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Chemistry > Bondings > Flashcards

Bondings Flashcards

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1
Q

When does ionic bonding happen and how ?

A

With metal + non-metal
When atoms lose or gain electrons

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2
Q

What does ionic bonding form

A

Giant ionic lattice by strong electrostatic forces of attraction

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3
Q

What are the properties of ionic bonding

A
  • Cannot conduct electricity when solid as ions are fixed and connot move but when dissolved in water it can
  • Soluble
  • Extremely high melting and boiling points due to strong attraction between ions
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4
Q

Why can’t ionic compunds conduct electricity when solid

A

Ions cannot move they are locked together by strong electostatic forces of attraction

And in water they are free to move

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5
Q

Properties of metallic bonding

A
  • Do conduct electricity
  • high melting point as electrons are very strong
  • insoluble in water
  • carry electrical currents and thermal energy
  • electrostatic attractions hold everything together
  • Sea of delocalised electrons
    *shiny
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6
Q

Metallic bonding

A

The electrons of the outer shell of the metal atom are delocalised (free to move around). There are strong forces of electrostatic attraction between the positive metal ions and the shared negative electrons.

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7
Q

What is covalent bonding?

A

A covalent bond is a strong bond that forms when a pair of electrons is shared between two atoms

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8
Q

Giant covalent

A

In giant covalent structures, all the atoms are bonded to each other by strong covalent bonds.

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9
Q

Properties of giant covalent

Examples

A
  • Very high melting and boiling points as lots of energy is needed to break bonds
  • don’t conduct electricity as they don’t contain charged particles apart from graphite or graphene
  • Every atom is connected bt strong covalent bonds
  • They are always solid at room temperature
  • They aren’t soluable in water

Diamond, Graphite and silicon dioxide

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10
Q

Simple covalent bonds

A

They have a small and fixed number of atoms

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11
Q

Examples of simple covalent bonds

A

Hydrogen
Hydrogen chloride
Water
Oxygen
Methane (co2+H)
Carbon dioxide

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12
Q

Properties of small covalent bonds

A
  • Low melting and boiling points because molecules are easily parted from each other
  • Usually gases or liquids at romm temperature
  • They all boil below room temperature
  • Does not conduct electricity because the molecules do not have any free electrons and an overall electric charge
  • Strong covalent bonds but weak intermolecular forces so not engough energy to keep bonds togather when boiling so not much energy is needed for covalent molecules to go from liquid to gas
  • If the molecule gets bigger so does the the strength of the inter molecular forces so more energy needed
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13
Q

Intermolecular

A

Forces of attraction between molecules

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14
Q

Weak intermolecular forces

A

The weak intermolecular forces between the molecules do not require a lot of energy to break

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15
Q

Diamond

Explain properties and bonding

A

-Diamond is made up by a network of carbon atoms that each form 4 covalent bonds
-Diamonds have high melting points because they have strong covalent bonds so it takes a lot of energy to break them
-They can’t conduct electricity as they have 4 bond so no extra electron to carry charges
-Rigid lattice structure making it really hard
-Can use to strengthen cutting tool

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16
Q

How are polymers made?

A

Polymers are molecules made up of long chains of covalently bonded carbon atoms

They are formed when lots of small molecules called monomers join together

17
Q

Properties of polymers

A

Most polymers are solid at room temperatures and have a high melting point

18
Q

Forces of attraction between polymers

A

The intermolecular forces of attraction happen between polymers molecules are relatively strong so it takes a lot of energy to break these forces

19
Q

Metallic bonding

A

Metalic bonding happens between 2 metals, they have a strong electrostatic forces attraction between the delocalised negative electrons and the positive metal ions
Its structure is a sea of delocalised electrons making a lattice
Metalic bonding is very strong

20
Q

Properties of metals

A

Have metalic bonding so needs lots of enerfy to be broken
Malleable layers of atoms in pure metal can slide over each other
Good conductors of electricity as delocalised electrons carry electrical charge and thermal energy
High melting and boiling points so shiny at room temperature
Sonorous

21
Q

What’s an alloy ?

A

An alloy is a mixture of metals

22
Q

Graphite

Properties

A

-Each carbon atoms only forms 3 covalent bonds creating hexagons
there’s no covalent bonds between layers so weakly bonded therefor they are free to move over each other
-High melting point
-Only three out of 4 outer electrons are used in bonds so each carbon atom has one electron that is delocalised and free to move, so conducts electricity
-Soft and slippery so its ideal as a lubricating material

23
Q

How are ionic bonds formed ?

A

When a metal transfers one or more electrons to a non-metal atom to form two oppositely charged ions and then theses two ions will then be attracted to each other by electrostatic forces forming an ionic bond

24
Q

Why do the charges on ions cancel out?

A

In an ionic compounds, the charges on the ion have to cancel out to leave a overall charge of zero

25
Q

What does ide mean

A

Ionic compounds that are monotomic ions (by itself) - sulfide s2-

26
Q

What does ate mean

A

Ionic compounds made from 3 or more different elements end in -ate
They contain more oxygen

Sulfate s04 ( 2-)

27
Q

What does ite mean

A

mean that it contains oxygen - less oxygen
Sulfite - s03 (2-)

28
Q

What is graphene?

A

A single layer of graphite
It is one atom thick making it a two dimentional substance
Its a sheet of carbon atoms joined together in hexagons

A type of fullerene

29
Q

Properties of graphene

A

An excellent conductor of electricity because it has delocalised electrons which are free to move around

30
Q

What is fullerene?

Properties

A

Fullerenes are molecules of cabon atoms with hollow shapes (balls)
They usually have a hexagonal rings of carbon atoms but they can also have 5 or 7 rings
They can be used to cage other molecules. The fullerene structure forms around other atoms or molecule which is then trapped inside,

31
Q

What can fullerene be used for

A

Pharmaceutical delivery, lubricants and catalysts

Carbon nanotubes have high tensile strength (can be streched) and good conductors of electricity

Chemistry (18 decks)

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