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Year 10 > Chemistry > Flashcards

Chemistry Flashcards

1
Q

Melting point: Simple covalent

A

Low

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2
Q

Melting point: giant covalent

A

High

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3
Q

Melting point: metallic

A

High

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4
Q

Melting point: giant covalent

A

High

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5
Q

Types of bonding

A

Giant ionic
Giant covalent
Simple covalent
Metallic

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6
Q

Why are melting points high in giant ionic, giant covalent and metallic?

A

Strong electrostatic force of attraction

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7
Q

Why are melting points low in simple covalent?

A

Weak intermolecular forces of attraction.

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8
Q

Why are intermolecular forces so easy to break?

A

They don’t require much energy to break.

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9
Q

Why can simple ionic compounds conduct when molten but not solid?

A

When solid, ionic compounds have their ions in fixed positions and so cannot carry charge. when molten, ionic compounds have their ions free to move and carry charge.

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10
Q

Why can metals conduct?

A

They have free delocalised electrons, able to move around the structure and carry charge.

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11
Q

Why is chlorine a gas at room temperature, but sodium chloride is not?

A

Chlorine is a gas as it has covalent bonding, meaning it has a low melting and boiling point with simple molecules. Sodium chloride is a solid at room temperature as it has ionic bonding, strong bonds, expands in all directions (lattice), large amounts of energy are needed to break bonds.

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12
Q

Why may an experiment be innacurate?

A

Solution may have been improperly stirred,
Concentrations may be differet,
Sample sizes may be inaccurate.

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13
Q

Graphite is soft, why?

A

Layers can Slide Over each other because there are no covalent bonds between layers

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14
Q

Diamond is hard, why?

A

It has four covalent bonds between the atoms and covalent bonds are strong.

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15
Q

Graphite conducts, why?

A

Graphite has delocalised electrons which can move throughout the whole structure.

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16
Q

Why are diamonds used in cutting bits?

A

They are hard (you may loose marks for strong)

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17
Q

Why are balls a bad way to show crystals

A

They are not in 3D
Particles should be different sizes

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18
Q

What kind of metal forms a coloured metal?

A

Transition metals

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19
Q

Atoms vs Ions

A

Atoms are nuteral, ions have a charge.

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20
Q

ionic compounds -ide vs -ate

A

Ide means the ionic compound is comprised of two or more elements, ate means it has three or more

21
Q

Ionic lattice structure

A

Ionic lattices are regular repeating patterns of oppositely charged atomic ions

22
Q

How are ions held together?

A

Ionic lattices are held together by the electrostatic force of attraction between positive and negative ions

23
Q

Why do ionic compounds have high melting points?

A

Ionic compounds have high melting points as it requires a lot of energy to break the electrostatic forces of attraction between molecules

24
Q

Why do covalent bonded compounds melt and boil at low temperatures?

A

Weak intermolecular forces between molecules

25
Q

Why do covalent substances not transmit electricity well?

A

Covalent substances have no free electrons to transmit energy

26
Q

Why do we use diamonds? What do we use them in?

A

Diamonds are hard, we use them in blade edges, drills, jewellery.

27
Q

Limitations if the dot and cross representation of bonding

A

Doesn’t illustrate the relative sizes of the atoms and fails to illustrate the 3D aspect of atoms.

28
Q

Weak Acids:

A

They do not fully ionise

29
Q

Strong Acids:

A

Fully ionise

30
Q

Acids with Carbonates:

A

Produces A salt, water and carbon dioxide.

31
Q

Acids + Metals

A

Salt + Hydrogen

32
Q

Acids ions:

A

H+ Ions

33
Q

Detecting Acids:

A

Litmus: Red
Methyl Orange: Red
Phenolphthalein: Clear

34
Q

What is relative formula mass?

A

Relative formula mass is the mass of all atoms in a substance.

35
Q

Ions

A

Charged atoms

36
Q

Cations

A

Positively charged

37
Q

Anions

A

Negatively charged

38
Q

Anions form from:

A

Non metals

39
Q

Cations form from:

A

Hydrogen or metals

40
Q

Covalent bonds

A

A shared pair of electrons

41
Q

Properties of covalent bonds:

A

Strong electrostatic forces
Form with metals and non metals
Produce molecules
Group number is number or bonds

42
Q

Strong covalent.

A

Low melting + boiling points
Non metals
Do not conduct as they are not charged with no free electrons.
Strong

43
Q

Giant molecular

A

Many covalent atoms in regular repeating lattice
Non metal, compounds, high melting + boiling points
Solid at room temperature.
Diamond, graphite

44
Q

What’s special about graphite?

A

Each atom bonded to three other carbon atoms, they are layers that connect with weak intermolecular forces, strong covalent bonds between atoms in layer. Regular lattice.

45
Q

Metallic bonding

A

Shiny, conductors, dense, high melting point.
Giant lattice of positively charged metal ions in sea of electrons. Malleable.

46
Q

What is metal reactivity?

A

The reactivity of a metal is linked to how easy it is for a metal to form its positive ion.

47
Q

What is the use of a fullerene

A

Lubricant

48
Q

Single bond

A

Two atoms share one pair of electrons

49
Q

Double bond

A

Two atoms with four electrons bonding

Year 10 (6 decks)

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