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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

(56 cards)

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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?

Study These Flashcards
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?

Study These Flashcards
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
What bonds hold together atoms of a molecule and what is their structure?
Covenant bonds, simple molecular structure (e.g. water)
26
Why do simple molecular structures have low boiling points?
As they have weak intermolecular forces that don’t need much energy to overcome
27
Why don’t simple molecules not conduct electricity?
As they have no overall charge and so can’t carry an electrical current
28
Why doesn’t the covenant bond itself not allow simple molecules to carry a charge?
As strong forces between -electrons and +nuclei hold electrons in place and can’t flow so can’t carry a current
29
What is a monomer?
A small simple molecule that can be joined in a chain to form a polymer
30
What are polymers?
A chain of covalently bonded carbon atoms
31
Why do longer polymers have higher melting points than shorter ones?
As longer ones have more intermolecular forces between them and the longer chains get tangled with each other
32
What is the definition of an allotrope?
Different structural forms of the same element
33
Describe the structure of fullerenes
Each carbon atom is covelently bonded to 3 others and the structure of molecules are often tubular or spherical
34
Explain the properties of fullerenes
- Low melting points because of weak intermolecular forces | - soft and slippery due to weak intermolecular forces
35
explain the structure of graphene
It’s similar to fullerene but isn’t a simple molecule and consists of sheets of carbon atoms with no fixed formula
36
Explain the properties of fullerenes
- 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
Give two covalent giant molecular structures which are allotropes of carbon
Diamond and graphite
38
Visualise the structure of graphite and diamond
Use page 45 of Pearson active chemistry for answer
39
Explain the properties of graphite
- 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
Why is graphite a layered structure?
As it has 3 covalent bonds to every carbon atom
41
Explain some properties of diamond
- 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
Give some uses of graphite
- 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
Give some uses of diamond
- Used to cut things due to its rigid ness | - electrical insulator as it has no free charged particles
44
Give some common properties of metals
- solids with high melting points - shiny when polished - malleable - high density - good conductors of electricity
45
Give some common properties if non-metals
- solids, liquids or gases with low melting points - not usually shiny(when solid) - brittle (when solid) - low density - poor conductors of electricity
46
What structure do atoms in a metallic element make?
A giant lattice
47
What is metallic bonding?
The electrostatic attraction between positive metal ions and the negative delocalised electrons
48
Why are metals good at conducting electricity?
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
Why are metals malleable?
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
What happens to electrons when a potential difference is applied to two point of a metal?
The electrons will flow towards the positive side as they transfer energy and form a current
51
Aluminium forms A^3+ ions. Why does it have a higher electrical conductivity than sodium?
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
What is the structure of ionic compounds?
Billions of ions held together in a lattice
53
What are the properties of ionic compounds?
- high melting/boiling points - many are soluble in water - conduct electricity when liquid or in a solution
54
What are the properties of simple molecular covalent structures?
- low melting/boiling points - few are soluble in water - most don’t conduct electricity
55
Where are giant covalent structures found?
In some non-metal elements and some compounds of non-metals
56
What is the structure of metallic bonds?
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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