3/22/25, 11:55
AM
BTEC APPLIED SCIENCE ALL EXAM QUESTIONS AND
ANSWERS WITH COMPLETE SOLUTIONS VERIFIED
LATEST UPDATE 2025/2026
Terms in this set (218)
What is Hund's rule? Orbitals must all be singly filled before they can be doubly occupied
Define the term ionic bond The electrostatic attraction between oppositely charged ions
What is the charge of an ion from group +1
1?
What is the charge of an ion from +2
group 2?
What is the charge of an ion from -2
group 6?
What is the charge of an ion from -1
group 7?
Na loses its 2s1 electron gaining a +ve charge.
Explain how atoms of sodium react
Cl gains an electron in the 3p subshell gaining a -ve
with atoms of chlorine
charge. The opposite charges attract to form NaCl
Each +ve ion is surrounded by 6 -ve ions and vice
Why do ionic bonds have such high
versa. Strong electrostatic attraction in every
melting points?
direction.
Requires a large amount of energy to break
State two factors that affect the Size of ion and charge on ion
strength of an ionic bond
When can ionic substances conduct When molten or in aqueous solution
electricity?
Conduct electricity when molten or aqueous
Describe the properties of ionic
solution High melting/boiling points
compounds
Usually soluble in water
Define the term covalent bond A shared pair of electrons
Which metals lose electrons from the Transition metals
4s subshell before the 3d subshell?
Why do metals have such high Strong force of attraction between positive ions and delocalised
melting points? electrons. This requires a large amount of energy to overcome.
State the two factors that affect the Size of ion
strength of metallic bonding Charge on ion
Explain how the charge on metal The larger the +ve charge the greater the attraction between the nucleus
ions affects the strength of the and the delocalised electrons
metallic bond
Explain how the size of the metal The smaller the +ve ion the closer the nucleus is to the delocalised
ions affects the strength of the electrons creating a greater attraction
metallic bond
Explain why metals conduct electricity The delocalised electrons 'carry' charge. Current flows because of this.
Particles are paced tightly so kinetic energy is passed from ion to ion.
Explain why metals conduct heat
The delocalised electrons also enable heat to be passed.
Explain why metals are ductile and The lattice structure allows layers of metal ions to slide over each
malleable other without disrupting bonding
1/
5
, 3/22/25, 11:55
AM
Van der Waals
Name the 3 forces between molecules Permanent dipole-dipole
Hydrogen bonds
Hydrogen bonds
Order the 3 forces between
Permanent dipole-
molecules in order of strongest to
dipole Van der Waals
weakest
Electrons move to one side, caused temporary dipole. This induces a temporary
How are Van der Waal's forces formed? dipole in neighbouring molecules. Attraction occurs between oppositely
charged dipoles
In what molecules do Van der Waal's Non-polar molecules
forces exist?
How are permanent dipole-dipole Permanent dipole in one molecule attracts oppositely charged
forces formed? permanent dipole in neighbouring molecule
In which molecules do permanent Polar molecules
dipole- dipole forces exist?
Which elements must be present for Hydrogen and either nitrogen, oxygen or fluorine
hydrogen bonds to exist?
When a more reactive element takes the place of a less reactive element
What is meant by the term
displacement? in a compound
Moles = mass ÷ relative atomic mass (molar
State the equation for determining
moles mass) (Mass= mr X moles)
Define the term Avogadro's Constant The number of atoms in a mole of a given substance
What is the equation for calculating % yield = (actual yield ÷ theoretical yield) x 100
% yield?
What is a group on the periodic table? A vertical column
What is a period on the periodic table? A horizontal row
The energy required to remove the outermost electron from one mole of
Define the term first ionisation energy
gaseous atoms to produce one mole of gaseous +1 ions
Define the term atomic radius The distance between the nucleus of an atom and the outermost electron
A measure of how well an atom attracts a bonding pair of electrons in
Define the term electronegativity
a covalent bond
Define the term malleability How easily a material can be hammered into shape
Define the term ductility How easily a material can be drawn into wires
Describe the trend in atomic radius Atomic radius increases
down any group
Explain the trend in atomic radius down Higher energy levels are filled. The orbitals in higher energy levels are
any group further from the nucleus
Describe the trend in first ionisation First ionisation energy decreases
energy down groups 1 and 2
Increased electron
Explain the trend in first ionisation shielding Greater
energy down groups 1 and 2 atomic radius
Smaller attraction to +ve nucleus
SO electron is easier to remove requiring less energy
2/
5
AM
BTEC APPLIED SCIENCE ALL EXAM QUESTIONS AND
ANSWERS WITH COMPLETE SOLUTIONS VERIFIED
LATEST UPDATE 2025/2026
Terms in this set (218)
What is Hund's rule? Orbitals must all be singly filled before they can be doubly occupied
Define the term ionic bond The electrostatic attraction between oppositely charged ions
What is the charge of an ion from group +1
1?
