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GCSE Chemistry 🧪 > Bonding ⛓️ > Flashcards

Bonding ⛓️ Flashcards

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1
Q

What is an ionic bond?

A

The electrostatic force between a positively charged and negatively charged ion between a metal and a non-metal.

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2
Q

What is an ion?

A

An ion is an atom or group of atoms with a positive or negative charge.

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3
Q

If an ion is positively charged, has it lost of gained electrons?

A

It has lost electrons.

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4
Q

What does it mean if an ionic compound ends in -ide?

A

The compound contains 2 elements.

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5
Q

What does it mean if an ionic compound ends in -ate?

A

The compound contains at least three elements, one of which is oxygen.

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6
Q

Describe the structure of an ionic compound.

A

Lattice structures.
Regular arrangement of ions.
Ions held together by strong electrostatic forces between ions with opposite charges.

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7
Q

What is a covalent bond?

A

The electrostatic force between the nucleus and the nucleus and the bonding pair of electrons between non-metals only.

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8
Q

True or false?
Covalent bonds are weak.

A

FALSE - they are strong

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9
Q

Why do ionic compounds have high melting points?

A

Strong electrostatic attraction between the positive and negative ions requires a lot of energy to overcome.

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10
Q

When do ionic compounds conduct electricity?
Why?

A

When molten or aqueous because the ions are charged and free to move. When sold, the ions are fixed in an ionic lattice so can’t move.

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11
Q

Why do simple molecular compounds have low melting and boiling points?

A

They have weak intermolecular forces which only require a little energy to overcome.

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12
Q

Do simple molecular compounds conduct electricity? Why/why not?

A

No because there are no charged particles.

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13
Q

Do giant covalent structures have a high melting point?

A

Yes because they have lots of strong covalent bonds which enquire a lot of energy to break.

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14
Q

How do metals conduct electricity and heat?

A

The positive ions are fixed in a sea of delocalised electrons. These electrons are free to move and carry charge/energy.

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15
Q

True or false?
Metals are insoluble in water

A

TRUE

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16
Q

Name two giant covalent structures formed from carbon atoms.

A

Graphite
Diamond

17
Q

Describe the structure and properties relating to graphite.

A

Each carbon atom bonded to 3 other carbon atoms.
Lays of hexagonal rings of carbon atoms.
Weak intermolecular forces between layers.
One delocalised electrons per carbon atom.

18
Q

Describe and explain the properties of graphite.

A

Graphite is soft / slippery because there are only weak intermolecular forces between layers which allow the layers to slide over one another.

Graphite conducts electricity because there is one delocalised electrons per carbon atom. The delocalised electrons are mobile charges.

19
Q

Describe the structure of diamond.

A

All carbon atoms are covalent,y bonded to four other carbon atoms.
No delocalised electrons.

20
Q

Describe the properties of diamond.

A

Very hard.
Very high melting point.
Doesn’t conduct electricity as there are no charged particles.

21
Q

What are the uses of graphite? Why?

A

Electrodes because graphite conducts electricity and has a high melting point.
Lubricant because it’s slippery (the layers in graphite can slide over each other).

22
Q

What is diamond used in cutting tools?

A

It’s very hard.

23
Q

What is fullerene?

A

A fullerene us a molecule made of carbon, shaped like a closed tube or hollow ball.

24
Q

Name two fullerenes.

A

Graphene
C60 - Buckminsterfullerene

25
Q

What are the properties of buckminsterfullerene?

A
  • Slippery due to weak intermolecular forces.
  • Low melting point.
  • Spherical.
  • Strong covalent bonds between carbon atoms in a molecules.
  • Large surface area.
26
Q

What is a polymer? Name a polymer.

A

Long chain molecules formed from many monomers. E.g Polyethene

27
Q

What are the properties of metals?

A
  • High melting points.
  • High density
  • Good conducts of electricity
  • Malleable and ductile
  • Generally shiny
28
Q

Explain why metals are malleable.

A

The atoms are arranged in uniform rows which can slide over one another.

29
Q

Limitations when representing ionic compounds of dot and cross diagrams?

A

No lattice structure or ionic bond

30
Q

Limitations when representing ionic compounds in 2D diagrams?

A

Only shows one layer, doesn’t show formation of ions.

31
Q

Limitations when representing ionic compounds of 3D diagrams?

A

Shows spaces between the ions, doesn’t show charges.

GCSE Chemistry 🧪 (11 decks)

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