BTEC APPLIED SCIENCE UNIT 1 CHEMISTRY
EXAM QUESTIONS AND ANSWERS LATEST
2025-2026 UPDATE
Why do ionic bonds have such high melting points? - Answer-Each +ve
ion is surrounded by 6 -ve ions and vice versa.
Strong electrostatic attraction in every direction.
Requires a large amount of energy to break
State two factors that affect the strength of an ionic bond - Answer-Size
of ion and charge on ion
When can ionic substances conduct electricity? - Answer-When molten
or in aqueous solution
Describe the properties of ionic compounds - Answer-Conduct
electricity when molten or aqueous solution
High melting/boiling points
Usually soluble in water
,Define the term covalent bond - Answer-A shared pair of electrons
Which metals lose electrons from the 4s subshell before the 3d
subshell? - Answer-Transition metals
Why do metals have such high melting points? - Answer-Strong force
of attraction between positive ions and delocalised electrons. This
requires a large amount of energy to overcome.
How many electrons can an s subshell hold? - Answer-2
How many electrons can a p subshell hold? - Answer-6
How many electrons can a d subshell hold? - Answer-10
Which subshells are available in the first energy level? - Answer-s
Which subshells are available in the second energy level? - Answer-s
and p
Which subshells are available in the third energy level? - Answer-s, p
and d
, What is Hund's rule? - Answer-Orbitals must all be singly filled before
they can be doubly occupied
Which elements do not fill the 4s subshell before the 3d subshell? -
Answer-Copper and chromium
Define the term ionic bond - Answer-The electrostatic attraction
between oppositely charged ions
What is the charge of an ion from group 1? - Answer-+1
What is the charge of an ion from group 2? - Answer-+2
What is the charge of an ion from group 6? - Answer--2
What is the charge of an ion from group 7? - Answer--1
Explain how atoms of sodium react with atoms of chlorine - Answer-Na
loses its 2s1 electron gaining a +ve charge.
Cl gains an electron in the 3p subshell gaining a -ve charge.
The opposite charges attract to form NaCl
State the two factors that affect the strength of metallic bonding -
Answer-Size of ion
, Charge on ion
Explain how the charge on metal ions affects the strength of the metallic
bond - Answer-The larger the +ve charge the greater the attraction
between the nucleus and the delocalised electrons
Explain how the size of the metal ions affects the strength of the
metallic bond - Answer-The smaller the +ve ion the closer the nucleus is
to the delocalised electrons creating a greater attraction
Explain why metals conduct electricity - Answer-The delocalised
electrons 'carry' charge. Current flows because of this.
Explain why metals conduct heat - Answer-Particles are paced tightly
so kinetic energy is passed from ion to ion. The delocalised electrons
also enable heat to be passed.
Explain why metals are ductile and malleable - Answer-The lattice
structure allows layers of metal ions to slide over each other without
disrupting bonding
Name the 3 forces between molecules - Answer-Van der Waals
Permanent dipole-dipole
Hydrogen bonds
EXAM QUESTIONS AND ANSWERS LATEST
2025-2026 UPDATE
Why do ionic bonds have such high melting points? - Answer-Each +ve
ion is surrounded by 6 -ve ions and vice versa.
Strong electrostatic attraction in every direction.
Requires a large amount of energy to break
State two factors that affect the strength of an ionic bond - Answer-Size
of ion and charge on ion
When can ionic substances conduct electricity? - Answer-When molten
or in aqueous solution
Describe the properties of ionic compounds - Answer-Conduct
electricity when molten or aqueous solution
High melting/boiling points
Usually soluble in water
,Define the term covalent bond - Answer-A shared pair of electrons
Which metals lose electrons from the 4s subshell before the 3d
subshell? - Answer-Transition metals
Why do metals have such high melting points? - Answer-Strong force
of attraction between positive ions and delocalised electrons. This
requires a large amount of energy to overcome.
How many electrons can an s subshell hold? - Answer-2
How many electrons can a p subshell hold? - Answer-6
How many electrons can a d subshell hold? - Answer-10
Which subshells are available in the first energy level? - Answer-s
Which subshells are available in the second energy level? - Answer-s
and p
Which subshells are available in the third energy level? - Answer-s, p
and d
, What is Hund's rule? - Answer-Orbitals must all be singly filled before
they can be doubly occupied
Which elements do not fill the 4s subshell before the 3d subshell? -
Answer-Copper and chromium
Define the term ionic bond - Answer-The electrostatic attraction
between oppositely charged ions
What is the charge of an ion from group 1? - Answer-+1
What is the charge of an ion from group 2? - Answer-+2
What is the charge of an ion from group 6? - Answer--2
What is the charge of an ion from group 7? - Answer--1
Explain how atoms of sodium react with atoms of chlorine - Answer-Na
loses its 2s1 electron gaining a +ve charge.
Cl gains an electron in the 3p subshell gaining a -ve charge.
The opposite charges attract to form NaCl
State the two factors that affect the strength of metallic bonding -
Answer-Size of ion
, Charge on ion
Explain how the charge on metal ions affects the strength of the metallic
bond - Answer-The larger the +ve charge the greater the attraction
between the nucleus and the delocalised electrons
Explain how the size of the metal ions affects the strength of the
metallic bond - Answer-The smaller the +ve ion the closer the nucleus is
to the delocalised electrons creating a greater attraction
Explain why metals conduct electricity - Answer-The delocalised
electrons 'carry' charge. Current flows because of this.
Explain why metals conduct heat - Answer-Particles are paced tightly
so kinetic energy is passed from ion to ion. The delocalised electrons
also enable heat to be passed.
Explain why metals are ductile and malleable - Answer-The lattice
structure allows layers of metal ions to slide over each other without
disrupting bonding
Name the 3 forces between molecules - Answer-Van der Waals
Permanent dipole-dipole
Hydrogen bonds