What is the charge of an ion from +2
group 2?
What is the charge of an ion from -2
group 6?
What is the charge of an ion from -1
group 7?
Na loses its 2s1 electron gaining a +ve charge.
Explain how atoms of sodium react
Cl gains an electron in the 3p subshell gaining a -ve
with atoms of chlorine
charge. The opposite charges attract to form NaCl
Each +ve ion is surrounded by 6 -ve ions and vice
Why do ionic bonds have such high
versa. Strong electrostatic attraction in every
melting points?
direction.
Requires a large amount of energy to break
State two factors that affect the Size of ion and charge on ion
strength of an ionic bond
When can ionic substances conduct When molten or in aqueous solution
electricity?
Conduct electricity when molten or aqueous
Describe the properties of ionic
solution High melting/boiling points
compounds
Usually soluble in water
Define the term covalent bond A shared pair of electrons
Which metals lose electrons from the Transition metals
4s subshell before the 3d subshell?
Why do metals have such high Strong force of attraction between positive ions and delocalised
melting points? electrons. This requires a large amount of energy to overcome.
State the two factors that affect the Size of ion
strength of metallic bonding Charge on ion
Explain how the charge on metal The larger the +ve charge the greater the attraction between the nucleus
ions affects the strength of the and the delocalised electrons
metallic bond
Explain how the size of the metal The smaller the +ve ion the closer the nucleus is to the delocalised
ions affects the strength of the electrons creating a greater attraction
metallic bond
Explain why metals conduct electricity The delocalised electrons 'carry' charge. Current flows because of this.
Particles are paced tightly so kinetic energy is passed from ion to ion.
Explain why metals conduct heat
The delocalised electrons also enable heat to be passed.
Explain why metals are ductile and The lattice structure allows layers of metal ions to slide over each
malleable other without disrupting bonding
1/
5
, 3/22/25, 11:55
AM
Van der Waals
Name the 3 forces between molecules Permanent dipole-dipole
Hydrogen bonds
Hydrogen bonds
Order the 3 forces between
Permanent dipole-
molecules in order of strongest to
dipole Van der Waals
weakest
Electrons move to one side, caused temporary dipole. This induces a temporary
How are Van der Waal's forces formed? dipole in neighbouring molecules. Attraction occurs between oppositely
charged dipoles
In what molecules do Van der Waal's Non-polar molecules
forces exist?
How are permanent dipole-dipole Permanent dipole in one molecule attracts oppositely charged
forces formed? permanent dipole in neighbouring molecule
In which molecules do permanent Polar molecules
dipole- dipole forces exist?
Which elements must be present for Hydrogen and either nitrogen, oxygen or fluorine
hydrogen bonds to exist?
When a more reactive element takes the place of a less reactive element
What is meant by the term
displacement? in a compound
Moles = mass ÷ relative atomic mass (molar
State the equation for determining
moles mass) (Mass= mr X moles)
Define the term Avogadro's Constant The number of atoms in a mole of a given substance
What is the equation for calculating % yield = (actual yield ÷ theoretical yield) x 100
% yield?
What is a group on the periodic table? A vertical column
What is a period on the periodic table? A horizontal row
The energy required to remove the outermost electron from one mole of
Define the term first ionisation energy
gaseous atoms to produce one mole of gaseous +1 ions
Define the term atomic radius The distance between the nucleus of an atom and the outermost electron
A measure of how well an atom attracts a bonding pair of electrons in
Define the term electronegativity
a covalent bond
Define the term malleability How easily a material can be hammered into shape
Define the term ductility How easily a material can be drawn into wires
Describe the trend in atomic radius Atomic radius increases
down any group
Explain the trend in atomic radius down Higher energy levels are filled. The orbitals in higher energy levels are
any group further from the nucleus
Describe the trend in first ionisation First ionisation energy decreases
energy down groups 1 and 2
Increased electron
Explain the trend in first ionisation shielding Greater
energy down groups 1 and 2 atomic radius
Smaller attraction to +ve nucleus
SO electron is easier to remove requiring less energy
2/
5
