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IGCSE CAMBRIDGE CHEMISTRY 2023. > Chemical Bonding. > Flashcards

Chemical Bonding. Flashcards

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1
Q

What is chemical bonding?

A

The joining, chemically of two or more atoms to form a compound.

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2
Q

What is an ion?

A

An ion is an electrically charged atom or group of atoms formed by the loss or gain of electrons.

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3
Q

Why would an atom loses or gain electrons in the outermost shell?

A

This loss or gain of electrons takes place to gain a full outer shell of electrons.

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4
Q

Ionisation of metals and non-metals:

A

Metals: all metals lose electrons to other atoms to become positively charged ions.

Non-metals: all non-metals gain electrons from other atoms to become negatively charged ions.

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5
Q

What holds the positive and negative charges of ionic compounds together?

A

The positive and negative charges are held together by the strong electrostatic forces of attraction between opposite charges.

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6
Q

What is an ionic bond?

A

An ionic bond is the electrostatic force of attraction between positive and negative ions.

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7
Q

What happens when an atom loses an electron?

A

When an atom loses an electron it forms positively charged ions called cations.

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8
Q

What happens when an atom gains electrons?

A

When an atoms gains electrons it forms negatively charged ions called anions.

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9
Q

What is a lattice structure?

A

A regular arrangement of alternating positive and negative ions.

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10
Q

How do you describe the forces of attraction between the positive and negative ions of a giant lattice structure?

A

The forces of attraction between the positive and negative ions of a giant lattice structure are very strong.

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11
Q

What are the 3 physical properties of ionic compounds?

A
  • Ionic compounds have high melting and boiling points.
  • Ionic compounds are soluble in water but insoluble in organic solvents.
  • Ionic compounds conduct electricity only when molten or when dissolved in water because the ions are mobile.
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12
Q

Why do Ionic compounds have a high melting and boiling point?

A

Because a lot of heat energy is required to break the strong force of attraction..

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13
Q

Why are ionic compounds soluble in water but not organic solvents?

A

They are soluble in water because the water molecules are able to separate the ions from one another and keep the ions in solution.

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14
Q

When are covalent compounds formed?

A

Covalent compounds are formed when electrons are shared between atoms.

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15
Q

What are the properties of covalent compounds?

A
  • Covalent compounds have low melting points and boiling points because the intermolecular attractive forces are weak.
  • Covalent compounds are insoluble in water but can dissolve in organic substances.
  • Covalent compounds do not conduct electricity because they have no free electrons or ions.
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16
Q

What are the allotropes of carbon?

A

Diamond and graphite are allotropes of carbon that have giant covalent structures.

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17
Q

What are the three properties of diamonds?

A
  • Diamond does not conduct electricity
  • Diamond has very high melting and boiling point.
  • Diamond is extremely hard and dense
18
Q

What is diamond used in?

A

Diamond is used in jewellery and as cutting tools.

19
Q

In a diamond, how is a giant tetrahedron covalent structure formed?

A

Each carbon atom bonds with four other carbons, forming a tetrahedron.

20
Q

What are the three properties of graphite?

A
  • Graphite conducts electricity.
  • Graphite has a very high melting point.
  • Graphite is soft and slippery.
21
Q

What are the covalent bonds of a diamond like.

A

All the covalent bonds in diamonds are identical and strong with no weak intermolecular forces.

22
Q

Why does graphite conduct electricity?

A

The free electrons that exist in between the layers and are free to move and carry charge, hence graphite can conduct electricity.

23
Q

In graphite, how is a giant hexagonal covalent structure formed?

A

Each carbon atom is bonded to three others forming layers of hexagonal-shaped forms, leaving one free electron per carbon atom.

24
Q

Why is graphite slippery and smooth?

A

The covalent bonds within the layers are very strong but the layers are connected to each other by weak intermolecular forces, hence the layers can slide over each other making graphite slippery and smooth.

25
Q

What is graphite used for?

A

Graphite is used in pencils, industrial lubricants and is also used to make carbon electrodes for electrolysis.

26
Q

Why do diamond and silicon (IV) oxide not conduct electricity?

A

Diamond and silicon (IV) oxide do not conduct electricity because all its valence electrons are used in bonding - no free electrons.

27
Q

In silicon (IV) oxide or silicon dioxide, how is a giant tetrahedron covalent structure formed?

A

A tetrahedron is formed because each silicon atom is bonded to four oxygen atoms but each oxygen atom is bonded to only two silicon atoms.

28
Q

What does silicon (IV) oxide or silicon dioxide or SiO2 naturally occur as?

A

SiO2 is a macromolecular compound that occurs naturally as sand and quartz.

29
Q

What are the 4 properties of silicon (IV) oxide?

A
  • Silicon (IV) oxide is very hard.
  • Silicon (IV) oxide has very high melting and boiling points.
  • Silicon (IV) oxide does not conduct electricity.
  • Silicon (IV) oxide has lots of very strong covalent bonds and no intermolecular forces.
30
Q

What is metallic bonding?

A

The electrostatic force of attraction between positive metal ions and a sea of delocalized electrons.

31
Q

Why are metallic bonds strong?

A

Metallic bonds are strong because of the attraction between the positive metal ions and the negatively charged delocalized electrons.

32
Q

What are the 3 properties of metals?

A
  • Metals have high melting and boiling points.
  • Metals are good thermal and electric conductors.
  • Metals are malleable(can be hammered into shape) and ductile (can be drawn into a wire).
  • Metals are lustrous.
  • Metals are sonorous.
33
Q

Why do metals have a high melting and boiling point?

A

There are many strong metallic bonds in giant metallic structures therefore a lot of heat energy is needed to overcome forces and break these bonds.

34
Q

Why are metals good conductors of electricity?

A

Metals can conduct electricity because the sea of delocalized electrons is able to move.

35
Q

Why are metals, good thermal conductors?

A

Conduction of heat is due to vibrations of the atoms passing on the energy from one atom to the next.

36
Q

Why are metals malleable and ductile?

A

The regular arrangement of metal ions means that the layers of ions are able to slide over each other easily without the metal shattering, making metals malleable and ductile.

37
Q

Practical studying:

A
  • Drawing Ionic Bonds.
  • Drawing Covalent Bonds.
  • Metallic Bonds.
38
Q

Metal + non-metal bonding =

A

Metal + non-metal = ionic bond.

39
Q

Non-metal + non-metal bonding =

A

Non-metal + non-metal = covalent.

40
Q

Metal + metal bonding =

A

Metal + metal = metallic.

41
Q

What is an alloy?

A

An alloy is a mixture of two or more elements , where at least one element is a metal

42
Q

What are the four properties of non-metals?

A
  • Non-metals are dull.
  • Non-metals are poor conductors of electricity and heat.
  • Non-metals are brittle.
  • Non-metals have a low boiling and melting point.

IGCSE CAMBRIDGE CHEMISTRY 2023. (10 decks)

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