Day 1  Day 2  Day 3  Day 4  Day 5  Day 6

Day 1

Question 1

What are the protons, neutrons and electrons in the following atoms/ions:

• Ca20402+

• Na1123+

• Cl1737-

• Al13273+

• Sc21453+

Day 2

Question 1

Write the electronic configuration for the following ions:

• Na+

• O2-

• Mg2+

• Cl-

• Al3+

• Ca2+

Day 3

Question 1

Write the electronic configuration for​​ the following atoms:

• Na

• Ar

• K

• Ca

• Fe

• Kr

Day 4

Question 1

Write the electronic configuration for the following atoms:

• Fe2+

• Sc3+

• Cu

• O

• C2-

• Pb2+

Day 5

Question 1

Magnesium exists naturally as three isotopes:

• ²⁴Mg (mass number 24, relative abundance 79%)

• ²⁵Mg (mass number 25, relative abundance 10%)

• ²⁶Mg (mass number 26, relative abundance 11%)

a) How many protons, neutrons and electrons are there in each isotope of neutral magnesium?
b) Calculate the relative atomic mass of magnesium to​​ 2 decimal places.

Question 2

Boron has two stable isotopes:

• ¹⁰B (mass number 10, relative abundance 19.9%)

• ¹¹B (mass number 11, relative abundance 80.1%)

a) How many protons, neutrons and electrons are present in each isotope of boron?
b) Calculate the relative atomic mass of boron.
c) Explain briefly why the relative atomic mass is not a whole number.

Day 6

Question 1

An element X has two stable isotopes:

• 63X​​ 

• 65X​​ 

The relative atomic mass of​​ X​​ is​​ 63.6.

a) Let the percentage abundance of​​ 63X​​ be​​ p. Write an equation to represent the average relative atomic mass.
b) Solve to find the percentage abundance of each isotope.