BTEC Applied Science All 2024
1. How many electrons can an s subshell hold? 2
2. How many electrons can a p subshell hold? 6
3. How many electrons can a d subshell hold? 10
4. What is Hund's rule? Orbitals must all be
singly filled before
they can be doubly
occupied
5. Define the term ionic bond The electrostatic
attraction between
oppositely charged
ions
6. What is the charge of an ion from group 1? +1
7. What is the charge of an ion from group 2? +2
8. What is the charge of an ion from group 6? -2
9. What is the charge of an ion from group 7? -1
10. Explain how atoms of sodium react with atoms of Na loses its 2s1
elecchlorine tron gaining a +ve
charge.
Cl gains an
electron in the 3p
subshell gaining a
-ve charge. The
opposite charges
attract to form
NaCl
,11. Why do ionic bonds have such high melting Each +ve ion is
surpoints? rounded by 6 -ve
ions and vice versa.
Strong electrostatic
attraction in every
direction.
Requires a large
amount of energy to
break
12. State two factors that affect the strength of an ionic Size of ion and
bond charge on ion
13. When can ionic substances conduct electricity? When molten or in
aqueous solution
14. Describe the properties of ionic compounds Conduct electricity
when molten or
aqueous solution
High melting/boiling
points
Usually soluble in
water
15. Define the term covalent bond A shared pair of elec-
trons
16. Which metals lose electrons from the 4s subshell Transition metals
before the 3d subshell?
17. Why do metals have such high melting points? Strong force of
attraction between
positive ions and
delocalised
, BTEC Applied Science All 2024
electrons. This
requires a large
amount of energy to
overcome.
18. State the two factors that affect the strength of Size of ion
metallic bonding Charge on ion
19. Explain how the charge on metal ions affects the
strength of the metallic bond
The larger the +ve charge the greater the attraction
between the nucleus
and the delocalised
electrons
20. Explain how the size of the metal ions affects the The smaller the +ve
strength of the metallic bond ion the closer the nu-
cleus is to the
delocalised
electrons creating a
greater attraction
21. Explain why metals conduct electricity The delocalised
electrons 'carry'
charge. Current
flows because of
this.
22. Explain why metals conduct heat Particles are paced
tightly so kinetic
energy is passed
from ion to ion. The
delocalised
electrons also
enable heat to be
passed.
, 23. Explain why metals are ductile and malleable The lattice structure
allows layers of
metal ions to slide
over each other
without disrupting
bonding
24. Name the 3 forces between molecules Van der Waals
Permanent dipole-
dipole
Hydrogen bonds
25. Order the 3 forces between molecules in order of Hydrogen bonds
strongest to weakest Permanent di-
pole-dipole
Van der Waals
26. How are Van der Waal's forces formed? Electrons move to
one side, caused
temporary dipole.
This induces a
temporary dipole in
neighbouring
molecules.
Attraction occurs
between oppositely
charged dipoles
27. In what molecules do Van der Waal's forces exist? Non-polar
molecules
28. How are permanent dipole-dipole forces formed? Permanent dipole
in one molecule attracts oppositely charged permanent dipole in
neighbouring molecule
1. How many electrons can an s subshell hold? 2
2. How many electrons can a p subshell hold? 6
3. How many electrons can a d subshell hold? 10
4. What is Hund's rule? Orbitals must all be
singly filled before
they can be doubly
occupied
5. Define the term ionic bond The electrostatic
attraction between
oppositely charged
ions
6. What is the charge of an ion from group 1? +1
7. What is the charge of an ion from group 2? +2
8. What is the charge of an ion from group 6? -2
9. What is the charge of an ion from group 7? -1
10. Explain how atoms of sodium react with atoms of Na loses its 2s1
elecchlorine tron gaining a +ve
charge.
Cl gains an
electron in the 3p
subshell gaining a
-ve charge. The
opposite charges
attract to form
NaCl
,11. Why do ionic bonds have such high melting Each +ve ion is
surpoints? rounded by 6 -ve
ions and vice versa.
Strong electrostatic
attraction in every
direction.
Requires a large
amount of energy to
break
12. State two factors that affect the strength of an ionic Size of ion and
bond charge on ion
13. When can ionic substances conduct electricity? When molten or in
aqueous solution
14. Describe the properties of ionic compounds Conduct electricity
when molten or
aqueous solution
High melting/boiling
points
Usually soluble in
water
15. Define the term covalent bond A shared pair of elec-
trons
16. Which metals lose electrons from the 4s subshell Transition metals
before the 3d subshell?
17. Why do metals have such high melting points? Strong force of
attraction between
positive ions and
delocalised
, BTEC Applied Science All 2024
electrons. This
requires a large
amount of energy to
overcome.
18. State the two factors that affect the strength of Size of ion
metallic bonding Charge on ion
19. Explain how the charge on metal ions affects the
strength of the metallic bond
The larger the +ve charge the greater the attraction
between the nucleus
and the delocalised
electrons
20. Explain how the size of the metal ions affects the The smaller the +ve
strength of the metallic bond ion the closer the nu-
cleus is to the
delocalised
electrons creating a
greater attraction
21. Explain why metals conduct electricity The delocalised
electrons 'carry'
charge. Current
flows because of
this.
22. Explain why metals conduct heat Particles are paced
tightly so kinetic
energy is passed
from ion to ion. The
delocalised
electrons also
enable heat to be
passed.
, 23. Explain why metals are ductile and malleable The lattice structure
allows layers of
metal ions to slide
over each other
without disrupting
bonding
24. Name the 3 forces between molecules Van der Waals
Permanent dipole-
dipole
Hydrogen bonds
25. Order the 3 forces between molecules in order of Hydrogen bonds
strongest to weakest Permanent di-
pole-dipole
Van der Waals
26. How are Van der Waal's forces formed? Electrons move to
one side, caused
temporary dipole.
This induces a
temporary dipole in
neighbouring
molecules.
Attraction occurs
between oppositely
charged dipoles
27. In what molecules do Van der Waal's forces exist? Non-polar
molecules
28. How are permanent dipole-dipole forces formed? Permanent dipole
in one molecule attracts oppositely charged permanent dipole in
neighbouring molecule
