Bonding Structures

Question 1

Giant Covalent: Examples of Giant Covalent Structure?

Answer 1

2 examples of Giant covalent structures: Diamond & Graphite.

Question 2

Giant Covalent: What is a allotrope?

Answer 2

materials both different types of the physical form of another. For example Carbon.

Question 3

Giant Covalent: Both Diamond and Graphite are both allotropes of carbon, meaning?

Answer 3

they are both different types of the physical form of Carbon.

Question 4

Giant Covalent: Structure of Diamond?

Answer 4

Giant covalent lattice of carbon atoms. Each Carbon atom is bonded to 4 others which tetrahedrally surround the atom.

Question 5

Giant Covalent: Structure of Graphite?

Answer 5

Arranged in layers of atoms. Each carbon atom is joined to 3 others, leaving one outer shell electron on each carbon is free to move and able to carry the current. Therefore, they are able to conduct electricity.

Question 6

Giant Covalent: Why is Graphite weak?

Answer 6

There are weak forces between the layers of atoms. They are able to slide over each other and therefore able to act as a lubricant.

Question 7

Giant Covalent: Why is Diamond hard?

Answer 7

Diamond is very hard as there are many bonds within the substance. It is the hardest natural substance and is often used in drilling.

Question 8

Giant Covalent: Why is Graphite and Diamond so hard?

Answer 8

They have a high melting point as a large amount of heat energy is needed to break their bonds. Down to the strong giant covalent bonds.

Question 9

Covalent: Define Covalent Bonding?

Answer 9

When an atom shares one or more pairs of electrons between atoms to obtain the electronic configuration of a noble gas.

Question 10

Covalent: Covalent bonds appear in ….

Answer 10

Covalent bonds appear in non-metals and create molecules.They can even appear in atoms of the same element, H2.

Question 11

Covalent: What do Molecules look like for Covalent Bonds?

Answer 11

Two or more atoms chemically bonded together. The covalently bonded atoms are held together by strong attraction between the bonding pair of electrons and the nuclei of the atoms.

Question 12

Covalent: Covalent bonds can be classified into two groups:

Answer 12

simple molecular structures & giant covalent structures.

Question 13

Covalent: Simple molecular Structures:

Answer 13

They have low melting/boiling points due to the fact that there are weak intermolecular forces of attraction.

Although, they do have strong covalent bonds. Therefore, they need less heat energy to overcome and break the weak bonds.

Some substances sumblime under heating. i.e. They turn directly into a gas from a solid.

Question 14

Covalent: Giant molecular Structures:

Answer 14

Diamond and Graphite,
High melting points
Strong Covalent Bonds. lots of energy needed to overcome them.

Question 15

Ionic Bonding: Define Ionic Bonding?

Answer 15

The transfer of one or more electrons between 1 atom to another.

Question 16

Ionic Bonding: If an atom loses an electron then the atom will form a:

Answer 16

positive ion. This is because there are now more protons than electrons in the atom.

Question 17

Ionic Bonding: If an atom gains an electron, the atom forms a:

Answer 17

negative ion as there are now more electrons than protons in the atom.

Question 18

Ionic Bonding: The charge of an ion is related:

Answer 18

to where the element’s position is in the periodic table.

Question 19

Ionic Bonding: If the element is in Group One than the ion will have a:

Answer 19

1+ charge

Question 20

Ionic Bonding: If the element is in Group Seven than the ion will have a:

Answer 20

1- charge

Question 21

Ionic Bonding: If the element is in Group Three than the ion will have a:

Answer 21

3+ charge

Question 22

Ionic Bonding: If the element is in Group Five than the ion will have a:

Answer 22

3- charge

Question 23

Ionic Bonding: Structure of ionic Bonding?

Answer 23

Ionic crystals are arranged in a 3D lattice structure. They are held together by electrostatic forces of attraction.

Question 24

Ionic Bonding: Ionic Bonding ability to conduct?

Answer 24

Ionic compounds are unable to conduct electricity as a solid due to the fact that there are no free moving electrons that are able to carry the current.

However, if they are in their molten state or in an aqueous solution, then the ions become free to move. (Electrolysis)

Question 25

Ionic Bonding: Boiling/ Melting points?

Answer 25

Ionic compounds have high melting points as there are strong intermolecular electrostatic forces of attraction between the oppositely charged ions. Therefore, a large amount of heat energy is needed to overcome and break the bonds.

Question 26

Ionic Bonding: Boiling/ Melting points: charge?

Answer 26

The higher the charge the higher the melting/boiling point. This is because a greater charge has stronger electrostatic forces of attraction and so need more heat energy to overcome and break the bonds.

Question 27

Metallic Bonding: Structure?

Answer 27

Metals form giant structures in which electrons in the outer shells of the metal atoms are free to move. The metallic bond is the force of attraction between these free electrons and metal ions.

Question 28

Metallic Bonding: Boiling point?

Answer 28

Metallic bonds are strong, so metals can maintain a regular structure and usually have high melting and boiling points.

Question 29

Metallic Bonding: Conducting?

Answer 29

Metals are good conductors of electricity and heat, because the free electrons carry a charge or heat energy through the metal.

Question 30

Metallic Bonding: Used to make things?

Answer 30

The free electrons allow metal atoms to slide over each other, so metals are malleable and ductile.

Question 31

Why Hydrogen chloride has a low boiling point?(2)

Answer 31

IF 2 MARKS ITS EASY!

• Weak forces of attraction
• Between molecules.