CC5-7 Ionic/Covalent Bonding and types of Substance

Question 1

Ionic Bonds

Answer 1

Ionic Bond-Strong electrostatic force of attraction between oppositely-charged ions(Metal and non-metal atoms)
Electrostatic Forces-Forces of attraction between all positively and negatively charged objects
Bonds- Forces of attraction that hold atoms together(can be weak or strong) eg. Noble Gases have stronger, more stable bonds
Cation- Positive Ion(More proton than E)1+
Anion-Negative Ion(More E than P)1-

Question 2

Filling Shells

Answer 2

Group 1- Lose 1 electron to gain outer shell,
Charge on Ion 1+
Group 2-Lose 2 electron to gain outer shell,
Charge on Ion 2+
Group 6- Gain 2 electron to complete outer shell, Charge on Ion 2-
Group 7- Gain 1 electron, charge on Ion 1-

Question 3

Ionic Lattices

Answer 3

Ionic Compounds formed by loss/gain of electrons, held together by strong electrostatic forces between oppositely charged ions.

• These strong ionic bonds allow bilions of ions to be packed together in a regular repeating arrangement called a lattice structure.
• In ionic compounds huge number of ions are arranged in a giant structure or lattice. This has a regular pattern so ionic compounds form crystals.

Question 4

Properties of Ionic compounds

Answer 4

Ionic Compounds have high BP/MPs as a lot of energy is needed to overcome the strong electrostatic forces and separate the oppositely charged ions.

Question 5

Electrical Conductivity

Answer 5

Ionic compounds conduct electricity when they are molten or dissolved in water(aq). They don’t conduct in solid.
In order for a substance to conduct:
-It must contain charged particles
-It must contain delocalised(free) electrons.

Question 6

Covalent Bonds

Answer 6

Covalent Bonds are formed when atoms share electrons
Covalent Bonds are usually formed between non-metal atoms and are produced by sharing pairs of electrons. By forming a C bond atoms become more stable as they have a full outer shell.
-Atoms in molecules are held together by strong electrostatic forces of attraction between the nucleus and E shells.

Question 7

Molecular Compounds

Answer 7

-Compounds contain atoms of more than 1 element, chemically joined together by bonds.
Some compounds exist as molecules-distinct groups of atoms joined by covalent bonds. They have covalent, simple molecular structures.
-Covalent bonds in a water molecule are strong forces of attraction. However there are also weak forces of attraction between molecules-intermolecular forces. These intermolecular forces hold water molecules together and must be overcome when turning liquid water into gas. Small simple molecules such as water often have low melting points and boiling points, as it doesn’t take much energy to overcome the weak intermolecular forces

Question 8

Allotropes of Carbon

Answer 8

Allotropes- Different structural forms of the same element. (The structure and bonding in different allotropes influence their uses eg Graphite and Diamond)
-Carbon can form simple molecules called fullerenes, in which each carbon atom is covalently bonded to 3 other Carbon Atoms.

Question 9

Possible 6 Marker: Compare Diamond and Grpahite

Answer 9

Diamond:
-Giant Covalent Structure
Each Carbon atom joined to 4 other carbon atoms by strong covalent bonds.
-Tetrahedral Structure
-No free electrons
-Used for cutting tools
Graphite:
-Each carbon atoms forms 3 covalent bonds with other carbon atoms
-Hexagonal ring shape
-Used in Lubricants and electrodes

Question 10

Properties of Metals

Answer 10

Metallic Bonding is the strong electrostatic attraction between the positive metal ions and the negative delocalised electrons
-Solids with high MP/BPs
-Shiny
-Malleable
-High density
-Good conductors of electricity
Metals contain delocalised electrons meaning they can conduct electricity and have a current as electrons are free to move

Question 11

Bonding Models

Answer 11

Giant Covalent: Found in a few non-metal eA giant covalent structure is a three-dimensional structure of atoms that are joined by covalent bonds.
Metallic Bonds are the electrostatic attraction between positive metal ions and negative delocalised electrons.