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Chemistry Gcse > ⭐️SC5, SC6, SC7, Ionic, Covelant Bonding And Substance Types > Flashcards

⭐️SC5, SC6, SC7, Ionic, Covelant Bonding And Substance Types Flashcards

1
Q

What are bonds?

A

Forces of attraction that hold atoms together

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2
Q

Why do atoms form ions?

A

To gain a full out shell by gaining or loosing electrons

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3
Q

What is a cation?

A

A positive ion

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4
Q

What’s an anion?

A

A negative ion

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5
Q

What is the force of attraction between positive an negative ions?

A

Electrostatic forces of attraction

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6
Q

What is an ionic bond?

A

The electrostatic forces of attraction between oppositely charged ions

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7
Q

What will atoms that easily form ions have?

A

A nearly full or near,y empty outer shell of electrons

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8
Q

What do ionic compounds often form as solids and why?

A

Crystals due to their regular lattice structure

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9
Q

What structure do ionic compounds always have?

A

A regular giant ionic lattice structure

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10
Q

What properties do ionic compounds have?

A
  • high melting and boiling points
  • don’t conduct electricity as a solid as ions are fixed
  • easily dissolve in water
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11
Q

When will an ionic compound conduct electricity?

A

as an aqueous solution or as a liquid as the ions become free to move and carry a charge

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12
Q

Which ionic compounds have higher melting points than the rest?

A

Ions with higher charges as it takes more energy to overcome the electrostatic forces of attraction

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13
Q

What former covenant bonds?

A

Non metal atoms by sharing a pair of electrons

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14
Q

What holds together atoms in a molecule?

A

Covenant bonds with strong electrostatic forces of attraction between the positive nuclei and negative electrons in the bonded atoms

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15
Q

What kind of forces are there between molecules?

A

Weak forces of attraction

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16
Q

How big are atoms?

A

Around 10^-10 meters in diameter

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17
Q

What is the valency of an element?

A

The number of covenant bonds formed by atoms of different elements

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18
Q

How do you find the valency of an element?

A

By finding the number of electrons needed to obtain a complete full outer shell

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19
Q

What’s the valency of Si?

A

4

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20
Q

What’s the valency of F?

A

1

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21
Q

What are the positives and negatives of 2D representation models

A

+ show what atoms the substance contains and and how atoms are connected
-don’t show the shape of the substance, or size of atoms

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22
Q

What are the positives and negatives of dot and cross diagrams?

A

+ where the electrons un the bonds or ions came from

-don’t show the size of the atom/ion or how it’s arranged

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23
Q

What are the positives and negatives of 3D models?

A

+show the arrangement of ions

-only show outer layer of substance - electrons can’t be seen

24
Q

What are the positives and negatives for the ball and stick model?

A

+help to visualise structures by showing the shape of the lattice in 3D, more realistic than 2D drawings

-make it look like there’s a big gap between atoms when really this is where electron shells interact, they don’t show correct scales of atoms or ions

25
Q

What bonds hold together atoms of a molecule and what is their structure?

A

Covenant bonds, simple molecular structure (e.g. water)

26
Q

Why do simple molecular structures have low boiling points?

A

As they have weak intermolecular forces that don’t need much energy to overcome

27
Q

Why don’t simple molecules not conduct electricity?

A

As they have no overall charge and so can’t carry an electrical current

28
Q

Why doesn’t the covenant bond itself not allow simple molecules to carry a charge?

A

As strong forces between -electrons and +nuclei hold electrons in place and can’t flow so can’t carry a current

29
Q

What is a monomer?

A

A small simple molecule that can be joined in a chain to form a polymer

30
Q

What are polymers?

A

A chain of covalently bonded carbon atoms

31
Q

Why do longer polymers have higher melting points than shorter ones?

A

As longer ones have more intermolecular forces between them and the longer chains get tangled with each other

32
Q

What is the definition of an allotrope?

A

Different structural forms of the same element

33
Q

Describe the structure of fullerenes

A

Each carbon atom is covelently bonded to 3 others and the structure of molecules are often tubular or spherical

34
Q

Explain the properties of fullerenes

A
  • Low melting points because of weak intermolecular forces

- soft and slippery due to weak intermolecular forces

35
Q

explain the structure of graphene

A

It’s similar to fullerene but isn’t a simple molecule and consists of sheets of carbon atoms with no fixed formula

36
Q

Explain the properties of fullerenes

A
  • lightest known material as each sheet is one atom thick
  • good electrical conductor as it allows free electrons to move across its surface
  • it’s very strong due to covelant bonds
37
Q

Give two covalent giant molecular structures which are allotropes of carbon

A

Diamond and graphite

38
Q

Visualise the structure of graphite and diamond

A

Use page 45 of Pearson active chemistry for answer

39
Q

Explain the properties of graphite

A
  • has high melting point due to many covenant bonds that must be broken
  • conducts electricity due not all electrons being held in covalent bonds giving allowing delocalised electrons to freely move and carry a charge
40
Q

Why is graphite a layered structure?

A

As it has 3 covalent bonds to every carbon atom

41
Q

Explain some properties of diamond

A
  • has high melting point as it’s got many strong covalent bonds
  • very hard due to the 4 covalent bonds to every carbon atoms giving it a tetrahedral arrangement
  • doesn’t conduct electricity as all electrons are strongly held in place with covalent bonds
42
Q

Give some uses of graphite

A
  • Used as a lubricant as each sheet is held by weak intermolecular forces allowing the layers to slide past each other
  • used in electrodes as it conducts electricity well
43
Q

Give some uses of diamond

A
  • Used to cut things due to its rigid ness

- electrical insulator as it has no free charged particles

44
Q

Give some common properties of metals

A
  • solids with high melting points
  • shiny when polished
  • malleable
  • high density
  • good conductors of electricity
45
Q

Give some common properties if non-metals

A
  • solids, liquids or gases with low melting points
  • not usually shiny(when solid)
  • brittle (when solid)
  • low density
  • poor conductors of electricity
46
Q

What structure do atoms in a metallic element make?

A

A giant lattice

47
Q

What is metallic bonding?

A

The electrostatic attraction between positive metal ions and the negative delocalised electrons

48
Q

Why are metals good at conducting electricity?

A

Because their outer shell electrons are lost from each atom. This leaves a giant lattice of positive metal ions surrounded by a sea of delocalised electrons

49
Q

Why are metals malleable?

A

As when a metal is hit, the layers of ions slide over each other and the sea of delocalised electrons hold the ions together so the metal changes shape without breaking

50
Q

What happens to electrons when a potential difference is applied to two point of a metal?

A

The electrons will flow towards the positive side as they transfer energy and form a current

51
Q

Aluminium forms A^3+ ions. Why does it have a higher electrical conductivity than sodium?

A

As magnetism forms the Mg 2+ ion and so doesn’t contribute as many electrons to the sea of delocalised electrons as Al 3+ does which has 3 electrons to contribute

52
Q

What is the structure of ionic compounds?

A

Billions of ions held together in a lattice

53
Q

What are the properties of ionic compounds?

A
  • high melting/boiling points
  • many are soluble in water
  • conduct electricity when liquid or in a solution
54
Q

What are the properties of simple molecular covalent structures?

A
  • low melting/boiling points
  • few are soluble in water
  • most don’t conduct electricity
55
Q

Where are giant covalent structures found?

A

In some non-metal elements and some compounds of non-metals

56
Q

What is the structure of metallic bonds?

A

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

Chemistry Gcse (24 decks)

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