molecular structure

Question 1

bond length (d)

Answer 1

nuclear separation distance (nm)

Question 2

bond energy

Answer 2

energy required to break the bond (kJ mol⁻¹)

Question 3

How many electrons form one chemical bond?

Answer 3

2

Question 4

When atoms are the same, how do nuclei share electrons?

Answer 4

equally

Question 5

When atoms are different, how do nuclei share electrons?

Answer 5

unequally

Question 6

What does the unequal sharing of electrons result in?

Answer 6

polar covalent bond

Question 7

dipole moment, µ =

Answer 7

charge, Q (C) x distance between charge, d (m)

Question 8

What is the most electronegative element?

Answer 8

fluorine

Question 9

What is the most electropositive element?

Answer 9

caesium

Question 10

The smaller the atoms, the ? the bond.

Answer 10

shorter

Question 11

The more electrons in a bond, the ? a bond.

Answer 11

shorter

Question 12

The larger the electronegativity difference between the bonded atoms the ? the bond.

Answer 12

shorter

Question 13

As bonds become shorter, the ? bond energy increases.

Answer 13

more

Question 14

The more electrons in a bond, the ? bond energy increases.

Answer 14

more

Question 15

The larger the electronegativity difference between the bonded atoms, the ? bond energy increases.

Answer 15

more

Question 16

What structure do ionic compound form?

Answer 16

ionic lattices

Question 17

Do ionic lattices have low or high melting points?

Answer 17

high

Question 18

valence electrons

Answer 18

electrons in the highest atomic orbital

Question 19

Lewis structure

Answer 19

visual representation of the valence electrons in a molecule

Question 20

Is the central atom in a molecule often the most electronegative or electropositive?

Answer 20

electropositive

Question 21

octet

Answer 21

set of 4 electrons associated with an atom

Question 22

VESPR

Answer 22

1) Valence
2) Electron
3) Shell
4) Pair
5) Repulsion

Question 23

2 electron pairs

Answer 23

linear

Question 24

3 electron pairs

Answer 24

trigonal planar

Question 25

4 electron pairs

Answer 25

tetrahedral

Question 26

5 electron pairs

Answer 26

trigonal bipyramidal

Question 27

6 electron pairs

Answer 27

octahedral

Question 28

What is the linear bond angle?

Answer 28

180°

Question 29

What is the trigonal planar bond angle?

Answer 29

120°

Question 30

What is the tetrahedral bond angle?

Answer 30

109.5°

Question 31

3 bonded pairs + 1 lone pair

Answer 31

trigonal pyramidal

Question 32

What is the trigonal pyramidal bond angle?

Answer 32

107°

Question 33

2 bonded pairs + 2 lone pairs

Answer 33

bent

Question 34

What is the bent bond angle?

Answer 34

105°

Question 35

What is the trigonal bipyramidal bond angle?

Answer 35

90° + 120°

Question 36

4 bonded pairs + 1 lone pair

Answer 36

seesaw

Question 37

What is the seesaw bond angle?

Answer 37

120°

Question 38

3 bonded pairs + 2 lone pairs

Answer 38

t-shaped

Question 39

What is the t-shaped bond angle?

Answer 39

90°

Question 40

2 bonded pairs + 3 lone pairs

Answer 40

linear

Question 41

What is the octahedral bond angle?

Answer 41

90°

Question 42

5 bonded pairs + 1 lone pair

Answer 42

square pyramidal

Question 43

What is the square pyramidal bond angle?

Answer 43

90°

Question 44

4 bonded pairs + 2 lone pairs

Answer 44

square planar

Question 45

What is the square planar bond angle?

Answer 45

90°

Question 46

valence bond theory

Answer 46

electrons are localised in bonds between 2 atoms / localised on a single atom, usually in pairs

Question 47

What are the conventions of the orbital overlap model?

Answer 47

1) each electron is assigned to a specific orbital 2) no 2 electrons have identical descriptions 3) the electrons obey the aufbau principal 4) only the valence orbitals are needed to describe bonding

Question 48

sigma (σ) bond

Answer 48

1) end-to-end overlap of atomic orbitals | 2) single bond

Question 49

pi (π) bond

Answer 49

1) parallel overlap of atomic orbitals | 2) double bond

Question 50

triple (σ) bond

Answer 50

1 σ bond + 2 π bonds

Question 51

What does hybridisation of atomic orbitals form?

Answer 51

hybrid orbitals