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Chemistry IG > Topic 2 > Flashcards

Topic 2 Flashcards

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1
Q

What needs to happen for a metal and non-metal atom to be stable?

A

For a metal atom to be stable it needs to lose electrons. For a non-metal atom to be stable it needs to gain electrons.

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2
Q

Why are atoms neutral?

A

They have the same number of protons and electrons

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3
Q

What is an atom that loses electrons called, and what is its charge?

A

Cation or a positive ion and it has a positive charge

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4
Q

What is an atom that gains electrons called?

A

Anion and it has a negative charge

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5
Q

What is an ion?

A

An atom that has gained or lost electrons

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6
Q

Note to remember for writing formulae for an ionic compound

A

The number of positive and negative charges must be equal, so the overall compound has no charge. Use criss cross method and swap charges around.

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7
Q

What is an ionic lattice structure?

A

A 3D structure of alternating positive and negative ions that forms crystalline powders

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8
Q

What are the forces in an ionic lattice?

A

Non-directional

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9
Q

What holds the positive and negative ions together?

A

Strong electrostatic forces of attraction between opposite charges

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10
Q

What to remember when drawing ionic bonds

A
  1. Draw electron arrangement
    - Only show valence electrons
    - Metal and non-metal electrons must look different
  2. Draw the ions
    - No valence electrons remain in metal ion
    - Metal atom electrons move to non-metal atom
  3. Ionic bond
    - Put square brackets around both ions
    - Add ion charge on the outside
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11
Q

List the 8 polyatomic ions to be memorized

A
  1. Ammonium (NH4 charge +1)
  2. Nitrite (NO2 charge -1)
  3. Nitrate (NO3 charge -1)
  4. Sulfite (SO3 charge 2-)
  5. Sulfate (SO4 charge 2-)
  6. Hydroxide (OH charge 1-)
  7. Phosphate (PO4 charge 3-)
  8. Carbonate (CO3 charge 2-)
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12
Q

Can metals chemically bond together?

A

No but they can be mixed to form alloys

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13
Q

What happens in metallic bonding?

A

Each metal atom loses its valence electrons. These electrons freely move through the lattice between the positively charged metal ions forming a sea of free moving (delocalised) electrons. This forms a strong electrostatic force of attraction.

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14
Q

What do metal ions form?

A

A 3D lattice with non-directional bonding

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15
Q

What do covalent substances contain?

A

Non-metal atoms

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16
Q

What happens in covalent bonds?

A

Atoms want to achieve a noble-gas configuration but instead of gaining or losing electrons, atoms share electrons

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17
Q

What’s a double bond?

A

2 pairs of electrons are shared. Eg CO2

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18
Q

What’s a triple bond?

A

Three pairs of electrons are shared. Eg N2

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19
Q

What are the 2 types of covalent substances?

A

Small molecules/ simple molecular
Giant covalent structures/networks

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20
Q

What is a simple molecular substance?

A

A covalent substance that is made up of a small number of non-metal atoms held together with a small number of covalent bonds

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21
Q

Why do covalent bonds have low melting and boiling points?

A

Covalent bonds between non-metal atoms are very strong, forming individual molecules. However, these molecules are held together by attractive forces between individual molecules which are very weak

22
Q

What is metallic bonding?

A

The electrostatic attraction between the positive ions in a giant metallic lattice and a ‘sea’ of delocalised electrons

23
Q

Explain in terms of structure and bonding why metals have good electrical conductivity

A

Metals have electrons that are delocalized which can carry a charge through the metal

24
Q

Explain in terms of structure and bonding why metals are malleable and ductile

A

Metals are surrounded by a ‘sea’ of delocalised electrons. When the slightly positive metal atoms are deformed, the free moving electrons flow around them shielding the cations from eachother.

25
Q

Explain in terms of structure and bonding why metals have high melting and boiling points

A

As the electrostatic force of attraction of the metallic bond is strong it requires a lot of energy to overcome resulting in metals being solid at room temp and having high melting and boiling points

26
Q

What is a giant covalent structure?

A

Networks made up of a large number of non-metal atoms, held together with a large number of strong covalent bonds

27
Q

What is an allotrope?

