Chapter 5 Electron Sturcture + Ionic Amd Covalemt Bonding And Structure

Question 1

Which shells have a higher energy

Answer 1

The ones further from the nucleus

Question 2

What is a shell divided into

Answer 2

Sub shells

Question 3

What is the principle quantum number and how do you find the maximum amount of electrons in a shell

Answer 3

The shell number
2n^2 where n=shell number

Question 4

What are the rules for each orbital

Answer 4

Shells are made from orbitals
Each one can hold 2 electrons with opposite spins
4 different types s,p,d,f

Question 5

Characteristics of s orbital

Answer 5

Spherical
From shell one each shell contains one s orbital
The greater the shell number the greater the radius of the s orbital
Contains 2 electrons in each shell

Question 6

Characteristics of a p orbital

Answer 6

3D dumbbell shape
From shell 2 each shell contains 3 p orbitals at right angles to each other
The max number of p electrons in each shell is 6

Question 7

D and f orbitals

Answer 7

D- from shell 3 each shell contains 5 d orbitals
Total d electrons is 10
F- from shell 4 each shell contains 7 f orbitals
Total f electrons is 14

Question 8

Definition of atomic orbital

Answer 8

A region within an atom that can hold up to electrons with opposite spins

Question 9

Describe what 1s^22s^22p^6 represents

Answer 9

The big numbers represent the shell number
The letters represent the sub shell
The powers represent the number of electrons

Question 10

Rules for electron configuration

Answer 10

1) electrons fill up the lowest energy sub shells first
2) electrons fill orbitals singularly before adding the second

Question 11

Exception to electron configuration rules

Answer 11

4S fills up before 3D
An exception to this is chromium and copper

Question 12

Describe the pattern on the periodic table

Answer 12

The s block is group one and two ( hydrogen and helium are 1s, lithium and beryllium are 2s)
The p block is group 3-0
The d block is the transition metals

Question 13

What is ionic bonding

Answer 13

Outer shell electron transferred from metal to non metal
Oppositely charged ions formed which are bonded by electrostatic attraction -multidirectional

Question 14

Define an ionic bond

Answer 14

The electrostatic attraction between oppositely charged ions

Question 15

What do the numbers in the formula of the ionically bonded substance represent

Answer 15

The ratio of the elements in the giant structure

Question 16

Structure of ionic compounds

Answer 16

Giant ionic lattice held by electrostatic forces
Each ion attracts oppositely charged ions from each direction

Question 17

Properties of an ionic substance

Answer 17

• High MP and BP=large amount of energy to break electrostatic forces (the greater the charge on the element the higher the mp and bp)
• Solubility= they dissolve in polar solvents however if the ionic attraction is too strong they can be slightly soluble or insoluble
• electrical conductivity =don’t conduct when solid, ions are fixed, do conduct when molten or aqueous as the ions are free to move and carry charge

Question 18

What is a covalent bond

Answer 18

Between non metals
Electron pairs occupy space between two atoms nuclei, it is unidirectional
Electrons attracted to both nuclei, this attraction overcomes the repulsion between the two nucleus

Question 19

Define covalent bond

Answer 19

A bond formed by a shared pair of electrons between two atoms. It is the attraction between the nuclei and the electrons

Question 20

What three things can atoms form when covalently bonded

Answer 20

Single unit eg H2
Giant covalent structure eg SiO2
Polyatimic ion NH4+

Question 21

Describe and define a molecule

Answer 21

Consists of a defined number of atoms covalently bonded
Is the smallest part of a covalent compound that can exist while maintaining the chemical properties of the compound

Question 22

Define lone pair

Answer 22

Is an outer shell pair of electrons that is not involved in chemical bonding

Question 23

How do you draw a dative bond

Answer 23

Arrow goes away from the atom with the lone pair of electrons
One dot either side of the arrow

Question 24

Common ions that contain dative bonds

Answer 24

Ammonium ion (NH4+) the H+ ion has no electrons NH3 has a lone pair
Oxonium ion (H3O+)

Question 25

Define dative covalent or coordinate bond

Answer 25

Shared pair of electrons which has been provided by one of the bonding atoms only

Question 26

What happens when there aren’t enough electrons to reach an octet (covalent)

Answer 26

Within period 2 this occurs to Be and B
They bond with what they can
Eg BF3
B ended up having 6 electrons in outer shell, missing two

Question 27

What happens when the octet is expanded (covalent)

Answer 27

Elements in group 5-7 from period three onwards
Down the periodic table more outer shell electrons are able to take part in bonding
Results in more than 8 in the outer shell

Question 28

Rules for expansion of the octet

Answer 28

Group 5
- can form 3 or 5(expansion) covalent bonds
Group 6
- can form 2, 4(expansion) or 6(expansion) covalent bonds
Group 7
- can form 1, 3(expansion), 5(expansion) or 7(expansion) covalent bonds

Question 29

Elements that can expand their octet

Answer 29

Group 5
P, As
Group 6
S
Se
Te
Group 7
Cl
Br
I
At

Question 30

The larger the bond enthalpy the …

Answer 30

Stronger the covalent bond