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Chemistry (My Flashcards) > Topic 1 - Ionic bonding > Flashcards

Topic 1 - Ionic bonding Flashcards

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1
Q

What is an ionic bond?

A

A bond between a metal and non-metal involving the transfer of electrons.

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2
Q

In terms of electrons, describe what happens to the metal and non-metal when an ionic bond forms

A
  • The metal atom loses electrons to become a positively charged ion (cation).
  • The non-metal gains electrons to become a negatively charged ion (anion).
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3
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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4
Q

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

A
  • It has lost electrons.
  • There are fewer negatively charged electrons to cancel out the charge of the positive protons.
  • This means the overall charge becomes positive.
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5
Q

Na+ has the atomic number 11 and the mass number 23. How many protons, neutrons and electrons are in this ion?

A
  • Protons: 11
  • Electrons: 10
  • Neutrons: 12
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6
Q

O2- has the atomic number 8 and the mass number 16. How many protons, neutrons and electrons are in this ion?

A
  • Protons: 8
  • Electrons: 10
  • Neutrons: 8
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7
Q

Why do elements in groups 1, 2, 6 and 7 readily form ions?

A

So they become more stable and achieve the electron structure of the noble gases (group 8).

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8
Q

What type of ions do elements in group 1 and 2 form?

A

Cations (positive)

  • Group 1 metals will form 1+ ions
  • Group 2 metals will form 2+ ions
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9
Q

What type of ions do elements in groups 6 and 7 form?

A

They are non-metals so form anions (negative)

  • Group 6 wil form 2- ions
  • Group 7 will form 1- ions
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10
Q

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

A

The compound contains 2 elements.

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11
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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12
Q

Describe the structure of an ionic compound

A
  • Lattice structure.
  • Regular arrangement of ions.
  • Ions held together by strong electrostatic forces between ions with opposite charges.
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13
Q

What is the chemical formula of sodium oxide, formed from Na+ and O2-?

A
  • Na2O
  • Charges must balance so 2 sodium ions are required
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14
Q

What is the chemical formula of magnesium hydroxide, formed from Mg2+ and OH-?

A
  • Mg(OH)2
  • Charges must balance so 2 hydroxide ions are required.
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15
Q

What is a covalent bond?

A

A bond formed when an electron pair is shared between two atoms.

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16
Q

What forms as a result of covalent bonding?

A

A molecule

17
Q

Draw a dot and cross diagram for the formation of methane (CH4)

A
18
Q

True or false? ‘Covalent bonds are weak’

A
  • FALSE
  • Covalent bonds are strong
19
Q

Which is smaller, an atom or a molecule?

A
  • An atom.
  • Simple molecules consist of atoms joined by strong covalent bonds within the molecule.
20
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.

21
Q

When do ionic compounds electricity? Why?

A

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

22
Q

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

A

They have weak intermolecular forces (forces between molecules) which only require a little energy to overcome.

23
Q

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

A

No because there are no charged particles.

24
Q

Do giant covalent structures have a high melting point? Explain your answer.

A

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

25
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.
26
Q

True or false? ‘Metals are insoluble in water’

A
  • cTRUE
27
Q

Name two giant covalent structures formed from carbon atoms

A
  • Graphite
  • Diamond
28
Q

Describe the structure and properties relating to graphite

A
  • Each carbon atom bonded to 3 other carbon atoms.
  • Layers of hexagonal rings of carbon atoms.
  • Weak intermolecular forces between layers.
  • One delocalised electron per carbon atom.
29
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 electron per carbon atom. The delocalised electrons are mobile charges.
30
Q

Describe the structure of diamond

A
  • All carbon atom are covalently bonded to four other carbon atoms.
  • No delocalised electrons
31
Q

Describe the properties of diamond

A
  • Very hard.
  • Very high melting point.
  • Doesn’t conduct electricity as there are no charged particles.
32
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).
33
Q

Why is diamond used in cutting tools?

A

It’s very hard

34
Q

What is a fullerene?

A

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

35
Q

Name two fullerenes

A
  • Graphene
  • C60 (buckminsterfullerene)
36
Q

What are the properties of the fullerene C60?

A
  • Slippery due to weak intermolecular forces.
  • Low melting point.
  • Spherical.
  • Strong covalent bonds between carbon atoms in a molecule.
  • Large surface area.
37
Q

What are the properties of graphene?

A
  • High melting point due to covalent bonding between carbon atoms.
  • Conducts electricity because it has delocalised electrons.
38
Q

Why is graphene useful in electronics?

A
  • It is extremely strong and has delocalised electrons which are free to move and carry charge.
  • It is only one atom thick as it is a single layer of graphite.

Chemistry (My Flashcards) (17 decks)

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