Bonding

Question 1

What is a covalent bond?

Answer 1

Sharing a pair of electrons between two atoms

Question 2

What is electronegativity?

Answer 2

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

Question 3

How does electronegativity increase throughout the periodic table?

Answer 3

It increases as you go to the right kf the period table
Also increases as you go up the table

Question 4

What causes a polar bond?

Answer 4

When the more electronegative element in a covalent bond pulls the share of electrons closer to itself

Question 5

What causes a non polar bond?

Answer 5

when two atoms in the bond are the same
they have an equal share of electrons
e.g. F2

Question 6

What is ionic bonding?

Answer 6

strong electrostatic force of attraction between oppositely charged ions
NOT A BOND BUT AN ATTRACTION

Question 7

What is the structure of an ionic bond?

Answer 7

giant ionic lattice

Question 8

What are some properties of ionic compounds?

Answer 8

• solid at room temp due to giant lattice
• high melting/boiling point due to strong electrostatic attraction
• don’t conduct electricity as solid bc ions arent free to move
• brittle

Question 9

What is metallic bonding?

Answer 9

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

Question 10

What factors effect the strength of a metallic bond?

Answer 10

• ionic charge (high=strong)
• atomic radius (small=stronger)
• number of delocalised electrons (more=stronger

Question 11

What are some properties of metals?

Answer 11

• good conductors as delocalised electrons are free to move
• high melting/boiling point due to strong attraction between positive ions and delocalised electrons
• malleable as layers of ions slide over each other

Question 12

What is Co-ordinate bonding?

Answer 12

When one atom provides both electrons needed to form a covalent bond

Question 13

LP-LP > BP- LP > BP-BP

Answer 13

idk just remember that

Question 14

What are properties of a symmetrical (non polar) molecule?

Answer 14

• bonded to the same atoms
• NO lone pairs

Question 15

What is a dipole?

Answer 15

occurs when there is an ineven distribution of electron density in a molecule

Question 16

What is a Van der Waals force?

Answer 16

a temporary dipole in one molecule induces a dipole in another
there is an attraction between δ+molecule and δ-

Question 17

What affects the strength of VDW forces?

Answer 17

Size/Mr of molecule (bigger=more forces)
Surface area contact (more SA = more forces)

Question 18

What is a permanent dipole dipole force?

Answer 18

occurs between polar molecules
the δ+ on one molecule attracts the δ- on a neighbouring molecule

Question 19

What is hydrogen bonding?

Answer 19

occurs between polar molecules which have a hydrogen directly bonded to oxygen nitrogen or fluorine
these are the most electronegative atoms, pulling pair if electrons closer to themselves leaving hydrogen very δ+

Question 20

What are some features of a Hydrogen bonding diagram?

Answer 20

• partial charges on ALL atoms
• all lone lairs shld be clearly shown
• hydrogen bond shown between lone pair and δ+ on other molecule

Question 21

Why is ice less dense than liquid water? (hydrogen bonding)

Answer 21

there’s fewer particles of water per unit of volume in the a solid state

in ice water molecules are further apart than in liquid

so theres more gaps between molecules

Question 22

Can a giant ionic lattice conduct electricity?

Answer 22

when molten or dissolved
this is because ions are free to move

but not when theyre solid

Question 23

What is the melting/boiling point of a giant ionic lattice?

Answer 23

HIGH
due to strong electrostatic attraction between opposite ions

Question 24

Dies a giant metallic lattice conduct electricity?

Answer 24

yes
delocalised electrons are free to move

Question 25

What is the boiling point if a giant metallic lattice?

Answer 25

HIGH
due to strong electrostatic attraction between positive ions and delocalised electrons

Question 26

Describe a simple molecular crystal structure?

Answer 26

weak intermolecular forces between molecules are broken
strong covalent bonds between atoms stay intact

Question 27

Can a simple molecular crystal structure conduct electricity?

Answer 27

NO
theres no delocalised electrons

Question 28

What is the boiling point of a simple molecular crystal structure?

Answer 28

LOW
due to weak intermolecular forces between molecules

Question 29

Describe the bonds in a Diamond?

Answer 29

strong covalent bonds between carbon atoms

Question 30

Can a diamond conduct electricity?

Answer 30

NO
no delocalised electrons

Question 31

What is the boiling point of a Diamond?

Answer 31

HIGH
strong covalent binds require alot of energy to break

Question 32

Describe the bonds in Graphite?

Answer 32

strong covalent bond between carbon atoms
weak VDW forces between layers

have delocalised electrons that can move between the layers

Question 33

Can Graphite conduct electricity?

Answer 33

YES
delocalised elctrons can move

Question 34

What is the boiling point of Graphite?

Answer 34

HIGH
strong covalent bonds require a lot of energy to break

Question 35

Describe the bonds in Graphene?

Answer 35

Strong covalent bonds between atoms
delocalised electrons across it’s surface

Question 36

Can graphene conduct electricity?

Answer 36

YES
delocalised electrons can move

Question 37

What is the boiling point of Graphene?

Answer 37

High
strong covalent bonds required alot of energy to break