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Chemistry > (Topic 2) Bonding, Structure And Properties Of Matter (CGP Book) > Flashcards

(Topic 2) Bonding, Structure And Properties Of Matter (CGP Book) Flashcards

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1
Q

What are ions?

A

Charged particles
Can be single atoms or groups of atoms

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2
Q

When are ions made?

A

When electrons are transferred

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3
Q

Why do electrons transfer?

A

So the atoms can gain a full outer shell leading to a stable atom

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4
Q

What happens when metals form ions?

A

Lose electrons from outer shell to form positive ions

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5
Q

What happens when nonmetals form ions?

A

They gain electrons in their outer shell to form negative ions

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6
Q

What are positive ions known as?

A

Cations

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7
Q

What are negative ions known as?

A

Anions

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8
Q

What happens during ionic bonding?

A

Metal and nonmetal react together
Metal atom loses electrons to form positively charged ion
Nonmetal gains these electrons to form negatively charged ion
These charged ions are strongly attached to one another by electrostatic forces

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9
Q

What do Dot and cross diagrams show?

A

The arrangement of electrons in an atom or ion

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10
Q

What is ionic bonding?

A

Transfer of electrons

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11
Q

What type of structure do ionic compounds have?

A

A giant ionic lattice

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12
Q

How is an ionic compound structured?

A

Ions form are closely packed regular lattice arrangement and there are very strong electrostatic forces of attraction between oppositely charged ions

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13
Q

Properties of ionic compounds?

A

All have high melting points and high boiling points due to strong bonds between ions, it takes a lot of energy to overcome this attraction
When solid, ions are held in place so compounds cannot conduct electricity
When ionic compound melt ions are free to move and carry electric charge
Ionic compounds dissolve in water, the ions separate and are all free to move in the solution so can carry electric charge

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14
Q

What is covalent bonding?

A

Sharing electrons

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15
Q

What happens during covalent bonding?

A

Nonmetal atoms bond together
They share pairs for electrons to make covalent bonds
Positively charged nuclei of the bonded atoms are attracted to the shared pair of electrons by electrostatic forces making covalent bonds very strong
Atoms only share electrons in their outer shells
Each covalent bond provides one extra shared electron for each atom
Each atom involves generally enough covalent bonds to fill up its outer shell

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16
Q

Where does covalent bonding happen?

A

In compounds of nonmetals and in non-metal elements

17
Q

What are simple molecular substances?

A

Made up of molecules containing a few atoms joined together by covalent bonds

18
Q

Examples of simple molecular substances?

A

Hydrogen, chlorine, oxygen, nitrogen, methane, water, and hydrogen chloride

19
Q

Properties of simple molecular substances?

A

Very strong covalent bonds, forces of attraction between these molecules are very weak
Melting and boiling points are very low
Most are gases or liquids at room temperature
As molecules get bigger strength of intermolecular forces increase some more energy is needed to break them so melting and boiling points increase
Do not conduct electricity as they are not charged so no free electrons or ions

20
Q

What are polymers?

A

Long chains of repeating units

21
Q

How are atoms in a polymer joined?

A

By strong covalent bonds

22
Q

Properties of polymers

A

Most are solid at room temperature
Week into molecular forces so have lower boiling points than ionic or giant molecular compounds

23
Q

What are giant covalent structures?

A

Macro molecules

24
Q

How are atoms bonded in giant covalent structures?

A

By strong covalent bonds

25
Q

Properties of giant covalent structures?

A

Very high high melting and boiling points as lots of energy energy needed to break covalent bonds
Don’t contain charged particles so do not conduct electricity

26
Q

Examples of giant covalent structures?

A

Diamond, graphite and silicon dioxide

27
Q

How is Diamond structured?

A

Each carbon atom forms four covalent bonds in a very rigid giant covalent structure

28
Q

How is graphite structured?

A

Each carbon atom forms three covalent bonds to create layers of hexagons
Each carbon atom also has one delocalised electron

29
Q

What are allotropes?

A

Different structural forms of the same element in the same physical state

30
Q

Properties of diamond?

A

Very hard
A lot of energy needed to break covalent bonds so has a very high melting point
Does not conduct electricity as has no free electrons

31
Q

Properties of graphite?

A

No covalent bonds between layers so only held together weakly, meaning they are free to move all each other, making it soft and slippery
High melting point as covalent bonds in the layers need lots of energy to break
Each carbon atom has one electron that is the localised graphite can conduct electricity and thermal energy

32
Q

What is graphene?

A

One layer of graphite
The shade of carbon atoms joint together in hexagons
The sheet is one atom thick making it a 2D substance

33
Q

Properties of graphene?

A

Covalent bonds make it very strong
Incredibly light
Contains delocalised electrons so can conduct electricity throughout the whole structure

34
Q

What are fullerenes?

A

Molecules of carbon shaped like closed tubes or hollow balls

35
Q

Uses of fullerenes?

A

The cage structure can be used to another atom or molecule, this could be used to deliver a drug into the body
Have a huge surface area, so make great catalysts
Lubricants

36
Q

What are nano tubes?

A

Tiny carbon cylinders

37
Q

Properties of nano tubes?

A

Can conduct electricity and thermal energy
Have high tensile strength

38
Q

Uses of nano tubes?

A

Electronics or strengthen materials without adding much weight

Chemistry (9 decks)

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