3.1.3 Bonding

Question 1

How does Ionic Bonding occur?

Answer 1

It is the electrostatic attraction between oppositely charged ions in a lattice

Question 2

What is the formula for Sulfate?

Answer 2

SO4 2-

Question 3

What is the formula for Hydroxide?

Answer 3

OH-

Question 4

What is the formula for nitrate?

Answer 4

NO3 -

Question 5

What is the formula for carbonate?

Answer 5

CO3 2-

Question 6

What is the formula for ammonium?

Answer 6

NH4 +

Question 7

What are single and multiple covalent bond ?

Answer 7

A single covalent bond contains a shared pair of electrons

Multiple covalent bond contains multiple pairs of electrons

Question 8

What is a co-ordinate (dative) bond?

Answer 8

It is when both electrons being shared come from the same atom

Question 9

How does metallic bonding work?

Answer 9

It occurs due to attraction between delocalised electrons and positive ions arranged in a lattice

Question 10

What are the four types of crystal structure?

Answer 10

• Ionic
• Metallic
• Macromolecular (giant covalent)
• Molecular

Question 11

Name 3 Giant Covalent structure
and describe their physical properties?

Answer 11

• Diamond (4 carbon bonds = very hard)
• Graphite (3 bonds per carbon, layers slide, conducts electricity)
• Ice (Hydrogen bonds, open lattice

Question 12

Name a simple Molecular structure describe its physical property?

Answer 12

Iodine (weak Van Der Waal forces)

Question 13

Name a giant Metallic structure and describe its physical property?

Answer 13

Magnesium (delocalised electrons, conducts electricity)

Question 14

Name a giant Ionic structure
and describe it physical property?

Answer 14

Sodium Chloride (NA+ ions and Cl- ion conduct electricity when molten)

Question 15

What are Bonding pairs?

Answer 15

Pair of electrons hared with another atom in a covalent bond

Question 16

What are Lone pair of electrons ?

Answer 16

Pair of electrons that are not in a covalent bond and therefore not shared

Question 17

How do Electrons pairs exist?

Answer 17

As electron clouds

Question 18

How are shapes of molecules formed?

Answer 18

The Electron clouds repel against each other causing them to be at angles (Valence-Shell Electron-Pair Repulsion Theory)

Question 19

How do electron clouds minimise the repulsion between each other?

Answer 19

They stay as far apart from each other a possible

Question 20

Rank what type of repulsion creates the biggest angle to the smallest angle?

Answer 20

• Lone pair + Lone pair (biggest angle)
• Bonding pair + Lone pair (second biggest angle)
• Bonding pair + Bonding pair (smallest angle

Question 21

Name the shapes of molecules with 2 electron pairs

Answer 21

Linear

Question 22

Name the shapes of molecules with 3 electron pairs

Answer 22

Trigonal Planar

Question 23

Name the shapes of molecules with 4 electron pairs

Answer 23

• Tetrahedral (no lone pairs)
• Trigonal pyramidal (1 lone pair)
• Bent (2 lone pairs)

Question 24

Name the shapes of molecules with 5 electron pairs

Answer 24

• Trigonal bipyramidal (no lone pairs)
• Seesaw (1 lone pair)
• T-shaped

Question 25

Name the shapes of molecules with 6 electron pairs

Answer 25

- Octahedral (no lone pairs) - Square Planar ( 2 lone pairs)

Question 26

What is Electronegativity?

Answer 26

An atom's ability to attract a pair of electrons in a covalent bond

Question 27

How does polarity in covalent bonds occur?

Answer 27

Due two atoms having different electronegativity one will attract electrons closer to itself making that side of the bond partially negative and the other side partially positive

Question 28

Why are not all molecules with polar bonds form a permanent dipole?

Answer 28

This is because even if though the bonds are polar the overall molecule is non polar because its symmetrical

Question 29

What is a dipole?

Answer 29

A difference in charge between two atoms caused by a shift in electron density

Question 30

What are the 3 intermolecular forces?

Answer 30

- Van Der Waal - Permanent Dipole-Dipole - Hydrogen Bond

Question 31

Rank the 3 intermolecular forces from strongest to weakest

Answer 31

- Hydrogen Bond - Permanent Dipole-Dipole - Van Der Waal

Question 32

How do Intermolecular Forces affect Physical properties of substances?

Answer 32

Boiling and Melting Point is affected by the strength of Intermolecular forces

Question 33

What is the importance of Hydrogen bonds to low density Ice and anomalous boiling points of compounds and what are these substances?

Answer 33

If it wasn't for Hydrogen compounds they would boil at much lower temperatures The substances are H20 (water), NH3 (Ammonia) and HF (Hydrogen fluoride)