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structure and bonding & organisation part 1 > Bonding - Structure and Bonding > Flashcards

Bonding - Structure and Bonding Flashcards

1
Q

What is ionic bonding?

A

Ionic bonding is the electrostatic force of attraction between a positively charged ion (metal) and a negatively charged ion (non-metal) and they transfer electrons.

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2
Q

What is covalent bonding?

A

When atoms share electrons (non-metal and non-metal)

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3
Q

What is metallic bonding?

A

With 2 positive ions (2 metals) and alloys. The electrostatic attraction between a lattice of positive ions surrounded by a sea of delocalised electrons. The sharing of delocalised electrons results in strong metallic bonding .

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4
Q

Name the properties of ionic compounds

A
  • High melting and boiling points
  • Can’t conduct electricity as a solid - they can when they are a liquid as ions are free to move
  • Solid at room temperature
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5
Q

Why do small covalent have low melting and boiling points (they are usually gases at room temperature)?

A

The intermolecular forces are weak, therefore it requires very little energy

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6
Q

Name 2 properties of small covalent molecules

A
  • They can’t conduct electricity
  • They have low melting and boiling points
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7
Q

Name 2 properties of large covelent molecules

Such as diamond and graphite

A
  • Higher melting and bioling points as they have many bonds
  • Most can’t conduct electricity but some do
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8
Q

Why are covalent bonds strong?

A

Covalent bonds are strong because the shared electrons are attracted to the nucleus of both atoms

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9
Q

Metallic Bonding

What are delocalised electrons?

A

Electrons that are free to move

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10
Q

Why are metals good conductors?

A

They have delocalised electrons which can move, the electrons can move which can carry an electric current/ thermal energy (heat) through the whole structure

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11
Q

Why are metals malleable?

A

Delocalised electrons allow metal atoms to slide past one another without being subjected by strong repulsive forces that could cause materials to shatter.

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12
Q

What are alloys?

A

A mixture of 2 or more different elements (one has to be a metal)

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13
Q

What is an example of an alloy?

A

Steel - it’s mostly iron but 2% of carbon

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14
Q

Name the properties of metals

A
  • Shiny
  • Malleable
  • Ductile
  • High melting/boiling points
  • Conductors of electricity and heat
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15
Q

True or False: Metallic bonds are weaker than ionic and covalent bonds.

A

True

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16
Q

What are cations?

A

Positive ions

17
Q

Describe the structure of metals

A

They have a regular,lattice,compact structure,giant structure,delocalised electrons and have cations

18
Q

What happens when cations slide over each other?

A

A dent is formed

19
Q

Why aren’t ionic substances malleable?

A

The like poles would cause repulsion and therefore make the whole thing shatter.

20
Q

What are anions?

A

Negative ions

21
Q

What are allotropes?

A

Different structural forms of the same elements and can have different physical properties and chemical behaviours.

22
Q

What is an example of an allotrope (carbon)?

A

Graphite, Charcoal and diamond

23
Q

Why do ionic substances have high melting and boiling points?

A

Because they have many bonds and the forces between the bonds are really strong, therefore they require lots of energy to break

24
Q

What group is not involves in ionic bonding?

A

Group 0, Noble Gases

25
Q

What does the mass number (top) mean?

A

Number of protons + number of neutrons (protons and neutrons in the nucleus)

26
Q

What does the atomic number (bottom) mean?

A

Amount of protons or electrons

27
Q

Why do ionic substances have high melting points?

A

Ionic substances have so many bonds and the forces in the bonds are really strong. Therefore, it requires lots of energy to break these bonds.

28
Q

What are ions?

A

Ions are atoms that have gained or lost electrons, therefore they have a charge

29
Q

Why can’t covalent compounds conduct electricity?

A

They don’t have any charged particles to conduct

30
Q

Why are ionic substances a solid at room temperature?

A
  • Electrostatic attraction/ionic bonds are strong
  • The electrostatic attraction comes from all directions between oppositely charged ions
  • Forming a giant lattice
  • Large amount of energy to needed to break the strong bonds
  • Therefore it has a high melting point
31
Q

Why does chlorine, a small covalent molecule, a gas at room temperature?

A
  • The covalent bonds between atoms
  • Forming simple molecules
  • Weak attraction between molecules
  • Therefore, a low boiling point
32
Q

What charge is an ion when it loses an electron?

A

Positive

33
Q

What charge is an ion when it gains an electron?

A

Negative

34
Q

What do metals rely on to keep the metal together?

A

Electrostatic force of attraction

structure and bonding & organisation part 1 (11 decks)

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