Chapter 5 - Electrons and bonding

Question 1

Where are shells with the highest energy levels located?

Answer 1

Further from the nucleus

Question 2

What are the four types of sub-shells?

Answer 2

S-orbital
P-orbital
D-orbital
F-orbital

Question 3

How many orbitals are there in an S sub-shell?

Answer 3

1

Question 4

How many electrons can fit in the S sub-shell?

Answer 4

2

Question 5

How many orbitals are there in the P sub-shell?

Answer 5

3

Question 6

How many electrons are can fit in the P sub-shell?

Answer 6

6

Question 7

How many orbitals are there in the D sub-shell?

Answer 7

5

Question 8

How many electrons can fit in the D sub-shell?

Answer 8

10

Question 9

How many orbitals are there in the F sub-shell?

Answer 9

7

Question 10

How many electrons can fit in the F sub-shell?

Answer 10

14

Question 11

What is an orbital?

Answer 11

An area of space that an electron moves in

Question 12

What is spin-pairing?

Answer 12

When there are two electrons in an orbital, they must spin in opposite directions

Question 13

What is the shape of S orbitals?

Answer 13

Spherical

Question 14

What is the shape of P orbitals?

Answer 14

Dumbbell

Question 15

How many P orbitals are there?

Answer 15

3

Question 16

What is sub shell notation?

Answer 16

You write the energy shell, then sub-shell, then the number of electrons, e.g. 1s2 2s2 2p6

Question 17

How to show electron configuration using the electrons in boxes method?

Answer 17

Each box represents one orbital and each arrow represents one electron
One arrow must go up and the other down

Question 18

What is important to remember about the 4s sub-shell?

Answer 18

It is at a lower energy level than the 3d sub-shell, so will fill first but also empties first
We also write the 3d sub-shell first

Question 19

In what manner will electrons fill orbitals with the same energy level?

Answer 19

Singly

Question 20

What is an ionic bond?

Answer 20

An eletrostatic attraction between two oppositely charged ions

Question 21

How can you work out the formula of an ionic compound?

Answer 21

Work out the charges on the ions and ensure it is balanced so the total charge is zero

Question 22

What is n electronic orbital?

Answer 22

A region around the nucleus that can hold up to two electrons

Question 23

What is a sub-shell?

Answer 23

Orbitals of the same type are grouped together

Question 24

What is important to remember about two electrons in the same orbital?

Answer 24

They must have opposite spins

Question 25

Why does the 4s shell fill before the 3d sub-shell?

Answer 25

It is at a lower energy level

Question 26

What is shorthand notation for electronic structure?

Answer 26

You write the symbol of the previous noble gas plus the outer electron sub-shells

Question 27

What are the three blocks of the periodic table?

Answer 27

S-block P-block D-block

Question 28

Where is the S-block?

Answer 28

The first two groups of the periodic table

Question 29

Where is the P-block?

Answer 29

The 6 groups on the right

Question 30

Where is the D-block?

Answer 30

The central 10 groups

Question 31

What does the block an element is in represent?

Answer 31

The highest energy electrons will be in that sub-shell

Question 32

What do dot and cross diagrams show?

Answer 32

The arrangement of electrons in an atom

Question 33

How to draw a dot and cross diagram?

Answer 33

Draw the outer shell of electrons inside a square bracket, using dots and crosses to show where the electrons came from. The charge should be indicated outside the bracket

Question 34

Example of a giant ionic lattice

Answer 34

Sodium chloride

Question 35

Why does sodium chloride have a high melting point?

Answer 35

It has very strong ionic bonds

Question 36

3 characteristics of ionic compounds

Answer 36

They can conduct electricity when molten but not solid High melting and boiling points Tend to dissolve in water

Question 37

Why can ionic compounds only conduct electricity when molten or dissolved?

Answer 37

In a solid, the ions are fixed in position by the ionic bonds, but when molten are mobile and can carry a charge

Question 38

Why do ionic compounds have high melting and boiling points?

Answer 38

A lot of energy is needed to overcome the strong electrostatic forces

Question 39

When will the melting point of an ionic lattice be higher?

Answer 39

For ions with greater charges, e.g. Ca 2+

Question 40

Why do ionic compounds tend to dissolve in water?

Answer 40

Water is a polar solvent, so the charged ends of the water molecule are attracted to the charged ions and pull the ions from the lattice, causing it to dissolve

Question 41

What does the solubility of an ionic compound depend upon?

Answer 41

The attractions within the lattice and the attraction between the ions and water molecules

Question 42

What is a covalent bond?

Answer 42

The strong electrostatic attraction between a shared pair of electrons and the nuclei of the bonded atoms

Question 43

What happens when two atoms bond covalently?

Answer 43

Orbital overlap occurs

Question 44

How to represent covalent bonds

Answer 44

Dot and cross diagrams with their outer orbitals overlapping

Question 45

What is the displayed formula?

Answer 45

It shows how the relative positioning of atoms and the bonds between them

Question 46

Give to exceptions to the octet rule

Answer 46

Boron trifluoride | Sulfur hexafluoride

Question 47

Why is boron trifluoride an exception?

Answer 47

Boron only has 6 outer electrons, not 8

Question 48

Why is sulfur hexafluoride an exception?

Answer 48

Sulfur has 12 electrons in its outer shell

Question 49

What are multiple covalent bonds?

Answer 49

When two atoms share more than one pair of electrons

Question 50

The best example of a double covalent bond

Answer 50

Oxygen, O2

Question 51

What is a double covalent bond?

Answer 51

When two atoms share two pairs of electrons

Question 52

The best example of a triple bond

Answer 52

Nitrogen, N2

Question 53

What is a triple bond?

Answer 53

The electrostatic attraction between three shared pairs of atoms and the nuclei of the bonded atoms

Question 54

What is special about CO2?

Answer 54

It has two double bonds

Question 55

What are dative covalent bonds?

Answer 55

Where both electrons come from one atom

Question 56

The best example of a dative covalent bond

Answer 56

NH3 and H+

Question 57

How do you know when to use a dative bond?

Answer 57

Draw the dot and cross diagram of the two components | Where there are two spare electrons on one atom, this becomes the dative bond