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chemistry. > Bonding, Structure and Properties of Matter > Flashcards

Bonding, Structure and Properties of Matter Flashcards

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1
Q

What are ionic bonds formed between?

A

Metal and non-metal elements.

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2
Q

What do strong electrostatic attraction do?

A

Attracts oppositely charged ions together in an ionic bond.

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3
Q

What do ionic compounds form on a large scale?

A

Ionic lattices.

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4
Q

What are the limitations of using dot and cross, ball and stick, two and three dimensional diagrams for ionic and covalent bonding?

A

› they don’t show the structure of the compound.
› the size of the ions aren’t shown.
› arrangement.

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5
Q

CHECK PAGE 51 IN CHEMISTRY REVISION GUIDE TO LEARN EMPIRICAL FORMULA.

A

CHECK ANSWERS AFTER TRYING IT OUT.

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6
Q

What are the 3 properties of ionic compounds?

A

› high melting points and boiling points - lots of energy needed to overcome many strong bonds.
› when solid, the ions are held in place so compounds can’t conduct electricity.
↳ when they are molten or dissolved, the ions are free to move and they’ll carry electric charge.
› giant ionic lattice structure - electrostatic forces of attraction between oppositely charged ions act in all directions.

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7
Q

Why do ionic compounds have high melting points?

A

› the ions have a closely packed regular lattice arrangement.
› they are very strong electrostatic forces of attraction between oppositely charge ions in all directions in the lattice.

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8
Q

Where are covalent bonds formed?

A

Between non-metal elements.

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9
Q

What is a covalent bond?

A

A shared pair of electrons between two non-metal atoms.

[it can happen in non-metals compounds and non mental elements]

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10
Q

Give 3 properties of simple covalent compounds.

A

› simple molecular structures.
› held together by very strong covalent bonds - forces of attraction between these molecules are very weak.
› most molecule substances are gases or liquids at room temperature.
›as they get bigger, the strength of the intercellular forces increases so more energy is needed to break them and the melting and boiling points increases.
› don’t conduct electricity as they aren’t charged so they are no free electrons or ions.

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11
Q

Why do simple covalent compounds not conduct electricity?

A

They aren’t charged so they are no free electrons or ions.

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12
Q

Why do simple covalent compounds have a low melting and boiling point?

A

Molecules are easily parted from each other.

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13
Q

What are the 3 different types of of giant covalent structures?

A

Diamond, graphite and silicon dioxide.

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14
Q

Describe a diamond giant covalent structure.

A

Each carbon atom forms four covalent bonds in a very rigid giant covalent structure.

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15
Q

Describe a graphite giant covalent structure.

A

Each carbon atom forms three covalent bonds to create layers of hexagons. Each carbon atom also has a delocalised (free) electron.

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16
Q

Describe a silicon dioxide giant covalent structure.

A

Sometimes called silica, this is what sand is made of. Each gram of sand is one giant structure of silicon and oxygen.

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17
Q

What are the 3 properties of a diamond covalent structures?

A

› really hard - four covalent bonds.
› very high melting point - covalent bonds take a lot of energy to break.
› doesn’t conduct electricity as it has no free electrons or ions.

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18
Q

What are the 4 properties of a graphite covalent structures?

A

› three covalent bonds creating sheets of carbon atoms arranged in hexagons.
› no covalent bonds between layers and held together weakly so free to move over each other.
↳ soft and slippery.
› high melting point.
› one electron thats delocalised (free) and can move so it conducts electricity and thermal energy.

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19
Q

What are the 4 properties of a graphene covalent structures?

A

GRAPHENE IS ONE LAYER OF GRAPHITE
› a sheet of carbon atoms joined together in hexagons.
›one atom thick - two dimensional substance.
›very strong and light.
› delocalised electrons so can conduct electricity through the whole structure.
› high melting point.

20
Q

What is a fullerenes?

A

Molecules of carbon shaped like a closed tubes or hollow balls which can be used to deliver drugs into the body and as lubricants.

21
Q

What do pure metals and alloys (mixture of metals) have in common?

A

Metallic bonding.

22
Q

Describe metallic bonding.

A

Positive metals ions surrounded by a sea of delocalised electrons.

23
Q

Why are alloys harder than pure metals?

A

› pure metals are often too soft when pure - most metals we use everyday are alloys.
› different elements have different sized atoms so when another element is mixed with a pure metal, the new metal atoms will distort the layers of metal atoms making it more difficult for them to slide over each other making alloys harder than pure metals.

24
Q

What are alloys?

A

A mixture of two or more metals or a metal and another element.

25
Q

What do these symbols mean?

a. (s)
b. (l)
c. (g)
d. (aq)

A

a. solid.
b. liquid.
c. gas.
d. aqueous.

26
Q

USE DATA TO PREDICT THE STATES OF MATTER AT GIVEN TEMPERATURE.

A

CHECK ANSWERS AFTER.

27
Q

What are the limitations of the particle theory?

A

› shape - particles aren’t solid or inelastic and aren’t spheres.
› no forces between particles - no way of knowing how strong they are.

28
Q

What are ions?

A

Charged particles made when electrons are transferred.

29
Q

What is ionic bonding?

A

The electrostatic attraction between oppositely charged ions.

30
Q

What are the properties of simple molecular substances?

A

> low melting and boiling point.
↳ mostly gases o liquids at room temperature.
don’t conduct electricity.
↳ there are no charged particles to carry charge.

31
Q

What are polymers?

A

Very long chains of repeating units.

32
Q

How are polymers at room temperature?

A

Usually solids as they have relatively strong intermolecular forces.

33
Q

What are giant covalent structures?

A

Solids containing atoms which are al bonded to each other by strong covalent bonds.

34
Q

What are the properties of giant covalent bonds?

A

> high melting and boiling point.
↳ lots of energy needed to overcome strong covalent bonds.
don’t conduct electricity.
↳ no charged particles to carry charge.

35
Q

What are nanotubes?

A

Cylindrical fullerenes used in nanotechnology, electronics and materials.

[they have a high length to diameter ratios]

36
Q

What are the properties of metals?

A

> high melting and boiling points.
↳ lots of energy needed to overcome strong metallic bonds.
good thermal conductors.
↳ energy transferred by delocalised electrons.
good electrical conductors.
↳ delocalised electrons carry charge.
soft and malleable.
↳ layers in metals slide over each other.

37
Q

What is the particle arrangement, movement and closeness of solids?

A

ARRANGEMENT ⟶ regular.
MOVEMENT ⟶ fixed position, vibrate.
CLOSENESS ⟶ very close together.

38
Q

What is the particle arrangement, movement and closeness of liquid?

A

ARRANGEMENT ⟶ random.
MOVEMENT ⟶ move around together.
CLOSENESS ⟶ close together.

39
Q

What is the particle arrangement, movement and closeness of gases?

A

ARRANGEMENT ⟶ random.
MOVEMENT ⟶ move quickly in all directions.
CLOSENESS ⟶ far apart.

40
Q

What is the process called when a solid changes state to a liquid?

A

Melting.

41
Q

What is the process called when a liquid changes state to a gas?

A

Boiling.

42
Q

What is the process called when a gas changes state to a liquid?

A

Condensing.

43
Q

What is the process called when a liquid changes state to a solid?

A

Freezing.

44
Q

What happens when a substance is being molten or boiled?

A

Substance heats up ⟶ particles gain energy ⟶ forces between particles weaken ⟶ particles break free from position.

45
Q

What happens when a substance is being condensed or frozen?

A

Substance cools down ⟶ particles lose energy ⟶ forces between particles form ⟶ particles held into position.

chemistry. (13 decks)

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