bonding and structure

Question 1

ionic bonding

Answer 1

electrostatic force of attraction between opposite charged ions
between non metal and metal

Question 2

ionic bonding properties

Answer 2

• stronger
• high MP (strong electrostatic forces between opposite charged ions in lattice)
• dont conduct electricity (no delocalised e-) but CAN conduct if MOLTEN OR DISSOLVED in h20
  -soluble in aq solvents
• regular patter giant ionic lattice

Question 3

covalent bonding

Answer 3

strong electrostatic attraction between shared pair of e- and nuclei of bonded atoms

Question 4

dative covalent bonding

Answer 4

forms when shared pair of electrons in covalent bond come from only one of bonding atoms

Question 5

ionic : bonding + structure

Answer 5

B: electrostatic force between opposite charge ions
s: giant ionic lattice
eg. sodium chloride, mg oxide

Question 6

covalent

Answer 6

B : shared pair of electrons
s: simple molecular (with intermolecular forces/ induced dipole-dipole) between molecules
eg co2 h20

Question 7

properties of giant ionic + simple molecular

Answer 7

giant:
- high BP+MP (due to strong electrostatic forces)
- soluble mostly
-can conduct electricity when molten/dissolved
- are crystalline solids

simple:
- low MP +BP (due to weak intermolecular forces)
- insoluble
- cant conduct electricity
- mostly gases/liquids

Question 8

electronegativity

Answer 8

relative tendency of an atom in a covalent bond to attract e- in covalent bond

Question 9

factors affecting electronegativity

Answer 9

• INCREASE ACROSS PERIOD (no of P increase , nuclear charge increase + atomic radii decreases (e- pulled in more)
• DECREASE DOWN A GROUP (shielding increases + nuclear charge increases + atomic radii increases)

Question 10

formation of permanent dipole (polar covalent) bond

Answer 10

forms when elements in bond have DIFFERENT electronegativities
unsymmetrical
when bond is polar covalent = has unequal distribution of e- in bond so produces a charge separation

Question 10

ionic compounds

Answer 10

have very large electronegativity difference

Question 10

induced dipole dipole aka LONDON FORCESSSS

Answer 10

occur between ALL simple covalent molecules
due to e- moving at high speeds in orbitals.
electron density therefore fluctuates so some parts of molecule become more/less negative = temporary dipoles form which cause dipoles to form in neighbouring molecules = aka induced dipoles

Question 11

hydrogen bonding

Answer 11

occurs when hydrogen is bonded to either oxygen, nitrogen or fluorine. big difference in electronegativity between H and O,N,F = strong permanent dipole
- strongest type of intermolecular bonding