Bonding

Question 1

ionic bonding

Answer 1

the electrostatic force of attraction between opositely charged ionsbformed by electron transfer

Question 2

do metal atoms lose or gain electrons

Answer 2

lose

Question 3

covalent bond

Answer 3

a shared pair of electrons

Question 4

dative covalent bond

Answer 4

the shared pair of electrons in a bond comes from one atom

Question 5

metallic bonding

Answer 5

the electrostatic force of attraction between positive metal ions and delocalised electrons

Question 6

factors that affect metallic bonding

Answer 6

1. number of protons- more protons=stronger bond
2. number of delocalised electrons per atom- more delocalised electrons=stronger bond
3. size of ion- smaller ion=smaller bond

Question 7

ionic bonding properties

Answer 7

•high boiling points- strong electrostatic forces
•good solubility in water
•poor conductivity when solid- ions can’t move
•good conductivity when molten

Question 8

molecular (simple covalent) bonding properties

Answer 8

•low melting and boiling points -weak intermolecular forces
•poor solubility in water
•poor conductivity when solid- no ions to conduct and electrons are localised
•poor conductivity when molten

Question 9

macromolecular (covalent) bonding properties

Answer 9

•high bpt and mpt- many strong covalent bonds
•insoluble in water
•poor conductivity apart from graphite

Question 10

metallic bonding properties

Answer 10

•high mpt and bpt- strong electrostatic forces
•insoluble in water
•good conductivity- delocalised electrons

Question 11

trigonal planar

Answer 11

3 bonding pairs
bond angle- 120
examples- BF3, NO3

Question 12

linear

Answer 12

2 bonding pairs
bond angle-180
examples- CO2,HCN

Question 13

tetrahedral

Answer 13

4 bonding pairs
bond angle-109.5
examples- SiCl4, SO4²‐

Question 14

trigonal pyramidal

Answer 14

3 bonding pairs, 1 lone pair
bond angle-107
examples- NCl3, PF3

Question 15

bent

Answer 15

2 bonding pairs, 2 lone pairs
bond angle- 104.5
examples-OCl2, H2S

Question 16

trigonal bipyrimidal

Answer 16

5 bonding pairs
bond angle- 120, 90
example- PCl5

Question 17

octahedral

Answer 17

6 bonding pairs
bond angle-90
example- SF6

Question 18

do lone pairs or bonding pairs repel more

Answer 18

lone pairs

Question 19

electronegativity

Answer 19

the tendency of an atom in a covalent bond to attract electrons towards itself

Question 20

what’s the most electronegative element

Answer 20

flourine

Question 21

factors affecting electronegativity

Answer 21

•increases across a period as number of protons increases and atomic radius decreases
•decreases down a group as distance between nucleus and outer electrons increase and shielding increases

Question 22

what type of bonding do compounds with small or none electronegativity have

Answer 22

pure covalent

Question 23

what type of bonding do compounds with a large electronegativity have

Answer 23

ionic

Question 24

when does a permanent dipole form

Answer 24

when the elements in the bond have different electronegativities

Question 25

polar covalent bond

Answer 25

unequal distribution of electrons

Question 26

symmetrical molecule

Answer 26

all bonds identical and no lone pairs, will never be polar even if individual bonds are polar

Question 27

Van der Waals forces

Answer 27

occur between all molecular substances and noble gases. Do not occur in ionic substances

Question 28

induced dipole

Answer 28

van der waals forces, when electrons are constantly moving and electron density fluctuates

Question 29

factors affecting size of van der waals

Answer 29

the more electrons the higher the chance of temporary dipoles, increases size of van der waals

Question 30

permanent dipole-dipole forces

Answer 30

•occur between polar molecules
•stronger than Van der Waals

Question 31

Hydrogen bonding

Answer 31

•occurs when hydrogen is attached to a Nitrogen, Oxygen or Fluorine
•there’s a large electronegativity between the H and the N,O,F
•occurs in addition with Van der Waals