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Chemistry > SC5,SC6 & SC7 > Flashcards

SC5,SC6 & SC7 Flashcards

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1
Q

What are bonds?

A

Bonds are forces of attraction that holds atoms together

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2
Q

What happens when bonds form between atoms?

A

Energy is released from the atoms which makes them more stable (less reactive)

More stable with a full outer shell

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3
Q

How are ions formed?

A

It’s the transfer of electrons between atoms which form charged particles (ions)

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4
Q

What is ionic bonding?

A

Metal and non metal

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5
Q

What happens when metals react?

A

They lose outer shell elections to leave a full electron shell

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6
Q

What happens when non-metals react?

A

They gain electrons to achieve a full electron shell

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7
Q

What are cations?

A

When metals lose electrons to form positive ions

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8
Q

What are anions?

A

When non-metals gain electrons to form negative ions

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9
Q

What are electrostatic forces?

A

The force of attraction between all positively and negatively charged objects

Hold oppositely charge ions together and form an ionic bond between them

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10
Q

How many electrons are lost or gained in group 1 elements?

What is the charge on the ion?

A

1 electron is lost

1+

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11
Q

How many electrons are lost or gained in group 2 elements?

What is the charge on the ion?

A

2 electrons are lost

2+

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12
Q

How many electrons are lost or gained in group 6 elements?

What is the charge on the ion?

A

2 electrons are gained

2-

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13
Q

How many electrons are lost or gained in group 7 elements?

What is the charge on the ion?

A

1 electron is gained

1-

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14
Q

What are ionic compounds?

A

They’re formed by the loss and gain of electrons

Held together by strong electrostatic forces of attraction between oppositely charged ions

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15
Q

What is a lattice structure?

A

The strong bonds allow ‘billions’ of ions that are packed together in a regular repeating arrangement called a lattice structure

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16
Q

What is the formula of ionic compounds?

A

Needs to contain the same number of positive charges as negative charges

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17
Q

What are the melting and boiling points like in ionic compounds?

A

The forces are strong
A lot of energy needed to overcome forces
Need to be heated on high temperatures before they change state
High melting and boiling points

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18
Q

What happens if an ion has more than 1 charge?

A

They attract other ions more strongly than ions with 1 charge
More energy needed to overcome electrostatic forces of attraction
Melting points = higher

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19
Q

When do ionic compounds conduct electricity?

A

When they are molten or dissolved in water

Not when they are solid

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20
Q

What are the conditions for a substance to conduct electricity?

A

Must contain charged particles (carry the current)

Particles must be free to move

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21
Q

Where are the negative ions (anions) attracted to?

A

They’re attracted to the positive electrode, called the anode

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22
Q

Where are the positive ions (cations) attracted to?

A

They’re attracted to the negative electrode, called the cathode

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23
Q

Do the ions or electrons move to conduct electricity?

A

The ions moving enable ionic compounds to conduct electricity

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24
Q

What are molecular substances?

A

Contain groups of atoms that are held together by strong bonds called covalent bonds

25
Q

What is a covalent bond?

When are covalent bonds formed?

A

A covalent bond is a shared pair of electrons

When non-metals react together
Produced by sharing pairs of electrons

26
Q

What happens when the bond forms?

A

It makes the atom more stable as they use the shared electrons to complete their outer shell

E.g noble gases

27
Q

What are the forces of attraction like in the bonded atom?

A

Strong electrostatic forces between the positive nuclei and negative electrons

Weak forces between molecules (intermolecular forces), doesn’t take much energy to overcome the weak intermolecular forces

28
Q

What are compounds?

A

Compounds contain atoms of more than one element, chemically joined together by bonds

29
Q

What is the conduction of electricity like in molecules?

A

They can’t conduct electricity as the electrons are free to move as there are strong electrostatic forces that hold the negatively charged electrons and positive nucleus together

30
Q

What is a polymer?

