Bonding, equations and formula

Question 0

What does bonding do

Answer 0

They invole changes in the outermost electron shells of the atom

Question 1

What are the three types of bonding

Answer 1

Ionic, Covalent, Metallic

Question 2

What is ionic bonding

Answer 2

A metal and a non metal bonding

Question 3

What is covalent bonding

Answer 3

2 non metals bonding

Question 4

What is metallic bonding

Answer 4

Two metals bonding

Question 5

What happens to metals when they react in ionic bonding

Answer 5

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.

Question 6

What happens when non metals react in ionic bonding

Answer 6

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.

Question 7

Are the atoms involved in ionic bonding more stable

Answer 7

Yes

Question 8

What happens to the oppositly charged atoms.

Answer 8

Millions of pairs attract and form a lattice

Question 9

What does column 1 show

Answer 9

The ions with 1 extra electron

Question 10

What does column 2 show

Answer 10

The elements which have 2 extra atoms

Question 11

What does column 3 show

Answer 11

The elements with 3 extra electrons

Question 12

What does column 6 show

Answer 12

The elements with two electrons missing to achieve a full shell

Question 13

What does column 7 show

Answer 13

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

Question 14

What do transition metals show

Answer 14

The number of electrons can change

Question 15

What is a complex ion

Answer 15

A ion made out of more than 1 element

Question 16

Simple ions

Answer 16

Ions only made of 1 type of atom

Question 17

When working out formulae, when would you use brackets

Answer 17

In compound ions

Question 18

How would you balance equations

Answer 18

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

Question 19

Covalent bonding

Answer 19

Two non metals share pairs of electrons

Strong attraction between bonding pair of electrons and nuclei

Question 20

Metallic bonding

Answer 20

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

Question 21

Giant ionic structure characteristics

Answer 21

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

Question 22

Crystalline

Answer 22

Regular arrangement of lattice

Crystals can be seen by microscope

Question 23

High melting and boiling point

Answer 23

Strong electrostatic forces

Large amount of energy needed to overcome them

Question 24

Brittle

Answer 24

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

Question 25

Soluble in water

Answer 25

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

Question 26

Insulator of electricity

Answer 26

No free electrons

Question 27

Electrolyte

Answer 27

Ions are free to move

Question 28

Simple molecule characteristics

Answer 28

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

Question 29

Low melting point

Answer 29

Small amount of energy breaks weak intermolecular bonds

Question 30

Insulators

Answer 30

No free delocalised electrons that can move aroun

Question 31

Not soluble in water unless reacted with

Answer 31

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

Question 32

Soluble in organic solvents

Answer 32

Solvent molecules are stronger than covalent compounds and break them apart

Question 33

Giant covalent structure

Answer 33

Diamond, graphite

Question 34

Diamond

Answer 34

``` Attached to 4 ions No intermolecular forces High melting point Hard Insulator Insoluble in water ```

Question 35

Graphite

Answer 35

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

Question 36

High melting point

Answer 36

Strong covalent bonds have to be overcome by lots of energy

Question 37

Hard

Answer 37

No intermolecular forces | Strong covalent bonds

Question 38

Soft and slippery

Answer 38

Layers of weak intermolecular forces broken easily

Question 39

Insulator

Answer 39

No free electrons

Question 40

Conductor

Answer 40

1 free delocalised electrons per carbon atom

Question 41

Insoluble in water

Answer 41

Covalent bonds too strong

Question 42

Metallic bonding

Answer 42

High melting and boiling points Conductors of heat Malleable Ductile

Question 43

High melting and boiling point

Answer 43

High attraction between ions | Large amount of energy needed to overcome attraction

Question 44

Conductors of heat

Answer 44

Delocalised electrons move through lattice

Question 45

Malleable, ductile

Answer 45

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

Question 46

Uses of diamond

Answer 46

Cutting

Question 47

Uses of graphite

Answer 47

Lubrication