a metal

A

Delocalised

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17
Q

Why do metals have high melting and boiling points

A
  • because a great deal of energy is required to break the strong metallic bonds
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18
Q

Why are metals good conductors (of heat and electricity)

A

Because the delocalised electrons can move

19
Q

Why can metal conduct heat

A

The moving electrons carry thermal energy

20
Q

Why can metals be bent and shaped

A

The layers of atoms are able to slide over each other

21
Q

What is an alloy

A

A mixture of metals

22
Q

Why are alloys harder than pure metals

A

The different sizes of atoms distort the layers making it more difficult for them to Slide Over each other

23
Q

What are electrostatic forces

A

Strong forces of attraction between ions

24
Q

Properties of ionic compounds

A
  • very high melting and boiling points as the strong electrostatic forces require a great deal of heat energy to break
  • cannot conduct electricity when solid because the ions can’t move (they are locked in place by strong electrostatic forces of attraction)
25
Q

Why can ionic compounds conduct electricity when they are melted or dissolved in water

A

The IONS can now move and carry the charge (not the electrons)

26
Q

Features of a solid

A
  • extremely hard to compress (particles are packed together in a regular pattern)
  • they have a fixed shape and cannot flow from place to place (the particles can vibrate but can’t move from place to place)
27
Q

Features of a liquid

A
  • extremely hard to compress (the particles are close together)
  • unlike solids, liquids take the shape of their container and flow from place to place (particles in a liquid can move)
28
Q

Features of a gas

A
  • extremely easy to compress (particles are widely spread)

- they spread out and fill the space of their container (the particles move quickly and randomly)

29
Q

the stronger the forces of attraction between the particles…

A

The more energy needed to break them and the higher the melting point

30
Q

Why does something have a low melting point

A

The forces of attraction between the particles are relatively weak, making them fairly easy to break

31
Q

Limitations of the simple particle model of solids liquids and gases

A
  • the simple particle model assumes that all particles are solid spheres (particles have different shapes and are not solid)
  • it is assumed that there are no forces between the particles (forces between particles have a major impact on the melting and boiling point of a substance)
32
Q

What state is aqueous

A

Dissolved in water (aq)

33
Q

What do ionic compounds form

A

-Giant structures where every positive ion is surrounded by a negative ion (giant ionic lattice)

34
Q

What do giant ionic lattices have

A
  • Strong forces of attraction between the positive and negative ions (electrostatic forces)
  • Electrostatic forces are called ionic bonds
35
Q

What are the properties of small molecules (covalent)

A
  • they have low melting and boiling points
  • they are usually gases or liquids at room temperature
  • they do not conduct electricity AS the molecules don’t have an overall electric charge
36
Q

Why do small molecules have low melting and boiling points

A
  • because the weak intermolecular forces between the molecules do not require a lot of energy to break
37
Q

What are the atoms in each molecule held by

A

Strong covalent bonds

38
Q

What does increasing the size of the molecule do (small covalent bonds)

A
  • their boiling point increases as the intermolecular forces increase and require more energy to break
39
Q

Key facts about giant covalent molecules

A
  • always solids at room temp as they have millions of strong covalent bonds
  • they always have high melting and boiling points
40
Q

What is diamond formed from

A

Carbon

41
Q

What does each carbon atom form in diamond

A
  • four strong covalent bonds to four other carbon atoms
42
Q

Why does diamond have a high melting and boiling point

A
  • they have a huge number of strong covalent bonds which have to be broken when diamond is melted
  • this requires a great deal of energy
43
Q

Property of diamond

A
  • cannot conduct electricity as there are no free electrons to carry electrical charge
44
Q

Key fact about silicone dioxide

A

- very high melting and boiling point

- a huge number of strong covalent bonds must be broken, this takes a great deal of energy

Chemistry (5 decks)

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