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Chemistry GCSE > Bonding > Flashcards

Bonding Flashcards

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1
Q

What creates an ionic bond?

A

Metals + non metals

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2
Q

What creates a covalent bond

A

Non metals only

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3
Q

What creates a metallic bond?

A

Metals only

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4
Q

Properties of ionic compounds

A

High melting and boiling points- the stronger the ion the stronger the bond

Dissolve in water- lattice breaks and ions are able to move

Do not conduct electricity as a solid- ions are stationary in the lattice

Conduct electricity in a solution Or as molten- ions move freely as they are not held in the lattice

Brittle- shatter when they are hit

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5
Q

What are ionic bonds held in

A

3D lattice

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6
Q

Definition on ionic bonding

A

The electrostatic attraction between oppositely charged ions

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7
Q

Definition in covalent bonding

A

The electrostatic attraction of a shared pair of electrons and the nuclei of two atoms

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8
Q

Examples of simple molecular covalent compounds

A

Oxygen, chlorine gas, water

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9
Q

Properties of simple molecular covalent compounds

A

Low melting and boiling points

Do not conduct electricity as they do now have charged particles that can move

Weak intermolecular forces

Strong covalent bonds

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10
Q

What happens when a simple molecular substance melts/boils

A

Weak intermolecular forces are broken, this requires little energy

Covalent bonds are not broken

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11
Q

Properties of buckminster fullerenes (Bucky balls)

A

Same as simple molecular

Don’t conduct electricity

Low melting points

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12
Q

Uses of Bucky balls

A

A lubricant

Delivering drugs to parts of the body

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13
Q

Properties of silicon dioxide (sand)

A

Structure- giant covalent lattice

Bonding- each oxygen atom is bonded to 2 silicon atoms/each silicon atoms is bonded to 4 oxygen atoms

Melting point- very high. Lots of energy needed to break strong covalent bonds

Strength- very hard. (Strong covalent bonds)

electrical conductivity- does not conduct electricity. No free moving charged particles

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14
Q

Properties of diamond

A

Structure- giant covalent lattice

Bonding- each carbon atom bonded to 4 others

Melting point- very high. Lots of every needed to break strong covalent bonds

Strength- very hard. Lots of energy needed to break strong covalent bonds

Electrical conductivity - doesn’t conduct. No free charged particles that can move

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15
Q

Properties of graphite

A

Structure- giant covalent lattice

Bonding- each carbon atom bonded to 3 others. 1 unbounded delocalised electron per carbon atom

Melting point- very high. Lots of energy needed to break strong covalent bonds

Strength- soft. Layers can slide over each other

Electrical conductivity- conducts. Delocalised electrons can flow

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16
Q

Definition of metallic bonding

A

The electrostatic attraction between delocalised electrons and positivity charged metal ions

17
Q

Properties of metallic compounds

A

Structure- 3D lattice

High melting and boiling points- strong metallic bonds require lots of energy to break

Conduct when solid and when molten- delocalised electrons can flow

Malleable&ductile- layers of metal ions can slide over each other

18
Q

What is the trend in melting point of metals

A

The melting point increases as metallic bond strength increases

This is due to a greater electrostatic attraction between 3+ delocalised electrons

Chemistry GCSE (4 decks)

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