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Chem 4th year > Atomic Structure And Bonding > Flashcards

Atomic Structure And Bonding Flashcards

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1
Q

Element

A

Made up of only one type of atom

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2
Q

Compound

A

Contains more than one type of atom held together by bonds

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3
Q

Proton

A

+1
1
Nucleus

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4
Q

Neutron

A

0
1
Nucleus

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5
Q

Electron

A

-1
1/1836
Shells

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6
Q

Mass number

A

Protons and neutrons

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7
Q

Atomic number

A

Protons

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8
Q

Isotope

A

Atoms of the same element which have the same atomic number but a different mass number

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9
Q

Relative atomic mass

A

The average mass of an atom of an element compared to 1/12 of the mass of a carbon -12 atom

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10
Q

Ar

A

(Mass of atom 1 x%) + (mass of atom 2 x%)
Divided by
Total number of atoms

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11
Q

Noble gases

A

They are unreactive because they have full outer shells

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12
Q

Ionic bonding

A

Metal and non metal react
Metals form positive ions
Non metals form negative ions
Opposite charged ions are electrostatically attracted to each other
Giant lattice is formed

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13
Q

Covalent bonding

A

Atoms share a pair of electrons and the shared electrons are attracted to both nuclei

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14
Q

When can ionic compounds conduct electricity

A

Cannot conduct electricity when solid because ions are fixed
Can conduct electricity when in aqueous or molten solution because ions are free to move and carry charge

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15
Q

Why do ionic compounds have high melting and boiling points

A

They have strong electrostatic attraction between the ions and a lot of energy is required to break them apart

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16
Q

Why do simple covalent molecules have low melting and boiling points

A

They have weak intermolecular forces and not a lot of energy is needed to overcome these forces

17
Q

Why do simple covalent molecules not conduct electricity

A

They have no charged particles free to move

18
Q

Diamond

A

Giant covalent structure
Each carbon atom is bonded to 4 other carbon atoms
Tetrahedral shape

19
Q

Why does diamond have a high melting and boiling point

A

It has many strong covalent bonds and a lot of energy is required to break these bonds

20
Q

Why does diamond not conduct electricity

A

It has no free charged particles

21
Q

Why is diamond very hard

A

It is a giant covalent lattice

22
Q

What is diamond used for

A

Cutting tools
Jewellery

23
Q

Graphite

A

Giant covalent structure
Each carbon atom is bonded to 3 other carbon atoms
Layers of hexagon

24
Q

Why does graphite have a high melting and boiling point

A

It has many strong covalent bonds and lots of energy is needed to break these bonds

25
Q

Why does graphite conduct electricity

A

The free delocalised electrons are free to move

26
Q

Why is graphite quite soft

A

There are weak forces of attraction between layers of carbon atoms

27
Q

What is graphite used for

A

Lubricant
Pencil
The free electrons allow the layers to slide over each other

28
Q

C60 Fullerene

A

Simple molecule
Each carbon atoms is bonded to 3 other carbon atoms
Spherical molecule with 60 carbons

29
Q

Why does C60 Fullerene have a low melting and boiling point

A

There are weak intermolecular forces so it does need much energy to break these forces

30
Q

Why does C60 Fullerene not conduct electricity

A

The delocalised electrons have to stay within the molecule and cannot move from one molecule to the other

31
Q

Metal definition

A

Strong electrostatic attraction between positive metal ions and a sea of delocalised electrons
Giant metallic lattice

32
Q

Why do metals have a very high melting and boiling point

A

It is a giant lattice with strong electrostatic attraction between the positive metal ions and sea of delocalised electrons and a lot of energy is needed to break bonds and overcome forces

33
Q

Why are metals malleable

A

The delocalised electrons allow the layers of metal ions to slide over each other

34
Q

Alloy

A

Mixture or atleast 2 elements where one of these is a metal

Chem 4th year (1 decks)

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