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Chemistry- Paper 1 > Bonding, Structure And The Properties Of Matter > Flashcards

Bonding, Structure And The Properties Of Matter Flashcards

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1
Q

What are the three types of strong chemical bonds?

A

Ionic, covalent and metallic

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2
Q

For ionic bonding how are the particles charged?

A

The particles are oppositely charged ions

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3
Q

For covalent bonding what are the particles?

A

The particles are atoms which share pairs of electrons

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4
Q

For metallic bonding what are the particles?

A

The particles are atoms which share delocalised electrons

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5
Q

Where does ionic bonding occur?

A

Ionic bonding occurs in compounds formed from metals combines with non- metals

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6
Q

Where does covalent bonding occur?

A

In most non-metallic elements and in compounds of non-metals

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7
Q

Where does metallic bonding occur?

A

Metallic bonding occurs in metallic elements and alloys

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8
Q

What sort of compound is a giant structure of ions?

A

Ionic compound

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9
Q

What are ionic compounds held together by?

A

By strong electrostatic forces of attraction between oppositely charged ions

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10
Q

What is it called in when all strong electrostatic forces of attraction act in all directions in the lattice?

A

Ionic bonding

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11
Q

An ionic compound is any compound that only contains what?

A

Ionic bonds

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12
Q

What is the structure of ionic compounds called

A

Giant ionic lattice

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13
Q

What do the ions in ionic compounds form?

A

The ions form a closely packed regular lattice arrangement

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14
Q

Why do all ionic compounds have high melting points and high boiling points?

A

Because of the many strong bonds between the ions. It takes a lot of energy to overcome this attraction

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15
Q

When ionic compounds are solid, what happens ?

A

The ions are held in place so the compounds can’t conduct electricity

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16
Q

What happens when ionic compounds melt?

A

The ions are free to move and they’ll carry electric current

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17
Q

What happens when some ionic compounds dissolve easily in water?

A

The ions separate and are all free to move in the solution so they’ll carry electric current

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18
Q

How do you find the empirical of an ionic compound from a diagram of the compound?

A

If it’s a dot and cross diagram, count up how many atoms there are of each element. Write it down to give you the emotional formula.
If it’s a 3D diagram of the ionic lattice, use it to work out what ions are in the ionic compound.
Then balance the charges of the ions so the overall charge on the compound is 0.

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19
Q

Ions are made when electrons are what?

A

Transferred

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20
Q

Are ions charged particles? Can they be single atoms or groups of atoms?

A

Yes ions are charged particles and they can be single atoms or groups of atoms

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21
Q

Atoms with full outer shell are very what

A

Very stable

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22
Q

What are atoms trying to do when the lose or gain electrons to form ions?

A

They’re trying to get a full outer shell

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23
Q

What happens when metals form ions?

A

They lose electrons from their outer shell to form positive ions

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24
Q

What happens when non-metals form ions?

A

They gain electrons into their outer shell to form negative ions

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25
Q

The number of electrons lost or gained is the same as what?

A

The same as the change on the ion

26
Q

What happens when a metal and a non-metal react together?

A

The metal atom loses electrons to form a positively charged ion and the non-metal gains these electrons to form a negatively charged ion

27
Q

What is it called when oppositely charged ions are strongly attracted to one another by electro static forces?

A

This attraction is called an ionic bond

28
Q

What groups are the most likely to form ions?

A

Groups 1 & 2 and 6 & 7

29
Q

Group 1 and 2 elements are metals and they lose electrons to form what?

A

To form positive ions (cations)

30
Q

Group 6 and 7 elements are non-metals. They gain electrons to form what?

A

To form negative ions (anions)

31
Q

Elements in the same group all have the same number of outer electrons. So they have to lose or gain the same number to get a full outer shell. And this means that they form ions with what?

A

They form ions with the same charges.

32
Q

What ions do group 1 elements form?

A

1+ ions

33
Q

What ions do group 2 elements form?

A

2+ ions

34
Q

What ions do group 6 elements form?

A

2- ions

35
Q

What ions do group 7 elements form?

A

1- ions

36
Q

A sodium atom (Na) is in group 2 so how many electrons does it lose to form a sodium ion with the same electronic structure as neon?

A

It loses 1 electron

37
Q

A magnesium atom (Mg) is in group 2 so how many electrons does it lose to form a magnesium ion with the same electronic structure as neon?

A

It loses 2 electrons

38
Q

A chlorine atom (Cl) is in group 7 so how many electrons does it gain to form a chloride ion with the same electronic structure as argon?

A

It gains 1 electron

39
Q

An oxygen atom (O) is in group 6 so how many electrons does it gain to form and oxide ion with the same electronic structure as neon?

A

It gains 2 electrons

40
Q

What do atoms form when they share pairs of electrons?

A

They form covalent bonds. These bonds between atoms are strong

41
Q

What can covalently bonded substances may consist of?

A

Small molecules

42
Q

Some covalently bonded substances have very large what?

A

Very large molecules such as polymers

43
Q

Some covalently bonded substances have giant covalent structures such as what?

A

Such as diamond and silicon dioxide

44
Q

What is covalent bonding?

A

Where atoms share electrons with each other so that they’ve got full outer shells

45
Q

What happens when non-metal atoms bond together?

A

They share pairs of electrons to make covalent bonds

46
Q

The positively charged nuclei of the bonded atoms are attracted to the shared pair of electrons by what, making covalent bonds very what?

A

By electrostatic forces, making covalent bonds very strong

47
Q

Each single covalent bond provides one extra what for each atom

A

One extra shared electron

48
Q

Where does covalent bonding happen?

A

It happens in compounds of non-metals and in non-metal elements

49
Q

What are the different ways of drawing covalent bonds?

A

Dot and cross diagrams
Displayed formula
3D model

50
Q

Hydrogen atoms have just one electron. How many more do they need to complete the first shell?

A

One so they often form single covalent bonds either with other hydrogen atoms or with other elements

51
Q

How many more electrons does each chlorine atom need to complete the outer shell?

A

Just one so two chlorine atoms can share one pair of electrons and form a single covalent bond

52
Q

How many more electrons does each oxygen atom need to complete its outer shell?

A

Two more so in oxygen gas two oxygen atoms share two pairs of electrons with each other making a double covalent bond

53
Q

How many more electrons does a nitrogen atom need to complete its outer shell?

A

Three more electrons so two nitrogen atoms share thee pairs of electrons to fill their outer shells. This creates a triple bond

54
Q

Substances containing covalent bonds usually have what structures?

A

Simple molecular structures

55
Q

The atoms within the molecules are held together by what?

A

Very strong covalent bonds but the forces of attraction between these molecules are very weak

56
Q

What do you need to do to melt or boil a simple molecular compound?

A

You only need to break the feeble intermolecular forces and not the covalent bonds.

57
Q

Why are the melting and boiling points of simple molecular compounds very low?

A

Because the molecules are easily parted from each other

58
Q

Most molecular substances are what at room temperature?

A

Gases or liquids

59
Q

As molecules get bigger the strength of the intermolecular forces does what?

A

Increase

60
Q

Why does the melting and boiling points increase as molecules get bigger?

A

Because as the strength of the intermolecular forces increase, more energy is needed to break them

61
Q

Why don’t molecular compounds conduct electricity?

A

Because they aren’t charged so there are no free electrons or ions

Chemistry- Paper 1 (2 decks)

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