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Chemistry > Bonding, equations and formula > Flashcards

Bonding, equations and formula Flashcards

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0
Q

What does bonding do

A

They invole changes in the outermost electron shells of the atom

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1
Q

What are the three types of bonding

A

Ionic, Covalent, Metallic

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2
Q

What is ionic bonding

A

A metal and a non metal bonding

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3
Q

What is covalent bonding

A

2 non metals bonding

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4
Q

What is metallic bonding

A

Two metals bonding

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5
Q

What happens to metals when they react in ionic bonding

A

They lose their outermost electrons to leave a full electron shell. This produces a charged atom/ion with a positive charge called cation. This process is called oxidation.

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6
Q

What happens when non metals react in ionic bonding

A

The non metal gains electrons to achieve a full electron shell. The atom becomes negatively charged and is called an anion. This process is called reduction.

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7
Q

Are the atoms involved in ionic bonding more stable

A

Yes

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8
Q

What happens to the oppositly charged atoms.

A

Millions of pairs attract and form a lattice

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9
Q

What does column 1 show

A

The ions with 1 extra electron

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10
Q

What does column 2 show

A

The elements which have 2 extra atoms

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11
Q

What does column 3 show

A

The elements with 3 extra electrons

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12
Q

What does column 6 show

A

The elements with two electrons missing to achieve a full shell

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13
Q

What does column 7 show

A

The elements which have 1 electron missing to achieve a full shell

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14
Q

What do transition metals show

A

The number of electrons can change

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15
Q

What is a complex ion

A

A ion made out of more than 1 element

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16
Q

Simple ions

A

Ions only made of 1 type of atom

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17
Q

When working out formulae, when would you use brackets

A

In compound ions

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18
Q

How would you balance equations

A

Count the number of atoms on each side. And add big numbers before a compound to change it. Never change the small numbers in a compound

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19
Q

Covalent bonding

A

Two non metals share pairs of electrons

Strong attraction between bonding pair of electrons and nuclei

20
Q

Metallic bonding

A

Metals are held together by metallic bonding
All electrons are delocalised
Attraction between positive ions and electrons

21
Q

Giant ionic structure characteristics

A 
Crystalline
High melting point and boiling point 
Brittle
Soluble in water
Do not conduct electricity when solid
Electrolyte
22
Q

Crystalline

A

Regular arrangement of lattice

Crystals can be seen by microscope

23
Q

High melting and boiling point

A

Strong electrostatic forces

Large amount of energy needed to overcome them

24
Q

Brittle

A

Distorted crystal will bring together like ions, repel and split crystal

25
Q

Soluble in water

A

Electrostatic forces in water overcome electrostatic forces in ion
H+ and -
O2- and +

26
Q

Insulator of electricity

A

No free electrons

27
Q

Electrolyte

A

Ions are free to move

28
Q

Simple molecule characteristics

A 
Solid, liquid or gas with low melting point
Strong covalent bonds
Insulator
Non electrolyte
Soluble in organic solvents
29
Q

Low melting point

A

Small amount of energy breaks weak intermolecular bonds

30
Q

Insulators

A

No free delocalised electrons that can move aroun

31
Q

Not soluble in water unless reacted with

A

Covalent molecules are not attracted to water molecules enough to break intermolecular forces

32
Q

Soluble in organic solvents

A

Solvent molecules are stronger than covalent compounds and break them apart

33
Q

Giant covalent structure

A

Diamond, graphite

34
Q

Diamond

A 
Attached to 4 ions
No intermolecular forces
High melting point
Hard
Insulator
Insoluble in water
35
Q

Graphite

A 
Attached to 3 other ions
Free delocalised electrons
Weak intermolecular forces
High melting point
Soft and slippery
Conductor
Insoluble in water
36
Q

High melting point

A

Strong covalent bonds have to be overcome by lots of energy

37
Q

Hard

A

No intermolecular forces

Strong covalent bonds

38
Q

Soft and slippery

A

Layers of weak intermolecular forces broken easily

39
Q

Insulator

A

No free electrons

40
Q

Conductor

A

1 free delocalised electrons per carbon atom

41
Q

Insoluble in water

A

Covalent bonds too strong

42
Q

Metallic bonding

A

High melting and boiling points
Conductors of heat
Malleable
Ductile

43
Q

High melting and boiling point

A

High attraction between ions

Large amount of energy needed to overcome attraction

44
Q

Conductors of heat

A

Delocalised electrons move through lattice

45
Q

Malleable, ductile

A

Electron can take shape of object
Electrostatic forces keep metal together
Ions move in layers by sliding over each other

46
Q

Uses of diamond

A

Cutting

47
Q

Uses of graphite

A

Lubrication

Chemistry (14 decks)

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