Bonding

Question 1

What are the three types of bonding?

Answer 1

Ionic, Covalent and Metallic

Question 2

What is the definition for Ionic bonding?

Answer 2

An Ionic bond is an electrostatic attraction between positive and negative (metal and non-metal) ions in a lattice.

Question 3

What is an Ionic lattice?

Answer 3

An Ionic lattice is made up of alternating positive and negative ions, they are held together with ionic bonds and the arrangement forms a giant ionic lattice structure.

Question 4

What are some properties of Ionic lattices?

Answer 4

Ionic lattices have high boiling points.
Ionic lattices are soluble in water.
Ionic lattices conduct electricity as liquid or aqueous.
Ionic lattices are hard and brittle.

Question 5

What is the definition for Covalent bonding?

Answer 5

A covalent bond is a shared pair of electrons (which are attracted to the nuclei in each atom).

Question 6

What are some properties of Covalent Compounds?

Answer 6

Covalent compounds usually have low melting and boiling points (Due to weak intermolecular forces).
Covalent compounds cannot usually conduct electricity.
Covalent compounds are not usually soluble in water (There are no charged particles that can move around freely).

Question 7

What is a Dative Covalent bond?

Answer 7

Where one of the atom’s when bonding instead of trading electrons, it donates two.

Question 8

What are some Giant Structures?

Answer 8

Covalent: Diamond, Ice, Graphite, Iodine
Metallic: Magnesium
Ionic: Sodium Chloride

Question 9

What are some properties of Metal?

Answer 9

Metal has a high melting point (It has high electrostatic forces holding the bonds together so lots of energy is needed to overcome this).
Metal has high density.
Metal can conduct electricity and thermal energy.
Metal is malleable / ductile (There are no rigid bonds between lattice layers, so atoms can slide when forces applied).

Question 10

What is the electron pair repulsion theory?

Answer 10

Electron pairs repel each other and arrange themselves in space to minimise repulsion by being as far apart as possible.

Question 11

What is the shape of an atom with 2 electrons?

Also what is it’s bond angles?

Answer 11

Linear

180Degrees

Question 12

What is the shape of an atom with 3 electrons?

Also what is it’s bond angles?

Answer 12

Trigonal Planar

120Degrees

Question 13

What is the shape of an atom with 4 electrons?

Also what is it’s bond angles?

Answer 13

Tetrahedral

109.5Degrees

Question 14

What is the shape of an atom with 5 electrons?

Also what is it’s bond angles?

Answer 14

Trigonal Bipyramidal

120Degrees and 90Degrees

Question 15

What is the shape of an atom with 6 electrons?

Also what is it’s bond angles?

Answer 15

Octohedral

90Degrees

Question 16

What is the definition of ​​Electronegativity​?

Answer 16

​​The power of an atom to attract the electron density in a covalent bond towards itself.

Question 17

What is the Pauling Scale?

Answer 17

It is used to measure electronegativity on a scale of 0 - 4, the larger the number the more electronegative the atom.

Question 18

What factors affect electronegativity?

Answer 18

Nuclear Charge.
Distance between the nucleus and the outer shell.
Shielding.

(Large nuclear charge have greater attraction for the bonding of electrons.)
(Small atoms bond closer to the nucleus so they have more electronegativity.)
(Less shielding means there is greater attraction between the nucleus and the bonding electrons.)

Question 19

What are the periodic trends of electronegativity?

Answer 19

Across a period​:
Electronegativity increases​
Same shielding, decreasing atomic radius and increasing nuclear charge.

Down a group​:
Electronegativity decreases:
Shielding and distance from nucleus increases