A

A polymer is formed when monomers (small,simple molecules) are joined in a chain

31
Q

What do most polymers contain?

A

Contain a chain of carbon atoms

32
Q

What are the features of longer polymers?

A

More intermolecular forces between them

Have higher melting and boiling points than shorter ones

33
Q

What are allotropes?

A

Different forms of the same element

34
Q

What are fullerenes?

A

Simple molecules formed by carbon in which each carbon atom is covalently bonded to 3 other carbon atoms

35
Q

What are the features of fullerenes?

A

They have weak intermolecular forces between molecules
Low melting point and boiling point
Soft and slippery
Molecules strong due to covalent bonds

36
Q

What is graphene?

A

Not a simple molecule
Consists of sheets of carbon atoms with no fixed formula
Light (one atom thick) but covalent bonds make it very strong

37
Q

Is graphene a good electrical conductor?

A

Yes it is because it’s electrons are free to move to across the surface

38
Q

Name to allotropes of carbon that aren’t simple structures?

A

Diamond and graphite (covalent, giant molecular structures)

39
Q

What is the melting point in diamond and graphite?

A

The melting point is high as it has strong covalent bonds that need lots of energy to be broken

40
Q

How many covalent bonds does graphite have?

A

3 covalent bonds for each atom

Gives a layered structure so not all electrons are held together in covalent bonds

41
Q

What are delocalised electrons?

A

Electrons that are free to move and can carry an electrical current

Graphite is a good conductor (and cheap and not reactive)

42
Q

Why is graphite soft?

A

Held together by weak forces of attraction which allow layers to slide past each other

43
Q

How many covalent bonds does diamond have?

A

Held together by 4 covalent bonds

44
Q

What is the structure like in diamond?

A

Rigid network of carbon atoms in a tetrahedral arrangement, held together by strong covalent bonds

45
Q

What is diamond useful for?

A

Tools

46
Q

Is diamond an electrical insulator?

A

Yes it is because it has no free charged particles

47
Q

What happens to the lecterns in the outer shell of metal atoms?

A

Lost from each atom and become free to move randomly throughout the metal

48
Q

What happens once the outer electrons are lost from the metal atom?

A

They form a giant lattice of positive metal ions surrounded by a sea of delocalised electrons

49
Q

What is metallic bonding?

A

Electrostatic attraction between the positive ions and the negative delocalised electrons
Attraction is strong so metals have high boiling and melting points

50
Q

Why are metals malleable?

A

The layers of ions slide over each other when the metal is hit
Sea of electrons holds ions together so metal changes shape

51
Q

How do metals conduct electricity?

A

Delocalised electrons move randomly between positive metals in all directions
When voltage applied, electrons move to positive side so transfers energy and forms an electrical current

52
Q

Why do some substances conduct electricity better than others?

A

The electrical conductivity of metals increases as the number of delocalised electrons increases

53
Q

Which has a higher electrical conductivity: magnesium or sodium?

A

Magnesium as it has a 2+ charge so contributes 2 electrons to the sea of electrons whereas sodium has a 1+ charge so only contributes 1 electron to the sea of electrons

Magnesium has better electrical conductivity than sodium

54
Q

What are simple molecules?

A

Non metal elements and compounds

55
Q

What are the properties of simple molecules?

A

Low melting/boiling points
Few soluble in water
Most don’t conduct electricity

56
Q

What are the bonds like between giant covalent?

A

Covalent bonds formed when atoms share pairs of electrons

57
Q

What are the properties of giant covalent structures?

A

High melting/boiling points
Insoluble in water
Most don’t conduct electricity (carbon as graphite does)

58
Q

What is the structure of metallics?

A

Billions of ions held together in a giant lattice structure of positive ions in a sea of negative delocalised electrons

59
Q

What is the properties of metallics?

A

High melting/boiling points
Insoluble in water
Conduct electricity when solid or liquid

Chemistry (7 decks)

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