BTEC Applied Science All UPDATED
ACTUAL Exam Questions and CORRECT
Answers
How many electrons can an s subshell hold? - CORRECT ANSWER -2
How many electrons can a p subshell hold? - CORRECT ANSWER -6
How many electrons can a d subshell hold? - CORRECT ANSWER - 10
What is Hund's rule? - CORRECT ANSWER - Orbitals must all be singly filled before
they can be doubly occupied
Define the term ionic bond - CORRECT ANSWER - The electrostatic attraction between
oppositely charged ions
What is the charge of an ion from group 1? - CORRECT ANSWER - +1
What is the charge of an ion from group 2? - CORRECT ANSWER - +2
What is the charge of an ion from group 6? - CORRECT ANSWER - -2
What is the charge of an ion from group 7? - CORRECT ANSWER - -1
Explain how atoms of sodium react with atoms of chlorine - CORRECT 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
,Why do ionic bonds have such high melting points? - CORRECT 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 - CORRECT ANSWER - Size of
ion and charge on ion
When can ionic substances conduct electricity? - CORRECT ANSWER - When molten or
in aqueous solution
Describe the properties of ionic compounds - CORRECT ANSWER - Conduct electricity
when molten or aqueous solution
High melting/boiling points
Usually soluble in water
Define the term covalent bond - CORRECT ANSWER - A shared pair of electrons
Which metals lose electrons from the 4s subshell before the 3d subshell? - CORRECT
ANSWER - Transition metals
Why do metals have such high melting points? - CORRECT ANSWER - Strong force of
attraction between positive ions and delocalised electrons. This requires a large amount of energy
to overcome.
State the two factors that affect the strength of metallic bonding - CORRECT ANSWER -
Size of ion
Charge on ion
, Explain how the charge on metal ions affects the strength of the metallic bond - CORRECT
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 - CORRECT
ANSWER - The smaller the +ve ion the closer the nucleus is to the delocalised electrons
creating a greater attraction
Explain why metals conduct electricity - CORRECT ANSWER - The delocalised
electrons 'carry' charge. Current flows because of this.
Explain why metals conduct heat - CORRECT 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 - CORRECT ANSWER - The lattice
structure allows layers of metal ions to slide over each other without disrupting bonding
Name the 3 forces between molecules - CORRECT ANSWER - Van der Waals
Permanent dipole-dipole
Hydrogen bonds
Order the 3 forces between molecules in order of strongest to weakest - CORRECT
ANSWER - Hydrogen bonds
Permanent dipole-dipole
Van der Waals
How are Van der Waal's forces formed? - CORRECT ANSWER - Electrons move to one
side, caused temporary dipole. This induces a temporary dipole in neighbouring molecules.
Attraction occurs between oppositely charged dipoles
ACTUAL Exam Questions and CORRECT
Answers
How many electrons can an s subshell hold? - CORRECT ANSWER -2
How many electrons can a p subshell hold? - CORRECT ANSWER -6
How many electrons can a d subshell hold? - CORRECT ANSWER - 10
What is Hund's rule? - CORRECT ANSWER - Orbitals must all be singly filled before
they can be doubly occupied
Define the term ionic bond - CORRECT ANSWER - The electrostatic attraction between
oppositely charged ions
What is the charge of an ion from group 1? - CORRECT ANSWER - +1
What is the charge of an ion from group 2? - CORRECT ANSWER - +2
What is the charge of an ion from group 6? - CORRECT ANSWER - -2
What is the charge of an ion from group 7? - CORRECT ANSWER - -1
Explain how atoms of sodium react with atoms of chlorine - CORRECT 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
,Why do ionic bonds have such high melting points? - CORRECT 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 - CORRECT ANSWER - Size of
ion and charge on ion
When can ionic substances conduct electricity? - CORRECT ANSWER - When molten or
in aqueous solution
Describe the properties of ionic compounds - CORRECT ANSWER - Conduct electricity
when molten or aqueous solution
High melting/boiling points
Usually soluble in water
Define the term covalent bond - CORRECT ANSWER - A shared pair of electrons
Which metals lose electrons from the 4s subshell before the 3d subshell? - CORRECT
ANSWER - Transition metals
Why do metals have such high melting points? - CORRECT ANSWER - Strong force of
attraction between positive ions and delocalised electrons. This requires a large amount of energy
to overcome.
State the two factors that affect the strength of metallic bonding - CORRECT ANSWER -
Size of ion
Charge on ion
, Explain how the charge on metal ions affects the strength of the metallic bond - CORRECT
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 - CORRECT
ANSWER - The smaller the +ve ion the closer the nucleus is to the delocalised electrons
creating a greater attraction
Explain why metals conduct electricity - CORRECT ANSWER - The delocalised
electrons 'carry' charge. Current flows because of this.
Explain why metals conduct heat - CORRECT 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 - CORRECT ANSWER - The lattice
structure allows layers of metal ions to slide over each other without disrupting bonding
Name the 3 forces between molecules - CORRECT ANSWER - Van der Waals
Permanent dipole-dipole
Hydrogen bonds
Order the 3 forces between molecules in order of strongest to weakest - CORRECT
ANSWER - Hydrogen bonds
Permanent dipole-dipole
Van der Waals
How are Van der Waal's forces formed? - CORRECT ANSWER - Electrons move to one
side, caused temporary dipole. This induces a temporary dipole in neighbouring molecules.
Attraction occurs between oppositely charged dipoles
