Bonding

Question 1

What are the three types of bonding?

Answer 1

1. Ionic bonding
2. Covalent bonding
3. Metallic bonding

Question 2

What is ionic bonding?

Answer 2

Ionic bonding is when a metal bond with a non-metal. It is the transfer of electrons from metals outer shell to the non-metals outer shell. Both forms ions and form an ionic compound.

Question 3

What is covalent bonding?

Answer 3

Covalent bonding is when 2 non-metals bond together by sharing a pair of electrons. As both need to gain electrons.

Question 4

What is metallic bonding?

Answer 4

Metallic bonding is the bond of 2 metal atom together. The metal atoms bond by releasing the electrons on their outer shell. This means there are localized electrons around the atoms.

Question 5

What are ionic compounds?

Answer 5

Ionic compound is a giant lattice structure of ions. The ions are held together by strong electrostatic forces of attraction between oppositely charged ions. They are solid at room temperature.

Question 6

What are the properties of ionic structures?

Answer 6

1. Ionic structures have a high melting and boiling point because the ionic bond or the electrostatic attraction holding the ions together are strong and requires a large amount of energy in order to be broken.
2. Ionic compounds can conduct electricity when it is melted or dissolved. As electricity is the movement of charged particles moving through. So, in liquid forms the ions become free to move.
3. Ionic compound can dissolve in water. As the water particles can break the ionic bond and dissolve the compound.

Question 7

What is simple covalent bond?

Answer 7

Simple covalent bond is when only one pair of electrons are shared between the non-metals. So, one electron from each atom.

Question 8

What is double covalent bond?

Answer 8

Double covalent bond is when two pairs of electrons share between the non-metal atoms. Which means 2 electrons from each atom.

Question 9

What is moving when ionic compound conduct electricity?

Answer 9

When ionic compound conduct electricity it is the ions (charged atoms) that are moving.

Question 10

What is holding the ionic compound together?

Answer 10

Electrostatic force of attraction holds the positive and negative ions together.

Question 11

What are simple covalent molecules?

Answer 11

Simple covalent molecules are molecules with only a few non-metals bonded together.

Question 12

Describe the properties of a simple covalent molecules

Answer 12

• low boiling and melting point as in the molecule there is weak inter-molecular forces holding between the covalent molecules. When, we are melting/boiling the covalent bond is not broken, instead the inter molecular forces are. These inter molecular forces are easily broken in low temperature.

2. They are gases at room temperature except for water. As the heat in room temperature is enough energy to break the inter molecular forces, allowing it to be a gas.
3. The simple covalent molecules cannot conduct electricity as the electrons in the outer shell of each non-metal atoms are in the covalent bond. So, there are no charged particles flowing around.

Question 13

What is a giant covalent strucute?

Answer 13

A giant covalent structure is like diamond and graphite that has many covalent bonds.

Question 14

Describe the properties of covalent bond?

Answer 14

1. Giant covalent bond has high melting and boiling point as there are many strong covalent bonds meaning there need to be a great amount of energy to break them.

Question 15

Diamond

Answer 15

Diamond is made up of carbon atoms bonded together by covalent bond. This is the hardest natural molecule as there is thousand of carbon atoms bonded together by covalent bond. Each carbon atom bonds with 4 other carbon atoms in order to have a full outer shell.

Question 16

Properties of Diamond

Answer 16

• Diamond is a form of carbon
• High melting and boiling point
• Cannot conduct electricity as there are no charges flowing through.

Question 17

Graphite

Answer 17

Graphite is another giant covalent structure. It is carbon atom bonded together by covalent. 3 carbon atoms bond per carbon atom.

There will be a spare electron left known as a localized electron.

Question 18

Properties of a graphite

Answer 18

Each carbon atom bonds with 3 other carbon atom.

Have high melting and boiling boiling as there are many covalent bonds presented.

Graphite is soft and slippery as they are in layers. Each layer is held together by weak forces, allowing them to slide through each other.

Graphite can conduct electricity as there is localized electrons flowing around the molecule. Therefore, it can conduct electricity as there is charged particles flowing around.

Question 19

Properties of metallic bonding

Answer 19

Most metals are solid at room temperature except mercury.

Metallic structure have high melting and boiling point as they have strong bonds (force of attraction).

Metallic strucutres conduct electricity as when they are bonded they release the valence electrons (delocatised electrons). These delocalised electrons are free to move meaning they are charged particles moving around, which is known as electricity.

Question 20

What is malleble?

Answer 20

Malleable means it can bend. Pure metals are malleble as it has layers that can slide over.

Question 21

What is an alloy?

Answer 21

An alloy is an metallic substance. They are metals with atoms from other elements added into the structure. The layer of atoms now cannot slid over each other. (not malleable)

Question 22

What is electrostatic attraction?

Answer 22

An electrostatic attraction is a force holding together positive and negative charges.

Question 23

Describe the electrostatic attraction between the 3 bonding?

Answer 23

In ionic structures the electrostatic force is between the positive and negative ions.

In covalent structures the electrostatic force is between the negative electrons attract to the positive in the nucleus.

In metallic structures, the electrostatic attraction is between the positively charged ions and negatively charges electrons.