IB Bonding

Question 1

(IB) COVALENT BONDING

Answer 1

The unpaired electron of each no-metal atom overlap to fill a bonding orbital

Question 2

(IB) What does each atom have a strong attraction to

Answer 2

it’s own electron and the electron of the neighbouring atom

Question 3

(IB) BOND LENGTH

Answer 3

The distance between the nuclei of 2 bonded atoms

Question 4

(IB) PERFECT DISTANCE

Answer 4

minimizes repulsions and maximizes attractions between the 2 atoms

Question 5

(IB) Factor that affect bond length

Answer 5

Size of atoms
Bond Order

Question 6

(IB) SIZE OF ATOMS

Answer 6

The valence electrons form the covalent bonds

Question 7

(IB) pattern for the size of atoms

Answer 7

the bigger the atom, the further the valence electrons from the nucleus, therefore the bond length increases.

Question 8

(IB) BOND LENGTH

Answer 8

of shared pairs of electron

• single covalent bond = bond order is 1
• double covalent bond = bond order is 2

Question 9

(IB) bond length pattern

Answer 9

as the bond order inc. the bond length dec.
- inc. #of electrons for the nuclei to be attracted to
- further overlap of bonding orbitals (VBT)

Question 10

(IB) BOND ENERGY (ENTHALPY)

Answer 10

Bond strength; how strong is the bond?
- how much energy is stored in the bond

Question 11

(IB) chemical reaction reactants to individual atoms

Answer 11

breaking bonds (requires energy) (endo)

Question 12

(IB) chemical reactions individual atoms to products

Answer 12

forming new bonds (releases energy) (exo)
- new attractions

Question 13

(IB) Difference in enthalply

Answer 13

how much energy released v. how much energy required

Question 14

(IB) EQUATION FOR ENTHALPY

Answer 14

sum of(bond energy enthalpy reactants) - sum of(bond energy enthalpy of bonds forming)

Question 15

(IB) COORDINATE COVALENT BOND

Answer 15

lone pair becomes a bond pair

Question 16

(IB) RADICAL

Answer 16

unpaired electron (most)
- unpaired electron occupies the same space as a lone pair

Question 17

(IB) properties of a RADICAL

Answer 17

• very unstable
• high potential energy
• very reactive

Question 18

(IB) EXPANDED OCTET

Answer 18

central atom is p3 or higher, since it has available space (d-sublevel) for more than 4 shared pairs of electron

Question 19

(IB) lone pair =

Answer 19

2 bonding electron

Question 20

(IB) central atom could have how many bond sites/lone pairs in an expanded octet

Answer 20

5-8

Question 21

(IB) RESONANCE STRUCTURES

Answer 21

multiple acceptable lewis structures that differ in the location of lone pairs and multiple bonds

Question 22

(IB) FAVOURED RESONANCE STRUCTURE

Answer 22

(IB) typically, one of the resonance structures is the most likely/favoured structure

Question 23

(IB) FORMAL CHARGE

Answer 23

(IB) calculation performed in order to determine the most likely/acceptable resonance structure

Question 24

(IB) formal charge formula

Answer 24

(# of valence electron) - (# of lone pair electron) - 1/2(# of bonding electron)

Question 25

(IB) what does the best resonance structure have

Answer 25

lowest difference in formal charge

Question 26

(IB) is high or low magnitude preferred for resonance structure

Answer 26

low magnitude

Question 27

(IB) what is the tie-breaker for a favoured resonance structure?

Answer 27

the more EN atom should have a more negative FC

Question 28

(IB) AMMONIUM

Answer 28

NH4^+

Question 29

(IB) HYDROXIDE

Answer 29

OH^-

Question 30

(IB) NITRATE

Answer 30

NO3^-

Question 31

(IB) HYDROGEN CARBONATE (BICARBONATE)

Answer 31

HO3^-

Question 32

(IB) CARBONATE

Answer 32

CO3^2-

Question 33

(IB) SULFATE

Answer 33

SO4^2-

Question 34

(IB) PHOSPHATE

Answer 34

PO4^3-