Chapter 5 - Electrons and Bonding

Question 1

How does group number relate to electronic structure?

Answer 1

The group number tells you how many electrons in the outermost shell.

Question 2

What is a shell?

Answer 2

Shells are energy levels, the energy levels increase as the shell number increases. The shell number may also be referred to as principal quantum number.

Question 3

What is an orbital?

Answer 3

A region around the nucleus that can hold up to two electrons with opposite spins.
It shows us a 95% probability of where an electron will exist.

Question 4

How many electrons can shell 1 hold?

Answer 4

2 electrons

Question 5

How many electrons can shell 2 hold?

Answer 5

8 electrons

Question 6

How many electrons can shell 3 hold?

Answer 6

18 electrons

Question 7

How many electrons can shell 4 hold?

Answer 7

32 electrons

Question 8

What shape is an s-orbital?

Answer 8

A spherical shape

Question 9

What shape is a p-orbital?

Answer 9

A dumb-bell shape

Question 10

What is an electron?

Answer 10

A cloud of negative charge, which has the shape of the orbital occupied by the electron.

Question 11

Which orbitals are in shell 1?

Answer 11

1 s-orbital

Question 12

Which orbitals are in shell 2?

Answer 12

1 s-orbital and 3 p-orbitals

Question 13

Which orbitals are in shell 3?

Answer 13

1 s-orbital, 3 p-orbitals and 5 d-orbitals.

Question 14

Which orbitals are in shell 4?

Answer 14

1 s-orbital, 3 p-orbitals, 5 d-orbitals and 7 f-orbitals

Question 15

What is a sub-shell?

Answer 15

All of the orbitals of the same type in the same shell.
e.g. s sub-shell and p sub-shells

Question 16

How many electrons can an s sub-shell hold?

Answer 16

2 electrons

Question 17

How many electrons can a p sub-shell hold?

Answer 17

6 electrons

Question 18

How many electrons can a d sub-shell hold?

Answer 18

10 electrons

Question 19

How many electrons can a f sub-shell hold?

Answer 19

14 electrons

Question 20

Order the sub-shells in terms of energy levels, starting from lowest.

Answer 20

s, p, d and f going up the shells.
With the exception of the 3d sub-shell which has a higher energy than 4s.

Question 21

Which sub-shells are in shell 1?

Answer 21

1s

Question 22

Which sub-shells are in shell 2?

Answer 22

2s, 2p

Question 23

Which sub-shells are in shell 3?

Answer 23

3s, 3p, 3d

Question 24

Which sub-shells are in shell 4?

Answer 24

4s, 4p, 4d, 4f

Question 25

What is the short notation for electronic structure?

Answer 25

The closest prior noble gas in square brackets and the remaining electronic configuration.

Question 26

How are orbitals drawn?

Answer 26

A square with two arrows in it pointing opposite directions to represent the opposite spins

Question 27

How are orbitals filled for ions?

Answer 27

Draw out the electronic structure of the atom. For a negative ion, add the extra electrons. For a positive ion, remove the electrons, if 4s is full remove the electrons from there before removing from 3d.

Question 28

What is the electronic structure of Chromium (Cr)?

Answer 28

1s2 2s2 2p6 3s2 3p6 4s1 3d5 As it is more stable due to both 4s and 3d being half-full.

Question 29

What is the electronic structure of Copper (Cu)?

Answer 29

1s2 2s2 2p6 3s2 3p6 4s1 3d10 As is makes a full 3d sub-shell and a half-full 4s sub-shell.

Question 30

What is ionic bonding?

Answer 30

Electrostatic attraction between positive and negative ions

Question 31

What are some common cations?

Answer 31

Metal ions and ammonium ions

Question 32

What are some common anions?

Answer 32

Non-metal ions and polyatomic ions

Question 33

What is a covalent bond?

Answer 33

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

Question 34

What two molecules is a covalent bond between?

Answer 34

Metal and non-metal

Question 35

Describe a single covalent bond.

Answer 35

A single shared pair of electrons from both the bonding atoms

Question 36

Describe multiple covalent bonding.

Answer 36

Multiple pairs of shared electrons from both the bonding atoms

Question 37

Describe a dative covalent bond.

Answer 37

A covalent bond where bond the electrons come from one of the bonding atoms only.

Question 38

What is average bond enthalpy?

Answer 38

Measurement of covalent bond strength.

Question 39

What is the structure of a giant ionic lattice?

Answer 39

Ions attraction oppositely charged ions in different directions Positive metal and negative non-metal ions all attracted to each other

Question 40

What are the properties of a giant ionic lattice?

Answer 40

High melting and boiling points - due to strong electrostatic forces between ions so high energy is required to overcome the forces of attraction Mostly water soluble, unless compound has too high charges then it doesn't dissolve in the water Conductive in molten and aqueous state but not solid - charge needs to be able to move freely in order to conduct electricity