bonding and structure 1.4/1.5

Question 1

whats the definition of ionic bonding

Answer 1

when there is a large change in difference in electronegativity. electrons are completely transferred from one atom to another. electrostatic attraction between the oppositely charge ions

Question 2

properties of ionic bonding

Answer 2

-high melting point (strong electrostatic forces)
- conduct electricity when molten or dissolved (free ions)
-most are soluble in water (polar water can break lattice)

Question 3

whats the definition of covalent bonding

Answer 3

small difference in electronegativity. the atoms are kept together as they share the same electrons

Question 4

whats the definition of coordinate bond

Answer 4

both electrons come from the same atom

Question 5

structure of graphite

Answer 5

brittle hexagonal layers held my van der waals forces. each carbon bonded to 3 others.

Question 6

properties of graphite

Answer 6

-soft and slippery
-conductor (free ion)
-insoluble
high melting/boiling point

Question 7

structure of diamond

Answer 7

tetrahedral, each carbon bonded to 4 others.

Question 8

properties of diamond

Answer 8

-hard due to tetrahedral structure
-poor conductor no free ions
- insoluble
- high melting point/ boiling point

Question 9

properties of simple covalent structures

Answer 9

• low melting point/ boiling point (weak intermolecular forces)
• dont conduct (no free ions)
• soluble in non polar solutes

Question 10

definition of electronegativity

Answer 10

the power of an atom to attract the electrons in a covalent bond

Question 11

which experiences the most repulsion ( lone pairs and bonding pairs)

Answer 11

2 bond pairs 1 loan 1 bond 2 loan pairs
——————————————————–>
increase in repulsion

Question 12

how does nuclear charge effect electronegativity

Answer 12

more protons, stronger attraction between nucleus and bonding pair electrons.
as nuclear charge increases the electronegativity of an element increases

Question 13

how does atomic radius effect electronegativity

Answer 13

if atomic radius increases electronegativity decreases as electrons further away from the nucleus are held less tightly.

Question 14

how does shielding effect electronegativity

Answer 14

an increased number of shells will result in a decreased electronegativity due to the outer electron being further away from the nucleus therefore held less tightly

Question 15

how do van der waals forces occur

Answer 15

happens when atoms electrons move to one side cause repulsion in the next molecules electrons to move to side

Question 16

factors that effect van der waals

Answer 16

-amount of electrons (down group 7 inc)
-number of point of contact

Question 17

how do permanent dipole dipole occur

Answer 17

polar molecules come close partially positive side attracts partially negative side

Question 18

factors that effect permanent dipole dipole

Answer 18

larger differences in electronegativity—-stronger dipoles

Question 19

how do hydrogen bonds occur

Answer 19

when hydrogen bonds with F,O,N

Question 20

factor that effects hydrogen bonding

Answer 20

larger the electronegativity the stronger dipoles

Question 21

anomalous properties of water

Answer 21

• ice is less dense than water( ice contains tetrahedral water contains bent)
  -high melting/boiling point- hydrogen bonds

Question 22

whats the definition of metallic bonding

Answer 22

electrostatic attraction between positive metal ions and delocalized electrons

Question 23

factors effecting metallic bonding

Answer 23

• larger the charge the stronger electrostatic attraction

Question 24

properties of metals

Answer 24

malleable - layers slide
conductor- sea of delocalised electrons
- insoluble - cant for hydrogen binds with water