M2 ,, Bonding And Structure

Question 1

Ionic bonding?

Answer 1

The electrostatic forces of attraction between oppositely charged ions formed by electron transfer

Question 2

Physical properties of ionic compounds?

Answer 2

They have high melting points because there are strong electrostatic attractive forces between the oppositely charged ions in a molecule
When solid it doesn’t conduct electricity because ions are held together tightly in the lattice and cannot move so no charge is conducted
When molten/solution ions are free to move so charge can be carried
Solubility in water is generally good

Question 3

Structure of ionic lattice?

Answer 3

Ions in ionic solids are arranged in giant ionic lattice
Sticks in diagram help show arrangement of ions, but they do not represent ionic bonds

Question 4

What’s covalent bonding?

Answer 4

Strong electrostatic attraction between a shared pair of electrons and the nuclei of the bonded atoms

Question 5

Dative covalent bonding?

Answer 5

Forms when the shared pair of electrons in the covalent bond come from only one of the bonding atoms, also called a co-ordinate bonding

Question 6

Covalent bonding structure?

Answer 6

Simple molecular - with induced dipole-dipole, permanent dipole-dipole forces between molecules

Question 7

Covalent bonding properties?

Answer 7

Bp/Mp is low because of weak intermolecular forces between molecules
Solubility in water is generall poor
Conductivity is low when solid because there’s no ions to conduct and ions are localised
When molten no conductivity cause there’s no ions
Mostly gases and liquids

Question 8

Linear?

Answer 8

2 bonding pairs, no lone pairs
Bond angle 180*

Question 9

Trigonal planar?

Answer 9

3 bonding pairs, 0 lone pairs
Bond angle 120*

Question 10

Tetrahedral?

Answer 10

4 bonding pairs, 0 lone pairs
Bond angle 109.5*

Question 11

Trigonal pyramidal?

Answer 11

3 bonding pairs, 1 lone pair
Bond angle 107*

Question 12

Bent?

Answer 12

2 bonding angles, 2 lone pairs
Bond angle is 104*

Question 13

Octahedral?

Answer 13

6 bonding pairs, 0 lone pairs
90*

Question 14

Define electronegativity?

Answer 14

It is the relative tendency of an atom in a covalent bond in a molecule to attract electrons in a covalent bond to itself

Question 15

Electronegativity across a period?

Answer 15

It increases as the number of protons increase and atomic radius decreases because electrons in the same shell are pulled in more

Question 16

Electronegativity down a group?

Answer 16

Decreases down a group because the distance between the nucleus and the outer electrons increases and the shielding of inner shell electrons increases

Question 17

Polar covalent bond?

Answer 17

It forms when the elements in the bond have different electronegativities, has dipole ends

Question 18

Symmetric molecules?

Answer 18

Will not be polar even if individual bonds are polar (co2)