Bonding and structures

Question 1

What is a covalent bond?

Answer 1

When two or more atoms share pairs of electrons

Question 2

With which atoms do covalent bonds form?

Answer 2

Two non-metals

Question 3

What type of bonding forms between two oxygen atoms?

Answer 3

Double covalent bonds

Question 4

What type of bonding forms between two nitrogen atoms?

Answer 4

Triple covalent bonds

Question 5

Why do non-metals form covalent bonds?

Answer 5

To complete their outer energy shell

Question 6

Are covalent bonds strong or weak ?

Answer 6

Very strong

Question 7

What are the two types of substances that can be made from covalent bonds?

Answer 7

Simple molecular substances and giant covalent structures

Question 8

What are the characteristics of a simple covalent molecule?

Answer 8

• Only NON-METAL atoms
• Strong bonds IN molecules
• Weak forces BETWEEN molecules
• When broken heated, molecules are not split apart so low boiling point
• Varied Solubility
• Poor Conductor

Question 9

In simple covalent molecules, what allows them to have a low boiling point?

Answer 9

Weak intermolecular forces of attraction require little energy to be broken

Question 10

What are most simple molecular molecules at room temperature?

Answer 10

Gases or liquids

Question 11

Learn these examples of simple covalent molecules

Answer 11

Chlorine
Oxygen
Water

Question 12

What are the properties of giant covalent structures?

Answer 12

• Only NON-METALS
• High Melting Point
• Insoluble in Water
• Poor Conductor

Question 13

What is the only exception to the property that giant covalent structures are poor conductors?

Answer 13

Graphite, free electron can carry a charge

Question 14

Properties of graphite

Answer 14

• 3 Bonds per Carbon
• Free Electrons
• Layers which make it soft and slippery
• Conductor

Question 15

Diamond

Answer 15

• 4 Bonds per Carbon
• No Free Electrons
• Hard
• Not a Conductor

Question 16

Main use of graphite

Answer 16

Lubricant, as layers slide over eachother

Question 17

What do ionic bonds form between?

Answer 17

Metals and non-metals

Question 18

In ionic bonding electrons are transported where?

Answer 18

From the metal atoms to the non-metal atoms

Question 19

What do metals become in ionic bonding?

Answer 19

Positively charged ions

Question 20

What is the electronic configuration of a ion in a ionic bond?

Answer 20

Full outer energy level (like a noble gas)

Question 21

Where on a ionic bond diagram does the charge and amount of atoms appear?

Answer 21

Top right

Bottom right

Question 22

What is ionic bonding?

Answer 22

Strong electrostatic attraction between oppositely charge ions

Question 23

Are ionic compounds soluble?

Answer 23

Yes

Question 24

What colour are most ionic compounds?

Answer 24

White

Question 25

What colour are group 1/2 ionic compounds?

Answer 25

Always White

Question 26

What does the formula of a giant structure show?

Answer 26

Fixed ratio of different elements

Question 27

Do ionic compounds conduct electricity when molten or in an aqueous solution?

Answer 27

Yes

Question 28

What are the melting and boiling points of ionic compounds?

Answer 28

Relatively high

Question 29

Ionic bonding always forms what type of compound?

Answer 29

Giant ionic structure

Question 30

Giant ionic structure

Answer 30

- High Melting Point - Soluble in Water - Conductor - Lattice structure

Question 31

How do giant ionic structures form into lattice?

Answer 31

Held together by the attraction between oppositely charged ions

Question 32

Why do ionic structures have high melting and boiling points?

Answer 32

The electrostatic attraction between oppositely charged ions is very strong, therefore a lot of energy is needed to break them apart

Question 33

What affects the strength of ionic bonding?

Answer 33

The stronger the charge, stronger forces of attraction occur E.g 2+ and 2- ions are stronger than 1+ and 1-ions

Question 34

What are ionic structures made from?

Answer 34

Crystals

Question 35

Metals

Answer 35

- have high melting points - are good conductors of heat and electricity - are hard and dense - malleable - ductile

Question 36

Describe metallic bonding

Answer 36

Positive ions in a lattice, surrounded by a sea of delocalised electrons

Question 37

What does metallic bonding allow metals to be?

Answer 37

Malleable, ductile, and very conductive

Question 38

How does metallic bonding enable metals to be conductive?

Answer 38

Delocalised electrons carry charge around the molecule

Question 39

Why does the metallic structure allow metals to be malleable?

Answer 39

Layers can slide over each other, still stuck together because of "electron sea"

Question 40

Properties of buckminsterfullerene

Answer 40

"Bucky ball" - 60 carbon atoms - arranged in a hollow sphere

Question 41

What is a fullerene?

Answer 41

Group of allotropes of carbon which are in the form of cages