UPDATED 2024 BTEC
Applied Science Unit 1
WITH QUESTIONS AND
VERIFIED CORRECT
ANSWERS GRADED A+
GUARANTEED PASS
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
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.
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 packed 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
Order the 3 forces between molecules in order of
strongest to weakest - ANSWER-Hydrogen bonds
Permanent dipole-dipole
Van der Waals
Applied Science Unit 1
WITH QUESTIONS AND
VERIFIED CORRECT
ANSWERS GRADED A+
GUARANTEED PASS
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
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.
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 packed 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
Order the 3 forces between molecules in order of
strongest to weakest - ANSWER-Hydrogen bonds
Permanent dipole-dipole
Van der Waals
