BTEC APPLIED SCIENCE UNIT 1 CHEMISTRY
LATEST EXAM 2025 WITH MULTIPLE CHOICE
OF QUESTIONS AND DETAILED CORRECT
ANSWERS ALREADY GRADED A+ AND 100 %
GUARANTEE PASS (BRAND NEW!!!!!!)
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
In what molecules do Van der Waal's forces exist? - CORRECT
ANSWER-Non-polar molecules
How are permanent dipole-dipole forces formed? - CORRECT
ANSWER-Permanent dipole in one molecule attracts oppositely
charged permanent dipole in neighbouring molecule
In which molecules do permanent dipole-dipole forces exist? -
CORRECT ANSWER-Polar molecules
Which elements must be present for hydrogen bonds to exist? -
CORRECT ANSWER-Hydrogen and either nitrogen, oxygen or
fluorine
What is meant by the term displacement? - CORRECT ANSWER-
When a more reactive element takes the place of a less reactive
element in a compound
State the equation for determining moles - CORRECT ANSWER-Moles
= mass ÷ relative atomic mass (molar mass)
LATEST EXAM 2025 WITH MULTIPLE CHOICE
OF QUESTIONS AND DETAILED CORRECT
ANSWERS ALREADY GRADED A+ AND 100 %
GUARANTEE PASS (BRAND NEW!!!!!!)
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
In what molecules do Van der Waal's forces exist? - CORRECT
ANSWER-Non-polar molecules
How are permanent dipole-dipole forces formed? - CORRECT
ANSWER-Permanent dipole in one molecule attracts oppositely
charged permanent dipole in neighbouring molecule
In which molecules do permanent dipole-dipole forces exist? -
CORRECT ANSWER-Polar molecules
Which elements must be present for hydrogen bonds to exist? -
CORRECT ANSWER-Hydrogen and either nitrogen, oxygen or
fluorine
What is meant by the term displacement? - CORRECT ANSWER-
When a more reactive element takes the place of a less reactive
element in a compound
State the equation for determining moles - CORRECT ANSWER-Moles
= mass ÷ relative atomic mass (molar mass)