A

Two or more physical forms in which an element can exist. E.g. diamond and graphite are both made of carbon

28
Q

Describe the giant covalent structure of diamond

A

Diamond’s structure is an allotrope of carbon where each atom is covalently bonded to 4 other carbon atoms in a tetrahedral arrangement. All the covalent bonds are identical, very strong and there are no intermolecular forces

29
Q

Describe the giant covalent structure of graphite

A

Graphite’s structure is an allotrope of carbon where each atom is covalently bonded to 3 other carbon atoms forming layers of hexagons leaving one free electron per carbon atom that becomes delocalised. The covalent bonds within the layers are very strong, but the layers are attracted to each other by weak intermolecular forces meaning graphite has an electrical charge

30
Q

What are the properties of diamond?

A
  • It does not conduct electricity
  • It has a very high melting point
  • It is extremely hard and dense
31
Q

Why is graphite a good lubricant?

A

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

32
Q

What are the properties of graphite?

A
  • Conducts electricity
  • Has a very high melting point
  • Is soft and slippery, less dense than diamond
33
Q

Why can diamond and silicon oxide not conduct electricity?

A

All the outer shell electrons in carbon are held in the four covalent bonds around each carbon atom, so there are no freely moving charged particles to carry the current

34
Q

Why is diamond used for cutting tools?

A

The rigid network of carbon atoms, held together by strong covalent bonds, makes diamond very hard.

35
Q

Why does diamond have a high melting point?

A

The four covalent bonds are very strong and extend in a giant lattice, so a very large amount of heat energy is needed to break the lattice thus it has a very high melting point

36
Q

Describe the similarity in properties between
diamond and silicon(IV) oxide

A

Both silicon oxide and diamond have tetrahedral structures meaning they both have no delocalised electrons so their properties are similar as they are both hard and have a high melting point

37
Q

Describe the giant covalent structure of
silicon(IV) oxide

A

Formed when silicon atoms covalently bond to 4 oxygen atoms in a tetrahedral strcture

38
Q

How is a covalent bond formed?

A

when a pair of electrons is shared between two non-metal atoms giving them a noble gas electronic configurations

39
Q

Explain in terms of structure and bonding why simple covalent substances have low melting and boiling points

A

Substances are made up of simple molecules and the atoms are joined by covalent bonds. Molecules have weak intermolecular forces so not much energy is needed to separate the molecules from each other

40
Q

Explain in terms of structure and bonding why simple covalent substances have poor electrical conductivity

A

There are no free moving charged particles in simple covalent substances so no covalent structures will conduct electricity in any state

41
Q

Are simple covalent molecular substances soluble?

A

Covalent molecular structures dissolve in covalent substances. Not many are soluble in water, but they are soluble in an organic solvent

42
Q

What is an ionic bond?

A

a strong force of attraction between oppositely charged ions

43
Q

Describe the formation of positive ions, known as cations

A

Atoms lose electrons from their outer shell when they form positive ions. These ions are positive because they contain more protons than electrons

44
Q

Describe the formation of negative ions, known as anions

A

A negative ion or anion is an atom that has gained electrons. These ions are negative because they contain more electrons than protons

45
Q

Describe the giant lattice structure of ionic
compounds

A

a regular arrangement of alternating positive and negative ions

46
Q

Explain in terms of structure and bonding why ionic compounds have high melting and boiling points

A

Ions have a regular arrangement in a lattice structure and they are attracted to each other by strong electrostatic forces of attraction. Large amounts of energy are needed to overcome and separate ions

47
Q

Explain in terms of structure and bonding why ionic compounds have good electrical conductivity when aqueous or molten and poor when solid

A

Ionic compounds are made of positive and negative ions that are charged. In a solid they can’t move but when in liquid, molten or dissolved they can conduct electricity

48
Q

Are ionic compounds soluble?

A

Most are soluble in water because water is attracted to the positive and negative ions and so will dissolve. Most aren’t soluble in organic solvents

49
Q

Why is a substance soluble?

A

because the solvent is attracted to the solute particles and that attractive force can overcome the attractive force between the solute

50
Q

What does a substance need to conduct electricity?

A

A substance must contain free moving/mobile charged particles (the charged particles can be ions or electrons)

Chemistry IG (9 decks)

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