BTEC Applied Science Unit 1 Chemistry Exam
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. Which subshells are available in the first energy level?: s
5. Which subshells are available in the second energy level?: s
and p
6. Which subshells are available in the third energy level?: s, p
and d
7. What is Hund's rule?: Orbitals must all be singly filled before they can be doubly
occupied
8. Which elements do not fill the 4s subshell before the 3d
subshell?: Copper and chromium
9. Define the term ionic bond: The electrostatic attraction between oppositely
charged ions
10. What is the charge of an ion from group 1?: +1
11. What is the charge of an ion from group 2?: +2
12. What is the charge of an ion from group 6?: -2
13. What is the charge of an ion from group 7?: -1
,14. Explain how atoms of sodium react with atoms of chlorine:
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
15. Why do ionic bonds have such high melting points?: 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
16. State two factors that affect the strength of an ionic bond:
Size of ion and charge on ion
17. When can ionic substances conduct electricity?: When molten or
in aqueous solution
18. Describe the properties of ionic compounds: Conduct electricity
when molten or aqueous solution
High melting/boiling points
Usually soluble in water
19. Define the term covalent bond: A shared pair of electrons
20. Which metals lose electrons from the 4s subshell before the
3d subshell?: -
Transition metals
,21. Why do metals have such high melting points?: Strong force of
attraction between positive
ions and delocalised electrons. This requires a large amount of energy to overcome.
22. State the two factors that affect the strength of metallic
bonding: Size of ion
Charge on ion
23. 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
24. Explain how the size of the metal ions affects the strength
of the metallic bond: The smaller the +ve ion the closer the nucleus is to the
delocalised electrons creating a greater attraction
25. Explain why metals conduct electricity: The delocalised electrons 'carry'
charge. Current flows because of this.
26. 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.
27. Explain why metals are ductile and malleable: The lattice structure
allows layers of metal ions to slide over each other without disrupting bonding
28. Name the 3 forces between molecules: Van der Waals
, Permanent dipole-dipole
Hydrogen bonds
29. Order the 3 forces between molecules in order of strongest
to weakest: Hy- drogen bonds
Permanent dipole-dipole
Van der Waals
30. 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
31. In what molecules do Van der Waal's forces exist?: Non-polar
molecules
32. How are permanent dipole-dipole forces formed?: Permanent
dipole in one molecule attracts oppositely charged permanent dipole in neighbouring
molecule
33. In which molecules do permanent dipole-dipole forces
exist?: Polar molecules
34. Which elements must be present for hydrogen bonds to
exist?: Hydrogen and either nitrogen, oxygen or fluorine
35. What is meant by the term displacement?: When a more reactive
element takes the place of a less reactive element in a compound
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. Which subshells are available in the first energy level?: s
5. Which subshells are available in the second energy level?: s
and p
6. Which subshells are available in the third energy level?: s, p
and d
7. What is Hund's rule?: Orbitals must all be singly filled before they can be doubly
occupied
8. Which elements do not fill the 4s subshell before the 3d
subshell?: Copper and chromium
9. Define the term ionic bond: The electrostatic attraction between oppositely
charged ions
10. What is the charge of an ion from group 1?: +1
11. What is the charge of an ion from group 2?: +2
12. What is the charge of an ion from group 6?: -2
13. What is the charge of an ion from group 7?: -1
,14. Explain how atoms of sodium react with atoms of chlorine:
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
15. Why do ionic bonds have such high melting points?: 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
16. State two factors that affect the strength of an ionic bond:
Size of ion and charge on ion
17. When can ionic substances conduct electricity?: When molten or
in aqueous solution
18. Describe the properties of ionic compounds: Conduct electricity
when molten or aqueous solution
High melting/boiling points
Usually soluble in water
19. Define the term covalent bond: A shared pair of electrons
20. Which metals lose electrons from the 4s subshell before the
3d subshell?: -
Transition metals
,21. Why do metals have such high melting points?: Strong force of
attraction between positive
ions and delocalised electrons. This requires a large amount of energy to overcome.
22. State the two factors that affect the strength of metallic
bonding: Size of ion
Charge on ion
23. 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
24. Explain how the size of the metal ions affects the strength
of the metallic bond: The smaller the +ve ion the closer the nucleus is to the
delocalised electrons creating a greater attraction
25. Explain why metals conduct electricity: The delocalised electrons 'carry'
charge. Current flows because of this.
26. 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.
27. Explain why metals are ductile and malleable: The lattice structure
allows layers of metal ions to slide over each other without disrupting bonding
28. Name the 3 forces between molecules: Van der Waals
, Permanent dipole-dipole
Hydrogen bonds
29. Order the 3 forces between molecules in order of strongest
to weakest: Hy- drogen bonds
Permanent dipole-dipole
Van der Waals
30. 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
31. In what molecules do Van der Waal's forces exist?: Non-polar
molecules
32. How are permanent dipole-dipole forces formed?: Permanent
dipole in one molecule attracts oppositely charged permanent dipole in neighbouring
molecule
33. In which molecules do permanent dipole-dipole forces
exist?: Polar molecules
34. Which elements must be present for hydrogen bonds to
exist?: Hydrogen and either nitrogen, oxygen or fluorine
35. What is meant by the term displacement?: When a more reactive
element takes the place of a less reactive element in a compound
